Answer:
( B) They all have their valence electrons in the same type of subshell.
Explanation:
With each period, a new shell is added to the atom.
Further, the groups are classified based on the type of subshell the last electron enters and number of valence electrons.
For all elements of same group, the last electron enters the same type of subshell.
Say, for group 1, last electron enters s orbital and they have 1 valence elctron.
for group 17, last electron enters p orbital and they have 7 valence electrons.
(A) and (D) are wrong because, energy level of the valence electrons is determined by the principle quantum number n and l and not by the type of subshell(only l) they enter.
(C) if the valence electron enters p orbital, then the elements will be placed in the p- block.
Answer:
Chlorine has 17 total electrons with electron configuration 1s^2 2s^2 2p^6 3s^2 3p^5.
What are the first two quantum numbers for the six electrons in the 2p subshell?
Explanation:
The principal quantum number represents the shell number in which the electron is present.
It is represented with "n".
The next quantum number is the azimuthal quantum number.
It represents the shape of the orbital.
It has values from 0 to (n-1).
Its value depends on the principal quantum number.
Chlorine has 17 total electrons with electron configuration 1s^2 2s^2 2p^6 3s^2 3p^5.
For the six elecetrons in 2p subshell:
The first two quantum number values are the same and their values are:
n=2 , l=1.
I believe <span>Na2SO3 is the solution to the problem.</span>
