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CH186—General Chemistry II > Exam 1 > Flashcards

Exam 1 Flashcards

(74 cards)

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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
examples of ion-dipole
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
26
magnitude of ion-dipole interactions depends on…
charge & size of ion
27
strongest ion-dipole interactions involve…
cations highly charged ions ions with smaller radii
28
define viscosity
resistance to flow
29
what increases viscosity?
IMFs larger surface area lower temp higher molecular weight
30
define surface tension
measure of elastic force on surface of a liquid
31
what is the cause of surface tension?
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
example of surface tension
capillary action
33
define vapor pressure
pressure exerted by a liquid’s vapor when the liquid and the vapor are in dynamic equilibrium
34
define volatile
liquids that evaporate more readily
35
volatile liquids have ______ IMFs and __ VP
weaker IMFs higher VP
36
higher temperature _______ VP
increases
37
define boiling point
temperature at which a liquid’s VP equals external pressure acting on liquid’s surface
38
define normal BP
BP at 1 atm (760 torr)
39
properties of solids are based on…
how molecules are held together
40
define melting point
temperature at which energies of individual particles allow them to break free of their fixed positions
41
regular repeating arrangement
crystalline solids
42
arrangement lacks regularity
amorphous solids
43
well-defined MP
crystalline solids
44
MP varies
amorphous solids
45
define unit cell
smallest repeating structure in a crystal
46
where two lines meet on a unit cell
lattice point
47
7 types of unit cells
* Simple cubic * Tetragonal * Orthorhombic * Rhombohedral * Monoclinic * Triclinic * Hexagonal
48
_primitive cubic_ total atoms L =
1 atom L = 2r
49
V =
V = L3
50
_body-centered cubic_ total atoms L =
2 atoms L = 4r/√3
51
_face-centered cubic_ total atoms L =
4 atoms L = √8(r)
52
define coordination number
how many particles one particle touches
53
body centered CN
8
54
face centered CN
12
55
5 steps to find density of a unit cell
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
corner atom = ___ of an atom
1/8
57
edge atom = ___ of an atom
¼
58
face atom = ___ of an atom
½
59
1 AMU = _______ grams
1 AMU = 1.66\*10-24 grams
60
1 gram = ________ AMU
1 gram = 6.022\*1023 AMU
61
how to convert from pm to cm
L (in pm) \* 1 m/1012 pm \* 100 cm/1 m = L (in cm)
62
D =
D = m/v
63
cations & anions held together by Coulumic attraction
ionic crystals
64
ionic crystal properties (5)
hard, brittle, high MP, poor conductor, often white/grainlike
65
large network of atoms connected by covalent bonds
covalent crystals
66
diamonds, graphite, silicon dioxide, silicon carbide
covalent crystals
67
covalent crystal properties (4)
hard, brittle, high MP, poor conductor
68
repeating structures held together by van der waals forces (hydrogen bonds, dispersion, dipole-dipole)
molecular crystals
69
sugar, ice, dry ice, caffeine
molecular crystals
70
molecular crystal properties (3)
soft, low MP, poor conductors
71
crystals likely to be organic
molecular
72
held together by van der waals forces - electrons are delocalized & shared
metallic crystals
73
metallic crystals properties (4)
strong, malleable, good conductors, variable MPs
74
4 types of crystals
ionic covalent molecular metallic

CH186—General Chemistry II (6 decks)

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