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Target: 10 Questions in 10 minutes
An IB Chemistry data booklet is helpful |
1. Which property will show a general decrease across the Periodic Table from Li to F?
- A. atomic radius
- B. electron affinity
- C. ionization energy
- D. electronegativity
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2. Which set of ions is listed in order of increasing ionic radius?
- A. Cl- < S2- < Ca2+ < K+
- B. S2- < Cl- < K+ < Ca2+
- C. K+ < Ca2+ < S2- < Cl-
- D. Ca2+ < K+< Cl- < S2-
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3. Which equation represents the electron affinity of calcium?
- A. Ca(g) + e- → Ca-(g)
- B. Ca(s) + e- → Ca-(s)
- C. Ca(g) → Ca+(g) + e-
- D. Ca(s) → Ca+(s) + e-
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4. The ionic radius of Mg2+ is less than that of F-. Which statement helps to explain this fact?
- A. Magnesium is in period 3 but fluorine is in period 2
- B. Mg2+ has more electrons than F-
- C. Magnesium is a metal and fluorine is a non-metal
- D. Mg2+ has more protons that F-
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5. Which of the following properties will generally decrease with increasing atomic number for both Alkali Metals and Halogens?
| I. Electronegativity |
| II. Ionic radius |
| III. First electron affinity |
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- A. I and II only
- B. II and III only
- C. I and III only
- D. I, II and III
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6. Which of the following are listed in the order of more exothermic first electron affinity?
- A. Cl, Br
- B. F, Na
- C. F, Cl
- D. Li, Na
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7. Which statement is correct?
- A. The ionic radius of sodium is greater than its atomic radius
- B. The electron affinity of fluorine is greater than that of oxygen
- C. The outer electrons in chlorine are more shielded from the nucleus than those in bromine
- D. The ionization energy of potassium is greater than that of lithium
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8. Which reason best explains why the magnesium ion is MUCH smaller than the magnesium atom?
- A. The magnesium ion has one electron shell less than the atom
- B. Both entities have 12 protons in the nucleus
- C. The magnesium atom has two electrons more than the ion
- D. Magnesium is a metal so forms positive ions
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9. Which statement about electronegativity is NOT correct?
- A. Sodium has a greater electronegativity value than caesium
- B. Metals generally have lower electronegativity values than non-metals
- C. Fluorine has a greater electronegativity value than lithium
- D. Argon has the highest electronegativity value in period 3
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10.Which row correctly states and explains the trend in the ionization energy from Be to Ba?
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Trend |
Because … |
| A |
increases |
the valence electrons are further from the nucleus in Ba |
| B |
increases |
Ba has a greater nuclear charge |
| C |
decreases |
the valence electrons are further from the nucleus in Ba |
| D |
decreases |
Ba has a greater nuclear charge |
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