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Chemistry Lecture > Exam One > Flashcards

Exam One Flashcards

1
Q

As the molecules of a gas attract each other into a liquid and then become fixed in a solid, the system is […] energy. This is an […] change.

A

loses; exothermic

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2
Q

Overcome the attractive forces that keep the particles fixed in place in a solid or near each other in a liquid. The system must […] energy. This is an […] change.

A

absorbs; endothermic

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3
Q

Melting or […]. The enthalpy change is […]. For freezing the enthalpy change is […].

A

fusion; positive; negative

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4
Q

Gas formation or […]. The enthalpy change is […]. For condensation, the enthalpy change is […].

A

vaporization; positive; negative

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5
Q

Sublimation:

A

solid goes to a gas

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6
Q

Sublimation calculation of enthalpy change:

A

heats of fusion + heats of vaporization

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7
Q

Deposition:

A

gas goes to solid

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8
Q

Deposition calculation of enthalpy change:

A

(-) heats of fusion + (-) heats of vaporization

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9
Q

Molecules with weaker IMF are held […] tightly at the surface and vaporize more […]. Weaker IMFs are, the […] the vapor pressure.

A

less; easily; higher

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10
Q

Vapor pressure and temperature can be converted to a linear relationship with the use of…

A

Clausius-Clapeyron

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11
Q

Clausius-Clapeyron Equation at one at two known temperatures:

A

lnP = (-Hvap/R) (1/T) + C

ln(P2/P1) = (-Hvap/R) (1/T2-1/T1)

R = 8.314 J/mol*K

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12
Q

% By Mass Equation:

A

mass of solute/ mass of solution

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13
Q

% By Volume Equation:

A

volume of solute/ volume of solution

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14
Q

Molality Equation:

A

amount of solute/ mass of solvent (kg)

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15
Q

Molarity Equation:

A

amount of solute/ volume of solution

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16
Q

Mole Fraction:

A

amount (mole of solute)/ amount of solution (mole solute + mole of solvent)

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17
Q

Regions of the phase diagram represent…

A

conditions of pressure and temperature at which the phase is stable

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18
Q

Solid-liquid line has a slightly positive slope because…

A

the solid is more dense than the liquid (except water)

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19
Q

The triple pint of a phase diagram where…

A

all three phases are in equilibrium (simultaneous work)

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20
Q

Critical point:

A

two densities become equal and the phase boundary disappears

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21
Q

How does the phase diagram for water differ?

A

the solid-liquid line has a negative slop because the solid form is less dense

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22
Q

How does the phase diagram for water differ?

A

the solid-liquid line has a negative slop because the solid form is less dense

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23
Q

List the 3 bonding forces:

A

ionic
covalent
metallic

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24
Q

List the 6 IMF forces:

A

ion-dipole (NaH2O)

H-bond (H to N, O, F)

ion-induced dipole (FeO2)

dipole-dipole (ICl-ICl)

dipole-induced dipole (HCl-ClCl)

dispersion (F2-F2)

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25
Q

Ion-Dipole forces: The prime example would be…

Why does this occur?

A

any ionic compound dissolving in water

the attraction between the negative pole and ion is greater than the between the ions themselves

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26
Q

If the dipole-dipole forces of 2 compounds have a similar mass, what can determine the stronger force?

A

the one with the greater dipole moment

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27
Q

For a NP molecule, distortion of an electron cloud induces a […].

A

temporary dipole moment

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28
Q

For a P molecule, distortion of an electron cloud induces an […].

A

increase in the already existing dipole moment

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29
Q

Polarizability:

A

how easily the electron cloud of an atom can be distorted

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30
Q

Which is more polarizable: smaller particles or larger ones?

A

larger; smaller molecules are held more closely to the nucleus

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31
Q

List the 2 trends of the PT when it comes to polarizability:

A
  1. increases down a group (atomic size increases and larger electron clouds are easier to distort)
  2. decreases across a period (increasing Zeff makes the atoms smaller and hold the electrons more tightly)
32
Q

Cations are […] polarizable than their parent atoms because they are smaller. Anions are […] polarizable because they are larger.

A

less; more

33
Q

When an ion distorts the electron cloud of a NP substance what forces result?

A

an ion-induced dipole

34
Q

When a P molecule causes the distortion to an NP electron cloud what forces result?

A

a dipole-induced dipole

35
Q

London dispersion occurs between all particles because they result from…

A

the motion of electrons

36
Q

Dispersions are also known as…

A

instantaneous dipole-induced dipole forces

37
Q

How can a dipole be formed in a dispersion electron cloud?

A

instantaneously there’s more electrons on one side of the nucleus than the other

38
Q

The relative strength of dispersion forces depends on the […] of the particles.

A

polarizability

39
Q

A linear chain of carbons vs a tetrahedral shape. If the two have equal mass which has the higher bp?

A

chain because there are more points at which dispersion forces act

40
Q

IMF: Ion + P =

A

ion-dipole forces

41
Q

IMF: Ion + NP =

A

ion-induced dipole forces

42
Q

IMF: P + NP =

A

dipole-induced dipole forces

43
Q

IMF: P + P =

A

dipole -dipole forces

44
Q

How to determine which compound has the highest vapor pressure?

Why is this the case?

A

the one with the strongest IMF has the lower vapor pressure

substances with stronger IMF mean fewer molecules will have enough kinetic energy to escape at a given temperature

45
Q

We can divide solids into two broad categories:

A
  1. crystalline

2. amorphous

46
Q

Crystalline solids:

A

well defined shapes because their particles occur in an orderly arrangement

47
Q

Amorphous solids:

A

poorly defined shapes because of the lack of orderly arrangement

48
Q

Unit cell:

A

the smallest portion of a crystal that, if repeated in all three directions, yields the crystal

49
Q

Coordination number:

A

in a crystal, the number of nearest neighbors surrounding a particle

in a complex ion, the number of ligand atoms bonded to the central metal ion

50
Q

List the three types of cubic cell units:

A
  1. simple
  2. body centered
  3. face centered
51
Q

The coordination of each cubic cell unit:

A

6 for simple

8 for body-centered

12 for face-centered

52
Q

How many particles make up a simple cubic? Explain with the formula.

A

1

(8 corners) x (1/8 particle shared between adj cells) = 1

53
Q

How many particles make up a body-centered cubic? Explain with the formula.

A

2

(8 corners) x (1/8 particle shared between adj cells) = 1 + 1 particle in the center = 2

54
Q

How many particles make up a face-centered cubic? Explain with the formula.

A

4

(8 corners) x (1/8 particle shared between adj cells) = 1 + (1/2 particle shared at the face) x (6 faces) = 4

55
Q

Atomic solids/ noble gases crystallize in a […].

A

cubic closest packing (face-centered cubic unit cell)

56
Q

Molecular solids have molecules at the lattice points and often adopt […].

A

cubic closest packing

57
Q

Ionic solids crystallize with one ion filling hold in the […] array of the other.

A

cubic closest packing

58
Q

Most metals have a […].

A

closest packed structure

59
Q

What are some examples of amorphous solids?

A

charcoal, rubber, glass

60
Q

Why can’t amorphous solids remain ordered?

A

the chains of atoms cannot orient themselves quickly enough so they solidify in a distorted jumble of misaligned rows and gaps

61
Q

Atomic physical properties (3)

A
  1. soft
  2. very low mp
  3. poor conductor
62
Q

Substances with strong IMF have a […] vapor pressure and are less […].

A

lower; volatile

63
Q

Molecular physical properties (3):

A
  1. fairly soft
  2. low-mod mp
  3. poor conductor
64
Q

Ionic physical properties (3):

A
  1. hard and brittle
  2. high mp
  3. good conductor (molten)
65
Q

Metallic physical properties (3):

A
  1. soft to hard
  2. low-high mp
  3. excellent conductor
66
Q

Network covalent physical properties (3):

A
  1. very hard
  2. very high mp
  3. poor conductor
67
Q

Examples of hexagonal packing:

A

Mg, Ti, Zn

68
Q

Example of cubic closest:

A

Ni, Cu, Pb, CO2, CH4, noble gases

69
Q

Solvent:

A

substance in which other substances dissolve; the most abundant component

70
Q

Solute:

A

substance that dissolves in a solvent

71
Q

Solubility:

A

maximum amount that dissolves in a fixed quantity of a given solvent at a given temperature

72
Q

Miscible:

A

soluble at any proportion

73
Q

Liquids that do not dissolve each other are […].

A

immiscible

74
Q

Solubility of alcohols in water: when is it too low that the mixture is insoluble?

A

when alcohols larger than three carbons solubility decreases; insoluble at 6 or more

75
Q

What is polar?

A

the uneven distribution of electron density

76
Q

What does it mean to be polar?

A

to have a separation of charge leading to a molecule or compound electrical dipole moments

Chemistry Lecture (7 decks)

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