A Gouy balance is used to determine the magnetic susceptibility of a substance. A strong electromagnet is placed next to the sample, which is on a balance. If the sample is paramagnetic, the mass reading of the balance will increase when the field is switched on. Based on their electron configurations, predict whether these elements are paramagnetic or diamagnetic.

Paramagnetic:
?
Diagmagnetic:
?

Elements:
Ar Be C P

Write their electron configuration, then determine if they have unpaired electrons.

13Al = 1s2 2s2 2p6 3s2 2p1. Yes, it has 1 unpaired electron so it is paramagnetic.

Is all the elements diamagnetic?

No. All of the elements are not dimagnetic. The Al I wrote is paramagnetic.

There is no Al. Only Ar. The elements are Ar, Be, C, P.

I know that. I wrote Al, thinking that if you knew how to do Al you would know how to do the others. I answered all of these at your other post.

To predict whether an element is paramagnetic or diamagnetic based on its electron configuration, we need to consider the presence of unpaired electrons. Paramagnetic substances have at least one unpaired electron, which will align with an applied magnetic field, causing the mass reading of the balance to increase. Diamagnetic substances, on the other hand, have all their electrons paired, and they will not be significantly affected by the magnetic field.

Let's determine the electron configuration of each element and identify whether they are paramagnetic or diamagnetic:

1. Argon (Ar): The atomic number of Argon is 18. After filling up the electron configuration, it becomes 1s^2 2s^2 2p^6 3s^2 3p^6. Argon has a completely filled 3p orbital, meaning all its electrons are paired. Therefore, Argon is diamagnetic.

2. Beryllium (Be): The atomic number of Beryllium is 4. Its electron configuration is 1s^2 2s^2. Beryllium has paired electrons in both the 1s and 2s orbitals, so it is diamagnetic.

3. Carbon (C): The atomic number of Carbon is 6. Its electron configuration is 1s^2 2s^2 2p^2. Carbon has two unpaired electrons in the 2p orbital, so it is paramagnetic.

4. Phosphorus (P): The atomic number of Phosphorus is 15. Its electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^3. Phosphorus has three unpaired electrons in the 3p orbital, so it is paramagnetic.

In summary:
- Argon (Ar) and Beryllium (Be) are diamagnetic.
- Carbon (C) and Phosphorus (P) are paramagnetic.