Bonding

Question 1

Ionic crystals

Answer 1

Ionic lattice
Strong electrostatic forces of attractions
High melting and boiling points
Solid at room temperature
The higher the charge and smaller the size of the ions the larger the melting point
Soluble in water
Conductors of heat and electricity when molten or dissovled

Question 2

Metallic structures

Answer 2

Atoms in layers surrounded by delocalised electrons
Conduct heat and electricity
Stron electrostatic attraction between metal ions and delocalised electrons
Ductile and malleable (layers can slide over each other)
High density (packed tightly)
High melting points

Question 3

Macromolecular

Answer 3

Strong covalent bonds requiring lots of energy to break
Do not conduct electricity or heat
High melting points
Insoluble

Question 4

Simple molecule

Answer 4

Low melting points
Bad conductors
Insoluble in water
Weak intermolecular forces between molecules

Question 5

What is subliming

Answer 5

Change from solid to gas

Question 6

What effects electronegativity

Answer 6

Distance of bonding electrons from nucleus
Size of nuclear charge
Shielding from other electrons

Question 7

Why does electronegativity increase across a period

Answer 7

Atomic radius decreases
Nuclear charge increases

Question 8

Why does electronegativity decrease group

Answer 8

Atomic radius increases (weaker attraction)
Shielding increases