What does first ionisation energy mean?
The successive ionisation energies for element A are listed in Table 1.1. Use Table 1.1 to work out the Periodic Table group to which A belongs. Justify your answer.
Along Period 3, first ionisation energies generally rise because the attraction between the nucleus and the outer electron increases. Explain why the first ionisation energy of sulfur is lower than the first ionisation energy of phosphorus.
In an $\text{Al}^{2+}$ ion the attraction from the nucleus to the outer electron is stronger than it is in an atom of Na. Compare the electronic structures of $\text{Al}^{2+}$ and an atom of Na and explain why the third ionisation energy of aluminium is greater than the first ionisation energy of sodium.
An isotope of copper has a relative isotopic mass of 65. Fill in Table 1.2 for an atom of copper-65.
Copper has a relative atomic mass of 63.5. Calculate the number of atoms in $1.05\ \text{g}$ of copper.
Copper melts at $1085^\circ\text{C}$ and has a high electrical conductivity. Explain these properties of copper with reference to its structure and bonding.