Question

1. fill in symbol and the number of valence electrons for the following neutral atoms.

1. the s sublevel contains a maximum of ____ number of orbitals and ____ number of electrons.

a. 3, 10
b. 3, 6
c. 1, 2
d. 2, 1

1. *the abbreviated electron configuration for vanadium (v), is:

a. ar4s²
b. ar4s²3d³
c. ar4s²4d⁸
d. ar4d²5s²

1. **the full electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d⁷ represents the element ______

a. copper
b. phosphorous
c. silver
d. krypton

1. **write the full electron configuration for sulfur.

Explanation:

Step1: Determine the symbol and valence electrons for Aluminum and Chlorine

• Aluminum's symbol is Al. It is in group 13 of the periodic table, so it has 3 valence electrons.
• Chlorine (Cl) is in group 17 of the periodic table, so it has 7 valence electrons.

Step2: Analyze the s - sublevel

The s - sublevel has 1 orbital. Each orbital can hold a maximum of 2 electrons. So the s - sublevel contains a maximum of 1 orbital and 2 electrons.

Step3: Find the abbreviated electron configuration for Vanadium (V)

Vanadium has an atomic number of 23. The noble gas core is [Ar] (atomic number 18). Then we fill the 4s and 3d orbitals. The electron configuration is [Ar]4s²3d³.

Step4: Identify the element from the electron configuration

Calculate the total number of electrons: \(2 + 2+6 + 2+6+2 + 7=27\). Copper (Cu) has an atomic number of 29, Phosphorous (P) has 15, Silver (Ag) has 47, and Krypton (Kr) has 36. This is not a correct electron configuration for any of the given options (there might be a typo. If it was \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}\), it would be Cu). But if we assume the given configuration: sum of electrons \(2+2 + 6+2+6+2+7 = 27\) (not a match, but if we consider rules of electron filling, for the options given, maybe a misprint. If we calculate based on the formula for number of electrons from configuration: \(\sum n_{i}\) where \(n_{i}\) is the number of electrons in each sub - shell.

Step5: Write the full electron configuration for Sulfur

Sulfur has an atomic number of 16. The electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}\)

Answer:

1.

Neutral Atom	Symbol	Number of valence electrons
Chlorine	Cl	7

1. c
2. b
3. (There is an error in the problem as the sum of electrons in \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}\) is \(2 + 2+6+2+6+2 + 7=27\) which does not match the given options. If it was \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}3d^{10}\) (Cu has 29 electrons: \(2+2+6+2+6+1 + 10=29\))
4. \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}\)