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Chapter 7: Problem 26

Describe briefly why the study of electromagnetic radiation has been important to our understanding of the arrangement of electrons in atoms.

Short Answer

Expert verified
The study of electromagnetic radiation has been crucial in understanding the arrangement of electrons in atoms. It led to the discovery of atomic spectra, which are unique to each element and provided information about electron movement within atoms, supporting the development of models like Bohr's quantized orbits. Furthermore, it revealed the wave-particle duality nature of electrons, contributing to more advanced atomic models such as the Quantum Mechanical Model. This deeper understanding of atomic structure has numerous applications in chemistry, physics, and technology.

Step by step solution

01

Electromagnetic radiation and electron behavior

Electromagnetic radiation, which includes light, has been fundamental in revealing the behavior and arrangement of electrons in atoms. When atoms absorb energy, their electrons become excited and jump to higher energy levels. When the electrons return to their original state, they emit photons (light). The emitted photons can be analyzed as a spectrum of light which is unique to each element.
02

Atomic spectra and electron arrangement

The study of electromagnetic radiation led to the discovery of atomic spectra. Atomic spectra are the specific patterns of light (lines of color) emitted by an atom's electrons when they transition between energy levels. Each element has its own unique atomic spectrum, which can be used to identify the element. This provided valuable information about electron movement within atoms and supported the development of atomic models.
03

The Bohr model and quantization

Niels Bohr used the principle of electromagnetic radiation in his atomic model, which introduced the idea of quantization. In this model, electrons orbit around the nucleus in specific energy levels or orbits. The quantization principle dictates that electrons can only absorb or emit energy in specific, discrete amounts, corresponding to moving between these orbits. Bohr's model helped to explain the specific wavelengths of light observed in atomic spectra.
04

Wave-particle duality and electron behavior

Further experiments and observations regarding electromagnetic radiation led to the concept of wave-particle duality. This means that electrons, as well as light, exhibit both particle-like and wave-like behavior. This revelation is crucial to our understanding of electrons' arrangement in atoms and contributes to the development of more sophisticated atomic models, such as the Quantum Mechanical Model.
05

Importance of electromagnetic radiation study

In conclusion, the study of electromagnetic radiation has been essential to our understanding of the arrangement of electrons in atoms. It has revealed valuable information about electron behavior, supported the development of atomic models, and allowed scientists to identify elements based on their unique atomic spectra. This deeper understanding of atomic structure has numerous applications, from chemistry to physics and technology, making the study of electromagnetic radiation crucial to our scientific advancement.

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Most popular questions from this chapter

An unknown element is a nonmetal and has a valence electron configuration of \(n s^{2} n p^{4} .\) a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound this element would form with potassium? d. Would this element have a larger or smaller radius than barium? e. Would this element have a greater or smaller ionization energy than fluorine?

Without looking at data in the text, sketch a qualitative graph of the third ionization energy versus atomic number for the elements Na through Ar, and explain your graph.

In each of the following sets, which atom or ion has the smallest ionization energy? a. \(\mathrm{Ca}, \mathrm{Sr}, \mathrm{Ba}\) b. \(\mathrm{K}, \mathrm{Mn}, \mathrm{Ga}\) c. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) d. \(\mathrm{S}^{2-}, \mathrm{S}, \mathrm{S}^{2+}\) e. \(\mathrm{Cs}, \mathrm{Ge}, \mathrm{Ar}\)

A certain microwave oven delivers 750 . watts \((\mathrm{J} / \mathrm{s})\) of power to a coffee cup containing 50.0 \(\mathrm{g}\) water at $25.0^{\circ} \mathrm{C}\( . If the wave- length of microwaves in the oven is \)9.75 \mathrm{cm},$ how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 $\mathrm{J} /^{\prime} \mathrm{C} \cdot \mathrm{g}$ and assume only the water absorbs the energy of the microwaves

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1\(s^{2} 2 s^{2} 3 p^{1}\) b. 1\(s^{2} 2 s^{2} 2 p^{6}\) c. 1\(s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?
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