Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 103

Elemental cesium reacts more violently with water than does elemental sodium. Which of the following best explains this difference in reactivity? (i) Sodium has greater metallic character than does cesium. (ii) The first ionization energy of cesium is less than that of sodium. (iii) The electron affinity of sodium is smaller than that of cesium. (iv) The effective nuclear charge for cesium is less than that of sodium. (v) The atomic radius of cesium is smaller than that of sodium.

Short Answer

Expert verified
The best explanation for the higher reactivity of cesium with water compared to sodium is option (ii), the first ionization energy of cesium being less than that of sodium. This is because a lower ionization energy means cesium can lose its valence electron more easily than sodium, which results in a more violent reaction with water.

Step by step solution

01

Understanding metallic character and reactivity

Metallic character refers to the properties of elements that are typical of metals, such as high electrical and thermal conductivity, malleability, and ductility. In general, metallic character increases as we move down and to the left in the periodic table. Therefore, cesium, being further down and to the left of sodium in the periodic table, has a greater metallic character than sodium.
02

Understanding ionization energy

Ionization energy is the energy required to remove an electron from an atom. In general, ionization energy decreases as we move down a group in the periodic table. This is due to the increased atomic size and a weaker force between the nucleus and the outer electrons. Since cesium is further down the periodic table than sodium, its first ionization energy is lower than that of sodium.
03

Understanding electron affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom. Electron affinity generally becomes more negative as we move across a period in the periodic table. This trend is not directly related to reactivity with water, so it doesn't help explain the difference in reactivity between sodium and cesium.
04

Understanding effective nuclear charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom, taking into account the shielding effect of inner electrons. The effective nuclear charge generally increases as we move across a period in the periodic table. This trend is not directly related to reactivity with water, so it doesn't help explain the difference in reactivity between sodium and cesium.
05

Understanding atomic radius

Atomic radius is the measure of the size of an atom. The atomic radius generally decreases as we move across a period and increases as we move down a group in the periodic table. Since cesium is further down the periodic table than sodium, its atomic radius is larger than that of sodium.
06

Conclusion

Based on our understanding of these properties, the best explanation for the higher reactivity of cesium with water compared to sodium is option (ii), the first ionization energy of cesium being less than that of sodium. This is because a lower ionization energy means cesium can lose its valence electron more easily than sodium, which results in a more violent reaction with water.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In the chemical process called electron transfer, an electron is transferred from one atom or molecule to another. (We will talk about electron transfer extensively in Chapter 20.) A simple electron transfer reaction is $$\mathrm{A}(g)+\mathrm{A}(g) \longrightarrow \mathrm{A}^{+}(g)+\mathrm{A}^{-}(g)$$ In terms of the ionization energy and electron afnity of atom A, what is the energy change for this reaction? For a representative nonmetal such as chlorine, is this process exothermic? For a representative metal such as sodium, is this process exothermic?

Using only the periodic table, arrange each set of atoms in order of increasing radius: (a) Ba, Ca, Na; (b) In, Sn, As; (c) Al, Be, Si.

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. \((\mathbf{a}) \mathrm{Cl}^{-},(\mathbf{b}) \mathrm{Sc}^{3+},(\mathbf{c}) \mathrm{Fe}^{2+},(\mathbf{d}) \mathrm{Zn}^{2+},(\mathbf{e}) \mathrm{Sn}^{4+}\)

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) Ti, Ba; (b) Ag, Cu; (c) Ge, Cl; (d) Pb, Sb.

In Table 7.8 , the bonding atomic radius of neon is listed as 0.58 A, whereas that for xenon is listed as 1.40 A. A classmate of yours states that the value for Xe is more realistic than the one for Ne. Is she correct? If so, what is the basis for her statement?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free