Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 121

How do metals and nonmetals differ with regard to their tendency to gain or lose electrons? With their tendency to form cations or anions?

Short Answer

Expert verified
Metals, typically found on the left side of the periodic table, tend to lose valence electrons to achieve a stable electron configuration, forming positively charged cations (e.g., Na+). Nonmetals, usually found on the right side of the periodic table, gain valence electrons and form negatively charged anions (e.g., Cl-) to achieve stability. This difference in tendencies to gain or lose electrons is due to the elements' electron configurations and positions in the periodic table.

Step by step solution

01

1. Understanding Metals and Nonmetals

First, let's understand the basic difference between metals and nonmetals. Most elements in the periodic table are either metals or nonmetals based on their physical and chemical properties. Metals are generally shiny, malleable, and good conductors of heat and electricity, while nonmetals usually have low conductivity and are not as shiny or malleable.
02

2. Electron Configuration and Reactivity

The key factor in determining the reactivity of an element and its tendency to gain or lose electrons lies in its electron configuration. Elements in the periodic table aim to achieve a stable electron configuration, usually by having filled valence electron shells.
03

3. Tendency of Metals to Lose Electrons

Metals, which are generally found on the left side of the periodic table, have fewer valence electrons (usually 1 to 3) in their outermost shell. To achieve a stable configuration, they tend to lose these valence electrons, resulting in a positive charge. This process is called ionization.
04

4. Tendency of Nonmetals to Gain Electrons

Nonmetals, on the other hand, are generally found on the right side of the periodic table and have more valence electrons (usually 5 to 7) in their outermost shell. To achieve a stable configuration, they tend to gain more electrons in their outermost shell, resulting in a negative charge. This process is called electron affinity.
05

5. Formation of Cations and Anions

\(\newline\)Metals, after losing their valence electrons, form positively charged ions called cations. For example, a sodium atom (Na) with one valence electron would lose its electron to form a sodium cation (Na+). On the other hand, nonmetals, after gaining electrons in their outermost shell, form negatively charged ions called anions. For example, a chlorine atom (Cl) with seven valence electrons would gain one electron to form a chloride anion (Cl-).
06

6. Conclusion

To summarize, metals and nonmetals differ in their tendencies to gain or lose electrons based on their electron configuration and position in the periodic table. Metals tend to lose electrons and form cations, while nonmetals tend to gain electrons and form anions.

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

How much more massive is an "average" oxygen atom than \(\mathrm{a}_{6}^{12} \mathrm{C}\) atom? (Use the periodic table for the atomic mass of oxygen.)

While an atom's mass number and its atomic mass are not the same, they are often quite close to one another. Consider the following: Uranium- 235 has an atomic mass of \(235.04393\) amu and a percent abundance of \(0.73 \%\). Uranium-238 has an atomic mass of \(238.0508\) amu and a percent abundance of \(99.27 \%\). Without doing any calculations or consulting any other sources, which of the following do you think represents the atomic mass of naturally occurring uranium? (a) \(234.04 \mathrm{amu}\) (b) \(236.03 \mathrm{amu}\) (c) \(237.03\) amu (d) \(238.03\) amu (e) \(238.07\) amu Explain how you made your choice.

A student says that the easiest way to convert a neutral sodium atom to a \(\mathrm{Na}^{+}\) cation is to add a proton to its nucleus. She reasons that this is \(\mathrm{so}\) because protons have a \(1+\) charge. What is wrong with her argument? What does a neutral Na atom become when a proton is added to its nucleus?

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$

How many electrons are there in \(\mathrm{Zr}^{4+}\) ? What \(2+\) cation has the same number of electrons as \(\mathrm{Zr}^{4+} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

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