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Chemistry > Regents > Flashcards

Regents Flashcards

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0
Q

Temperature

A

Average kinetic energy

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1
Q

Amount of energy required to steal the outermost electron

A

Ionization energy

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2
Q

Particles of an ideal gas are separated by great distances, compared to their size

A

Kinetic molecular theory

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3
Q

What happens when a bond is broken

A

Energy is absorbed

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4
Q

What happens when a bond is formed

A

Energy is released

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5
Q

What does a catalyst do

A

Creates an alternate pathway, increasing the rate of the reaction by lowering the activation energy

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6
Q

Where does oxidation and reduction occur?

A

Oxidation-anode

Reduction-cathode

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7
Q

Same molecular formula but different structural formula

A

Isomer

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8
Q

Amount of attraction for electrons in a chemical bond

A

Electronegativity F or closest to fluorine

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9
Q

Difference between potential energy of the products and potential energy of the reactants

A

Heat of the reaction

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10
Q

Atoms that bond with each other to form chains, rings, or networks

A

Carbon atoms

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11
Q

Electrical energy to chemical energy

A

Electrolytic cell

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12
Q

MaVa=MbVb

A

Titration

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13
Q

Dense (+) charged in the center of empty space (protons & neutrons)

A

The nucleus

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14
Q

Mass of protons, neutrons, and electrons…

A

Protons: 1.0073amu. +
Neutrons: 1.0087amu. 0
Electrons: 0.0005amu. -

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15
Q

Atoms with the same number of protons but different number of neutrons

A

Isotope

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16
Q

Weighted average of all isotopes

A

Average atomic mass

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17
Q

A nucleus that is unstable

A

Radioactive

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18
Q

What determined the stability of a nucleus

A

The number of neutrons vs the number of protons

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19
Q

Change in the identity (#P) In a nucleus

A

Transmutation

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20
Q

If unstable nucleus undergoes a…

A

Transmutation to become stable

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21
Q

For nuclei with more than 83 protons

A

Alpha decay

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22
Q

For nuclei with too many neutrons

A

Beta decay

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23
Q

For nuclei with too many protons

A

Positron

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24
Q

The time required for half of a radioactive sample to become stable

A

Half life

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25
Q

A large nucleus breaks releasing energy

A

Fission Nuclear power

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26
Q

2 small nuclei fuse together release tons of energy

A

Fusion Sun/bomb

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27
Q

Isotopes with short half lives used to treat and protect health problems
( 131-I: thyroid disorders)
( 60-Co: finding and fighting cancer)

A

Medical tracers

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28
Q

Determines the age of fossils
( 238-U: date the earth)
( 14-C: dates organic fossils)

A

Radioactive dating

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29
Q

Fission, fission, atomic bomb, radiation

Matter converted to energy

A

Artificial transmutation

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30
Q

How do you determine the charge of an atom?

A

Number of protons - number of electrons

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31
Q

p>#e

1P
0e
Charge=1+

A

Cation

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32
Q

p=#e

1p
1e
Charge=0

A

Neutral atom

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33
Q

p<#e

1p
2e
Charge=1-

A

Anion

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34
Q

Atoms with a charge due to more or less electrons

A

Ion

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35
Q

What are the energy levels in a Bohr model

A

1st=2 electrons
2nd=8 electrons
3rd=18 electrons
4th=32 electrons

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36
Q

If heat or electrics is added what happens to electrons

A

They jump to an excited state

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37
Q

How is light produced

A

Excited by energy electron hops up to an excited state then falls back done to ground state and energy is released as light

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38
Q

Partial rainbow that only shows transitions between Es and Gs

A

Line emission spectrum

39
Q

Shows all colors in the rainbow

A

Continuous spectrum

40
Q

Revised version of the Bohr model

A

Wave-mechanical model

41
Q

Regions of probably electron density (electron location)

A

Electron move in ORBITALS

42
Q

Group of same type of atoms

A

Element

43
Q 
High Melting/boiling point 
High density
Shiny
High conductivity of heat and electricity 
Malleable and ductile
A

Metal

44
Q 
Low melting and boiling point 
Low density 
Dull
Poor conductor 
Brittle
A

Non-metal

45
Q 
Middle melting/boiling point
Middle density
Middle luster
Middle conductivity 
Middle hardness
A

Metalloid

46
Q

Elements in which two atoms are bonded

A

Diatomic elements

BrOFINClH

47
Q

Size of an atom in pm from the nucleus to the outer shell, size increases down a group due to pull of electrons

A

Atomic radius

48
Q

Size of an ion compared to it’s atom

A

Ionic radius

49
Q

Why are cations smaller than anions

A

Less electrons than protons

50
Q

High atomic radius =?

A

Low ionization energy

51
Q

Mutual attraction between two atoms to form a stable octet of valence electrons

A

Chemical bond

52
Q

What are the three types of bonds

A

Covalent: 2 nM ^ electronegativity
Ionic: M and nM high and low electronegativity
Metallic: 2 M Low electronegativity

53
Q

The ability of an atom to attract electrons in a bond

A

Electronegativity

54
Q

Decrease the size=?

A

Increase electronegativity

55
Q

Steps for Lewis structures

A
  1. Make an electron check list
  2. Put atom with the lowest EN that isn’t H in the center
  3. Place all other atoms around
  4. Place electrons around to for stable octets
56
Q

Based on difference in EN

A

Polarity

57
Q 
Strong
Hard
Not conductivity in solid
Conductivity in water
Dissolves in water 
High mp/bp
A

Ionic

58
Q 
Medium 
Soft
Not conductivity in solid or water
Dissolves in h2o 
Medium mp/bp
A

Polar covalent

59
Q 
Medium
Soft
Not conductivity in solid or water
Doesn't dissolve in water
Low mp/bp
A

No polar covalent

60
Q 
Weak 
Hard
Conductive in solid
Doesn't dissolve in water
High mp/bp
A

Metallic

61
Q

What indicates a chemical reaction

A

Heat or light is given off
A color change occurs
A gas is given off
A solid precipitates out

62
Q

Will of the atoms of the left my so be also on the right

A

Law of conservation of mass

63
Q

Ability of an atom to react and form an ion

A

Chemical activity

64
Q

2 become 1

A

Synthesis

65
Q

1 breaks apart

A

Decomposition

66
Q

Element + compound–> new compound + new element

A

Single displacement

67
Q

AB+CD–> AD + CB

A

Double displacement

68
Q

CxHy + O2–> Co2(g) + H2O(g)

A

Combustion

69
Q

The simplest whole number ratio of Atoms for a family of compounds

A

Empirical formula

70
Q

Mols=grams
——-
GFM

A

Gram to mole conversions

71
Q

Energy from a machine

A

Mechanical

72
Q

Energy from a feeling of warmth

A

Thermal

73
Q

Energy from movement and bonds

A

Chemical

74
Q

Energy from light

A

Light

75
Q

Energy from moving electrons

A

Electrical

76
Q

Energy from fission reactions

A

Nuclear

77
Q

Transfer of thermal energy from hot to cold

A

Heat

78
Q

Amount of energy needed to raise a 1.0 g of a sample by 1° C or 1K

A

Specific heat

79
Q

Below 1 J/g/k

A

Heats up quickly, cools down quickly

80
Q

Above 1 J/g/k

A

Heats up slowly, cools down slowly

81
Q

Atoms and molecules can react if they collide with proper speed and orientation

A

Collision theory

82
Q

Rate influencing factors

A

1) Temperature
2) Concentration
3) Surface area
4) Nature of reactions

83
Q

Gasses dissolve at…

A

Low temp

high pressure

84
Q

Real gases act most ideal at…

A

High temp

Low pressure

85
Q

Adding more solvent to a concentrated solution

A

Dilutions

86
Q

Physical properties of a solution that depend on only amount not what it is

A

Colligative properties

87
Q

Factors of colligative properties

A

Love freezing point

High boiling point

88
Q

Use double displacement

A

Arrhenius reaction

89
Q

A compound that acts as both an acid and a base

A

Amphoteric

90
Q

An experiment in which a known amount of acid is fully neutralized by an unknown amount of base

A

Titration

91
Q

Rules for assigning oxidation numbers

A

1) oxi # for all elements is 0
2) oxi # for single atom ions is their charge
3) oxi # for group 1 is +1 and group 2 is +2
4) oxi # for o is always -2
5) oxi # for H is +1 except when bonded to a group one or 2 metal (-1)

92
Q

One product of saponification

A

Soap

93
Q

Yeast

A

Fermentation

94
Q

Which organic reaction includes an acid

A

Esterification

95
Q

Form long chains long chains from small molecules

A

Polymerization

Chemistry (1 decks)

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