Atomic structure：練習問題

Compared to the isotope \(^{56}Fe\), an atom of the isotope \(^{58}Fe\) has:

A beam of protons, neutrons, and electrons travels at a constant velocity into an electric field between two horizontal plates. The upper plate is positively charged and the lower plate is negatively charged.
Which statement describes the behavior of the particles?

The graph of successive ionisation energies for a Period 2 element shows a large jump between the second and third ionisation energies, and a very large jump between the eighth and ninth ionisation energies.
Which of the following species is a free radical of this element?

Which factor is primarily responsible for the general increase in first ionisation energy across Period 3?

Successive ionisation energies for an element Y are shown in the table below.

\(1^{st}\): 590 kJ mol\(^{-1}\)
\(2^{nd}\): 1145 kJ mol\(^{-1}\)
\(3^{rd}\): 4912 kJ mol\(^{-1}\)
\(4^{th}\): 6474 kJ mol\(^{-1}\)
\(5^{th}\): 8144 kJ mol\(^{-1}\)

What is the most likely formula for the chloride of element Y?

State the full electronic configuration of the sulfide ion, \(S^{2-}\).

Explain why the first ionisation energy of magnesium is higher than that of aluminium, despite aluminium having a higher nuclear charge.

An unknown element \(X\) has the following successive ionisation energies: \(578\), \(1817\), \(2745\), \(11577\), and \(14842 \text{ kJ mol}^{-1}\). Identify the Group of the Periodic Table to which element \(X\) belongs and justify your answer.

(a) Define the term isotope in terms of subatomic particles. (1)

(b) A specific ion of chlorine is represented by the notation \( ^{37}_{17}\text{Cl}^- \). Determine the number of protons, neutrons, and electrons present in this ion. (2)

(c) Explain why isotopes of the same element, such as \( ^{35}\text{Cl} \) and \( ^{37}\text{Cl} \), exhibit identical chemical properties. (1)

(a) Define first ionisation energy and write an equation, including state symbols, to represent the second ionisation energy of magnesium. (2)

(b) The successive ionisation energies for an element \( X \) in Period 3 are 578, 1817, 2745, 11577, and 14842 \( \text{kJ mol}^{-1} \). Identify the group to which element \( X \) belongs and explain your reasoning by referring to the electronic structure. (2)

(c) Explain why the first ionisation energy of sulfur is lower than that of phosphorus, despite sulfur having a higher nuclear charge. (1)