Unit 3

Question 1

Why is an Ion charged

Answer 1

Because it has an unequal number of protons and electrons

Question 2

What groups ionic bonding between

Answer 2

Metals and non-metals

Question 3

What is an ionic bond

Answer 3

Went to ions have opposite charges so they attract each other the force of attraction between them is strong

Question 4

What form positive ions

Answer 4

Hydrogen and metals

Question 5

What do non-metals form

Answer 5

Negative ions and their names end in -ide

Question 6

Why do groups four and five not usually form ions

Answer 6

Because they would have to lose or gain several electrons and that would take too much energy

Question 7

Why does group 0 not form ions

Answer 7

Because they have a full outer shell already

Question 8

What type of metals town form more than one ion

Answer 8

Transition metals

Question 9

What are compound ions

Answer 9

When ions can be formed from groups of joined atoms

Question 10

What are the properties of an ionic compound

Answer 10

Ionic compounds have high melting and boiling points. This is because ionic bonds are very strong, so it takes a lot of heat energy to break up the lattice.
Ionic compounds are usually soluble in water. The water molecules can attract the ions away from the lattice. The ions can then move freely, surrounded by water molecules.
Ionic compounds can conduct electricity when they are melted or dissolved. When melted the lattice breaks up on the ions are free to move. Since they are charged, this means they can conduct electricity. The solutions of ionic compounds conduct electricity to because they are also free to move.

Question 11

What is a lattice?

Answer 11

Ionic lattice structure each positive ion is surrounded by several negative ions

Question 12

What is covalent bonding between?

Answer 12

Nonmetals only since nonmetals need to gain electrons

Question 13

What is a single covalent bond

Answer 13

When a pair of electrons are shared

Question 14

What is a double covalent bond

Answer 14

Two pairs of electrons are shared

Question 15

What is a triple covalent bond

Answer 15

When 3 Pairs of electrons are shared

Question 16

What is A covalent compound

Answer 16

When atoms of different elements share electrons with each other

Question 17

Why are molecules in a covalent bond not flat

Answer 17

Because each electron repel each other and try to get as far apart from each other

Question 18

What are the solids in a molecular substance

Answer 18

Crystaline

Question 19

What happens when you cool down and molecular liquid or gas

Answer 19

The molecules lose energy so they start moving slowly and at the freezing point, they form a lattice

Question 20

What are the properties covalent bonding

Answer 20

Have lower melting and boiling points. This cause the forces between the molecules molecules are weak
Do not conduct electricity. This is because molecules are not charged, so they cannot conduct, even when melted

Question 21

What is a giant covalent structure for a macromolecules

Answer 21

Made of billions of atoms bonded together in a covalent structure

Question 22

Diamond-giant covalent structure

Answer 22

Diamond is made of carbon atoms held in a strong lattice. Each carbon atom forms a covalent bond to four others. Eventually billions of carbon atoms bond together To form a Crystal of diamond

Question 23

What are Diamond Properties

Answer 23

Hard because each atom is held by for strong bonds
It has a very high melting point because of the strong bonds
It can’t conduct electricity because there are no free electrons to carry the charge

Question 24

What is similar to diamond

Answer 24

Silica

Question 25

Graphite

Answer 25

Like diamond graphite is made only of carbon atoms. So Diamond is and graphite are allotropes of Carbon (means they are two forms of the same element). Graphite, unlike diamond, is one of the softest solids on Earth. In graphite, each carbon atom forms a covalent bond to 3 others. This gives rings of six atoms

Question 26

What are graphite properties

Answer 26

Soft and slippery because the sheets can slide over each other
It’s a good conductor of electricity because each carbon has for outer electrons and graphite bond three only so the four electron is free to move carrying a charge.

Question 27

What are the uses of diamond

Answer 27

Jewellery

For tools for drilling and cutting

Question 28

What are the uses of silica

Answer 28

In sandpaper
For making glass and lenses
In bricks for lining furnaces

Question 29

What are the uses for graphite

Answer 29

As a lubricant for engines
For pencil lead which is mixed with clay
For electrodes and connecting brushes in generators

Question 30

What are the properties of silica

Answer 30

They are hard and can scratch things
Hard .let’s light through
High melting point

Question 31

What is a metallic bond

Answer 31

Is the force of attraction between free electrons and metal ions

Question 32

Why do metals have high melting points?

Answer 32

This is because it takes a lot of heat energy to break up the lattice

Question 33

Why metals are malleable and ductile

Answer 33

Malleable-they can be bent and pressed into shapes
Ductile-They can be drawn into wires

This is because the layers can slide without the metallic bond breaking, because the electrons are free to move to

Question 34

Why are metals good conductors of heat

Answer 34

It’s because the free electrons take in heat energy, which makes them move faster and they quickly transfers heat through the metal structure

Question 35

Why are metals good conductors of electricity

Answer 35

This is because the free electrons can move through the lattice Carrying the charge