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Chapter 2: Problem 42

Do both members of the following pairs have the same number of protons? Neutrons? Electrons? (a) \({ }_{8}^{16} \mathrm{O}\) and \({ }_{8}^{17} \mathrm{O}\) (b) \({ }_{18}^{40} \mathrm{Ar}\) and \({ }_{19}^{41} \mathrm{~K}\) (c) \({ }_{27}^{60} \mathrm{Co}\) and \({ }_{28}^{60} \mathrm{Ni}\)

Short Answer

Expert verified
a) Same protons and electrons, different neutrons. b) Different protons and electrons, same neutrons. c) Different protons, neutrons, and electrons.

Step by step solution

01

- Determine the number of protons

The number of protons in an atom is given by the atomic number (the lower left number). For (a) \(_{8}^{16} \mathrm{O}\) and \(_{8}^{17} \mathrm{O}\), both have 8 protons. For (b) \(_{18}^{40} \mathrm{Ar}\) and \(_{19}^{41} \mathrm{~K}\), the number of protons is 18 for Ar and 19 for K. For (c) \(_{27}^{60} \mathrm{Co}\) and \(_{28}^{60} \mathrm{Ni}\), Co has 27 protons and Ni has 28.
02

- Determine the number of neutrons

To find the number of neutrons, subtract the atomic number from the mass number (upper left number). For (a) \(_{8}^{16} \mathrm{O}\) and \(_{8}^{17} \mathrm{O}\), the neutrons are 16-8=8 and 17-8=9, respectively. For (b) \(_{18}^{40} \mathrm{Ar}\) and \(_{19}^{41} \mathrm{~K}\), the neutrons are 40-18=22 and 41-19=22. For (c) \(_{27}^{60} \mathrm{Co}\) and \(_{28}^{60} \mathrm{Ni}\), the neutrons are 60-27=33 and 60-28=32.
03

- Determine the number of electrons in neutral atoms

In neutral atoms, the number of electrons equals the number of protons. For (a) \(_{8}^{16} \mathrm{O}\) and \(_{8}^{17} \mathrm{O}\), each has 8 electrons. For (b) \(_{18}^{40} \mathrm{Ar}\) and \(_{19}^{41}\mathrm{~K}\), the electrons are 18 for Ar and 19 for K. For (c) \(_{27}^{60} \mathrm{Co}\) and \(_{28}^{60} \mathrm{Ni}\), Co has 27 electrons and Ni has 28.

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Key Concepts

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

Atomic Number
The atomic number is a fundamental property of an element. It denotes the number of protons in the nucleus of an atom. Each element has a unique atomic number, which defines its identity. For example, Oxygen (O) has an atomic number of 8, which means it has 8 protons. This number is usually written as a subscript to the left of the chemical symbol. It is crucial because it also determines the number of electrons in a neutral atom, balancing the positive charge of protons with the negative charge of electrons.

This unique number also helps to place the element in its correct position on the periodic table, ensuring we can predict its chemical behavior.
Mass Number
The mass number is the sum of protons and neutrons in the nucleus of an atom. It is not the same as the atomic weight you see on the periodic table, which is an average value. Mass number is specifically for a single isotope of an element. Isotopes are variations of elements that have the same number of protons but different numbers of neutrons.

For example, the mass number of \(\text{O}^{16}_{8}\) is 16, formed by 8 protons plus 8 neutrons, whereas \(\text{O}^{17}_{8}\) has a mass number of 17 due to its additional neutron, summing up 8 protons and 9 neutrons.
Protons
Protons are positively charged particles found in the nucleus of an atom. They play a critical role in defining the element and its properties. The number of protons in an atom is equal to the atomic number. For instance, the atomic number of Carbon (C) is 6, meaning every carbon atom has 6 protons. The proton count is fixed for each element; altering the number of protons transforms it into a different element entirely.

Protons contribute significantly to the mass of an atom. Despite their minute size, their positive charge balances the negative charge of electrons, maintaining the atom's overall neutrality.
Neutrons
Neutrons are neutrally charged particles that reside in the nucleus alongside protons. Unlike protons and electrons, neutrons have no electric charge, but they add to the mass of the atom. The number of neutrons varies among isotopes of the same element. For example, \(\text{O}_{8}^{16}\) and \(\text{O}_{8}^{17}\) both have 8 protons but 8 and 9 neutrons, respectively.

Neutrons play a vital role in stabilizing the nucleus. They prevent the protons from repelling each other due to their like charges. This balance allows atoms to exist in a stable state.
Electrons
Electrons are negatively charged particles that orbit the nucleus of an atom. The number of electrons in a neutral atom is equal to its number of protons. Thus, an atom with an atomic number of 8 will also have 8 electrons. Electrons are much smaller than protons or neutrons but are crucial for chemical bonding and reactivity.

They occupy different energy levels or shells around the nucleus. The arrangement of electrons in these shells determines the atom’s chemical properties and how it will interact with other atoms.

For instance, Argon (Ar) with an atomic number of 18 has 18 electrons spread out in its shells in a specific way, making it chemically inert.

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Most popular questions from this chapter

Correct each of the following formulas: (a) Barium oxide is \(\mathrm{BaO}_{2}\). (b) Iron(II) nitrate is \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) (c) Magnesium sulfide is \(\mathrm{MnSO}_{3}\). (d) Potassium iodide is \(\mathrm{P}_{2} \mathrm{I}_{3}\).

Nitrogen forms more oxides than any other element. The percents by mass of \(\mathrm{N}\) in three different nitrogen oxides are (I) \(46.69 \%\), (II) \(36.85 \%\), and (III) \(25.94 \% .\) For each compound, determine (a) the simplest whole-number ratio of \(\mathrm{N}\) to \(\mathrm{O}\) and (b) the number of grams of oxygen per \(1.00 \mathrm{~g}\) of nitrogen.

Which of Dalton's postulates about atoms are inconsistent with later observations? Do these inconsistencies mean that Dalton was wrong? Is Dalton's model still useful? Explain.

Give the formulas of the compounds in each set: (a) Lead(II) oxide and lead(IV) oxide (b) Lithium nitride, lithium nitrite, and lithium nitrate (c) Strontium hydride and strontium hydroxide (d) Magnesium oxide and manganese(II) oxide

The monatomic ions of Groups \(1 \mathrm{~A}(1)\) and \(7 \mathrm{~A}(17)\) are all singly charged. In what major way do they differ? Why?
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