/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 60 Challenge For a \(\mathrm{NH}_{4... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 60

Challenge For a \(\mathrm{NH}_{4}^{+}\) ion, identify its molecular shape, bond angle, and hybrid orbitals.

Short Answer

Expert verified
The \(\mathrm{NH}_{4}^{+}\) ion has a tetrahedral shape, \(109.5^\circ\) bond angle, and \(sp^3\) hybrid orbitals.

Step by step solution

01

Identify the central atom and its valence electrons

The central atom in the ammonium ion, \(\mathrm{NH}_{4}^{+}\), is nitrogen (N). Nitrogen typically has 5 valence electrons. However, in \(\mathrm{NH}_{4}^{+}\), nitrogen shares electrons with four hydrogen atoms.
02

Determine the charge and adjust electron count

Since \(\mathrm{NH}_{4}^{+}\) has a positive charge, this indicates the loss of one electron from the total valence electrons. Without this charge, there would be 5 (from N) + 1x4 (from each H) = 9 electrons, but we lose one due to the \(1^+\) charge.
03

Use VSEPR theory to determine shape

According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, \(\mathrm{NH}_{4}^{+}\) has four bonding pairs and no lone pairs. This leads to a tetrahedral shape.
04

Determine bond angles

A tetrahedral molecular shape features bond angles of \(109.5^\circ\). Consequently, the \(\mathrm{H-N-H}\) bond angles in \(\mathrm{NH}_{4}^{+}\) are \(109.5^\circ\).
05

Identify hybridization

The sp3 hybridization occurs when one s orbital and three p orbitals combine, which is found in the \(\mathrm{NH}_{4}^{+}\) ion due to the four equivalent \(\mathrm{N-H}\) bonds, indicating \(sp^3\) hybrid orbitals.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Understanding Molecular Shape
Molecular shape refers to the 3D arrangement of atoms in a molecule. This arrangement is primarily influenced by the electron pair repulsion as explained by the VSEPR theory. For the ammonium ion, \(\mathrm{NH}_{4}^{+}\), the molecular shape is tetrahedral. This shape arises because four hydrogen atoms are symmetrically positioned around the nitrogen central atom. Each hydrogen atom connects to the nitrogen atom through a covalent bond.

The VSEPR theory suggests that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion. In the case of \(\mathrm{NH}_{4}^{+}\), the absence of lone pairs means only bond pairs are considered.
  • This symmetrical distribution results in a geometric arrangement referred to as tetrahedral.
  • This shape is common whenever a central atom forms four bonds.
Evaluating Bond Angles
Bond angles are crucial in determining the geometry of a molecule. In the tetrahedral shape of \(\mathrm{NH}_{4}^{+}\), the bond angles are found to be \(109.5^\circ\). This specific angle is a result of the symmetrical distribution of the hydrogen atoms around the nitrogen.

To understand why \(109.5^\circ\) is the bond angle in a tetrahedral shape:
  • Imagine the hydrogen atoms spread out in 3D space, trying to stay as far from each other as possible, according to VSEPR theory.
  • This results in equal bond angles, each exactly \(109.5^\circ\) apart from each other.
Such a configuration helps reduce electron pair repulsion, stabilizing the overall structure of the molecule.
Exploring sp3 Hybridization
Hybridization is a concept where atomic orbitals mix to form new hybrid orbitals, which influences bond formation. In \(\mathrm{NH}_{4}^{+}\), the nitrogen atom undergoes \(sp^3\) hybridization.

To break it down:
  • Nitrogen starts with one s orbital and three p orbitals.
  • These orbitals mix to form four equivalent \(sp^3\) hybrid orbitals.
Each \(sp^3\) orbital forms a covalent bond with a hydrogen atom, allowing for the four hydrogen atoms to evenly distribute around nitrogen in a tetrahedral arrangement.

The \(sp^3\) hybridization explains why the bonds in \(\mathrm{NH}_{4}^{+}\) are identical and contribute to the integrity of its tetrahedral shape.

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

Challenge What is the formula for periodic acid?

Draw the Lewis structures for the molecules \(S F_{4}\) and \(S F_{6} .\) Analyze each structure to determine whether the molecule is polar or nonpolar.

Generalize Describe the general characteristics of covalent network solids.

Define the term bond angle

Draw the Lewis structure for BH \(_{3}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

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.