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Chapter 2: Problem 63

Write the symbol of each atom using the \(\left(_{Z}^{A} X\right)\) format.

Short Answer

Expert verified
To write the symbol of an atom using the \(\left(_{Z}^{A} X\right)\) format, follow these steps: 1. Identify the element using its atomic number (\(Z\)). 2. Determine the mass number (\(A\)), which is the sum of protons and neutrons. 3. Write the symbol using the format \(\left(_{Z}^{A} X\right)\), where \(Z\) is the atomic number, \(A\) is the mass number, and \(X\) is the element symbol. For example, for Carbon-12: \(\left(_{6}^{12} C\right)\).

Step by step solution

01

Identify the element

Find the element's symbol in the periodic table using the atomic number (\(Z\)) given in the exercise. The atomic number is the number of protons, which determines the element's identity.
02

Determine the mass number

Use the mass number given in the exercise (\(A\)), which is the sum of protons and neutrons in the atomic nucleus.
03

Write the symbol using the \(\left(_{Z}^{A} X\right)\) format

Use the atomic number, mass number, and element symbol to write the symbol of the atom using the given format, i.e., \(\left(_{Z}^{A} X\right)\). For example, in the case of Carbon-12 (12 is the mass number of the isotope), the break down would look like this:
04

Identify the element

In this case, Carbon is the element with an atomic number of 6.
05

Determine the mass number

The mass number is given as 12.
06

Write the symbol using the \(\left(_{Z}^{A} X\right)\) format

Insert the atomic number, mass number, and element symbol to obtain the symbol for Carbon-12: \(\left(_{6}^{12} C\right)\).

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Most popular questions from this chapter

Two elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00 g of Q. In the second compound, 7.00 g of R combines with 4.50 g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?

Indium oxide contains 4.784 \(\mathrm{g}\) of indium for every 1.000 \(\mathrm{g}\) of oxygen. In \(1869,\) when Mendeleev first presented his version of the periodic table, he proposed the formula $\operatorname{In}_{2} \mathrm{O}_{3}$ for indium oxide. Before that time it was thought that the formula was InO. What values for the atomic mass of indium are obtained using these two formulas? Assume that oxygen has an atomic mass of 16.00 .

What number of protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, what number of electrons are present? a. \(^{235}_{92} \mathrm{U}\) b. \(_{13}^{27} \mathrm{Al}\) c. \(_{26}^{57} \mathrm{Fe}\) d. \(_{82}^{208} \mathrm{Pb}\) e. \(_{37}^{86} \mathrm{Rb}\) f. \(_{20}^{41} \mathrm{Ca}\)

A chemistry instructor makes the following claim: “Consider that if the nucleus were the size of a grape, the electrons would be about 1 mile away on average.” Is this claim reasonably accurate? Provide mathematical support.

For each of the following ions, indicate the number of protons and electrons the ion contains. a. \(\quad \mathrm{Ba}^{2+}\) b. \(\mathrm{Zn}^{2+}\) c. \(\mathrm{N}^{3-}\) d. \(\mathrm{Rb}^{+}\) e. \(\mathrm{Co}^{3+}\) f. \(\mathrm{Te}^{2-}\) g. \(\mathrm{Br}^{-}\)
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