The Periodic Table - exam practice
The Periodic Table
Question 1 of 5
Melting points show a trend across a period.
The melting points of some period 3 elements are shown in the table below.
Explain the trend shown in melting point, in terms of structure and bonding.
Define the term first ionisation energy.
State and explain the trend in first ionisation energy of the elements in group 2.
The first ionisation energy of aluminium is lower than that of magnesium.
Give the full electronic configurations of an atom of aluminium and an atom of magnesium.
Explain the difference in the first ionisation energies of the two metals.
This question is about the periodicity of the period 3 elements.
State and explain the general trend in first ionisation energy across period 3.
Give one example of an element which deviates from the general trend in first ionisation energy across Period 3.
Explain why this deviation occurs.
Identify the element in period 3 that has the highest melting point.
Explain your answer in terms of structure and bonding.
Identify the metallic element in period 3 that has the highest melting point.
Explain your answer in tems of structure and bonding
The melting points of the period 3 elements are shown in the table below.
Explain the trend in melting points across the elements of period 3 in terms of their structure and bonding.
Phosphorus undergoes many reactions.
State the full electronic configuration of the phosphorus atom.
State, giving a reason, whether the phosphorus atom or the phosphide ion has a larger radius.
Outline why the phosphorus atom has a smaller atomic radius than the sodium atom.
Considering only the elements in periods 1-3, name the element with the highest first ionisation energy.