Chapter 2: Problem 46
Give the names of the nonmetals that correspond to the following symbols: As, I, Xe, He, C, Si.
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A certain element has only two naturally occurring isotopes: one with 18 neutrons and the other with 20 neutrons. The element forms \(1-\) charged ions when in ionic compounds. Predict the identity of the element. What number of electrons does the \(1-\) charged ion have?
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.
You have two distinct gaseous compounds made from element \(\mathrm{X}\) and element \(\mathrm{Y}\). The mass percents are as follows: Compound I: \(30.43 \% \mathrm{X}, 69.57 \% \mathrm{Y}\) Compound II: \(63.64 \% \mathrm{X}, 36.36 \% \mathrm{Y}\) In their natural standard states, element \(\mathrm{X}\) and element \(\mathrm{Y}\) 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 \(\mathrm{X}\) and element \(\mathrm{Y}\).
A sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) contains \(2.02 \mathrm{~g}\) of hydrogen, \(32.07 \mathrm{~g}\) of sulfur, and \(64.00 \mathrm{~g}\) of oxygen. How many grams of sulfur and grams of oxygen are present in a second sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) containing \(7.27 \mathrm{~g}\) of hydrogen?
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 \(\mathrm{In}_{2} \mathrm{O}_{3}\) 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 \(16.00\).
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