General Chemistry Questions
Electronic Structure and Periodic Table
1. What value or values of ml are allowable for an orbital with l = 2?
a. 0
b. 2
c. -1
d. none of the above
e. all of the above
2. According to Bohr Theory, which of the following transitions in the hydrogen atom
will give rise to the least energetic photon?
Use the equation: En = (-2.18 x 10-18 J)(1/n2)
a. n = 5 to n = 3
b. n = 6 to n = 1
c. n = 4 to n = 3
d. n = 5 to n = 4
e. n = 6 to n = 5
3. Consider a 3dxz orbital. Which of the following statements is incorrect?
a. The xz plane is a nodal surface.
b. The xz plane divides the electron probability distribution into two identical
mirror-image halves.
c. The xy plane divides the electron probability distribution into two identical
mirror-image halves.
d. The yz plane divides the electron probability distribution into two identical
mirror-image halves.
e. The nucleus is located at a node.
4. The electronic configuration of the element whose atomic number is 26 is:
a. 1s2 2s2 2p6 3s2 3p6 4s0 3d8
b. 1s2 2s2 2p6 3s2 3p6 3d6 4s2
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d6
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d4 4p2
e. none of the above
5. Which of the following has the largest radius?
a. F
b. N
c. C
d. O
e. Ne
,6. Which of the following elements has the largest ionization energy?
a. Na
b. Ne
c. F
d. K
e. Rb
7. Which of the following has the greatest electron affinity (most negative value)?
a. Cl
b. K
c. He
d. Na
e. Rb
8. Which of the following species is not isolectronic with any of the others?
a. V3+
b. Ca2+
c. Ar
d. Cl-
e. S2-
9. In Bohr's model of the hydrogen atom, the radius of an orbit
a. is proportional to n2.
b. is smallest for the highest energy state.
c. increases when a photon of light is emitted from an excited atom.
d. can have any value that is larger than the ground-state radius.
e. none of the above
10. Which of the following atoms is not a one-electron system?
a. H
b. He+
c. Li2+
d. Be2+
e. O7+
11. Which of the following statements about periodic properties is incorrect?
a. Both electron affinity and ionization energy decrease down a group.
b. Atomic size increases to the right across a period.
c. Ionization energy increases to the right across a period.
d. Atomic size increases down a group.
e. Electron affinity increases to the right across a period.
, Bonding
1. Which one of the following is most likely to be an ionic compound?
a. HNF2
b. H2CO
c. N2H4
d. CaCl2
e. CH3Cl
2. In which of the following processes does the enthalpy change (ΔH) directly represent
the magnitude of the lattice energy of KCl(s)?
a. Cl2(g) + 2K(s) → 2KCl(s)
b. KCl(s) → K+(aq) + Cl-(aq)
c. KCl(s) → K+(g) + Cl-(g)
d. KCl(s) → K(s) + Cl-(g)
e. KCl(s) → K(s) + Cl(g)
3. Order the following by increasing bond strength: N≡N, N=N, N-N
a. N≡N, N=N, N-N
b. N≡N, N-N, N=N
c. N-N, N=N, N≡N
d. N=N, N-N, N≡N
e. N=N, N≡N, N-N
4. Which of the following compounds has the greatest bond polarity?
a. PH3
b. NH3
c. HF
d. H2S
e. CH4
5. Which of the following is not planar?
a. BCl3
b. ClF3
c. PCl3
d. XeF4
e. C2H4
Electronic Structure and Periodic Table
1. What value or values of ml are allowable for an orbital with l = 2?
a. 0
b. 2
c. -1
d. none of the above
e. all of the above
2. According to Bohr Theory, which of the following transitions in the hydrogen atom
will give rise to the least energetic photon?
Use the equation: En = (-2.18 x 10-18 J)(1/n2)
a. n = 5 to n = 3
b. n = 6 to n = 1
c. n = 4 to n = 3
d. n = 5 to n = 4
e. n = 6 to n = 5
3. Consider a 3dxz orbital. Which of the following statements is incorrect?
a. The xz plane is a nodal surface.
b. The xz plane divides the electron probability distribution into two identical
mirror-image halves.
c. The xy plane divides the electron probability distribution into two identical
mirror-image halves.
d. The yz plane divides the electron probability distribution into two identical
mirror-image halves.
e. The nucleus is located at a node.
4. The electronic configuration of the element whose atomic number is 26 is:
a. 1s2 2s2 2p6 3s2 3p6 4s0 3d8
b. 1s2 2s2 2p6 3s2 3p6 3d6 4s2
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d6
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d4 4p2
e. none of the above
5. Which of the following has the largest radius?
a. F
b. N
c. C
d. O
e. Ne
,6. Which of the following elements has the largest ionization energy?
a. Na
b. Ne
c. F
d. K
e. Rb
7. Which of the following has the greatest electron affinity (most negative value)?
a. Cl
b. K
c. He
d. Na
e. Rb
8. Which of the following species is not isolectronic with any of the others?
a. V3+
b. Ca2+
c. Ar
d. Cl-
e. S2-
9. In Bohr's model of the hydrogen atom, the radius of an orbit
a. is proportional to n2.
b. is smallest for the highest energy state.
c. increases when a photon of light is emitted from an excited atom.
d. can have any value that is larger than the ground-state radius.
e. none of the above
10. Which of the following atoms is not a one-electron system?
a. H
b. He+
c. Li2+
d. Be2+
e. O7+
11. Which of the following statements about periodic properties is incorrect?
a. Both electron affinity and ionization energy decrease down a group.
b. Atomic size increases to the right across a period.
c. Ionization energy increases to the right across a period.
d. Atomic size increases down a group.
e. Electron affinity increases to the right across a period.
, Bonding
1. Which one of the following is most likely to be an ionic compound?
a. HNF2
b. H2CO
c. N2H4
d. CaCl2
e. CH3Cl
2. In which of the following processes does the enthalpy change (ΔH) directly represent
the magnitude of the lattice energy of KCl(s)?
a. Cl2(g) + 2K(s) → 2KCl(s)
b. KCl(s) → K+(aq) + Cl-(aq)
c. KCl(s) → K+(g) + Cl-(g)
d. KCl(s) → K(s) + Cl-(g)
e. KCl(s) → K(s) + Cl(g)
3. Order the following by increasing bond strength: N≡N, N=N, N-N
a. N≡N, N=N, N-N
b. N≡N, N-N, N=N
c. N-N, N=N, N≡N
d. N=N, N-N, N≡N
e. N=N, N≡N, N-N
4. Which of the following compounds has the greatest bond polarity?
a. PH3
b. NH3
c. HF
d. H2S
e. CH4
5. Which of the following is not planar?
a. BCl3
b. ClF3
c. PCl3
d. XeF4
e. C2H4
