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Chapter 2: Problem 102

Cesium, Cs, is used in photoelectric cells ("electric eyes"). The cesium nucleus has a charge of \(+55\). What is the number of electrons in the neutral atom? in the \(\mathrm{Cs}^{+}\) ion?

Short Answer

Expert verified
Neutral Cs atom has 55 electrons; Cs^{+} ion has 54 electrons.

Step by step solution

01

Understanding the Context

A neutral atom has an equal number of protons and electrons. Cesium (Cs) has a nuclear charge of +55, which indicates it has 55 protons in its nucleus.
02

Identifying Electrons in Neutral Atom

For the neutral cesium atom, since the charge is zero, the number of electrons must equal the number of protons to balance the charge. Therefore, a neutral Cs atom has 55 electrons.
03

Understanding Ion Formation

In the formation of a positive ion ( Cs^{+} ), the atom has lost electrons. The positive sign with the ion symbol indicates the atom has lost one electron.
04

Finding the Electrons in the Ion

The Cs^{+} ion, having lost one electron compared to the neutral atom, has 54 electrons.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Neutral Atoms
Neutral atoms are fundamental building blocks in chemistry. They are neutral because they have an equal number of protons and electrons. This balance results in no overall electrical charge.
For example, a neutral cesium (Cs) atom has 55 protons, as indicated by its nuclear charge of +55. Hence, it must also possess 55 electrons to maintain this neutrality.
Neutral atoms are the starting point when discussing ions and chemical reactivity.
  • The number of protons defines the element and remains constant in chemical reactions.
  • Electrons can be gained or lost, leading to ion formation.
This understanding is essential when diving into more complex topics like ionic compounds or conducting electricity.
Ion Charge and Its Significance
Ion charge is a key concept in understanding chemical reactions and bonding. Atoms can become ions by losing or gaining electrons.
A positively charged ion, called a cation, forms when an atom loses one or more electrons. This results in more protons than electrons, creating a net positive charge.

In the case of cesium, when it forms a \(\text{Cs}^{+}\) ion, it has lost one electron compared to its neutral state, giving it 54 electrons.
  • Ion charge plays a crucial role in the formation of ionic bonds.
  • The magnitude of this charge can affect the atom's reactivity and interaction with other ions.
Understanding how ions form and behave is key for grasping broader chemical processes.
The Role of Photoelectric Cells
Photoelectric cells are fascinating devices that convert light energy into electrical energy. Cesium is often used in these cells due to its ability to release electrons when exposed to light.
This phenomenon is based on the photoelectric effect, where light dislodges electrons from the surface of a material. When light hits the cesium, electrons gain energy and are emitted, creating an electric current.
  • Photoelectric cells are used in various applications, such as automatic lighting and solar panels.
  • The efficiency of these cells relies on the type of material and the light's energy.
  • Cesium, with its readiness to lose electrons, enhances the effectiveness of photoelectric cells.
By studying the photoelectric effect, we gain insights into both quantum mechanics and practical applications in renewable energy technologies.

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Most popular questions from this chapter

You have the mythical metal element " \(\mathrm{X}\) " that can exist as \(\mathrm{X}^{+}, \mathrm{X}^{2+}\), and \(\mathrm{X}^{5+}\) ions. a. What would be the chemical formula for compounds formed from the combination of each of the \(\mathrm{X}\) ions and \(\mathrm{SO}_{4}^{2-}\) ? b. If the name of the element \(X\) is exy, what would be the names of each of the compounds from part a of this problem?

The mass-to-charge ratio for the positive ion \(\mathrm{F}^{+}\) is \(1.97 \times 10^{-7} \mathrm{~kg} / \mathrm{C}\). Using the value of \(1.602 \times 10^{-19} \mathrm{C}\) for the charge on the ion, calculate the mass of the fluorine atom. (The mass of the electron is negligible compared with that of the ion, so the ion mass is essentially the atomic mass.)

For each of the following pairs of ions, write the formula of the corresponding compound. a. \(\mathrm{Co}^{2+}\) and \(\mathrm{Br}^{-}\) b. \(\mathrm{NH}_{4}{ }^{+}\) and \(\mathrm{SO}_{4}^{2-}\) c. \(\mathrm{Na}^{+}\) and \(\mathrm{PO}_{4}{ }^{3-}\) d. \(\mathrm{Fe}^{3+}\) and \(\mathrm{NO}_{3}^{-}\)

One isotope of a metallic element has mass number 119 and has 69 neutrons in the nucleus. An atomic ion has 48 electrons. Write the symbol for this ion (give the symbol for the nucleus and give the ionic charge as a right superscript).

For each of the following binary compounds, decide whether the compound is expected to be ionic or molecular. a. \(\mathrm{SeF}_{4}\) b. \(\mathrm{LiBr}\) c. \(\mathrm{SiF}_{4}\) d. \(\mathrm{Cs}_{2} \mathrm{O}\)
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