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Chapter 5, The Periodic Law


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
a.
Mendeleev.
c.
Bohr.
b.
Moseley.
d.
Ramsay.
 

2. 
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing
a.
atomic number.
c.
reactivity.
b.
density.
d.
atomic mass.
 

3. 
Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar
a.
properties.
c.
densities.
b.
atomic numbers.
d.
colors.
 

4. 
The most useful source of general information about the elements for anyone associated with chemistry is a
a.
calculator.
c.
periodic table.
b.
table of metric equivalents.
d.
table of isotopes.
 

5. 
What are the elements with atomic numbers from 58 to 71 in the periodic table called?
a.
the lanthanide elements
c.
the actinide elements
b.
the noble gases
d.
the alkali metals
 

6. 
In the modern periodic table, elements are ordered according to
a.
decreasing atomic mass.
c.
increasing atomic number.
b.
Mendeleev's original design.
d.
the date of their discovery.
 

7. 
The periodic law allows some properties of an element to be predicted based on its
a.
position in the periodic table.
c.
symbol.
b.
number of isotopes.
d.
color.
 

8. 
Elements in a group or column in the periodic table can be expected to have similar
a.
atomic masses.
c.
numbers of neutrons.
b.
atomic numbers.
d.
properties.
 

9. 
A horizontal row of blocks in the periodic table is called a(n)
a.
group.
c.
family.
b.
period.
d.
octet.
 

10. 
The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is
a.
4.
c.
11.
b.
10.
d.
18.
 

11. 
For groups 1, 2, and 18, the atomic number of the fourth element in the group is ____ more than the preceding element.
a.
3
c.
18
b.
4
d.
20
 

12. 
For elements in Groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern 8, 8, 18, ____, 32.
a.
18
c.
24
b.
20
d.
26
 
 
2007chapter5_files/i0140000.jpg
 

13. 
Refer to the figure above. To which group do fluorine and chlorine belong?
a.
alkaline-earth metals
c.
halogens
b.
transition elements
d.
actinides
 

14. 
The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period
a.
2.
c.
6.
b.
3.
d.
13.
 

15. 
Identify the sublevels in a period that contains 32 elements.
a.
s, f
c.
s, p, d
b.
s, p
d.
s, p, d, f
 

16. 
Because the first energy level contains only the 1s sublevel, the number of elements in this period is
a.
1.
c.
4.
b.
2.
d.
8.
 

17. 
Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel?
a.
8
c.
16
b.
10
d.
18
 

18. 
The period of an element can be determined from its
a.
reactivity.
c.
symbol.
b.
density.
d.
electron configuration.
 
 
2007chapter5_files/i0210000.jpg
 

19. 
In the elements shown in the figure above, the s sublevel of the highest occupied energy level
a.
always contains one electron.
b.
always contains two electrons.
c.
varies in the number of electrons it contains.
d.
is always empty.
 

20. 
Neutral atoms with an s2p6 electron configuration in the highest energy level are best classified as
a.
metalloids.
c.
nonmetals.
b.
metals.
d.
gases.
 

21. 
Elements in which the d-sublevel is being filled have the properties of
a.
metals.
c.
metalloids.
b.
nonmetals.
d.
gases.
 

22. 
The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to Group
a.
3.
c.
10.
b.
7.
d.
17.
 

23. 
Strontium's highest occupied energy level is 5s2. To what group does strontium belong?
a.
Group 2
c.
Group 6
b.
Group 4
d.
Group 8
 

24. 
If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is
a.
ns1.
c.
n – s.
b.
2n.
d.
np1.
 

25. 
Periods with occupied f sublevels
a.
have only Group 1 and 2 elements.
c.
have 32 groups.
b.
are not assigned group numbers.
d.
contain only Group 18 elements.
 

26. 
Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong?
a.
Group 2
c.
Group 5
b.
Group 3
d.
Group 12
 

27. 
In nature, the alkali metals occur as
a.
elements.
c.
complex ions.
b.
compounds.
d.
gases.
 

28. 
The most characteristic property of the noble gases is that they
a.
have low boiling points.
c.
are gases at ordinary temperatures.
b.
are radioactive.
d.
are largely unreactive.
 

29. 
Compared to the alkali metals, the alkaline-earth metals
a.
are less reactive.
c.
are less dense.
b.
have lower melting points.
d.
combine more readily with nonmetals.
 

30. 
Atomic size is determined by measuring the
a.
radius of an individual atom.
b.
distance between nuclei of adjacent atoms.
c.
diameter of an individual atom.
d.
volume of the electron cloud of adjacent atoms.
 

31. 
When an electron is acquired by a neutral atom, the energy change is called
a.
electron affinity.
c.
ionization energy.
b.
electronegativity.
d.
electron configuration.
 

32. 
In a row in the periodic table, as the atomic number increases, the atomic radius generally
a.
decreases.
c.
increases.
b.
remains constant.
d.
becomes unmeasurable.
 

33. 
In the alkaline-earth group, atoms with the smallest radii
a.
are the most reactive.
c.
are all gases.
b.
have the largest volume.
d.
have the highest ionization energies.
 

34. 
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
a.
sodium has four or five electrons.
b.
the atomic radius has increased.
c.
a d-electron has been removed.
d.
the noble gas configuration has been reached.
 

35. 
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a.
The nuclear charge increases.
c.
The number of energy levels increases.
b.
The number of neutrons increases.
d.
A new octet forms.
 

36. 
The electrons available to be lost, gained, or shared when atoms form molecules are called
a.
ions.
c.
d electrons.
b.
valence electrons.
d.
electron clouds.
 

37. 
The number of valence electrons in Group 1 elements is
a.
1.
c.
8.
b.
2.
d.
equal to the period number.
 

38. 
In Group 2 elements, the valence electrons are in sublevel
a.
d.
c.
s.
b.
p.
d.
f.
 

39. 
The number of valence electrons in Group 2 elements is
a.
2.
c.
18.
b.
8.
d.
equal to the period number.
 

40. 
Across a period, the atomic radii of d-block elements generally
a.
increase.
c.
remain constant.
b.
decrease.
d.
increase and then decrease.
 



 
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