Exam Review Flashcards
(113 cards)
1
Q
avogadro’s constant
A
NA = 6.02 x 10^23
2
Q
n
A
amount of a substance; unit moles
3
Q
m
A
mass; unit grams
4
Q
M
A
molar mass; unit g/mol
5
Q
N
A
number of entities
6
Q
brownian motion
A
the random movement of microscopic particles suspended in a liquid or gas
7
Q
kinetic molecular theory
A
idea that all substances are composed of entities that are in constant, random motion
8
Q
SI unit for pressure
A
1 Pa = 1 N/m^2
9
Q
STP
A
- standard temp and pressure
- 0 degrees Celsius & 101.325 kPa
10
Q
SATP
A
- standard ambient temp and pressure
- 25 degrees Celsius & 100 kPa
11
Q
T
A
temp in Kelvin
12
Q
t
A
temp in degrees Celsius
13
Q
V
A
Volume
14
Q
P
A
pressure in kPa
15
Q
law of combining volumes
A
gases always react to produce products in whole number ratios
16
Q
avogadro’s law
A
the volume of a gas is directly related to the amount of the gas when temp and pressure are constant
17
Q
molar volume
A
volume that one mole of gas occupies at a certain temp and pressure
18
Q
R
A
- universal gas constant that relates to pressure volume, amount, & temp
- 8.314 kPa L/ mol K
19
Q
metric conversion
A
G –M–khda BASE dcm–u–n
20
Q
mole, mass and molar mass equation
A
- n = m/M
- mol to mass = x g/1 mol
- mass to mol = 1 mol/x g
21
Q
number of entities equation
A
- N = nNA
- mol to entities = 6.02 x 10^23/ 1 mol
- entities to mol = 1 mol/ 6,02 x 10^23 entities
22
Q
temp equation
A
T = t + 273
23
Q
charles law
A
V1/T1 = V2/T2
24
Q
Boyle’s law
A
P1V1 = P2V2
25
Gay-lussac's Law
P1/T1 = P2/T2
26
combined gas law
P1V1/T1 = P2V2/T2
27
Avogadro's law equation
V1/n1 = V2/n2
28
ideal gas law
PV = nRT
29
density
m/V
30
radioactive decay
the spontaneous disintegration of unstable isotopes
31
nuclear radiation
energy or very small particles emitted from the nucleus of a radioisotope as it decays
32
alpha particle
- a product of nuclear decay emitted by certain radioisotopes
- positively charged particle with the same structure as the nucleus of a helium atom
33
beta particle
- a product of nuclear decay emitted by a certain radioisotopes
- a negatively charged particle identical to an electron
34
gamma ray
form of high-energy electromagnetic radiation emitted by certain radioisotopes
35
radioisotope
an isotope that spontaneously decays to produce two or more smaller nuclei and radiation
36
radioactive
having the potential to emit nuclear radiation upon decay
37
atomic mass given isotopic abundance equation
atomic mass = % abundance of isotope 1 (mass of isotope 1) + abundance of isotope 2 (mass of isotope 2) ....
38
column of periodic table
group
39
row of periodic table
period
40
atomic radius
- measurement of the size of an atom
- unit is picometers (pm)
41
effective nuclear charge
net force experienced of an electron in an atom due to positively charged nucleus
42
ionic radius
- measurement of the size of an ion
- unit is picometers (pm)
43
ionization energy
quantity of energy required to remove an electron from an atom or ion in a gaseous state
44
electron affinity
the energy change that occurs when an electron is added to a neutral atom in the gaseous state
45
electronegativity
ability of an atom to attract bonding electrons to itself
46
electronegativity difference
- difference in electronegativities of two bonded atoms or ions
- EN > = 1.7 is ionic
- EN < 1.7 is a covalent bond
47
non polar covalent bond
covalent bond formed between atoms with identical (or very similar) electronegativities
- EN = 0
48
polar covalent bonds
a covalent bond
formed between atoms with signifi cantly
different electronegativities resulting in a
bond with localized positive and negative
charges or poles
- 0
49
oxyanion
negatively charged polyatomic ion that has oxygen
50
hydrate
ionic compound that contains water as part of its crystal structure
51
intermolecular force
attraction between molecules
52
dipole-dipole force
an intermolecular
force of attraction that forms between the
slightly positive end of one polar molecule
and the slightly negative end of another polar molecule
53
london dispersion force
weak attraction force acting between all entities caused by temporary imbalance of electrons within entities
54
van der Waals forces
weak forces of attraction between molecules
including dipole-dipole and london dispersion forces
55
hydrogen bonds
unusually strong dipole-dipole force between a hydrogen atom attached to N, O, F and another N, O or F molecule
56
surface tension
caused by forces of attraction between molecules that leads to the formation of skin like film on the surface of a liquid
57
precipitate
a solid produced as a result of the reaction of two solutions
58
catalyst
a substance that makes a chemical reaction occur faster without itself being consumed in the reaction
59
law of conservation of mass
during a reaction the total mass of reactants equals the total mass of products
60
activity series
list of elements arranged in order of their observed reactivity in single displacement reactions
61
solubility
quantity of solute that dissolves in a given quantity of solvent at a given temp
62
complete combustion
hydrocarbon and oxygen produces carbon dioxide, water and energy
63
incomplete combustion
hydrocarbon and oxygen might produce carbon dioxide, carbon monoxide, soot, water, and energy
64
oxide
compound made of oxygen and another element
65
acidic oxide
oxide that forms an
acidic solution when dissolved in water; a
non-metallic oxide
66
basic oxide
oxide that forms a basic
solution when dissolved in water; a
metallic oxide
67
qualitative analysis
identifying substances present in a
sample; no measurements are involved
68
quantitative analysis
measuring the quantity of a substance in a
sample, providing numerical data
69
percentage composition equation
% element = m element/ m sample x 100%
70
law of definite proportions
a compound always contains the same proportion of elements by mass
71
molecular formula equation
x = M of compound / M of empirical formula
72
limiting reagent
- reactant that is
completely consumed in a chemical
reaction
- reactant that determines how
much product will be formed
73
excess reagent
reactant that is still
present after the reaction is complete
74
theoretical yield
eamount or mass
of product predicted based on the chemical equation
75
actual yield
amount or mass of
product actually collected
76
percent yield equation
actual yield / theoretical yield x 100%
77
transpiration
evaporation of water
from the leaves of a plant
78
aquifer
layer of underground rock that hold a large amount of water
79
heterogeneous mixture
contains two or more phases
80
concentration
ratio of the quantity of
solute to the quantity of solution or solvent
81
concentrated solution
solution with a relatively large quantity of solute dissolved
per unit volume of solution
82
dilute solution
a solution with a relatively
small quantity of solute dissolved per unit
volume of solution
83
alloy
solution of two or more metals
84
amalgam
an alloy (solution) of mercury with other metals
85
hydration
process in which ions are surrounded by water molecules
86
dissociation
separation of individual
ions from an ionic compound as it
dissolves in water
87
miscible
able to mix to form a solution
88
immiscible
unable to mix to form a
solution
89
saturated solution
solution that
contains the maximum quantity of solute
at a given temperature and pressure
90
unsaturated solution
a solution in
which more solute can dissolve at a given
temperature and pressure
91
supersaturated solution
solution
that contains more than the maximum
quantity of solute that it should at a given
temperature and pressure
92
solubility curve
a graph of the
solubility of a substance over a range
of temperatures
93
amount concentration equation
c = n of solute / V of solution
94
amount concentration (c)
amount (in moles) of solute dissolved per litre of
solution; unit symbol mol/L
95
dilution equation
ccVc = cdVd
96
percent concentration equation
c = quantity of solute / quantity of solvent
- % V/V
- % W/V
- % W/W
97
parts per gram concentration equation
cppm = m solute / m solvent x 10^6
98
total ionic equation
chemical equation in which all highly soluble ionic
compounds are written as dissociated ions
99
spectator ions
ions that are not involved in a chemical reaction
100
net ionic equation
a chemical equation that includes only the entities that react
during the reaction
101
filtrate
clear liquid (solvent and any dissolved substances) collected after a
mixture is filtered to remove any solid
components
102
flame test
diagnostic test used to identify a specific element
103
Bronsted - lowry theory of acids and bases
- acids are substances that can provide a proton for another substance
- bases are substances that can receive a proton from another substance
104
conjugate acids and bases
- base is the particle remains once an acid releases a proton
- acid is the particle that results when the base accept a proton
105
strong acid
- substance that ionizes completely in water; strong acids have
strong acidic properties
- eg. low pH and high reactivity
106
weak acid
- a substance that only partially ionizes in water
- e.g., moderate pH and
mild reactivity)
107
titration
procedure used to determine
the concentration of a solution using a
standardized solution
108
equivalence point
point in a titration
when neutralization is complete
109
endpoint
- point during a titration
when a sudden change in an observable
property of the solution occurs
- usually a
change in colour of an acid–base indicator
or a significant change in pH
110
a name of an indicator
methyl red
thymol blue
111
ideal gas
a hypothetical gas composed
of particles that have no size, travel in
straight lines, and have no intermolecular forces
112
partial pressure
pressure that a gas
in a mixture would exert if it were the only
gas present in the same volume and at the
same temperature
113
dalton's law of partial pressures
- the total pressure of a
mixture of non-reacting gases is equal
to the sum of the partial pressures of the
individual gases
- P total = P1 + P2 +.....
