Sch4U Final Examination

Front 1

photon

Back 1

a quantum of electromagnetic radiation

Front 2

Heisenberg uncertainty pronciple

Back 2

there is a “fundamental limitation to just how precisely we can know both the position and the momentum of a particle at a given time”

Front 3

electron configuration

Back 3

representation of the arrangement of electrons within the energy levels and orbitals of an atom

Front 4

Aufbau principle

Back 4

Each additional electron that is added to an electron configuration must occupy the lowest available orbital

Front 5

Hund's Rule

Back 5

Electrons must be distributed amongst orbitals of equal energy in such a way that as many electrons as possible remain unpaired, with parallel spins.

Front 6

Pauli exclusion principle

Back 6

No two electrons within an atom can have the same set of four quantum numbers

Front 7

principle quantum number

Back 7

represents the main energy level of the electron and has a whole number value, i.e. n = 1, n = 2, etc.

Front 8

angular momentum quantum number

Back 8

has integral values from zero to n – 1 for each value of n. This number describes the type of orbital (s, p, d, or f) in which the electron is found.

Front 9

magnetic quantum number

Back 9

has integral values between –l and +l, and describes the sublevel within each orbital type in which the electron is found

Front 10

spin quantum number

Back 10

describes the orientation of the electron within a particular orbital, is given the value of +1/2 or -1/2

Front 11

electronegativity

Back 11

a measure of the tendency of an atom to attract a bonding pair of electrons

Front 12

dipole moment

Back 12

property of a molecule whose charge distribution can be represented by a centre of positive charge and a centre of negative charge

Front 13

intermolecular forces

Back 13

force of attraction between two individual molecules or ions

Front 14

intramolecular forces

Back 14

force of attraction between two atoms or ions within a molecule

Front 15

VSEPR theory

Back 15

theory that predicts the basic shape of molecules

Front 16

van der Waals force or London dispersion force

Back 16

weak intermolecular force, typically occurring between molecules that contain non-polar bonds

Front 17

induced dipole

Back 17

a temporary shift in the electron density of a bond within a molecule, resulting in a weak intermolecular force

Front 18

ionic bond

Back 18

electrostatic force of attraction between positive and negative ions

Front 19

covalent bond

Back 19

bond resulting from the sharing of pairs of electrons between two atoms

Front 20

polar

Back 20

bond in which the electrons are shared unequally

Front 21

non-polar bond

Back 21

bond in which the electrons are shared equally

Front 22

resonance

Back 22

a state that occurs when more than one valid Lewis structure can be written for a particular molecule

Front 23

formal charge

Back 23

the difference between the number of valence electrons on the free atom and the number of valence electrons assigned to the atom in the molecule.

Front 24

localized electrons

Back 24

electrons that are fixed between two atoms

Front 25

delocalized electrons

Back 25

electrons that are free to move about the entire structure of a molecule

Front 26

phase diagram

Back 26

A convenient way of representing the phases of a substance in a
closed system as a function of temperature (x-axis) and pressure (y-axis)

Front 27

sublimation curve

Back 27

line on a phase diagram separating the solid phase from the gas phase

Front 28

melting curve

Back 28

line on a phase diagram separating the solid phase from the liquid phase

Front 29

vaporization curve

Back 29

line on a phase diagram separating the liquid phase from the gas
phase

Front 30

critical temperature

Back 30

the temperature above which a vapour cannot be liquefied, no
matter what pressure is applied

Front 31

critical pressure

Back 31

the minimum pressure required to liquefy a substance at the critical
temperature (there is no maximum because it does not matter if the pressure goes above
this minimum)

Front 32

critical point

Back 32

the point on a phase diagram where the critical temperature and the critical
pressure converge; also the end point of the vapourization curve

Front 33

triple point

Back 33

the point on a phase diagram at which all three states of a substance are
present and coexist

Front 34

hydrocarbon

Back 34

organic compound chiefly composed of hydrogen and carbon atoms

Front 35

saturated

Back 35

hydrocarbon containing all carbon-to-carbon single bonds

Front 36

unsaturated

Back 36

hydrocarbon containing at least one double or triple bond

Front 37

alcohol

Back 37

organic compound characterized by the presence of a hydroxyl group

Front 38

aldehyde

Back 38

organic compound characterized by the presence of a terminal carbonyl group

Front 39

ether

Back 39

organic compound characterized by a C-O-C group

Front 40

ester

Back 40

organic compound formed through the condensation reaction of an alcohol and a carboxylic acid

Front 41

ketone

Back 41

organic compound characterized by the presence of a central carbonyl group

Front 42

amine

Back 42

organic compound characterized by the presence of an amino group

Front 43

carboxylic acid

Back 43

organic compound characterized by the presence of a carboxyl group

Front 44

hydroxyl group

Back 44

-OH

Front 45

carbonyl group

Back 45

-C=O

Front 46

carboxyl group

Back 46

O
ll
C-OH

Front 47

amino group

Back 47

-NH2

Front 48

dynamic equilibrium (or simply equilibrium)

Back 48

state in which there are no VISIBLE changes to a reaction system, but the rate of the forward reaction is equal to the rate of the reverse reaction.

Front 49

equilibrium constant

Back 49

the ratio of the equilibrium concentrations of the reactants and the products

Front 50

heterogeneous equilibrium

Back 50

an equilibrium reaction involving more than one phase (i.e. gases and liquids)

Front 51

reaction quotient

Back 51

equilibrium expression expressed in terms of the initial concentrations, rather than the equlibrium concentrations

Front 52

Le Chatelier's Principle

Back 52

if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change.

Front 53

solubility product constant

Back 53

equilibrium expression used to describe the dynamic that exists between dissolved and undissolved solute in a saturated solution

Front 54

sparingly soluble

Back 54

salts that dissociate in limited amounts when in solution

Front 55

molar solubility

Back 55

the amount of a sparingly soluble salt (in mol/L) that will dissolve into solution

Front 56

common ion effect

Back 56

equilibrium condition in which one of the ions in the solution is common to both of the dissolved salts --- when a second salt is added, the common ion is added to the solution which decreases the solubility of the already sparingly soluble first salt

Front 57

Ka/Kb

Back 57

acid dissociation constant/base dissociation constant

Front 58

Lewis acid

Back 58

an electron-pair acceptor

Front 59

Lewis base

Back 59

an electron pair donor

Front 60

buffer

Back 60

a solution that resists a change in its pH when either hydrogen or hydroxide ions are added

Front 61

kinetics

Back 61

the study of chemical reaction rates and the factors that affect them

Front 62

reaction rate

Back 62

the change in concentration of a reaction over a specified period of time

Front 63

rate law

Back 63

representation of the rate of a reaction as a mathematical relationship

Front 64

half-life

Back 64

the time required for the reactant concentration in a reaction to decrease by half

Front 65

collision theory

Back 65

molecules must collide in order for them to react

Front 66

activation energy

Back 66

the amount of energy that must be overcome in order to produce a chemical reaction

Front 67

reaction intermediate

Back 67

a species in a chemical reaction that is neither a reactant nor a product

Front 68

reaction mechanism

Back 68

a series of steps that collectively make up a chemical reaction

Front 69

slow step

Back 69

the rate-determining step of a reaction mechanism

Front 70

fast step

Back 70

step within a reaction mechanism that does not affect the speed of the reaction

Front 71

exothermic

Back 71

a reaction that releases energy

Front 72

endothermic

Back 72

a reaction that absorbs energy

Front 73

lattice energy

Back 73

the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

Front 74

Hess's Law

Back 74

in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step, or a series of steps

Front 75

specific heat capacity

Back 75

the amount of energy required to raise the temperature of one gram of a particular substance by 1oC

Front 76

ionization energy

Back 76

energy required to remove an electron from a gaseous atom or ion

Front 77

system

Back 77

term used in thermochemistry to describe a chemical reaction

Front 78

surroundings

Back 78

term used in thermochemistry to describe everything outside a chemical reaction

Front 79

standard enthalpy of formation

Back 79

the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states

Front 80

reaction enthalpy

Back 80

the difference in enthalpy between the reactants and products in a chemical reaction

Front 81

bond energy

Back 81

the amount of energy released when a bond is formed, or the amount of energy absorbed when a bond is broken

Front 82

standard state

Back 82

state of an element or compound under standard conditions

Front 83

calorimetry

Back 83

Measurement of the amount of heat evolved or absorbed in a chemical reaction, change of state, or formation of a solution.

Front 84

elementary step

Back 84

a reaction whose rate law can be written from its molecularity

Front 85

initial rate

Back 85

rate of a reaction taken shortly after the start of the reaction

Front 86

molecularity

Back 86

the number of species that must collide to produce the reaction indicated by a particular elementary step

Front 87

reaction order

Back 87

with respect to a certain reactant, is defined as the power to which its concentration term in the rate equation is raised

Front 88

oxidation

Back 88

loss of electrons by an atom or ion in a redox reaction

Front 89

reduction

Back 89

gain of electrons by an atom or ion in a redox reaction

Front 90

half-reaction

Back 90

one of two parts of a redox reaction (either oxidation or reduction)

Front 91

oxidizing agent

Back 91

a reactant that accepts electrons from another reactant in a redox reaction

Front 92

reducing agent

Back 92

a reactant that donates electrons to another reactant in a redox reaction