Match the following species with their corresponding ground state electronic configuration.

	Column 1 (Atom/Ion)		Column  2 (Electronic configuration)
A.	Cu	1.	$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}$
B.	Cu2+	2.	$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^2$
C.	Zn2+	3.	$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^1$
D.	Cr3+	4.	$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^9$
		5.	$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^3$

 

	A	B	C	D
1.	4	2	5	1
2.	3	4	1	5
3.	3	2	1	4
4.	4	2	1	3

Match the quantum numbers with the information provided by them:

Match the ensuing rules with the corresponding statements:
 

Match types of wave in Column-I with the corresponding frequency in Column-II and mark the appropriate option:

A 25-watt bulb emits monochromatic yellow light with a wave length of 0.57µm. The rate of emission of quanta per second would be :

1. 7.17 × 10^–19 s^–1

2. 4.13 × 10¹⁶ s^–1

3 . 7.17 × 10¹⁹ s^–1

4 . 1.26 × 10²⁰ s^–1
${\mathrm{}}^{}$

The wavelength of light emitted when the electron in a H atom undergoes the transition from an energy level with n = 4 to an energy level with n = 2, is :

1. 586 mm

2. 486 nm

3. 523 nm

4. 416 pm

The wave number for the longest wavelength transition in the Balmer series of atomic hydrogen would be :

\(1 .   1 . 52   \times   10^{6}   m^{- 1}\)
\(2 .   3 . 14   \times   10^{6}   \left(cm\right)^{- 1}\)
\(3 .   15 . 2   \times   10^{6}   m^{- 1}\)
\(4 .   1 . 52   \times   10^{6}   \left(cm\right)^{- 1}\)

A photon detector receives a total energy of \(3.15 \times 10^{-18}\) J from radiation with a wavelength of 600 nm. How many photons are received by the detector?

$1.$ ${10}^2$
$2.$ $10$
$3.$ $50$
$4.$ $20$

If the velocity of the electron is 1.6 × 10⁶ ${\mathrm{ms}}^{-1}$. Find the de-Broglie wavelength associated with this electron:

$1.$ $590$ $\mathrm{pm}$
$2.$ $455$ $\mathrm{pm}$
$3.$ $512$ $\mathrm{pm}$
$4.$ $401$ $\mathrm{pm}$