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Chapter 3: Problem 48

How much more massive is an "average" titanium (Ti) atom than a \({ }_{6}^{12} \mathrm{C}\) atom? (Use the periodic table for the atomic mass of titanium.)

Short Answer

Expert verified
An average titanium atom is 35.87 u more massive than a \( _{6}^{12} \mathrm{C}\) atom.

Step by step solution

01

Find the atomic mass of Titanium (Ti)

Using the periodic table, locate the element Titanium (Ti). The atomic mass of Ti is approximately 47.87 u (unified atomic mass units).
02

Find the atomic mass of Carbon (\( _{6}^{12} \mathrm{C}\))

From the given exercise, we can see that the isotope of Carbon we are dealing with is \( _{6}^{12} \mathrm{C}\). The superscript 12 indicates the atomic mass of this isotope, which is 12 u.
03

Calculate the difference in atomic masses

Now, we will subtract the atomic mass of carbon from the atomic mass of titanium to find the difference: Difference in atomic masses = Atomic mass of Ti - Atomic mass of \( _{6}^{12} \mathrm{C}\) Difference in atomic masses = 47.87 u - 12 u
04

Calculate the result

Now, subtract the two atomic masses: Difference in atomic masses = 35.87 u So, an average titanium atom is 35.87 u more massive than a \( _{6}^{12} \mathrm{C}\) atom.

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Most popular questions from this chapter

(a) In what unique way did Mendeleev order the elements to make his discovery? (b) What was his discovery? (c) How does his ordering differ from the modern ordering?

For each pair, indicate which atom loses an electron more easily: (a) \(\mathrm{Na}\) or \(\mathrm{K}\) (b) Na or Al (c) \(\mathrm{Rb}\) or \(\mathrm{Ca}\) (d) \(\mathrm{S}\) or \(\mathrm{Cl}\) (e) Br or Kr

Atom A has 35 protons and 44 neutrons in its nucleus. Atom \(\mathrm{B}\) has 35 protons and 46 neutrons in its nucleus. Should we expect similar or different chemical properties for these atoms? Explain.

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