3.1 - The periodic table and periodicity

Question 1

What are the factors that affect electronegativity ?

Answer 1

• Nuclear charge
• Atomic radius
• Shielding

Question 2

Define the term ‘electronegativity’ ?

Answer 2

Electronegativity - The power of an atom to attract the electrons in a covalent bond

Question 3

Explain how nuclear charge affects electronegativity ?

Answer 3

• The more protons in the nucleus, the stronger the electrostatic attraction between the nucleus and bonding pairs of electrons

Question 4

Explain how atomic radius affects electronegativity ?

Answer 4

• The smaller the atomic radius, the mallee the distance between the outer shell electrons and nucleus
• This means the electrostatic attraction between the nucleus and bonding pairs of electrons is stronger

Question 5

Explain how shielding affects electronegativity ?

Answer 5

• As the number of shields increases there are more electrons between the nucleus and the bonding pairs of electrons
• This means the electrostatic attraction between the nucleus and bonding pairs of electrons in weaker electrons

Question 6

What is the trend in electronegativity down the group ?

Answer 6

As you go down the group, the electronegativity decreases

Question 7

Explain the trend in electronegativity down the group ?

Answer 7

• As you go down the group the atomic radius and shielding increases
• This means there is more distance and a larger number of electrons between the nucleus and the bonding pairs of electrons
• This weak rand the electrostatic force between the nucleus and bonding pairs of electrons

Question 8

What is the trend in electronegativity across the period ?

Answer 8

As you go across the period, the electronegativity increases

Question 9

Explain the trend in electronegativity across the period ?

Answer 9

• As you go across the period the atomic radius decreases and the number of protons increases meaning the relative nuclear charge increases
• This means there is shorter distance between the nucleus and bonding pairs of electrons
• This means that the electrostatic attraction between the nucleus and bonding pairs of electrons is stronger