Ions, structure and metallic bonding

Question 1

Simple ions form when

Answer 1

Atoms lose or gain electrons

Question 2

Negative ions

Answer 2

Anions- more electrons

Question 3

Positive ions

Answer 3

Cations-more protons

Question 4

Pairs for ionic compound

Answer 4

1&7

2&6

Question 5

An ionic compound overall charge

Answer 5

0

Question 6

Ionic bonding

Answer 6

Is when a metal and non metal react together

Question 7

Ionic bond

Answer 7

Is oppositely charged ions that are strongly attracted to each other by electrostatic forces

Question 8

Dot and cross diagram

Answer 8

E.g. 2.8.1 + 2.8.7 –> 2.8 +2.8.8

Question 9

Ionic compound has

Answer 9

A giant ionic lattice and the ions form a closely packed regular lattice. Very strong electrostractic forces of attraction between the ions.

Question 10

Ionic compound properties

Answer 10

High melting points
High boiling points
*due to strong attraction 
Don't conduct electricity but can in molten or liquid form 
High solubility

Question 11

Covalent bonding is

Answer 11

A strong bond that forms when a pair of electrons is shared between two atoms.

Question 12

Simple molecular substances are

Answer 12

Made up of molecules containing a few atoms joined by covalent bonds

Question 13

Other dot and cross diagram

Answer 13

Put the two reacting electrons in the intersection(s) and place remaining electrons on the circles forming a vent diagram shape

Question 14

Properties of simple molecular

Answer 14

Feeble inter molecular forces
Low boiling points
Low melting points
*due forces of attraction are weak
Increase as molecules get bigger 
Don't conduct electricity

Question 15

Polymers are

Answer 15

Made of covalently bonded carbon chains

Question 16

Fullerenes are

Answer 16

Molecules of carbon shaped into closed tubes or hollow balls

Question 17

Giant covalent structures properties

Answer 17

Strong covalent bonds
High melting and boiling points
Due to energy needed to break bonds
Don't have charged particles, don't conduct electricity 
Aren't soluble in water

Question 18

Example of a giant covalents

Answer 18

Diamond-four bonds,rigid lattice structure,doesn’t conduct electricity
Graphite-three bonds,no bonds between layers,conducts electricity
Graphene-layer of graphite, example of fullerene,hexagon shape

Question 19

How are fullerenes used

Answer 19

For trapping other molecules

Huge surface area - industrial catalysts

Question 20

Metallic bonding involves

Answer 20

Delocalised electrons
The electrons in the outer shell of the metal atoms are delocalised (free to move) there are strong forces between the positive metal ions and the electrons. They hold the atoms together in the regular structure.

Question 21

Physical properties of metals

Answer 21

• very strong
• high melting and boiling points
• shiny
• aren’t soluble in water
• malleable
• conduct heat and electricity

Question 22

Non metals properties

Answer 22

• dull looking
• low melting and boiling points
• don’t conduct heat or electricity