1State and explain the trend in the first ionisation energies of the elements in group 2 from magnesium to barium (3)
- decrease
- ions get bigger / more (energy) shells
- weaker attraction of ion to lost electron
2This question is about the elements in Period 3 of the periodic table
State the element in Period 3 that has the highest melting point.
Explain your answer
(3)
- Silicon / Si
- COVALENT (bonds)
- strong or many of the (covalent) bonds need to be BROKEN / needs a lot of energy to BREAK the (covalent) bonds
3State the element in period 3 that has the highest first ionisation energy. Explain your answer (3)
Argon / Ar
Large(st) number of protons / large(st) nuclear charge
Same amount of shielding / same number of shells / same number of energy levels
4Suggest the element in period 3 that has the highest electronegativity value (1)
Chlorine / Cl
5Which one of the following is a fundamental particle that would not be deflected by an electric field?
6State, in terms of fundamental particles, why the isotopes 10B and 11B have similar chemical reactions (1)
- same number of electrons (in outer shell or orbital)
- Same electronic configuration / arrangement
7Q3c Complete Table 2 by suggesting a value for the third ionisation energy of boron (1)
range between 3500 and 10 000 kJ mol-1
8Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron (1)
electron being removed from a positive ion (therefore needs more energy) / electron being removed is closer to the nucleus.