CHE 100
Worksheet # 5
Due __________
1.
The accepted value for the boiling point of diethylether is 35oC. What is the percent
error for a measured value of 37oC as the boiling point of diethylether?
a) -4.3%
b) -8.6%
c) 5.7%
d) 4.3%
2.
37 -35 x 100 = 2 x 100 = 5.7% (Note – should be 1 sf – 6%)
35
35
increasing atomic number
decreasing atomic number
increasing atomic mass
decreasing atomic mass
_____b________
Which of the following is a quantized property of an electron.
a)
b)
c)
d)
5.
_______a_______
In which of the following sets of elements are all members of the set in the same
group in the periodic table?
a) 9F, 10Ne, and 11Na
b) 9F, 17Cl, and 35Br
c) 20Ca, 26Fe, and 34Se
d) 7N, 15P, and 16S
4.
_______c_______
The periodic law states that when elements are arranged in order of
_______ their properties repeat themselves at regular intervals.
a)
b)
c)
d)
3.
Name _________Key_____________________
energy
mass
charge
charge to mass ratio
______a________
What is the maximum number of electrons in the n=3 shell?
a)
b)
c)
d)
2
16
8
18
______d________
Pg. 2
6.
Which of the following subshells is highest in energy?
a) 6s
b) 3d
c) 2p
d) 5d
7.
(look at Aufbau diagram)
______d________
Which of the following subshell notation for electron occupancy is an
impossibility?
a) 4d9
b) 6s2
c) 5f13
d) 2d1
8.
_______d_______
Which statement about orbitals is INCORRECT?
a) Different subshells have different shapes.
b) Two electrons can occupy each lobe of a p orbital.
c) At a given time, an electron can only be at one point in an orbital
d) An orbital is a region of space where an electron is most likely to be found
_______b_______
9.
The electron configuration 1s22s22p63s23p64s23d104p65s24d1 is that for the element
(total 39 electrons)
a)
b)
c)
d)
e)
10.
31Ga
33AS
Br
36Kr
39Y
35
_______e_______
Which one of the following elements would be in the same group of the periodic
table as the element whose configuration is 1s22s22p63s23p4?
a) 15P
b) 18Ar
c) 34Se
d) 9F
______c________
Pg. 3
11.
Which of the following pairings is incorrect?
a)
b)
c)
d)
e)
12.
47Ag
2
4
6
8
3
_______a_______
Which of the following elements would be expected to have the greatest metallic
character?
a) 12Mg
b) 31Ga
c) 3Li
d) 38Sr
e) 88Ra
14.
_______e_______
How many unpaired electrons are in a Zr atom?
a)
b)
c)
d)
e)
13.
– d area of periodic table
– d area of periodic table
52Te – p area of periodic table
87Fr – s area of periodic table
92U – d area of periodic table
26Fe
________e_______
Which of the following elements has the smallest atomic radius?
a)
b)
c)
d)
e)
11Na
13Al
15P
17Cl
12Mg
_______d_______
Pg. 4
15.
In each horizontal line circle the correct symbol or formula which has
1) Electron configuration ends
in 6p3
a) 33As
b) 51Sb c)73Ta d) 83Bi
2) 1s22s22p63s23p64s23d104p65s2
a) 24Cr
b) 34Se c) 38Sr
3) 7s subshell begins filling
a) 37Rb
b) 55Cs
c)56Ba d) 87Fr
4) 3rd shell contains 7 electrons
a) 17Cl
b) 21Sc
c)
5) 3rd shell becomes completely
filled
a) Mg
b) He
c) Be
d) Zn
6) Number of electrons in the
4d subshell of 45Rh
a) 0
b) 5
c) 7
d) 10
7) Contains a total of twentyone “p” electrons
a) 36Kr
b)
c) 54Xe d)
8) Contains an equal number of
“d” and “p” electrons
a)
b) 30Zn c) 36Kr d) 50Sn
9) All orbitals in the outermost
subshell are half filled
a) 9F
16S
b)
51Sb
34Se
c)
39Y
33As
d) 52Te
d)
d)
47Ag
83Bi
56Ba
Pg. 5
Electron Configurations and Orbital diagrams
1. K
1s22s22p63s23p64s1
Z = 19
[Ar] 4s1
or


         _ or
1s
2s
2p
3s
3p
4s
[Ar] _
4s
________________________________________________________________________
2. V
1s22s22p63s23p64s23d 3
Z = 23
or
[Ar] 4s23d 3
          _
1s
2s
2p
3s
3p
4s
_ _
3d
__ __
or
[Ar]  _ _ _ __ __
4s
3d
________________________________________________________________________
3.
Co
Z = 27
1s22s22p63s23p64s23d
7
or
[Ar] 4s23d 7
         _  _ _ _
1s
2s
2p
3s
3p
4s
3d
or
[Ar]  
4s

_
3d
_ _
________________________________________________________________________
4.
Zr
Z = 40
1s22s22p63s23p64s23d104p65s24d2
[Kr]  _
5s
_
__
4d
or [Kr] 5s24d 2
__ __
________________________________________________________________________
Pg. 6
5.
Br
Z = 35
2
2
6
2
6
2
10
6
2
10
5
2
10
or [Ar] 4s 3d 4p
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p
5
[Ar]       _
4s
3d
4p
________________________________________________________________________
6.
Zn
1s22s22p63s23p64s23d 10
Z = 30
[Ar] 4s23d 10
or
[Ar]     
4s
3d
_____________________________________________________________
7.
Mo
[Kr] 5s24d 4
Z = 42
[Kr]  _
5s
_
_ _ __
4d
Note: Shown above is the correctly predicted electron configuration and orbital diagram for Mo,
however the observed behavior of Mo follows an anomalous filling pattern. Additional stability is gained
by “borrowing” an electron from the 5s to half-fill the 4d subshell, and the observed electron
configuration for Mo is [Kr] 5s14d 5.
_____________________________________________________________
8.
Ag
[Kr] 5s24d 9
Z = 47
[Kr]      _
5s
4d
Note: Shown above is the correctly predicted electron configuration and orbital diagram for Ag,
however the observed behavior of Ag follows an anomalous filling pattern. Additional stability is gained
by “borrowing” an electron from the 5s to fill the 4d subshell, and the observed electron configuration
for Ag is [Kr] 5s14d 10.
________________________________________________________________________
9.
Te
Z = 52
1s22s22p63s23p64s23d104p65s24d105p4 or
[Kr] 5s24d105p4
[Kr]       _ _
5s
4d
5p
________________________________________________________________________
10. Rb
Z = 37
1s22s22p63s23p64s23d104p65s1
or
[Kr] 5s1
[Kr] _
5s
_____________________________________________________________