Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 152

Predict the formula for lithium nitride, made from lithium, \(\mathrm{Li}\), and nitrogen, \(\mathrm{N}\). Explain your reasoning.

Short Answer

Expert verified
The formula for lithium nitride is \(\text{Li}_3\text{N}\). This is because lithium forms a +1 ion and nitrogen forms a -3 ion. To create a neutral compound, we need three lithium ions to balance the charge of one nitrogen ion. This results in the formula \(\text{Li}_3\text{N}\).

Step by step solution

01

Determine the charges of the ions

Lithium, as an alkali metal, tends to lose its single valence electron to form a positive ion with a charge of +1. Following the formula: \(\text{Charge of Lithium ion} = +1\) Nitrogen, on the other hand, tends to gain 3 more electrons to complete its outer electron shell, forming a negative ion with a charge of -3. Using the formula: \(\text{Charge of Nitrogen ion} = -3\)
02

Combine the ions to form a neutral compound

Now, we have the charges of each ion, we need to combine them in a ratio that results in a neutral compound. In this case, we can balance the charges by using 3 lithium ions and 1 nitrogen ion, as the total charge will be 0 in this ratio. \((\text{Charge of Lithium ion} \times 3) + (\text{Charge of Nitrogen ion} \times 1) = 0\) \((+1 \times 3) + (-3 \times 1) = 0\) \((+3) + (-3) = 0\)
03

Write the formula for lithium nitride

Having found the ratio of the ions needed for a neutral charge (3 lithium ions to 1 nitrogen ion), we can write the formula for lithium nitride: \[\text{Li}_3\text{N}\] Thus, the formula for lithium nitride, made from lithium (Li) and nitrogen (N), is \(\text{Li}_3\text{N}\), with the reasoning based on achieving a neutral charge in the compound by combining the ions in a specific ratio.

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

Of the atoms \(\mathrm{Na}, \mathrm{Cl}, \mathrm{K}, \mathrm{Br}\), which has the largest atomic radius? Which has the largest first ionization energy?

Draw a simple Bohr model (no subshells) for an oxygen atom. How many electrons are in the valence shell? How many more electrons can be put into the valence shell?

Order the following atoms from smallest to largest, judging from their relative positions in the periodic table: \(\mathrm{Cs}, \mathrm{Fe}, \mathrm{Ti}, \mathrm{Hf}\)

Which subshell has the lowest energy? (a) \(4 s\) (b) \(3 p\) (c) \(2 p\) (d) \(3 s\) (e) \(2 s\)

What is the octet rule, and what is the justification behind it?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

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