Question 1 of 10
Ionization energy increases down a group because the number of protons increases and it's
more difficult to lose electrons because they are being pulled closer.
False
True
Question 2 of 10
Which of the following has the largest ionization energy?
N
Si
Al
P
Question 3 of 10
Which of the following elements has the lowest ionization energy?
Cesium (Cs)
Sodium (Na)
Lithium (Li)
Rubidium (Rb)
Question 4 of 10
Order the elements in decreasing ionization energy. Na, S, Al, F, K, O
Al, O, K, F, S, Na
F, O, S, Al, Na, K
Na, S, F, K, O, Al
K, Na, Al, S, O, F
Question 5 of 10
What is the definition of ionization energy?
The energy required to add an electron
The energy required to remove an electron
The amount of energy to attract or bond an electron
None of the above are correct
Question 6 of 10
Which of the following best explains why ionization energy decreases down a group?
None of the above.
Ionization energy decreases because electrons are closer and require more energy to remove.
Ionization energy increases, because electrons are closer to the nucleus.
Ionization energy decreases because electrons are further away and require less energy to
remove.
Question 7 of 10
Which has the set of elements has the element with the highest ionization energy?
N, O, C, H, S
Mg, Ca, Be, B, N
Al, Si, Ge, F, N, K
N, Xe, Rn, Fr
Question 8 of 10
Mg, Be, Ca, Sr are all in the same __________.
Group
Period
Question 9 of 10
True or false. There are 18 periods and 7 groups.
False
True
Question 10 of 10
Which of the following elements is in period 6 and group 4?
C
Hf
Ge
*
Zr
Question 11 of 11
How does atomic radius affect ionization energy?
a)Atomic radius does not affect ionization energy.
b)A smaller atomic radius means a higher ionization energy.
c)A larger atomic radius means a higher ionization energy.
d)A smaller atomic radius means a lower ionization energy.
Question 12 of 12
What factor makes removing a valence electron easier than a core electron?
a)Nuclear Pull
b)ZEFF
c)Electron repulsion
d)Electron shielding