Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 80

A monatomic ion has a charge of +2 . The nucleus of the parent atom has a mass number of \(55 .\) If the number of neutrons in the nucleus is 1.2 times that of the number of protons, what is the name and symbol of the element?

Short Answer

Expert verified
The element is Iodine, with the symbol 'I'

Step by step solution

01

Determine the number of protons

First, it is crucial to know that the charge of a monatomic ion represents the difference between the number of protons and electrons. Since this ion has a charge of +2, it means that there are two more protons than electrons. Hence, the number of protons should be the atomic number in a neutral atom (protons = electrons). This information allows the calculation of the atomic (proton) number as \(A = Z + 2\), with A as the given mass number and Z as the atomic number that we want to determine. Substituting the given A value: \(55 = Z + 2 \rightarrow Z = 55 - 2 = 53\).
02

Verification of the atomic structure

Having determined Z, we now verify the given atomic structure in terms of the number of neutrons. The exercise stated that the number of neutrons is 1.2 times that of the number of protons. Taking Z = 53, the number of neutrons would then be \(1.2 * 53 = 63.6\). Since the number of neutrons must be a whole number, it is reasonable to consider 64 as the rounded-off number of neutrons. The sum of Z and the number of neutrons should be equal to the mass number \(A = 55\), which is inconsistent with the calculated number of neutrons, implying an error or approximation. Therefore, the provided atomic structure does not match with the calculated number of protons and neutrons.
03

Identify the element

The element can be identified using the determined atomic number (Z = 53). Elements are uniquely defined by their atomic number, i.e., their number of protons. Looking up Z = 53 in a periodic table, one finds the element Iodine, symbol 'I'.

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

Define molecular formula and empirical formula. What are the similarities and differences between the empirical formula and molecular formula of a compound?

Elements whose names end with "-ium" are usually metals; sodium is one example. Identify a nonmetal whose name also ends with "-ium."

List the types of radiation that are known to be emitted by radioactive elements.

Roughly speaking, the radius of an atom is about 10,000 times greater than that of its nucleus. If an atom were magnified so that the radius of its nucleus became \(10 \mathrm{~cm},\) what would be the radius of the atom in miles? \((1 \mathrm{mi}=1609 \mathrm{~m} .)\)

A sample of a radioactive element is found to be losing mass gradually. Explain what is happening to the sample.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

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