Structure and Bonding

Question 1

What is an ion?

Answer 1

An ion is a charged particle

Question 2

How are ions formed?

Answer 2

Ions are formed when atoms gain/lose electrons

Question 3

Do metals lose or gain electrons?

Answer 3

They lose electrons to form an overall positive charge

Question 4

Do non-metals lose or gain electrons?

Answer 4

they gain electrons to form an overall negative charge

Question 5

How is the charge of an ion determined?

Answer 5

By how many electrons it gains or loses

Question 6

What is an ionic compound?

Answer 6

An ionic compound forms when a metal and a non-metal bond together creating an ionic bond. The metal loses electrons and the non-metal gains electrons

Question 7

What forces are found in ionic bonds?

Answer 7

There are strong electrostatic attractions between the oppositely charged ions

Question 8

What structure do ionic compounds have?

Answer 8

Giant 3D ionic lattice

Question 9

Describe the arrangement of the ions in an ionic compound

Answer 9

Ions in an ionic compound are regularly arranged

Question 10

Do ionic compounds conduct electricity?

Answer 10

Only when molten or dissolved (only when the ions are free to move)

Question 11

Describe and explain the melting/boiling points of ions

Answer 11

Ions have high melting and boiling points. This is due to the strong electrostatic forces between the oppositely charged ions which require a lot of energy to be broken/weakened

Question 12

What forces are found in covalent bonds?

Answer 12

There are strong electrostatic forces between the positively charged nuclei of the atoms and the negatively charged, shared electrons

Question 13

When do covalent bonds form?

Answer 13

Covalent bonds form when non-metals bond together

Question 14

Are most covalent compounds simple or giant?

Answer 14

Simple

Question 15

What are the properties of simple covalent compounds?

Answer 15

1. Low melting/boiling points due to weak intermolecular forces between molecules
2. Very strong covalent bonds within atoms
3. They do not conduct electricity as there are no free electrons or ions

Question 16

What are the 3 giant covalent structures?

Answer 16

1. Diamond
2. Graphite
3. Silicon Dioxide

Question 17

What are the properties of giant covalent structures?

Answer 17

1. Very high melting/boiling points
2. Do not conduct (except for graphite)

Question 18

Describe the structure of a giant covalent compound

Answer 18

All the atoms in a giant covalent compound are bonded together by strong, covalent bonds

Question 19

Describe the structure of diamond

Answer 19

Made entirely of carbon. Each carbon atom is bonded to 4 other carbon atoms

Question 20

Describe the structure of graphite

Answer 20

Made entirely of carbon. Each carbon atom is bonded to 3 other carbon atoms meaning each carbon atom has a delocalised electron

Graphite has hexagon sheets called graphene. Graphene layers are weakly held together so they can easily slide over each other making graphite soft

Question 21

Describe the conductivity of graphite

Answer 21

Each carbon atom in graphite has a delocalised electron which can carry electrical charge or thermal energy throughout the structure. Therefore, graphite conducts both heat and electricity

Question 22

Describe metallic structures

Answer 22

• They are giant structures
• The delocalised electrons of the metal atoms are free to move throughout the structure
• Strong electrostatic forces between positive metal ions and shared negative electrons

Question 23

Do metallic structures conduct?

Answer 23

Yes. The delocalised electrons in metallic structures can carry electrical charge, and thermal energy throughout the metallic compound

Question 24

What are the properties of metals?

Answer 24

1. Solid at room temperature due to high melting/boiling points
2. Malleable
3. Good electricity and heat conductors

Question 25

Are pure metals harder than alloys?

Answer 25

No. Alloys are harder than pure metals due to the distorted layers

Question 26

Why are layers in alloys distorted?

Answer 26

The different atoms of the different metals vary in size causing distorted layers

Question 27

Why do these distorted layers make alloys stronger than pure metals?

Answer 27

The distorted layers cannot easily slide over each other causing alloys to be harder than pure metals

Question 28

What are alloys?

Answer 28

Alloys are mixtures of different metals

Question 29

Why are alloys useful?

Answer 29

Alloys are useful as they are stronger than pure metals. Pure metals are usually too soft to use in the real world.