Explanation:
Let’s go through each question one by one.
Question 1: Which of the following is a p orbital?
- A p orbital has a dumbbell shape — two lobes on opposite sides of the nucleus, with a node (zero electron probability) at the nucleus.
- The first image shows two lobes along the z-axis — that’s a pₓ, pᵧ, or p_z orbital (depending on orientation). This matches the classic p orbital shape.
- The second image is spherical — that’s an s orbital.
- The third image has four lobes in a cloverleaf pattern — that’s a d orbital (e.g., dₓy or dₓ²−y²).
- The fourth image also has four lobes but aligned along axes — also a d orbital (likely dₓ²−y²).
✔ So the correct choice is the
first image (dumbbell-shaped along z-axis).
Question 2: If you have a shell with n = 3, how many subshells does it have?
- For a given principal quantum number *n*, the possible subshells are labeled by azimuthal quantum number *ℓ*, where ℓ = 0, 1, 2, ..., (n − 1).
- So for n = 3: ℓ can be 0, 1, or 2 → that’s s, p, and d subshells.
- That’s
three subshells.
✔ Answer: Three.
Question 3: What is the maximum number of electrons that a d subshell can hold?
- A d subshell has ℓ = 2.
- The number of orbitals in a subshell is given by: 2ℓ + 1.
So for d: 2(2) + 1 = 5 orbitals.
- Each orbital holds max 2 electrons → 5 × 2 =
10 electrons.
✔ Answer: Ten.
Final Answer:
1. First option (dumbbell-shaped orbital)
2. Three
3. Ten
Parent Tip: Review the logic above to help your child master the concept of atomic orbitals worksheet.
