Ionic, Covalent And Metallic Bonding

Question 1

What is bonding?

Answer 1

The way atoms or ions are held together

Question 2

Why is bonding needed?

Answer 2

To be stable and to reach the octet/duplet configuration

Question 3

What are the three types of bonding?

Answer 3

Ionic, covalent, metallic

Question 4

What is ionic bonding?

Answer 4

• bonding between metal and non-metal
• transfer of electrons
• metals donate electrons; non-metals accept electrons

Question 5

Name one example of ionic bonding

Answer 5

Compounds

Question 6

What is covalent bonding?

Answer 6

• bonding between non-metal and non-metal
• shares electrons

Question 7

Name three examples of covalent bonding

Answer 7

Compound, element, molecule

Question 8

What is metallic bonding?

Answer 8

• bonding between metal and metal
• sea of delocalised electrons around protons
• electrostatic forces

Question 9

What is the difference of forces between particles in ionic and simple covalent compounds?

Answer 9

Ionic - electrostatic forces
Simple covalent - weak intermolecular forces

Question 10

What is volatility?

Answer 10

The ability to turn into gas

Question 11

What is the difference of solubility between ionic and simple covalent compounds?

Answer 11

Ionic - usually soluble in water and polar solvent, not organic solvent
Simple covalent - usually soluble in organic solvent, not water

Question 12

What is the difference of conductivity between ionic and simple covalent compounds? Why does it behave that whay?

Answer 12

Ionic - conducts electricity when molten or aqueous; has free ions, doesn’t use electrons
Simple covalent - doesn’t conduct electricity; no free moving ions/ electrons

Question 13

What is the difference of structure between ionic and simple covalent compounds?

Answer 13

Ionic - giant lattice structure, regular arrangement of alternating positive and negative
Simple covalent - has strong covalent bonds between atoms, weak intermolecular forces between compounds

Question 14

What is the difference in state of matter between ionic and simple covalent compounds?

Answer 14

Ionic - solid
Simple covalent - liquid or gas

Question 15

What is an allotrope?

Answer 15

Same element (carbon), different molecular structure

Question 16

What are the four types of giant covalent structures?

Answer 16

Graphite, diamond, buck minster fullerene (buckyball), silicon dioxide (sand)

Question 17

What is the difference between graphite, diamond and silicon dioxide’s molecular structure

Answer 17

Diamond and silicon dioxide - tetrahedron
Graphite - hexagonal layers

Question 18

Why can graphite conduct electricity but not diamond?

Answer 18

Graphite has free moving electrons, diamond doesn’t

Question 19

Why do giant covalent structures have low volatility?

Answer 19

Because of strong covalent bonds

Question 20

Why do giant covalent structures have low high MP and BP?

Answer 20

Because of many strong covalent bonds

Question 21

Why is graphite used for pencil lead and lubricant?

Answer 21

Because it’s soft due to its weak attraction between layers and the layers can slide past each other

Question 22

Name three applications of diamond

Answer 22

• drill bits
• cutting tools
• jewellery

Question 23

Why are diamond and silicon dioxide hard?

Answer 23

Because of strong covalent bonds and its lack of intermolecular forces

Question 24

Describe how the atoms of silicon dioxide are bonded

Answer 24

1 Silicon (Si) bonded to 4 Oxygen (O)
1 Oxygen (O) bonded to 2 Silicon (Si)

Question 25

What is the difference between free moving and delocalised?

Answer 25

Free moving - can move anywhere as long as it follows a fixed path Delocalised - can move randomly anywhere; no fixed path to move along

Question 26

Describe the atomic structure of a metallic structure

Answer 26

Metal lattice; positively charged ions are surrounded by sea of delocalised electrons

Question 27

What is the force of attraction in a metallic structure?

Answer 27

Electrostatic force

Question 28

Why are metallic structures good conductors of heat and electricity?

Answer 28

Heat - closely packed, transfer heat easier/faster Electricity - delocalised electrons move throughout structure

Question 29

Why do metallic structures have high MP and BP?

Answer 29

Because of their strong electrostatic forces; it takes up a lot of energy to overcome its forces

Question 30

Why are metallic structures malleable and ductile?

Answer 30

Because they’re arranged in layers; when force is applied the layers will slide