Bonding and physical properties

Question 1

Describe the arrangement of particles in a solid, and provide evidence

Answer 1

• Regular arrangement
• Crystals have straight edges

Question 2

Describe the spacing of particles in a solid, and provide evidence

Answer 2

• Close
• Not easily compressed

Question 3

Describe the movement of particles in a solid, and provide evidence

Answer 3

• Just vibrate
• Slow diffusion

Question 4

Describe the arrangement of particles in a liquid, and provide evidence

Answer 4

• Random arrangement
• Particles change shape to fit the shape of a container

Question 5

Describe the spacing of particles in a liquid, and provide evidence

Answer 5

• Close
• Not easily compressed

Question 6

Describe the movement of particles in a liquid, and provide evidence

Answer 6

• Rapid ‘jostling’
• Slow diffusion, evaporation

Question 7

Describe the arrangement of particles in a gas, and provide evidence

Answer 7

• Random
• Will fit it’s container

Question 8

Describe the spacing of particles in a gas, and provide evidence

Answer 8

• Far apart
• Easy to compress

Question 9

Describe the movement of particles in a gas, and provide evidence

Answer 9

• Rapid movement
• Rapid diffusion, exertion of pressure

Question 10

Describe the forces in giant ionic structures

Answer 10

Ions are held together by strong electrostatic forces of attraction

Question 11

Describe the forces in giant covalent structures

Answer 11

Atoms are held together by strong covalent bonds

Question 12

Describe the forces in simple covalent structures

Answer 12

Molecules are held together by weak intermolecular forces of attraction

Question 13

Describe the forces in giant metallic structures

Answer 13

Metal ions are held together by a sea of delocalised electrons

Question 14

Describe how the structure of diamond links to its function

Answer 14

• Diamond is made up of the element carbon, and each carbon atom is covalently bonded to 4 other carbon atoms.
• Diamond has a high melting and boiling point due to its huge number of covalent bonds, which requires a great deal of energy to overcome.
• Diamond cannot conduct electricity because there are no free electrons to carry electrical charge through the structure.

Question 15

Describe how the structure of graphite links to its function

Answer 15

• Graphite is formed by the element carbon, where each carbon atom is covalently bonded to 3 other carbon atoms, in the form of hexagonal rings.
• Graphite has a high melting and boiling point because graphite has many strong covalent bonds, which requires a great deal of energy to overcome.
• Graphite is soft and slippery because there are no covalent bonds between the layers, so they can slide over each other.
• Graphite is also an excellent conductor of heat and electricity because each carbon atom has a delocalised electron, which carries a charge through the structure.