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CH186—General Chemistry II > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

only compressible state of matter

A

gas

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2
Q

specific volume, but fill container

A

liquids

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3
Q

only state of matter that cannot diffuse

A

solids

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4
Q

specific shape & volume

A

solids

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5
Q

no specific volume - fills container

A

gases

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6
Q

3 things that cause change in state of matter

A

temperature

pressure

charge

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7
Q

determines state of matter

A

IMFs

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8
Q

define IMFs

A

short range attractive & repulsive forces between molecules

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9
Q

4 types of IMFs

A
  • dipole-dipole interactions
  • dispersion forces
  • hydrogen bonds
  • ion-dipole interactions
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10
Q

only non-van der waals IMF

A

ion-dipole

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11
Q

explain dipole-dipole

A

polar molecules - polarity caused by differences in electronegativity among atoms in molecule

partial charges result in a dipole

+ parts of molecule attracted to - parts of other molecules

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12
Q

examples of dipole dipole

A

H2O

HF

HCl

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13
Q

most electronegative parts of PT

A

top right

H

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14
Q

most electronegative element (4)

A

fluorine

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15
Q

____ and _____ of dipole dipole interactions determines properties

A

strength and number

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16
Q

strength of IMFs is reflected in….

A

BP

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17
Q

describe hydrogen bonding

A

subset of dipole-dipole interactions

includes H bound to N, O, or F

when H is bound to highly electronegative atoms, it acquires a highly positive charge & attracts other electronegative atoms

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18
Q

explain dispersion forces

A

result from instantaneous dipoles & induced dipoles

occur among ALL molecules

constantly happening

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19
Q

describe instantaneous dipole

A

nonuniform distribution of electrons (even in a nonpolar molecule)

temporary, moves back and forth

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20
Q

describe induced dipole

A

when an instantaneous dipole polarizes neighboring molecules

“pushes” electrons

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21
Q

_____ and _____ determines magnitude of dispersion forces

A

size & shape

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22
Q

which shape creates greater dispersion forces?

A

linear

more surface area

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23
Q

which molecules have largest instantaneous dipoles?

A

large

nonpolar

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24
Q

describe ion-dipole interactions

A

ions interacting with neutral polar molecules

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25
Q

examples of ion-dipole

A

salt dissolving in water (Na+ becomes surrounded by the O side of the water molecule, Cl- becomes surrounded by the H sides of the water molecule)

ammonia

acetic acid

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26
Q

magnitude of ion-dipole interactions depends on…

A

charge & size of ion

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27
Q

strongest ion-dipole interactions involve…

A

cations

highly charged ions

ions with smaller radii

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28
Q

define viscosity

A

resistance to flow

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29
Q

what increases viscosity?

A

IMFs

larger surface area

lower temp

higher molecular weight

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30
Q

define surface tension

A

measure of elastic force on surface of a liquid

31
Q

what is the cause of surface tension?

A

the surface molecules are the only ones that do not have IMFs in all directions; because nothing attracts them from the top, they cohere to molecules below the surface

32
Q

example of surface tension

A

capillary action

33
Q

define vapor pressure

A

pressure exerted by a liquid’s vapor when the liquid and the vapor are in dynamic equilibrium

34
Q

define volatile

A

liquids that evaporate more readily

35
Q

volatile liquids have ______ IMFs and __ VP

A

weaker IMFs

higher VP

36
Q

higher temperature _______ VP

A

increases

37
Q

define boiling point

A

temperature at which a liquid’s VP equals external pressure acting on liquid’s surface

38
Q

define normal BP

A

BP at 1 atm (760 torr)

39
Q

properties of solids are based on…

A

how molecules are held together

40
Q

define melting point

A

temperature at which energies of individual particles allow them to break free of their fixed positions

41
Q

regular repeating arrangement

A

crystalline solids

42
Q

arrangement lacks regularity

A

amorphous solids

43
Q

well-defined MP

A

crystalline solids

44
Q

MP varies

A

amorphous solids

45
Q

define unit cell

A

smallest repeating structure in a crystal

46
Q

where two lines meet on a unit cell

A

lattice point

47
Q

7 types of unit cells

A
  • Simple cubic
  • Tetragonal
  • Orthorhombic
  • Rhombohedral
  • Monoclinic
  • Triclinic
  • Hexagonal
48
Q

primitive cubic

total atoms

L =

A

1 atom

L = 2r

49
Q

V =

A

V = L3

50
Q

body-centered cubic

total atoms

L =

A

2 atoms

L = 4r/√3

51
Q

face-centered cubic

total atoms

L =

A

4 atoms

L = √8(r)

52
Q

define coordination number

A

how many particles one particle touches

53
Q

body centered CN

A

8

54
Q

face centered CN

A

12

55
Q

5 steps to find density of a unit cell

A
  1. find number of atoms
  2. find total mass (in units requested)
  3. find length of the unit cell (in units requested)
  4. find volume
  5. find density
56
Q

corner atom = ___ of an atom

A

1/8

57
Q

edge atom = ___ of an atom

A

¼

58
Q

face atom = ___ of an atom

A

½

59
Q

1 AMU = _______ grams

A

1 AMU = 1.66*10-24 grams

60
Q

1 gram = ________ AMU

A

1 gram = 6.022*1023 AMU

61
Q

how to convert from pm to cm

A

L (in pm) * 1 m/1012 pm * 100 cm/1 m = L (in cm)

62
Q

D =

A

D = m/v

63
Q

cations & anions held together by Coulumic attraction

A

ionic crystals

64
Q

ionic crystal properties (5)

A

hard, brittle, high MP, poor conductor, often white/grainlike

65
Q

large network of atoms connected by covalent bonds

A

covalent crystals

66
Q

diamonds, graphite, silicon dioxide, silicon carbide

A

covalent crystals

67
Q

covalent crystal properties (4)

A

hard, brittle, high MP, poor conductor

68
Q

repeating structures held together by van der waals forces (hydrogen bonds, dispersion, dipole-dipole)

A

molecular crystals

69
Q

sugar, ice, dry ice, caffeine

A

molecular crystals

70
Q

molecular crystal properties (3)

A

soft, low MP, poor conductors

71
Q

crystals likely to be organic

A

molecular

72
Q

held together by van der waals forces - electrons are delocalized & shared

A

metallic crystals

73
Q

metallic crystals properties (4)

A

strong, malleable, good conductors, variable MPs

74
Q

4 types of crystals

A

ionic

covalent

molecular

metallic

CH186—General Chemistry II (6 decks)

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