Chapter 1 Multiple Choice Questions

1. What is an atomic orbital?

Any wavefunction obtained as a solution of the Schrödinger equation.

The wavefunction describing an electron in an atom.

Any wavefunction that describes an electron.

2. What is penetration?

The potential presence of an electron inside the shells of other electrons.

The high probability of finding s electrons at the nucleus.

Presence of more than one subshell within one atomic shell.

3. Find the correct trend in atomic radii.

Atomic radii generally increase down a group and from left to right across a period

Atomic radii remain constant down a group and decrease from left to right across a period

Atomic radii generally increase down a group and decrease from left to right across a period.

4. Chemical elements are organized in Mendeleev's periodic table. The location of the transition metals is:

the Lanthanoid and Actinoid groups

the groups occupying the p-block

groups 3 through 11

5. Discrete lines in the emission spectrum of hydrogen atoms suggest that:

Electrons can occupy only certain, discrete energy levels in the atom.

Electrons occupy continuous energy levels (i.e., any levels) in the atom.

Emission spectral lines do not tell us anything about the energy levels of the electrons in atoms.

6. Two wave functions spread in the same region of space and interact with each other. This interaction yields a resultant wave function with an amplitude that exceeds the amplitudes of the individual wave functions. Therefore:

The interaction is constructive; i.e., it is highly likely to find electrons in the interaction region.

The interaction is destructive; i.e., it is highly unlikely to find electrons in the interaction region.

The interaction is constructive; i.e., it is highly unlikely to find electrons in the interaction region.

7. The square of a wave function, Ψ², is found to be zero for a certain region of an atom. This finding is interpreted as:

It is highly likely to find the electron in this region.

The probability of finding the electron in the region where Ψ²=0 is null.

The probability of finding the electron in the region where Ψ²=0 is low.

8. The set of orbitals that is defined by quantum numbers n = 2 and l = 2 is:

not permitted

one 2s orbital

three 2p orbitals

9. Which of the following correctly defines electron affinity:

E_a = E(A,s) – E(A^–, s) at T = 0K

E_a = E(A,g) – E(A^–, g) at T = 273K

E_a = E(A,g) – E(A^–, g) at T = 0K

10. Which of the following statements is correct?

Elements that are found in the lower left corner of the periodic table possess the highest value of the first ionization energy, while those found in the upper right corner possess the lowest value. In addition, elements in the top right corner of the periodic table possess the highest values of electron affinity.

Elements that are found in the lower left corner of the periodic table possess the lowest value of the first ionization energy, while those found in the upper right corner possess the highest value. In addition, elements in the top right corner of the periodic table possess the highest values of electron affinity.

Elements that are found in the lower left corner of the periodic table possess the lowest value of the first ionization energy, while those found in the upper right corner possess the highest value. In addition, elements in the top right corner of the periodic table possess the lowest values of electron affinity.

Chapter 1 Multiple Choice Questions

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