Download Unit 2.2 test review (AK)

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Unit 4 Test Review-Answer Key
1. Define electronegativity.
a. Electronegativity is a measure of the ability of an atom in a chemical compound to attract
electrons when they are chemically combined with atoms of another element.
2. Explain the group trend for electronegativity.
Group Trend – DECREASE as you move down
3. Explain the period trend for electronegativity.
Period Trend – INCREASE from left to right
4. Which of the following elements has the largest electronegativity: Fluorine (F) or Iodine (I)? Explain
your answer choice. Fluorine (F) has the largest electronegativity because the electrons in Fluorine have
the largest attraction to the nucleus.
5. Which of the following elements has the largest electronegativity: Sodium (Na) or Sulfur (S)? Explain
your answer choice. Sulfur (S) has the largest electronegativity because the electrons in Sulfur have the
largest attraction to the nucleus.
6. Define ionization energy.
Ionization Energy is the energy required to overcome the attraction of the protons and
remove one electron from a neutral atom of an element
7. Explain the group trend for ionization energy.
Group Trend – ionization energy DECREASES as you move down
8. Explain the period trend for ionization energy.
Period Trend – ionization energy INCREASES as you move left to right
9. Which of the following elements requires the LEAST amount of ionization energy: Strontium (Sr) or
Silver (Ag)? Explain your answer choice.
Strontium (Sr) because strontium electrons have less attraction for
the nucleus.
10. Which of the following elements requires the LEAST amount of ionization energy: Carbon (C) or Lead
(Pb)? Explain your answer choice.
Lead (Pb) because lead electrons further out from the pull of the nucleus are
easier to remove.
11. Potassium (K) has an ionization energy of 419 kJ/mol. Bromine (Br) has an ionization energy of 1140
kJ/mol. Which of the following is a possible explanation for the trend?
Bromine has strong attractive forces between the nucleus and the electrons. It takes more
energy to remove an electron from Bromine than Potassium.
12. Define atomic radius.
Atomic radius is ½ the distance between the nuclei of identical atoms that are bonded
together.
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13. Explain the group trend for atomic radius.
Group Trend – atomic size INCREASES as you move down
14. Explain the period trend for atomic radius.
Period Trend – size DECREASES as you move left to righ
15. Which of the following elements has the smallest atomic radius: Magnesium (Mg) or Barium (Ba)?
Explain your answer.
Magnesium (Mg) less energy levels, so smaller atomic radius.
16. Which of the following elements has the largest atomic radius: Gallium (Ga) or Bromine (Br)? Explain
your answer.
Bromine (Br) due to the pull of the electrons into the nucleus creating a smaller
atomic radius.
17. The atomic radius of Phosphorus (P) is 1.10 Å. The atomic radius of Antimony (Sb) is 1.41 Å.
Estimate the atomic radius of Arsenic (As).
In between 1.10 — 1.41
18.
19. Write the longhand electron configuration for Antimony (Sb).
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3
20. Which of the following pairs of atoms would have the SAME electron configuration?
a. Mg & Ar
b. Na+1 & Ne
c. K+1 & Br –1
d. Ca & S
21. Identify the element show in each of the following orbital diagrams.
a.
b.
c.
Carbon
Sulfur
Nickel
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22. Which orbital notation represents a p-block element in Period 2?
a.
b.
c.
23. Which element has the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s1? Potassium, K
24. Which element has the noble gas configuration of [Ar] 4s2 3d10 4p1? Gallium, Ga
25. Which element has the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4?
Selenium, Se
26. Which element has the noble gas configuration of [Ne] 3s1? Sodium, Na