Periodicity - Module 3

Question 1

What does a row represent on the periodic table ?

Answer 1

Number of shells

Question 2

What is the order of sub shells

Answer 2

S P D F

Question 3

Definition of First Ionisation Energy

Answer 3

Energy required to remove 1 mol of electrons from 1 mol of atoms of an element in the gaseous state to form 1 mol of gaseous ions

Question 4

Give the equation for the first ionisation energy of sodium

Answer 4

Na(g) —-> Na+ + E-

Question 5

Give the factors effecting first ionisation energy

Answer 5

Nuclear charge
Atomic radius
Shielding
Atomic attraction

Question 6

What happens to ionisation energy as you move down a group ? NASA

Answer 6

Nuclear charge - increases as no of protons increases , increased attractive force
Atomic radius - increases as no of shells increases
Shielding - increases as there are more full shells of electrons
Attraction - Decreases

Question 7

What happens to ionisation energy as you move across a period ? NASA

Answer 7

Nuclear charge - increases
Atomic radius - decreases slightly as electrons more attracted to nucleus
Shielding - same
Attraction - increases so ionisation energy increases

Question 8

What happens to ionisation energy as more electrons are removed and why

Answer 8

ie increases as it is harder to remove an electron from a positive ion

Question 9

What does a large jump in an ionisation energy graph show ?

Answer 9

A change of shell