chem 106 quiz 1 Flashcards

1
Q

properties of a gas

A

no fixed shape
no fixed volume
compressible
diffusion rapid

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2
Q

properties of liquids

A

no fixed shape
fixed volume
incompressible
diffusion slower

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3
Q

properties of solids

A
fixed shape
fixed volume
incompressible
molecules locked in place (bonds)
diffusion extremely slow
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4
Q

boiling points can indicate

A

the strength of the intermolecular attractive force

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5
Q

ΔHfusion represents the phase change from

A

solid > liquid

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6
Q

ΔHvaporization represents the phase change from

A

liquid > gas

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7
Q

which is typically larger? ΔHfusion or ΔHvaporization? why?

A

ΔHvaporization because completely breaking attractive forces

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8
Q

intermolecular forces (from strongest to weakest)

A

ion-dipole
dipole-dipole (Hydrogen bonding)
dispersion

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9
Q

all molecules have ? forces

A

dispersion; strongest for nonpolar tho

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10
Q

? molecules have dipole-dipole forces

A

polar

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11
Q

ion-dipole forces are present in

A

mixtures of ionic compounds and polar compounds

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12
Q

surface tension and viscosity are affected by

A

intermolecular forces

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13
Q

dispersion forces are always weak in ? molecules but can be significant in molecules with ?

A

small; higher molar mass

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14
Q

Hydrogen bonds are present in molecules containing

A

hydrogen bonded directly to fluorine, oxygen, or nitrogen (but remember - hydrogen bonds are intermolecular/external)

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15
Q

the higher the temperature, the (lower/higher) the average kinetic energy of the collection of molecules

A

higher

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16
Q

ΔHvaporization is always (negative/positive) because the process is (endothermic/exothermic)

A

positive; endothermic

17
Q

ΔHcondensation is always (negative/positive) because the process is (endothermic/exothermic)

A

negative; exothermic

18
Q

boiling point

A

the temperature at which the liquid’s vapor pressure equals the external pressure

19
Q

normal boiling point

A

the temperature at which its vapor pressure equals 1 atm

20
Q

Clausius-Clapeyron equation

A

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

21
Q

the boiling point increases with increasing ? because of the high ?

A

ΔHvap; intermolecular forces

22
Q

the pressure of vaporization (decreases/increases) with increasing IMFs and BP

A

decreases

23
Q

reaction rates double every

A

10*C

24
Q

solid to liquid

A

melting

25
Q

liquid to solid

A

freezing

26
Q

liquid to gas

A

vaporization

27
Q

gas to liquid

A

condensation

28
Q

gas to solid

A

deposition

29
Q

solid to gas

A

sublimation

30
Q

examples of crystalline solids

A

salt, diamond

31
Q

examples of amorphous solids

A

glass, plastic, rubber

32
Q

unit cell

A

smallest repeating unit from which you can build the whole crystal

33
Q

cubic unit cell

A

cube with atoms on the vertices; 1 atom per unit cell

34
Q

body centered cubic

A

cube with atoms on the vertices and one in the center; 2 atoms per unit cell

35
Q

face centered cubic

A

cube with atoms on the vertices and in the centers of the faces; 4 atoms per unit cell (most efficient packing)