What is the electronic configuration of carbide C-4?
Thought it was 1s2 2s2 sp2.
Thanks from Sheryl
C is atomic number 6.
Electronic configuration of the neutral atom is 1s2, 2s2, 2p2.
The carbide ion, C^-4, has four more electrons. So the extra four electrons must be added. Where do you think they go?
4 extra valance electrons.
That's the only way it can be C^-4. Now where do they go? What is the electron configuratiion.
1s2 2s2 2p6? I must have been thinking we were doing the periodic table.
Right. And note that the addition of 4 electrons make a full N = 2 level with 8. Note also that the loss of 4 electrons (remember C is in group IV so it can gain four or lose four) it has 1s2 2s0 2p0; i.e., the outside shell (which is now n= 1) is full with its two electrons.
And note also that since C is in group IV and can "gain or lose four electrrons" it usually does neither and shares its electrons in covalent bonds.
Well, if you think about it, carbide C-4 is quite the electrician. It likes to play with electrons, gaining or losing them as it pleases. It's like the class clown of the periodic table. Instead of following the typical rules, it decides to share its electrons and make some cozy covalent bonds. So, the electronic configuration of carbide C-4 would be 1s2 2s0 2p0, with a dash of rebelliousness.
That's correct! Carbon (C) is in group IV of the periodic table, which means it has 4 valence electrons. In the case of carbide (C^-4), it gains 4 extra electrons to achieve a stable configuration. The electronic configuration of carbide (C^-4) would be 1s2 2s2 2p6.
It's important to note that carbon usually forms covalent bonds by sharing electrons rather than gaining or losing them completely.
Exactly! Carbon (C) is in Group IV of the periodic table, which means it has four valence electrons. In its neutral state, carbon has an electronic configuration of 1s2 2s2 2p2.
Now, to determine the electronic configuration of the carbide ion (C^-4), we know that it has gained four extra electrons. These electrons will fill up the available energy levels starting from the lowest energy level (1s) and moving upward.
Since carbon already has a full 2s and 2p subshell, the extra electrons will fill up the next available subshell, which is the 2nd energy level (n = 2). In the 2nd energy level, there are a total of 8 electrons. Therefore, the electronic configuration of carbide C^-4 is 1s2 2s2 2p6.
It's important to note that in most cases, carbon tends to form covalent bonds by sharing its electrons rather than gaining or losing them. However, in the case of carbide (C^-4), it has gained four electrons to achieve stability.