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WorksheetsEffective Nuclear Charge
Total questions: 15
Worksheet time: 15mins
How does the effective nuclear charge relate to atomic radius?
An increase in effective nuclear charge decreases the atomic radius
An increase in effective nuclear charge increases the atomic radius
The effective nuclear charge has no effect on the atomic radius
The effective nuclear charge only affects isotopes
What trend in atomic radius occurs as you move from left to right across a period in the periodic table?
The atomic radius increases because the nuclear charge decreases
The atomic radius decreases because the nuclear charge increases
The atomic radius remains constant because the number of energy levels remains the same
The atomic radius increases because the number of neutrons increases
Why does Fluorine (F) have a smaller atomic radius than Lithium (Li)?
Because Fluorine has fewer protons than Lithium
Because Fluorine has more energy levels than Lithium
Because Fluorine has a higher nuclear charge, pulling electrons closer
Because Lithium is a gas at room temperature
Effective nuclear charge measures the attraction a valence electron feels to the nucleus of an atom. It is calculated by subtracting the (a) from the (b)
number of core electrons
total number of protons
number of valence electrons
total number of neutrons
Match the effective nuclear charge to the correct atom
Mg
+2
Al
+3
P
+5
Cl
+7
Ar
+8
Considering the metals: Na, Mg, and Al we note that (a) has the highest effective nuclear charge. During an experiment we note that Al is the least reactive of the three metals. We would predict (b) to be the most reactive.
Al
Na
Mg
Ionization energy increases moving from left to right accross the periodic table because
effective nuclear charge increases
the valence electrons are further from the nucleus
The two atoms with the same effective nuclear charge as Mg are
Ca
Be
Na
Al
What is the effective nuclear charge experienced by a valence electron in a chlorine atom?
A) +7
B) +17
C) +10
D) +1
Which of the following elements has the highest effective nuclear charge for its valence electrons?
A) Sodium (Na)
B) Magnesium (Mg)
C) Aluminum (Al)
D) Silicon (Si)
How does effective nuclear charge affect ionization energy?
A) Higher effective nuclear charge decreases ionization energy
B) Higher effective nuclear charge increases ionization energy
C) Effective nuclear charge has no effect on ionization energy
D) Effective nuclear charge only affects ionization energy in metals
In an experiment, which element would you expect to have a smaller atomic radius due to a higher effective nuclear charge?
A) Potassium (K)
B) Calcium (Ca)
C) Gallium (Ga)
D) Germanium (Ge)
What is the relationship between effective nuclear charge and electron shielding?
A) Effective nuclear charge increases with more electron shielding
B) Effective nuclear charge decreases with more electron shielding
C) Effective nuclear charge is unaffected by electron shielding
D) Effective nuclear charge is the same as electron shielding
Which of the following statements best describes the trend in effective nuclear charge across a period in the periodic table?
A) It decreases because the number of protons decreases
B) It increases because the number of protons increases
C) It remains constant because the number of energy levels remains the same
D) It fluctuates due to changes in electron configuration
Why does the effective nuclear charge increase as you move from left to right across a period?
A) Because the number of core electrons increases
B) Because the number of valence electrons increases
C) Because the number of protons increases while the shielding effect remains constant
D) Because the atomic mass increases
