Download WORKSHEET 36: ATOMIC PROPERTIES

Name ______________________________
AP Chemistry
Date_______________ Block __________
Periodic Review
1. Give full and abbreviated (noble gas core) electronic configurations for the following.
a) Br
FULL
______________________________
b) Cr
c) Fe
d) S2-
NOBLE GAS CORE
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FULL
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NOBLE GAS CORE
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FULL
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NOBLE GAS CORE
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FULL
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NOBLE GAS CORE
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2. For each of the following sets of orbitals, indicate which orbital is higher in energy.
a) 1s, 2s
_________
b) 2p, 3p
_________
c) 4s, 3d
_________
d) 3px, 3py, 3pz
_________
3. Indicate the block (s, p or d) in which each of the following elements found.
BLOCK
a) Sc
______
b) P
______
c) Fr
______
d) Ni
______
e) As
______
4. An atom has two electrons with principal quantum number (n) = 1, eight electrons with
principal quantum number (n) = 2 and seven electrons with principal quantum number (n) = 3.
From these data, supply the following values (if insufficient information is given, say so)
a) the mass number.
b) the atomic number.
_________
_________
c) the electron configuration.
___________________________
5. Identify the element from the electron configurations of atoms shown below.
a) [Ne] 3s2 3p2
_________
b) [Ar] 4s2 3d7
_________
c) [Xe] 6s2
_________
6. State which atom or ion is represented by the following sets of atomic numbers and electronic
configurations.
Atomic #
Electronic Configuration
a)
8
1s2 2s2 2p4
________
b)
11
1s2 2s2 2p6
________
c)
14
1s2 2s2 2p6 3s2 3p2
________
d)
22
1s2 2s2 2p6 3s2 3p6 3d2
________
8. Consider the element Scandium, atomic # 21.
a) If the electronic configuration of the element were constructed into which orbital (and into which
shell) would the final electron be placed? _________
10. Identify the element that is composed of atoms whose last electron;
a) enters and fills the 4s sub-shell
________
b) enters but does not fill the 4s sub-shell
________
c) is the first to enter the 2p sub-shell
________
d) is the next to the last to enter the 4p sub-shell
________
e) is the second to enter the 4d sub-shell
________
11. Write the full electronic configuration for argon.
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12. Identify two positive and two negative ions that are isoelectronic (same number of electrons)
with argon.
Two Positive ions
________
________
Two Negative ions
________
________
13. Using orbital diagrams complete the electronic configurations of the following elements.
4s
3d
4p
Element
   V
4s
3d
4p
Element
   Ar
4s
3d
4p
Element
   Zn
14. State the number of unpaired electrons in each of the electronic configurations in question 13.
# of unpaired electrons
V
________
Ar
________
Zn
________
15. Write three possible sets of quantum numbers for the highest energy electrons in the
aluminum atom.
n
l
ml
ms
Electron # 11
Electron # 12
Electron # 13
16. Calculate the wavelength of the energy released when an electron in a hydrogen atom falls
back to the first shell after being promoted to the fifth shell.
h = 6.626 x 10-34 J sec, c = 3.00 x 108 m sec-1
17. How would you expect the magnitude of the energy released in a similar process (5 th shell 
1st shell transition) in question 16 to vary for a He+ ion? Explain your answer.
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18. Which atomic theory is violated by the following sets of quantum numbers representing
beryllium’s outer shell electrons? Explain your answer.
n
2
2
l
0
0
ml
0
0
ms
+½
+½
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19. Identify the following atoms as either paramagnetic or diamagnetic.
Ga
____________________________
Cr
____________________________
Ni
____________________________
1. Complete the table. (5)
Element
Rb
Cs
Ga
At
Se
Predicted charge on its ion
2. Define Ionization Energy. (2)
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3. Using the metal magnesium as an example, write two separate equations to show the
first and second ionization energy of magnesium. (Remember state symbols are
important as they from part of the definition). (4)
First Ionization
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Second Ionization
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4. Which of the following elements (one from each pair) would you expect to have the
highest first ionization energy? Explain your answers. (4)
Ca and Be
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Na and Ar
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5. Consider the table of the first four ionization energies for element A shown below.
Ionization
Energy in
kJ/mol
1st
2nd
3rd
4th
578
1817
2745
11580
(i)
In which group does A appear on the periodic table? (1)
__________
(ii)
Predict the formula of the compound A forms with chlorine. (1)
__________
(iii)
What is the minimum number of electrons that A must have? (1)
__________
6. Are there any atoms for which the second ionization energy is greater than the first?
Explain your answer. (2)
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7. Define electron affinity. (2)
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8. Write an equation to summarize the process of second electron affinity of oxygen. (2)
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9. Consider the table of ionization energies for element X shown below.
Ionization
Energy in
kJ/mol
1st
2nd
3rd
4th
5th
6th
737
1450
7732
10540
13360
17995
(i)
In which group will X be found? (1) __________
(ii)
Explain your answer to 9(i). (2)
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(iii)
Predict the formula of X’s bromide. (1) ___________
10. Explain carefully why elements in the same group react in similar ways? (1)
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11. Explain carefully, the factor, when moving up and down groups I & II, that determines
the pattern of reactivity that is observed? (2)
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12. From the data below predict the boiling point of Radon. (1) _______________________
Noble Gas
Helium
Neon
Argon
Krypton
Xenon
Boiling Point/K
4.21
27.1
87.3
120
165
13. Arrange the following atoms into order of increasing first ionization energy. Sr, Cs, S, F
and As. (1)
LOWEST
HIGHEST
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14. What do you understand by the term, shielding? (2)
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