Questions: Question 8 Which electrons would have the greatest effective nuclear charge? a. the valence electrons in aluminum b. the valence electrons in fluorine c. the se will have the same effective nuclear charge d. the valence electrons in phosphorus

Question 8
Which electrons would have the greatest effective nuclear charge?
a. the valence electrons in aluminum
b. the valence electrons in fluorine
c. the se will have the same effective nuclear charge
d. the valence electrons in phosphorus

Transcript text: Question 8 Which electrons would have the greatest effective nuclear charge? a. the valence electrons in aluminum b. the valence electrons in fluorine c. the se will have the same effective nuclear charge d. the valence electrons in phosphorus

Solution

Solution Steps

Step 1: Understanding Effective Nuclear Charge

The effective nuclear charge (\(Z_{\text{eff}}\)) is the net positive charge experienced by an electron in an atom. It is calculated by considering the actual nuclear charge and subtracting the shielding effect caused by other electrons. The formula is:

\[ Z_{\text{eff}} = Z - S \]

where \(Z\) is the atomic number (total positive charge from protons) and \(S\) is the shielding constant (approximate number of inner electrons).

Step 2: Analyzing the Elements

Aluminum (Al): Atomic number \(Z = 13\). The valence electrons are in the 3rd shell.
Fluorine (F): Atomic number \(Z = 9\). The valence electrons are in the 2nd shell.
Phosphorus (P): Atomic number \(Z = 15\). The valence electrons are in the 3rd shell.

Step 3: Comparing Effective Nuclear Charge

The effective nuclear charge is generally higher for elements with fewer electron shells because the valence electrons are closer to the nucleus and experience less shielding. Fluorine, having its valence electrons in the 2nd shell, will experience a higher effective nuclear charge compared to aluminum and phosphorus, which have their valence electrons in the 3rd shell.