Quantum Numbers

Q. Which of the following sets of quantum numbers represent the highest energy of an atom ?

1. $n=3,l=0,m=0,s=+\frac{1}{2}$
2. $n=3,l=1,m=1,s=+\frac{1}{2}$
3. $n=3,l=2,m=1,s=+\frac{1}{2}$
4. $n=4,l=0,m=0,s=+\frac{1}{2}$

Q.

What is the shape of the p-orbital?

Q. Which of the following statements regarding an orbital is correct?

1. An orbital is a definite trajectory around the nucleus in which electrons can move
2. An orbital always has a spherical trajectory
3. An orbital is a region around the nucleus where the probability of finding all the electrons is 90% to 95%
4. An orbital is characterized by three distinct quantum numbers n, l and m

Q.

The orientation of an atomic orbital is governed by

1. Azimuthal quantum number

2. Spin quantum number

3. Magnetic quantum number

4. Principal quantum number

Q.

What does the magnetic quantum number specifies ?

Q. The magnitude of the orbital angular momentum of an electron is given by $L=\frac{\sqrt{5}h}{\pi }$. How many orbitals of this kind are possible for the subshell?

1. 4
2. 11
3. 9
4. 5

Q. Which one of the quantum numbers describes shape of an orbital?

1. Principal quantum number
2. Azimuthal quantum number
3. Magnetic quantum number
4. Spin quantum number

Q. Which of the following set of quantum numbers is impossible for an electron?

1. $n=1,l=0,m_l=0,m_s=+\frac{1}{2}$
2. $n=9,l=7,m_l=-6,m_s=-\frac{1}{2}$
3. $n=2,l=1,m_l=0,m_s=+\frac{1}{2}$
4. $n=3,l=2,m_l=-3,m_s=+\frac{1}{2}$

Q. Calculate the magnitude of spin angular momentum of an electron.

1. $\frac{\sqrt{3}h}{4\pi }$
2. $\frac{\sqrt{h}}{4\pi }$
3. $\frac{\sqrt{3}h}{\pi }$
4. $\frac{\sqrt{h}}{\pi }$

Q. A transition metal cation $M^{3+}$ has magnetic moment $\sqrt{35}BM$. The number of unpaired electrons in ns orbital of $M^{3+}$ is :
(Note: transition metal exhibit ferromagnetic property)

1. 5
2. 3
3. 2
4. \N

Q.

The spin magnetic momentum of electrons in an ion is 4.84 BM. Its total electronic spin will be

1. $\pm 1$

2. $\pm 2$

3. $\ge$ $\sqrt{\frac{h}{4\pi }}$

4. $\pm 2.5$

Q. What are the values of orbital angular momentum of the electrons in the orbitals 1s, 3s, 3d and 2p ?

1. 0, 0, $\sqrt{6}$ $\hslash$, $\sqrt{2}$ $\hslash$
2. 1, 1, $\sqrt{4}$ $\hslash$, $\sqrt{2}$ $\hslash$
3. 0, 1, $\sqrt{6}$ $\hslash$, $\sqrt{3}$ $\hslash$
4. 0, 0, $\sqrt{20}\hslash$, $\sqrt{6}$ $\hslash$

Q. Which of the following orbital is non-directional?

1. $s$
   
2. $p$
   
3. $d$
   
4. $f$
   
   

Q. What is the minimum possible atomic number of the element containing four electrons in the ground state with magnetic quantum number $m_l$=$+1$ ?

1. $18$
2. $14$
3. $12$
4. $16$

Q. Which shell would be the first to have 'g' subshell?

1. $3^{rd}$
2. $4^{th}$
3. $5^{th}$
4. $6^{th}$

Q. Which of the following set of quantum numbers is permissible?

1. $4,1,+2,+\frac{1}{2}$
2. $4,2,-1,+\frac{1}{2}$
3. $4,0,0,1$
4. $4,4,+2,-\frac{1}{2}$

Q. Which one of the quantum numbers describes shape of an orbital?

1. Principal quantum number
2. Azimuthal quantum number
3. Magnetic quantum number
4. Spin quantum number

Q. How many 'd' electrons in $C{u}^{+}$ can have the spin quantum $\left(\frac{-1}{2}\right)$?

Q.

If the azimuthal quantum number of an electron is 2 then the shape of the orbital is ______

Q.

The quantum number not obtained from Schrodinger’s wave equation is:

1. n

2. l

3. m

4. s

Q. The orbital angular momentum of an electron is $\sqrt{3}\frac{h}{\pi }$. Which of the following may be a permissible value of angular momentum of an electon revolving in an unknown Bohr's orbit?

1. $\frac{h}{\pi }$
2. $\frac{h}{2\pi }$
3. $\frac{3h}{2\pi }$
4. $\frac{2h}{\pi }$

Q. Number of orbitals represented by $n=3,l=2$ and $m=+2$ is:

1. $1$
2. $7$
3. $3$
4. $5$

Q. If the subsidiary quantum number of a subenergy level is 4, the maximum and minimum values of the spin multiplicities are:

1. 9, 1
2. 10, 1
3. 10, 2
4. 4, -4

Q. Calculate the maximum number of electrons which can be present in a shell having principal quantum number 3.

1. 8
2. 4
3. 16
4. 18

Q. The ground state energy of hydrogen atom is $–13.6eV$. Consider an electronic state $\psi$ of $H{e}^{+}$ whose energy, azimuthal quantum number and magnetic quantum number are $-3.4eV,2and0$, respectively. Which of the following statement(s) is(are) true for the state $\psi$ ?

1. It is a $4d$ state
2. It has 3 radial nodes
3. It has 2 angular nodes
4. All statements are incorrect

Q. The minimum number of waves made by a Bohr electron in an orbit of maximum magnetic quantum number $+2$:

1. $3$
2. $4$
3. $2$
4. $1$

Q. Which of the following set of quantum numbers is correct for an electron in 5d orbital?

1. $n=5,l=3,m=2,s=+\frac{1}{2}$
2. $n=5,l=4,m=3,s=+\frac{1}{2}$
3. $n=5,l=2,m=3,s=+\frac{1}{2}$
4. $n=5,l=2,m=2,s=+\frac{1}{2}$

Q. How many degenerate orbitals are present in a subshell if the electron associated with it has an orbital angular momentum $=\frac{2\sqrt{3}h}{2\pi }$

1. No degenerate orbitals
2. Seven degenerate orbitals
3. Three degenerate orbitals
4. The number of degenerate orbitals is same as the subshell which has orbital magnetic moment ${\mu }_L=3.46\text{BM}$

Q. What is the maximum number of electrons in an atom that can have the quantum numbers of $n=4,m_e=+1$

1. 4
2. 15
3. 6
4. 1

Q. The orbital angular momentum of a 4p electron will be :

1. $4\frac{h}{2\pi }$
2. $\sqrt{2}\frac{h}{2\pi }$
3. $\sqrt{6}\frac{h}{4\pi }$
4. $\sqrt{2}\frac{h}{4\pi }$