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Chapter 2: Problem 106

To four significant figures, all of the following masses are possible for an individual titanium atom except one. The exception is (a) 45.95 u; (b) 46.95 u; (c) 47.87 u; (d) 47.95 u; (e) 48.95 u; (f) 49.94 u.

Short Answer

Expert verified
The impossible atomic mass for an individual titanium atom is (e) 48.95 u.

Step by step solution

01

Understanding taken values

Each number given is atomic mass to four significant figures, Therefore we can easily compare them. We examine \((a) 45.95 \,u;\) \((b) 46.95\, u;\) \((c) 47.87 \,u;\) \((d) 47.95 \,u;\) \((e) 48.95 \,u;\) and \((f) 49.94 \,u.\) atomic weights to current approx weight of titanium which is 47.87 u.
02

Identifying impossible mass

Compare every given atomic weight with the atomic weight of titanium, which is 47.87 u, obviously the value that exceeds the most from this weight will be the impossible mass for an individual titanium atom.
03

Select the right option

An analysis shows that options (a), (b), (c), (d), (e) and (f) lies close to the atomic weight of Titanium except (e) 48.95 u, which seems to be exceeding the atomic weight of Titanium most when compared with other options.

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Most popular questions from this chapter

Briefly describe (a) the law of conservation of mass (b) Rutherford's nuclear atom (c) weighted-average atomic mass (d) a mass spectrum

Germanium has three major naturally occurring isotopes: \(^{70}\) Ge \((69.92425 \mathrm{u}, 20.85 \%),^{72} \mathrm{Ge}(71.92208 \mathrm{u},\) \(27.54 \%),^{74} \mathrm{Ge}(73.92118 \mathrm{u}, 36.29 \%) .\) There are also two minor isotopes: \(^{73}\) Ge \(\left(72.92346 \text { u) and }^{76} \mathrm{Ge}\right.\) (75.92140 u). Calculate the percent natural abundances of the two minor isotopes. Comment on the precision of these calculations.

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 \(\mathrm{M}^{3+}\)

\begin{tabular}{l} There are four naturally occurring isotopes of \\ \hline \end{tabular} chromium. Their masses and percent natural abundances are \(49.9461 \mathrm{u}, 4.35 \% ; 51.9405 \mathrm{u}, 83.79 \% ; 52.9407 \mathrm{u}\) \(9.50 \% ;\) and \(53.9389 \mathrm{u}, 2.36 \% .\) Calculate the weightedaverage atomic mass of chromium.

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