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Chemistry Final
Chemistry Final
115 terms
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A #Chemistry final to review for cumulative exam
Flashcards
115 cards
F
Practice quiz
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Host live
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Questions
115
Answers
1
Why did chemistry develop over time?
explore the nature of the atom
create art
meet people's needs
satisfy curiosity
2
gas to solid
deposition
condensation
evaporation
boiling
3
# of oxygen atoms in 3H
2
O
1
6
3
2
4
charge of an proton
positive
negative
neutral
5
intermolecular forces that form only between polar molecules
hydrogen bonds
ionic bonds
dispersion forces
dipole-dipole
6
liquid to gas when vapor pressure equals atmospheric pressure
evaporation
boiling
condensation
vaporization
7
water
solid
liquid
gas
plasma
8
Creation Mandate
Matthew
Genesis
Exodus
Psalms
9
(
l
)
"yields" or "produces"
liquid reactant or product
solid reactant or product
substance is dissolved in water
10
charge of a neutron
neutral
negative
positive
11
constant volume of gas, increase temperature -> pressure will
increase
decrease
12
2H
2
O + 234.7 kJ → 2H
2
+ O
2
exothermic
endothermic
13
qualitative data
mass
length
temperature
color
14
reason for the ability of gasses to be squeezed into smaller volumes
expansible
elastic
permeable
compressible
15
charge of an electron
positive
neutral
negative
16
physical property
compound exploding
metal being hammered into a sheet
metal rusting
chemical reacting with water
17
(
s
)
"yields" or "produces"
substance is dissolved in water
solid reactant or product
liquid reactant or product
18
direct change from solid to gas
boiling
sublimation
adhesion
cohesion
19
Avogadro's number
6.22 x 1023
6.022 x 1023
6.023 x 1022
6.23 x 1022
20
↓
substance dissolved in water
solid reactant or product
precipitate
liquid reaction or product
21
metal that is liquid at room temperature
magnesium
barium
lithium
mercury
22
elements with larger atomic numbers than uranium
posturanium
hyperuranium
transuranium
suburanium
23
any change from liquid to gas
sublimation
boiling
evaporation
vaporization
24
charged atom
isotope
element
compound
ion
25
charge of an electron
positive
neutral
negative
26
branch of science that studies the transfer of energy during chemical reactions
thermodynamics
thermochemistry
chemokinetics
thermokinetics
27
minimum amount of kinetic energy for a reaction to occur
reaction order
activation energy
reaction mechanism
activated complex
28
gas has the ability to take the shape of its container
effusion
effusion
fluidity
diffusion
29
subatomic particle with the most mass
proton
neutron
electron
30
mixture of atoms from multiple metals that has metal properties
alloy
electron sea
network
metalloid
31
mass of 4.5 moles of carbon atoms (C=16.00)
54.0 g
45.0 g
49.3 g
54.4 g
32
neutrons + protons
atomic mass
atomic number
atomic mass unit
mass number
33
dust
plasma
gas
liquid
solid
34
study of the rates of reactions and the steps by which they occur
reaction order
kinetics
activation energy
reaction rate
35
PV = nRT
ideal gas law
combined gas law
Avogadro's law
Gay-Lussac's law
36
perspective from which we see & interpret life
hypothesis
worldview
model
reasoning
37
collection of gas by water displacement requires adjusting for
atmospheric pressure
water pressure
vapor pressure
partial pressure
38
chemical property
metal rusting
chemical reacting with water
metal being hammered into a sheet
compound exploding
39
gas can be squeezed into a smaller volume
diffusion
effusion
compressibility
effusion
40
number of electrons with a full
s
and
p
sublevel in the first energy level
8
2
10
3
41
O
2
heterogeneous mixture
polyatomic element
monatomic element
diatomic element
42
solution with 2 substances - the component with the smaller amount
solvent
solute
43
sodium iodide
NaIO
NaI
NaIO2
NaIO3
44
→ with Δ above it
indicates a precipitate
heat needs to be applied for the reaction to occur
a substance dissolved in water
"yields" or "produces"
45
solution that contains the same amount of dissolved solute that normally occurs at equilibrium
saturated
unsaturated
hypersaturated
supersaturated
46
→
heat needs to be applied for the reaction
precipitate
substance dissolved in water
"yields" or "produces"
47
maximum number of electrons in an orbital
8
4
2
1
48
greatest number of steps to convert
moles of a reactant to moles of a product
grams of a reactant to moles of a product
moles of a reactant to grams of a product
grams of a reactant to grams of a product
49
strongest
can't tell
double bond
triple bond
single bond
50
determines polarity of a polar bond
difference in bond angles
difference in bond types
difference in electronegativity
difference in group numbers
51
lowest density
gas
solid
liquid
52
P
2
O
2
diphosphorous dioxide
biphosphorus bioxide
phosphorous oxide
diphosphorus dioxygen
53
solid to liquid
condensation
evaporation
sublimation
melting
54
(
g
)
"yields" or "produces"
substance is dissolved in water
liquid reactant or product
gaseous reactant or product
55
constant quantity of gas, decrease volume -> pressure will
decrease
increase
56
a valid element
Cs
CL
C
Cu
57
HCl (
aq
)
hydrochloric acid
hydrogen chloride
hydrogen monochloride
hydrogen monochlorate
58
a mole of water = ? hydrogen atoms & ? oxygen atoms
two moles / one mole
one mole / one mole
one mole / two moles
two moles / two moles
59
tri-
5
3
4
6
60
a substance that changes a reaction rate without being permanently changed or consumed
enzyme
activated complex
catalyst
inhibitor
61
measure of an atom's ability to attract electrons
polarity
electron affinity
electronegativity
ionization energy
62
tetra-
3
6
5
4
63
gas moves through a tiny opening into an evacuated chamber
expansibility
effusion
diffusion
effusion
64
attraction of particles of a liquid to the particles of another material
sublimation
cohesion
adhesion
boiling
65
Fe
monatomic element
heterogeneous mixture
polyatomic element
compound
66
comparing an unknown quantity to a standard unit
dimension
derivation
graduation
measurement
67
solution with 2 substances - the component with the larger amount
solute
solvent
68
one measurement increases and the other increases
inverse
direct
69
quantitative data
mass
color
temperature
length
70
gas quickly expands to fill a low pressure region
effusion
expansibility
diffusion
effusion
71
reason atoms bond
gain stability, lose energy
share electrons
transfer electrons
lose stability, gain energy
72
solution that contains more dissolved solute than normally occurs at equilibrium
saturated
supersaturated
hypersaturated
unsaturated
73
lightest element in the universe
silicon
hydrogen
sulfur
helium
74
penta-
5
4
6
3
75
digits considered significant in a measurement
positive
nonzero
estimated
negative
76
liquid to solid
boiling
freezing
condensation
deposition
77
type of data significant digits apply to
pure
measured
counted
defined
78
fulfills the Creation Mandate
breeding disease-resistant plants
developing a malaria vaccine
abortion
creating stain-resistant fabrics
79
temperature scale to be used when calculating gas law equations
F
K
A
C
80
Z
electrons
neutrons
neutrons and protons
protons
81
hexa-
6
3
5
4
82
semiconductors
halogens
transition metals
metals
metalloids
83
a piece of lead weighs more than a piece of foam twice the size
density
ductility
conductivity
malleability
84
central atom in a Lewis structure
most unpaired electrons
with the most electrons
greatest electronegativity
metal
85
attraction of particles of a liquid to the particles of the same material
adhesion
cohesion
boiling
sublimation
86
air
colloid
suspension
compound
solution
87
fraction equal to 1 that contains the original unit and its equivalent value in a new unit
conversion factor
derived unit
pure number
exponential factor
88
unit for molar mass
g/mol
u/mol
kg/mol
mol/mol
89
created out of nothing
ex nihilo
ad nimo
ab hilexa
ex integra
90
11200 grams
11.2 kilograms
11.20 kilograms
112 kilograms
112.0 kilograms
91
structure of a diamond
ionic crystal
covelent molecular crystal
covalent network crystal
atomic crystal
92
molar mass of C
6
(H
12
O
6
)
2
(C=12.00, H=1.008, O=16.00)
174.0 g
324.5 g
180.1 g
288.2 g
93
constant quantity of gas, decrease temperature -> volume will
decrease
increase
94
solution that contains less dissolved solute than normally occurs at equilibrium
hypersaturated
supersaturated
unsaturated
saturated
95
conditions necessary for a reaction to occur
proper orientation of collision
sufficient force
proper temperature
sufficient pressure
96
(
aq
)
substance is dissolved in water
gaseous reactant or product
"yields" or "produces"
liquid reactant or product
97
solution
homogeneous compound
heterogeneous mixture
homogeneous mixture
heterogeneous compound
98
maximum amount of product created from a given amount of reactant
theoretical yield
empirical yield
percent yield
actual yield
99
change in temperature while ice is melting
no change
rises
falls
100
oxygen
plasma
solid
liquid
gas
101
temperature and pressure combination where water can exist in any state
fiduciary point
triple point
liquid-solid point
critical temperature
102
subatomic particle with the least mass
neutron
electron
proton
103
number of neutrons
14
6
20
8
104
hydrogen bonds form between hydrogen and
bromine
oxygen
carbon
sulfur
105
22.4 L at STP
standard volume
combining volume
absolute volume
molar volume
106
ratio of water to oxygen in 2 H
2
+ O
2
--> 2 H
2
O
1:1
2:2
1:2
2:1
107
one measurement increases and the other decreases
direct
inverse
108
general rule for substances the form solutions
unlike dissolves unlike
like dissolves like
unlike dissolves like
like dissolves unlike
109
property of gases that explains the smell of fish spread through a refrigerator
compressibility
elasticity
permeability
expansibility
110
P
4
monatomic element
diatomic element
polyatomic element
heterogeneous mixture
111
least number of steps to convert
moles of a reactant to moles of a product
grams of a reactant to grams of a product
moles of a reactant to grams of a product
grams of a reactant to moles of a product
112
H
2
O
2
polyatomic element
diatomic element
heterogeneous mixture
compound
113
uniform mixing and spreading of gases over time
osmosis
pressure
diffusion
expansibility
114
gas easily mingles with another porous substance
expansibility
effusion
diffusion
permeability
115
average kinetic energy in the particles of a substance
heat
temperature
enthalpy
entropy
