Ionic

Question 1

How are ions formed?

Answer 1

By electron loss or gain?

Question 2

What are groups 1,2,3 (left or table)

Answer 2

Metals

Question 3

What are groups 5,6,7 (right side)

Answer 3

Non - Metals

Question 4

What charge is Ag

Answer 4

Ag+

Question 5

What charge is Zn

Answer 5

Zn2+

Question 6

Hydrogen

Answer 6

H+

Question 7

Hydroxide

Answer 7

OH-

Question 8

Ammonium

Answer 8

NH4+

Question 9

Carbonate

Answer 9

CO3^2-

Question 10

Nitrate

Answer 10

NO3^-

Question 11

Sulfate

Answer 11

SO4^2-

Question 12

Ionic bonding

Answer 12

Strong electrostatic force of attraction between oppositely charged ions

Question 13

Why do giant ionic lattices have high boiling points?

Answer 13

• held together by many strong covenant bonds
• a large amount if energy required to break the bonds and cause the substance to melt

Question 14

Why do ionic compounds not conduct electricity when solid?

Answer 14

• when solid the ions are in the fixed lattice so can’t move
• when liquid/molton the ions can move

Question 15

How is a covalant bond formed?

Answer 15

Is formed between atoms by sharing a pair of electrons

Question 16

What are covelnat bonds?

Answer 16

The string electrostatic for of attraction between a shared pair of electrons and the nuclei of both bonding atoms

Question 17

What are the diatomic molecules?

Answer 17

Hydrogen,oxygen,nitrogen,halogens,hydrogen

Question 18

Why are substances with simple molecular structure gases or liquids

Answer 18

There is weak intermolecular forced of attraction between the molecules

Question 19

Why do the boiling points of substances with simple molecular structure increases with relative molecular mass?

Answer 19

As molecular mass increases, the force of attraction becomes stringer and therefore more energy is required to break the bonds

Question 20

Why do substances with giant covalent structures are solids with a high melting point?

Answer 20

They are held together by many string covenant bonds therefore a large amount of energy is required

Question 21

How do the structures of diamond influence their physical properties?

Answer 21

Electrical conductivity - cant conduct, molecules are neutral + can’t move
Hardness - very hard, has a rigid tetrahedral arrangement + difficult to break covalent bonds

Question 22

How does the structure of graphite influence their physical properties?

Answer 22

Conductivity- can conduct - it has delocalised electrons that can move
Hardness - it is soft because the layers can slide over each other and the attractions between layers are weak

Question 23

How does the structure of C60 fullerene influence their physical properties?

Answer 23

• conductivity- can’t conduct - no charged particles tear can move
• hardness - soft and slippery: weak intermolecular forces of attraction, molecules aren’t in fixed position

Question 24

Do covenant binds conduct electricity?

Answer 24

Not usually

Question 25

Physical properties of metal?

Answer 25

Conductivity - it can, they have delocalised electrons that can move freely Malleability - they are malleable: regular arrangement of atoms/ions in layers, layers can easily slide over each other

Question 26

Define a covalent bond

Answer 26

The string electrostatic force of attraction between a shared pair of electrons and the nuclei of both bonding atoms