Chapter 6 Review
Name _________________________________
Fill in the following table.
Element
Symbol
Group
Period
Block
Electron Configuration
Family
Mercury
Hg
12
6
d
[Xe] 6s24f14 5d10
Transition elements
Boron
B
13
2
p
[He]2s22p1
Metalloid
Potassium
K
1
4
s
[Ar]4s1
Alkali Metal
Krypton
Kr
18
4
p
[Kr]
Noble Gas
Lead
Pb
14
6
p
[Xe]6s24f145d106p2
Other Metal
Uranium
U
N/A
N/A
f
[Rn] 7s2 5f3
Inner Transition
Metal
Chlorine
Cl
17
3
p
[Ne]3s23p5
Halogen
Lutium
Lu
N/A
N/A
f
[Xe] 6s2 4f14
Inner Transition
Metal
Radium
Ra
2
7
s
[Rn]7s2
Alkaline Earth Metal
Carbon
C
14
2
p
[He}2s22p2
Nonmetal
Determine the number of valence electrons for each for the following elements and draw
their Lewis Dot Structures.
# of Valence
Electrons
Lewis Dot Structure
2
Ca
Silicon
4
Si
Xenon
8
Xe
Oxygen
6
O
Element
Calcium
Characteristics of Metals and Nonmetals
Which of the following elements are likely to conduct electricity? (Circle all that apply)
Cl
Sr
Si
Li
Ar
Sn
C
Br
Which of the following are likely to be brittle solids or gases at room temperature?
(Circle all that apply)
Cl
Sr
Si
Li
Ar
Sn
C
Br
Periodic Trends
Which of the following elements would you expect to have the larger atomic radius,
carbon or nitrogen? Sodium or potassium? Explain.
Carbon. Electrostatic force increases as the number of protons in an atom increases (as
you go from left to right in the periodic table). As the electrostatic force increases,
electrons are pulled closed to the nucleus, thereby decreasing the atomic radius.
Potassium. Because the valence electron of potassium is farther away from the nucleus
than sodium’s valence electron, it experiences less electrostatic force and is not pulled
toward the nucleus to the same extent as sodium’s electron.
Which of the following would you expect to have the higher ionization energy, sodium or
chlorine? Barium or beryllium? Explain.
Chlorine. Ionization energy is the energy required to remove an electron from an atom.
Chlorine, being a non-metal has a high affinity for electrons. Sodium, being a metal,
freely looses electrons. It therefore takes less energy to remove an electron from a metal
as compared to a non-metal.
Beryllium. Beryllium’s valence electrons reside closer to the nucleus and those of
Barium. Because they are closer in proximity to the nucleus, beryllium’s valence
electrons experience a stronger electrostatic force than barium’s valence electrons. It
takes more energy to overcome the force that electrons close to the nucleus experience
that it does for electrons that are further away.
Which of the following would you expect to have the highest electronegativity, fluorine
or boron? Fluorine or chlorine? Explain.
Fluorine. Electronegativity is a measure of atom’s ability to attract electrons. The atom
that needs to gain fewer electrons to achieve stability will have a greater ability to attract
electrons.
Fluorine. Fluorine’s valence electrons reside closer to the nucleus than those of chlorine.
The fluorine nucleus can more easily attract electrons to its outer shell because the
electrostatic force the electrons would experience at that distance would be greater than
the force that electrons being added to chlorine’s outer shell would experience.