Atomic Structure And Bonding

Question 1

Define isotope

Answer 1

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons.

Question 2

Describe the bonding and structure of an ionic compound.

Answer 2

Giant ionic lattice structure with a strong electrostatic forces of attraction between the oppositely charged ions.

Question 3

Explain why graphite/diamond/silicon dioxide have higher m.p/b.ps

Answer 3

They have giant molecular structures. The strong and extensive covalent bonds require a lot of energy to break.

Question 4

Why do substances with SMS have low b.p/m.p?

Answer 4

Only a small amount of energy is required to overcome the weak intermolecular forces of attraction between the molecules.

Question 5

Why can diamond/silicon dioxide not conduct electricity?

Answer 5

All valence electrons of (ELEMENT) are used for covalent bonding. There are no free moving electrons to allow diamond/silicon dioxide to conduct electricity.

Question 6

Why can graphite conduct electricity?

Answer 6

3/4 valence electrons of each carbon atom are used for covalent bonding with other carbon atoms. Each carbon atom has one non-bonding electron. There are free moving electrons for electrical conduction.

Question 7

Why is diamond hard?

Answer 7

Each carbon atom is held by strong covalent bonds to another 4 C atoms in a tetrahedral arrangement. Large amounts of energy is required to overcome the strong and extensive covalent bonds between the carbon atom.

Question 8

What 3 metals form amphoteric oxides?

Answer 8

Zn/Al/Pb