3-Bonding

Question 1

Noble gases

Answer 1

Only group that exist as individual atoms not bonded to other atoms, monatomic elements, their outer energy level of electrons is full making it stable therefore very unreactive

Question 2

Why do atoms form bonds?

Answer 2

To have a full outer energy level and to achieve a stable electron arrangement

Question 3

Covalent bonding

Answer 3

Two non metal atoms share electrons, its the strong electrostatic attraction between the positively charged nuclei of each non metal atom and the shared pair of negatively charged electrons, strong bonds

Question 4

Covalent molecular

Answer 4

Atoms that share pairs of electrons form molecules

Question 5

Molecule

Answer 5

Group of atoms held together by covalent bonds

Question 6

Diatomic molecules

Answer 6

A molecule containing only two atoms. Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

Question 7

Bonding diagrams

Answer 7

Show how the outer electrons are shared, to make atoms outer electrons stable

Question 8

Covalent compound

Answer 8

Same rules apply, bigger molecules

Question 9

Covalent molecules

Answer 9

2 atoms= linear= O-O
3 atoms= angular
4 atoms= trigonal pryrimidal
5 atoms= tetrahedral

Question 10

Covalent networks

Answer 10

Made up of non metal atoms which are joined together by covalent bonds in a giant network structure
Structure egs: boron, carbon, silicon

Question 11

Covalent molecular solubility, melting and boiling points, electricity conductors?

Answer 11

Covalent molecular substances which are not soluble in water may dissolve in other solvents
Have low melting and boiling and melting points as only weak forces of attraction between the molecules are broken when a substance changes state
Covalent molecular substances do not conduct electricity because they don’t have charged particles which are free to move

Question 12

Covalent network solubility, melting and boiling points, electricity conductors?

Answer 12

In general, covalent network substances do not conduct electricity, graphite is an exception because it has delocalised electrons in its structure
do not dissolve
have very high melting and boiling points because the large network of covalent bonds is not easily broken

Question 13

Ionic bonding

Answer 13

Non metal and metal join
Ionic bond is a strong electrostatic attraction between positive metal ions and negative non metal ions
In ionic bonding, metals are oxidised and non metals are reduced

Question 14

Reduction

Answer 14

Is a gain f electrons y a reactant in any reactions

Question 15

Oxidation

Answer 15

A loss of electrons by a reactant in any reactions

Question 16

Ionic compound solubility, conducting electricity and the melting and boiling points

Answer 16

Most ionic compounds are soluble in water because as it dissolves, water molecules surround the separated ions.
ionic compounds have high melting and boiling points because they have strong bonds. When ionic compounds are molten they can conduct electricity because they contain charged particles (ions) but when solid the ions are free to move so molten ionic compounds conduct electricity and solid ionic compounds don’t conduct electricity

Question 17

Explain electrolysis

Answer 17

The positive ions are attracted to the negative electrode, when they get to the electrode, they pick up two electrons.
The negatively charged ions are attracted to the positive electrode when they get to the electrode they lose their extra electrons.

Question 18

Electrolysis

Answer 18

The breaking of a compound by passing electricity though it

Question 19

Direct current

Answer 19

Must be used in electrolysis, direct current allow one electrode to remain positive and the others to remain negative and this allows the product to form at separate electrodes

Question 20

Electrolyte

Answer 20

A substance which conducts electricity in solution or as a melt