Structure And Bonding

Question 1

Ionic bonding is

Answer 1

The electrostatic forces of attractions between oppositely charged ions

Question 2

Why do compounds with giant ionic lattices have high melting and boiling points

Answer 2

• ESFOA between positive and negative ions
• very strong
• require large amounts of energy to overcome
• therefore have high melting and boiling points

Question 3

Do ionic compounds conduct electricity

Answer 3

Not when solid, only when molten or in aqueous solution

Question 4

Covalent bonding is

Answer 4

The electrostatic forces of attraction between nuclei and shared pairs of electrons

Question 5

Why substances with a simple molecular structure are gases or liquids, or solids with low melting and boiling points

Answer 5

• weak intermolecular forces between molecules
• require little energy to overcome
• low melting/boiling points therefore liquids/gases

Question 6

Do covalent compounds conduct electricity

Answer 6

• no

- molecules have no mobile charged particles to carry current

Question 7

Why diamonds is strong with a high melting point

Answer 7

• giant covalent lattice
• 4 covalent bonds per C
• very strong
• require large amount of energy to overcome
  therefore high melting point

Question 8

Why does diamond not conduct electricity

Answer 8

• no charged particles that are mobile

- cannot carry charge

Question 9

Why graphite is useful in pencil lead

Answer 9

• giant covalent structure in layers
• weak attraction between layers
• require little energy to overcome
• can slide over each other and deposit on paper

Question 10

Why graphite has a high melting point

Answer 10

• giant covalent structure
• 3 covalent bonds per atom
• very strong
• requires large amounts of energy to overcome therefore high melting point

Question 11

Why does graphite conduct electricity

Answer 11

• giant covalent structure in layers
• 3 covalent bonds per atoms leaves one delocalised
• can carry current

Question 12

Fullerenes have low melting/boiling points and can’t conduct electrons. Why?

Answer 12

• molecules
• weak intermolecular forces between molecules
• require little energy to overcome

Question 13

Metallic bonding is

Answer 13

The electrostatic forces of attraction between metal cations and delocalised electrons

Question 14

Why are metals malleable

Answer 14

The metal ions slide over eachother and settle in a new position

Question 15

Why are metals tough solids with high melting points

Answer 15

• esfoa between metal cations and delocalised electrons
• strong
• require a lot of energy to overcome

Question 16

Why metals are good conductors of electricity

Answer 16

• delocalised electrons in metallic lattice

- can move and conduct electricity

Question 17

what are ions

Answer 17

Ions are electrically charged particles formed when atoms lose or gain electrons

Question 18

Charge of Ag

Answer 18

+

Question 19

Charge of Cu

Answer 19

2+

Question 20

Charges of Fe

Answer 20

2+, 3+

Question 21

Charge of Pb (lead)

Answer 21

2+

Question 22

Charge of Zn

Answer 22

2+

Question 23

Hydroxide charge

Answer 23

OH-

Question 24

Hydrogen charge

Answer 24

H+

Question 25

Ammonium charge

Answer 25

NH4 +

Question 26

Carbonate charge

Answer 26

CO3 2+

Question 27

Nitrate charge

Answer 27

NO3 -

Question 28

Sulfate charge

Answer 28

SO4 2-

Question 29

How is a covalent bond formed

Answer 29

two non-metal atoms by sharing a pair of electrons in order to fill the outer shell

Question 30

explain why the melting and boiling points of substances with simple molecular structures increase with increasing relative molecular mass

Answer 30

• larger molecules (molecules with more mass) have more forces of attraction between them
• these forces, although weak, must be overcome if the substance is to boil, and larger molecules have more attractions which must be overcome.

Question 31

Metals have a regular arrangement of

Answer 31

layers of positive ions surrounded by a sea of delocalised electrons.