/*! 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 22 Determine whether each of the fo... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 2: Problem 22

Determine whether each of the following statements is true or false. If false, correct the statement to make it true: \((\mathbf{a})\) The nucleus has most of the mass and comprises most of the volume of an atom. (b) Every atom of a given element has the same number of protons. (c) The number of electrons in an atom equals the number of neutrons in the atom. (d) The protons in the nucleus of the helium atom are held together by a force called the strong nuclear force.

Short Answer

Expert verified
(a) False - mass not volume; (b) True; (c) False - electrons equal protons; (d) True.

Step by step solution

01

Assess the Nucleus

Statement (a): The nucleus is the center of the atom and contains protons and neutrons. It holds most of the atom's mass due to the mass of protons and neutrons but occupies a very small volume compared to the entire atom. Thus, the statement is false. Correction: The nucleus has most of the mass but occupies a very small volume of an atom.
02

Evaluate Proton Count Consistency

Statement (b): The number of protons in an atom defines the element, and each atom of a given element has the same number of protons. Therefore, this statement is true.
03

Compare Electron and Neutron Numbers

Statement (c): The number of electrons in a neutral atom equals the number of protons, not neutrons. The number of neutrons can vary within isotopes of the same element. Thus, the statement is false. Correction: The number of electrons in a neutral atom equals the number of protons in the atom.
04

Understand Nuclear Forces

Statement (d): Protons in the nucleus are positively charged and repel each other, but they are held together by the strong nuclear force, which is accurate for helium and all atomic nuclei. Thus, this statement is true.

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.

Nucleus
The nucleus is the central part of an atom and can be thought of as the atom's core. Although it contains most of the atom's mass, it takes up only a small fraction of the atom's volume. This is because the nucleus is densely packed with protons and neutrons, the two subatomic particles that are much heavier than electrons.
Electrons orbit the nucleus and account for the vast majority of an atom's volume. This contrast between mass and volume makes the nucleus quite exceptional. In summary, when we talk about the nucleus:
  • It houses protons and neutrons.
  • It holds most of the atom's mass.
  • It occupies a very small volume compared to the entire atom.
Protons
Protons are positively charged particles found within the nucleus. They play a crucial role in defining an atom's identity. Each element is characterized by a unique number of protons, known as its atomic number. This means that every atom of a specific element has the same number of protons.
For instance, all hydrogen atoms have exactly one proton, while all carbon atoms have six. This consistency is why the number of protons is often referred to as the fingerprint of an element. Therefore, keep in mind:
  • Protons have a positive charge.
  • They determine the identity of an element.
  • The atomic number equals the number of protons.
Neutrons
Neutrons are neutral particles found in the nucleus alongside protons. They do not carry any charge, which is why they are called 'neutrons.' However, they play an essential role in stabilizing the nucleus despite not affecting an element's identity.
Atoms of the same element can have different numbers of neutrons, leading to variations known as isotopes. For example, carbon-12 and carbon-14 are isotopes of carbon with six and eight neutrons, respectively. When learning about neutrons, remember:
  • Neutrons have no charge (neutral).
  • They help stabilize the nucleus.
  • Isotopes are atoms with the same number of protons but different numbers of neutrons.
Strong Nuclear Force
The strong nuclear force is the powerful force that holds protons together in the nucleus. Protons are all positively charged, and like charges repel each other. Without the strong nuclear force, this repulsion would cause the nucleus to fly apart.
This force acts over very short distances within the nucleus, making it much stronger than the repulsive electromagnetic force between protons. Thus, it effectively binds protons (and neutrons) together, maintaining the integrity of the nucleus. Key points about the strong nuclear force include:
  • It's the most powerful force over short distances.
  • It binds protons and neutrons in the nucleus.
  • It overcomes the proton-proton repulsive force.

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

Name the following ionic compounds: \((\mathbf{a}) \mathrm{KCN},(\mathbf{b}) \mathrm{NaBrO}_{2},\) (c) \(\mathrm{Sr}(\mathrm{OH})_{2}\), (d) CoTe, (e) \(\mathrm{Fe}_{2}\left(\mathrm{CO}_{3}\right)_{3},\), (f) \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}\), (h) \(\mathrm{NaH}_{2} \mathrm{PO}_{4}\), (i) \(\mathrm{KMnO}_{4}\), (g) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{3},\), , (j) \(\mathrm{Ag}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\).

Consider an atom of \({ }^{58} \mathrm{Ni}\). (a) How many protons, neutrons, and electrons does this atom contain? (b) What is the symbol of the ion obtained by removing two electrons from \({ }^{58} \mathrm{Ni}\) ? (c) What is the symbol for the isotope of \({ }^{58} \mathrm{Ni}\) that possesses 33 neutrons?

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: $$ \begin{array}{lcc} \hline \text { Compound } & \text { Mass of Iodine (g) } & \text { Mass of Fluorine (g) } \\ \hline 1 & 4.75 & 3.56 \\ \hline 2 & 7.64 & 3.43 \\ 3 & 9.41 & 9.86 \\ \hline \end{array} $$ (a) Calculate the mass of fluorine per gram of iodine in each compound. (b) How do the numbers in part (a) support the atomic theorv?

Give the chemical names of each of the following familiar compounds: \((\mathbf{a}) \mathrm{NaCl}(\) table salt \(),(\mathbf{b}) \mathrm{NaHCO}_{3}(\) baking soda \()\) (c) \(\mathrm{NaOCl}\) (in many bleaches), (d) \(\mathrm{NaOH}\) (caustic soda), (e) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\) (smelling salts), \(,(\mathbf{f}) \mathrm{CaSO}_{4}\) (plaster of Paris).

Fill in the gaps in the following table, assuming each column represents a neutral atom. $$ \begin{array}{l|l|l|l|l|l} \hline \text { Symbol } & { }^{89} \mathrm{Y} & & & & \\ \text { Protons } & & 78 & & & 89 \\ \text { Neutrons } & & & 123 & & \\ \text { Electrons } & & & 81 & 50 & \\ \text { Mass no. } & & 195 & & 119 & 227 \\ \hline \end{array} $$
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

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.