Metallic Bonding_Key Questions

Question 1

What does the Metalic Bonding Model Teach you?

Answer 1

teaches you how the properties of metals can be explained in terms of the structure of the particles in metals model helps understand why metals behave as they do

Question 2

Metals are usually hard and tend to have high boiling points. What does this tell us about the structure?

Answer 2

The forces between the particles must be strong

Question 3

Metals conduct electricity in the solid state and in the molten liquid state. What does this tell us about the structure?

Answer 3

Metals have charged particles that are free to move

Question 4

Metals are malleable and ductile. What does this tell us about the structure?

Answer 4

The attractive forces between the particles must be stronger than the repulsive forces between the particles when the layers of particles are removed

Question 5

Metals generally have high densities. What does this tell us about the structure?

Answer 5

The particles are closely packed in a metal

Question 6

Metals are good conductors of hear. What does this tell us about the structure?

Answer 6

There must be a way of quickly transferring energy throughout a metal object

Question 7

Metals are lustrous or reflective. What does this tell us about the structure?

Answer 7

Free electrons are present, so metals can reflect light and appear shiny.

Question 8

Metals tend to react by losing electrons. What does this tell us about the structure?

Answer 8

Electrons must be relatively easily removed from metal atoms

Question 9

What are electrons?

Answer 9

• the particles that enable metals to conduct electricity - they can move between the lattice of metal atoms - negatively charged electrons can be lost from the outer shell of metal atoms, forming positive ions (cations)

Question 10

What does a sold piece of metal contain?

Answer 10

• positive ions are arranged in a closely packed structure - negatively charged electrons move freely throughout the lattice. Called delocalised electrons as they belong to the lattice as a whole rather than staying in the shell of a particular atom - delocalised electrons come from the outer shells of the atoms. - positive cations are held in the lattice the electrostatic force of attraction between these cations and the delocalised electrons

Question 11

What are the limitations of the Metallic Bonding Model?

Answer 11

The following properties of metals cannot be explained using the metallic bonding model: - Metals have a range of melting points, hardness and densities of different metals - Differences in electrical conductivities of metals - Magnetic nature of metals, such as cobalt, iron and nickel

Question 12

Describe the forces that hold the calcium’s lattice together

Answer 12

Strong electrostatic forces of attraction between Ca2+ ions and the delocalised valence electrons

Question 13

Barium is an element in Group 2 of the periodic table. It has a melting point of 850 degrees and conducts electricity in the solid State. Describe how the properties of Barium can be explained in terms of its bonding structure.

Answer 13

Barium has a high melting temperature because there are strong attractive forces between the positive ions and the delocalised electrons. Barium conducts electricity because the delocalised electrons from the outer shell are free to move.

Question 14

The atomic number of calcium is 20. How many electrons are in an atom of calcium and in Ca2+ atom?

Answer 14

20 in Ca, 18 in Ca2+

Question 15

Using the Metallic Bonding Model, explain how Copper wire conducts Energy.

Answer 15

When a current is applied to the copper wire, the free-moving, delocalised electrons move from one end to the other and so the copper wire conducts electricity.

Question 16

Using the Metallic Bonding Model, explain how a metal spoon used to stir a boiling mixture becomes too hot to hold

Answer 16

• The delocalised electrons in the metal spoon obtain energy from the boiling mixture and move more quickly. - These electrons move freely throughout the spoon, colliding with other electrons and metal ions, transferring energy so that the spoon becomes warmer and, eventually, too hot to hold.

Question 17

Draw a diagram to represent a calcium metal lattice.

Answer 17