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General Chemistry > Exam 1 > Flashcards

Exam 1 Flashcards

Chapters 1, 2, and 3

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1
Q

Giga_

A

10^9

G

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2
Q

Mega_

A

10^6

M

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3
Q

Kilo_

A

10^3

k

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4
Q

Hecto_

A

10^2

h

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5
Q

Deka_

A

10^1

da

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6
Q

Deci_

A

10^-1

d

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7
Q

Centi_

A

10^-2

c

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8
Q

Milli_

A

10^-3

m

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9
Q

Micro_

A

10^-6

weird backwards y/u thing

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10
Q

Nano_

A

10^-9

n

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11
Q

Electrical Current Units

A

amperes (A)

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12
Q

Mole

A

amount of a substance (mol)

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13
Q 
Select the correct relationship between these metric units of length or distance
A. 1km = 100m
B. 1mm = 10cm
C. 1 nm = 10^9m
D. 10^6microm = 1m
A

D. 10^6 micrometers = 1 meter

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14
Q

Round the answer for the mathematical operation below to the appropriate number of significant figures

(1.23g - 0.567g)/(0.34442 cm^3) = ?

A

1.9 g/cm^3

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15
Q

How many sig figs are in 0.04550?

A

4

leading 0s are insignificant

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16
Q

How many sig figs are in 100?

A

1

trailing 0s only count if captive

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17
Q

How many sig figs in 101.05?

A

5

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18
Q

How many sig figs in 350.0?

A

4

zeros trailing are only significant if decimal place is present

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19
Q

Neon has a boiling point of 27.0 K. Express this temperature in Fahrenheit.

A

-411 degrees F

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20
Q

Significant Figures In Multiplication and Division

A

of sig figs in result = # in the least precise measurement used in the calculation

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21
Q

Significant Figures in Addition and Subtraction

A

of sig figs in result depends on # of DECIMAL PLACES in the least accurate measurement

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22
Q

Significant Figures in Addition and Subtraction

A

of sig figs in result depends on # of DECIMAL PLACES in the least accurate measurement

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23
Q

If matter has constant properties and composition then it is considered __

A

a pure substance

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24
Q

If matter doesn’t have constant properties and composition then it’s considered __

A

a mixture

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25
Q

If a pure substance can be simplified chemically then it’s considered __

A

a compound

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26
Q

If a pure substance can’t be simplified then it’s considered __

A

an element

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27
Q

If a mixture is uniform throughout, it is considered __

A

homogeneous

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28
Q

If a mixture is not considered uniform throughout, then it’s considered __

A

heterogeneous

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29
Q

Physical Property

A

can be observed without changing into another substance

Ex. volume, boiling point, color

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30
Q

Chemical Property

A

can be observed only by reacting it to form another substance
Ex. flammability, toxicity

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31
Q

Intensive Properties

A

independent of amount of substance present

Ex. color, melting point, if you have a small flake of gold and a big one, they have the same properties

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32
Q

Extensive Properties

A

varies with the quantity of the substance present

Ex. volume, mass

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33
Q

Solid Gas

A

S–>G = sublimation

G –> S = crystalization

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34
Q

Density

A

ratio of mass of an object/substance to volume of the object/substance

d = m/v

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35
Q

Is density an intensive or extensive property?

A

intensive

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36
Q 
Which of these are chemical properties of matter?
I. corrosiveness
II. density
III. flammability
IV. melting point
A

I and III

37
Q

Leucippus and Democritus

A

keyed the term “atomos” which is Greek for “indivisible”

38
Q

Aristotle View of Elements

A

thought there were only 4

  1. fire
  2. earth
  3. water
  4. air
39
Q

John Dalton’s 5 Postulates

A
  1. matter is comprised of atoms
  2. an element has only 1 type of atom
  3. each element contains different types of atoms
  4. a compound = 2+ elements in whole # ratio
  5. atoms neither created nor destroyed
40
Q

Law of Definite Proportions

A

a compound will always be found in nature with the same proportion of elements, otherwise, it is a different compound

Ex. water will always have 2 hydrogens and 1 oxygen

41
Q

Law of Multiple Proportions

A

whenever the same 2 elements form more than 1 compound

the different masses of 1 element that combines with the same mass of the other element are in the ratio of small whole numbers

Ex. mass of CO= 12.01+16 = 1:1
but CO2= 12.01+32 = 2:1

42
Q

Thompson’s Atomic Structure

A

discovered that atoms have negatively charged particles w/ constant mass to charge ratio

accidentally discovered electrons

cathode ray

charge = 1.759 x 10^8 C (coulombs)

43
Q

Millikan’s Atomic Structure

A

determined mass and charge of electron

oil drop experiment

used Thompson’s mass to charge ratio

m = 9.109 x 10^28

44
Q

Charge is Measured in ___

A

coulombs

C

45
Q

Thomson’s Atomic Model

A

plum pudding

electron distributed evenly through spherical space

46
Q

Nagaoka’s Atomic Model

A

like Saturn

positively charged sphere

47
Q

Rutherford’s Experiment

A

nobel prize

nucleus based

48
Q

Subatomic Particles

A

neutron
electron
proton

49
Q

Neutron
amu
mass
charge

A

1.00867 ~ 1 amu
1.67 x 10^-24 g
0 C

50
Q

Proton
amu
mass
charge

A
  1. 00728 ~ 1 amu
  2. 67 x 10^-24 g
  3. 602 x 10^-19 C
51
Q

Electron
amu
mass
charge

A
  1. 485799 x 10^-4 ~ 0 amu
  2. 10939 x 10^-28 g
    - 1.602 x 10^-19 C
52
Q

Atomic Mass

A

top left corner of element box

total number of nucleons (protons and neutrons) in nucleus

53
Q

Elemental Symbol

A

1 or 2 letter symbol identifying atom

54
Q

Atomic Number

A

bottom left of element box
number of protons in nucleus
determines identity of element

55
Q

Ion

A

element or molecule with a charge

56
Q

Isotopes

A

results from changes in neutron number

throws off atomic mass

57
Q

How do you determine the number of protons, neutrons, and electrons in an element in any state?

A

subtract # of protons from atomic mass to find neutrons

subtract number of electrons from number of protons to find number of electrons

58
Q

Average Atomic Mass

A

weighted average of masses of all isotopes of an element

59
Q

Natural Abundance

A

proportion of a particular isotope

displayed in percentages

60
Q

Chemical Nomenclature

Polyatomic Ion Names, Formulae, and Charges

A

Special study deck made just for this

61
Q

Predict the formula for the binary ionic compound formed by Al and O

A

Al2O3

play with them until the charges cancel each other out

62
Q

What’s the molecular mass of sulfuric acid?
H2SO4
What unit is molecular mass measured in?

A

98.08 amu

atomic mass units

63
Q

Formula Mass

A

sum of average atomic masses of all atoms in substance’s formula

64
Q

Molecular Mass

A

formula mass of a covalent substance

65
Q

Ionic Compounds

A

don’t exist as molecules

average atomic masses of ions can be approximated to be equal to average atomic masses of neutral ions

66
Q

Mole

A

unit that represents 6.022 x 10^23 particles

Avogadro’s number

67
Q

Particles to Moles to Mass

A

particles / (6.022 x 10^23) = moles / (1 mole / # g) = g

68
Q

Mass to Moles to Particles

A

grams x (1 mol / # g) = moles x (6.022 x 10^23) = particles

69
Q

What’s the total number of atoms in 1 mole of CO2?

A

3 x (6.022 x 10^23)

70
Q

Molar Mass

A

(M)

mass of one mole of a compound

71
Q

Isomers

A

compounds with the same chemical formula but with different molecular structures

72
Q

Covalent Bonds

A

bond b/w 2 atoms created by sharing one or more pairs of electrons

73
Q

Ionic Compounds

A

consists of charged particles

total charge has to be zero

74
Q

Pnictogen Family

A

G15 P2-6

75
Q

Solvent

A

part of a solution that’s present in the greatest amount

76
Q

Solute

A

any component in a solution other than the solvent

77
Q

How to calculate the amount of solute within a solution

A

(amount of solute) / (amount of solvent or total solution)

78
Q

Molarity

equation

A

(mols of solute) / (L of solution) = n/v = M

79
Q

Dilution Equation

A

M1V1 = M2V2

80
Q

Stock vs Standard Solution

A

stock - high concentration solution used to prepare lower concentration solution

standard - made from stock solution (lower concentration)

81
Q

Combination Reactions

A

2 or more substances combined to form one product

SO3(g) + H2O(L) –> H2SO4(L)

82
Q

Aqueous

A

dissolved in water; unseen but present

83
Q

4 Steps to Balance a Chemical Equation

A
  1. write out correct formulas for reactants and products (including physical state)
  2. balance element appearing in only one reactant product first (1st count how much of everything you have)
  3. play around with it until number of atoms on each side is equal
  4. balance O2 last
84
Q

Molecular vs. Ionic Equations

A

M - reactants and/or products written as undissociated molecules

I - ionic species represented as dissolved ions; break up the ions into positive and negative charge and work from there

85
Q

What is the net ionic equation for

AgNO3(aq) + KCl(aq) –> AgCl(s) + KNO3(aq)

A

Ag+ + NO3- + K+ + Cl- –> AgCl(s) + Cl-(aq) + NO3-

86
Q

Precipitate

A

solid product formed from a reaction in a solution

can be predicted using solubility rules

turns into (s) in chemical equation

87
Q

How can precipitation reactions be written?

A

using ionic equations

88
Q

Solubility Rules NAG SAG

Always Soluble

A

Nitrates (NO3-)
Acetates (C2H3O2)
Group 1

Sulfates (SO4^2-)
Ammonium (NH4+)
Group 17 (F-, Cl-, Br-, I-)

89
Q

Solubility Rules PMS & CaStro Bear

Exceptions

A

Pb^2+ (lead)
Mercury (Hg^2+)
Silver (Ag+)

Ca^2+
Sr^2+
Ba^2+

General Chemistry (3 decks)

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