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Chapter 2: Problem 79

(a) What are the charges of an electron, a proton, and a neutron? (b) What are the masses (in amu, to one significant figure) of an electron, a proton, and a neutron?

Short Answer

Expert verified
(a) Electron: -1, Proton: +1, Neutron: 0. (b) Electron: 0 amu, Proton: 1 amu, Neutron: 1 amu.

Step by step solution

01

Identify the charge of an electron

An electron has a negative electrical charge. The charge of an electron is commonly expressed as \[-1 \text{ e} = -1.6 \times 10^{-19} \,\text{C}\].
02

Identify the charge of a proton

A proton has a positive electrical charge. The charge of a proton is commonly expressed as \[+1 \text{ e} = +1.6 \times 10^{-19} \,\text{C}\].
03

Identify the charge of a neutron

A neutron has no electrical charge, or it is neutral. Hence, its charge is \[0 \text{ e} = 0 \,\text{C}\].
04

Identify the mass of an electron

The mass of an electron is approximately \[0.0005 \text{ amu}\], which when rounded to one significant figure, can be approximated to \[0.001 = 0 \text{ amu}\].
05

Identify the mass of a proton

The mass of a proton is approximately \[1.007 \text{ amu}\], which when rounded to one significant figure, is \[1 \text{ amu}\].
06

Identify the mass of a neutron

The mass of a neutron is approximately \[1.008 \text{ amu}\], which when rounded to one significant figure, is \[1 \text{ amu}\].

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Charge
Electrons are fundamental subatomic particles with a specific electrical charge. They are a key component of atoms and play a vital role in chemical reactions and electricity. Electrons carry a negative charge which is exactly equal and opposite to that of a proton, making it
  • -1 ext{ e}, which is the elementary charge unit.
  • In terms of coulombs, this charge is precisely \[-1.6 \times 10^{-19} \text{ C}\].
Because electrons are negatively charged, they are attracted to the positively charged protons in the nucleus of an atom. This attraction helps hold the atom together, giving it stability. Understanding this negative charge characteristic is crucial as it allows electrons to move, which is the basis for electricity conduction.
Proton Mass
Protons are another fundamental component of atoms, known for their positive electrical charge. But apart from their charge, their mass is a critical feature that contributes to an atom's overall mass. Protons possess a mass that is significantly greater than that of electrons,
  • The mass of a proton is approximately \[1.007 \text{ amu}\]
  • For simplicity, this is often expressed as \[1 \text{ amu}\] rounding to one significant figure.
In the atomic nucleus, protons, along with neutrons, contribute almost all of an atom's mass. Their positive charge exactly balances the negative charge of electrons, resulting in neutral atoms when the numbers of protons and electrons are equal. This delicate balance between charges ensures the stability of the atom's structure.
Neutron Properties
Neutrons play a crucial role in the atomic nucleus due to their neutral charge. They neither possess a positive nor a negative charge,
  • Neutrons have a charge of \[0 ext{ e} = 0 \text{ C}\], meaning they are neutral.
  • Despite their neutral charge, their mass is similar to that of a proton, \[1.008 \text{ amu}\],
  • which simplifies to \[1 \text{ amu}\] when rounded.
This neutrality allows neutrons to act as a buffer between the repulsive forces of protons in the nucleus. Without neutrons, protons would repel each other due to their like charges, potentially destabilizing the atom. Neutrons, therefore, provide a balancing force, essential for the cohesion of the atomic nucleus.

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Most popular questions from this chapter

Answer true or false. (a) To say that "energy is quantized" means that only certain energy values are allowed. (b) Bohr discovered that the energy of an electron in an atom is quantized. (c) Electrons in atoms are confined to regions of space called "principal energy levels." (d) Each principal energy level can hold a maximum of two electrons. (e) An electron in a 1 s orbital is held closer to the nucleus than an electron in a \(2 s\) orbital. (f) An electron in a 2s orbital is harder to remove from an atom than an electron in a 1 s orbital. (g) An sorbital has the shape of a sphere, with the nucleus at the center of the sphere. (h) Each \(2 p\) orbital has the shape of a dumbbell, with the nucleus at the midpoint of the dumbbell. (i) The three \(2 p\) orbitals in an atom are aligned parallel to each other. (j) An orbital is a region of space that can hold two electrons. (k) The second shell contains one \(s\) orbital and three \(p\) orbitals. (1) In the ground-state electron configuration of an atom, only the lowest- energy orbitals are occupied. \((\mathrm{m}) \mathrm{A}\) spinning electron behaves as a tiny bar magnet, with a North Pole and a South Pole. (n) An orbital can hold a maximum of two electrons with their spins paired. (o) Paired electron spins means that the two electrons are aligned with their spins North Pole to North Pole and South Pole to South Pole. (p) \(A n\) orbital box diagram puts all of the electrons of an atom in one box with their spins aligned. (q) An orbital box diagram of a carbon atom shows two unpaired electrons. (r) A Lewis dot structure shows only the electrons in the valence shell of an atom of the element. (s) A characteristic of Group 1A elements is that each has one unpaired electron in its outermost occupied (valence) shell. (t) A characteristic of Group 6A elements is that each has six unpaired electrons in its valence shell.

There are only two naturally occurring isotopes of antimony: \(^{121} \mathrm{Sb}(120.90 \mathrm{amu})\) and \(^{123} \mathrm{Sb}(122.90 \mathrm{amu})\) The atomic weight of antimony given in the Periodic Table is \(121.75 .\) Which of the two isotopes has the greater natural abundance?

(Chemical Connections \(2 \mathrm{B}\) ) Which are the two most abundant elements, by weight, in: (a) the Earth's crust? (b) the human body?

Answer true or false. (a) Matter is divided into elements and pure substances. (b) Matter is anything that has mass and volume (occupies space). (c) A mixture is composed of two or more pure substances. (d) An element is a pure substance. (e) A heterogeneous mixture can be separated into pure substances, but a homogeneous mixture cannot. (f) \(\quad\) A compound consists of elements combined in a fixed ratio. (g) A compound is a pure substance. (h) All matter has mass. (i) All of the 118 known elements occur naturally on Earth. (j) The first six elements in the Periodic Table are the most important for human life. (k) The combining ratio of a compound tells you how many atoms of each element are combined in the compound. (1) The combining ratio of 1: 2 in the compound \(\mathrm{CO}_{2}\) tells you that this compound is formed by the combination of one gram of carbon with two prams of oxygen.

Other isotopes used in PET imaging are fluorine- 18 nitrogen-13, and oxygen-15. None of these isotopes occurs in nature; all must be produced in the laboratory. Give the number of protons, neutrons, and electrons in an atom of each of these artificial isotopes.
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