Q. What is the effect of increasing atomic number on electronegativity within a group?
-
A.
It increases
-
B.
It decreases
-
C.
It remains the same
-
D.
It fluctuates
Solution
Electronegativity decreases down a group because the increased distance between the nucleus and valence electrons reduces the nucleus's pull.
Correct Answer:
B
— It decreases
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Q. What is the primary factor that determines the atomic radius of an element?
-
A.
Number of protons
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B.
Number of neutrons
-
C.
Number of electron shells
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D.
Number of valence electrons
Solution
The atomic radius increases with the number of electron shells, as each additional shell is further from the nucleus.
Correct Answer:
C
— Number of electron shells
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Q. What is the primary reason for the increase in melting point as you move from sodium to aluminum in the periodic table?
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A.
Increase in atomic mass
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B.
Increase in metallic bonding strength
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C.
Decrease in ionization energy
-
D.
Increase in number of valence electrons
Solution
The increase in metallic bonding strength due to more delocalized electrons contributes to higher melting points.
Correct Answer:
B
— Increase in metallic bonding strength
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Q. What is the relationship between atomic radius and ionization energy?
-
A.
Directly proportional
-
B.
Inversely proportional
-
C.
No relationship
-
D.
Fluctuates
Solution
Atomic radius and ionization energy are inversely proportional; as atomic radius increases, ionization energy decreases.
Correct Answer:
B
— Inversely proportional
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Q. What is the relationship between atomic size and metallic character?
-
A.
Directly proportional
-
B.
Inversely proportional
-
C.
No relationship
-
D.
Fluctuates
Solution
Metallic character increases with atomic size, as larger atoms can lose electrons more easily.
Correct Answer:
A
— Directly proportional
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Q. What is the trend in atomic size as you move down a group in the periodic table?
-
A.
It increases
-
B.
It decreases
-
C.
It remains constant
-
D.
It fluctuates
Solution
Atomic size increases down a group due to the addition of electron shells.
Correct Answer:
A
— It increases
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Q. What is the trend in first ionization energy as you move down a group in the periodic table?
-
A.
It increases
-
B.
It decreases
-
C.
It remains constant
-
D.
It fluctuates
Solution
First ionization energy decreases down a group due to increased distance from the nucleus and increased electron shielding.
Correct Answer:
B
— It decreases
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Q. Which element has the smallest atomic radius?
-
A.
Helium
-
B.
Hydrogen
-
C.
Lithium
-
D.
Beryllium
Solution
Helium has the smallest atomic radius due to its high effective nuclear charge and minimal electron shielding.
Correct Answer:
A
— Helium
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Q. Which of the following elements would have the largest first ionization energy?
-
A.
Lithium
-
B.
Beryllium
-
C.
Boron
-
D.
Carbon
Solution
Carbon has a larger first ionization energy than lithium, beryllium, and boron due to its higher effective nuclear charge.
Correct Answer:
D
— Carbon
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Q. Which of the following elements would you expect to have the largest atomic radius?
-
A.
Lithium
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B.
Sodium
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C.
Potassium
-
D.
Rubidium
Solution
Rubidium has the largest atomic radius due to having the most electron shells among the given options.
Correct Answer:
D
— Rubidium
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Q. Which trend is observed in ionization energy across a period in the periodic table?
-
A.
It decreases
-
B.
It increases
-
C.
It remains constant
-
D.
It fluctuates
Solution
Ionization energy generally increases across a period due to increasing nuclear charge, which holds electrons more tightly.
Correct Answer:
B
— It increases
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Showing 1 to 11 of 11 (1 Pages)
