Question

question 47 (1 point)
which of the following statements correctly compares the relative size of an ion to its neutral atom?
a the radius of an anion is identical to the radius of its neutral atom.
b the radius of an anion is greater than the radius of its neutral atom.
c the radius of a cation is greater than the radius of its neutral atom.
d the radius of a cation is identical to the radius of its neutral atom.

question 48 (1 point)
which of the following factors contributes to the increase in ionization energy from left to right across a period?
a an increase in the size of the nucleus
b an increase in the shielding effect
c fewer electrons in the highest occupied energy level
d an increase in the number of protons

question 49 (1 point)
as you move from left to right across the second period of the periodic table
a ionization energy increases.
b atomic radii increase.
c atomic mass decreases.
d electronegativity decreases.

Explanation:

Question 47

• Anions are formed by adding electrons. The added electrons increase electron - electron repulsion, causing the electron cloud to expand. So, the radius of an anion is greater than that of its neutral atom.
• Cations are formed by losing electrons. Losing electrons reduces electron - electron repulsion, and the remaining electrons are pulled closer to the nucleus. So, the radius of a cation is smaller than that of its neutral atom.

• As we move from left to right across a period, the number of protons in the nucleus increases. This increases the nuclear charge.
• The shielding effect (due to inner - shell electrons) remains relatively constant across a period (since the number of inner - shell electrons does not change significantly across a period).
• The increase in nuclear charge (due to more protons) attracts the electrons in the highest occupied energy level more strongly, making it more difficult to remove an electron (higher ionization energy).

• As we move from left to right across a period (e.g., the second period), the number of protons in the nucleus increases.
• Ionization energy: The increase in nuclear charge (due to more protons) attracts the electrons more strongly. So, ionization energy increases from left to right across a period.
• Atomic radii: The increased nuclear charge pulls the electrons closer to the nucleus. So, atomic radii decrease from left to right across a period.
• Atomic mass: Generally, atomic mass increases from left to right across a period as we move to elements with more protons, neutrons, etc.
• Electronegativity: Electronegativity increases from left to right across a period (except for noble gases) as the atom has a greater ability to attract electrons in a chemical bond due to the increased nuclear charge.

Answer:

B. The radius of an anion is greater than the radius of its neutral atom.

Question 48