Atomic structure, periodic trends: Practice Questions

Which of the following combinations correctly identifies the relative mass and relative charge of an electron?

Which statement best explains why Fluorine is more reactive than Iodine in Group VII?

Elements X, Y, Z, and W are four consecutive elements in Period 3 of the Periodic Table, listed in order of increasing atomic number. The first ionization energies (\(IE_1\)) in kJ mol\(^{-1}\) for these elements are approximately:

X: 786, Y: 1012, Z: 1000, W: 1251

Which of the following statements concerning the second ionization energies (\(IE_2\)) of these elements is correct?

An atom of element \(X\) has an atomic number of \(16\). Which of the following correctly describes the position of \(X\) in the Periodic Table?

Which of the following correctly describes the trend in reactivity for the Group I metals Lithium, Sodium, and Potassium?

State the relative mass and the relative charge of a proton.

Explain why the melting point of Group I elements (alkali metals) decreases down the group from lithium (\( \text{Li} \)) to potassium (\( \text{K} \)).

The first ionization energies of three consecutive elements, \( \text{X} \), \( \text{Y} \), and \( \text{Z} \), show a sharp decrease from \( \text{Y} \) to \( \text{Z} \). Given that \( \text{Y} \) is a noble gas in Period 2, explain why the atomic radius of \( \text{Z} \) is significantly larger than that of \( \text{Y} \).

Boron (\( \text{B} \)) is an element with an atomic number of 5 and a mass number of 11.

(a) Calculate the number of neutrons present in the nucleus of a boron atom.

(b) State the electronic arrangement of a neutral boron atom.

(c) Identify the group number and period number of boron in the Periodic Table.

(d) Boron is classified as a metalloid. Explain what this term means in terms of the properties of the element compared to metals and non-metals.

The periodic arrangement of elements allows chemists to understand and predict physical and chemical properties based on atomic structure and electron configurations.

(a) The first eight successive ionization energies (\(IE\)) in \( \text{kJ mol}^{-1} \) for an element X in Period 3 are as follows:
\( IE_1: 1251 \)
\( IE_2: 2298 \)
\( IE_3: 3822 \)
\( IE_4: 5159 \)
\( IE_5: 6542 \)
\( IE_6: 9362 \)
\( IE_7: 11018 \)
\( IE_8: 33604 \)

Identify element X and justify your answer using the data provided. (2 points)

(b) Argon (\( Z=18 \)) is located immediately to the right of element X in Period 3. Compare the first ionization energy of Argon with that of element X, and provide a reason for the difference based on their atomic structures. (2 points)

(c) Arrange the atoms Fluorine (\( Z=9 \)), Chlorine (\( Z=17 \)), and Sodium (\( Z=11 \)) in order of increasing atomic radius. Justify your arrangement by referring to their electronic arrangements and nuclear charges. (2 points)

(d) Transition metals and their compounds are widely utilized as catalysts in industrial chemistry.
(i) Identify the transition metal catalyst used in the Contact Process for the manufacture of sulphuric acid and state its oxidation state in the catalyst compound.
(ii) Explain, in general terms, why transition metals are effective as catalysts. (2 points)