electrons and ionisation

Drawing shape of s- orbital and p orbital

Writing electronic config of ions such as Fe 2+

The electrons are removed from 4s sub shell first not from the 3d sub-shell first as electrons in the 4s sub-shell are higher in energy than electrons in the 3d sub-shell

Using electronic config of two elements across period 2 one for group 2 and group 7 then the same for period 3 to explain why electronic config is an example of a periodic trend

Main answer in MS: across period 2 the s subshell fills first followed by the p sub-shell, same pattern or trend of filling the subshells repeated in other periods

Across each period elements repeat the pattern of electrons filling the s subshell then p subshell

OR since groups are mentioned (given in the ALLOW part of MS)

Elements in the same group have the same number of electrons in their outer shells or sub shell

My forms 2+ ions but Cl usually forms 1- ions in their reactions explain why

Mg loses 2 electrons, Cl gains an electron to gain a full shell

two elements contains 5 unpaired d electrons

The one that has electronic config ending 3d5 and also the one before it, not sure why chat GPT says the one before it has 4s1 and 3d5 instead of 4s2

How many p orbitals occupied by electrons in a .. atom

Include those that have only one electron

6 marker about electronic config and transition metals

Describe the relative energies of the 2s orbital and each of the 3 2p orbitals in an atom

P orbitals have greater energy than s orbitals

The three p-orbitals have equal energy

State the number of electrons in the fourth shell

32

How many orbitals are there in the 3rd shell

9

Number of electrons in a 3p orbital

2

krypton is found in period 4 of the periodic table explain how the electronic config confirms this

The highest shell number is 4

In the electron in box representation of an element what property of electrons is represented by the arrows

Spin

In electron in box representation of an element all arrows are pointing in the same direction identify error made

The paired electrons should have opposite spins

Define the term first ionisation energy

Energy required to remove 1 mol of electrons from 1 mol of gaseous atoms

Write an equation with state symbols to show the FIE of oxygen, second ionisation

O (g) —> O 1+ (g) + e-

O+ (g) —> O 2+ (g) + e-

Explain the trend in FIE down a group

Decreases down the group

Atomic radius increases, outer electron is further away from nucleus

Shielding increases

Outer electron experiences weaker nuclear attraction so less energy required to remove outer electron

Oxygen is in group 6 how would successive ionisation energies show this

There would be a large increase between the sixth and seventh ionisation energy values

Explain why the FIE of O (group 6) is lower than the FIE of N (group 5)

Oxygen has two paired electrons in its 2p subshell whereas nitrogen has no paired electrons

The paired Electrons in oxygen repel one another so it is easier to remove them

Explain why the FIE of N (group 5) is higher than the FIE of C (group 4)

Nitrogen has more protons than carbon

So there is increased attraction between the nucleus and the outer electrons in nitrogen making outer electrons harder to remove

Shielding is similar across a period so has no effect here

The variation in FIE across a period of the periodic table provided evidence for what structure within an atom

subshells

Out of Li (Group 1, 3electrons) , Be (Group 2, 4 electrons) and F (group 7 ,9 electrons) which has the largest second ionisation energy

Lithium as the second electron is on the first shell which is closer to the nucleus compared to the second electron of Be and f which is still in the second shell, attraction for outer electron to nucleus is stronger so more energy is needed to remove this electron

Explain why xe has a lower FIE than neon

Xe has a bigger atomic radius, more shells

Xe has more shielding

The nuclear attraction decreases, outermost electrons of Xe experience less attraction to nucleus , increased shielding/ distance outweighs the increased nuclear charge

Explain how the attraction between nucleus and outermost electron varies across period 3

Attraction between nuclei and outermost electrons increases across period, the nuclear charge increases, outer electrons are in the same shell, experience similar shielding as they have same number of shells, atomic radius decreases

explain why ionisation energy increases with ionisation number

radius decreases, attraction between remaining electrons and nucleus increases

same number of protons attract fewer electrons

explain how ionisation energy values provides evidence for electron shells

large increase shows a different/ new shell

large increase between ..  and .. ionisation energy value

using ionisation energy values to suggest what group the element is in (group 6)

large increase between 6th and 7th ionisation energies

this is when electron is being removed from the 2nd energy level, lower energy level/shell, from an energy level closer to the nucleus

Using electron in box representation determine which element has highest FIE

If you can’t figure out don’t guess look where these elements would be as you know trend down the group and across periods so

Notice

For a couple of transition metals it is 4s1 and 3d10 or something like copper shown in lesson SharePoint resources , previously pointed out by PMT exam questions , cha gpt said some elements have half filled 4d orbitals I AM NOT SURE ABOUT THIS THO AT ALL I THINK IT IS ALWAYS 4S2 3D WHATEVER

Even tho FIE of Sr is greater than FIE or Rb , the SECOND IE of Rb is she water than SIE of Sr explain why

2nd IE of Rb involved removing electron from shell closer to the nucleus

Stronger nuclear attraction of Rb , outermost electron of Rb experiences less shielding