Name: __________________________
Periodic Properties of the Elements
Chapter 7 Assessment
Test A-1
Show all work, including units, for all mathematical calculations.
Objective 1: Periodic Table & Effective Nuclear Charge (2 pts each)
1. What is meant by the term effective nuclear charge?
2. Which experiences a greater effective nuclear charge in a Be atom, the 1s electrons or the 2s
electrons. Explain.
3. Arrange the following atoms in order of increasing effective nuclear charge experienced by the
electrons in the n=3 electron shell: K, Mg, P, Rh, and Ti. Explain the basis for your order.
Score: _________________/6
Objective 2: Atomic and Ionic Radii (2 points each)
1.
Arrange the following atoms in order of increasing atomic radius:
a. F, P, S, As
b. Si, S, Ge, Se
c. Ca, Mg, Be
2. Which neutral atom is isoelectronic with each of the following ions:
a. N3_________________
b. Ba2+
_________________
c. Se2-
_________________
d. Bi3+
_________________
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3. For each of the following sets of atoms and ions, arrange the members in order of increasing
size:
a. Se2-, Te2-, Se,
b. Co3+, Fe2+, Fe3+
c. Ca, Ti4+, Sc3+
Score: ______________/20
Objective 3: Ionization Energies; Electron Affinities (2 points each)
1. Write equations that show the process that describe the first, second, and third ionization
energies of a boron atom.
a.
b.
c.
2. Based on their positions in the periodic table, predict which atom of the following pairs will have
the larger first ionization energy:
a. Cl, Ar
______________
b. Be, Ca
______________
c. K, Co
______________
d. S, Ge
______________
e. Sn, Te
______________
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3. Write the complete electron configurations for the following ions:
a.
Si2+
b. Te2-
c. Ni2+
d. S-2
4. Write an equation for the process that corresponds to the electron affinity of the Mg+1 ion:
Write the electron configurations of the species involved (2 answers required)
Score: __________________/28
Objective 4: Properties of Metals and Nonmetals
1. For each of the following pairs, which element will have the greater metallic character: (2 pts
each)
a. Li or Be
______________
b. Li or Na
______________
c. Sn or P
______________
d. Al or B
______________
2. Write balanced equations for the following reactions: (4 points each)
a. Potassium oxide with water
b. Diphosphorus trioxide with water
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c. Chromium (III) oxide with dilute hydrochloric acid
d. Selenium dioxide with aqueous potassium hydroxide
Score: ______________________/24
Objective 5: Group Trends in Metals and Nonmetals
1.
Write a balanced equation for the reaction that occurs in each of the following cases: (4 points
each)
a. Potassium metal burns in an atmosphere of chlorine gas
b. Strontium oxide is added to water
c. A fresh surface of lithium metal is exposed to oxygen gas
d. Sodium metal is reacted with molten sulfur
e. Barium metal is heated in an atmosphere of hydrogen gas
f.
Lithium reacts with sulfur
g. Fluorine reacts with magnesium metal
Score: _____________________/28
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Objective 6: Distributed Practice
1.
pH calculations
Calculate the pH of the following solutions: (2 pts each)
a. [H30+] = 1.3 x 10-4 M
______________
b. [H3O+] = 4.9 x 10-12 M
______________
c. [OH-] = 3.9 x 10-5 M
______________
d. [OH-] = 7.3 x 10 -11 M
______________
2. Stoichiometry: Limiting & Excess Reagents
Magnesium metal reacts with nitrogen gas forming an ionic compound of magnesium nitride.
a. Write this balanced equation (3 points).
b. Calculate the maximum yield of product formed when 5 grams of magnesium and 50
Liters of Nitrogen gas (at STP) (5 points).
c. Calculate the amount of excess reagent that remains unused in this reaction (5 points).
Score: ________________/21
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