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Chapter 1: Problem 46

Write the atomic symbol \(\left(\frac{1}{2} X\right)\) for each of the isotopes described below. a. number of protons \(=27,\) number of neutrons \(=31\) b. the isotope of boron with mass number 10 c. \(Z=12, A=23\) d. atomic number \(53,\) number of neutrons \(=79\) e. \(Z=20,\) number of neutrons \(=27\) f. number of protons \(=29,\) mass number 65

Short Answer

Expert verified
The atomic symbols for the given isotopes are as follows: a. \(\left(_{27}^{58}\textrm{Co}\right)\) b. \(\left(_{5}^{10}\textrm{B}\right)\) c. \(\left(_{12}^{23}\textrm{Mg}\right)\) d. \(\left(_{53}^{132}\textrm{I}\right)\) e. \(\left(_{20}^{47}\textrm{Ca}\right)\) f. \(\left(_{29}^{65}\textrm{Cu}\right)\)

Step by step solution

01

a. Isotope with 27 protons and 31 neutrons

Step 1: \(Z = 27\) Step 2: \(A = Z + \textrm{neutrons} = 27 + 31 = 58\) Step 3: \(X = \textrm{Cobalt (Co)}\) (Element with 27 protons) The atomic symbol for this isotope is \(\left(_{27}^{58}\textrm{Co}\right)\).
02

b. Isotope of boron with mass number 10

Step 1: \(Z = 5\) (Boron has 5 protons) Step 2: \(A = 10\) Step 3: \(X = \textrm{Boron (B)}\) The atomic symbol for this isotope is \(\left(_{5}^{10}\textrm{B}\right)\).
03

c. Isotope with Z=12 and A=23

Step 1: \(Z = 12\) Step 2: \(A = 23 \) Step 3: \(X = \textrm{Magnesium (Mg)}\) (Element with 12 protons) The atomic symbol for this isotope is \(\left(_{12}^{23}\textrm{Mg}\right)\).
04

d. Isotope with atomic number 53 and 79 neutrons

Step 1: \(Z = 53\) Step 2: \(A = Z + \textrm{neutrons} = 53 + 79 = 132\) Step 3: \(X = \textrm{Iodine (I)}\) (Element with 53 protons) The atomic symbol for this isotope is \(\left(_{53}^{132}\textrm{I}\right)\).
05

e. Isotope with Z=20 and 27 neutrons

Step 1: \(Z = 20\) Step 2: \(A = Z + \textrm{neutrons} = 20 + 27 = 47\) Step 3: \(X = \textrm{Calcium (Ca)}\) (Element with 20 protons) The atomic symbol for this isotope is \(\left(_{20}^{47}\textrm{Ca}\right)\).
06

f. Isotope with 29 protons and mass number 65

Step 1: \(Z = 29\) Step 2: \(A = 65\) Step 3: \(X = \textrm{Copper (Cu)}\) (Element with 29 protons) The atomic symbol for this isotope is \(\left(_{29}^{65}\textrm{Cu}\right)\).

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Most popular questions from this chapter

In a reaction, \(34.0 \mathrm{g}\) of chromium(III) oxide reacts with \(12.1 \mathrm{g}\) of aluminum to produce chromium and aluminum oxide. If \(23.3 \mathrm{g}\) of chromium is produced, what mass of aluminum oxide is produced? )

Section I-5 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 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?

Dalton assumed that all atoms of the same element were identical in all their properties. Explain why this assumption is not valid.

Consider 100.0 -g samples of two different compounds consisting only of carbon and oxygen. One compound contains \(27.2 \mathrm{g}\) of carbon and the other has \(42.9 \mathrm{g}\) of carbon. How can these data support the law of multiple proportions if 42.9 is not a multiple of \(27.2 ?\) Show that these data support the law of multiple proportions.

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