For the energy levels in an atom,which one of | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The correct statement is $(b)$. The second principal energy level $(n=2)$ consists of $2s$ and $2p$ subshells. The $2s$ subshell has $1$ orbital a

Vedclass · Accepted Answer

The second principal energy level can have four sub-energy levels and contains a maximum of eight electrons

Vedclass · Answer

(B) The correct statement is $(b)$. The second principal energy level $(n=2)$ consists of $2s$ and $2p$ subshells. The $2s$ subshell has $1$ orbital and the $2p$ subshell has $3$ orbitals,totaling $4$ orbitals. Each orbital can hold $2$ electrons,so the maximum capacity is $4 	imes 2 = 8$ electrons. Option $(a)$ is incorrect as there are theoretically infinite energy levels. Option $(c)$ is incorrect because the $M$ shell $(n=3)$ can hold $2n^2 = 2(3)^2 = 18$ electrons. Option $(d)$ is incorrect because according to the $(n+l)$ rule,$4s$ $(4+0=4)$ has lower energy than $3d$ $(3+2=5)$.

For the energy levels in an atom,which one of the following statements is correct?

Similar Questions

Write down about the electron spin quantum number $(s)$.

Statement $1$: The energy of an electron is determined by the principal quantum number.
Statement $2$: The principal quantum number $(n)$ indicates the distance of the electron from the nucleus.

What will be the maximum number of electrons in any atom having quantum numbers $n = 4, l = 2, m = -2$?

The electronic configuration of the phosphide ion $(P^{3-})$ is similar to which of the following?

Arrange the following orbitals in increasing order of energy based on the given values of principal quantum number $(n)$ and azimuthal quantum number $(l)$:
$(1) n = 4, l = 1$
$(2) n = 4, l = 0$
$(3) n = 3, l = 1$
$(4) n = 3, l = 2$

Vedclass Test Series

Exam Paper Generator

Online Exam Module