UltravioletVisibleInfrared5 14-13 12 14.3and corresponding wavelengths in theThe emission spectrum then consists of discretelines rather than a continuum in which light isemitted at all frequencies. Many such electronictransitions take place with emission of light inthe visible region of wavelength 370-700 nm;these transitions can be observed with relativelyspset of "orbits" is not equal). The wavelengthof light in the electromagnetic spectrum corrsponding to changes in electronic states in hdrogen were described empirically by Rydbeaccording to the formula:simple equipment and the human eye. It is alsopossible to examine changes in energy states of1.R.1.1.H.n=5n=4Lyman seriesn=36-1High energyn=26 25+2Balmer4 2seriesn=1H.3 2OHayden-McNeil, LLCn-26 3Low energyn=3Paschen seriesn=4Figure 2.2 Transitions in the hydrogen atom (shown schematically-not to scale) 2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave-length, energy, and frequency: 6→ 5, 3 → 1, 7 → 3. Note that the energy levels in Figure 2.2are shown schematically, so you must calculate the energy difference between any two levelsin order to answer this question. Show all calculations below or on the following page.Wavelength:Energy:Frequency:

2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6 → 5, 3 → 1, 7-→ 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:

2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave- length, energy, and frequency: 6 → 5, 3 → 1, 7-→ 3. Note that the energy levels in Figure 2.2 are shown schematically, so you must calculate the energy difference between any two levels in order to answer this question. Show all calculations below or on the following page. Wavelength: Energy: Frequency:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

Ultraviolet
Visible
Infrared
5 1
4-1
3 1
2 1
4.
3
and corresponding wavelengths in the
The emission spectrum then consists of discrete
lines rather than a continuum in which light is
emitted at all frequencies. Many such electronic
transitions take place with emission of light in
the visible region of wavelength 370-700 nm;
these transitions can be observed with relatively
sp
set of "orbits" is not equal). The wavelength
of light in the electromagnetic spectrum corr
sponding to changes in electronic states in h
drogen were described empirically by Rydbe
according to the formula:
simple equipment and the human eye. It is also
possible to examine changes in energy states of
1.
R.
1.
1.
H.
n=5
n=4
Lyman series
n=3
6-1
High energy
n=2
6 2
5+2
Balmer
4 2
series
n=1
H.
3 2
OHayden-McNeil, LLC
n-2
6 3
Low energy
n=3
Paschen series
n=4
Figure 2.2 Transitions in the hydrogen atom (shown schematically-not to scale)

2. Rank the following three transitions in the hydrogen atom in terms of lowest to highest wave-
length, energy, and frequency: 6→ 5, 3 → 1, 7 → 3. Note that the energy levels in Figure 2.2
are shown schematically, so you must calculate the energy difference between any two levels
in order to answer this question. Show all calculations below or on the following page.
Wavelength:
Energy:
Frequency:

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