Assessment 1 - Bonding, Trends and etc.

Question 1

Ionization energy trends

Answer 1

Decreases as we go down

Increases as we go across

Question 2

Atomic size trends

Answer 2

Increases as we go down

Decreases as we go across

Question 3

Electronegativity trends

Answer 3

Decreases down

increases across

Question 4

Metallic nature trends

Answer 4

increases down

decreases across

Question 5

Factors that effect ionisation energy

Answer 5

Nuclear charge - greater the nuclear charge, the greater the charge
Distance from nucleus - the further away, the less amount of ionization energy needed

Question 6

Elements

Answer 6

Cannot be separated into simpler substances. eg - gold, oxygen, aluminium

Question 7

Compounds

Answer 7

(always pure) two or more elements chemically combined. eg - sugar, water. rubber, salt

Question 8

Homogeneous mixture;

Answer 8

uniform composition throughout - sea water, air, solder, petrol

Question 9

Heterogeneous mixture

Answer 9

non uniform composition. eg - limestone, rock, cement

Question 10

Metallic bonds

Answer 10

Form between metal atoms. Valence electrons are very mobile or delocalised. Includes - all metals
High electrical conductivity
high thermal conductivity
malleable and ductile
high density

Question 11

Ionic bonds

Answer 11

Metal and non metal
High melting and boiling points
brittle - difficult to scratch
Good conductivity when molten or aqueous
Transfer of electrons between these atoms create positive and negative ions.
Includes NaCl, MgSO etc

Question 12

Covalent bonds

Answer 12

Molecular or non-molecular

Non metals - electrons are shared in a common bond

Question 13

How do metals form a strongly bonded crystal lattice?

Answer 13

• Result from delocalized attraction between the positively charged metal ions and the delocalised and negatively charged electrons

Question 14

Why are metals good conductors of electricity?

Answer 14

• mobile and loosely held valence electrons

Question 15

Why are metals malleable and ductile?

Answer 15

non directional - so layers of positive ions can simply slip over each other

Question 16

Covalent molecular

Answer 16

• Low melting/boiling points
• don’t conduct electricity
• soft and easily scratched
• low solubility

Question 17

Covalent network

Answer 17

Hard and brittle
non-conductors
very high melting and boiling points
inert, insoluble
E.g - Diamond, silicon and graphite