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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-1
(pp. 123–125)
SKILL BUILDER
Use the K-W-L Chart to organize your ideas about the periodic table. In the K column, write what
you already know about the periodic table. In the W column, write questions that you have about
the periodic table. As you read, record the answers to your questions in the L column. You can add
to this chart or create a new one for future sections of Chapter 5.
K
What I Know
W
What I Want to Know
L
What I Learned
MORE SKILL BUILDING
1. Explain how Mendeleev developed the periodic table.
____________________________________________________________________________________
____________________________________________________________________________________
____________________________________________________________________________________
2. Explain the term periodicity. How does the term apply to chemistry?
____________________________________________________________________________________
____________________________________________________________________________________
____________________________________________________________________________________
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. Which statement is true?
a. The modern periodic table was developed at the First International Congress of Chemists.
b. Motion needs to vary uniformly in order to vary periodically.
c. In his periodic table, Mendeleev arranged the elements in order of their atomic numbers.
d. Mendeleev left “gaps” in his periodic table to account for missing elements.
2. Which was Stanislao Cannizzaro’s contribution to modern chemistry?
a. He developed a method for measuring the mass of an atom.
b. He created an accurate periodic table.
c. He discovered the elements scandium, gallium, and germanium.
d. He coined the term periodicity to account for chemical properties.
Modern Chemistry
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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-2
(pp. 125–127)
VOCABULARY
Define.
1. periodic law ________________________________________________________________________
__________________________________________________________________________________
2. periodic table _______________________________________________________________________
__________________________________________________________________________________
3. actinides __________________________________________________________________________
__________________________________________________________________________________
4. lanthanides ________________________________________________________________________
__________________________________________________________________________________
GRAPHIC ORGANIZER
On a separate sheet of paper, create a time line to show the dates and major events in the
development of the periodic table. Begin your time line with 1860, the First International Congress
of Chemists.
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. The noble gases are alike in that they all
a. are exceptions to the periodic law.
b. were included on Mendeleev’s periodic table.
c. are rather unreactive.
d. are radioactive at normal temperatures and pressures.
2. The noble gases, the lanthanides, and the actinides were added to the periodic table
a. by Mendeleev.
b. after Mendeleev’s time.
c. by Henry Moseley and Ernest Rutherford.
d. during the First International Congress of Chemists.
Modern Chemistry
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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-3
(pp. 128–131)
VOCABULARY
Complete each sentence.
1. Elements in the same row on the periodic table are said to be in the same _______________________.
2. Noble gases are very stable. Therefore, they are usually _______________________.
3. As stated by ___________________________________, elements with similar properties appear at
regular intervals when they are arranged in order of increasing atomic number.
4. The periodic table is arranged so that ____________________________________________________
_________________________________________________________________________________.
5. An element’s electron configuration can show you _________________________________________.
GRAPHIC ORGANIZER
Use the periodic table in your book to fill in the missing information in the chart.
Element
Symbol
Ca
Atomic Number
Atomic Mass
Electron Configuration
73
[Ar]3d64s2
Na
1s2
Zn
50
Au
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. The length of each period on the periodic table is best determined by
a. the research that was done by Ernest Rutherford.
b. the number of electrons that can occupy the sublevels being filled in that period.
c. the atomic masses of the elements in that row.
d. the number of elements in the columns, or groups.
2. All of the group 18 elements besides helium are
a. noble gases.
b. p-block elements.
c. d-block elements.
d. both a and b.
Modern Chemistry
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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-4
(pp. 132–133)
VOCABULARY
Select the term in Column B that matches the expression in Column A.
Column A
Column B
1. s block _____
a. period
2. lithium and sodium _____
b. hydrogen
3. radium and barium _____
c. alkaline-earth metals
4. 1s1 _____
d. lanthanide
5. row _____
e. alkali metals
6. thorium _____
f. reactive metals
7. cerium _____
g. actinide
SKILL BUILDER
Give the group, period, and block in which the elements with each of the following electron
configurations are located. Do not use the periodic table.
[Rn]7s2
[Ar]3d104s24p3
[Kr]4d105s25p5
[Ne]3s23p6
[Xe]6s1
[Ar]3d104s2
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. Which statement is true of alkali metals?
a. They are usually stored in water.
b. They are found in nature as free elements.
c. They are unable to combine with nonmetal elements.
d. They are soft enough to cut with a knife.
2. Alkaline-earth metals are
a. easier to melt than alkali metals.
b. found in nature as free elements.
c. denser and stronger than alkali metals.
d. radioactive at normal temperatures and pressures.
Modern Chemistry
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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-5
(pp. 134–138)
VOCABULARY
Define.
1. a. transition elements ________________________________________________________________
_______________________________________________________________________________
b. What do the transition elements have in common? _______________________________________
_______________________________________________________________________________
2. main group elements _________________________________________________________________
__________________________________________________________________________________
3. halogens __________________________________________________________________________
__________________________________________________________________________________
GRAPHIC ORGANIZER
On a separate sheet of paper, create a chart like the one below to summarize the properties of each
group of elements. List such properties as reactivity, ability to conduct electricity, and so on.
Group
Chemical Properties
halogens
metalloids
p-block
metals
actinides
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. The configuration (n – 1)d1ns2 represents elements in
a. group 3.
b. period 3.
c. group 4.
d. the halogen group.
2. The electron configuration ns2np6 represents
a. a halogen.
b. a metalloid.
c. a noble gas
d. an alkaline-earth metal.
Modern Chemistry
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Name ______________________________________ Date ____________ Class _______________________
Modern Chemistry • CHAPTER 5
HOMEWORK 5-6
(pp. 138–139)
VOCABULARY
Write true or false for each statement.
1. The halogens are less reactive than metalloids. ____________
2. The metalloids are in the p block of the periodic table. ____________
3. Mercury, tungsten, and vanadium are alkali metals. ____________
4. Transition metals are generally unable to conduct electricity. ____________
5. Elements in the d block do not always have the same outer electron configurations. ____________
6. All of the actinides have been found naturally on Earth. _____________
GRAPHIC ORGANIZER
Complete the chart by supplying the missing information.
Electron Configuration
Block
Period
Group/Type
Element
[Xe]4f 45d106s26p6
6
1/ alkali metal
5
11/transition metal
[Ar]3d54s1
[He]2s2
fluorine
STANDARDIZED TEST PREP
Circle the letter of the best answer.
1. Which is true of groups 3–12 on the periodic table?
a. They are alkali metals.
b. They are more reactive than alkaline-earth metals.
c. They exist as gases at normal temperatures.
d. They are able to conduct electricity.
2. Which is true of halogens?
a. They are the most reactive of the metals.
b. They are all liquids at room temperature.
c. They have seven electrons in their outer energy levels.
d. both a and c.
Modern Chemistry
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CHAPTER 5 REVIEW
The Periodic Law
MIXED REVIEW
SHORT ANSWER
Answer the following questions in the space provided.
1. Consider a neutral atom with 53 protons and 74 neutrons to answer the following questions.
a. What is its atomic number?
b. What is its mass in amus?
c. Is the element’s position in a modern periodic table determined by
its atomic number or by its atomic mass?
2. Consider an element whose outermost electron configuration is 3d104s24px.
a. To which period does the element belong?
b. If it is a halogen, what is the value of x?
c. The group number will equal (10 2 x). True or False?
3.
a. Metalloids are found in which block, s, p, d, or f ?
b. The hardest, densest metals are found in which block, s, p, d, or f ?
4.
a. Name the most chemically active halogen.
b. Write its electron configuration.
c. Write the configuration of the most-stable ion this element makes.
5. Referring only to the periodic table at the top of the Section 5-2 Review on page 35, answer the
following questions on periodic trends.
a. Which has the larger radius, Al or In?
b. Which has the larger radius, Se or Ca?
c. Which has a larger radius, Ca or Ca2?
d. Which has greater ionization energies as a class, metals or
nonmetals?
e. Which has the greater ionization energy, As or Cl?
f. An element with a large negative electron affinity is most likely
to form a positive ion, a negative ion, or a neutral atom?
MODERN CHEMISTRY
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CHAPTER 5 MIXED REVIEW
39
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MIXED REVIEW continued
g. In general, which has a stronger electron attraction, large atoms or
small atoms?
h. Which has greater electronegativity, O or Se?
i. In the covalent bond between Se and O, to which atom is the
electron pair more closely drawn?
j. How many valence electrons are there in a neutral atom of Se?
6.
Identify all of the ions below that do not have noble gas stability.
K S2 Ca I Al3 Zn2
7. Using only the periodic table in Section 5-2 Review on page 35, give the noble-gas notation of the
following:
a. Br
b. Br
c. the element in Group 13, Period 5
d. the lanthanide metal with the smallest atomic number
8. Use position in the periodic table and electron configurations to describe the chemical properties of
calcium and oxygen.
9. Copper’s electron configuration might be predicted to be 3d 94s2. But in fact, its configuration is
3d104s1. The two elements below copper in Group 11 behave similarly. (Confirm this in the
periodic table in Figure 5-6 on pages 130–131 of the text.)
a. Which configuration is apparently more stable?
b. Is the d subshell completed in the atoms of these three elements?
c. Every element in Period 4 has four levels of electrons established.
True or False?
40
CHAPTER 5 MIXED REVIEW
MODERN CHEMISTRY
HRW material copyrighted under notice appearing earlier in this work.