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Chapter 2: Problem 102

What is the correct symbol for the species that contains 18 neutrons, 17 protons, and 16 electrons?

Short Answer

Expert verified
The correct symbol for the species that contains 18 neutrons, 17 protons, and 16 electrons is \(^{35}Cl^{+}\).

Step by step solution

01

Determine the Element

The atomic number of an atom is equal to the number of protons. Here the number of protons is 17, which means the atom belongs to the element Chlorine(Cl) because Chlorine has an atomic number of 17.
02

Calculate the Mass Number

The mass number of an atom is found by adding the number of protons and neutrons together. Here, protons are 17 and neutrons are 18. Therefore, the mass number would be \(17 + 18 = 35\).
03

Identify the Charge

The charge of the ion is determined by the difference between the number of protons and electrons. If there are more protons than electrons, the ion has a positive charge. If there are more electrons than protons, it has negative charge. Here, protons are 17 and electrons are 16, so it has a charge of \(+1\). The difference is \(17 - 16 = +1\).

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Most popular questions from this chapter

Refer to the periodic table inside the front cover and identify (a) the element that is in group 11 and the sixth period (b) an element with atomic number greater than 50 that has properties similar to the element with atomic number 18 (c) the group number of an element \(\mathrm{E}\) that forms an ion \(\mathrm{E}^{2-}\) (d) an element \(M\) that you would expect to form the ion \(\mathrm{M}^{3+}\)

When a solid mixture consisting of \(10.500 \mathrm{g}\) calcium hydroxide and \(11.125 \mathrm{g}\) ammonium chloride is strongly heated, gaseous products are evolved and \(14.336 \mathrm{g}\) of a solid residue remains. The gases are passed into \(62.316 \mathrm{g}\) water, and the mass of the resulting solution is \(69.605 \mathrm{g}\). Within the limits of experimental error, show that these data conform to the law of conservation of mass.

In one experiment, the reaction of \(1.00 \mathrm{g}\) mercury and an excess of sulfur yielded \(1.16 \mathrm{g}\) of a sulfide of mercury as the sole product. In a second experiment, the same sulfide was produced in the reaction of \(1.50 \mathrm{g}\) mercury and \(1.00 \mathrm{g}\) sulfur. (a) What mass of the sulfide of mercury was produced in the second experiment? (b) What mass of which element (mercury or sulfur) remained unreacted in the second experiment?

Assuming that the seventh period of the periodic table has 32 members, what should be the atomic number of (a) the noble gas following radon (Rn); (b) the alkali metal following francium (Fr)?

Deuterium, \(^{2} \mathrm{H}(2.0140 \mathrm{u}),\) is sometimes used to replace the principal hydrogen isotope \(^{1} \mathrm{H}\) in chemical studies. The percent natural abundance of deuterium is 0.015\%. If it can be done with 100\% efficiency, what mass of naturally occurring hydrogen gas would have to be processed to obtain a sample containing \(2.50 \times 10^{21}^{2} \mathrm{H}\) atoms?
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