/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 92 What is the sum of the oxidation... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 92

What is the sum of the oxidation numbers of the atoms in a molecule?

Short Answer

Expert verified
Answer: The sum of the oxidation numbers in H2O is 0.

Step by step solution

01

Understanding Oxidation Numbers

Oxidation numbers are used to describe the distribution of electrons in a molecule. The oxidation number of an atom in a molecule is the charge that the atom would have if the electrons in the molecule were completely transferred to the atoms that have a greater affinity for electrons (i.e., the more electronegative atoms). Some general rules for assigning oxidation numbers are as follows: 1. For an atom in its elemental form, the oxidation number is always 0. 2. For a monatomic ion, the oxidation number equals the charge of the ion. 3. Oxygen usually has an oxidation number of -2, except in peroxides where it is -1. 4. Hydrogen usually has an oxidation number of +1 when bonded to non-metals and -1 when bonded to metals. 5. The oxidation number of other atoms depends on the specific compound.
02

Assigning Oxidation Numbers to Atoms in a Molecule

To assign oxidation numbers to the atoms in a molecule, we apply the general rules mentioned above and consider the electronegativity of the atoms involved. In some cases, such as polyatomic ions, the sum of the oxidation numbers of all the atoms in the ion must equal the charge of the ion. For example, let's consider the molecule H2O (water): 1. The oxidation number of hydrogen is +1. 2. The oxidation number of oxygen is -2.
03

Calculating the Sum of Oxidation Numbers in the Molecule

Now that we have assigned oxidation numbers to the atoms in the molecule, we can calculate the sum of the oxidation numbers. In our example, H2O, we have: Sum = (2 脳 +1) + (-2) Sum = 2 - 2 Sum = 0 The sum of the oxidation numbers in H2O is 0.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Chemical Bonding
Chemical bonding is the force that holds atoms together in a molecule. Atoms bond with each other to gain stability, often by achieving a full outer shell of electrons, similar to noble gases. There are several types of chemical bonds, including:
  • Ionic Bonds: Formed when electrons are transferred from one atom to another, leading to the formation of positive and negative ions. This bond type is typical between metals and non-metals.
  • Covalent Bonds: Involves the sharing of electron pairs between atoms. This form of bonding is usually found between non-metal atoms.
  • Metallic Bonds: Occurs in metals, where electrons are shared over many nuclei allowing them to conduct electricity and heat.
Chemical bonding is fundamental for understanding how molecules form and the properties they exhibit. It is crucial to know which type of bonding is present to determine the behavior and reactivity of the substance.
Electronegativity
Electronegativity refers to the tendency of an atom to attract electrons towards itself when it is part of a chemical bond. Atoms with high electronegativity pull electrons more strongly towards themselves, leading to polarity in covalent bonds. This can result in:
  • Polar Covalent Bonds: Where there is an unequal sharing of electrons. This creates a dipole moment where one side of the molecule is slightly positive and the other is slightly negative. Water is a classic example.
  • Nonpolar Covalent Bonds: Electron sharing is equal between atoms of similar electronegativity.
Electronegativity is a crucial concept when determining oxidation numbers. In any bond, the more electronegative atom gains a partial negative charge. This understanding helps in calculating electronic distribution and defining the nature of chemical interactions.
Oxidation States
Oxidation states, also known as oxidation numbers, are a way of keeping track of electrons during chemical reactions. They are particularly important in redox reactions where electron transfer occurs. Key points include:
  • An atom's oxidation state in its elemental form is zero.
  • For ions, the oxidation state equals the ion's charge.
  • In molecules, atoms have a range of oxidation states depending on their bonding and the overall charge of the ion or molecule.
The sum of oxidation numbers in a neutral molecule is zero. In polyatomic ions, the sum must equal the overall charge. Knowing the oxidation state helps in understanding how atoms interact, rearrange, and the role of each element in a compound.
Hydrogen and Oxygen Bonding
Hydrogen and oxygen often participate in forming water molecules, a classic example of hydrogen and oxygen bonding. Each water molecule consists of two hydrogen atoms and one oxygen atom. Here鈥檚 how their bonding works:
  • Oxygen's Role: Oxygen is highly electronegative and attracts electrons more strongly than hydrogen, creating a polar covalent bond. This makes the oxygen side more negative compared to the hydrogen end.
  • Hydrogen's Role: In water (H鈧侽), each hydrogen atom shares its electron with oxygen, resulting in two hydrogen-oxygen polar covalent bonds. The oxidation number for hydrogen here is +1, while it is -2 for oxygen.
This differences in electronegativity leads to water's distinct polar nature, which is responsible for its solvent properties and ability to dissolve various substances, defining its critical role in chemical reactions and biological systems.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Synthesis and Toxicity of Chlorine Chlorine was first prepared in 1774 by heating a mixture of \(\mathrm{NaCl}\) and \(\mathrm{MnO}_{2}\) in sulfuric acid: \(\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnO}_{2}(s) \rightarrow\) $$ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Cl}_{2}(g) $$ a. Assign oxidation numbers to the elements in each compound, and balance the redox reaction in acid solution. b. Write a net ionic equation describing the reaction for formation of chlorine. c. If chlorine gas is inhaled, it causes pulmonary edema (fluid in the lungs) because it reacts with water in the alveolar sacs of the lungs to produce the strong acid HCl and the weaker acid HOCl. Balance the equation for the conversion of \(\mathrm{Cl}_{2}\) to \(\mathrm{HCl}\) and \(\mathrm{HOCl}\).

The water-soluble uranyl cation, \(\mathrm{UO}_{2}^{+}\), can be removed by reaction with methane gas: $$ \mathrm{UO}_{2}^{+}(a q)+\mathrm{CH}_{4}(g) \rightarrow \mathrm{UO}_{2}(s)+\mathrm{HCO}_{3}^{-}(a q) $$ a. Assign oxidation numbers to the reactants and products. b. Balance the equation in acidic solution. c. How many electrons are transferred for each atom of uranium that reacts?

What is the difference between a strong acid and a weak acid?

Fuel Cells The electrolyte in an electricity-generating device called a fuel cell consists of a mixture of \(\mathrm{Li}_{2} \mathrm{CO}_{3}\) and \(\mathrm{K}_{2} \mathrm{CO}_{3}\) heated to \(650^{\circ} \mathrm{C} .\) At this temperature the ionic solids melt. Explain how this mixture of molten carbonates can conduct electricity.

Give the oxidation number of nitrogen in each of the following: (a) elemental nitrogen \(\left(\mathrm{N}_{2}\right) ;\) (b) hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right) ;(\mathrm{c})\) ammonium ion \(\left(\mathrm{NH}_{4}^{+}\right)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.