Combining Atoms

Question 1

What is metallic bonding?

Answer 1

Electrostatic forces of attraction between metal cations and seas of delocalized electrons

Question 2

What is ionic bonding?

Answer 2

Electrostatic forces of attraction between oppositely charged ions

Question 3

What is covalent bonding?

Answer 3

Bonds formed by the sharing of electrons between non-metallic atoms

Question 4

MP and BP of metallic bonds

Answer 4

HIGH

Question 5

Reason for MP and BP of metallic bonds being so

Answer 5

HIGH
Strong electrostatic forces of attraction between cations and delocalized electrons - requires more heat energy to overcome bonds

Question 6

MP and BP of ionic bonds

Answer 6

HIGH

Question 7

Reason for MP and BP of ionic bonds being so

Answer 7

HIGH
Strong electrostatic forces of attraction between cations and anions- requires more heat energy to overcomes

Question 8

States of metallic compounds

Answer 8

Solid at room temperature (except for Hg)

Question 9

States of ionic compounds

Answer 9

Solid at room temperature

Question 10

States of covalent compounds

Answer 10

Can be solid/liquid/gas

Question 11

States of continuous covalent lattice

Answer 11

Always solid

Question 12

Examples of continuous covalent bonds

Answer 12

Diamond (Carbon)
Sand
Glass (Silica)
Graphite

Question 13

MP and BP of molecular covalent bonds

Answer 13

LOW (lower than ionic)

Question 14

Reason for MP and BP of molecular covalent bonds being so

Answer 14

Weak forces of attraction between molecules (does not require much energy to break)

Question 15

With melting and boiling, what is broken for each bonding type?

Answer 15

Metallic and Ionic- PRIMARY BONDS
Covalent- Intermolecular forces

Question 16

Conditions for conductivity

Answer 16

1. Charged particles
2. Freely moving

Question 17

Electrical conductivity of metallic compounds + reason

Answer 17

Very good conductors- freely moving electrons

Question 18

Electrical conductivity of ionic compounds

Answer 18

NO- when solid
YES- when molten or aqueous

Question 19

Why can’t ionic compounds conduct electricity in solid state?

Answer 19

Although the particles are charged, they are not free to move

Question 20

Electrical conductivity of ALL covalent compounds

Answer 20

Do not conduct electricity

Question 21

Why do covalent compounds not conduct electricity?

Answer 21

They meet neither of the conditions-

No freely moving particles
No charged particles

Question 22

What are the 2 main diff. between molecular CC and continuous CC?

Answer 22

Molecular- finite space, can be solid/liquid/gas
Continuous- infinitely continuous- always solid

Question 23

Describe the flexibility of metallic compounds

Answer 23

Metals are malleable and ductile

Question 24

Describe the flexibility of ionic compounds

Answer 24

Ionic compounds are BRITTLE
(crystalline - brittle)

Question 25

Solubility of Metallic compounds

Answer 25

Insoluble in water

Question 26

Solubility of ionic substances

Answer 26

Some are soluble/some insoluble

Question 27

Solubility of molecular covalent substances

Answer 27

Some are soluble (sugar) Some insoluble (fats, oils)

Question 28

Solubility of continuous covalent compounds

Answer 28

Insoluble (do not dissolve)

Question 29

If a substance dissolves in water but does not conduct electricity, what is it likely to be?

Answer 29

A molecular covalent compound

Question 30

If a substance dissolves in water and does conduct electricity, what is it likely to be?

Answer 30

An ionic compound

Question 31

How are ionic compounds represented?

Answer 31

Empirical formulae (primary ratio)

Question 32

What happens when bonds are formed/broken?

Answer 32

Energy is released/required

Question 33

What exactly happens in ionic bonding?

Answer 33

Valence electrons are transferred from one atom to another to formed positively and negatively charged ions.

Question 34

List the subshell configuration pattern.

Answer 34

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10