How many electrons in an atom can have each of the following quantum number or sublevel designations?
(a)n=2; l=1; m=0
(b)5s
(c)n=4; l=1
b is 2.
What do you think for the others (and why)?
To determine the number of electrons in an atom that can have each quantum number or sublevel designation, you need to apply the principles of electron configuration.
In the electron configuration, electrons are distributed into different sublevels, which are described by the quantum numbers n, l, and m.
(a) For the quantum numbers n=2, l=1, m=0:
1. Determine the maximum number of electrons that can occupy a sublevel by using the formula: 2(2l + 1). In this case, l=1, so the maximum number of electrons in this sublevel is 2(2(1) + 1) = 6.
(b) For the sublevel designation 5s:
1. Identify the principal quantum number (n) as 5, which indicates the fifth energy level.
2. Recognize that the s-sublevel can accommodate a maximum of 2 electrons.
Therefore, the 5s sublevel can contain a maximum of 2 electrons.
(c) For the quantum numbers n=4, l=1:
1. Determine the maximum number of electrons that can occupy a sublevel by using the formula: 2(2l + 1). In this case, l=1, so the maximum number of electrons in this sublevel is 2(2(1) + 1) = 6.
Hence, the maximum number of electrons that can have each of the given quantum number or sublevel designations are:
(a) 6 electrons
(b) 2 electrons
(c) 6 electrons.