Electronegativity and Intermolecular Forces

Question 1

Define Electronegativity

Answer 1

The tendency for an atom to attract the electron density in a covalent bond towards itself

Question 2

What factors affect electronegativity

Answer 2

Nuclear charge
Electron Shielding
Nuclear Radius

Question 3

Explain what happens to electronegativity going down a group

Answer 3

Electronegativity decreases due to increased electron shielding that increases the atoms size, expanding the size of the atom and reducing electrostatic attraction while also increasing forces of repulsion between the bonding electron and the electrons in their orbitals

Question 4

Explain what happens to electronegativity going across a period.

Answer 4

Electronegativity increases as the electron shielding remains constant. The atoms become smaller as outer shell electrons increase, increasing nuclear charge and increasing electrostatic attraction between bonding electrons.

Question 5

What happens in polar bonds

Answer 5

Uneven sharing of electrons

Question 6

What are van der waals forces

Answer 6

Uneven distribution of electrons in an atom or molecule stimulates temporary dipoles causing weak electrostatic attraction. Also know as London dispersal forces, grows stronger with more electrons

Question 7

What is hydrogen bonding

Answer 7

A hydrogen atom between 2 very electronegative atoms
Only occurs with O N and F
Must have a lone pair of electrons

Question 8

What is the order of intermolecular forces from strongest to weakest

Answer 8

Hydrogen bonding
dipole - dipole
van der waals