An atom in its ground state contains 18 electrons. How many of these electrons are in orbital with l = 0 values?

oops. That's not right. There are 6 s electrons so there are 6 with l = 0.

1s2 2s2 2p6 3s2 3p6 = 18 total

s electrons have l = 0 and there are two so you have 6 s electrons.
p electrons have l = -1, 0, +1 so there will be 2 s electrons for the 2p and 2 s electrons for the 3p for 4 more. I count a total of 10.

there are actually 6 electrons with l =0 values

as explained that s electrons have l=0

fttyyyu

I'm sorry, I don't understand what "fttyyyu" means. Can you please provide more context or rephrase your message?

To determine the number of electrons in an orbital with l = 0 values, we need to understand the different quantum numbers associated with an atom.

In an atom, each electron is described by four quantum numbers: n, l, ml, and ms.

- The principal quantum number (n) specifies the energy level or shell in which the electron resides.
- The azimuthal quantum number (l) defines the shape of the orbital and can have values from 0 to n-1.
- The magnetic quantum number (ml) describes the orientation of the orbital and can range from -l to +l.
- The spin quantum number (ms) represents the spin of the electron and can be either +1/2 or -1/2.

For an orbital with l = 0, it means the orbital has spheric symmetry and is called an s orbital.

In an s orbital, there is only one possible ml value, which is 0. So, for an s orbital, there can only be one electron.

Now, knowing that an atom in its ground state contains 18 electrons, we need to find out how many of these electrons occupy s orbitals.

In the ground state electron configuration of an atom, the electrons fill orbitals in order of increasing energy. Following the Aufbau principle, the electron configuration for an atom with 18 electrons would be:

1s² 2s² 2p⁶ 3s² 3p⁶

From this electron configuration, we can see that there are a total of 10 electrons in the n = 1 and n = 2 energy levels.

Now, we need to determine how many of these electrons are in the s orbitals. The 1s orbital can hold a maximum of 2 electrons, and the 2s orbital can also hold a maximum of 2 electrons.

Therefore, there are a total of 2 + 2 = 4 electrons in the s orbitals.

Hence, in an atom with 18 electrons in its ground state, there are 4 electrons in orbitals with l = 0 values (s orbitals).

So actually how many of these electrons are in orbital with 0 values , correct answer?