Question
Match List I with List II : List I (Quantum Numbers ) $n$, $l$ Choose the correct answer from the options given below :List II (Orbital) A. 2, 1 I. 3d B. 4, 0 II. 2p C. 5, 3 III. 4s D. 3, 2 IV. 5f
This question was previously asked in
NEET UG Re-Exam 2026 Question Paper (21-Jun-2026)
The correct answer is
A-II, B-III, C-IV, D-I
Matching Quantum Numbers ($n, l$) to Atomic Orbitals
To match the quantum numbers ($n$, $l$) with the correct atomic orbital notation, we need to understand the meaning of each quantum number:
- The principal quantum number, $n$, indicates the electron shell or energy level. It can be any positive integer ($1, 2, 3, \dots$).
- The azimuthal or angular momentum quantum number, $l$, indicates the shape of the orbital and the subshell. The possible values of $l$ range from $0$ to $n-1$.
- $l=0$ corresponds to an 's' orbital.
- $l=1$ corresponds to a 'p' orbital.
- $l=2$ corresponds to a 'd' orbital.
- $l=3$ corresponds to an 'f' orbital.
The orbital notation is formed by combining the value of $n$ with the letter corresponding to $l$ (e.g., $n=2, l=1$ is denoted as 2p).
Matching Process
Let's match each pair from List I to List II:
- A. $n=2, l=1$: Since $l=1$, it represents a 'p' orbital. With $n=2$, the orbital is 2p. This matches with II.
- B. $n=4, l=0$: Since $l=0$, it represents an 's' orbital. With $n=4$, the orbital is 4s. This matches with III.
- C. $n=5, l=3$: Since $l=3$, it represents an 'f' orbital. With $n=5$, the orbital is 5f. This matches with IV.
- D. $n=3, l=2$: Since $l=2$, it represents a 'd' orbital. With $n=3$, the orbital is 3d. This matches with I.
Summary of Matches
| List I Item | Quantum Numbers ($n, l$) | List II Item | Corresponding Orbital |
|---|---|---|---|
| A | (2, 1) | II | 2p |
| B | (4, 0) | III | 4s |
| C | (5, 3) | IV | 5f |
| D | (3, 2) | I | 3d |
The correct matching is A-II, B-III, C-IV, D-I.
Was this answer helpful?
Similar Questions
- In a qualitative analysis, $Bi^{3+}$ is detected by appearance of precipitate of $BiO(OH)(s)$. Calculate pH when the following equilibrium exists at 298 K :
$$BiO(OH) (s) \rightleftharpoons BiO^+ (aq) + OH^- (aq)$$
$K = 4 \times 10^{-10}$
(Given : $\log 2 = 0.3010$) - When $1 \text{ dm}^3$ of $CO_2$ gas is passed over hot coke, the volume of gaseous mixture after complete reaction at STP becomes $1.4 \text{ dm}^3$. The composition of the gaseous mixture at STP is :
- A solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at cathode is :
(Given : Molar mass of Cu = $63 \text{ g mol}^{-1}$, $1 \text{ F} = 96487 \text{ C mol}^{-1}$) - Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T (K).
$\ln k = 14.34 - \frac{1.25 \times 10^4}{T}$
The energy of activation in $\text{kcal mol}^{-1}$ for the reaction is :
(Given : $k \text{ in s}^{-1}$, $R = 1.987 \text{ cal mol}^{-1} \text{ K}^{-1}$) - Match List I with List II :
List I (Order of reaction) List II (Unit of rate constant) A. Zero order I. $mol^{-1} L s^{-1}$ B. First order II. $mol^{-2} L^2 s^{-1}$ C. Second order III. $s^{-1}$ D. Third order IV. $mol L^{-1} s^{-1}$
Choose the correct answer from the options given below : At 298 K, a certain buffer solution contains equal concentrations of $X^{-}$ and $HX$. $K_b$ for $X^-$ is $10^{-10}$. What is the pH of this buffer solution ?
- At a certain temperature T (K), during a process, 500 J is absorbed by the system and work of 200 J is done by the system. Then change in internal energy of the system is :
Consider the following reaction :
$2A (g) + B (g) \rightarrow 2D (g)$
$\Delta U^\ominus = -10 \text{ kJ mol}^{-1}$ and $\Delta S^\ominus = -44 \text{ J K}^{-1}$ at 298 K.
Identify the correct option with $\Delta G^\ominus$ for the reaction and spontaneity of the reaction at 298 K. (Given : $R = 8.31 \text{ J mol}^{-1} \text{K}^{-1}$)- A bulb is rated at 150 watt, converting 8% energy into light. If energy of one photon is $4.42 \times 10^{-19} \text{ J}$, how many photons are emitted by the bulb per second ?
- Given below are certain reactions. Identify the reaction for which $K_p \neq K_c$.
Important Questions from Physical Chemistry
- Consider the following electrochemical cell :
$\text{Pt} \mid \text{O}_2\text{(g)}(1\text{bar}) \mid \text{HCl(aq)} \parallel \text{M}^{2+}\text{(aq, 1.0 M)} \mid \text{M(s)}$
The pH above which, oxygen gas would start to evolve at anode is _________ (nearest integer).
Given :
$\begin{bmatrix} \text{E}^\circ_{\text{M}^{2+}/\text{M}} = 0.994 \text{ V} \\ \text{E}^\circ_{\text{O}_2/\text{H}_2\text{O}} = 1.23 \text{ V} \end{bmatrix} \text{standard reduction potential}$
and $\frac{\text{RT}}{\text{F}} (2.303) = 0.059 \text{ V}$ at the given condition - X and Y are the number of electrons involved, respectively during the oxidation of $\text{I}^-$ to $\text{I}_2$ and $\text{S}^{2-}$ to S by acidified $\text{K}_2\text{Cr}_2\text{O}_7$. The value of X + Y is ______.
- Consider two Group IV metal ions $\text{X}^{2+}$ and $\text{Y}^{2+}$.
A solution containing 0.01 M $\text{X}^{2+}$ and 0.01 M $\text{Y}^{2+}$ is saturated with $\text{H}_2\text{S}$. The pH at which the metal sulphide YS will form as a precipitate is ______. (Nearest integer)
(Given: $\text{K}_{sp}(\text{XS}) = 1 \times 10^{-22}$ at $25^\circ\text{C}$, $\text{K}_{sp}(\text{YS}) = 4 \times 10^{-16}$ at $25^\circ\text{C}$, $[\text{H}_2\text{S}] = 0.1\text{M}$ in solution, $\text{K}_{a1} \times \text{K}_{a2}(\text{H}_2\text{S}) = 1.0 \times 10^{-21}$, $\log 2 = 0.30$, $\log 3 = 0.48$, $\log 5 = 0.70$) - Electricity is passed through an acidic solution of $\text{Cu}^{2+}$ till all the $\text{Cu}^{2+}$ was exhausted, leading to the deposition of 300 mg of Cu metal. However, a current of 600 mA was continued to pass through the same solution for another 28 minutes by keeping the total volume of the solution fixed at 200 mL. The total volume of oxygen evolved at STP during the entire process is ______ mL. (Nearest integer)
[Given:
$\text{Cu}^{2+}\text{(aq)} + 2\text{e}^- \rightarrow \text{Cu(s)} \quad \text{E}^\circ_{\text{red}} = +0.34 \text{ V}$
$\text{O}_2\text{(g)} + 4\text{H}^+ + 4\text{e}^- \rightarrow 2\text{H}_2\text{O} \quad \text{E}^\circ_{\text{red}} = +1.23 \text{ V}$
Molar mass of Cu = $63.54 \text{ g mol}^{-1}$
Molar mass of $\text{O}_2$ = $32 \text{ g mol}^{-1}$
Faraday Constant = $96500 \text{ C mol}^{-1}$
Molar volume at STP = 22.4 L] - Two liquids A and B form an ideal solution at temperature T K. At T K, the vapour pressures of pure A and B are 55 and $15 \text{ kN m}^{-2}$ respectively. What is the mole fraction of A in solution of A and B in equilibrium with a vapour in which the mole fraction of A is 0.8?
Need Expert Advice?
More Questions from NEET
