Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 96

One isotope of a nonmetallic element has mass number 77 and 43 neutrons in the nucleus. The anion derived from the isotope has 36 electrons. Write the symbol for this anion.

Short Answer

Expert verified
The symbol for the anion is \(Se^{2-}\)

Step by step solution

01

Calculate the Number of Protons

Subtract the number of neutrons from the mass number to find the number of protons. Here, that would be \(77 - 43 = 34\). This is the atomic number of the element.
02

Identify the Element

Refer to the periodic table, and look for the element that has an atomic number 34. That element is Selenium (Se).
03

Determine the Charge of the Ion

Since the ion has two more electrons (36) than protons (34), it carries a charge of -2.
04

Write the Symbol for the Ion

We write the symbol for the element, followed by the charge of the ion in superscript. Here, it will be \(Se^{2-}\).

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

Calculate the number of neutrons in \({ }^{239} \mathrm{Pu}\).

Write the names and symbols for four elements in each of the following categories: (a) nonmetal, (b) metal, (c) metalloid.

In Section 2.1 it was pointed out that mass and energy are alternate aspects of a single entity called mass-energy. The relationship between these two physical quantities is Einstein's famous equation, \(E=m c^{2},\) where \(E\) is energy, \(m\) is mass, and \(c\) is the speed of light. In a combustion experiment, it was found that \(12.096 \mathrm{~g}\) of hydrogen molecules combined with \(96.000 \mathrm{~g}\) of oxygen molecules to form water and released \(1.715 \times 10^{3} \mathrm{~kJ}\) of heat. Calculate the corresponding mass change in this process and comment on whether the law of conservation of mass holds for ordinary chemical processes. (Hint: The Einstein equation can be used to calculate the change in mass as a result of the change in energy. \(1 \mathrm{~J}=1 \mathrm{~kg} \mathrm{~m}^{2} / \mathrm{s}^{2}\) and \(\left.c=3.00 \times 10^{8} \mathrm{~m} / \mathrm{s} .\right)\)

The following phosphorus sulfides are known: \(\mathrm{P}_{4} \mathrm{~S}_{3}\) \(\mathrm{P}_{4} \mathrm{~S}_{7},\) and \(\mathrm{P}_{4} \mathrm{~S}_{10} .\) Do these compounds obey the law of multiple proportions?

Write the appropriate symbol for each of the following isotopes: (a) \(Z=11, A=23\) (b) \(Z=28, A=64\).
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

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