Module 5 DEFINITIONS

Question 1

Partial pressure (P)

Answer 1

Contribution that the gas makes towards the total pressure P

Question 2

Bronstead Lowry acid

Answer 2

Proton donor

Question 3

Bronstead Lowry base

Answer 3

Proton acceptor

Question 4

Buffer solution

Answer 4

System that minimised pH changes when small amounts of acid or base added

Question 5

Equivalence point

Answer 5

In titration the volume of one solution that exactly reacts with the volume of another solution

Question 6

Lattice Enthalpy

Answer 6

Enthalpy change when one mole of an ionic compound is formed from its gaseous ions under standard conditions

Question 7

Enthalpy of atomisation

Answer 7

Enthalpy change when one mole of gaseous atoms formed from element in standard state and standard conditions.

Question 8

First electron affinity

Answer 8

Enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of 1- ions

Question 9

Enthalpy of solution

Answer 9

When one mole of solute dissolves in a solvent (if solvent is water it forms aqueous ions)

Question 10

Entropy

Answer 10

Dispersal of energy within chemicals making up the chemical system

Question 11

Enthalpy of hydration

Answer 11

Dissolving of gaseous ions in water to form one mole of aqueous ions

Question 12

Half cell

Answer 12

Contains chemical species present in redox half equation

Question 13

Primary cell

Answer 13

Non rechargeable

Question 14

Secondary cell

Answer 14

Rechargeable

Question 15

Fuel cell

Answer 15

Uses energy from reaction of a field with oxygen to create voltage

Question 16

Transition metals

Answer 16

D-block elements that form at least one ion with a partially filled D orbital

Question 17

Complex ion/ ligand

Answer 17

Complex ion formed when one or more molcules or negatively charges ions bond to central metal ion (molecules/ions= ligands)

Question 18

Bidente ligands

Answer 18

Donate two lone pairs of electrons forming two coordinate bonds