/*! 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 68 \({ }_{92} \mathrm{U}^{235}\) an... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 27: Problem 68

\({ }_{92} \mathrm{U}^{235}\) and \({ }_{92} \mathrm{U}^{238}\) differ as (a) \({ }_{92} \mathrm{U}^{235}\) has 2 protons less (b) \({ }_{92} \mathrm{U}^{238}\) has 3 protons more (c) \({ }_{92} \mathrm{U}^{238}\) has 3 neutrons more (d) None of the above

Short Answer

Expert verified
(c) \({ }_{92} \mathrm{U}^{238}\) has 3 neutrons more

Step by step solution

01

Identify the given isotopes

We have two isotopes of Uranium provided: \({ }_{92} \mathrm{U}^{235}\) and \({ }_{92} \mathrm{U}^{238}\). Both isotopes have the same number of protons because they are isotopes of the same element.
02

Determine the number of protons

For any uranium isotope, the atomic number is 92, which represents the number of protons. Therefore, both \( { }_{92} \mathrm{U}^{235} \) and \( { }_{92} \mathrm{U}^{238} \) have 92 protons.
03

Calculate the number of neutrons

Neutrons are determined by subtracting the number of protons from the mass number. For \( { }_{92} \mathrm{U}^{235} \), neutrons = \( 235 - 92 = 143 \). For \( { }_{92} \mathrm{U}^{238} \), neutrons = \( 238 - 92 = 146 \).
04

Compare the number of neutrons

We find that \( { }_{92} \mathrm{U}^{238} \) has 146 neutrons and \( { }_{92} \mathrm{U}^{235} \) has 143 neutrons. Therefore, \( { }_{92} \mathrm{U}^{238} \) has 3 more neutrons than \( { }_{92} \mathrm{U}^{235} \).

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 Uranium Isotopes
Uranium isotopes such as \( { }_{92} \mathrm{U}^{235} \) and \( { }_{92} \mathrm{U}^{238} \) are variants of the element uranium.These isotopes have the same atomic number but different mass numbers.The atomic number is 92 for uranium, indicating the number of protons, whereas the mass number differs because of the varying number of neutrons.
  • \( { }_{92} \mathrm{U}^{235} \) is known for its use in nuclear reactors and weapons due to its ability to sustain a fission chain reaction.
  • \( { }_{92} \mathrm{U}^{238} \), while plentiful, is not fissile but can be converted into \( { }_{94} \mathrm{Pu}^{239} \), a fissile material.
To understand isotopes more fully, consider them as family members with the same last name (protons) but different middle names (neutrons).
They behave similarly chemically but differ in nuclear properties.
Exploring Atomic Structure and Its Significance
Atomic structure is central to understanding isotopes and elemental behavior in chemistry. Every atom consists of protons, neutrons, and electrons.
  • Protons are positively charged particles located in the atomic nucleus.
  • Neutrons, which have no charge, also reside in the nucleus.
  • Electrons are negatively charged and orbit the nucleus.
The number of protons (atomic number) defines the element鈥檚 identity, while the sum of protons and neutrons (mass number) defines the isotope of the element. For example, in uranium, the atomic number is 92, indicating 92 protons.
The mass number tells us how many total particles are in the nucleus, guiding our understanding of isotopic characteristics.
Neutron Calculation Simplified
Calculating the number of neutrons is straightforward and pivotal for distinguishing between isotopes.Neutrons add to the atomic mass and affect nuclear properties, like stability.
Here's how to calculate the number of neutrons:
  • Identify the mass number, which is the upper number often denoted at the top left of the element symbol.
  • Subtract the atomic number (number of protons) from the mass number.
For instance, for \( { }_{92} \mathrm{U}^{235} \), you subtract 92 from 235, yielding 143 neutrons.And for \( { }_{92} \mathrm{U}^{238} \), subtracting 92 from 238 gives 146 neutrons.
This calculation highlights that \( { }_{92} \mathrm{U}^{238} \) has 3 MORE neutrons than \( { }_{92} \mathrm{U}^{235} \), which is crucial information in identifying isotopic differences clearly.

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

A If Avogadro number is \(6 \times 10^{23}\), then number of protons, neutrons and electrons is \(14 \mathrm{~g}\) of \({ }_{6} \mathrm{C}^{14}\) are respectively (a) \(36 \times 10^{23}, 48 \times 10^{23}, 36 \times 10^{23}\) (b) \(36 \times 10^{23}, 36 \times 10^{23}, 36 \times 10^{23}\) (c) \(48 \times 10^{23}, 36 \times 10^{23}, 48 \times 10^{23}\) (d) \(48 \times 10^{23}, 48 \times 10^{23}, 36 \times 10^{23}\) \(\mathrm{F}\)

\(M_{x}\) and \(M_{y}\) denote the atomic masses of the parent and the daughter nuclei respectively in a radioactive decay. The \(Q\)-value of a \(\beta^{-}\)decay is \(Q_{1}\) and that for a \(\beta^{+}\) decay is \(Q_{2}\). If \(m_{e}\) denotes the mass of an electron, then which of the following statements is correct? [NCERT Exemplar] (a) \(Q_{1}=\left(M_{x}-M_{y}\right) c^{2}\) and \(Q_{2}=\left(M_{x}-M_{y}-2 m_{e}\right) c^{2}\) (b) \(Q_{1}=\left(M_{x}-M_{y}\right) c^{2}\) and \(Q_{2}=\left(M_{x}-M_{y}\right) c^{2}\) (c) \(Q_{1}=\left(M_{x}-M_{y}-2 m_{e}\right) c^{2}\) and \(Q_{2}=\left(M_{x}-M_{y}+2 m_{e}\right) c^{2}\) (d) \(Q_{1}=\left(M_{x}-M_{y}+2 m_{e}\right) c^{2}\) and \(Q_{2}=\left(M_{x}-M_{y}+2 m_{e}\right) c^{2}\)

Two radioactive sources \(A\) and \(B\) of half lives \(1 \mathrm{~h}\) and 2h respectively initially contain the same number of radioactive atoms. At the end of two hours, their rates of disintegration are in the ratio of (a) \(1: 4\) (b) \(1: 3\) (c) \(1: 2\) (d) \(1: 1\)

If in a Thomson's mass spectrograph, the ratio of the electric field and magnetic field, in order to obtain concident parabola of singly ionised and doubly ionised positive ions are \(1: 2\) and \(3: 2\) respectively, then the ratio of masses of particles will be (a) \(3: 1\) (b) \(2: 1\) (c) \(9: 4\) (d) \(9: 2\)

An electron jumps from the 4 th orbit to 2 nd orbit of hydrogen atom. Given the Rydberg's constant \(R=10^{5} \mathrm{~cm}^{-1}\), the frequency in hertz of the emitted radiation will be (a) \(\frac{3}{16} \times 10^{5}\) (b) \(\frac{3}{16} \times 10^{15}\) (c) \(\frac{9}{16} \times 10^{15}\) (d) \(\frac{3}{4} \times 10^{15}\)
See all solutions

Recommended explanations on Physics Textbooks

Engineering Physics

Read Explanation

Kinematics Physics

Read Explanation

Fluids

Read Explanation

Mechanics and Materials

Read Explanation

Measurements

Read Explanation

Modern Physics

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.