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Chapter 2: Problem 49

Write the empirical formula corresponding to each of the following molecular formulas: (a) \(\mathrm{Al}_{2} \mathrm{Br}_{6}\), (b) $\mathrm{C}_{8} \mathrm{H}_{10}\( (c) \)\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{2}$ (d) \(\mathrm{P}_{4} \mathrm{O}_{10}\) (e) $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}\( (f) \)\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6}$

Short Answer

Expert verified
Empirical formulas: (a) \(AlBr_{3}\), (b) \(C_{4}H_{5}\), (c) \(C_{2}H_{4}O\), (d) \(P_{2}O_{5}\), (e) \(C_{3}H_{2}Cl\), (f) \(BNH_{2}\)

Step by step solution

01

(a) Determine empirical formula for Al₂Br₆

To find the simplest whole number ratio of Al and Br, let's find the greatest common divisor (GCD) for the subscripts 2 and 6. The GCD of 2 and 6 is 2. Divide the subscripts by the GCD: Al: 2 / 2 = 1 Br: 6 / 2 = 3 Empirical formula: \(AlBr_{3}\)
02

(b) Determine empirical formula for C₈H₁₀

To find the simplest whole number ratio of C and H, let's find the GCD for the subscripts 8 and 10. The GCD of 8 and 10 is 2. Divide the subscripts by the GCD: C: 8 / 2 = 4 H: 10 / 2 = 5 Empirical formula: \(C_{4}H_{5}\)
03

(c) Determine empirical formula for C₄H₈O₂

To find the simplest whole number ratio of C, H, and O, let's find the GCD for the subscripts 4, 8, and 2. The GCD of 4, 8, and 2 is 2. Divide the subscripts by the GCD: C: 4 / 2 = 2 H: 8 / 2 = 4 O: 2 / 2 = 1 Empirical formula: \(C_{2}H_{4}O\)
04

(d) Determine empirical formula for P₄O₁₀

To find the simplest whole number ratio of P and O, let's find the GCD for the subscripts 4 and 10. The GCD of 4 and 10 is 2. Divide the subscripts by the GCD: P: 4 / 2 = 2 O: 10 / 2 = 5 Empirical formula: \(P_{2}O_{5}\)
05

(e) Determine empirical formula for C₆H₄Cl₂

To find the simplest whole number ratio of C, H, and Cl, let's find the GCD for the subscripts 6, 4, and 2. The GCD of 6, 4, and 2 is 2. Divide the subscripts by the GCD: C: 6 / 2 = 3 H: 4 / 2 = 2 Cl: 2 / 2 = 1 Empirical formula: \(C_{3}H_{2}Cl\)
06

(f) Determine empirical formula for B₃N₃H₆

To find the simplest whole number ratio of B, N, and H, let's find the GCD for the subscripts 3, 3, and 6. The GCD of 3, 3, and 6 is 3. Divide the subscripts by the GCD: B: 3 / 3 = 1 N: 3 / 3 = 1 H: 6 / 3 = 2 Empirical formula: \(BNH_{2}\)

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Most popular questions from this chapter

What fraction of the \(\alpha\) particles in Rutherford's gold foil experiment are scattered at large angles? Assume the gold foil is two layers thick, as shown in Figure \(2.9,\) and that the approximate diameters of a gold atom and its nucleus are 270 \(\mathrm{pm}\) and \(1.0 \times 10^{-2} \mathrm{pm}\), respectively. Assume that the gold nuclei in each layer are offset from each other.

Predict whether each of the following compounds is molecular or ionic: $(\mathbf{a}) \mathrm{BI}_{3}(\mathbf{b}) \mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}(\mathbf{c}) \mathrm{Zr}\left(\mathrm{NO}_{3}\right)_{2}\( (d) \)\mathrm{N}_{2} \mathrm{H}_{4}(\mathbf{e})\( \)\mathrm{OsCO}_{3}(\mathbf{f}) \mathrm{H}_{2} \mathrm{SO}_{4}(\mathbf{g}) \mathrm{HgS}(\mathbf{h}) \mathrm{IOH}$

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 \(\mathrm{H}_{2}\) is taken under conditions that prevent decomposition into \(\mathrm{H}\) atoms. The two naturally occurring isotopes of hydrogen are ${ }^{1} \mathrm{H}\( (atomic mass \)=1.00783 \mathrm{u}\(; abundance \)\left.99.9885 \%\right)\( and \){ }^{2} \mathrm{H}\( (atomic mass \)=2.01410 \mathrm{u}$; abundance \(\left.0.0115 \%\right)\). (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) Define atomic number and mass number. (b) Which of these can vary without changing the identity of the element?

(a) What is a hydrocarbon? (b) Pentane is the alkane with a chain of five carbon atoms. Write a structural formula for this compound and determine its molecular and empirical formulas.
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