Metallic bonding

Question 1

Explain metallic bonding

Answer 1

When there are no nonmetals to gain electrons, the metals become positive and the electrons become delocalized. The cations are surrounded by a sea of electrons.

Question 2

What gives metals the characteristics of malleability, ductility, conducting electricity and heat, and shine/luster?

Answer 2

The delocalized electrons make it easier to move.

Question 3

Relationship between delocalized e- and hardness/strength

Answer 3

As the number of delocalized e- increases, the strength and hardness of the metal increases.

Question 4

Relationship between the size of the cation and the strength of the metallic bond

Answer 4

The smaller the cation, the stronger the metallic bond because they can get closer together.

Question 5

Na+1 and Mg+2

Answer 5

Mg+2 is smaller and has more delocalized e- so it has a stronger metallic bond.

Question 6

Why do transition metals have greater delocalized e-?

Answer 6

They have the 4s and 3d so they have greater metallic bonding.

Question 7

Alloy

Answer 7

Homogeneous mixture (solid solution)

Question 8

The effects of adding another element to the metal

Answer 8

It changes the properties of the original metal. Disrupts the layers making the metal less malleable and stronger.

Question 9

Interstitial alloy

Answer 9

The added atoms are smaller than the original metal atoms and fits into the spaces between metal atoms.

Question 10

Steel

Answer 10

interstitial alloy of iron and carbon

Question 11

Substitutional alloy

Answer 11

the added atoms are similar in size to the original metal atoms and replace some of the original metal atoms. (Less movement - less malleable and ductile and harder.)

Question 12

Brass

Answer 12

copper and zinc (substitutional)

Question 13

Bronze

Answer 13

copper and tin (substitutional)