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Chapter 2: Problem 97

An element's most stable ion forms an ionic compound with bromine, having the formula \(\mathrm{XBr}_{2}\). If the ion of element \(\mathrm{X}\) has a mass number of 230 and has 86 electrons, what is the identity of the element, and how many neutrons does it have?

Short Answer

Expert verified
The element X is Polonium (Po) with a +2 charge when forming an ionic compound with bromine, and it has 146 neutrons.

Step by step solution

01

Determining the charge of element X

Since the ionic compound has the formula \(\mathrm{XBr}_{2}\), it means that the ion of element X has a charge that balances with the charges of two bromide ions. The bromide ion (\(\mathrm{Br}^-\)) has a charge of -1. Therefore, the ion of element X must have a charge of +2 to balance the charges. So, element X has lost 2 electrons to form this ionic compound.
02

Finding the number of protons

Element X has 86 electrons in its neutral state. When it loses 2 electrons and acquires a +2 charge, it has 84 electrons. Since the number of protons is equal to the number of electrons in a neutral atom, element X has 84 protons.
03

Identifying the element

Using the periodic table, we can identify element X by looking for the element with an atomic number (number of protons) of 84. The element with an atomic number of 84 is Polonium (Po).
04

Calculating the number of neutrons

The mass number of an element is the sum of the protons and neutrons in its nucleus. Since Polonium (X) has a mass number of 230 and 84 protons, we can find the number of neutrons using the formula: Number of Neutrons = Mass Number - Number of Protons Number of Neutrons = 230 - 84 Number of Neutrons = 146 So, the ion of element X is Polonium with a +2 charge (Po^2+) and has 146 neutrons.

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Most popular questions from this chapter

Section \(2.3\) describes the postulates of Dalton's atomic theory. With some modifications, these postulates hold up very well regarding how we view elements, compounds, and chemical reactions today. Answer the following questions concerning Dalton's atomic theory and the modifications made today. a. The atom can be broken down into smaller parts. What are the smaller parts? b. How are atoms of hydrogen identical to each other, and how can they be different from each other? c. How are atoms of hydrogen different from atoms of helium? How can \(\mathrm{H}\) atoms be similar to He atoms? d. How is water different from hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) even though both compounds are composed of only hydrogen and oxygen? e. What happens in a chemical reaction, and why is mass conserved in a chemical reaction?

If the volume of a proton were similar to the volume of an electron, how will the densities of these two particles compare to each other?

A sample of chloroform is found to contain \(12.0 \mathrm{~g}\) of carbon, \(106.4 \mathrm{~g}\) of chlorine, and \(1.01 \mathrm{~g}\) of hydrogen. If a second sample of chloroform is found to contain \(30.0 \mathrm{~g}\) of carbon, what is the total mass of chloroform in the second sample?

For each of the following sets of elements, label each as either noble gases, halogens, alkali metals, alkaline earth metals, or transition metals. a. \(\mathrm{Ti}, \mathrm{Fe}, \mathrm{Ag}\) b. \(\mathrm{Mg}, \mathrm{Sr}, \mathrm{Ba}\) c. \(\mathrm{Li}, \mathrm{K}, \mathrm{Rb}\) d. Ne, \(\mathrm{Kr}, \mathrm{Xe}\) e. \(\mathrm{F}, \mathrm{Br}, \mathrm{I}\)

Which of the following is true about an individual atom? Explain. a. An individual atom should be considered to be a solid. b. An individual atom should be considered to be a liquid. c. An individual atom should be considered to be a gas. d. The state of the atom depends on which element it is. e. An individual atom cannot be considered to be a solid, liquid, or gas. Justify your choice, and for choices you did not pick, explain what is wrong with them.
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