Section 2 Periodic table and bonding

Question 1

When does ionic bonding take place?

Answer 1

Between a metal and a non metal

Question 2

What is an anion?

Answer 2

A negatively charged particle (An ion that forms when the atom gains electrons)

Question 3

What is a cation?

Answer 3

A positively charged ion (An ion that forms when the atom loses electrons)

Question 4

What do elements in the same group have in common?

Answer 4

They have the same number of electrons in the outer shell

Question 5

What do elements in the same period have in common?

Answer 5

They have the same number of electron shells

Question 6

What are the properties of ionic compounds?

Answer 6

.They have a giant lattice
.They have a high melting and boiling point as there are loads of strong ionic bonds
.They can’t conduct electricity as a solid but can as a liquid or a solution

Question 7

What is the definition of ionic bonding?

Answer 7

A strong electrostatic attraction between oppositely charged ions

Question 8

What do the elements in groups 1,2 and 3 do in ionic bonding?

Answer 8

They lose electrons which forms positive ions (Cations)

Question 9

What is the definition of covalent bonding?

Answer 9

A strong electrostatic attraction between shared pairs of electrons and nuclei

Question 10

When does covalent bonding happen?

Answer 10

Between a non metal and a non metal

Question 11

What are the two types of covalent bonds?

Answer 11

Simple molecular

Giant covalent

Question 12

What are the properties of simple covalent structures?

Answer 12

.Low melting and boiling points as the weak intermolecular forces between the bonds are weak
.Poor conductors of electricity

Question 13

What are the properties of giant covalent structures?

Answer 13

.Giant lattice
.High melting/boiling point
.Don’t conduct electricity

Question 14

Why can graphite conduct electricity?

Answer 14

.Because in graphite each carbon atom only forms 3 covalent bonds creating layers of carbon atoms
.They layers can slide over each other meaning it is malleable
.Only three of the four electrons are used meaning graphite has one delocalized electron so graphite can conduct electricity

Question 15

Why can ionic compounds conduct electricity as a liquid/solution and not a solid

Answer 15

Because when an ionic compound has melted the ions are able to move meaning they can conduct electricity

However in a solid the ions are in a fixed position meaning they can’t conduct

Question 16

What is the definition of metallic bonding?

Answer 16

The strong electrostatic attraction between the nuclei of positive ions and the delocalized electrons

Question 17

What are the properties of metals?

Answer 17

.Can conduct electricity because of the sea of delocalized electrons which can move through the structure
.Malleable as they’re organized in neat layers which can slide over each other
.High melting/boiling point

Question 18

Why are metals malleable?

Answer 18

.The layers of ions in a metal can slide over each other

Question 19

Why can metals conduct electricity?

Answer 19

As the delocalised electrons can freely move

Question 20

Why are the noble gases stable?

Answer 20

As they already have a full outer shell of electrons