question 1 (1 point)
(02.06 lc)
the effective nuclear charge is the sum of all forces on electrons by the positively charged nucleus.
a true
b false

question 2 (1 point)
(02.06 lc)
the effective nuclear charge of atoms increases as you go from left to right in a row on the periodic table.
a true
b false

question 3 (1 point)
(02.06 lc)
electrons further from the nucleus are partially shielded from the pull of the nucleus.
a true
b false

question 4 (1 point)
(02.06 mc)
as you move from left to right across a period, what happens to the atomic radii?
a they increase, because of the higher number of occupied energy levels.
b they increase, because of the weaker attraction of electrons to the nucleus.
c they decrease, because of the stronger effective nuclear charge.
d they decrease, because of the increased atomic mass.

Question

question 1 (1 point)
(02.06 lc)
the effective nuclear charge is the sum of all forces on electrons by the positively charged nucleus.
 a true
 b false

question 2 (1 point)
(02.06 lc)
the effective nuclear charge of atoms increases as you go from left to right in a row on the periodic table.
 a true
 b false

question 3 (1 point)
(02.06 lc)
electrons further from the nucleus are partially shielded from the pull of the nucleus.
 a true
 b false

question 4 (1 point)
(02.06 mc)
as you move from left to right across a period, what happens to the atomic radii?
 a they increase, because of the higher number of occupied energy levels.
 b they increase, because of the weaker attraction of electrons to the nucleus.
 c they decrease, because of the stronger effective nuclear charge.
 d they decrease, because of the increased atomic mass.

Accepted Answer

# Brief Explanations:
- Question 1: Effective nuclear charge is the net positive charge experienced by valence electrons, not the sum of all forces on electrons by the nucleus. Inner - shell electrons shield outer - shell electrons from the full nuclear charge. So the statement is false.
- Question 2: As you move from left to right across a period in the periodic table, the number of protons in the nucleus increases while the number of electron shells remains the same. This leads to an increase in the effective nuclear charge. So the statement is true.
- Question 3: Inner - shell electrons shield outer - shell electrons from the full pull of the nucleus. Electrons further from the nucleus are indeed partially shielded. So the statement is true.
- Question 4: As you move from left to right across a period, the effective nuclear charge increases because the number of protons increases while the number of electron shells remains constant. This stronger effective nuclear charge pulls the electrons closer to the nucleus, causing the atomic radii to decrease.

# Answer:
Question 1: b. False
Question 2: a. True
Question 3: a. True
Question 4: d. They decrease, because of the stronger effective nuclear charge.

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