give electron configuration for a> Na
b) Na+ c) O
d)O ^2-
the electron configuration for sodium is
11
Na
SODIUM
22.99 amu
1.0
+1
[Ne]
3s1
I imagine that the question is looking for the full electronic config. in each case.
So for Na
1s^2 2s^2 2p^6 3s^1
a) Na: To determine the electron configuration for sodium (Na), we need to refer to the periodic table. Sodium is in the third period of the periodic table, so it has three energy levels. The electron configuration can be determined by filling up the energy levels in order of increasing energy.
The electron configuration for sodium is: 1s^2 2s^2 2p^6 3s^1. This means that sodium has 11 electrons distributed across three energy levels. The first energy level (1s) has 2 electrons, the second energy level (2s and 2p) has 8 electrons (2s^2 2p^6), and the third energy level (3s) has 1 electron.
b) Na+: Sodium loses one electron to form a sodium ion (Na+). The electron configuration for Na+ can be determined by subtracting 1 electron from the neutral sodium atom. Therefore, the electron configuration for Na+ is: 1s^2 2s^2 2p^6.
c) O: Oxygen is in the second period of the periodic table, so it has two energy levels. The electron configuration for oxygen is: 1s^2 2s^2 2p^4. This indicates that oxygen has 8 electrons distributed across two energy levels. The first energy level (1s) has 2 electrons, and the second energy level (2s and 2p) has 6 electrons (2s^2 2p^4).
d) O^2-: Oxygen gains two electrons to form an oxygen ion with a charge of -2 (O^2-). The electron configuration for O^2- can be determined by adding 2 electrons to the neutral oxygen atom. Therefore, the electron configuration for O^2- is: 1s^2 2s^2 2p^6.