Match List I with List II List I List II A. Lyman i. n_1 =3 B. Balmar…

The correct answer is option 1. A-ii, B-iv, C-i, D-iii.

List I	List II
A. Lyman	ii. \(n_1 =1\)
B. Balmar	iv. \(n_1 = 2\)
C. Paschen	i. \(n_1 = 3\)
D. Brackett	iii. \(n_1 = 4\)

The Lyman, Balmer, Paschen, and Brackett series are spectral lines observed in the emission spectrum of hydrogen-like atoms. They are named after the scientists who discovered them and are categorized based on the final energy level (or shell) of the electron involved in the transition.

Here's an explanation of the matches:

A. Lyman series corresponds to transitions to the n=1 energy level.

This series involves transitions where the electron jumps from higher energy levels (n>1) down to the first energy level (n=1). These transitions result in the emission of ultraviolet (UV) photons.

B. Balmer series corresponds to transitions to the n=2 energy level.

This series involves transitions where the electron jumps from higher energy levels (n>2) down to the second energy level (n=2). These transitions result in the emission of visible light, specifically in the visible spectrum.

C. Paschen series corresponds to transitions to the n=3 energy level.

This series involves transitions where the electron jumps from higher energy levels (n>3) down to the third energy level (n=3). These transitions result in the emission of infrared (IR) photons.

D. Brackett series corresponds to transitions to the n=4 energy level.

This series involves transitions where the electron jumps from higher energy levels (n>4) down to the fourth energy level (n=4). These transitions result in the emission of infrared (IR) photons, typically in the longer-wavelength infrared region compared to the Paschen series.

Therefore, the correct match is 1. A-ii, B-iv, C-i, D-iii

Each series represents a specific set of electron transitions within the hydrogen atom, resulting in the emission of photons with characteristic wavelengths associated with each series.