"Periodic Properties Worksheet With Answers Key"

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Periodic Properties Worksheet Key
1. State which atom is larger according to periodic trends.
a) Br, F
Br
b) Ca, Mg
Ca
c) C, Si
Si
d) He, Ar
Ar
2. Explain the difference in size for each of the pairs in Problem 1.
The outer electrons of the larger atom are in a subshell further away from the
nucleus than the outer electrons of the smaller atom.
3. State which atom is smaller according to periodic trends.
a) P, S
S
b) Be, Li
Be
c) I, Xe
Xe
d) As, Ge
As
4. Explain the difference in size for each of the pairs in Problem 3.
The outer electrons of both atoms are in the same subshell; however, the smaller
atom has a greater nuclear charge that attracts the electrons closer to the nucleus.
1
Periodic Properties Worksheet Key
1. State which atom is larger according to periodic trends.
a) Br, F
Br
b) Ca, Mg
Ca
c) C, Si
Si
d) He, Ar
Ar
2. Explain the difference in size for each of the pairs in Problem 1.
The outer electrons of the larger atom are in a subshell further away from the
nucleus than the outer electrons of the smaller atom.
3. State which atom is smaller according to periodic trends.
a) P, S
S
b) Be, Li
Be
c) I, Xe
Xe
d) As, Ge
As
4. Explain the difference in size for each of the pairs in Problem 3.
The outer electrons of both atoms are in the same subshell; however, the smaller
atom has a greater nuclear charge that attracts the electrons closer to the nucleus.
2
5. State which atom has a smaller first ionization energy according to periodic trends.
a) O, S
S
b) K, Na
K
c) Cd, Zn
Cd
d) Al, Ga
Ga
6. Explain the difference in ionization energy for each of the pairs in Problem 5.
The outer electrons of the atom with the smaller ionization are in a subshell further
away from the nucleus than the outer electrons of the atom with the larger ionization
energy.
7. State which atom has a larger ionization energy according to periodic trends.
a) Ba, Cs
Ba
b) Cl, S
Cl
c) Sc, Ti
Ti
d) Sb, Sn
Sb
8. Explain the difference in size for each of the pairs in Problem 8.
The outer electrons of both atoms are in the same subshell; however, the atom with
the larger ionization has a greater nuclear charge that attracts the electrons closer to
the nucleus making the electrons more difficult to remove.
9. Explain why the second ionization energy of rubidium is higher than the second ionization
energy of strontium.
The second electron removed from the rubidium atom is from the 4p subshell;
whereas, the second electron removed from strontium is from the 5s subshell. Since
the 4p subshell has a lower energy (a more negative energy) than the 5s subshell,
the second ionization energy of rubidium is much greater than the second ionization
energy of strontium.
3
10. State which atom has a larger electron affinity according to periodic trends.
a) As, P
P
b) Li, Na
Li
c) Ge, Si
Si
d) S, Se
S
11. Explain the difference in electron affinity for each of the pairs in Problem 10.
The outer subshell of the atom with the larger electron affinity is closer to the
nucleus; therefore, when an electron is added to the atom, the electron goes closer
to the nucleus and experiences more attraction. More attraction implies more
electron affinity.
12. State which atom has a smaller electron affinity according to periodic trends.
a) Co, Ni
Co
b) C, N
C
c) Br, Se
Se
d) S, Cl
S
13. Explain the difference in size for each of the pairs in Problem 12.
The outer subshell of both atoms are the same; however, the atom with the smaller
electron affinity has a smaller nuclear charge causing less attraction for the incoming
electron. Smaller attraction implies a smaller electron affinity.
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14. Which of the following is smaller?
2+
a) Mg, Mg
2+
Mg
Cations are smaller than the neutral
3+
b) Al, Al
atom because they have fewer
3+
Al
electrons. Removing electrons either
empties a larger subshell or reduces
+
c) Cs, Cs
the repulsion with a subshell.
+
Cs
15. Which of the following is larger?
2-
a) O, O
2-
O
Anions are larger than the neutral
atom because they have more
3-
b) P, P
electrons in the same subshell which
3-
P
causing increased repulsion. The
increased repulsion causes the
-
c) I, I
electrons to move further from each
-
I
other making the anion larger.
16. Arrange in order of increasing size
2+
3+
a) Fe, Fe
, Fe
3+
2+
Fe
, Fe
, Fe
Increasing number of electrons
causes increasing repulsion which
3+
4+
b) Ti, Ti
, Ti
causes increasing size.
4+
3+
Ti
, Ti
, Ti
-
2+
-
-
+
2+
3-
+
2-
+
2-
17. Arrange in order of increasing size: Br
, Ca
, Cl
, F
, Li
, Mg
, N
, Na
, O
, Rb
, S
First determine the number of electrons in each ion since each of these ions will
have the same number of electrons as a noble gas.
-
-
2+
-
-
-
-
-
+
-
2+
-
3-
-
Br
- 36 e
, Ca
- 18 e
, Cl
- 18 e
, F
- 10 e
, Li
- 2 e
, Mg
- 10 e
, N
- 10 e
,
+
-
2-
-
+
-
2-
-
Na
- 10 e
, O
- 10 e
, Rb
- 36 e
, S
- 18 e
Group the ions according to number of electrons. Size will increase according to
number of electrons (in the case of ions with noble gas electron configurations).
+
-
-
2+
3-
+
2-
-
2+
-
2-
-
-
+
-
Li
- 2 e
F
, Mg
, N
, Na
, O
- 10 e
Ca
, Cl
, S
- 18 e
Br
, Rb
- 36 e
Arrange ions in groups in order of decreasing nuclear charge which causes
decreased attraction and increasing size. Then put groups together.
+
2+
+
-
3-
2-
2-
-
2+
+
-
Li
, Mg
, Na
, F
, N
, O
, S
, Cl
, Ca
, Rb
, Br
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