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Magazine Chapter 12: Problem 8
How many moles of atomic oxygen are present in \(1 \mathrm{mol}\) of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2} ?\)
Short Answer
Expert verified
There are 8 moles of atomic oxygen.
Step by step solution
01
Identify the Chemical Formula
The chemical formula provided is \(\text{Ca}_{3}(\text{PO}_{4})_{2}\). This is a compound called Calcium Phosphate.
02
Count the Atoms in the Formula Unit
Within one formula unit of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\), identify the number of oxygen atoms. The formula contains two phosphate ions \((\text{PO}_{4})_{2}\). Each \(\text{PO}_{4}\) ion has 4 oxygen atoms.
03
Calculate the Total Number of Oxygen Atoms
Since there are two \(\text{PO}_{4}\) ions, multiply the oxygen atoms by 2: 4 oxygen atoms \times\ 2 = 8 oxygen atoms.
04
Determine Moles of Oxygen
Since there are 8 oxygen atoms in one formula unit of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\), and you have 1 mole of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\), there are 8 moles of atomic oxygen present.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
chemical formula
A chemical formula represents the elements present in a compound and the ratio in which these elements combine. It provides a clarity about the composition of the compound. For example, the chemical formula \(\text{Ca}_{3}(\text{PO}_{4})_{2}\) represents Calcium Phosphate. Let's break this down:
- \(\text{Ca}\) stands for calcium.
- \(\text{P}\) stands for phosphorus.
- \(\text{O}\) stands for oxygen.
atoms in a formula unit
Understanding how to count atoms in a formula unit is crucial for solving chemistry problems. Let鈥檚 take the formula unit of Calcium Phosphate, \(\text{Ca}_{3}(\text{PO}_{4})_{2}\) once more as an example.
- The \(\text{Ca}_{3}\) part means every formula unit has 3 calcium atoms.
- The \((\text{PO}_{4})_{2}\) part requires you to multiply every sub-unit in \(\text{PO}_{4}\) by 2:
- Each \(\text{P}\) in \(\text{PO}_{4}\) has 1 phosphorus atom, so 2 \(\text{PO}_{4}\) units have 2 phosphorus atoms total.
- Each \(\text{PO}_{4}\) has 4 oxygen atoms, resulting in 2 \(\text{PO}_{4}\) multiplying to 8 oxygen atoms total.
mole calculation
Calculating moles involves understanding Avogadro's number, which is \(6.022 \times 10^{23}\). This number represents the quantity of units (atoms, molecules, ions) in a mole. When dealing with moles, you convert between mass, volume, number of particles, and the number of moles using this concept. For example, if you have one mole of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\):
- You have \(6.022 \times 10^{23}\) formula units of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\).
- In each formula unit, there are 3 calcium atoms, 2 phosphorus atoms, and essentially 8 oxygen atoms (as previously calculated).
- Therefore, one mole of \(\text{Ca}_{3}(\text{PO}_{4})_{2}\) contains 8 moles of oxygen atoms.
phosphate ions
Phosphate ions are a vital part of many chemical compounds. The formula for a phosphate ion is \(\text{PO}_{4}^{3-}\). This means it has one phosphorus atom bonded to four oxygen atoms and carries a overall charge of -3.
- In Calcium Phosphate \(\text{Ca}_{3}(\text{PO}_{4})_{2}\), there are two \(\text{PO}_{4}\) ions.
- Each of these phosphate ions further contributes to the total number of oxygen atoms in the formula unit.
Calcium Phosphate
Calcium Phosphate, represented by \(\text{Ca}_{3}(\text{PO}_{4})_{2}\), is a common compound found in many biological systems and materials. Here鈥檚 a quick overview:
- It's a significant component of bone and teeth in living organisms.
- It鈥檚 used in fertilizers.
- In medicine, it's involved as an agent in many supplements.
- Structurally, it has 3 Calcium atoms, 2 Phosphate ions each with 1 Phosphorus and 4 oxygen atoms (total of 8 oxygen atoms per formula unit).
