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Chem 120 > Exam 1 (1-6) > Flashcards

Exam 1 (1-6) Flashcards

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1
Q

scientific notation

A

to the right is NEGATIVE

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2
Q

scientific notation

A

to the left is POSITIVE

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3
Q

multiply / divide sig figs

A

number with least number of sig figs

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4
Q

add / subtract sig figs

A

number with least number of decimal points

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5
Q

deci

A

-1

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6
Q

centi

A

-2

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7
Q

milli

A

-3

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8
Q

micro

A

-6

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9
Q

nano

A

-9

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10
Q

pico

A

-12

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11
Q

femto

A

-15

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12
Q

kilo

A

3

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13
Q

mega

A

6

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14
Q

giga

A

10

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15
Q

metric length unit

A

meter

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16
Q

SI length unit

A

meter

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17
Q

metric volume unit

A

Liter

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18
Q

SI volume unit

A

cubic meter

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19
Q

metric temperature unit

A

celsius

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20
Q

SI temperature unit

A

K

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21
Q

measured vs exact numbers

A

measured = obtained by measuring devices & are never exact

exact = counted our definitions in measurements with never ending # of sigs

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22
Q

density =

A

mass / volume

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23
Q

units for density

A

g / mL

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24
Q

pure substances

A

elements
compounds

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25
Q

elements

A

1 element

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26
Q

compounds

A

2+ elements chemically bonded

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27
Q

mixtures

A

2+ compounds physically combined

homogeneous
heterogeneous

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28
Q

homogeneous

A

2+ compounds
same composition throughout

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29
Q

heterogeneous

A

2+ compounds
NO uniform composition

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30
Q

solids

A

definite shape
definite volume

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31
Q

liquids

A

NO definite shape
definite volume

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32
Q

gas

A

NO definite shape
NO definite volume

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33
Q

physical properties

A

change in physical state / shape
does NOT alter chemical composition or identity

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34
Q

chemical properties

A

ability of substance to interact with others and to change into another
change is in the composition or identity

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35
Q

energy

A

capacity to do work

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36
Q

kinetic energy

A

energy of motion

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37
Q

potential enegry

A

stored energy

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38
Q

thermal energy

A

energy released as heat

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39
Q

units of heat

A

calorie or joule

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40
Q

metric unit of heat

A

calorie

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41
Q

SI unit of heat

A

joule

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42
Q

conversion Cal to cal

A

1 Cal = 1,000 calories

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43
Q

conversion cal to joules

A

1 cal = 4.184 joules

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44
Q

what is the definition of a calorie

A

heat needed to raise the temperature by 1C of 1 g

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45
Q

C to K conversion

A

K = C +273

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46
Q

C to F conversion

A

F = 1.8C +32

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47
Q

equation for specific heat

A

q / (mass)(change in temp)

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48
Q

q in specific heat equation

A

heat transfered

metric = calories
SI = joules

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49
Q

mass in specific heat equation

A

grams

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50
Q

change in temperature in specific heat equation

A

Celsius

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51
Q

metals vs nonmetals

A

metals:
conductors
malleable / ductile
shiny

nonmetals:
not conductors
not malleable or ductile
brittle

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52
Q

metalloids

A

in between properties of metals and nonmetals

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53
Q

groups of periodic table

A

alkali metals
alkaline earth metals
transition elements
halogens
noble gases

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54
Q

what is the smallest unit of an element

A

an atom

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55
Q

protons

A

positive charge
inside nucleus
1 amu

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56
Q

who discovered proton

A

ruther ford
gold foil experiment
(atom is mostly empty space)

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57
Q

neutrons

A

neutral charge
inside nucleus
1 amu

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58
Q

who discovered neutron

A

chadwick

59
Q

electrons

A

negative charge
in energy shells
1/2000 of an amu

60
Q

who discovered electron

A

jj thompson
cathode ray

61
Q

atomic number

A

number of protons and electrons

62
Q

atomic mass

A

average weight of all isotopes

63
Q

mass #

A

number of protons and neutrons

64
Q

isotopes have same / different what

A

same P
different N

65
Q

how to calculate atomic mass

A

(mass x abundance) + (mass x abundance)
for all isotopes

66
Q

how many energy levels are there

A

7

67
Q

higher energy level = ____ energy

A

higher

68
Q

how many sublevels are there

A

4
s,p,d,f

69
Q

how many orbitals does s have

A

1

70
Q

how many orbitals does p have

A

3

71
Q

how many orbitals does d have

A

5

72
Q

how many orbitals does f have

A

7

73
Q

how many electrons are in orbitals

A

2 in each orbital

74
Q

what is an orbital

A

space where probability is high to find electrons

75
Q

electron configuration

A

coefficient
letter
superscript

76
Q

what does coefficient of electron configuration mean

A

energy level

77
Q

what does letter of electron configuration mean

A

sublevel

78
Q

what does superscript of electron configuration mean

A

number of electrons in the sublevel

79
Q

valence electrons

A

electrons in outermost energy level

80
Q

how to determine valence electrons

A

electron configuration
(count electrons in last energy level — coefficient)
group number

81
Q

electron dot symbol

A

lewis structure
indicates valence electrons as dots

82
Q

atomic radii across a period

A

decreases

83
Q

atomic radii down a group

A

increases

84
Q

ionization energy across a period

A

increases

85
Q

ionization energy down a group

A

decreases

86
Q

metallic character across a period

A

decreases

87
Q

metallic character down a group

A

increases

88
Q

reason for atomic trends across a period

A

increase in protons increases the effective nuclear charge

89
Q

reason for atomic trends down a group

A

increase in energy levels

90
Q

zeff =

A

Z - S
total electrons - shielding electrons (nonvalence)

91
Q

ionic compound

A

metal + nonmetal
loss / gain of electrons

92
Q

covalent compound

A

nonmetal + nonmetal
sharing of electrons

93
Q

cation

A

positive ion
loss of electrons

94
Q

anion

A

negative ion
gain electrons

95
Q

cations size

A

cations = smaller than atoms

more P compared to E means stronger pull on Es

96
Q

anions size

A

anions = larger than atom

more electrons = weaker pull

97
Q

name for ionic compounds

A

M + NM
metal = name
nonmetal = name end with “ide”

98
Q

metals with variable change

A

most transition elements + Tin and Lead

99
Q

name for metals with variable change

A

same as regular ionic compounds
add roman numeral to metal to clarify which ion it forms

100
Q

polyatomic ions

A

2+ atoms with a charge

101
Q

name for polyatomic ions

A

metal = name
ion = name ending with “ate”

102
Q

ite

A

polyatomic ion with 1 less O

103
Q

hydro - ous

A

polyatomic ion with 2 less O

104
Q

per

A

polyatomic ion with 1 more O

105
Q

hydrogen OR bi

A

polyatomic ion with 1 more H+

106
Q

carbonate

A

CO3 -2

107
Q

sulfate

A

SO4 -2

108
Q

phosphate

A

PO4 3-

109
Q

nitrate

A

NO3 -1

110
Q

chlorate

A

ClO3 -1

111
Q

fluroate

A

FO3 -1

112
Q

iodate

A

IO3 -1

113
Q

bromate

A

BrO3 -1

114
Q

hydroxide

A

OH -1

115
Q

ammonium

A

NH4 +1

116
Q

name for covalent compounds

A

NM + NM
1st = name
2nd = name ending it “ide”

prefixes describe number of each (no charge)

117
Q

prefixes for covalent compounds

A

mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca

118
Q

states of ionic vs covalent

A

ionic = s at room temp
covalent = l / g at room temp

119
Q

bonds in ionic compounds

A

ionic bonds

120
Q

bonds in covalent compounds

A

intermolecular forces:

hydrogen
dipole-dipole
london dispersion forces

121
Q

hydrogen bonds

A

POLAR
intermolecular forces between H & very electronegative atom

hydrogen + NOF
N, O, F

122
Q

dipole-dipole forces

A

POLAR
second strongest

123
Q

dispersion forces

A

NONPOLAR
weakest

124
Q

vsepr steps

A

1.) lewis dot structure
2.) delta EN
3.) polarity, geometry, shape

125
Q

geometry: 2 groups around central atom

A

linear

126
Q

linear geometry:
2 groups bonded
1 group bonded

A

linear
linear

127
Q

geometry: 3 groups around central atom

A

trigonal planar

128
Q

trigonal planar geometry:
3 groups bonded
2 groups bonded
1 group bonded

A

trigonal planar
bent
linear

129
Q

geometry: 4 groups around central atom

A

tetrahedral

130
Q

tetrahedral geometry:
4 groups bonded
3 groups bonded
2 groups bonded

A

tetrahedral
trigonal pyramidal
bent

131
Q

what is a “group” in vsepr

A

atom with bond
lone electron pair

(single, double, and triple bonds are all considered 1)

132
Q

nonpolar electronegativity

A

0 - 0.4

133
Q

polar electronegativity

A

0.5 - 1.8

134
Q

ionic electronegativity

A

1.8 +

135
Q

arrows in lewis structure go which way

A

arrows point towards more electronegative atom
represents a dipole

136
Q

what is a dipole in lewis structure

A

arrow that points towards more electronegative atom

137
Q

if bonds are nonpolar, molecule is ___

A

ALWAYS nonpolar

138
Q

if bonds are polar, molecule is ___

A

polar OR nonpolar

if dipoles cancel out based on geometry, its NP, if not its polar

139
Q

when do atoms become partially positive or negative

A

covalent bonds

the atom that keeps electrons most of the time becomes partially negative
others become partially positive

140
Q

transition elements that do NOT have variable change

A

Silver (+1)
Zinc (+2)
Cadmium (+2)

141
Q

Zinc ion charge

A

+2

142
Q

Cadmium ion charge

A

+2

143
Q

Silver ion charge

A

+1

143
Q

Silver ion charge

A

+1

Chem 120 (2 decks)

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