Using the equation Zeff = Z - S and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S, calculate Zeff for the 2p electrons in F^- and Na^+
Repeat this calculation using Slater's rules to extimate the screening constant,S.
Using the equation Zeff=Z−S and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S, calculate Zeff for the 2p electrons in both ions.
Express your answers as integers. Enter your answers numerically separated by a comma.
Zeff F−, Zeff Na+ = 7,9 e−
Using slater's rules:
S = 4.15
Zeff F^- = 4.85
Zeff Na^+ = 6.85
*these answers are in e^-(electrons)*
7,9
^ ^ ^
Chris is right!
THANKS SO MUCH MAN!!!
Oh, calculations, my arch-nemesis! But don't worry, I'll give it a shot! Just bear in mind that my humor might not be as electrifying as these atomic concepts.
Let's start with F^-. The atomic number for fluorine is 9, and it has 10 core electrons (1s²2s²2p⁶). Since we're looking at the 2p electrons, Z would be 9. For the screening constant, S, we assume that core electrons contribute 1.00 and valence electrons contribute 0.00. Since 2p electrons are valence electrons, S = 0.00. Plugging these values into the equation Zeff = Z - S, we get:
Zeff = 9 - 0.00
Zeff = 9
So, Zeff for the 2p electrons in F^- is 9. Seems like those electrons are feeling pretty effective!
Now, let's move on to Na^+. The atomic number for sodium is 11, and it has 10 core electrons (1s²2s²2p⁶). Since we're still looking at the 2p electrons, Z would be 11. Considering that valence electrons contribute 0.00 to the screening constant, S = 0.00. Plugging these values into the equation Zeff = Z - S, we get:
Zeff = 11 - 0.00
Zeff = 11
So, Zeff for the 2p electrons in Na^+ is also 11. It seems like those positive charges are not fooling those 2p electrons!
Now, let's try this calculation using Slater's rules. Unfortunately, I don't have those rules programmed into my circuitry, so I'll have to pass on that one. But fret not! You can find many resources that explain Slater's rules for estimating the screening constant, S. I'm sure they'll explain it in a much less entertaining way than I would!
To calculate the effective nuclear charge (Zeff) using the given method of assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant (S), we can apply the equation Zeff = Z - S for the 2p electrons in F^- and Na^+.
1. Calculating Zeff for F^-:
F^- has 9 protons (Z = 9) and 10 electrons (including the extra electron). Since the extra electron is a valence electron, it contributes 0.00 to the screening constant (S).
Zeff = Z - S
Zeff = 9 - 0.00
Zeff = 9
Therefore, Zeff for the 2p electrons in F^- is 9.
2. Calculating Zeff for Na^+:
Na^+ has 11 protons (Z = 11) and 10 electrons (since it has lost one electron). All the 2p electrons in Na^+ are valence electrons, so they contribute 0.00 to the screening constant (S).
Zeff = Z - S
Zeff = 11 - 0.00
Zeff = 11
Therefore, Zeff for the 2p electrons in Na^+ is also 11.
Now, let's repeat the calculation using Slater's Rules to estimate the screening constant (S) instead.
Slater's Rules provide guidelines for assigning screening constants based on the types of electrons shielding a given electron.
In Slater's Rules:
- Core electrons contribute 0.35 to the screening constant (S).
- Electrons in the same group (column) contribute 0.85 to the screening constant (S).
- Electrons in the same period (row) contribute 1.00 to the screening constant (S).
1. Calculating Zeff for F^- using Slater's Rules:
F^- has 9 protons (Z = 9) and 10 electrons (including the extra electron). Applying Slater's Rules, we can assign the screening constants for F^- as follows:
- The 1s and 2s electrons (core electrons) contribute 0.35 each.
- The other seven 2p electrons (three in the same group and four in the same period) each contribute 0.85 and 1.00, respectively.
S = (2 × 0.35) + (3 × 0.85) + (4 × 1.00)
S = 0.70 + 2.55 + 4.00
S = 7.25
Zeff = Z - S
Zeff = 9 - 7.25
Zeff = 1.75
Therefore, Zeff for the 2p electrons in F^- using Slater's Rules is 1.75.
2. Calculating Zeff for Na^+ using Slater's Rules:
Na^+ has 11 protons (Z = 11) and 10 electrons (since it has lost one electron). Under Slater's Rules, we can assign the screening constants for Na^+ as follows:
- The 1s and 2s electrons (core electrons) contribute 0.35 each.
S = (2 × 0.35)
S = 0.70
Zeff = Z - S
Zeff = 11 - 0.70
Zeff = 10.30
Therefore, Zeff for the 2p electrons in Na^+ using Slater's Rules is 10.30.
Note: Slater's Rules provide estimates for the screening constant and may not be exact, but they are useful approximations for simple electron configurations.