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Chemistry HL > Definitions > Flashcards

Definitions Flashcards

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1
Q

Relative Atomic Mass (Ar)

A

The weighted average of the masses of the isotopes relative to 1/12 of a carbon-12 atom

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2
Q

Relative Molecular Mass (Mr)

A

The mass of one molecule of a substance relative to 1/12 of the mass of carbon-12 atom

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3
Q

Mass Number

A

The sum of the protons and neutrons in the nucleus of an atom

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4
Q

Atomic Number

A

The number of protons in the nucleus of an atom

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5
Q

Isotope

A

Atoms of the same element with different numbers of neutrons

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6
Q

First Ionisation Energy

A

The minimum energy required to remove one mole of electrons from an atom in its gaseous state

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7
Q

Electronegativity

A

A measure of the tendency of an atom in a molecule to attract a binding pair of electrons towards itself

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8
Q

Ligand

A

An atom, ion or molecule that can donate a pair of electrons to a central metal ion to form a dative covalent (coordinate) bond
[LEWIS BASES]

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9
Q

Exothermic Reaction

A

A reaction that releases heat to the surroundings
(As a result of forming products with stronger bonds than the reactants. Exothermic reactions have negative ∆H values)

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10
Q

Endothermic Reaction

A

A reaction that absorbs heat from its surroundings
(As a result of forming products with weaker bonds than the reactants. Endothermic reactions have positive ∆H values)

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11
Q

Standard State

A

The most stable state of an element or compound under the specified conditions

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12
Q

Standard Conditions

A

Temperature: 298K
Pressure: 100 kPa (1 atm)

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13
Q

Standard Enthalpy Change of a reaction (ΔH θ)

A

The heat energy transferred under standard conditions for a reaction

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14
Q

Average Bond Enthalpy

A

The energy required to break one mole of the same type of bond in the gaseous state averaged over a variety of similar compounds

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15
Q

Standard Enthalpy change of Formation

A

The enthalpy change when 1 (one) mole of a substance is formed from its elements in their standard states, under standard condtitions

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16
Q

Standard Enthalpy of Combustion

A

The enthalpy change when 1 (one) mole of a substance in its standard states burns completely in excess oxygen under standard conditions

17
Q

Lattice Enthalpy

A

The amount of energy required to separate one mole of ionic compound into isolated gaseous ions under standard conditions

18
Q

Electron Affinity

A

The energy change when 1 (one) mole of gaseous atom gains 1 (one) mole of electrons to form a gaseous ion, under standard conditions

19
Q

Rate of Reaction

A

The increase in concentration of products or the decrease in concentration of reactants per unit time

20
Q

Activation Energy

A

The minimum energy needed (by reactants) to start/initiate a reaction

21
Q

Arrhenius Acid/Base

A

Acid is an H+ donor; Base is an OH- donor

22
Q

Brønsted Lowry Acid

A

An acid is a proton (hydrogen ion) donor

23
Q

Brønsted Lowry Base

A

A base is a proton (hydrogen ion) acceptor

24
Q

Lewis Acid

A

An acid is an electron pair acceptor

25
Q

Lewis Base

A

A base is an electron pair donor

26
Q

Oxidation

A

The loss of electrons from a species during a chemical reaction

27
Q

Reduction

A

The gain of electrons by a species during a chemical reaction

28
Q

Oxidizing Agent

A

A species that brings about oxidation by removing electrons from another reactant.
During the reaction the oxidizing agent gains electrons and so is reduced

29
Q

Reducing Agent

A

A species that brings about reduction by giving electrons to another reactant.
During the reaction the reducing agent loses electrons and so is oxidized

30
Q

Standard Electrode Potential

A

The is the electrode potential of a half-cell relative to the hydrogen half-cell, which is assigned a value of zero. (Also known as standard reduction potential)
It is measured at standard conditions
Standard conditions for SHE
- H2(g) at 100 kPa and 298K
- acidic solution, [H+] 1.0 mol dm^-3
- inert platinum electrode

Chemistry HL (1 decks)

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