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Chapter 4: Problem 44

Give the oxidation number for the following species: \(\mathrm{H}_{2}, \mathrm{Se}_{8}, \mathrm{P}_{4}, \mathrm{O}, \mathrm{U}, \mathrm{As}_{4}, \mathrm{~B}_{12}\)

Short Answer

Expert verified
The oxidation numbers for the given species are: \(H_{2} = 0\), \(Se_{8} = 0\), \(P_{4} = 0\), \(O = 0\), \(U = 0\), \(As_{4} = 0\), \(B_{12} = 0\)

Step by step solution

01

Understand the concept of Oxidation Number

Oxidation number is the charge an atom would have if electrons in each bond were given to the more electronegative atom. For a molecule, sum of oxidation numbers of all the atoms is zero. For elements in their molecular form, the atoms are identical and there is no electronegativity difference so the bond is nonpolar, hence the atoms have oxidation state = 0.
02

Identify Oxidation Number for \(H_{2}\)

As \(H_{2}\) is an element in its molecular form which is hydrogen, its oxidation state is 0.
03

Identify Oxidation Number for \(Se_{8}\)

In \(Se_{8}\), which is an element in its molecular form (selenium), all selenium atoms have the same electronegativity, hence its oxidation state is 0.
04

Identify Oxidation Number for \(P_{4}\)

For \(P_{4}\), it is an element in its molecular form (phosphorus), its oxidation state is 0.
05

Identify Oxidation Number for \(O\)

The element \(O\) stands for oxygen. In its atomic form, its oxidation state is 0.
06

Identify Oxidation Number for \( U \)

The symbol \(U\) stands for Uranium. Its atomic form gives it an oxidation state of 0.
07

Identify Oxidation Number for \(As_{4}\)

As \(As_{4}\) is an element in its molecular form which is arsenic, its oxidation state is 0.
08

Identify Oxidation Number for \(B_{12}\)

In \(B_{12}\), it is an element in its molecular form (boron), hence its oxidation state is 0.

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Most popular questions from this chapter

Calculate the volume in \(\mathrm{mL}\) of a solution required to provide the following: (a) \(2.14 \mathrm{~g}\) of sodium chloride from a \(0.270 \mathrm{M}\) solution, (b) \(4.30 \mathrm{~g}\) of ethanol from a \(1.50 M\) solution, (c) 0.85 g of acetic acid ( \(\left.\mathrm{CH}_{3} \mathrm{COOH}\right)\) from a \(0.30 \mathrm{M}\) solution.

Based on oxidation number, explain why carbon monoxide (CO) is flammable but carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) is not.

What volume of a \(0.500 M \mathrm{HCl}\) solution is needed to neutralize each of the following: (a) \(10.0 \mathrm{~mL}\) of a \(0.300 \mathrm{M} \mathrm{NaOH}\) solution (b) \(10.0 \mathrm{~mL}\) of a \(0.200 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution

A \(1.00-\mathrm{g}\) sample of a metal \(\mathrm{X}\) (that is known to form \(\mathrm{X}^{2+}\) ions) was added to a \(0.100 \mathrm{~L}\) of \(0.500 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4}\). After all the metal had reacted, the remaining acid required \(0.0334 \mathrm{~L}\) of \(0.500 \mathrm{M} \mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the metal and identify the element.

A \(3.664-\mathrm{g}\) sample of a monoprotic acid was dissolved in water and required \(20.27 \mathrm{~mL}\) of a \(0.1578 \mathrm{M}\) \(\mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the acid.
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