Effective nuclear charge and Slater rules - One Line Questions
1.
Which of the following is the correct order of shielding effectiveness for electrons in different shells towards an outer electron? —
(n-1) > (n-2) > same n
2.
According to Slater's rules, what is the shielding value (S) for an electron in the 1s orbital of a hydrogen atom? —
0
3.
In Slater's rules, for an electron in a d or f orbital, what is the shielding contribution from other electrons in the same (n) shell? —
0.85
4.
Consider a 3d electron in Scandium (Sc), Z=21. Configuration: [Ar] 3d^1 4s^2. What is the shielding contribution from the 4s electrons to the 3d electron? —
0.30
5.
Calculate the shielding constant (S) for a 1s electron in Neon (Ne) using Slater's rules. —
0.70
6.
In Slater's rules, electrons in the same principal quantum shell (n) but different subshells (l) contribute how much to the shielding constant (S) for each other? —
0.35
7.
For an electron in the (n) shell, what is the shielding contribution from electrons in the (n-1) shell according to Slater's rules? —
0.85
8.
What is the shielding contribution from electrons in shells with principal quantum number (n-2) or lower, according to Slater's rules? —
1.00
9.
Calculate the shielding constant (S) for a 3s electron in Sodium (Na) using Slater's rules. Sodium configuration: [Ne] 3s^1. —
0.85
10.
In Slater's rules, what is the shielding contribution of a 1s electron for another 1s electron in the same atom? —
0.35
11.
What is the approximate shielding constant (S) for a 4s electron in Potassium (K) [Ar] 4s^1 using Slater's rules? —
0.85
12.
Calculate the effective nuclear charge (Zeff) for a 4s electron in Potassium (K). —
1.00
13.
Calculate the effective nuclear charge (Zeff) for a 3s electron in Sodium (Na). —
1.20
14.
Calculate the shielding constant (S) for a 2p electron in Oxygen (O) [He] 2s^2 2p^4 using Slater's rules. —
1.70
15.
What is the atomic number (Z) of Sodium (Na)? —
11
16.
Calculate the shielding constant (S) for a 3d electron in Scandium (Sc) using Slater's rules. Other electrons: [Ar] (18 electrons). —
10.15
17.
Calculate the shielding constant (S) for a 3s electron in Argon (Ar) [Ne] 3s^2 3p^6 using Slater's rules. —
11.70
18.
Calculate the shielding constant (S) for a 3p electron in Chlorine (Cl) using Slater's rules. Chlorine configuration: [Ne] 3s^2 3p^5. —
10.75
19.
Calculate the effective nuclear charge (Zeff) for a 3d electron in Scandium (Sc). —
10.85
20.
What is the atomic number (Z) of Chlorine (Cl)? —
17
21.
What is the atomic number (Z) of Argon (Ar)? —
18
22.
Calculate the shielding constant (S) for a 3d electron in Iron (Fe) [Ar] 3d^6 4s^2 using Slater's rules. Consider the 3d electron. —
22.05
23.
Which of the following electrons experiences the highest effective nuclear charge? —
1s electron in Helium
24.
Consider an electron in the 3p orbital of Phosphorus (Z=15). Which electrons contribute significantly to shielding it according to Slater's rules? —
3s electrons and electrons in shells n-1 and lower
25.
Which electron group is considered when calculating the shielding constant (S) for a 3d electron in Slater's rules? —
3s, 3p
26.
What is the atomic number (Z) of Iron (Fe)? —
26
27.
Calculate the effective nuclear charge (Zeff) for a 3d electron in Iron (Fe). —
3.95
28.
Calculate the effective nuclear charge (Zeff) for a 3p electron in Chlorine (Cl). —
6.25
29.
Calculate the effective nuclear charge (Zeff) for a 2p electron in Oxygen (O). —
6.10
30.
What is the atomic number (Z) of Oxygen (O)? —
8
31.
Calculate the effective nuclear charge (Zeff) for a 3s electron in Argon (Ar). —
6.30
32.
What is the atomic number (Z) of Neon (Ne)? —
10
33.
Calculate the effective nuclear charge (Zeff) for a 1s electron in Neon (Ne). —
9.30
34.
The concept of effective nuclear charge is crucial for understanding trends in: —
Atomic size and ionization energy
35.
How does the effective nuclear charge generally change across a period in the periodic table? —
Increases
36.
How does the effective nuclear charge generally change down a group in the periodic table? —
Decreases
37.
What is the primary reason for the decrease in effective nuclear charge down a group? —
Increase in the number of electron shells, leading to greater shielding.
38.
What is the primary reason for the increase in effective nuclear charge across a period? —
Addition of protons to the nucleus with minimal increase in shielding.
39.
How does the effective nuclear charge experienced by a 3d electron change from Scandium (Sc) to Iron (Fe)? —
It increases slightly.
40.
What is the primary effect of the poor shielding by d and f electrons on the effective nuclear charge? —
It leads to a slight increase in Zeff for outer electrons.
41.
Which of the following elements has the highest effective nuclear charge for its valence electrons? —
Carbon (C)
42.
Why is the shielding contribution from electrons in the same shell (n) less effective than from electrons in inner shells (n-1)? —
Outer shell electrons are further from the nucleus and do not penetrate as effectively.
43.
The shielding effect is also known as: —
Screening effect
44.
Which of the following is NOT a factor considered in Slater's rules for calculating shielding? —
Principal quantum number (n) of the electron.
45.
What does Slater's rules aim to calculate? —
The shielding constant (S) for an electron.
46.
Which factor primarily reduces the effective nuclear charge experienced by an electron? —
Repulsion from other electrons (shielding effect).
47.
What is the definition of effective nuclear charge (Zeff)? —
The actual nuclear charge experienced by an electron in a multi-electron atom.
48.
Slater's rules provide an approximation. What is a known limitation of these rules? —
They overestimate shielding for d and f electrons.
49.
How is the effective nuclear charge (Zeff) calculated using the shielding constant (S) and the atomic number (Z)? —
Zeff = Z - S
50.
Which statement best describes the trend of effective nuclear charge (Zeff) in transition metals? —
Zeff increases slightly with each added d electron due to poor shielding by d electrons.