Three quantum numbers are derived from Schrodinger’s equation that describe the probability of finding an electron around a nucleus: the principal quantum number, the angular momentum quantum number, and the magnetic quantum number. Define each quantum number.

Principal Quantum Number- This quantum number designates the principal electron shell.

Angular Momentum Quantum Number-This quantum number determines the shape of an orbital and thus the angular distribution.

Magnetic Quantum Number- This quantum number determines the number of orbital number and their orientation within a subshell.

Step-by-step explanation:

Principal Quantum Number, n

This quantum number designates the principal electron shell. It denotes the energy and the most probable distance of the electron from the nucleus. Its value is always greater than or equal to 1, that is, n ≥ 1. It can takes values from n = 1,2,3,4The value n= 1 denotes the first principal shell, n = 2 denotes the second principal shell and so on.

Angular Momentum Quantum Number l

This quantum number determines the shape of an orbital and thus the angular distribution. It can take values from 0 to (n - 1). That is l = 0,1,2,...,(n - 1)

The magnetic Quantum Number, m

This quantum number determines the number of orbital number and their orientation within a subshell. The value of the magnetic quantum number varies from -l to +l. That is m = -l,(-l -1), (-l -2),..., 0, +(l -2), +(l -1), +l

that is the sum

step-by-step explanation:

there are no other answers without knowing the variables values

f(x) = y

f(-3) = -5

step-by-step explanation: