bonding

Question 1

Describe Ionic Bonding [6]

Answer 1

between metals and non-metals.
metals lose electrons to form positive ions.
non-metals gain electrons to form negative ions.
it is a transfer of electrons.
Electrostatic force of attraction holds ions together.
has a lattice structure in a regular arrangement of alternating positive and negative ions.

Question 2

Describe Covalent Bonding [3]

Answer 2

between two non-metals.
it is a shared pair of electrons.
atoms are held together by strong covalent bonds.

Question 3

describe and explain the melting point of simple covalent bonds

Answer 3

Low, because molecules are held together by weak intermolecular forces, therfore requires little energy to break

Question 4

describe and explain the conductivity of simple covalent bonds

Answer 4

Doesn’t conduct, because there are no mobile charge carriers.

Question 4

describe and explain the melting point of giant covalent bonds

Answer 4

Very high, because there are a lot of covalent bonds that require a lot of energy to break

Question 5

describe and explain the conductivity of giant covalent bonds

Answer 5

Doesn’t conduct, except graphite because carbon atoms have three bonds which leaves them with a delocalised electron between layers.

Question 6

describe and explain the melting point of ionic bonds

Answer 6

High.
because a lot of energy is needed to weaken the electrostatic force of attraction

Question 7

describe and explain the conductivity of ionic bonds

Answer 7

only when molten or aqueous.
in a solid, the ions are fixed, but when molten or aqueous, the ions can move

Question 8

describe and explain the melting point of metalic bonds

Answer 8

High.
because a lot of energy is needed to weaken the electrostatic force of attraction

Question 9

describe and explain the conductivity of metalic bonds

Answer 9

conducts, because it has delocalised electrons which can move through the structure

Question 10

Graphite [8] 3 description, 5 explanation

Answer 10

-Giant Covalent
+Lots of covalent bonds in layers
+Weak intermolecular forces of attraction between layers
-conducts Electricity
+Carbon atoms in Graphite form 3 bonds so it has delocalized electron (mobile charge carrier)
-High melting point
+because lots of covalent bonds that require a lot of energy to break
+still and giant structure even though it has intermolecular forces

Question 11

Diamond [6]

Answer 11

-Giant covalent Structure
+Lots of covalent bonds
-High Melting points
+Because lots of covalent bond require a lot of energy to break
-Doesn’t conduct electricity
+Because no mobile carriers

Question 12

Name three giant covalent substances [3]

Answer 12

Diamond, Graphite, Silica (Silicon dioxide)