Atomic Radius Sample Questions
1.
Consider the following elements – Na, Ba, and S.
Which of these has the smallest atomic radius?
a. Na
d. Too little
b. Ba
information
c. S
2.
Let’s look at C, Ge, and Pb. Which of these has the
largest atomic radius?
a. C
d. Too little
b. Ge
information
c. Pb
3.
Consider the following elements – Be, Si, and F.
Which of these has the smallest atomic radius?
a. Be
d. Too little
b. Si
information
c. F
4.
Let’s look at Sr, As, and O. Which of these has the
largest atomic radius?
a. Sr
d. Too little
b. As
information
c. O
5.
Consider the following elements – Sn, Sb, and I.
Which of these would be the smallest atomic radius?
a. Sn
d. Too little
b. Sb
information
c. I
6.
Explain why the alkali metal in each row is larger
than the alkaline earth metal in each row.
Alkaline Earth have more protons to pull in the
electrons
7. If P and N have the same number of valence electrons,
why is N smaller than P?
P has more energy levels
Electronegativity Sample Questions
1.
Consider the following elements – Na, Ba, S, and Ar.
Which of these has the largest electronegativity?
a. Na
c. S
b. Ba
d. Ar
2.
Let’s look at C, Ge, and Pb. Which of these has the
smallest electronegativity?
a. C
d. Too little
b. Ge
information
c. Pb
3.
Consider the following elements – Be, Si, F, and Li.
Which of these has the largest electronegativity?
a. Be
c. F
b. Si
d. Li
4.
Let’s look at Sr, As, and O. Which of these has the
largest electronegativity?
a. Sr
d. Too little
b. As
information
c. O
5.
Consider the following elements – Sn, Sb, and I.
Which of these would be the smallest
electronegativity?
a. Sn
d. Too little
b. Sb
information
c. I
6. Why does oxygen draw the bonding electrons closer
when it bonds with carbon?
Oxygen’s nucleus has more protons, so it pulls the
electrons in more
7. If P and N have the same number of valence electrons,
why does N draw the bonding electrons closer when bonded
to P?
The valence electrons in P are further from the
nucleus in a higher energy levels
Ionization Energy Sample Questions
1.
Consider the following elements – Na, Ba, and S.
Which of these has the smallest ionization energy?
a. Na
d. Too little
b. Ba
information
c. S
2.
Let’s look at C, Ge, and Pb. Which of these has the
largest ionization energy?
a. C
d. Too little
b. Ge
information
c. Pb
3.
Consider the following elements – Be, Si, and F.
Which of these has the largest ionization energy?
a. Be
d. Too little
b. Si
information
c. F
4.
Let’s look at Sr, As, and O. Which of these has the
largest ionization energy?
a. Sr
d. Too little
b. As
information
c. O
5. Consider the following elements – Sn, Sb, and I.
Which of these would be the smallest ionization
energy?
a. Sn
d. Too little
b. Sb
information
c. I
6. Explain why it is easier to remove an electron from
the alkali metal in each row than the alkaline earth
metal.
Alkaline Earth have more protons to pull in the
electrons
7. If P and N have the same number of valence electrons,
why is N tougher to remove an electron from than P?
P has more energy levels, it’s easier to remove
electrons further away from the nucleus
The Big “Why”s
1.
Define atomic radius:
½ the distance between the nuclei of two touching
atoms
2.
How does the atomic radius change as you go from top to
bottom in a group? WHY?
Increases because the number of energy levels is
increasing
3.
How does the atomic radius change as you go from left to
right in a group? WHY?
Decreases because the increasing number of protons is
drawing the electrons in more
4.
How does the atomic radius change when a cation is
formed? WHY?
It becomes smaller because you are losing electrons
(typically a the whole outer energy level)
5.
How does the atomic radius change when a anion is formed?
WHY?
It becomes larger because electrons are being added
and the positive nucleus can’t hold them in as closely
6.
Define electronegativity:
A measure of the attraction for electrons
7.
How does the electronegativity change as you go from top to
bottom in a group? WHY?
Decreases with increasing energy levels
8.
How does the electronegativity change as you go from left to
right in a group? WHY?
Increases with increasing positive charge in the nucleus,
except Nobel Gases because they already have 8 valence
electrons.
9.
Define ionization energy:
The energy needed to remove an electron.
10. How does the ionization energy change as you go from top
to bottom in a group? WHY?
Decreases with increasing energy levels
11. How does the ionization energy change as you go from left
to right in a group? WHY?
Increases with increasing positive charge in the nucleus,