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Flashcardlet > Science: Honors Chemistry > Flashcards

Science: Honors Chemistry Flashcards

0
Q

Summer work:

A quantity adopted as a standard of measurement

A

Unit

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1
Q

Summer work:

The temperature at which the minimum average kinetic energies of all particles occur

A

Absolute zero

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2
Q

Summer work:

The energy of an object that is due to the object’s motion

A

Kinetic energy

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3
Q

Summer work:

A change of matter from one form to another without a change in physical properties

A

Physical change

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4
Q

Summer work:

Any change in matter in which energy is released

A

Exothermic

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5
Q

Summer work:

A measure of the size of a body or region in 3-dimensional space

A

Volume

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6
Q

Summer work:

Elements that exist as single atoms

A

Monatomic

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7
Q

Summer work:

A measure of the average kinetic energy of the particles in an object, a measure of how hot or cold something is

A

Temperature

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8
Q

Summer work:

A substance or molecule that participates in a chemical reaction

A

Reactant

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9
Q

Summer work:
The energy transferred between objects that are at different temperatures. Energy is always transferred from higher-temperature objects to lower-temperature objects

A

Heat

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10
Q

Summer work:

A change that occurs when one or more substances change into entirely new substances with different properties

A

Chemical change

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11
Q

Summer work:

A substance that forms in a chemical reaction

A

Product

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12
Q

Summer work:
Changes in which the identity of a substance doesn’t change
Ex: state change

A

Physical changes

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13
Q

Summer work:

A measure of the amount of matter in an object. Not affected by the forces that act on the object

A

Mass

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14
Q

Summer work:
Consists of 2 or more atoms combined (bonded together) in a definite ratio, the smallest unit of a substance that keeps all of the physical and chemical properties of that substance

A

Molecule

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15
Q

Summer work:

The change of a substance from a liquid to a gas

A

Evaporation

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16
Q

Summer work:

The physical forms of matter: solid, liquid, gas, and plasma

A

States of matter

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17
Q

Summer work:

Law that states energy cannot be created or destroyed but can be changed from one form to another

A

Law of Conservation of Energy

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18
Q

Summer work:

The identities of substances change and new substances form

A

Chemical changes

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19
Q

Summer work:
A property of matter that describes a substance’s ability to participate in chemical reactions and can only be identified when an object tries to undergo a chemical change
Ex: flammability, reactivity w/ acid or oxygen

A

Chemical property

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20
Q

Summer work:
A characteristic of a substance that does not involve a chemical change
Ex: mass, color, texture

A

Physical property

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21
Q

Summer work:

A measure of the gravitational force exerted on an object (mass). Depends on gravity, varies with location.

A

Weight

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22
Q 
Summer work:
Evidence of chemical change:
1) evolution of a \_\_
2) formation of a \_\_\_\_
3) release or absorption of \_\_\_
4) \_\_ \_\_\_ in the reaction system
A

Gas
Precipitate
Energy
Color change

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23
Q

Summer work:

Anything that has mass and takes up space

A

Matter

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24
Q

Summer work:

Any substance that has a definite composition

A

Chemical

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25
Q

Summer work:

The smallest unit of an element that maintains the properties of that element

A

Atom

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26
Q

Summer work:

A pure substance that are not elements made up of atoms of 2 or more different elements joined by chemical bonds

A

Compound

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27
Q

Summer work:
The quantity of heat required to raise a unit of mass of homogeneous material 1 K or 1*C in a specified way given constant pressure and volume

A

Specific heat

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28
Q

Summer work:

Something that has magnitude, size, or amount

A

Quantity

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29
Q

Summer work:

Any change in matter in which energy is absorbed

A

Endothermic

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30
Q

Summer work:

The process by which one or more substances change to produce one or more different substances

A

Chemical reactions

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31
Q

Summer work:
Pure substance that contain only one kind of atom that cannot be separated or broken down into simpler substances by chemical means

A

Element

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32
Q

Summer work:

_ L = ____ mL = ____ cm^3

A

1
1000
1000

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33
Q

Summer work:
Something that has a uniform structure or composition throughout, pure substances are distributed uniformly throughout the mixture

A

Homogeneous

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34
Q

Summer work:

A sample of matter that has definite chemical & physical properties

A

Pure substance

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35
Q

Summer work:

The capacity to do work. Cannot be created or destroyed.

A

Energy

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36
Q

Summer work:

Composed of dissimilar components, contains substances that are not evenly mixed

A

Heterogeneous

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37
Q

Summer work:
The mass of the object divided by its volume; often expressed as grams per cubic cm for solids and liquids and as grams per liter for gases

A

Density

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38
Q

Summer work:
Have fixed volume & shape

Have fixed volume but not a fixed shape

Have neither fixed volume nor fixed shape

A

Solids
Liquids
Gases

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39
Q

Summer work:
A sample of matter that contains 2 or more pure substances, a combination of 2 or more substances that are not chemically combined

A

Mixture

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40
Q

Stoichiometry:

Proportional relationship between 2 or more substances during a chemical reaction

A

Stoichiometry

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41
Q

Stoichiometry:

% yield= (____ yield/ ____ yield) x 100

A

Experimental

Theoretical

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42
Q

Stoichiometry:
The chemical which will effectively determine the amount of products that are formed & the chemical which will run out first as the reaction occurs and the reactants are consumed

A

Limiting Reagent

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43
Q

Stoichiometry:

The other reactants, the ones that are leftover when the limiting reagent runs out, are said to be _ __

A

In excess

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44
Q

Stoichiometry:
Coefficients in a balanced chemical equation show the relative # of moles of each substance in the reaction. You can use the coefficients as a conversion factor

A

Mole ratio

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45
Q

Gases:

The amount of force being exerted on a surface. Can be thought of as the weight of the atmosphere on top of an object.

A

Pressure

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46
Q

Gases:
1 atm = 14.7 psi
(___ __ __ ___)

A

Pounds per square inch

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47
Q

Gases:

The movement of individual molecules through a hole in a solid

A

Effusion

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48
Q

Gases:

Law of partial pressures equation

A

Total pressure= pressure #1 + pressure #2 (etc)

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49
Q

Gases:

For a fixed amount of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional

A

Boyle’s Law

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50
Q

Gases:
The atmosphere is __% Nitrogen, __% oxygen, __% Argon, <__% of other gases. 99.9% of Earth’s atmosphere can be found in the __ & ____

A 
78%
21%
1%
1%
Troposphere 
Stratosphere
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51
Q

Gases:

Random motion of small particles is called

A

Brownian motion

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52
Q

Gases:

The ratio between the pressure volume product and the temperature of a system remains constant

A

The combined gas law

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53
Q

Gases:

More collisions = __ pressure

A

Greater

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54
Q

Gases:

Gay-Lussac’s Law (pressure/temperature law) equation

A

P1/T1=P2/T2

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55
Q

Gases:

A 1 square inch column column of air weighs ~ __ lbs. This is defined as 1 ___ of pressure.

A

14.7

Atmosphere

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56
Q

Gases:
For gases collected over a liquid, the __ __ of the liquid must be accounted for. __ is present b/c some of the molecules are able to escape the surface of the liquid. The __ __ of the liquid is dependent on temperature

A

Partial pressure
Vapor
Vapor pressure

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57
Q

Gases:

Boyle noticed that pressure & volume of gases were __ __. As pressure went up, volume went __

A

Inversely proportional

Down

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58
Q

Gases:

Boyle’s Law equation

A

P1V1=P2V2

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59
Q

Gases:

Declared by John Dalton. States total pressure is the sum of the individual pressures added together

A

Law of partial pressures

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60
Q

Gases:

Melting & Boiling points are directly affected by: __ & __

A

Temperature

Pressure

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61
Q

Gases:

Molar mass equation

A 
M=mRT/PV
M: molar mass
m: mass given
R: .0821
T: temperature 
P: pressure 
V: volume
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62
Q

Gases:

Graham’s law equation

A

Rate 1/ Rate 2 = (molar mass 2/ molar mass 1)^.5

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63
Q

Gases:

The general movement of particles from an area of higher concentration to an area of lower concentration

A

Diffusion

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64
Q

Gases:

Density equation

A 
D=MP/RT
D: density
M: molar mass
P: pressure
R: .0821
T: temperature
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65
Q

Gases:

Formula for pressure

A

P= F/A
P: pressure
F: force (lbs)
A: area (in^2)

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66
Q

Gases:
Einstein effectively proves the existence of atoms by explaining Brownian motion as the result of __ __ between the ___ & __ __

A

Random collisions
Particles
Gas molecules

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67
Q 
Gases:
Real gases are:
1) \_\_ point particles
2) \_\_ infinitely compressible 
3) show at least a small amount of \_\_ to other molecules
A

Not
Not
Attraction

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68
Q

Gases:

For a fixed amount of an ideal gas kept at a fixed volume, pressure & temperature are directly proportional

A

Gay-Lussac’s Law

The pressure/temperature law

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69
Q

Gases:

Avogadro stated that equal volumes of gases contain __ number of particles

A

Equal

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70
Q

Gases:
Theory used to explain macroscopic properties of gases such as:
1)
2)
3)
Due to the __ of tiny particles (atoms/molecules)

A 
Kinetic-Molecular Theory
1) pressure
2) temperature
3) volume 
Motion
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71
Q

Gases:

Ideal gas law equation

A 
PV=nRT
P: pressure (atm)
V: volume (L)
n: moles
R: .0821 
T: temperature (K)
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72
Q

Gases:

The combined gas law equation

A

(P1V1)/T1=(P2V2)/T2

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73
Q

Gases:
Gay-Lussac stated as the temperature of a gas increases, the volume __ __. Lussac called this __ __ b/c he used this person’s stuff

A

Increases proportionally

Charles’s law

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74
Q

Gases:

For a fixed amount of an ideal gas kept at a fixed pressure, volume and temperature are directly proportional

A

Charles’s Law

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75
Q

Gases:

Gas pressure can be measured using a __

A

Manometer

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76
Q 
Gases:
Properties of gases
1) great \_\_ b/w particles
2) is a \_\_\_
3) low \_\_\_
4) highly \_\_\_\_
5) \_\_ fill a container
A 
distance
fluid 
density
compressible 
Completely
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77
Q 
Gases:
Ideal gases consist of:
1) random moving \_\_ \_\_ that 
2) are \_\_ compressible and
3) have no intermolecular \_\_\_
A

Point particles
Infinitely
Attractions

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78
Q

Gases:

Charles’s law equation

A

V1/T1=V2/T2

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79
Q

Gases:

Avogadro’s Law equation

A

V1/n1=V2/n2

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80
Q

Gases:

Gay-Lussac stated as the temperature of a gas increases, the pressure __ __

A

Increases proportionally

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81
Q

Gases:

For an ideal gas kept at a fixed pressure and temperature, volume and moles are directly proportional

A

Avogadro’s Law

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82
Q

Solutions:

Solutions must be a __ mixture

A

Homogeneous

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83
Q

Solutions:

A solution that cannot dissolve any more solute under the given conditions

A

Saturated solution

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84
Q

Solutions:

When ionic compounds dissolve in water, they ___. Compounds that break up into ions when dissolved are called ____

A

Dissociate

Electrolytes

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85
Q

Solutions:

Calculating concentration equation

A

% conc = ( solute / total solution ) * 100

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86
Q

Solutions:

Solutions can be in the phases of __, ___, & ___

A

Solids
Liquids
Gases

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87
Q

Solutions:

Solubilities of gases generally __ with increasing ___, but ___ with increasing ___

A

Decrease
Temperature
Increase
Pressure

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88
Q

Solutions:

Polar molecules dissolve __ molecules. Non polar molecules dissolve __ molecules

A

Polar

Non polar

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89
Q

Solutions:

A solution holding more dissolved solute than what is required to reach equilibrium at a given temperature

A

Supersaturated solution

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90
Q

Solutions:

The concentration of a solution expressed in moles of solute / liters of solution. Abbreviated __

A

Molarity

M

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91
Q

Solutions:
A typical solution consists of a __ solute dissolved in a __ solvent. When both substances are in the same ___, the substance that there is the most of is the ____.

A

Solid
Liquid
Phase
Solvent

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92
Q

Solutions:

When a substance is written with square brackets, [ ], = “__ __ __”. M pronounced “__” when used in a sentence

A

The concentration of

Molar

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93
Q

Solutions:
Ability of one substance to dissolve into another at a given ___ & ___. Expressed in terms of the amount of __ that will dissolve in a given amount of __ to produce a __ __

A 
Solubility
Temperature & pressure 
Solute
Solvent
Saturated solution
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94
Q

Solutions:

Dilution equation

A

M1V1 = M2V2
M: molarity
V: volume

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95
Q

Solutions:

Solubilities of solids generally __ with increasing __, but generally ___ with increasing ___

A

Increase
Temperature
Remain constant
Pressure

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96
Q

Solutions:
Solids that dissolve but don’t dissociate. Non-ionic solids that will dissolve in water, but will not conduct electricity

A

Non-electrolytes

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97
Q

Solutions:

Dissolved salts. Ionic solids that will dissolve in water and conduct electricity

A

Electrolytes

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98
Q

Solutions:

A solution that contains less solute than a saturated solution and that is able to dissolve additional solute

A

Unsaturated solution

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99
Q

Solutions:

Saturated solutions occur when __ is reached between __ & __ of the __. This is know as __ __

A 
Equilibrium
Dissolving
Recrystallizing
Solute
Dynamic Equilibrium
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100
Q

Solutions:
ppm= __ __ __ or __ __ / __ __
ppb= __ __ __ or __ __ / __ __

A

Parts per million
mg solute / kg solution
Parts per billion
ug solute / kg solution

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101
Q

Solutions:
Solutions have two parts:
__: substance being dissolved (changes phases)
__: substance doing the dissolving

A

Solute

Solvent

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102
Q

Equilibrium:
Reactions where almost all of the reactants are turned into products. Very little, if any reactant remains when the reaction is complete

A

Completion reactions

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103
Q

Equilibrium:
State of balance in which the rate of a forward reaction equals the rate of the reverse reactions and the concentrations of products and reactants remain unchanged. It is a state of __ ___

A

Chemical equilibrium

Dynamic equilibrium

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104
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Exothermic:
Lowering temperature

A

Shift right

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105
Q

Equilibrium:

If Keq >1, then the reaction is considered __, because there will be more __ than __ at equilibrium

A

Favorable
Product
Reactants

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106
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Concentration:
Add

A

Shift to opposite side

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107
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Exothermic:
Raising temperature

A

Shift left

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108
Q 
Equilibrium: 
The system responds to 3 different kinds of stress:
1) changes in 
2) changes in 
3) changes in
A

Concentrations of reactants or products
Temperature
Pressure

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109
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Increase in pressure

A

Shift to side with fewer gas molecules

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110
Q

Equilibrium:

States that a system in equilibrium will oppose a change in a way that helps eliminate the change

A

Le Chatelier’s Principle

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111
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Endothermic:
Raising temperature

A

Shift right

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112
Q

Equilibrium:

For Keq constant, do not include ___ or __ as their concentrations don’t change

A

Solids

Liquids

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113
Q

Equilibrium:

If Keq=1, then neither reactants nor products are ___, both exist in __ __ at equilibrium

A

Favored

Equal amounts

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114
Q

Equilibrium:

Reduction of the solubility of a salt in the solution due to the addition of a common ion

A

Common ion effect

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115
Q

Equilibrium:

The Equilibrium constant equation

A

Keq= [products]^x / [reactants]^y

Where [ ] is the concentration in molarity of each substance and its coefficient is the exponent

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116
Q

Equilibrium:

Is Keq for the special case of a slightly soluble salt in water

A

Ksp

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117
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Endothermic:
Lowering temperature

A

Shift left

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118
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Decrease pressure

A

Shift to side with more gas molecules

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119
Q

Equilibrium:

A reaction in which the products re-form the original reactants

A

Reversible reactions

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120
Q

Equilibrium:

If Keq <1, then the reaction is considered __, because there will be more ___ than ___ at equilibrium

A

Unfavorable
Reactants
Products

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121
Q

Equilibrium:
Change H < 0 = __ reaction
Change H > 0 = __ reaction

A

Exothermic

Endothermic

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122
Q

Equilibrium:
Effect of change on equilibrium (describe the shift):
Concentration:
Subtract

A

Shift to same side

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123
Q

Acids & Bases:

Calculating pOH & [OH-]

A 
pOH = -log[OH-]
[OH-]= 10^-pOH
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124
Q

Acids & Bases:

__ have a pH < 7, __ have a pH > 7

A

Acids

Bases

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125
Q

Acids & Bases:

Only a small fraction of its molecules are ionized at any given time, producing only a few hydronium ions

A

Weak acids

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126
Q

Acids & Bases:

Arrhenius definition of a base

A

Any substance that forms hydroxide ions in solution

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127
Q

Acids & Bases:

Compounds that can reversibly change color depending on the pH of the solution or other chemical change

A

Indicators

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128
Q

Acids & Bases:

A solution is considered __ if the concentrations of the hydronium & hydroxide ions are equal (pH of 7)

A

Neutral

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129
Q

Acids & Bases:
Value used to express the acidity or basicity of a solution. It is defined as the logarithm of the reciprocal of the concentration of hydronium ions

A

pH

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130
Q

Acids & Bases:

Arrhenius definition of an acid

A

Any substance that forms hydronium ions in solution

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131
Q

Acids & Bases:

Self-ionization constant of water

A

Kw

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132
Q

Acids & Bases:

Releases few hydroxide ions in solution

A

Weak bases

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133
Q 
Acids & Bases:
Properties of acids:
1) Solutions \_\_ \_\_ well
2) react with many \_\_
3) \_\_ taste
4) acids generate \_\_ \_\_ (\_\_) in water
A

Conduct electricity
Metals
Sour
Hydronium ions (H3O+)

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134
Q

Acids & Bases:

What does pH stand for?

A

Power of hydrogen

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135
Q 
Acids & Bases:
Self Ionization of water
Equilibrium equation:
[H3O+]=[OH-]= \_\_\_\_
\_\_\_\_ Kw = [\_\_][\_\_]
A

H2O (base) + H2O (acid) <-> H3O+ + OH-
1x10^-7 M
1.00x10-14=[H3O+][OH-]

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136
Q

Acids & Bases:

pH equation

A 
pH = -log [H3O+] or pH = -log[H+]
[H3O+]= 10^-pH or [H+]= 10^-pH
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137
Q

Acids & Bases:

Examples of indicators

A

Phenolphthalein, thymol blue, pH paper, universal indicator

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138
Q

Acids & Bases:

Describes a substance, such as water, that has the properties of an acid and a base

A

Amphoteric

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139
Q

Acids & Bases:

Ionizes completely in a solvent, producing a lot of hydroxide ions

A

Strong bases

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140
Q

Acids & Bases:

pH+pOH=__

A

14

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141
Q

Acids & Bases:

The __ of the two ion concentrations is always equal to __

A

Product

Kw

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142
Q

Acids & Bases:

A substance that donates a proton to another substance

A

Bronsted-Lowry Acids

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143
Q

Acids & Bases:
[H+]> 1x10^-7: ___
[H+]< 1x10^-7: ___

A

Acid

Base

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144
Q

Acids & Bases:

Ionize completely in water, producing a lot of hydronium ions

A

Strong acids

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145
Q

Acids & Bases:

A substance that accepts a proton from another substance

A

Bronsted-Lowry Bases

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146
Q 
Acids & Bases:
Properties of Bases:
1) \_\_
2) \_\_ taste
3) \_\_ to the touch
4) generate \_\_ \_\_ (\_\_) in water
A

Electrolytes
Bitter
Slippery
Hydroxide ions (OH-)

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147
Q

Atomic Theory:
English chemist / physicist / meteorologist:
Many areas of influence:
The behavior of gases, interactions of light & heat, and the behavior of chemicals

A

John Dalton

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148
Q

Atomic Theory:
Discovered negatively charged particles (electrons). Proposed the “plum pudding” model. Postulated positive particles. Did the cathode ray experiment

A

JJ Thomson

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149
Q

Atomic Theory:
Aimed alpha radiation at light elements like boron. Found it gave off an extremely penetrating radiation. Thought it produced high energy gamma rays.

A

Walther Bothe & Herbert Becker

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150
Q

Atomic Theory:
All atoms of a given element must have the same number of ____. In order to be neutral, atoms must have the same number of ___ as ___ (charges must cancel out to 0)

A

Protons
Electrons
Protons

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151
Q

Atomic Theory:

The sum of the protons and neutrons in an atom equals the ___

A

Mass number

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152
Q

Atomic Theory:
Updated atomic model:
Discarded __ __ model
Electrons must orbit around central ____ -> Planetary model
Nearly all of the mass is located in the dense, central, positively charged ____

A

Plum pudding
Nucleus
Nucleus

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153
Q

Atomic Theory:
Positively charged, easily stopped

Negatively charged, stopped by a sheet of aluminum

High energy light (no charge), penetrates a lot of material

A

Alpha radiation
Beta radiation
Gamma radiation

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154
Q

Atomic Theory:
Said matter is composed of indivisible parts. The parts are called atomos. Properties of matter are due to the size, shape, and weight of the atomos. His idea was not popular and was abandoned for over 2000 years.

A

Democritus

155
Q

Atomic Theory:

Average mass of all naturally occurring isotopes. Provides more accurate mass of a typical sample. A weighted average.

A

Atomic mass (weight)

156
Q

Atomic Theory:

____ of an atom is sum of its protons, neutrons, & electrons. Measured in ____.

A

Mass

Daltons

157
Q

Atomic Theory:
Matter can neither be created or destroyed (in a chemical reaction), but only changed from one form to another. Total mass of reactants must equal total mass of products.

A

Law of Conservation of Mass

158
Q

Atomic Theory:
Experiment that discovered the electron. Gas filled tube with metal plates with a positive end (anode) and a negative end (cathode).

A

Cathode ray experiment

159
Q

Atomic Theory:
Said you can continue to split a substance in half until you broke it down into the elements. (Elements could be divided in half indefinitely)

A

Aristotle

160
Q

Atomic Theory:
Continued work of Bothe & Becker: Aimed Bothe’s new beam at paraffin, ejected high energy protons, misinterpreted results.
Died from radiation exposure.

A

Irene Joliot-Curie

161
Q

Atomic Theory:
When two or more different compounds are made up of the same elements, their percent compositions will always be different.

A

Law of Multiple Proportions

162
Q

Atomic Theory:
Shot a beam of particles to a piece of gold foil. Most particles pass straight through foil but some particles are scattered. Showed plum pudding model was incorrect. Created the Rutherford model.

A

Gold foil experiment

163
Q

Atomic Theory:
Did not believe the work of Joliot-Curie (she said beam was light waves). Discovered neutron (no charge, mass slightly more than a proton)

A

James Chadwick

164
Q

Atomic Theory:
Discovered the positively charged dense central portion of the atom (nucleus) using his “gold foil experiment”. Atoms are mostly empty space. Discovered the proton.

A

Ernest Rutherford

165
Q

Atomic Theory:
Danish physicist. Worked on the electron/nucleus problem. Father of Quantum Mechanics. Solution: electrons are located in specific ___ __. Electrons move in a ___ orbit around the nucleus. Areas between orbits are __ ___

A

Niels Bohr
Energy levels
Definite
Not allowed

166
Q

Atomic Theory:
Heavy, positive charge, repelled by the nucleus

Nearly massless, negative charge, repelled by the electrons surrounding an atom

Heavy, no charge, no interactions with nucleus or electrons (can pass through a lot of material, if fast enough can break nucleus apart)

A

Protons
Electrons
Neutrons

167
Q

Atomic Theory:
A compound always contains the same elements in exactly the same proportions by weight. Compounds will always have the exact same percent composition. It is intrinsic (doesn’t matter how much you have, the percentage will always be the same)

A

Law of Definite Proportions

168
Q

Atomic Theory:
Atoms can have more or less ___. ____: atoms with the same # of protons, but different # of neutrons. Isotopes occur in different proportions in nature.

A

Neutrons

Isotopes

169
Q 
Atomic Theory: 
Dalton's Atomic Theory:
1) Matter is composed of \_\_\_
2) All atoms of a given element are \_\_\_ 
3) Properties of different elements are \_\_\_\_\_
4) Atoms combine in \_\_\_\_ \_\_\_\_
5) We cannot \_\_\_ or \_\_\_ atoms
A 
Atoms
Identical
Different
Whole numbers
Create, destroy
170
Q

Atomic Theory:
Explanation that is testable by doing experiments

Observation of something with rules that we follow without explanations

A

Theory

Law

171
Q

Periodic Trends:

Describe the halogens

A 
Group 17 [np^5]
All nonmetals
Gases (F,Cl); liquid (Br); solids (I,At)
Name means "salt former" 
Very toxic!
React with sodium to form a salt with a 1-to-1 ratio
172
Q

Periodic Trends:
Rearranged table according to electronic charge in 1914. Became # of protons after 1918. Noticed his new table had spots for #’s 43, 61, 72 & 75. Produced the modern periodic table we know today.

A

Henry Moseley

173
Q

Periodic Trends:

Describe the lanthanoids

A

1st row on bottom of table [4f^x]
AKA Lanthanides & rare earths
Ce is not so rare (25th most abundant)
So similar that they are very difficult to separate (Moseley)
Most deflect UV- used in sunglasses
Shiny, silvery white, soft, react violently with most nonmetals, tarnish in air

174
Q

Periodic Trends:

The higher the electronegativity, the ____ the atoms ____ for electrons

A

Harder

Pull

175
Q

Periodic Trends:
What two elements are usually found as 8 atoms?
What element is usually found as 4 atoms?

A

Sulfur and Selenium

Phosphorus

176
Q

Periodic Trends:

Measure of how badly an element wants to gain an electron

A

Electronegativity

177
Q

Periodic Trends:
What element has the highest electronegativity?
What element has the lowest electronegativity?

A

Fluorine

Francium

178
Q

Periodic Trends:

A horizontal row of elements in the periodic table. Have the same # of occupied ___ ___. ___ similar at all.

A

Period
Energy levels
Not

179
Q

Periodic Trends:
Electronegativity ____ from left to right
Electronegativity ____ from top to bottom

A

Increases

Decreases

180
Q

Periodic Trends:

The amount of energy required to remove an electron

A

Ionization energy

181
Q

Periodic Trends:

What are the 4 groups of representative elements?

A

Alkali Metals (Group 1)
Alkaline Earth Metals (Group 2)
Halogens (Group 17)
Noble Gases (Group 18)

182
Q

Periodic Trends:

Describe the noble gases

A

Group 18 [np^6]
Un reactive gases- colorless & odorless
Some of the last natural elements to be discovered
Once called “inert gases”
Monatomic in nature (1 atom)
Don’t combine with other atoms because their outer p-orbital are full

183
Q

Periodic Trends:
When 2 atoms have the same number of electrons but a different amount of protons, the one with ___ protons will pull the electrons in tighter and make the atom ____

A

More

Smaller

184
Q

Periodic Trends:

What are some common salts of alkali metals?

A 
LiCl
NaCl
KCl
RbCl
CsCl
FrCl
185
Q

Periodic Trends:

A vertical column is called a ___ or ____. Have ____ properties

A

Group
Family
Similar

186
Q

Periodic Trends:

What are the 4 trends in the periodic table?

A

Atomic Radius
Electronegativity
Ionization Energy
Reactivity

187
Q

Periodic Trends:
The atomic radius ______ from left to right
The atomic radius _____ from top to bottom

A

Decreases

Increases

188
Q

Periodic Trends:
Most reactive metals are ____ ___ and to the ____
Most reactive nonmetals are ____ ___ and to the ____

A

Further down
Left
Higher up
Right

189
Q

Periodic Trends:
What element has the highest ionization energy?
What element has the lowest ionization energy?

A

Fluorine

Francium

190
Q

Periodic Trends:
Atoms in their _____ ____ tend to be more dangerous/poisonous than those in their ____ ____
(Exceptions: __ & __)

A

Elemental state
Reacted state
Cu & Pb

191
Q

Periodic Trends:
Typically placed in its own category. Most of the time, behaves like a nonmetal. Under certain circumstances, can behave like a metal.

A

Hydrogen

192
Q

Periodic Trends:

What are the groups that are non-representatives?

A

Groups 13-16 (Boron, Carbon, Nitrogen, Oxygen): have more differences than similarities
Transition metals
Lanthanoids
Actinoids

193
Q

Periodic Trends:

What are properties of metals?

A

Lustrous (shiny); malleable (pounded into thin sheets); ductile (pulled into wires); conductive (heat & electricity); form solid oxides when burned; tend to react with acids to form hydrogen gas

194
Q

Periodic Trends:

What are some common salts of alkali earth metals?

A 
BeCl,2
MgCl,2
CaCl,2
SrCl,2
BaCl,2
RaCl,2
195
Q

Periodic Trends:

Exhibit nearly perfect periodicity. All members of these groups behave as expected.

A

Representative elements

196
Q

Periodic Trends:

What were some problems with Mendeleev’s table?

A

Based on atomic mass, had to switch a few elements (tellurium & iodine) to keep reactivities in order.
Believed he predicted too many elements.
Used it for half a century

197
Q

Periodic Trends:

Describe the alkaline earth metals

A

Group 2 [ns^2]
Harder & denser then alkali metals
Lustrous, oxidize slowly when exposed to air
React with water or steam to form a base
React with chlorine to form a salt with 1-to-2 ratio

198
Q

Periodic Trends:

How is the modern periodic table set up?

A

A chart of the elements showing the repeating pattern of their properties. Elements are arranged in rows and columns by increasing atomic #. Atomic # increases by 1 between each element.

199
Q

Periodic Trends:
Arranged known elements in a table by atomic mass in 1863. Noticed a repeating pattern every 8th element in 1865. Was laughed at by peers.

A

John Newlands

200
Q

Periodic Trends:

What are some common salts of halogens?

A 
NaF
NaCl
NaBr
NaI
NaAt
201
Q

Periodic Trends:

Describe the transition metals

A 
Groups 3 to 12 [nd^x]
Central portion of periodic table
Behavior & appearance vary
Have a variable oxidation state (charge)
Different oxidation states that can produce different colors
Often used to make pigments
202
Q

Periodic Trends:
_______ is by far most abundant
(4 out of every 5 atoms in the universe)

A

Hydrogen

203
Q

Periodic Trends:

What are properties of nonmetals?

A

Tend to be:
Dull; brittle (when solid); insulators; form gaseous oxides; don’t react much with acids; have lower melting & boiling points (than metals)

204
Q

Periodic Trends:

Describe metalloids

A

AKA: “semi-metals” or “staircase elements”
Combination of properties of metals & nonmetals.
Boron, silicon, germanium, arsenic, antimony, tellurium, & polonium

205
Q

Periodic Trends:

What did Moseley’s new periodic table do?

A

Gave experimental meaning to atomic #. Gave reason for tellurium & iodine being switched. Easily separated rare earth metals. Used to predict how many elements remained between others.

206
Q

Periodic Trends:
7 elements always form _____ molecules when they are isolated in their elemental state (ALWAYS!).
Means two atoms
Two atoms of the same element bond together.
5 gases, 1 liquid, & 1 solid.

A

Diatomics

207
Q

Periodic Trends:

Why does the atomic radius increase from top to bottom? Why does the atomic radius decrease from left to right?

A

More energy levels to fill

More charge, attraction pulls them in tighter

208
Q

Periodic Trends:

What are the names of all groups/families?

A 
Alkali metals
Alkaline earth metals
Halogens
Nobles gases
Transition metals
Inner transition metals- lanthanoids (rare earths), Actinoids
209
Q

Periodic Trends:

Atoms are less dangerous as ___

A

Ions

210
Q

Periodic Trends:
Produced a more orderly table independent of Newlands’ work in 1869. Also used atomic mass. Left blanks for yet-undiscovered elements. Predicted properties of Ga, Sc, and Ge which were discovered in 1875,77, & 86. Credited with developing the periodic table.

A

Dmitri Mendeleev

211
Q

Periodic Trends:

Describe the Alkali metals

A

Group 1 [ns^1]
Soft, lustrous, oxidize when exposed to air
Difficult to isolate- never found in nature
React (violently) with water to form a base
React with chlorine to form a salt with a 1-to-1 ratio

212
Q

Periodic Trends:

Other families have similarities, but do not behave exactly as expected. Some lumped together for other reasons.

A

Non-representatives

213
Q

Periodic Trends:

Chemical properties repeat every 8 elements

A

Law of Octaves

214
Q

Periodic Trends:
When an atom changes to a(n):
Anion- it gets _____
Cation- it gets _____

A

Bigger

Smaller

215
Q

Periodic Trends:
Which element has the largest atomic radius?
Which element has the smallest atomic radius?

A

Francium

Hydrogen or Helium

216
Q

Periodic Trends:
Ionization energy _____ from left to right
Ionization energy _____ from top to bottom

A

Increases

Decreases

217
Q

Periodic Trends:
Elements are found on different parts of the periodic table:
____ to the left (majority of elements)
____ to the right (18 elements)
____ found on a “staircase” dividing metals & nonmetals (7 elements)
____&____(metals) added to bottom to make table manageable

A

Metals
Nonmetals
Metalloids
Lanthanoids & Actinoids

218
Q

Periodic Trends:
The reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons

A

Electron shielding

219
Q

Periodic Trends:

Describe the Actinoids

A 
2nd row on bottom of table [5f^x]
AKA Actinides
All are radioactive
Not as similar as the lanthanoids
Only Th and U are common in nature
Most are man-made
Nuclear fallout
Particle colliders
220
Q

Periodic Trends:

What are the 7 diatomic elements?

A 
Hydrogen
Oxygen
Fluorine
Bromine
Iodine
Nitrogen
Chlorine
221
Q 
Quantum Mechanics:
s orbitals: \_\_\_\_, larger n = bigger \_\_\_
p orbitals: \_\_\_ \_\_\_, larger n = bigger \_\_\_\_
d orbitals: only possible when n>_
f orbitals: only possible when n>_
A 
Spherical
Sphere
Dumbbell shape
Dumbbell
2
3
222
Q

Quantum Mechanics:
4 quantum numbers (specify location of electrons in atom):
1) n (principle) = ___ ___ (n>0). Lower the #, closer to the nucleus
2) l (azimuthal) = ___ ___. __ are abbreviated s, p, d, f
3) m = _____ ____. s=1, p=3, d=5, f=7
4) m(s) = ____. Opposite directions

A

Energy level
Orbital shape, Shapes
Suborbital orientation
Spin

223
Q

Quantum Mechanics:
The Dreaded Double Slit:
When light passes through 2 narrow slits, it creates interference patterns just like ___ on a pond. We see the same interference patterns when we shoot ___ at a double slit. Electrons are ___ & __.

A

Waves
Electrons
Particles
Waves

224
Q

Quantum Mechanics:

Add one electron in each suborbital before pairing up

A

Hund’s Rule

225
Q

Quantum Mechanics:
A measure of how often a wave passes a point. Waves per second = ____ (Hz)
Means “per second”

A

Frequency

Hertz

226
Q

Quantum Mechanics:

J: ___, unit for energy

A

Joules

227
Q

Quantum Mechanics:

Performed the double slit experiment & proved light existed as a wave.

A

Thomas Young

228
Q

Quantum Mechanics:

Particle of light

A

Photon

229
Q

Quantum Mechanics:
Research with black-body radiation led to the idea that energy is quantized. Energy of an oscillator is strictly proportional to its frequency. As frequency increases, energy of photon (quanta) increases and vise versa.

A

Max Planck

230
Q

Quantum Mechanics:

___ is constant (c)

A

Speed of light

231
Q

Quantum Mechanics:
The more you know about the position of a particle, the less you know about its momentum (speed and direction) and vice versa. The act of measuring causes an inherent ____ in the universe!

A

Heisenberg’s Uncertainty Principle

Uncertainty

232
Q

Quantum Mechanics:
Electrons fill orbitals with the ____ energy first. s can have _ electrons. p can have _ electrons. d can have _ electrons. f can have _ electrons. Electron orbital diagrams created by drawing a box for each orbital. Put electrons in one-by-one, obeying ____ ___

A 
Lowest
2
6
10
14
Hund's Rule
233
Q

Quantum Mechanics:
No 2 electrons can have the same 4 quantum numbers. Electrons cannot stack up on each other. If an orbital is full, the next electron must go to a higher orbital. This is what makes matter solid. Each electron must have a different set of quantum #’s.

A

Pauli Exclusion Principle

234
Q

Quantum Mechanics:

Louis de Broglie tells us why we have specific orbits. Only standing waves can exist within a ___

A

Space

235
Q

Quantum Mechanics:
Shorter wavelengths have ___ energies and frequency
Longer wavelengths have ___ energies and frequency

A

Higher

Lower

236
Q

Quantum Mechanics:
Take a cat. Put it in a box with a device that may or may not kill it. Is the cat dead or alive? It is both! The cat exists in a “superposition” (a state between dead and alive) until you check, then the wave function collapses and the cat is dead or alive (but not both). The idea has been proven.

A

Schrodinger’s Cat

237
Q

Quantum Mechanics:
Neils Bohr proposed:
Electrons are limited to ___ ___ around the nucleus
Electrons become ___ (absorb energy) and “jump” to a ___ ____

A

Specific orbits
Excited
Higher orbital

238
Q 
Quantum Mechanics:
\_\_\_ are in orbitals. Orbitals differ in: 
1)
2)
3)
Electrons have \_\_\_
A 
Electrons
Size
Shape
Orientation
Spins
239
Q

Quantum Mechanics:
Described light via the corpuscular theory: Light is composed of tiny, discreet packets called “corpuscles”. More influential, so his theory won out.

A

Sir Isaac Newton

240
Q

Quantum Mechanics:

Since different wavelengths are emitted, we can calculate the difference in ___ between ___

A

Energy

Orbitals

241
Q

Quantum Mechanics:

Described light using a wave theory. Light propagates through space just like ripples on a pond.

A

Christiaan Hyugens

242
Q

Quantum Mechanics:
___ & ___ are inversely related. When one increases, the other must decrease. Waves with __ wavelengths have __ frequencies.
Waves with __ wavelengths have __ frequencies

A

Wavelength & frequency
Long, low
Short, high

243
Q

Quantum Mechanics:

Heisenberg killed _____ & Schrodinger’s wave equation brought in probabilities. There are no absolute answers, only ___

A

Determinism

Probabilities

244
Q

Quantum Mechanics:
Albert Einstein proved light acts as a particle (photon). Light was already proven as a wave. Light behaves like a wave and a particle at the same time. Depends on how/what you are measuring

A

Wave-Particle Duality

245
Q

Quantum Mechanics:
Height of a wave:
Highest point of a wave:
Lowest point of a wave:

A

Amplitude
Peak
Trough

246
Q

Quantum Mechanics:

Distance between identical sections on a wave. Measured in meters

A

Wavelength

247
Q

Quantum Mechanics:
Photons of different wavelengths have different ___. Calculate energy using E= hv
h= ____ ____ : 6.626 x 10^-34 J•s

A

Energies

Planck’s constant

248
Q 
Quantum Mechanics:
s orbitals: _ possibility
p orbitals: _ possibilities
d orbitals: _ possibilities
f orbitals: _ possibilities
A

1
3
5
7

249
Q

Quantum Mechanics:

Atoms are “built up”. Add a proton to the nucleus. Add an electron to the lowest possible orbital.

A

Aufbau Principle

250
Q

Quantum Mechanics:
Unsatisfied with Heisenberg’s mathematical picture, came up with a wave-like model. All matter can be described as a wave function. All positions are equally possible, but not all positions are equally probable

A

Erwin Schrodinger

251
Q

Quantum Mechanics:
All electromagnetic waves travel at the same ___ in a vacuum (space).
Speed of light = c = ___ x 10* m/s
Usually rounded to __ x 10* m/s

A

Wave speed
Speed
2.998
3.0

252
Q

Quantum Mechanics:
When gaseous atoms/molecules are heated, they emit ___. __ is specific to each substance. Spectral analysis shows discrete ___

A

Light
Color
Lines

253
Q

Quantum Mechanics:
According to his wave equation, all possible outcomes exist at one time until you ___ it! The act of ____ causes one (and only one) result to “pop” into existence.

A

Measure

Measuring

254
Q

Quantum Mechanics:
Bohr’s Model:
Electrons only permitted in ___ orbits. The __ state is the open orbit closest to nucleus (lowest available energy). The __ state is an orbit farther away from nucleus (it has higher energy). ___ __ # (n) is given to determine orbit. Small n means a small ___ (closer to nucleus). n>0

A 
Circular
Ground
Excited
Principal Quantum
Radius
255
Q

Quantum Mechanics:
A rhythmic disturbance that carries energy through matter or space. Travels at a constant speed through a medium. Can change speed if the medium changes. Speed is product of ____ & _____

A

Waves
Wavelengths
Frequency

256
Q

Quantum Mechanics:

Said if light can behave as both a wave and a particle, then it reasons that things like electrons can as well

A

Louis de Broglie

257
Q

Quantum Mechanics:
One consequence of the uncertainty principle is that the electron could no longer be considered as in an ___ location in its orbital. The electron has to be described by every point where the electron could possibly ____

A

Exact

Inhabit

258
Q

Quantum Mechanics:
Occurs when electrons absorb energy and jump to a higher energy level and when electrons lose energy and fall back down to a lower orbital. When electrons lose energy, the emit a photon of light.

A

Light emission

259
Q 
Quantum Mechanics:
3 properties of waves:
1) \_\_\_ \_\_\_: when 2 waves come in contact with each other. Can be either: a) \_\_\_\_: waves amplitudes combine and doubles. b) \_\_\_\_: waves cancel out
2) \_\_\_\_: spreading out beyond a barrier
3) \_\_\_\_: bending of light
A 
Wave interference
Constructive
Destructive
Defraction
Refraction
260
Q

Bonding:

___ form when atoms attempt to fill their outer s & p orbitals to be ______ with the noble gases

A

Ions

Isoelectronic

261
Q

Bonding:

Atoms with ____ electronegativity will share electrons

A

Similar

262
Q

Bonding:
Ions are ___ ___ & have the same configuration as a ___ ___, but ions have a ____ and ____ ____ when dissolved in ____, unlike the ____ ____

A 
More stable
Noble gas
Charge
Conduct electricity
Water
Noble gases
263
Q

Bonding:
Form from metals
Can be ___ metals or ___

A

Metallic substance
Pure
Alloy

264
Q

Bonding:
Aluminum tends to form ions with a ____ charge
Zinc tends to form ions with a ____ charge
Silver tends to form ions with a ____ charge

A

+3
+2
+1

265
Q

Bonding:

Prefixes 1-10

A

1) mono
2) di
3) tri
4) tetra
5) penta
6) hexa
7) hepta
8) octo
9) nona
10) deca

266
Q

Bonding:

Bonds form between atoms due to the interactions of _____

A

Electrons

267
Q

Bonding:

Properties of ions are _____ ____ from their neutral counterpart

A

Completely different

268
Q

Bonding:
Form between a nonmetal and another nonmetal
Share electrons

A

Covalent compound

269
Q

Bonding:
Electrons closest to the nucleus
Unable to participate in bonding
Shielded by electrons farther away

A

Core electrons

270
Q

Bonding:

Properties are dictated by the ___ & ___ of an element’s ___

A

Number
Configuration
Electrons

271
Q

Bonding:

Atoms will attempt to gain or lose electrons to have 8 electrons in their outer s & p orbitals

A

Octet Rule

272
Q

Bonding:
Ions made up of more than 1 atom
In ______ ions, ____ ___ form between atoms within the ion
Electrons have been ___ or ____ during formation

A 
Polyatomic
Polyatomic
Covalent bonds
Gained
Lost
273
Q 
Bonding: 
Metallic substances:
Usually \_\_\_, but a few \_\_\_\_ at or near room temperature
Will not dissolve in \_\_\_ or \_\_\_
All metals \_\_\_ \_\_\_ at least a little bit
A

Solid, liquids
Water, oil
Conduct electricity

274
Q

Bonding:

Roman numerals 1-10

A 
I
II
III
IV
V
VI
VII
VIII
IX
X
275
Q

Bonding:

Few bonds are strictly ___ or ____

A

Ionic

Covalent

276
Q

Bonding:

All compounds are neutral, so the total charge must add up to _

A

0

277
Q

Bonding:
& block elements almost always obey the octet rule
& block elements do not always follow the octet rule

A

s p

d f

278
Q 
Bonding: 
All ionic compounds are called \_\_\_
They have \_\_\_ \_\_\_ melting points
All are \_\_\_ at room temperature
Will \_\_\_ in water (if they \_\_\_\_)
A 
Salts
Very high
Solid
Dissociate
Dissolve
279
Q

Bonding:
When writing formulas containing polyatomic ions, it is important to remember that the _____ are part of the polyatomic ion

A

Subscripts

280
Q

Bonding:
Ions made up of single atoms
Ex: Mg^+2, Br^-1

A

Monatomic ions

281
Q

Bonding:

When the outer s & p orbitals are full, the atom is very _____

A

Stable

282
Q

Bonding:
Electrons farthest from the nucleus
Determine the chemical reactivity of the atom

A

Valence electrons

283
Q

Bonding:

This means you must have an equal # of _ & _ charges

A

+

-

284
Q

Bonding:
Anions are named by dropping the ___ ____ of the element and adding “-__”
Chlorine becomes ___
Oxygen becomes ____

A

Final syllable
-ide
Chloride
Oxide

285
Q

Bonding:
Change ending of the second element to “-ide”
Use prefixes to indicate the # of atoms each element present

A

Rules for naming covalent compounds

286
Q

Bonding:

The unequal sharing of electrons within a bond leads to the formation of an ___ ____

A

Electric dipole

287
Q

Bonding:
Cations form when atoms ____ electrons, leaving more ____ than ____
All ___ form cations

A

Lose
Protons
Electrons
Metals

288
Q 
Bonding: 
Ionic compounds:
Will not dissolve in \_\_
Do not consist of \_\_\_\_\_
\_\_\_\_\_ structure
As a solid, are \_\_\_\_\_\_
When molten (liquid) & aqueous, they are \_\_\_\_ \_\_\_
A 
Oil
Molecules
Crystalline
Insulators
Good conductors
289
Q

Bonding:

Elements with __ electronegativity will pull electrons away from those with __ electronegativity

A

High

Low

290
Q

Bonding:

Cation and anion get pulled apart

A

Dissociate

291
Q 
Bonding: 
Tend to form ions with what charge:
Group 1:
Group 2:
Group 15:
Group 16:
Group 17:
A 
\+1
\+2
-3
-2
-1
292
Q

Bonding:

The ___ of covalent compounds tell you how many ____ you have of each element

A

Prefixes

Atoms

293
Q

Bonding:

A positively charged ion

A

Cation

294
Q

Bonding:

If you have more than 1 polyatomic ion, you must put the _____ outside of ______

A

Subscript

Parentheses

295
Q

Bonding:
Forms when 2 or more ions combine
Repeating pattern of ions
Transfer electrons

A

Ionic compound

296
Q

Bonding:

A separation of positive and negative charge

A

Dipole

297
Q

Bonding:

Since d&f block elements have lots of orbitals with nearly overlapping energies, many form ions with more than one _____

A

Charge

298
Q

Bonding:

The difference in electronegativity between bonding atoms

A

Ionic character

299
Q 
Bonding:
If binary (2 elements): "ide"-> hydro-----ic acid
If tertiary (polyatomic ion): "ates" -> -----ic acid. "ites"-> ------ous acid
A

Rules for naming acids

300
Q

Bonding:
If first element is a metal it’s _____
If first element is a nonmetal, its ____
If first element is hydrogen, its ____

A

Ionic
Covalent
Acid

301
Q

Bonding:
Related to polarity
The greater the difference in _____, the greater the ___ ____
Ionic > Polar covalent > non polar covalent

A

Bond strength
Electronegativity
Bond strength

302
Q

Bonding:
____ bonds form when electrons are transferred from 1 atom to another
____ bonds form when electrons are shared between 2 atoms
____ bonds form when electrons between atoms are delocalized and are free to move around in an electron sea (this is what permits electrical conductivity)

A

Ionic
Covalent
Metallic

303
Q

Bonding:
Since an s-orbital can hold _ electrons and a p-orbital can hold _, atoms are stable when they have _ electrons in their valence shell

A

2
6
8

304
Q

Bonding:
Anions form when atoms ___ electrons, leaving more ____ than ____
Most ____ will form anions

A

Gain
Electrons
Protons
Nonmetals

305
Q

Bonding:
____ have no special name
Na+ is the _____ ___

A

Cations

Sodium ion

306
Q

Bonding:

Are nonreactive because they have full s & p orbitals

A

Noble gases

307
Q 
Bonding:
There are 3 categories of bond types:
1)\_\_\_\_: NaCl
2)\_\_\_\_: O2
3)\_\_\_\_: Al, Ca, Fe
A

Ionic
Covalent
Metallic

308
Q

Bonding:
The ____ ion
Carbon has _ valence electrons and Nitrogen has _
A ____ bond forms between C & N sharing _ electrons each
Carbon ___ an extra electron
The whole molecule acquires a ___ charge

A 
Cyanide
4, 5
Covalent
3
Steals
Negative
309
Q

Bonding:

A negatively charged ion

A

Anion

310
Q

Bonding:

Orbitals are stabilized when they are completely __, completely ___, or to a lesser extent, ______

A

Full
Empty
Half-full

311
Q

Bonding:
Covalent compounds:
Have __ melting points
Can be ____, ____, or ____ at room temperature
They may dissolve in ___ or ___, but usually not both
Will not ____ in water
Will not ____ ____ (few exceptions)

A 
Low
Solid, liquid, gas
Water, oil
Dissociate
Conduct electricity
312
Q

Bonding:
Ionic Character:
If the difference is less than or equal to 0.4, bond is _____.
Electrons are ____ ____.
If the difference is greater than 0.4 and less than or equal to 1.6, bond is ____ ____.
Electrons are ____ ___.
If the difference is greater than 2, bond is ___.
Electrons are ____.

A 
Covalent
Equally shared
Polar covalent
Unequally shared
Ionic
Transferred
313
Q

Bonding:
Name cation, then the anion
If cation charge fixed, use name from periodic table
If cation charge isn’t fixed, use Roman numeral in parenthesis to specify charge of cation
If anion is single element, drop last syllable and add “-ide”
If anion is a polyatomic ion, use that name

A

Rules for naming ionic compounds

314
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 6
Unshared: 0

A

sp^3d^2

Octahedral

315
Q 
Molecular shapes:
To determine the direction of the dipole moment:
1) 
2) 
3)
A

1) determine the types of bonds within the molecule
2) draw individual bond dipoles for polar bonds
3) check for molecular symmetry

316
Q

Molecular shapes:
In order for a molecule to be polar, it must:
1)
2)

A

1) Have polar bonds

2) Be asymmetrical

317
Q

Molecular shapes:

Unequal forces between bonds, polar

A

Asymmetrical

318
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 3
Unshared: 0

A

sp^2

Trigonal Planar

319
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 2
Unshared: 0

A

sp

Linear

320
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 2
Unshared: 3

A

sp^3d

Linear

321
Q

Molecular shapes:

1) If H is having FON, what IMFAs does the molecule have?
2) If H is not having FON, what IMFAs does the molecule have?

A

1) hydrogen bonding, dipole-dipole, LDFs

2) dipole-dipole, LDFs

322
Q

Molecular shapes:

What are the 5 IMFAs?

A

1) Ion-ion
2) Ion-dipole
3) Hydrogen bonding
4) Dipole-dipole
5) London Dispersion Forces (LDFs)
(Only 3, 4, & 5 on quiz)

323
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 2
Unshared: 2

A

sp^3

Bent

324
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 4
Unshared: 2

A

sp^3d^2

Square Planar

325
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 2
Unshared: 1

A

sp^2

Bent

326
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 5
Unshared: 0

A

sp^3d

Trigonal Bipyramid

327
Q

Molecular shapes:

What IMFA do all molecules have?

A

London dispersion forces

328
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 3
Unshared: 2

A

sp^3d

T-shaped

329
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 4
Unshared: 1

A

sp^3d

See-saw

330
Q

Molecular shapes:

Equal forces from all sides, nonpolar

A

Symmetrical

331
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 5
Unshared: 1

A

sp^3d^2

Square Pyramid

332
Q

Molecular shapes:
What shapes are always non polar because they are symmetrical?
(Only when central atom is surrounded by the same elements)
(Put shared and unshared and shape)

A 
2,0: linear
3,0: trigonal planar
4,0: tetrahedral
5,0: trigonal Bipyramid
6,0: octahedral
2,3: linear
4,2: square planar
333
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 3
Unshared: 1

A

sp^3

Trigonal pyramid

334
Q

Molecular shapes:

In a polar bond, the higher electronegative element is slightly ____ and the other is _____

A

Negative

Positive

335
Q

Molecular shapes:
Electron pairs on central atom:
Shared: 4
Unshared: 0

A

sp^3

Tetrahedral

336
Q

Uncertainty in Measurement:

Use ___ ___ to eliminate all placeholding zeroes

A

Scientific notation

337
Q

Uncertainty in Measurement:
When a number is in scientific notation, the number being multiplied by 10* has all ____ ____
Ex: 2.590 x 10^4 has _ sig figs

A

Significant figures

4

338
Q 
Uncertainty in Measurement:
Sig fig rules do not apply when:
1) not \_\_\_\_\_ something
2) \_\_\_\_\_ something
3) have a defined \_\_\_\_ or \_\_\_\_
A

Measuring
Counting
Values
Counts

339
Q

Uncertainty in Measurement:
Even odd rule: if a number ends in exactly .5, look at the number in front of it. If the number in front is even, round ___. If the number in front is odd, round ___.

A

Down

Up

340
Q

Uncertainty in Measurement:

How closely several measurements agree

A

Precision

341
Q

Uncertainty in Measurement:
Rules for multiplying/dividing sig figs:
The answer cannot have more sig figs than there are in the measurement with the ___ number of sig figs

A

Least

342
Q

Uncertainty in Measurement:

How close a measurement is to the true value

A

Accuracy

343
Q

Uncertainty in Measurement:
To identify how many sig figs are in a measurement, follow these rules:
1) All _____ digits are significant
2) All ___ between nonzero digits are always significant
3) ___ in front of nonzero digits are never significant
4) ____ after all nonzero digits are only significant if a ___ __ is present anywhere in the number

A

Nonzero
Zeroes
Zeroes
Zeroes, decimal point

344
Q

Uncertainty in Measurement:
Rules for adding/subtracting sig figs:
The answer cannot have more __ to the __ of the decimal point than there are in the measurement with the ____ number of ___ to the right of the decimal point

A

Digits
Right
Smallest
Digits

345
Q

Uncertainty in Measurement:
Measurements are made __ place beyond where the measuring device is marked. Includes all certain digits and _ estimated digit

A

1

1

346
Q

The Mole:
Formula that shows the composition of a compound in terms of relative number and kinds of atoms in the simplest, whole number ratio

A

Empirical formula

347
Q

The Mole:

Masses of _ are so small that expressing them in terms of _ is not convenient

A

Atoms

Grams

348
Q

The Mole:

Mass in grams of 1 mole of an element. The unit is /. It is numerically equivalent to the __ __ of an element

A

Molar mass
Grams/mole (g/mol)
Atomic mass

349
Q

The Mole:

1 mole of a substance = ___ x __^__ particles

A

6.02x10^23

350
Q

The Mole:

Mole: Number of atoms in exactly _ grams of __-__. It is the SI base unit for _.

A

12
Carbon-12
Quantity

351
Q

The Mole:

To convert between moles and mass, we use the __ __

A

Molar mass

352
Q

The Mole:

Percentage by mass of each element in a compound. Helps verify a substance’s identity

A

Percent composition

353
Q

The Mole:

The actual formula of a single molecule of a compound. Sometimes can be same as empirical formula

A

Molecular formula

354
Q

The Mole:

The number of particles present in 1 mole of a substance is called ___ ___

A

Avogadro’s number

355
Q

Chemical Equations:
Molecules that act to lower the activation energy of a reaction. Are not consumed by the reaction, but play a role in enabling the reaction to proceed with __ energy requirements

A

Catalysts

Lower

356
Q

Chemical Equations:

Change in __ is always a physical change. For proof, you need a __ __ to show at least one new substance has formed

A

State

Chemical analysis

357
Q

Chemical Equations:

A measure of the amount of molecules per set volume

A

Concentration

358
Q

Chemical Equations:

Compound is completely oxidized and broken up by oxygen (w/ flame). CO2 & H2O are always the products

A

Combustion (or burning)

359
Q

Chemical Equations:

Direct combination of elements to produce a compound. Single product

A

Synthesis (or combination) reaction

360
Q

Chemical Equations:

__ reactions absorb energy, so are only spontaneous if the ___ is higher than the ___ ___

A

Endothermic
Temperature
Activation energy

361
Q

Chemical Equations:

Substances created

A

Products

362
Q

Chemical Equations:

Process by which one or more substances change to produce one or more different substances

A

Chemical reactions

363
Q

Chemical Equations:

Compounds break down into constituent elements and/or smaller molecules. 1 reactant

A

Decomposition (or analysis) reaction

364
Q

Chemical Equations:

The higher the ___ the faster the reaction

A

Concentration

365
Q

Chemical Equations:
In order for a reaction to occur the reactants must:
1) ____
2) have enough __ __
3) have the correct ___ when they collide
4) form ____ favorable products

A

Collide
Activation energy
Orientation
Energetically

366
Q

Chemical Equations:

Amount of energy needed to initiate a reaction. Without enough __, molecules that react very violently will __ __ at all

A

Activation energy
Energy
Not react

367
Q

Chemical Equations:

Original substances

A

Reactants

368
Q

Chemical Equations:

The more __ present in a confined space, the greater the chance they will __

A

Molecules

Collide

369
Q

Chemical Equations:

Takes a long time for molecules in the _ of “chunk” to contact other reactant (have _ surface area)

A

Center

Low

370
Q

Chemical Equations:

To speed up reaction, break __ pieces into __ pieces with high surface areas

A

Big

Smaller

371
Q

Chemical Equations:

Balance equations by inserting __ in front of the compounds

A

Coefficients

372
Q

Chemical Equations:

An ion from one compound switches places with similarly charged ion from another compound

A

Double replacement (or displacement)

373
Q

Chemical Equations:

For a reaction that proceeds at room temperature, ___ the temperature will speed up the reaction. There are exceptions

A

Increasing

374
Q

Chemical Equations:

Once started, ___ reactions often produce enough energy to maintain a ___ reaction

A

Exothermic

Spontaneous

375
Q

Chemical Equations:

An element will replace a similar element in a compound

A

Single Replacement (or displacement)

376
Q

Chemical Equations:
A representation of a chemical reaction that uses symbols to show the relationship between the reactants and the products

A

Chemical equations

377
Q

Chemical Equations:
Reactions that occur spontaneously at room temperature have __ activation energies. Reactions that require high temperatures have __ __ activation energies

A

Low

Very high

378
Q 
Chemical Equations:
Evidence of a reaction
1)
2)
3)
4)
5)
A

1) changes in energy
2) formation of a gas
3) formation of a precipitate
4) change in color
5) odor

379
Q

Chemical Equations:

Affects the number of molecules that have the correct activation energy for the reaction

A

Temperature

380
Q

Chemical Equations:

How to write net ionic equations:

A

1) Write all the compounds that are soluble as ions (put charges)
2) cross out any spectator ions that are on both the left and right side

381
Q 
Chemical Equations:
Physical state of substances
(s):
(l): 
(g):
(aq):
A

(s) : solid
(l) : liquid
(g) : gas
(aq) : aqueous solution (dissolved in water)

382
Q

Chemical Equations:

What drives a reaction?

A

Makes a gas (which escapes)
Makes a solid (which precipitates)
Makes water
Changes oxidation state (charge)

383
Q

Chemical Equations:

A measure of the ratio of the amount of surface to volume of a substance

A

Surface area

384
Q

Chemical Equations:
Triangle over arrow indicates __ added to the reaction.
Double arrow indicates an ____ reaction
A substance’s name over the arrow indicates the use of a ___

A

Heat
Equilibrium
Catalyst

385
Q

Chemical Equations:
Strong acids and strong bases combine to form water and a salt. Acids: have an _ in front
Bases: usually __

A

Neutralization (or acid-base) reaction
H
OH

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