Topic 1

Question 1

State the number or orbitals and electrons in the s sub-shell

Answer 1

1 orbital and 2 electrons

Question 2

State the number or orbitals and electrons in the p sub-shell

Answer 2

3 orbitals and 6 electrons

Question 3

State the number or orbitals and electrons in the d sub-shell

Answer 3

5 orbital and 10 electrons

Question 4

State the number or orbitals and electrons in the f sub-shell

Answer 4

7 orbitals and 14 electrons

Question 5

Define relative atomic mass

Answer 5

Is the weighted mean mass of an atom of an element compared to 1/12th the mass of carbon 12 atom

Question 6

Define relative isotopic mass

Answer 6

Is the mass of an atom of an isotope compared to 1/12th the mass of carbon 12 atom

Question 7

How can mass spectrometry be used to determine the relative molecular mass of a molecule

Answer 7

The heaviest ion has the greatest m/z value and is likely a molecular ion.
You would look at the peak with the highest value

Question 8

Define first ionisation energy

Answer 8

The energy per mole needed to remove an electron from gaseous state

Question 9

Define second ionisation energy

Answer 9

Energy per mole needed to remove an electron fro gaseous ions with a single positive charge

Question 10

What are the factors that influence ionisation energies

Answer 10

1) nuclear charge - the more protons in the nucleus, the greater the attraction
2)atomic radius- the bigger the atom, the further the distance is from the other electron and the nucleus. Therefore a weaker attraction to the nucleus
3)shielding- when an electro on in its outer shell is repelled by the electron in its inner shell, the weaker the attraction in the nucleus.

Question 11

Describe the increase of the first ionisation energy across the period

Answer 11

As the number of protons increases it creates a greater attraction between the nucleus and outer electron

Question 12

What is successive ionisation energy

Answer 12

Provides evidence for quantum shells. There is a large increase in first ionisation energy from one shell to the next.

Question 13

S,p,d block classifies what elements

Answer 13

S- metals
D- transition
P- non-metals

Question 14

Why does the first ionisation energy decrease down the group.

Answer 14

Energy of the sub shells in which electrons are removed increases
Shielding increase

Question 15

What is periodicity

Answer 15

Is a repeating pattern of physical and chemical properties across different periods