3.1.3 - Bonding

Question 1

Ionic Bonding

Answer 1

Occurs between a metal and a non-metal. Electrons are transferred from the metal to the non-metal to achieve full outer shells. When electrons are transferred, it creates ions. Oppositely charged ions attract through electrostatic forces to form a giant ionic lattice

Question 2

Common compound ions

Answer 2

Sulfate
Hydroxide
Nitrate
Carbonate
Ammonium

Question 3

Covalent Bonding

Answer 3

Forms between two non-metals. Electrons are shared between the two outer shells to achieve a full outer shell. Multiple electron pairs can be shared to produce multiple covalent bonds

Question 4

Dative Bonding

Answer 4

Dative or coordinate bonds form when both of the electrons in the shared pair are supplied from a single atom. Once a dative bond has formed, it is treated as a standard covalent bond

Question 5

Metallic Bonding

Answer 5

Consists of a lattice of positively charged ions surrounded by a ‘sea’ of delocalised electrons. This produces a very strong electrostatic force of attraction between these oppositely charged particles

Question 6

Ionic Crystal Structure

Answer 6

High melting and boiling point. The electrostatic forces holding the ionic lattice together are strong and require a lot of energy to overcome. When molten or in solution, ionic substances can conduct electricity. Ionic substances are often brittle materials

Question 7

Metallic Crystal Structre

Answer 7

Often good conductors. Also malleable as the layers of positive ions are able to slide over one another. Have high melting points and are nearly always solid at room temperature.

Question 8

Simple Molecular Crystal Structure

Answer 8

Consist of covalently bonded molecules held together with weak van der waals forces. These are very weak forces, so simple molecular substances have low melting and boiling points. Very poor conductors as they have no charged particles

Question 9

Macromolecular Crystal Structure

Answer 9

These substances are covalently bonded into a giant lattice structure. Each atom has multiple covalent bonds which are very strong, giving it a very high melting point. Macromolecular substances are rigid.

Question 10

Linear

Answer 10

2 bonding pairs and a bond angle of 180

Question 11

Bent

Answer 11

2 bonding pairs, 2 lone pairs and a bond angle of 104.5

Question 12

Trigonal planar

Answer 12

3 bonding pairs and a bond angle of 120

Question 13

Triangular pyramid

Answer 13

3 bonding pairs, 1 lone pair and a bond angle of 107

Question 14

Tetrahedral

Answer 14

4 bonding pairs and a bond angle of 109.5

Question 15

Trigonal bipyramid

Answer 15

5 bonding pairs and bond angles of 90 and 120

Question 16

Octahedral

Answer 16

6 bonding pairs and a bond angle of 90

Question 17

Electronegativity

Answer 17

The power of an atom to attract negative charge towards itself within a covalent bond

Question 18

Induced dipole

Answer 18

Can form when the electron orbitals around a molecule are influenced by another charged particle

Question 19

Van der waals forces

Answer 19

Weakest type of intermolecular force. It acts as an induced dipole between molecules

Question 20

Permanent dipole

Answer 20

Acts between molecules with a polar bond. The δ- and δ+ regions attract each other and hold the molecules together in a lattice-like structure

Question 21

Hydrogen bonding

Answer 21

Strongest type of intermolecular force. Only form between hydrogen and nitrogen / oxygen / fluorine. The lone pair on these atoms forms a bond with a hydrogen atom from another molecule.