When writing a possible excited state electron configuration there are two rules, which are?

When writing a possible excited state electron configuration there are two rules, which are?

Answers

1)Oxygen atoms have 8 electrons and the shell structure is 2.6. The ground state electron configuration of ground state gaseous neutral oxygen is [He]. 2s2. 2p4 and the term symbol is 3P2.

Explanation:

2)If the element were to become excited, the electron could occupy an infinite number of orbitals. However, in most texts the example will be the next available one. So for oxygen, it might look like this: 1s22s22p33s1 - where the valence electron now occupies the 3s orbital in an excited (i.e. not ground) state

Explanation:

Well ik its not math for this but for the first one if u add

22+22+13+1 u get 58

then second one 1+22+22+2=47

1+22+22+24+1=70

1+22+22+13+1=59

U notice how that most or some are all going up to 50 except the third one

So that means its 1s22s22p24s1

If an element (abbreviated X) has a ground state electron configuration of (Ne)3s23p4, then the formula of the compound that X forms with sodium is Na2X. True

The element with a ground state electron configuration of 1s22s22p63s2 is an alkaline earth metal. True

The element with a ground state electron configuration of (Kr)5s24d105p5 has 15 valence electrons. True

The ground state electron configuration for Cu is (Ar)4s13d10. True

Explanation:

The ground state electron configuration for the undiscovered element 115 is (Rn)7s25f146d107p3. Is not the correct electron configuration for the element moscovium. It is no longer undiscovered but is now well known. The correct electron configuration is Moscovium: [Rn]5f14 6d10 7s2 7p3 OR

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 5f14 6d10 7s2 7p3.

The electron configuration of 1s22s22p63s23p64s13d8 is an excited state electron configuration for Ni.. This statement has to be false because the excited electron must be promoted to a higher energy level. Which was not reflected in the configuration written above.

As it travels through space, electromagnetic radiation hope this helps
The ground state electron configuration of carbon is 1s22s22p2. An excited state electron configuration of carbon is 1s22s12p3. This is the state of carbon when it undergoes chemical bonding to form four covalent bonds, as in methane, CH4. However, the experimental evidence shows that all four bonds have the same energy, which can only be explained by the concept that the 2s and 2p orbitals hybridize to form four sp3 orbitals, each with one unpaired electron.
What I don’t understand

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