How many electrons in an atom can have the following designations?

5px

2s

n = 4

5p

7py

4f

how do u do these?

You need to remember that

n = principal quantum number and can take on values of 1, 2, 3, .....

l (as in ell) takes on integral values of 0, 1, 2, etc with the maximum being n-1.

ms can take on integral values from -ell to + ell (including zero).

ms takes on only two values; i.e., +1/2 and -1/2.
You need the above for the n=4 problem. For the others, we have 1 s orbital, 3 p orbitals, 5d orbitals, 7f orbitals.

Now, for one of the problems.
Pick 5px. There are 3 p orbitals, each p is orthogonal (that is they are mutally perpendicular to each other) so the 5px can hold two electrons, the 5py can hold two electrons and the 5pz can hold two electrons.
5p can hold 6.
7py is same as any px, py, or pz.
If there are 7 f orbitals and each hold 2 electrons, then there must be ...... total.
That should be enough to get you started.

To determine the number of electrons in an atom based on the given designations, you need to understand the electron configuration of atoms and the rules that govern the filling of electron orbitals.

Here is the step-by-step breakdown for each designation:

1. 5px:
The "5px" designation refers to the fifth energy level (n = 5) and the px orbital. Each orbital can hold a maximum of 2 electrons. Since there is only one "5px" orbital, it can contain 2 electrons.

Answer: The "5px" designation can have 2 electrons.

2. 2s:
The "2s" designation refers to the second energy level (n = 2) and the s orbital. The s orbital can also hold a maximum of 2 electrons.

Answer: The "2s" designation can have 2 electrons.

3. n = 4:
The "n = 4" designation refers to the fourth energy level. In this case, since it does not specify any particular orbital, we assume it includes all orbitals within that energy level. Therefore, to determine the maximum number of electrons, we sum up the maximum number of electrons in each orbital up to the fourth energy level.

For the fourth energy level (n = 4):
s orbital: 2 electrons
p orbitals: 6 electrons (3 orbitals x 2 electrons each)
d orbitals: 10 electrons (5 orbitals x 2 electrons each)
f orbitals: 14 electrons (7 orbitals x 2 electrons each)

Adding up all these electrons together, we get:
2 + 6 + 10 + 14 = 32

Answer: The "n = 4" designation can have a maximum of 32 electrons.

4. 5p:
The "5p" designation refers to the fifth energy level (n = 5) and the p orbital. Each p orbital can hold a maximum of 2 electrons. However, there are three p orbitals (px, py, and pz) in total, giving a total capacity of 6 electrons.

Answer: The "5p" designation can have 6 electrons.

5. 7py:
The "7py" designation refers to the seventh energy level (n = 7) and the py orbital. Like earlier, each orbital can hold a maximum of 2 electrons. However, since it specifies only the py orbital, there will be only one py orbital at the seventh energy level.

Answer: The "7py" designation can have 2 electrons.

6. 4f:
The "4f" designation refers to the fourth energy level (n = 4) and the f orbital. Each orbital can hold a maximum of 2 electrons. Since the f orbital has a total of seven orbitals (fx, fy, fz, fx', fy', fz', fz''), it can contain a maximum of 14 electrons.

Answer: The "4f" designation can have 14 electrons.

I hope the step-by-step breakdown helps you understand how to determine the number of electrons for each designation. Let me know if you have any further questions!

To determine the number of electrons in an atom with specific designations, you need to understand the electron configuration notation. The electron configuration describes the distribution of electrons among different energy levels and sublevels within an atom.

To find the number of electrons for each designation, you first need to know the maximum number of electrons that can occupy each sublevel:

- The s sublevel can hold a maximum of 2 electrons.
- The p sublevel can hold a maximum of 6 electrons.
- The d sublevel can hold a maximum of 10 electrons.
- The f sublevel can hold a maximum of 14 electrons.

Using this information, let's determine the number of electrons for each designation you provided:

1. 5px: The "5" represents the principal energy level, and "p" indicates the sublevel. The p sublevel can hold a maximum of 6 electrons, so the number of electrons in the 5px orbital is 1.

2. 2s: The "2" represents the principal energy level, and "s" indicates the sublevel. The s sublevel can hold a maximum of 2 electrons, so the number of electrons in the 2s orbital is 2.

3. n = 4: The "n" represents the principal energy level, and "4" indicates the level. Since no specific sublevel is mentioned, we consider all sublevels within the n = 4 energy level. The 4s sublevel can hold a maximum of 2 electrons, and the 4p sublevel can hold a maximum of 6 electrons. Therefore, the number of electrons for n = 4 is 8 (2 from 4s and 6 from 4p).

4. 5p: The "5" represents the principal energy level, and "p" indicates the sublevel. The p sublevel can hold a maximum of 6 electrons, so the number of electrons in the 5p orbital is 6.

5. 7py: The "7" represents the principal energy level, and "p" indicates the sublevel. However, there is no such principle energy level as 7 in the electron configuration. So, the designation 7py is not valid.

6. 4f: The "4" represents the principal energy level, and "f" indicates the sublevel. The f sublevel can hold a maximum of 14 electrons, so the number of electrons in the 4f orbital is 14.

It's important to note that electron configurations can be quite complex but follow a specific order and set of rules. The designations you provided are obtained based on these rules and can be determined using the periodic table and knowledge of electron sublevel filling order.