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Chapter 7: Problem 25

Explain why elements produce their own characteristic colors when they emit photons.

Short Answer

Expert verified
Elements produce their own characteristic colors when they emit photons due to the specific energy levels of their electrons. As electrons transition from higher to lower energy levels, they emit photons of specific energies. These energies correspond to specific frequencies of light (colors). Different elements have different energy levels, hence they emit light of different colors.

Step by step solution

01

Explaining Electron States

Atoms consist of a nucleus and surrounding electrons. These electrons inhabit different energy levels. Electrons in an atom are not allowed to have any energy they want, but are limited to specific energy levels. The electrons prefer to stay in the lowest energy level, called the ground state. But they can move to a higher energy level if they gain energy, for example by absorbing a photon (a particle of light).
02

Describing Energy Transitions

If an electron at a high energy level drops to a lower one, it has to lose energy. This lost energy is emitted as a photon. The energy of a photon corresponds to a certain frequency of light according to the Planck’s relation equation: E = hf, where E is the energy of the photon, h is Planck's constant, and f is the frequency of the photon. The higher the energy difference, the higher the frequency.
03

Linking Photon Energy to Visible Colors

The frequency of a photon determines its color. The human eye can perceive only a small range of these frequencies, which we call visible light. Lower frequency (lower energy) corresponds to red light, while higher frequency (higher energy) corresponds to violet light, with all the other colors in between.
04

Describing Characteristic Colors

Each type of atom has its own set of energy levels. The different energy levels in different atoms means that we see different colors when electrons in different elements transition between energy levels. Thus, each element has a unique color signature.

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Most popular questions from this chapter

Comment on the correctness of the following statement: The probability of finding two electrons with the same four quantum numbers in an atom is zero.

Make a chart of all allowable orbitals in the first four principal energy levels of the hydrogen atom. Designate each by type (for example, \(s, p\) ) and indicate how many orbitals of each type there are.

For each of the following pairs of hydrogen orbitals, indicate which is higher in energy: (a) \(1 s, 2 s ;\) (b) \(2 p\), \(3 p ;\) (c) \(3 d_{x y}, 3 d_{y z};\) (d) \(3 s, 3 d ;\) (e) 4f, \(5 s.\)

Describe the shapes of \(s, p,\) and \(d\) orbitals. How are these orbitals related to the quantum numbers \(n, \ell\) and \(m_{\ell} ?\)

What is the wavelength, in \(\mathrm{nm},\) of radiation that has an energy content of \(1.0 \times 10^{3} \mathrm{~kJ} / \mathrm{mol} ?\) In which region of the electromagnetic spectrum is this radiation found?
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