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AP Chemistry > Thou Shalt Not Forget > Flashcards

Thou Shalt Not Forget Flashcards

1
Q

Compounds are separated into elements by?

A

Chemical Changes

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2
Q

Mixtures are separated into elements by?

A

Physical changes

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3
Q

Filtering separates mixtures based on differences in?

A

Particle size, large particles are trapped on the filter paper and the soluble compound goes through it

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4
Q

Distillation separates mixtures based on differences in?

A

Boiling point

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5
Q

What component moves up the farthest in paper chromatography?

A

The most similar in polarity to the “mobile phase”

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6
Q

What is conserved in chemical and physical changes?

A

Mass

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7
Q

When reading a volume of a liquid in a container, you can estimate by?

A

Reading in between the graduated markings, giving one more sig fig

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8
Q

Measuring devices from least precise to most precise?

A

Beaker, graduated cylinder, volumetric flasks, and burette

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9
Q

Density equals?

A

Mass/ volume

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10
Q

The % composition for a pure compound?

A

Does not change

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11
Q

Gas mixtures are homogeneous because of?

A

The constant random motion of the particles

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12
Q

Gases are compressible because of?

A

The large space between the particles

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13
Q

Gas pressure is caused by?

A

Collisions of particles with the walls of the container

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14
Q

More collisions=?

A

More pressure

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15
Q

Pressure and volume are?

A

Inversely related

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16
Q

Temperature and volume are?

A

Directly related

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17
Q

Temperature and pressure are?

A

Directly related

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18
Q

Doubling the volume of the container will?

A

Cut the pressure in half

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19
Q

Heating a rigid container will?

A

Increase the pressure of the gas

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20
Q

A heated balloon will?

A

Expand

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21
Q

PV=

A

nRT

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22
Q

Temperature=

A

Kelvin

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23
Q

Volume=

A

Liters

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24
Q

Pressure=

A

atm

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25
Q

Gas constant, R=

A

.0826

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26
Q

One mole of an ideal gas at STP=

A

22.4 liters

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27
Q

Gas pressure and number of moles are?

A

Directly related

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28
Q

If you double the moles of gas in a container?

A

The pressure will double

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29
Q

Molar mass=

A

dRT/P

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30
Q

Density=

A

g/L

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31
Q

The more molar mass a gas has?

A

The slower it moves at a given temperature

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32
Q

Temperature=

A

Average Kinetic Energy

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33
Q

Gases at the same temperature have?

A

The same average kinetic energy

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34
Q

Collecting a gas by water displacement?

A

P(total)=P(dry gas) + P(water vapor)

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35
Q

Real gases behave most like an ideal gas at?

A

High temperature and low pressure

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36
Q

The more polar a gas is and the larger a gas is, the more it will?

A

Deviate from ideal behavior

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37
Q

Small, nonpolar gases are?

A

The most ideal

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38
Q

An electron is where when farther away from the nuclues?

A

A higher energy level

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39
Q

An electron with less Coulombic attraction to the nucleus is?

A

Easier to remove, it has a lower 1st ionization energy

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40
Q

Moving across a row on the periodic table, the Z eff increases, therefore the valence electrons?

A

Are more attracted to the nucleus, the atomic radius decreases and the ionization energy increases

41
Q

When reading a PES graph, the higher the peak?

A

The more electrons there are in that sublevel

42
Q

A larger binding energy means that?

A

The electrons are closer to the nucleus

43
Q

What are the ionization levels?

A

1s2 2s2 2s6 3s2 3p6 4s2 3d10 4p6

44
Q

When writing the electron configuration for a cation, remove the?

A

Valence electrons first, p orbital and s orbital, then d orbita

45
Q

Isotopes of the same element have?

A

Same number or protons, different number of neutrons

46
Q

Mass spectroscopy graphs measure?

A

Atomic masses of isotopes

47
Q

Elements in the same group (vertical columns) have?

A

Similar chemical and physical properties

48
Q

Metals are on what side of the zig-zag line?

A

Left side

49
Q

Nonmetals are on what side of the zig-zag line?

A

Right side

50
Q

Cation are smaller than anions because?

A

You are removing valence electrons farther from the nucleus

51
Q

Anions are bigger that cations because?

A

Adding extra electrons increases electron-electron repulsions

52
Q

Covalent bonds are formed between?

A

Two nonmetals sharing electrons

53
Q

Ionic bonds are formed when?

A

A metal transfers electrons to a nonmetal and the opposite charges attract

54
Q

The greater the electronegativity difference between two atoms?

A

The more polar the bond becomes

55
Q

Combustion reactions make?

A

CO2 and H2O

56
Q

H2, O2, N2, Cl2, Br2, I2, F2

A

Diatomic elements, when in a compound, their number of atoms can vary

57
Q

Empirical formula rhyme?

A

% to mass, mass to mole, divide by small, times til whole…..get the simplest whole # ratio of the moles (or atoms) in the compound

58
Q

The molecular formula for a compound is?

A

A whole # multiple of the empirical formula ratio

59
Q

Percent yield=

A

(experimental)/(theoretical)

60
Q

%error=

A

(experimental-theoretical)/ theoretical

61
Q

The amount of product for a reaction is determined by?

A

The limiting reactant

62
Q

Carbon makes a total of how many bonds in a compound?

A

4

63
Q

Bond angle, 4 domains?

A

109.5 degrees

64
Q

Bond angle, 3 domains?

A

120 degrees

65
Q

Bond angle, 2 domains?

A

180 degrees

66
Q

Hybrid orbitals, 4 domains?

A

sp3

67
Q

Hybrid orbitals, 3 domains?

A

sp2

68
Q

Hybrid orbitals, 2 domains?

A

sp

69
Q

Asymmetrical molecules=

A

Dipoles don’t cancel, polar molecule

70
Q

Symmetrical molecules=

A

Dipoles cancel, nonpolar molecule

71
Q

Single bond=

A

Sigma

72
Q

Double bond=

A

Sigma + pi bond

73
Q

Triple bond=

A

Sigma + two pi bonds

74
Q

What is lattice energy?

A

The energy needed to break an ionic bond in a compound, increases as ion’s charge increases, decreases as radii of ions increase (deduced from Coulomb’s Law)

75
Q

What does formal charge involve?

A

Comparing the # of valence electrons an atom has to the # of electrons around it in the Lewis structure (“split” the bonded electrons evenly between the atoms)

76
Q

When drawing Lewis Dot Structure, you should?

A

Obey the octet rule first, use formal charge if necessary, put extra electrons on the larger central atom, and make double or triple bonds if you have too few electrons

77
Q

First IMF

A

London Dispersion

78
Q

Second IMF

A

Dipole-dipole

78
Q

Third IMF

A

Hydrogen Bonding

79
Q

Fourth IMF

A

Ion-dipole

80
Q

All molecules have what force

A

London Dispersion Forces

81
Q

What makes LDF stronger?

A

Larger molecule, Larger electron cloud, more polarizable

82
Q

Larger Electron cloud= more LDF = ?

A

More polarizable

83
Q

All polar molecules contain what forces?

A

Dipole-dipole, which is stronger when more polar

84
Q

Hydrogen bonds are between?

A

NOF, and another hydrogen bonded to NOF in a compound

85
Q

Boiling points and melting points increase as?

A

IMF increases

86
Q

As IMF increases, vapor pressure and volatility?

A

Decreases

87
Q

Molecular solids have what melting and boiling points?

A

Low ones

88
Q

Do molecular solids conduct electricity?

A

No

89
Q

Ionic solids have what boiling and melting points?

A

High

90
Q

When do ionic solids conduct electricity?

A

As a liquid or aq

91
Q

Two covalent network solids are?

A

SiO2 (quartz) and diamonds

92
Q

SiO2 (quartz) and diamonds have what melting and boiling points?

A

Very High

93
Q

What are metallic bonds between?

A

Metals

94
Q

Do metallic bonds conduct electricity?

A

Yes, always

95
Q

What is a metallic bond’s texture?

A

It varies

96
Q

What breaks as a molecular solid boils or melts?

A

IMFs between the molecules

97
Q

What is made when a smaller atoms fits in the gaps between the larger atoms in a metallic crystal?

A

Interstitial alloy

98
Q

What is made when the radii of the metals are similar in size are substituted into the crystal lattice?

A

Substitutional alloy

AP Chemistry (5 decks)

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