Periodic Table blocks and periodic trendsEdexcel International A Level Chemistry: Flashcards
What these 14 flashcards ask
- Which elements are in the s block?
- What are the maximum numbers of electrons in the s, p and d sub-shells?
- How many electrons can the third shell hold?
- What is a periodic property?
- Why are logarithms of ionisation energies plotted?
- Why does melting temperature rise from Na to Al?
- Why does silicon have the highest melting temperature in Period 3?
- Why are P₄, S₈ and Cl₂ low melting?
- Why does S₈ melt higher than Cl₂?
- Why does argon have the lowest melting temperature in Period 3?
- Why does the first ionisation energy generally increase across a period?
- Why is the first ionisation energy of Al lower than Mg?
- Why is the first ionisation energy of O lower than N?
- Why does the first ionisation energy decrease down a group?
Exam questions on Periodic Table blocks and periodic trends
- A student is sorting elements of the first four periods into the s, p and d blocks of the Periodic Table.Explain what is meant by the term periodic property and give one example.2 marks
- Melting and boiling temperatures vary across Period 2. Lithium melts at 181 °C and beryllium at 1287 °C. Carbon, as diamond, sublimes above 3500 °C. Nitrogen boils at −196 °C, oxygen at −183 °C, fluorine at −188 °C and neon at −246 °C.Explain why the melting temperature of beryllium is much higher than that of lithium.2 marks
- A student plots log₁₀ of the successive ionisation energies of magnesium against the number of electrons removed. The successive ionisation energies of magnesium are, in kJ mol⁻¹: 738, 1451, 7733, 10 543, 13 630, 17 995, 21 703, 25 656, 31 642, 35 462, 169 988 and 189 368.Calculate log₁₀ of the first three ionisation energies of magnesium, to two decimal places, and state one reason why logarithms are used.3 marks
Written by the Exaim team, led by Shaun Daswani (Head of Upper Secondary, Improve ME Institute; MSc Financial Mathematics, Imperial College London; BSc, UCL) and Jason Daswani (operational lead, Improve ME Institute; LSE).