Structure Of Atom

1. Recall the formulas for calculating the number of nodes:
Number of radial nodes = n - l - 1
Number of angular nodes = l
Total number of nodes = n - 1

where:
n is the principal quantum number
l is the azimuthal quantum number

2. Determine the quantum numbers for a 3p orbital:
For a 3p orbital:
n = 3
l = 1 (since p orbital corresponds to l = 1)

3. Calculate the number of radial and angular nodes:
Number of angular nodes = l = 1
Number of radial nodes = n - l - 1 = 3 - 1 - 1 = 1
The number of angular and radial nodes in a 3p orbital are 1 and 1 respectively.

Final Answer:
(B) 1, 1

The ion in question is 16 32S²⁻, which is the sulfide ion with a 2-negative charge. Let's determine the number of protons, neutrons, and electrons in this ion:

Explanation:

Protons: The atomic number of sulfur (S) is 16, which means it has 16 protons in its nucleus. The number of protons does not change with the charge of the ion, so the number of protons is 16.

Neutrons: The mass number of sulfur is 32 (as shown in the notation 16 32S), which is the sum of protons and neutrons. Therefore, the number of neutrons is: So, the number of neutrons is 16.

Electrons: The sulfide ion (S²⁻) has gained 2 electrons, which means the number of electrons is the number of protons plus 2. Since there are 16 protons, the number of electrons is: So, the number of electrons is 18.

Conclusion:

The number of protons, neutrons, and electrons in the ion 16 32S²⁻ are:

• Protons: 16
• Neutrons: 16
• Electrons: 18

Answer: Option D: 16, 16, 18