Download Unit 5

Ions and the Octet Rule
1)
Ca
2)
Ca+2
3)
S-2
4)
S
5)
I
6)
I-1
7)
Se-2
8)
Se
9)
Al+3
10)
Al
11*)
Xe
12*)
Si
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13)
B
14)
B?
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P?
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P
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3)
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?
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?
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1)
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??
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?-?
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?+?
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?
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?-?
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?+3
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29)
Identify the following elements based on their electron configuration or orbital notation and their overall charge.
a) 1s2 2s2 2p3 (neutral)
_____
b) 1s2 2s2 2p6 3s2 3p6 (+2)
_____
c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
30)
31)
(-3)
_____
d) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O (neutral)
1s
2s 2p
3s 3p
3d
4s 4p
4d
4f
5s
_____
e) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O OOO
1s
2s 2p
3s 3p
3d
4s 4p
4d
4f
5s 5p
_____
(+1)
Write the electron configuration for each of the following ions and tell which noble gas each is isoelectronic with.
a) Al+3
_____
b) Te-2
_____
c) Sr+2
_____
d) Ga+3
_____
e) I-1
_____
Write the electron configuration for each of the following ions.
a) F-1
b) Na+1
c) Be+2
d) P-3
e) K+1
f) S-2
g) Ba+2
32)
Write the electron configuration for each of the following ions. Tell which noble gas each ion is isoelectronic with.
a) Se-2
_____
b) O-2
_____
c) Sb-3
_____
d) Mg+2
_____
e) Pb+4
_____
33)
Write the electron configuration for O and O-2. How many electrons are in each valence energy level?
34)
Identify the following elements given their electron configuration and their charge.
a) 1s2 2s2 2p6 (-2)
_____
b) 1s2 2s2 2p6 (+3)
_____
c) 1s2 2s2 2p6 3s2 3p6 (-1)
_____
d) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
(+2)
e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 6s2 6p6
_____
(+1)
_____
35)
Write the electron configuration for Br and its ion. How many electrons are in each of the valence energy levels?
36)
Write the electron configuration for Ca and its ion. How many electrons are in each of the valence energy levels?
37)
Write the electron configuration for Cl and its ion. How many electrons are in each of the valence energy levels?
38)
Write the electron configuration for Na and its ion. How many electrons are in each of the valence energy levels?
39)
Write the electron configuration for Sb and its ion. How many electrons are in each of the valence energy levels?
40)
Identify the following elements given their electron configuration and their charge.
a) 1s2 2s2 2p6 (-4)
_____
b) 1s2 2s2 2p6 (+1)
_____
c) 1s2 2s2 2p6 3s2 3p6 (-3)
_____
d) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
(neutral)
_____
e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 6s2 6p6
41)
(-1)
_____
Identify the following elements based on their electron configuration or orbital notation and their overall charge:
a) 1s2 2s2 2p6 3s2 3p5 (neutral)
_____
b) 1s2 2s2 2p6 3s2 3p6 (-3)
_____
c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
d) O | O OOO
1s
2s 2p
(+1)
_____
(+3)
_____
e) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O
1s 2s 2p
3s 3p
3d
4s 4p
4d
4f
5s
42)
_____
Select the member of each pair that is larger.
a) Ca or P
43)
(neutral)
b) Cl or Cl-
Arrange in order of increasing radius:
c) Na or Na+
Ca+2, Cl-, K+, S-2
d) I- or Te
_____ : _____ : _____ : _____
Periodic Trends
44)
On the Periodic Table, a horizontal row is called a __________ and a vertical column is called a __________.
45)
Which would behave more similarly: elements in any one group or elements in any one period.
__________________________________________________________________________________________
46)
What similarity is there among the outermost energy levels of elements within the same group?
__________________________________________________________________________________________
47)
Arrange in order of increasing ionization potential:
Ca, Cl, Rb, S, Sr
___ : ___ : ___ : ___ : ___
48)
Arrange in order of increasing atomic radius:
As, I, P, Sb
___ : ___ : ___ : ___
49)
AR _____ as you move from the top to the bottom of a group on the PTE.
50)
Explain why atomic radius changes as it does as we move from left to right in the Periodic Table.
decreases
increases
__________________________________________________________________________________________
51)
Arrange in order of increasing atomic radius:
F, H, In, S, Hg
___ : ___ : ___ : ___ : ___
52)
Where on the PTE do we find elements with the lowest ionization potential?
_________________________
53)
Where on the PTE do we find the most un-reactive elements?
_________________________
54)
_________________________ is the amount of energy needed to pull an electron away from an isolated atom.
55)
Elements sodium and chlorine are both in period 3. Why is the ionization potential of chlorine so much greater?
__________________________________________________________________________________________
56)
Arrange in order of increasing ionization potential:
As, I, P, Sb
___ : ___ : ___ : ___
57)
Why it is more difficult to remove an electron from an atom that is located at the top of a group than the bottom.
__________________________________________________________________________________________
58)
Arrange in order of increasing atomic radius:
Ca, Cl, Rb, S, Sr
___ : ___ : ___ : ___ : ___
59)
Arrange in order of increasing ionization potential:
Br, Cs, F, Ge, Se
___ : ___ : ___ : ___ : ___
60)
A positive ion is an atom that has _____.
a) gained an electron
61)
b) gained a proton
c) lost an electron
d) lost a proton
b) gained 2 protons
c) lost 2 electrons
d) lost 2 protons
Metallic elements tend to _____ electrons and form _____ ions.
a) gain
64)
d) lost a proton
A Mg+2 ion is a Mg atom that has _____.
a) gained 2 electrons
63)
c) lost an electron
A Cl- ion is a Cl atom that has _____.
a) gained an electron
62)
b) gained a proton
b) lose
c) positive
Based on their actual electronegativity the following are arranged as follows:
Based on the electronegativity trend the following are arranged as follows:
Why the difference?
d)
negative
Zn : Fe : Cu : Se
Fe : Cu : Zn : Se
__________________________________________________________________________________________
65)
Why should fluorine have the highest electronegativity?
__________________________________________________________________________________________
66)
The ionization potential _____ as one moves down a group of elements.
decreases
increases
67)
The ionization potential _____ as one moves from left to right across a period.
decreases
increases
68)
The atomic radius _____ as one moves from left to right across a period.
decreases
increases
69)
Arrange in order of increasing electronegativity:
___ : ___ : ___ : ___ : ___
70)
Within the same period, cations are larger than anions.
True
71)
Arrange in order of increasing atomic radius:
___ : ___ : ___ : ___ : ___ : ___
72)
Which of the transition metals should have the smallest ionization energy?
_____
73)
Which of the noble gases should be the most likely to react with another atom?
_____
74)
Which of the noble gases should be the least likely to react with another atom?
_____
75)
Which family should have the highest electronegativity?
a) alkali metals
76)
F, O, S, P, Na
K, Ca, Se, Br, Ba, I
b) alkaline earth metals
c) halogens
False
d) noble gases
Explain above answer:
_______________________________________________________________________________
Other Periodic Trends
77)
Explain the size difference between a sodium ion and chlorine ion.
78)
Explain the size difference between a fluorine atom, neon atom and a sodium ion.
79)
Explain the size difference between an atom and its ion.
80)
Explain the size difference between a series of isoelectronic atoms / ions.
81)
Research the pattern for density.
82)
Research the pattern for melting and boiling point.