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Chem 20 > review > Flashcards

review Flashcards

1
Q

what are lewis structures and what do they show

A

electron diagrams for individual elements showing valence electrons

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2
Q

what are intramolecular forces

A

the forces within a molecule

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3
Q

what forces hold a molecule together

A

bonds

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4
Q

what types of bonds are there

A

covalent and ionic

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5
Q

ionic bonds do not _____

A

share electrons

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6
Q

ionic bonding

metals ____ valence electrons

A

loose

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7
Q

ionic bonding

non metals _____ valence electrons

A

gain

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8
Q

covalent bonds do ______

A

share electrons

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9
Q

what are covalent bonds

A

bonds holding molecular compounds together

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10
Q

what are covalent bind structures also called

A

lewis structures

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11
Q

which element goes in the middle with covalent bond structures

A

the element with the most bonding electrons

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12
Q

exception to each element needing 8 valence electrons

A

hydrogen (2)

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13
Q

when do double and triple bonds form

A

when each element should have 8 valence electrons and there should be no lone pairs

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14
Q

make vespr shapes

A 
linear 
bent 
trigonal pyramidal 
trigonal planar
tetrahedral
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15
Q

where are electronegativities found

A

on the periodic table

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16
Q

what does the electro negativity show

A

how badly an element wants electrons

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17
Q

the higher the electro negativity the _____ it pulls

A

stronger

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18
Q

arrow points towards element with _____ electronegativty

A

higher

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19
Q

what do you do with the difference in electro negativity between 2 atoms

A

the diffference determines the bond

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20
Q

electronegativity 3.3-1.7 is _____

A

mostly ionic

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21
Q

electronegativity 1.7-0.5 is ________

A

polar covalent

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22
Q

electronegativity 0.5-0 is ______

A

slightly polar covalent

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23
Q

electronegativity 0 is ______

A

non polar covalent

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24
Q

another word for non polar covalent is

A

perfect sharing

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25
Q

polarity of a linear with middle atom bonded to the same atoms

A

non polar

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26
Q

polarity of a linear with middle atom bonded to different atoms

A

polar

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27
Q

polarity of a trigonal planar with middle atom bonded to the same atoms

A

non polar

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28
Q

polarity of a trigonal planar with middle atom bonded to different atoms

A

polar

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29
Q

polarity of a bent

A

polar

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30
Q

polarity of a tetrahedral with middle atom bonded to the same atoms

A

non polar

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31
Q

polarity of a tetrahedral with middle atom bonded different atoms

A

polar

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32
Q

what do intermolecular forces cause

A

cause attraction between molecules

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33
Q

intermolecular forces are weaker than ______

A

bonding within a molecule

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34
Q

what are intermolecular forces responsible for and why

A

responsible for boiling points and melting points of compounds

since when you boil/melt a molecule you are only breaking these forces between molecules

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35
Q

intermolecular forces occur between ______

A

molecular compounds

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36
Q

dipole dipole three things

A

occur between polar molecular compounds only

slightly positive end of one molecule is attracted to the slightly negative end of another molecule

permanent attractions

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37
Q

london dispersion three things

A

OCCUR BETWEEN NON POLARS

occur between all molecular compounds

caused by electrons in atoms and molecules constantly being in motion (making it polar)

forces are stronger as the molecule becomes larger or has more electrons

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38
Q

hydrogen bonding two things

A

NOF

hydrogen has such a low electronegativity compared to these three so it has its electrons pulled so far away from it. something else

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39
Q

why are metals solid at room temp

A

metal atoms have very strong forces between them

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40
Q

how to melt metals

A

need to add lots of energy (high temp) to overcome these strong forces

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41
Q

what are the big circles on a metallic bond model

A

metal cations

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42
Q

what are the small circles on a metallic bond model

A

sea of delocalized electrons

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43
Q

which has stronger forces of attraction ionic compounds or metallic

A

metallic

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44
Q

how to melt ionic compounds

A

need to add lots of energy (high temp) to overcome these strong forces

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45
Q

what kind of structure do ionic compounds have

A

crystal structure

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46
Q

how do crystal structures form

A

so that oppositely charged ions are as close together as possible

47
Q

what is a crystal lattice

A

a 3-D array of alternating positive and negative ions

48
Q

are intermolecular forces within or between

A

between

49
Q

what are the intramolecular forces

A

metallic
ionic
covalent
network covalent

50
Q

are intramolecular forces within or between

A

within

51
Q

scale of forces from lowest to highest

A 
london dispersion 
dipole dipole 
hydrogen bond 
covalent 
ionic 
network covalent
52
Q

what is the scale of forces used for

A

used for ordering compounds based on their boiling points

53
Q

if two molecular compounds only have london dispersion which has the higher boiling point

A

bigger molecule/ moles le with more electrons

54
Q

what is constant in boyle’s law

A

temperature

55
Q

Boyle’s law formula

A

p1 v1=p2 v2

56
Q

what is constant in charles law

A

pressure

57
Q

charles law formula

A

V1/T1=V2/T2

58
Q

when do you use combined gas law

A

when all three variables change

59
Q

combined gas law formula

A

P1 V1/T1=P2 V2/T2

60
Q

when do you use ideal gas law

A

when given mass or number of moles

61
Q

what to do if given info about pressure and temperature and it’s in a sealed container

A

use combined gas law

V1=V2

62
Q

what are electrolytes and examples

A

compounds that conduct electricity in water because they break apart into ions

ionic compounds
acids

63
Q

are molecular compounds electrolytes and why or why not

A

non electrolytes because they do not break down into ions

64
Q

what is solubility

A

the ability to dissolve

65
Q

when is the solution saturated

A

when the solution is holding as much solute as possible and adding anymore solute will not be able to dissolve

66
Q

what does a saturated solution usually have

A

a small amount of undissolved solute at the bottom that is in constant equilibrium with the solute that is dissolved in the solution (they switch places with each other all the time)

67
Q

steps for preparing a standard solution

A

weigh out solute

dissolve in half amount of water in a beaker

pour into final volume volumetric flask

fill flask to mark and invert to mix

68
Q

when can you use dilution

A

when you have a solution that has too high of a concentration

69
Q

dilution formula

A

V1 C1= V2 C2

70
Q

properties of acids 9 things

A 
sour taste 
electrolytes 
neutralizes bases
turns litmus red 
turns bromothymol blue yellow 
turns phenolphthalein colourless 
reacts with metals to produce H2
ph less than 7
71
Q

properties of bases 8 things

A 
bitter taste
electrolytes
neutralizes acids 
turns litmus blue 
turns bromothymol blue blue 
turns phenolphthalein pink
ph greater than 7
72
Q

properties of neutral substances 3 things

A

electrolytes and non electrolytes
do not affect indicators the same way
ph of 7

73
Q

arrhenius definition of an acid

A

has H+ at the beginning of the compound

74
Q

modified arrhenius definition of an acid

A

reacts with water to form hydronium ions

75
Q

arrhenius definition of a base

A

has hydroxide ions at the end of an ionic compound

76
Q

modified arrhenius definition of a base

A

reacts with water to form hydroxide ions

77
Q

weak acids and bases dont ______

A

don’t 100% break down to form hydronium and hydroxide ions

78
Q

strong acids

A 
HCl
HBr
HI
HClO4
H2SO4
HNO3
79
Q

strong bases

A

group 1 and 2 cations with OH

80
Q

what are monoprotic acids

A

only have 1 H+ ion to give away

81
Q

monoprotic bases

A

can only accept 1 H+ ionor has 1 OH- ion (ions with only 1- charge)

82
Q

polyprotic acids

A

Have more than 1 H+ to give away

83
Q

polyprotic bases

A

can accept more than 1 H+ ion (ions that have more than 1- charge)

84
Q

ph scale interpretation

A

0 is strong acid

14 is strong base

85
Q

poh scale interpretation

A

0 is strong base

14 is strong acid

86
Q

ph formula

A

-log[hydronium ion conc.]

87
Q

poh formula

A

-log[hydroxide ion conc.]

88
Q

hydroxide ion conc. formula

A

[OH]=10^-poh

89
Q

hydronium ion conc. formula

A

[H3O]=10^-ph

90
Q

percent yield formula

A

% yield=actual/predicted (100)

91
Q

percent error formula

A

actual-predicted/ predicted (100)

92
Q

where is endpoint labelled

A

on the curve at ph 7

93
Q

where is equivalent point labelled

A

on the x axis where it lines up with ph 7

94
Q

titration curve for acid titrated with base

A

up to down

95
Q

titration curve for base titrated with acid

A

down to up

96
Q

ppm formula

A

mass of solute (mg)/mass of solution (kg)

97
Q

percentage by volume formula

A

volume of solute (ml)/ volume of solution (ml) (100)

98
Q

percentage weight by volume formula

A

mass of solute (g)/volume of solution (ml) (100)

99
Q

percentage weight by weight formula

A

mass of solute (g)/mass of solution (g) (100)

100
Q

calculate mass when give litres and percent concentration

A

divide concentration by 100 mo to get it out of percent

convert L amount to ml and multiply by that number

101
Q

law of combining volumes

A

use molar ratio

102
Q

decreasing the volume of a gas ______ it’s _______

A

decreases

space between molecules

103
Q

if the temp of a gas is increased the _____ of the molecule is _______

A

kinetic energy

increased

104
Q

gases that are _____ will dissolve in water

A

polar

105
Q

a gas that is ______ can be collected by displacement of water

A

non polar

106
Q

increasing kinetic energy of molecules _______ the number of collisions with the walls of the container and ____ the pressure

A

increases

increases

107
Q

decreasing the number of collisions with the walls of a container ______ the free on the walls of the container

A

decreases

108
Q

if the gas container is a steel canister the ____ will increase if the number of collisions with the wall increases

A

pressure

109
Q

if the container is a rubber balloon and the kinetic energy of the particles inside decreases, the space between the molecules will _____

A

decrease

110
Q

if a sample glass is heated in a closed flask, the ___ increases

A

number of collisions

111
Q

the mass of a gas in an open 10 L container at 20 degrees is _____ than the mass of a gas in an open 10 L container at 49 degrees

A

greater

112
Q

____ and ____ are always polar

A

bent and trigonal

pyramidal

113
Q

intermolecular forces weakest to strongest

A

LD
DD
HB

Chem 20 (5 decks)

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