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Part Two-Quantum Numbers

Answer the questions on quantum numbers below. One example has been done for you. Example: What are the first two quantum numbers for the electrons located in subshell 2p? Answer: Energy level (n = 2), p subshell (l = 1)

4. What are the first two quantum numbers for the electrons located in subshell 4d?

5. What are the first three quantum numbers for the electrons located in subshell 2s?

6. How many electrons can be held in a sublevel l = 3?

7. How many electrons can be held in the energy level n = 4?

8. How many electrons in an atom can share the quantum numbers n = 4 and l = 3?

4. Principal and Azimuthal (subsidiary) quantum number

5. Principal, Azimuthal (subsidiary), and magnetic quantum number

6. 10 electrons

7. 32 electrons

8. 36 electrons

Explanation:

4. Principal and Azimuthal (subsidiary) quantum number because in 4d, 4 represent principal quantum number and d - represents azimuthal quantum number (having l - value as 3)

5. Principal, Azimuthal (subsidiary), and magnetic quantum number are the first three because 2 stands for principal, s-for azimuthal (l=0) and magnetic quantum number for s - orbital = 0

6. 10 electrons, because for sublevel with l = 3, is a d-sub-level, and d - can take 10-electrons

7. 32 electrons, using the relationship 2*n^2 for the maximum number of electrons in a shell,

, n = 4, hence 2*4^2 = 32

8. 36 electrons, because n=4 and n = 3 can have the maximum configuration of [Ar]4s^2 3d^10 4p^6

This will sum up to 36 - electrons, since Argon has 18 - electrons.

18+2+10+6=36 electrons