/*! 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 31 Name the three subatomic particl... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 31

Name the three subatomic particles found in an atom and give their relative masses and charges.

Short Answer

Expert verified
The three subatomic particles found in an atom are protons, neutrons, and electrons. Protons have a relative mass of 1 amu and a charge of +1. Neutrons have a relative mass of 1 amu and no charge (charge of 0). Electrons have a relative mass of about 1/1836 amu (approximated to 0 amu) and a charge of -1.

Step by step solution

01

Protons

Protons are positively charged subatomic particles found in the nucleus of an atom. They have a relative mass of 1 atomic mass unit (amu) and a charge of +1.
02

Neutrons

Neutrons are neutral subatomic particles, which means they don't have a charge. They are also located in the nucleus of an atom. Neutrons have a relative mass of 1 amu, similar to protons, but their electric charge is 0.
03

Electrons

Electrons are negatively charged subatomic particles that orbit the nucleus of an atom in various energy levels. The relative mass of an electron is significantly smaller than that of protons and neutrons, approximately 1/1836 amu, which is often approximated to 0 amu in some calculations. Electrons have a charge of -1.
04

Summary

The three subatomic particles found in an atom are protons, neutrons, and electrons. Protons have a relative mass of 1 amu and a charge of +1, neutrons have a relative mass of 1 amu and no charge (charge of 0), and electrons have a relative mass of about 1/1836 amu (approximated to 0 amu) and a charge of -1.

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.

Protons
Protons are one of the three main types of subatomic particles that compose the atomic structure. They reside within the nucleus, the core of an atom. With a positive charge of +1, they play a vital role in defining the identity of an atom. Each element on the periodic table is distinguished by its unique number of protons, also known as its atomic number. Protons have a significant mass, approximately 1 atomic mass unit (amu), making them about 1836 times heavier than electrons. Protons and neutrons collectively contribute to most of an atom's mass. Given their positive charge and mass, they significantly influence the behavior of atoms in chemical reactions.
Neutrons
Neutrons are neutral subatomic particles, found alongside protons in the nucleus of an atom. They carry no electric charge, expressed as 0, and this neutrality helps stabilize the nucleus, especially in heavier atoms where the presence of multiple protons would otherwise cause intense repulsive forces. Neutrons also have a mass close to 1 amu. When it comes to determining the atomic mass or isotopes of an element, neutrons play a crucial role. Isotopes are variants of elements that have the same number of protons but different numbers of neutrons, resulting in various atomic masses but identical chemical properties.
Electrons
Electrons are the lightest and smallest of the subatomic particles, orbiting around the nucleus within regions called electron shells or energy levels. Their negative charge of -1 balances the positive charge of the protons in the nucleus, leading to electrically neutral atoms under normal circumstances. Electrons are incredibly dynamic and are fundamental to chemical bonding and electricity. Their relative mass is around 1/1836 amu, which is why, in some calculations, their mass contribution is approximated to 0 amu, focusing on the mass from protons and neutrons.
Atomic Mass Unit
The atomic mass unit (amu) is a standard unit of mass that quantifies the mass of subatomic particles. By definition, 1 amu is 1/12th the mass of a carbon-12 atom. This scale provides a convenient way to express the masses of protons, neutrons, and electrons in a way that reflects their actual weight differences. The use of amu makes it possible to compare the masses of different atoms and isotopes, which is essential for understanding atomic structure and the behavior of elements in various chemical processes.
Atomic Structure
Understanding atomic structure is fundamental to grasping the nature of matter. At its core, an atom consists of a nucleus containing protons and neutrons, surrounded by a cloud of electrons in various orbits. The behavior and characteristics of an element depend heavily on its atomic structure, including the arrangement and number of each subatomic particle. The atomic structure not only defines the identity of elements, their isotopes, and the charting of the periodic table, but it also underpins the intricacies of chemical reactions, bonding, and the physical properties of substances.

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

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$

Although not discussed until the next chapter, what process do you think chemists mean by an atom's second ionization energy?

A student claims that isotopes of the same element have the same number of electrons and protons. Is she correct? Justify your answer.

Write the full atomic symbol for the only atom that has its mass number equal to its atomic number.

Suppose \(12.0 \mathrm{~g}\) of silicon (Si) reacts with \(70.0 \mathrm{~g}\) of oxygen \(\left(\mathrm{O}_{2}\right)\) to give \(25.6 \mathrm{~g}\) of the compound silicon dioxide \(\left(\mathrm{SiO}_{2}\right) .\) In the process, all the silicon gets used up, but some oxygen is left over. (a) For the law of conservation of matter to be obeyed, how much oxygen is unused? (b) What is the percent \(\mathrm{Si}\) in \(\mathrm{SiO}_{2} ?\) (c) What is the percent \(\mathrm{O}\) in \(\mathrm{SiO}_{2}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemical Analysis

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.