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Chapter 2: Problem 44

Determine the molecular and empirical formulas of the following: (a) The organic solvent benzene, which has six carbon atoms and six hydrogen atoms; (b) the compound silicon tetrachloride, which has a silicon atom and four chlorine atoms and is used in the manufacture of computer chips; (c) the reactive substance diborane, which has two boron atoms and six hydrogen atoms; (d) the sugar called glucose, which has six carbon atoms, twelve hydrogen atoms, and six oxygen atoms

Short Answer

Expert verified
(a) Benzene: Molecular Formula - C_6H_6; Empirical Formula - C_6H_6. (b) Silicon tetrachloride: Molecular Formula - SiCl_4; Empirical Formula - SiCl_4. (c) Diborane: Molecular Formula - B_2H_6; Empirical Formula - BH_3. (d) Glucose: Molecular Formula - C_6H_12O_6; Empirical Formula - CH_2O.

Step by step solution

01

Identify the elements and their atom counts in each compound

First, let's list the given compounds and the number of atoms for each element: (a) Benzene: 6 carbon atoms and 6 hydrogen atoms. (b) Silicon tetrachloride: 1 silicon atom \(\) and 4 chlorine atoms. (c) Diborane: 2 boron atoms \(\) and 6 hydrogen atoms. (d) Glucose: 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms.
02

Write the molecular formulas

Now, we'll write the molecular formulas for each compound using the given atom counts for each element: (a) Benzene: C_6H_6 (b) Silicon tetrachloride: SiCl_4 (c) Diborane: B_2H_6 (d) Glucose: C_6H_12O_6
03

Finding the empirical formulas

To find the empirical formulas, we'll simplify the whole-number ratios of atoms in each molecular formula. If a formula is already in its simplest form, it will be the same as the molecular formula. (a) Benzene: C_6H_6. The whole-number ratio of C and H is already 1:1, so the empirical formula is the same as the molecular formula. Empirical formula: C_6H_6 (b) Silicon tetrachloride: SiCl_4. The whole-number ratio of Si and Cl is already 1:4, so the empirical formula is the same as the molecular formula. Empirical formula: SiCl_4 (c) Diborane: B_2H_6. The whole-number ratio of B and H is 1:3, so the empirical formula is BH_3. (d) Glucose: C_6H_12O_6. The whole-number ratio of C, H, and O is 1:2:1, so the empirical formula is CH_2O. So, the molecular and empirical formulas are: (a) Benzene: Molecular Formula - C_6H_6; Empirical Formula - C_6H_6. (b) Silicon tetrachloride: Molecular Formula - SiCl_4; Empirical Formula - SiCl_4. (c) Diborane: Molecular Formula - B_2H_6; Empirical Formula - BH_3. (d) Glucose: Molecular Formula - C_6H_12O_6; Empirical Formula - CH_2O.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Formula
The molecular formula of a compound provides information about the exact number of each type of atom present in a molecule of that compound. This is very useful because it allows us to understand the composition at a glance.
For instance, benzene has the molecular formula \(C_6H_6\). This tells us it is composed of 6 carbon atoms and 6 hydrogen atoms. Glucose, a common sugar, is represented as \(C_6H_{12}O_6\), meaning it contains 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms in every molecule.
  • Gives precise atom numbers
  • Shows molecule's full composition
  • Critical for identifying chemical properties
The molecular formula is essential for chemists when they need to understand the chemical behavior or possibilities of the molecules they are working with.
Empirical Formula
The empirical formula of a compound gives the simplest whole-number ratio of atoms of each element present within the compound. It's a basic version of the molecular formula, providing an idea of the proportion but not the exact quantities of atoms.
For example, benzene鈥檚 molecular formula \(C_6H_6\) has an empirical formula of \(CH\) because the whole-number ratio of carbon to hydrogen is 1:1. Another example is glucose, \(C_6H_{12}O_6\), which has an empirical formula \(CH_2O\). In this case, the ratio is 1:2:1, simplified to the smallest whole numbers.
  • Shows simplest atom ratios
  • Lack exact atom counts
  • Great for quick assessments
Knowing both the molecular and empirical formulas is crucial since they collectively provide a comprehensive understanding of a compound's chemical structure.
Organic Compounds
Organic compounds are primarily composed of carbon atoms and usually include hydrogen, often oxygen or nitrogen, and sometimes other elements. A common feature among organic compounds is their carbon-hydrogen bonds, which are key to the compound's properties and behaviors.
Formulas like benzene \(C_6H_6\) and glucose \(C_6H_{12}O_6\) showcase how carbon acts as a backbone, allowing the formation of various functional groups that define each organic compound's distinct characteristics.
  • Contains carbon atoms
  • Typically includes hydrogen
  • Vital for life processes
Understanding organic chemistry is essential due to the vast number of organic compounds and their importance in living organisms and industrial applications.
Inorganic Compounds
Inorganic compounds, unlike organic compounds, typically do not contain carbon-hydrogen bonds. They can consist of a diverse range of elements and structures, frequently found in non-living systems or as simple salts and metals.
Silicon tetrachloride \(SiCl_4\), used in computer chip manufacturing, is an example of an inorganic compound, where a silicon atom is bonded with four chlorine atoms. Its simplicity and lack of carbon-hydrogen bonding categorize it as inorganic.
  • Lacks carbon-hydrogen bonds
  • Can include metals and salts
  • Found widely in industrial and geological processes
Inorganic chemistry covers a broad spectrum and is crucial for understanding mineral and chemical interactions in non-organic systems.

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Most popular questions from this chapter

Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of \(H_{2}\) is taken under conditions that prevent decomposition into H atoms. The two naturally occurring isotopes of hydrogen are \({ }^{1} \mathrm{H}\) (atomic mass \(=1.00783\) amu; abundance \(99.9885 \%\) ) and \({ }^{2} \mathrm{H}\) (atomic mass \(=2.01410\) amu; abundance 0.0115\%). (a) How many peaks will the mass spectrum have? (b) Give the relative atomic masses of each of these peaks. (c) Which peak will be the largest, and which the smallest?

(a) Figure \(2.5\) shows the apparatus used in the Millikan oil-drop experiment with the positively charged plate above the negatively charged plate. What do you think would be the effect on the rate of oil drops descending if the charges on the plates were reversed (negative above positive)? (b) In his original series of experiments, Millikan measured the charge on 58 separate oil drops. Why do you suppose he chose so many drops before reaching his final conclusions?

Using the periodic table, predict the charges of the ions of the following elements: (a) \(\mathrm{Ga}\), (b) \(\mathrm{Sr}\), (c) As, (d) Br, (e) Se.

Write the correct symbol, with both superscript and subscript, for each of the following. Use the list of elements inside the front cover as needed: (a) the isotope of platinum that contains 118 neutrons, (b) the isotope of krypton with mass number 84, (c) the isotope of arsenic with mass number \(75,(\mathrm{~d})\) the isotope of magnesium that has an equal number of protons and neutrons.

How many of the indicated atoms are represented by each chemical formula: (a) carbon atoms in \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOCH}_{3}\) (b) oxygen atoms in \(\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}\). (c) hy- drogen atoms in \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4} ?\)
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