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Chapter 4: Problem 21

Is each of the following statements true or false? a. A proton and an electron have opposite charges. b. The nucleus contains most of the mass of an atom. c. Electrons repel each other. d. A proton is attracted to a neutron.

Short Answer

Expert verified
a. True, b. True, c. True, d. False

Step by step solution

01

Evaluating Statement a

A proton has a positive charge, and an electron has a negative charge. Since their charges are opposite, this statement is true.
02

Evaluating Statement b

The nucleus of an atom contains protons and neutrons, which are much heavier than electrons. Therefore, the nucleus contains most of the mass of an atom. This means the statement is true.
03

Evaluating Statement c

Electrons are negatively charged particles, and like charges repel each other according to Coulomb's Law. Therefore, electrons repel each other. This statement is true.
04

Evaluating Statement d

A proton is positively charged and a neutron is neutral, meaning it has no charge. There is no attractive force between a proton and a neutron based purely on charge. Thus, this statement is false.

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Key Concepts

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

Proton and Electron Charges
In an atom, protons and electrons exhibit opposite charges. A proton carries a positive charge, denoted as \(+1\) or simply \(+\). On the other hand, an electron has a negative charge, symbolized as \(-1\) or just \(-\). Because their charges are opposite, they naturally attract each other according to Coulomb's Law. This attraction is fundamental in holding the electrons in the vicinity of the atomic nucleus, creating a balanced and stable atom.

Understanding the basics of these charges is essential to grasp how atomic and subatomic particles interact. Opposition in charges leads to attraction, maintaining the structure of atoms and influencing numerous chemical properties.
Atomic Nucleus
The nucleus is the dense core at the center of an atom. It comprises protons and neutrons, collectively known as nucleons. The proton-neutron composition makes the nucleus incredibly heavy compared to the distribution of electrons around it. Since neutrons and protons have significant mass and electrons are much lighter, the nucleus accounts for almost all the atom's mass.

This concentration of mass plays a crucial role in the atom's stability. The understanding of the nucleus's role within the atom further elucidates its impact on the diverse behavior and properties of elements in nature.
Electron Repulsion
Electrons, each possessing a negative charge, repel each other due to Coulomb's Law which states that like charges repel. This repulsion governs their spatial distribution around the nucleus. Electrons form specific energy levels or shells where the force of repulsion arranges them at maximum distances from one another within those limits. This principle shapes the atom's electron configuration, crucial for determining bonding behavior and reactivity.
This repulsive force impacts the arrangement and chemical bonding of atoms. Understanding electron repulsion helps make sense of the periodic table, chemical reactions, and molecular structures.
Proton-Neutron Interaction
Within the nucleus, protons and neutrons experience different forces than the ones influencing electrons. A proton, being positively charged, and a neutron, being neutral, do not attract or repel each other based on electrical charge. Nevertheless, the interaction between them is stabilized by the strong nuclear force鈥攁 fundamental force in physics holding nucleons together to counteract the repulsive force between like-charged protons.
The strong nuclear force is essential for nuclear stability, binding protons and neutrons tightly within the nucleus, preventing disintegration and allowing stable forms of matter to exist.

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Most popular questions from this chapter

Consider the following atoms in which \(\mathrm{X}\) represents the chemical symbol of the element: \((4.4,4.5)\) \({ }_{11}^{22} \mathrm{X},{ }_{10}^{22} \mathrm{X},{ }_{10}^{19} \mathrm{X},{ }_{92}^{238} \mathrm{X},{ }_{92}^{236} \mathrm{X}\) a. Which atoms have the same number of protons? b. Which atoms are isotopes? Of what element? c. Which atoms have the same mass number?

The most prevalent isotope of gold is Au- \(197 .(4.5)\) a. How many protons, neutrons, and electrons are in this isotope? b. What is the atomic symbol of another isotope of gold with 116 neutrons? c. What is the atomic symbol of an atom with an atomic number of 78 and 116 neutrons?

Write the atomic symbol for each of the following: \((4.5)\) a. an atom with 47 protons and mass number of 107 b. an atom with 74 protons and 110 neutrons c. an atom with atomic number 70 and 100 neutrons d. an atom with 50 electrons and 70 neutrons

The most abundant isotope of nickel is \({ }_{28}^{58} \mathrm{Ni}\). (4.4) a. How many protons, neutrons, and electrons are in \(\frac{58}{28} \mathrm{Ni}\) ? b. What is the atomic symbol of another isotope of nickel with 35 neutrons? c. What is the name and symbol of an atom with the same mass number as in part \(\mathbf{b}\) and 34 neutrons?

Silicon has three naturally occurring isotopes: \(\mathrm{Si}-28\) that has a percent abundance of \(92.23 \%\) and a mass of \(27.977 \mathrm{amu}, \mathrm{Si}-29\) that has a \(4.68 \%\) abundance and a mass of \(28.976 \mathrm{amu}\), and Si- 30 that has a \(3.09 \%\) abundance and a mass of \(29.974\) amu. Calculate the atomic mass for silicon using the weighted average mass method. \((4.5)\)
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