past paper questions Flashcards
state what is meant by two arrows in the first box, (↑↓)
2 electrons spinning with opposite spins
state why the arrows are all pointing in the same direction in the 3p boxes.
3 e- with the same direction of spin
explain why iodine and chlorine have many similar chemical reactions
1- there is 7 e- in their outer shell
2- number of electrons govern chemical reactions
explain why the first ionisation energy of magnesium is higher than of sodium. (3)
1- Mg has a higher nuclear charge
2- stronger attraction to the e-
3- same level of shielding as they’re in the same quantum shell
The difference in rates of reaction of Sr and Ba with water is due to the difference in sum of 1st & 2nd ionisation energy. Discuss this suggestion. (6)
1- Ba has more protons, therefore greater nuclear charge
2- Ba experiences more shielding
3- sum of 1st & 2nd ionisation energy of Ba is lower
4- Ba has a larger atomic radius
5- Ba is more reactive
6- therefore outweighs larger nuclear charge
explain the trend in the values of the first ionisation energies for the group containing sulfur. (3)
1- first ionisation energy decrease although num. of protons increases
2- 1+ electron shell further away from nucleus
3- e- experience more shielding
explain why the difference between the 2nd & 3rd ionisation energies of Ca is much larger than the difference between the 1st & 2nd ionisation energies. (2)
- 1st & 2nd electron removed from the same sub-shell
- 3rd e- removed from a sub-shell closer to the nucleus
the elements zinc & scandium are d-block elements but not transition metals;
discuss this statement with electron configurations. (4)
- both elements have last added e- in subshell
- neither forms stable ion with incomplete d-subshell
- therefore are not transition metals
Zn3+: [Ar] 3d10 -> full d subshell
sc3+: [Ar] -> empty d subshell