C2.2

Question 1

What type of ions do metals form

Answer 1

Metals lose electrons to form positive ions

Question 2

What type of ions do non-metals form

Answer 2

Metals gain electrons to form negative ions

Question 3

What PH solution do metals and non metals form when their oxides are dissolved in water

Answer 3

Non metals - acidic solutions
Metals - alkaline solutions

Question 4

Physical properties of metals

Answer 4

Shiny, high melting and boiling point, solid, malleable, ductile (can be pulled into wires) and are good conductors

Question 5

Physical properties of non metals

Answer 5

Dull, low melting and boiling points, 1/2 solid and 1/2 gas, brittle, no-ductile, insulators

Question 6

What is a horizontal row in the periodic table called

Answer 6

A period

Question 7

What is a vertical column in the periodic table

Answer 7

A group

Question 8

What does the group number mean

Answer 8

It is the number of electrons that are in the outer shell.

Question 9

What does the period number mean

Answer 9

The number of electron shells that the element has

Question 10

An atom will always follow the easiest path to become an ion

Answer 10

For example sodium loses an electron

Question 11

What happens when a metal reacts with a non metal

Answer 11

When a metal reacts with a non metal electrons are transferred from the metal to the non-metal so both achieve a more stable electronic structure.

Question 12

What can you model an ionic compound with

Answer 12

A dot and cross diagram, where the dots and crosses represent electrons.

Question 13

What must you do to the charges

Answer 13

Balance the charges so that they are equal

Question 14

Properties of an ionic structure

Answer 14

High melting point as there are lots of strong ionic bonds
Brittle as the layers slide over each other when a force is applied -> some charges come close together -> electrostatic repulsion -> shattering
Not conductive in a solid.
Conductive in liquid as positive ions and negative ions are free to move so can complete a circuit.
Soluble in polar solvents.

Question 15

What is the bond in an ionic compound

Answer 15

The bond in an ionic compound is between the positively charged metal ion and the negatively charged non metal ion

Question 16

What is a covalent bond

Answer 16

A covalent bond is a shared pair of electrons between two non metal atoms. By sharing electrons they complete their outer shells.

Question 17

what is a simple molecule

Answer 17

A molecule that only contains a few atoms. They can be modelled using a dot and cross diagram

Question 18

What is the electrostatic force of attraction in a covalent bond

Answer 18

they are between the positively charged nucleus of the atoms and the shared electrons

Question 19

Why do simple molecules have a low boiling and melting point

Answer 19

They have a low boiling and melting point as the intermolecular forces between molecules are weak.

Question 20

What is a giant covalent substance

Answer 20

A giant covalent substance consists of lots of non-metal atoms covalently bonded and in a repeating pattern called a giant lattice/giant covalent lattice.

Question 21

What is the chemical formula for giant covalent structures written as

Answer 21

The chemical formula is written empirically

Question 22

Diamond

Answer 22

Properties -
hard as it has many strong covalent bonds a high melting point and a high boiling point
Unreactive
transmits light
Bonding - each carbon atoms is bonded to 4 other carbon atoms (each atom is stable and un reactive)
No intermolecular forces only covalent bonds

Question 23

Graphite

Answer 23

Properties:
brittle
soft
conducts electricity as there are delocalised electrons
good conductor of heat
lubricant as layers of graphite can slide over each other
Bonding:
Weak intermolecular forces between layers
Each carbon atom bonded to 3 carbons
Each carbon has one double bond an a single bond

Question 24

Silicon dioxide

Answer 24

Properties:
Transparent
Brittle
Bonding:
Each silicon atom is bonded to 4 oxygens and each oxygen to 2 silicons
Formula SiO2

Question 25

What are polymers made from

Answer 25

Polymers are made from many smaller molecules called monomers. They are able to join end to end in chemical reactions producing longer polymer molecules.

Question 26

What are monomers

Answer 26

Monomers are simple molecules consisting of a few non-metals joined together by covalent bonds

Question 27

Properties of polymers

Answer 27

Can’t conduct electricity
Lots of covalent bonds
Longer polymers have high melting/boiling pints as the longer they get the stronger intermolecular forces are

Question 28

A property of metals (melting and boiling points)

Answer 28

All metals (apart from mercury) are solid at room temperature. Their atoms are packed together in a regular way forming a giant metallic lattice.

Question 29

Structure of metals

Answer 29

Positive metallic ions surrounded by a sea of delocalised electrons

Question 30

What is the electrostatic forces of attraction in a metal

Answer 30

Strong electrostatic forces of attraction between the delocalised electrons and positively charged metal ions

Question 31

Properties of metaks

Answer 31

Malleable - as the layers of metal ions can slide over each other and the sea of delocalised electrons is free to move meaning that when the do bonds aren’t broken
Conducts electricity - it has free to move delocalised electrons
High melting point - lots of strong metallic bonds
Ductile

Question 32

How did Mendeleev organise the periodic table

Answer 32

Mendeleev organised the elements by increasing atomic mass.
If an element shared properties with a group of elements it was rearranged so they were together
He left gaps where no known elements fitted with the chemical properties of the group.

Question 33

what does group 8 consist of

Answer 33

Unreactive gases

Question 34

What is the pattern of chemical properties in the periodic table

Answer 34

Elements arranged in order of increasing atomic number
Electronic structure is determined by the number of electrons
Electronic structure determines its chemical structure