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Chapter 1: Problem 53

Four \(\mathrm{Fe}^{2+}\) ions are key components of hemoglobin, the protein that transports oxygen in the blood. Assuming that these ions are \(^{53} \mathrm{Fe}^{2+}\), how many protons and neutrons are present in each nucleus, and how many electrons are present in each ion?

Short Answer

Expert verified
In each nucleus of the \(^{53}\mathrm{Fe}^{2+}\) ion, there are 26 protons and 27 neutrons. Each ion has 24 electrons.

Step by step solution

01

Determine the atomic number and mass number for \(^{53}\mathrm{Fe}^{2+}\)

First, let us determine the atomic number (Z) and mass number (A) for \(^{53}\mathrm{Fe}^{2+}\). The atomic number of iron (Fe) is Z = 26, which represents the number of protons in the nucleus. The mass number (A) is the sum of protons and neutrons in the nucleus. The given isotope of iron is \(^{53}\mathrm{Fe}\), so A = 53.
02

Determine the number of neutrons

Now that we have both the atomic number (Z) and the mass number (A), we can determine the number of neutrons present in the nucleus. The number of neutrons (N) can be found using the following formula: \(N = A - Z\) Substitute the values for A and Z: \(N = 53 - 26\) \(N = 27\) There are 27 neutrons in the nucleus of each \(^{53}\mathrm{Fe}\) isotope.
03

Determine the number of electrons in \(^{53}\mathrm{Fe}^{2+}\) ion

The given ion is \(\mathrm{Fe}^{2+}\), which means that two electrons have been removed to produce a positive charge of +2. To find the number of electrons (e) in each ion, subtract the charge from the atomic number (Z) as following: \(e = Z - Charge\) \(e = 26 - 2\) \(e = 24\) There are 24 electrons in each \(^{53}\mathrm{Fe}^{2+}\) ion.
04

Final Answer

In each nucleus of the \(^{53}\mathrm{Fe}^{2+}\) ion, there are 26 protons and 27 neutrons. Each ion has 24 electrons.

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Most popular questions from this chapter

You have two distinct gaseous compounds made from element \(\mathrm{X}\) and element Y. The mass percents are as follows: Compound I: \(30.43 \%\) X, \(69.57 \%\) Y Compound II: \(63.64 \% \mathrm{X}, 36.36 \% \mathrm{Y}\) In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas \(\mathrm{X}^{\prime \prime}+2\) volumes "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound I 2 volumes "gas \(\mathrm{X}^{\prime \prime}+1\) volume "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element \(X\) and element Y.

Which (if any) of the following can be determined by knowing the number of protons in a neutral element? Explain your answer. a. the number of neutrons in the neutral element b. the number of electrons in the neutral element c. the name of the element

These questions concern the work of J. J. Thomson. a. From Thomson's work, which particles do you think he would feel are most important for the formation of compounds (chemical changes), and why? b. Of the remaining two subatomic particles, which do you place second in importance for forming compounds, and why? c. Propose three models that explain Thomson's findings and evaluate them. To be complete you should include Thomson's findings.

Write the symbol of each atom using the \(_{z}^{\text {A }}\)X format.

Write the atomic symbol \(\left(\frac{4}{2} X\right)\) for each of the following isotopes. a. \(Z=8,\) number of neutrons \(=9\) b. the isotope of chlorine in which \(A=37\) c. \(Z=27, A=60\) d. number of protons \(=26,\) number of neutrons \(=31\) e. the isotope of I with a mass number of 131 f. \(Z=3,\) number of neutrons \(=4\)
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