building up periodic table

Question 1

Aufbau principle

Answer 1

Each new element has one more nuclear charge than the preceding element - charge is neutralised by the addition of an electron in the lowest energy level possible

Question 2

If two electrons occupy the same orbital, why do they have different quantum numbers?

Answer 2

The electrons occupying the same orbital have different spins ( ms ) where one is up (+) and one down (-)

Question 3

What is ionisation energy?

Answer 3

The minimum energy required to remove an electron from an atom in its gaseous form in its ground state of electron configuration

Question 4

Why is it more difficult to remove an electron from a cation in comparison to a neutral atom?

Answer 4

There is more attraction to ??????

Question 5

What is oxidation state

Answer 5

The most likely ionic formulation based on relative electronegativities of the elements involved

Question 6

What is electronegativity

Answer 6

It is the power to attract a bonding pair of electrons

Question 7

What does homonuclear diatomic mean

Answer 7

The electron density is shared equally - usually found in diatomic molecules

Question 8

what is the electron configuration of Cr

Answer 8

[Ar] 4s1 3d5

Question 9

what is the electronic configuration of Cu

Answer 9

[Ar]4s1 3d10

Question 10

how does atomic radius change across a period and why?

Answer 10

DECREASES -
nuclear charge increases as you gain an extra proton
additional electrons enter the same outer shell
attraction increases between the CENTRE of the atom and THE OUTERMOST VALENCE ELECTRON

Question 11

how does atomic radius change down a period?

Answer 11

INCREASES 
gain an extra shell as you move down a period 
one shell further out 
increased distance from the nucleus 
increased shielding