past paper questions Flashcards

1
Q

state what is meant by two arrows in the first box, (↑↓)

A

2 electrons spinning with opposite spins

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2
Q

state why the arrows are all pointing in the same direction in the 3p boxes.

A

3 e- with the same direction of spin

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3
Q

explain why iodine and chlorine have many similar chemical reactions

A

1- there is 7 e- in their outer shell
2- number of electrons govern chemical reactions

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4
Q

explain why the first ionisation energy of magnesium is higher than of sodium. (3)

A

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

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5
Q

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)

A

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

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6
Q

explain the trend in the values of the first ionisation energies for the group containing sulfur. (3)

A

1- first ionisation energy decrease although num. of protons increases
2- 1+ electron shell further away from nucleus
3- e- experience more shielding

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7
Q

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)

A
  • 1st & 2nd electron removed from the same sub-shell
  • 3rd e- removed from a sub-shell closer to the nucleus
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8
Q

the elements zinc & scandium are d-block elements but not transition metals;
discuss this statement with electron configurations. (4)

A
  • 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

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