Periodic Table WS 8
Chemical Periodicity Review Sheet
H/Chemistry
A.
Completion
Use this completion exercise to check your knowledge of the terms and your understanding of the
concepts introduced in this chapter. Each blank can be completed with a term, short phrase, or number.
The periodic table organizes the elements into vertical _____________ and horizontal _____________
in order of increasing _____________. The table is constructed so that elements that have similar chemical
properties are in the same __________. The elements in Groups 1A through 7A (or 1,2, 13-17) are called the
_____________________ . The ______________ make up Group 18. The elements in Groups 2 and 13 are
interrupted in periods 4 through 7 by the ___________________________ and in periods 6 and 7 by the
___________________________.
The atoms of the noble gas elements have their outermost s and ___ sublevels filled. The outermost s
and p sublevels of the representative elements are _____________ _____________.
Atomic radii generally ___________ as you move from left to right in a period. Atomic radius
generally ___________ within a given group because there are more ___________________ occupied and an
increased _______________ effect, despite an increase in nuclear ______________.
The energy required to remove an electron from an atom is known as the _____________ . This
quantity generally ______________ as you move left to right across a period, and ________________ as you
move down a group. Its trend is the opposite to that of __________________________.
The ability of a bonded atom to attract electrons to itself is known as __________________, and this
quantity ____________________ as we move from left to right across a period, and _________________ as we
move down a group.
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Periodic Table WS 8
B.
True-False
Classify each of these statements as always true (AT); sometimes true (ST); or never true (NT).
_______ 1. In his periodic table, Mendeleev arranged the elements in ascending order of atomic number.
_______ 2. The representative elements are also called the main-block elements.
_______ 3. The outermost s or p sublevels are only partially filled for the representative elements.
_______ 4. Chlorine has the electron configuration 1s22s22p63s23p7.
_______ 5. The element in Group 14 (4A), period 3, is gallium.
_______ 6. The radius of an atom cannot be measured directly.
C.
Questions and Problems
Answer the following questions or solve the following problems in the space provided. Show your work.
1. Construct a graph showing the first ionization energies plotted against atomic number for the elements in
period 3. Use the information from the chart below. Use the horizontal axis for atomic number and the
vertical axis for ionization energy.
Element
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Ionization Energy (kJ/mol)
First
Second Third
1,312
2,371
5.247
520
7,297
11,810
900
1,757
14,840
800
2,430
3,659
1,086
2,352
4,619
1,402
2,857
4,577
1,314
3,391
5,301
1,681
3,375
6,045
2,080
3,963
6,276
495.8 4,565
6,912
737.6 1,450
7,732
577.4 1,816
2,744
786.2 1,577
3,229
1,012
1,896
2,910
999.6 2,260
3,380
1,255
2,297
3,850
1,520
2,665
3,947
418.8
3,069
4,600
589.5
1,146
4,941
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Periodic Table WS 8
11
12
13
14
15
16
17
2. List the outer electron configurations for the atoms in period 3, from left to right.
3. List the elements of Group 15 (5A). Tell whether each is a solid, liquid or gas, and whether it is a metal,
nonmetal or metalloid.
4. Circle which element in the following pairs has the greater ionization energy.
a. boron, carbon
b. magnesium, calcium
Explain your reasoning.
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c. sulfur, oxygen
d. sodium, silicon
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Periodic Table WS 8
5. Circle which element in the following pairs has the greater electronegativity.
a. calcium, gallium
b. lithium, oxygen
c. chlorine, sulfur
d. bromine, arsenic
Explain your reasoning.
6. Write electron dot diagrams for the following atoms:
a. silicon
b. rubidium
c. barium
adapted from Addison-Wesley Chemistry, 1987
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d. tin
e. iodine
f. arsenic