Bonding N5 U1 P3

Question 1

Point of forming bonds

Answer 1

When atoms form bonds, they can achieve stable electron arrangement
They can loose gain or share electrons to become stable

Question 2

Types of bonding

Answer 2

Covalent bonding
Covalent molecular
Covalent networks
Ionic bonding
(Metallic bonding)

Question 3

Covalent bonding definition

Answer 3

A covalent bonding is the strong electrostatic attaractin between the two positively charged nuclei of each non-metal atom and the shared pair of negatively charged electrons

Question 4

Covalent molecular

Answer 4

Atoms that share pairs of electrons to form molecules
A molecule is a group of atoms held together by covalent bonds
Strong covalent bonds
Weak attractions between molecules
Low melting and boiling points
Do not conduct electricity

Question 5

Diatomic molecules

Answer 5

A diatomic molecule contains only two atoms
Hydrogen
Oxygen
Nitrogen
Fluorine
Chlorine
Bromine
Iodine

Question 6

Type of bonding formed

Answer 6

Single, double or triple
-Number of electrons that are shared, gained, or lost to become stable

Question 7

Bonding diagrams

Answer 7

Shows how outer electrons are shared to form covalent bonds in a molecule

Question 8

Bonding diagram example- hydrogen

Answer 8

Hydrogen atoms are unstable as they only have one outer electron
To become stable two hydrogens overlap to share a pair of electrons and both become stable as they now have two

Question 9

Shapes of simple covalent molecules

Answer 9

Number of atoms Name of shape Number of bonds
2 Linear 1
3 Angular 2
4 Trigonal pyramidal 3
5 Tetrahedral 4

Question 10

Dash and wedge projections

Answer 10

Represent a molecule three-dimensional structure
— in the plane of page
◀️ comes forward out of plane of page;infront
⏪ goes back out of plane of page: behind

Question 11

Covalent networks

Answer 11

Made up of non-metal atoms which are all joined together by covalent bonds in a giant network structure
High melting and boiling points
Do not conduct electricity
Examples- boron carbon and silicon

Question 12

Ionic bond

Answer 12

An ionic bond is a strong electrostatic attraction between positive metal ion and negative non-metal ions
(opposites attract)
High melting and boiling points
Conduct electricity

Question 13

Ionic compound structure

Answer 13

Ionic compounds form lattice structures of oppositely charges ions with each positive ion surround by negative ions and each negative on surrounded by positive ions

Question 14

Ion formation- lithium

Answer 14

Lithium is in group one, with one outer electron, once it is lost lithium ion Li+ is formed, also balanced

Question 15

Ion formation- oxygen

Answer 15

Oxygen has six outer electrons, gains two to forms oxygen ion O2-

Question 16

Ion electron equations- OILRIG

Answer 16

In ionic bonding, the metals are oxidised, and the non-metals are reduced
OIL- Oxidation Is Loss of electrons (positive electrode)
RIG-Reduction is gain of electrons (negative electrode)
Data booklet -> reduction, -< oxidation

Question 17

Forming ionic compounds- sodium and chloride

Answer 17

Sodium has one outer electron
Chlorine has seven outer electrons
Sodium loses an electron, chlorine gains the electron, forming ions Na+ and Cl-
Two oppositely chard ions are formed, which attract, millions of these pairs form a giant ionic lattice structure

Question 18

Non- conductor and conductor

Answer 18

No delocalised electrons [electrons that are not shared]- non conductor
Delocalised electrons [electrons that are shared]- conductor

Question 19

Positive and negative ions

Answer 19

Metal atoms lose electrons to form positive ions
Non-metal atoms gain electrons to form negative ions