Bonding

Question 1

What type of bonding exists in monatomic gases?

Answer 1

LD Forces

Question 2

What are London Dispersion Forces

Answer 2

They are weak attraction between atoms

Question 3

Explain why sodium has a lower melting point than magnesium

Answer 3

Sodium has a stronger attractive force between the cations and the delocalised electron. Therefore, metallic bonding in magnesium is stronger than in sodium

Question 4

Explain why sodium has a higher melting point than Caesium

Answer 4

This is because Caesium is larger in size. Which means the charge gets spread out evenly and caesium can be separated by using lesser energy.

Question 5

Explain why Xenon has a higher bp than Argon

Answer 5

This is because it has more outer electrons to be evenly distributed which therefore means that it will have more LDF

Question 6

What type of bonding contains positive ions and delocalized electrons

Answer 6

Metallic bonding

Question 7

Why does silicon have a significantly higher melting point than nitrogen

Answer 7

This is because Silicon is a covalent network which means that when it melts strong covalent bonds are broken. Nitrogen is a diatomic molecule which has LDF between the molecules

Question 8

Why does sulphur have a higher mpt than Chlorine

Answer 8

This is because Sulfur has a bigger molecule which means it has more electrons and stronger LDF

Question 9

Why does Potassium have a higher mpt than Argon

Answer 9

This is because Potassium has metallic bonding and Argon which is monoatomic have very strong LDF

Question 10

Explain how LDF arises

Answer 10

It occurs due to temporary fluctuations in electron density within the atom or molecule

Question 11

Explain how permanent dipole- permanent dipole interactions arises

Answer 11

It occurs due to the difference in electronegativity between the atoms in a molecule which leads to the formation of a permanent dipole force.

Question 12

Explain how hydrogen bonding occurs

Answer 12

It occurs due to hydrogen bonds being covalently bonded to highly electronegative elements like Nitrogen, Oxygen and Fluorine (NOF)

Question 13

What type of forces do polar substances have

Answer 13

They have permanent dipole/permanent dipole interactions.

Question 14

What type of forces do Non-polar substances have?

Answer 14

They have London Dispersion Forces (LDF)

Question 15

What is a covalent bond

Answer 15

It is two positive nuclei sharing electrons.

Question 16

What is a polar covalent bond

Answer 16

It occurs when two atoms share electrons unequally due to difference in electronegativity

Question 17

What is a non-polar/pure covalent bond

Answer 17

It occurs 2 atoms share electrons equally due to having the SAME electronegativity

Question 18

Name the 3 types of intermolecular bonding

Answer 18

LDF
Permanent dipole-permanent dipole interactions
Hydrogen bonding

Question 19

Explain why HCL has a higher boiling point than H2

Answer 19

This is because the LDF (Van der Waals Force) in HCL is stronger than the LDF in H2

Question 20

Explain why the boiling point of HALOGENS increases going down the group?

Answer 20

Intermolecular forces increases going down the group

LDF’s are the forces broken btw the molecules

The more the electron the stronger the LDF’s