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Chapter 2: Problem 153

Fluorine occurs naturally as a single isotope. How many protons, neutrons, and electrons are present in deuterium fluoride \(\left({ }^{2} \mathrm{HF}\right) ?\) (Deuterium is \({ }^{2} \mathrm{H}\).)

Short Answer

Expert verified
Deuterium fluoride has 10 protons, 11 neutrons, and 10 electrons.

Step by step solution

01

Identify Fluorine Details

Fluorine naturally appears as a single isotope \(^{19}\text{F}\). It has an atomic number of 9, which means it has 9 protons and, for a neutral atom, 9 electrons. The number of neutrons is determined by subtracting the atomic number from the atomic mass, i.e., \(19 - 9 = 10\) neutrons.
02

Identify Deuterium Details

Deuterium is a heavier isotope of hydrogen \(^{2}\text{H}\), consisting of 1 proton, 1 electron, and 1 neutron. The atomic number of hydrogen is 1, so deuterium has 1 proton, and its mass number is 2, thus it has \(2 - 1 = 1\) neutron.
03

Combine in Deuterium Fluoride

Deuterium fluoride \(^{2}\text{HF}\) is a compound consisting of one deuterium atom and one fluorine atom. Thus, the total count of subatomic particles is the sum of those in deuterium and fluorine. This results in 1 + 9 = 10 protons, 1 + 10 = 11 neutrons, and 1 + 9 = 10 electrons.

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Key Concepts

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

Deuterium and Its Unique Characteristics
Deuterium, often referred to as heavy hydrogen, distinguishes itself from regular hydrogen by having one extra neutron. This gives it a mass number of 2 since it contains 1 proton and 1 neutron, unlike typical hydrogen which only has 1 proton and no neutrons.

In the field of chemistry and physics, deuterium ( ^2 ext{H} ) is especially interesting because it creates heavier versions of compounds, like deuterium fluoride ( ^2 ext{HF} ).

This extra neutron hardly affects how atoms bond chemically, but it does make deuterium-containing compounds slightly denser. Understanding deuterium's composition helps in discerning its role in forming compounds like deuterium fluoride.
Fluorine: A Single-Isotope Element
Fluorine is a unique element in that it is primarily found in nature as just one isotope, ^{19} ext{F}. This characteristic simplifies its atomic structure analysis, as all naturally occurring fluorine atoms share the same number of subatomic particles.

Fluorine's atomic number is 9, which tells us it has 9 protons. For neutral atoms, the number of electrons equals the number of protons, so in neutral fluorine, there are also 9 electrons.

To find the number of neutrons in fluorine, we can subtract the atomic number from the atomic mass, which gives us: 19 - 9 = 10 neutrons.
  • Protons: 9
  • Neutrons: 10
  • Electrons: 9

This consistency makes studying fluorine's chemical behavior more straightforward and predictable.
Understanding the Atomic Structure of Compounds
The atomic structure of a compound is determined by the sum of the subatomic particles from each of its components.

In deuterium fluoride ( ^2 ext{HF} ), we combine the atomic structures of deuterium and fluorine to understand the whole picture.

From deuterium, we have:
  • 1 proton
  • 1 neutron
  • 1 electron

And from fluorine:
  • 9 protons
  • 10 neutrons
  • 9 electrons

When creating the compound, we add these values together:
  • Total Protons: 1 + 9 = 10
  • Total Neutrons: 1 + 10 = 11
  • Total Electrons: 1 + 9 = 10

Understanding the detailed atomic structure helps predict the compound's behavior, providing insights into its chemical reactions and properties.

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Most popular questions from this chapter

Look at the alphabetical list of elements inside the front cover. Give the names corresponding to the following symbols: (a) \(\mathrm{B}\) (b) \(\mathrm{Rh}\) (c) Cf (d) Os (e) \(\mathrm{Ga}\)

Ibuprofen was initially synthesized by a process developed by Boots Co. in the \(1960 \mathrm{~s}\). Six reaction steps were utilized, and the percent atom economy was \(40 \%\). For every one mole of ibuprofen produced, 1 mole of Na, 23 moles of \(\mathrm{H}, 1\) mole of \(\mathrm{N}, 7\) moles of \(\mathrm{C}\), 8 moles of \(\mathrm{O}\), and 1 mole of \(\mathrm{Cl}\) were unused and considered as waste. (a) Calculate the mass (g) of each element wasted for every one mole of ibuprofen produced. (b) Calculate the total mass ( \(\mathrm{g}\) ) wasted for every one mole of ibuprofen produced. (c) Yearly production of ibuprofen is approximately 30 million lbs, which is equivalent to \(6.6 \times 10^{7}\) moles. Calculate the total mass (kg) of matter wasted in the annual production ibuprofen.

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An element is a shiny, silver-colored solid at room temperature and pressure. It conducts electricity and can be found in nature in its pure form. Classify the element as a metal, nonmetal, or semimetal and specify its general location in the periodic table.

A compound of zinc and sulfur contains \(67.1 \%\) zinc by mass. What is the ratio of zinc and sulfur atoms in the compound?
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