Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 14

Under appropriate conditions, both hydrogen and nitrogen can form monatomic anions. What are the Lewis symbols for these ions? What are the Lewis structures of the compounds (a) lithium hydride; (b) calcium hydride; (c) magnesium nitride?

Short Answer

Expert verified
The Lewis symbols for hydrogen and nitrogen ions are \(H^-\) with two dots and \(N^{3-}\) with eight dots respectively. The Lewis structures for \(LiH\) consist of \(Li^+\) with no dots and \(H^-\) with two dots. \(CaH_2\) has \(Ca^{2+}\) with no dots and two \(H^-\) with two dots each. The structure of \(Mg_3N_2\) includes three \(Mg^{2+}\) with no dots and two \(N^{3-}\) each with eight dots.

Step by step solution

01

Lewis Symbols for Hydrogen and Nitrogen Ions

In order to draw the Lewis symbols for hydrogen and nitrogen ions, we need to understand that anions are formed when an atom gains electrons. In its elemental state, hydrogen has 1 electron. When it gains an electron, it forms a monatomic anion and its Lewis symbol will be \(H^-\) with two dots around it representing the two valence electrons. Nitrogen, having 5 valence electrons, needs to gain 3 more electrons to fulfill the octet rule, forming \(N^{3-}\). The Lewis symbol will therefore be \(N^{3-}\) surrounded by eight dots symbolizing the eight valence electrons.
02

Lewis Structure for Lithium Hydride

Lithium hydride (\(LiH\)) is composed of lithium ions (\(Li^+\)) and hydride ions (\(H^-\)). Lithium loses one electron to form \(Li^+\) and hydrogen gains one electron to form \(H^-\). The lewis structure will therefore include Lithium with no dots (since it loses the electron it initially had) and hydride with two dots (since it gains an additional electron).
03

Lewis Structure for Calcium Hydride

Calcium hydride (\(CaH_2\)) is formed when calcium ions (\(Ca^{2+}\)) bonds with two hydride ions (\(2H^-\)). Calcium loses two electrons and each hydride gains one electron. In the Lewis structure, calcium will be shown without any dots (since it loses 2 valence electrons) and each hydride will have two dots around them.
04

Lewis Structure for Magnesium Nitride

Magnesium nitride (\(Mg_3N_2\)) consists of magnesium ions (\(Mg^{2+}\)) and nitride ions (\(N^{3-}\)). In this compound, three magnesium atoms each lose two electrons and two nitrogen atoms each gain three electrons to follow the octet rule. The Lewis structure will involve three magnesium ions with no dots and two nitride ions surrounded by eight dots each.

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

The following statements are not made as carefully as they might be. Criticize each one. (a) Lewis structures with formal charges are incorrect. (b) Triatomic molecules have a planar shape. (c) Molecules in which there is an electronegativity difference between the bonded atoms are polar.

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) \(\mathrm{Al}(\mathrm{OH})_{3}\); (c) \(\mathrm{NH}_{4} \mathrm{F}\); (d) \(\mathrm{KClO}_{3}\); (b) \(\mathrm{Ca}(\mathrm{CN})_{2}\); (e) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\).

Explain the important distinctions between (a) ionic and covalent bonds; (b) lone-pair and bond-pair electrons; (c) molecular geometry and electron-group geometry; (d) bond dipole and resultant dipole moment; (e) polar molecule and nonpolar molecule.

One of the following ions has a trigonal-planar shape: $\mathrm{SO}_{3}^{2-} ; \mathrm{PO}_{4}^{3-} ; \mathrm{PF}_{6}^{-} ; \mathrm{CO}_{3}^{2-} .$ Which ion is it? Explain.

Of the following species, the one with a triple covalent bond is (a) \(\mathrm{NO}_{3}^{-} ;\) (b) \(\mathrm{CN}^{-} ;\) (c) \(\mathrm{CO}_{2} ;\) (d) \(\mathrm{AlCl}_{3}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Physical 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