# The transition having smallest energy (b) highest frequency and (c) shortest wavelength among the given transitions. Concept introduction: Electronic transitions that take place in excited H atom is, a. Lyman series: electronic transitions take place to the n = 1 level and it is in ultraviolet region. b. Balmer series: electronic transitions take place from n &gt; 2 to the n = 2 level and it is in visible region. c. Ritz-Paschen series: electronic transitions take place from n &gt; 3 to the n = 3 level and it is in infrared region. d. Brackett series: electronic transitions take place from n &gt; 4 to the n = 4 level. e. Pfund series: electronic transitions take place from n &gt; 5 to the n = 5 level Planck’s equation, E = hν = hc λ where, E = energy h = Planck's constant ν = frequency λ= wavelength c= speed of light The energy increases as the wavelength of the light decrease. Also the energy increases as the frequency of the light increases. As the energy gap between two transition states increases the wavelength of the radiation emitted decreases.

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter 6, Problem 60GQ

(i)

Interpretation Introduction

## Interpretation: The transition having smallest energy (b) highest frequency and (c) shortest wavelength among the given transitions.Concept introduction: Electronic transitions that take place in excited H atom is, a. Lyman series: electronic transitions take place to the n = 1 level and it is in ultraviolet region. b. Balmer series: electronic transitions take place from n > 2 to the n = 2 level and it is in visible region. c. Ritz-Paschen series: electronic transitions take place from n > 3 to the n = 3 level and it is in infrared region. d. Brackett series: electronic transitions take place from n > 4 to the n = 4 level. e. Pfund series: electronic transitions take place from n > 5 to the n = 5 level Planck’s equation,    E = hν =hcλwhere, E = energyh = Planck's constantν = frequencyλ= wavelengthc= speed of lightThe energy increases as the wavelength of the light decrease. Also the energy increases as the frequency of the light increases. As the energy gap between two transition states increases the wavelength of the radiation emitted decreases.

(ii)

Interpretation Introduction

### Interpretation: The transition having highest frequency among the given transitions.Concept introduction: Electronic transitions that take place in excited H atom is, a. Lyman series: electronic transitions take place to the n = 1 level and it is in ultraviolet region. b. Balmer series: electronic transitions take place from n > 2 to the n = 2 level and it is in visible region. c. Ritz-Paschen series: electronic transitions take place from n > 3 to the n = 3 level and it is in infrared region. d. Brackett series: electronic transitions take place from n > 4 to the n = 4 level. e. Pfund series: electronic transitions take place from n > 5 to the n = 5 level As the energy gap between two transition states increases the frequency of the radiation emitted also increases.

(iii)

Interpretation Introduction

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