Bonding, Structure And Properties

Question 1

Metallic bonding

Answer 1

Occurs in metals

Results from an electrostatic attraction between positively charged metal ions and a sea of delocalised electrons.

Metallic bonds are strong

As electrons can move from metal ion to metal ion, metals conduct electricity

Question 2

Ionic bonding

Answer 2

Ionic bonding are the electrostatic forces of attraction between positive ions and negative ions.

Ionic bonds are strong
Ionic compounds have a lattice structure
Ionic compounds dissolve in water. When they dissolve the lattice breaks

Ionic compounds have high m.p. and b.p. This means they are solids at room temp.

When an ionic compound is dissolved in water a solution called an electrolyte is formed. Electrolytes conduct electricity

Question 3

Electrolysis

Answer 3

Electrolysis is the breaking down of compounds using electricity

Question 4

Covalent bonding

Answer 4

A covalent bond is a shared pair of electrons between atoms
Atoms share electrons to gain a full, stable outer shell of electrons

The atoms are held together in a covalent bond by the electrostatic attraction between the positively charged nuclei of each atom between the negatively charged electrons
Covalent substances do not conduct electricity (apart from graphite)

Most covalent substances don’t dissolve in water
Low m.p and b.p

Question 5

What are the 7 diatomic elements and what is a diatomic molecule?

Answer 5

Hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine and bromine

Question 6

Shapes of molecules

Answer 6

Linear
Angular
Pyramidal
Tetrahedral

Question 7

Bonding summary

Answer 7

Metallic conducts as a solid, conducts as a liquid but doesn’t dissolve in water

Covalent doesn’t conduct as a solid, doesn’t conduct as a liquid and doesn’t conduct as a solution

Ionic doesn’t conduct as a solid, does conduct as a liquid and does conduct as a solution

Question 8

Covalent networks

Answer 8

Covalent substances also exist as giant networks. We call these covalent networks

Examples of covalent networks are: diamond (carbon) and sand (silicon dioxide)

They only contain strong covalent bonds and therefore are solids and have extremely high melting and boiling points

Question 9

Ions

Answer 9

An ionic bond is the attraction of the oppositely charged ions

Ionic bonds are strong

Ionic compounds have a lattice structure of positive and negative ions