Bonding

Question 1

What is ionic bonding?

Answer 1

Ionic bonding is when ions are held together by electrostatic attraction.

Question 2

Ionic crystal is a giant latices of ions give one example of a giant ionic lattice:

Answer 2

NaCl

Question 3

How does the ionic structure explain the behaviour of ionic compounds?

Answer 3

Ionic compounds conduct electricity when they are molten or dissolved. When the items are liquid electrons are free to move and carry a charge however when they are solid the ions are fixed in a position by strong ionic bonds.

Ionic compounds have high melting points. Giant ionic lattice is are held together by strong electrostatic forces and so lots of energy is needed to overcome these forces.

Ionic compounds tend to dissolve in water. Water molecules are polar and so these polar molecules Paul ions away from the ionic lattice causing it to dissolve.

Question 4

Give an example of a giant covalent structure:

Answer 4

Graphite/diamond

Question 5

The structure of graphite explains its properties. State these properties and explain what causes them.

Answer 5

Graphite feels slippery and is used as a dry lubricant in pencils - The weak bonds between the layers in graphite are easily broken so layers can slide over one another.

Graphite is an electrical conductor - do you localised electrons in graphite aren’t attached to any particular carbon atom and so are free to move along the sheets carrying a charge.

Graphite has a low density and is used to make strong, lightweight sports material - The layers between each sheet are far apart causing it to have a low density.

Graphite has a high melting point - Strong covalent bonds between the hexagon sheets cause it to have a high melting point.

Graphite is insoluble in any solvent - The covalent bonds in the sheets are too strong to break.

Question 6

State the properties of diamond’s and what causes them:

Answer 6

Diamond has a high melting point due to the strong covalent bonds.

Dyment is extremely hard do you to strong covalent bonds

Diamond is a good thermal conductor due to vibration is travelling easily through the stiffer lattice caused by the strong covalent bonds.

Diamond cannot conduct electricity as the outer electrons are held in localised funds.

Diamond is indissoluble due to the strong covalent bonds.

Question 7

What is a dative/co-ordinate bond?

Answer 7

A covalent bond in which the shared pair of electrons originates from the same atom.

Question 8

What is the bond angle of a linear molecule and give an example of one.

Answer 8

BeCl2

180°

Question 9

What is the bond angle of a trigonal planar and give an example of one.

Answer 9

BF3

120°

Question 10

What is the bond angle of a tetrahedral structure and give an example of one.

Answer 10

NH4+

109.5°

Question 11

What is the bond angle in I trigonal pyramidal molecule and give an example of one.

Answer 11

PF3

107°

Question 12

What is the bond angle in a bent molecule give an example of one:

Answer 12

H2O

104.5°

Question 13

What are the bond angles in a trigonal bipyramidal molecule and give an example of one:

Answer 13

PCl5

120° and 90°

Question 14

What are the bond angles in a seesaw molecule and give an example of one:

Answer 14

102° and 87°

SF4

Question 15

What is the bond angles in a T-shaped molecule and give an example of one:

Answer 15

ClF3

88°

Question 16

What is the bond angle in and octahedral molecule and give an example of one what is the bond angle in and octahedral molecule and give an example of one:

Answer 16

SF6

90°

Question 17

What is the bond angle in a square playing or molecule and give an example of one:

Answer 17

XeF4

90°

Question 18

Definition of a polar bond:

Answer 18

A covalent bond between two atoms in which electrons are not equally shared, giving one atom a slight positive charge and a slight negative charge.

Question 19

Give an example of a polar molecule and a non-polar molecule:

Answer 19

Water is polar

Carbon Dioxide is non-polar

Question 20

What are the types of intermolecular forces?

Answer 20

Induced dipole-dipole / Van Der Waals forces

Permanent dipole-dipole forces

Hydrogen bonding

Question 21

How do Van der Waals forces effects boiling points?

Answer 21

The larger the molecule the stronger the Van der Waals forces and so the higher the boiling point.

Question 22

What is the strongest type of intermolecular forces?

Answer 22

Hydrogen bonding

Question 23

What type of bonding is present metals?

Answer 23

Metallic bonding.

Question 24

How does metallic bonding explain the properties of metals?

Answer 24

The high melting point is because of the strong electrostatic attraction between the positive metal ion and the sea of the delocalised electrons.

They are good thermal conductors as the delocalised electrons can pass kinetic energy to one another.

Metals are good electrical conductors because the delocalised electrons can move and carry a current.

Metals are because of the strength of the metallic bonds.

The melting point of metals vary depending on the number of delocalised electrons per atom. The more delocalised electrons there are the stronger the bonding will be and so the higher the melting point.