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Chem Grade 11 > Exam Review > Flashcards

Exam Review Flashcards

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1
Q

avogadro’s constant

A

NA = 6.02 x 10^23

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2
Q

n

A

amount of a substance; unit moles

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3
Q

m

A

mass; unit grams

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4
Q

M

A

molar mass; unit g/mol

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5
Q

N

A

number of entities

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6
Q

brownian motion

A

the random movement of microscopic particles suspended in a liquid or gas

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7
Q

kinetic molecular theory

A

idea that all substances are composed of entities that are in constant, random motion

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8
Q

SI unit for pressure

A

1 Pa = 1 N/m^2

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9
Q

STP

A
  • standard temp and pressure
  • 0 degrees Celsius & 101.325 kPa
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10
Q

SATP

A
  • standard ambient temp and pressure
  • 25 degrees Celsius & 100 kPa
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11
Q

T

A

temp in Kelvin

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12
Q

t

A

temp in degrees Celsius

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13
Q

V

A

Volume

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14
Q

P

A

pressure in kPa

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15
Q

law of combining volumes

A

gases always react to produce products in whole number ratios

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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

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17
Q

molar volume

A

volume that one mole of gas occupies at a certain temp and pressure

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18
Q

R

A
  • universal gas constant that relates to pressure volume, amount, & temp
  • 8.314 kPa L/ mol K
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19
Q

metric conversion

A

G –M–khda BASE dcm–u–n

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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
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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
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22
Q

temp equation

A

T = t + 273

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23
Q

charles law

A

V1/T1 = V2/T2

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24
Q

Boyle’s law

A

P1V1 = P2V2

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25
Q

Gay-lussac’s Law

A

P1/T1 = P2/T2

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26
Q

combined gas law

A

P1V1/T1 = P2V2/T2

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27
Q

Avogadro’s law equation

A

V1/n1 = V2/n2

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28
Q

ideal gas law

A

PV = nRT

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29
Q

density

A

m/V

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30
Q

radioactive decay

A

the spontaneous disintegration of unstable isotopes

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31
Q

nuclear radiation

A

energy or very small particles emitted from the nucleus of a radioisotope as it decays

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32
Q

alpha particle

A
  • a product of nuclear decay emitted by certain radioisotopes
  • positively charged particle with the same structure as the nucleus of a helium atom
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33
Q

beta particle

A
  • a product of nuclear decay emitted by a certain radioisotopes
  • a negatively charged particle identical to an electron
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34
Q

gamma ray

A

form of high-energy electromagnetic radiation emitted by certain radioisotopes

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35
Q

radioisotope

A

an isotope that spontaneously decays to produce two or more smaller nuclei and radiation

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36
Q

radioactive

A

having the potential to emit nuclear radiation upon decay

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37
Q

atomic mass given isotopic abundance equation

A

atomic mass = % abundance of isotope 1 (mass of isotope 1) + abundance of isotope 2 (mass of isotope 2) ….

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38
Q

column of periodic table

A

group

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39
Q

row of periodic table

A

period

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40
Q

atomic radius

A
  • measurement of the size of an atom
  • unit is picometers (pm)
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41
Q

effective nuclear charge

A

net force experienced of an electron in an atom due to positively charged nucleus

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42
Q

ionic radius

A
  • measurement of the size of an ion
  • unit is picometers (pm)
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43
Q

ionization energy

A

quantity of energy required to remove an electron from an atom or ion in a gaseous state

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44
Q

electron affinity

A

the energy change that occurs when an electron is added to a neutral atom in the gaseous state

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45
Q

electronegativity

A

ability of an atom to attract bonding electrons to itself

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46
Q

electronegativity difference

A
  • difference in electronegativities of two bonded atoms or ions
  • EN > = 1.7 is ionic
  • EN < 1.7 is a covalent bond
47
Q

non polar covalent bond

A

covalent bond formed between atoms with identical (or very similar) electronegativities
- EN = 0

48
Q

polar covalent bonds

A

a covalent bond
formed between atoms with signifi cantly
different electronegativities resulting in a
bond with localized positive and negative
charges or poles
- 0<EN<1.7

49
Q

oxyanion

A

negatively charged polyatomic ion that has oxygen

50
Q

hydrate

A

ionic compound that contains water as part of its crystal structure

51
Q

intermolecular force

A

attraction between molecules

52
Q

dipole-dipole force

A

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
Q

london dispersion force

A

weak attraction force acting between all entities caused by temporary imbalance of electrons within entities

54
Q

van der Waals forces

A

weak forces of attraction between molecules
including dipole-dipole and london dispersion forces

55
Q

hydrogen bonds

A

unusually strong dipole-dipole force between a hydrogen atom attached to N, O, F and another N, O or F molecule

56
Q

surface tension

A

caused by forces of attraction between molecules that leads to the formation of skin like film on the surface of a liquid

57
Q

precipitate

A

a solid produced as a result of the reaction of two solutions

58
Q

catalyst

A

a substance that makes a chemical reaction occur faster without itself being consumed in the reaction

59
Q

law of conservation of mass

A

during a reaction the total mass of reactants equals the total mass of products

60
Q

activity series

A

list of elements arranged in order of their observed reactivity in single displacement reactions

61
Q

solubility

A

quantity of solute that dissolves in a given quantity of solvent at a given temp

62
Q

complete combustion

A

hydrocarbon and oxygen produces carbon dioxide, water and energy

63
Q

incomplete combustion

A

hydrocarbon and oxygen might produce carbon dioxide, carbon monoxide, soot, water, and energy

64
Q

oxide

A

compound made of oxygen and another element

65
Q

acidic oxide

A

oxide that forms an
acidic solution when dissolved in water; a
non-metallic oxide

66
Q

basic oxide

A

oxide that forms a basic
solution when dissolved in water; a
metallic oxide

67
Q

qualitative analysis

A

identifying substances present in a
sample; no measurements are involved

68
Q

quantitative analysis

A

measuring the quantity of a substance in a
sample, providing numerical data

69
Q

percentage composition equation

A

% element = m element/ m sample x 100%

70
Q

law of definite proportions

A

a compound always contains the same proportion of elements by mass

71
Q

molecular formula equation

A

x = M of compound / M of empirical formula

72
Q

limiting reagent

A
  • reactant that is
    completely consumed in a chemical
    reaction
  • reactant that determines how
    much product will be formed
73
Q

excess reagent

A

reactant that is still
present after the reaction is complete

74
Q

theoretical yield

A

eamount or mass
of product predicted based on the chemical equation

75
Q

actual yield

A

amount or mass of
product actually collected

76
Q

percent yield equation

A

actual yield / theoretical yield x 100%

77
Q

transpiration

A

evaporation of water
from the leaves of a plant

78
Q

aquifer

A

layer of underground rock that hold a large amount of water

79
Q

heterogeneous mixture

A

contains two or more phases

80
Q

concentration

A

ratio of the quantity of
solute to the quantity of solution or solvent

81
Q

concentrated solution

A

solution with a relatively large quantity of solute dissolved
per unit volume of solution

82
Q

dilute solution

A

a solution with a relatively
small quantity of solute dissolved per unit
volume of solution

83
Q

alloy

A

solution of two or more metals

84
Q

amalgam

A

an alloy (solution) of mercury with other metals

85
Q

hydration

A

process in which ions are surrounded by water molecules

86
Q

dissociation

A

separation of individual
ions from an ionic compound as it
dissolves in water

87
Q

miscible

A

able to mix to form a solution

88
Q

immiscible

A

unable to mix to form a
solution

89
Q

saturated solution

A

solution that
contains the maximum quantity of solute
at a given temperature and pressure

90
Q

unsaturated solution

A

a solution in
which more solute can dissolve at a given
temperature and pressure

91
Q

supersaturated solution

A

solution
that contains more than the maximum
quantity of solute that it should at a given
temperature and pressure

92
Q

solubility curve

A

a graph of the
solubility of a substance over a range
of temperatures

93
Q

amount concentration equation

A

c = n of solute / V of solution

94
Q

amount concentration (c)

A

amount (in moles) of solute dissolved per litre of
solution; unit symbol mol/L

95
Q

dilution equation

A

ccVc = cdVd

96
Q

percent concentration equation

A

c = quantity of solute / quantity of solvent
- % V/V
- % W/V
- % W/W

97
Q

parts per gram concentration equation

A

cppm = m solute / m solvent x 10^6

98
Q

total ionic equation

A

chemical equation in which all highly soluble ionic
compounds are written as dissociated ions

99
Q

spectator ions

A

ions that are not involved in a chemical reaction

100
Q

net ionic equation

A

a chemical equation that includes only the entities that react
during the reaction

101
Q

filtrate

A

clear liquid (solvent and any dissolved substances) collected after a
mixture is filtered to remove any solid
components

102
Q

flame test

A

diagnostic test used to identify a specific element

103
Q

Bronsted - lowry theory of acids and bases

A
  • acids are substances that can provide a proton for another substance
  • bases are substances that can receive a proton from another substance
104
Q

conjugate acids and bases

A
  • base is the particle remains once an acid releases a proton
  • acid is the particle that results when the base accept a proton
105
Q

strong acid

A
  • substance that ionizes completely in water; strong acids have
    strong acidic properties
  • eg. low pH and high reactivity
106
Q

weak acid

A
  • a substance that only partially ionizes in water
  • e.g., moderate pH and
    mild reactivity)
107
Q

titration

A

procedure used to determine
the concentration of a solution using a
standardized solution

108
Q

equivalence point

A

point in a titration
when neutralization is complete

109
Q

endpoint

A
  • 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
Q

a name of an indicator

A

methyl red
thymol blue

111
Q

ideal gas

A

a hypothetical gas composed
of particles that have no size, travel in
straight lines, and have no intermolecular forces

112
Q

partial pressure

A

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
Q

dalton’s law of partial pressures

A
  • 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 +…..

Chem Grade 11 (1 decks)

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