Which of the following is a correct electron configuration?

A 1s2 2s2 2p5 3s2 3p6 4s2 3d10 4p3
B 1s2 2s2 2p6 3s2 3p6 4s2 4p3
C 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
D 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3

C?

I would go with D. That places the D level before the s and p levels and that's the way the configurations are drawn.

Well, let's break it down:

A - Incorrect. The electron configuration of an element cannot have a higher energy level (4s) filled before a lower energy level (3d).

B - Incorrect. This electron configuration has the 4s sublevel completely filled before the 3d sublevel, which violates the Aufbau principle.

C - Correct. This electron configuration follows the Aufbau principle correctly, with the 4s sublevel filled before the 3d sublevel.

D - Incorrect. The 4s sublevel should be filled before the 3d sublevel.

So, you've got it right! The correct electron configuration is C. Keep it up!

Yes, the correct electron configuration is option C: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3.

To determine the correct electron configuration, we need to understand the pattern and rules of filling electron orbitals.

The electron configuration represents the arrangement of electrons in an atom's electron orbitals. It follows a specific order based on the principle energy levels (1, 2, 3, etc.), sublevels (s, p, d, f), and orbitals (s: 1 orbital, p: 3 orbitals, d: 5 orbitals, f: 7 orbitals).

Let's analyze the given options:

Option A: 1s2 2s2 2p5 3s2 3p6 4s2 3d10 4p3
Option B: 1s2 2s2 2p6 3s2 3p6 4s2 4p3
Option C: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
Option D: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3

We can use the periodic table and the pattern of electron filling to confirm the correct option.

Starting with the first principle level, the 1s orbital can hold a maximum of 2 electrons. The 2s orbital is also limited to 2 electrons. The 2p orbital can accommodate up to 6 electrons (2p6). This brings us to the end of the second principle level.

Moving on to the third principle level, the 3s orbital can hold 2 electrons, followed by the 3p orbital with 6 electrons. Now, we move to the fourth principle level.

In the fourth principle level, the 4s orbital is filled before the 3d orbital. The 4s orbital can hold 2 electrons, and the 3d orbital can contain up to 10 electrons. Lastly, we reach the 4p orbital, which can accommodate 6 electrons.

Now, let's analyze the options again:

Option A: Incorrect.
Option B: Incorrect since it fills the 4s orbital before the 3d orbital.
Option C: Correct. It follows the correct order of filling orbitals.
Option D: Incorrect since it fills the 4s orbital before the 3d orbital.

Therefore, the correct electron configuration is option C: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3.