Short Answer Questions on Structure and Bonding (Chemistry)
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Module
Introductory Chemistry I
Institution
The University Of The West Indies
Book
Chemistry(3)
This contains 5 papers with short answer questions on the following topics:
- Structure and Bonding
- Ionic bonding and crystalline structures
- Covalent bonding
- Molecular Orbital Theory
- Intermolecular Forces
1. Suggest a reason for the large decrease in electron affinity between Lithium and Beryllium.
2. Refer only to the periodic table and arrange the following ionization energies in order of increasing
value: the first ionization energy of F; the second ionization energy of Ba; the second ionization
energy of Na; the third ionization energy of Mg.
3. How would you expect the sizes of the hydrogen ion (H+), and the hydride ion (H-), to compare
with that of the H atom and the He atom? Explain.
4. The Na+ ion and the Ne atom are isoelectronic. The first ionization energy of Ne(g) has a value
2081 kJmol-1 whereas the second ionization energy of Na(g) has a value of 4562 kJmol-1. Why
are these values not the same?
5. Arrange the following in expected order of increasing radius: Br, Li+ Se, I-. Explain your answer.
6. Use Slater’s rules to determine Zeff for (i) a 3d electron and (ii) a 4 s electron of a Ground State
Cu atom. Comment on your results.
7. Use Slater’s rules to determine Zeff for the valence electron in each Group 1 element. Given that
the ionization energy (IE) is
𝐼𝐸 = 1312.1 𝑘𝐽𝑚𝑜𝑙−1 (𝑍2eff)
𝑛2
Determine the IE for each element and comment on the observed trend in the values.
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