write the orbital notation for the following set of quantum numbers

n=1, l=0, m=0

There is only one orbital in the n = 1 shell because there is only one way in which a sphere can be oriented in space.

So orbital notation will be 1s.

Great job, this ain't for engineers..

To write the orbital notation for the given set of quantum numbers (n=1, l=0, m=0), we need to understand the meaning of these quantum numbers and how they relate to the orbital notation.

The quantum number 'n' represents the principal quantum number, which specifies the energy level or shell of the electron. The possible values for 'n' are integers starting from 1.

The quantum number 'l' represents the azimuthal quantum number or the orbital shape. It determines the subshell or orbital type within a given energy level. The possible values of 'l' range from 0 to n-1. The orbital shapes corresponding to different 'l' values are as follows:
- l = 0: s orbital
- l = 1: p orbital
- l = 2: d orbital
- l = 3: f orbital

The quantum number 'm' represents the magnetic quantum number, which determines the orientation or direction of the orbital in space. The possible values of 'm' range from -l to +l, including zero.

Given n=1, l=0, and m=0, we have:
- n=1, so the electron is in the first energy level or shell.
- l=0, so the electron is in the s-subshell.
- m=0, so the electron occupies the s-orbital with zero magnetic orientation.

Since the orbital notation follows a specific pattern, the orbital notation for the given set of quantum numbers (n=1, l=0, m=0) would be:
1s^2

Here, '1' represents the principal quantum number and 's' indicates the orbital shape. The superscript '2' denotes that there are two electrons in the 1s orbital, as each orbital can accommodate a maximum of two electrons according to the Pauli exclusion principle.