What is a possible quantum number set for an electron in the 3s orbital of a magnesium atom
1 answer:
- <em>n</em> = 3
- <em>l</em> = 0
= 0
= 1/2 or -1/2
There are four quantum numbers in an electron that orbits the atom.
- <em>n</em>, the principal quantum number.
- <em>l</em>, the angular quantum number.
<em>n</em> is a positive integer. The value of n indicates the main shell of the electron. The electron in question is in the 3s orbital. As a result, <em>n</em> = 3.
<em>l</em> is a non-negative integer. The value of <em>l</em> indicates the type of subshell ("orbital") of the electron. The types of subshells possible depends on the main shell. For example, both s and p orbitals exist in the second main shell. However, only the s orbital exists in the first main shell. The value of <em>l</em> ranges from 0 to <em>n</em> - 1.
- <em>l</em> = 0 indicates an <em>s</em> orbital.
- <em>l</em> = 1 indicates a <em>p</em> orbital.
- <em>l</em> = 2 indicates a <em>d</em> orbital.
- <em>l</em> = 3 indicates an <em>f</em> orbital.
The electron in question is in an <em>s</em> orbital. As a result, <em>l </em>= 0.
is an integer. The value of
indicates the position of the electron within the subshell. The range of
depends on the value of <em>l</em>.
ranges from -<em>l</em> to <em>l </em>(that's <em>-l</em>, ..., -1, 0, 1, ... <em>l</em>). Accordingly, there are 2 <em>l</em> + 1 orbitals in a <em>l</em> subshell. <em>l </em>= 0 for this 3s<em> </em>electron. There's only one orbital in the 3s subshell. The only
value possible for this electron is 0.
The value of is either - 1/2 or 1/2. It indicates the position of an electron within a single orbital. The value of
does not depend on that of <em>n</em>, <em>l</em>, or
. However, by the Pauli Exclusion Principle, at least one of the four numbers must differ for two electrons in the same atom. In case all three of <em>n</em>, <em>l</em>, and
are the same, the two electrons must differ in
. However, this question asks only for the number of one single electron. Thus, giving either - 1/2 or 1/2 shall work.
Vitz et. al, "5.8 Quantum Numbers (Electronic)", <em>ChemPRIME (Moore et al.)</em>, Chemistry Libretexts. 27 Oct 2017.
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Answer: Option (c) is the correct answer.
Explanation:
A limiting reagent is defined as a reagent that completely gets consumed in a chemical reaction. A limiting reagent limits the formation of products.
For example, we have given 5 mol of A and the reaction is
Whereas when 4 mol B will react with 2 mol of A. Hence, 8 mol of B will react with 4 mol A as follows.
= 4 mol
As, the given moles of A is more than the required moles. Thus, it is considered as an excess reagent.
Hence, B is a limiting reagent because it limits the formation of products.
Thus, we can conclude that limiting reactant is the term used to describe the reactant that is used up completely and controls the amount of product that can be produced during a chemical reaction.