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IEB Gr12 Chemistry > All IEB Definitions for Chemistry > Flashcards

All IEB Definitions for Chemistry Flashcards

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1
Q

Molar mass

A

the mass in grams of one mole of that substance.

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2
Q

Solution

A

a homogenous mixture of solute and solvent.

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3
Q

Solute

A

the substance that dissolved in the solution.

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4
Q

Solvent

A

the substance in which another substance is dissolved, forming a solution.

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5
Q

Concentration

A

the amount of solute per unit volume of solution.

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6
Q

Yield

A

a measure of the extent of a reaction, generally measured by comparing the amount of product against the amount of product that is possible.

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7
Q

Intramolecular bond

A

a bond which occurs between atoms within molecules.

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8
Q

Intermolecular force

A

a force of attraction between molecules, ions, or atoms of noble gases.

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9
Q

Covalent bond

A

a sharing of at least one pair of electrons by two non-metal atoms.

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10
Q

Non-polar covalent (pure covalent)

A

an equal sharing of electrons.

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11
Q

Polar covalent

A

an unequal sharing of electrons leading to a dipole forming.

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12
Q

Ionic bond

A

a transfer of electrons and subsequent electrostatic attraction.

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13
Q

Metallic bonding

A

bonding between a positive kernel and a sea of delocalised electrons.

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14
Q

Electronegativity

A

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

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15
Q

Organic molecules

A

molecules containing carbon atoms.

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16
Q

Hydrocarbon

A

a compound containing only carbon and hydrogen atoms.

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17
Q

Homologous series

A

a series of similar compounds which have the same functional group and have the same general formula, in which each member differs from the previous one by a single CH2 unit.

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18
Q

Saturated compound

A

a compound in which all of the bonds between carbon atoms are single bonds.

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19
Q

Unsaturated compound

A

a compound in which there is at least one double and/or triple bond between carbon atoms.

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20
Q

Functional group

A

an atom or a group of atoms that form the centre of chemical activity in the molecule.

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21
Q

Structural isomers

A

compounds having the same molecular formula but different structural formulae.

22
Q

Heat of reaction (ΔH)

A

the net change of chemical potential energy of the system.

23
Q

Exothermic reactions

A

reactions which transform chemical potential energy into thermal energy.

24
Q

Endothermic reactions

A

reactions which transform thermal energy into chemical potential energy.

25
Q

Activation energy

A

the minimum energy required to start a chemical reaction or the energy required to form the activated complex.

26
Q

Activated complex

A

a high energy, unstable, temporary transition state between the reactants and the products.

27
Q

Reaction rate

A

the change in concentration per unit time of either a reactant or product.

28
Q

Catalyst

A

a substance that increases the rate of the reaction but remains unchanged at the end of the reaction.

29
Q

Closed system (in chemistry)

A

a system in which mass is conserved inside the system but energy can enter or leave the system freely.

30
Q

Open system (in chemistry)

A

a system in which both energy and matter can be exchanged between the system and its surroundings.

31
Q

Le Châtelier’s principle

A

when an external stress (change in pressure, temperature or concentration) is applied to a system in dynamic chemical equilibrium, the equilibrium point will change in such a way as to counteract the stress.

32
Q

Lowry-Brønsted theory

A

an acid is defined as a proton donor. A base is defined as a proton acceptor.

33
Q

Ionisation

A

the reaction of a molecular substance with water to produce ions.

34
Q

Strong acid

A

an acid that ionises completely in an aqueous solution.

35
Q

Weak acid

A

an acid that only ionises partially in an aqueous solution.

36
Q

Dissociation

A

the splitting of an ionic compound into its ions.

37
Q

Strong base

A

a base that dissociates completely in an aqueous solution.

38
Q

Weak base

A

a base that only dissociates/ionises partially in an aqueous solution.

39
Q

Amphoteric (amphiprotic) substance

A

a substance that can act as either an acid or a base.

40
Q

Neutralisation (equivalence point)

A

the point where an acid and base have reacted so neither is in excess.

41
Q

Salt

A

a substance in which the hydrogen of an acid has been replaced by cation.

42
Q

Hydrolysis of a salt

A

a reaction of an ion (from a salt) with water.

43
Q

Standard solution

A

a solution of known concentration.

44
Q

Redox reaction

A

a reaction involving the transfer of electrons.

45
Q

Oxidation

A

the loss of electrons.

46
Q

Reduction

A

the gain of electrons.

47
Q

Oxidising agent

A

a substance that accepts electrons.

48
Q

Reducing agent

A

a substance that donates electrons.

49
Q

Anode

A

the electrode where oxidation takes place.

50
Q

Cathode

A

the electrode where reduction takes place.

51
Q

Electrolyte

A

a substance that can conduct electricity by forming free ions when molten or dissolved in solution.

IEB Gr12 Chemistry (9 decks)

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