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Chapter 5: Problem 122

What is a binary compound? Is atmospheric oxygen an example of a binary compound?

Short Answer

Expert verified
A binary compound is a chemical compound composed of exactly two different elements. Atmospheric oxygen (O2) is not a binary compound, as it consists of only one element (oxygen) with two atoms bonded together, making it a homoatomic compound.

Step by step solution

01

Definition of a Binary Compound

A binary compound is a chemical compound composed of exactly two different elements. These elements can be bonded together in various ways such as ionic or covalent bonds.
02

Atmospheric Oxygen

Atmospheric oxygen exists primarily as O2, which is two oxygen atoms bonded together. This is an example of a homoatomic compound, where all the atoms comprising the compound are of the same element.
03

Comparison

Since atmospheric oxygen (O2) consists of only one element (oxygen) even though it has two atoms bonded together, it cannot be considered a binary compound, as a binary compound must be composed of exactly two different elements.

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Key Concepts

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

Chemical Compound
A chemical compound is a substance formed when two or more elements chemically bond together. These bonds could be either ionic or covalent. When elements combine to form a compound, they create a substance with different properties than the individual elements.
Understanding chemical compounds is crucial in chemistry because they make up everything around us, from the water we drink to the materials in our smartphones.
There are different types of chemical compounds based on the number of elements involved and how they bond:
  • Binary Compounds: Composed of exactly two different elements. These can be further classified depending on their bonding, such as ionic or covalent.
  • Complex Compounds: Formed from three or more different elements, often with varying combinations of ionic and covalent bonds.
Learning about these compounds helps in predicting their behavior and properties.
Elements
Elements are pure substances consisting entirely of one type of atom. They serve as the building blocks for all matter, and each element is defined by its unique atomic number, which corresponds to the number of protons in its nucleus.
Elements can participate in forming compounds, though they cannot be broken down into simpler substances by chemical means.
In the periodic table, elements are organized in such a way that shows periodic trends, which helps us understand their properties and how they might interact to form compounds.
  • Hydrogen: The lightest and most abundant element in the universe.
  • Oxygen: An essential element in the formation of water, and crucial for respiration in many life forms.
  • Iron: A metallic element commonly used in construction and manufacturing.
Ionic Bonds
Ionic bonds form when one atom transfers one or more electrons to another atom, resulting in the creation of ions. These ions attract each other due to their opposite charges.
This type of bond is typical between metals and non-metals. Metals tend to lose electrons and become positively charged ions, whereas non-metals tend to gain electrons, becoming negatively charged ions.
The resulting compound is held together by strong electrostatic forces, leading to properties such as high melting and boiling points.
Common examples of ionic compounds include:
  • Sodium Chloride (NaCl): Commonly known as table salt, formed from sodium and chlorine.
  • Magnesium Oxide (MgO): Used in medicine and industry, formed from magnesium and oxygen.
Covalent Bonds
Covalent bonds occur when two atoms share one or more pairs of electrons. This form of bonding is prevalent between non-metal elements.
The shared electrons allow each atom to achieve a stable electron configuration, often filling their outer shells. Covalent bonds can be strong and durable, resulting in compounds with distinct properties, like lower melting and boiling points compared to ionic compounds.
  • Water (H2O): A molecule formed by sharing electrons between hydrogen and oxygen.
  • Carbon Dioxide (CO2): Consists of two double bonds between carbon and oxygen atoms.
This bond type is critical in forming the complex molecules necessary for life, like proteins and DNA.

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Most popular questions from this chapter

How does a polar covalent bond differ from. a covalent bond? Give examples of diatomic molecules that contain a polar covalent bond and of diatomic molecules that contain a covalent bond.

Draw a dot diagram for ethylene, \(\mathrm{C}_{2} \mathrm{H}_{4}\).

It is convenient to classify substances as ionic or covalent. How would you classify sodium sulfate? Explain fully.

Does \(\mathrm{BeH}_{2}\) have all of its atoms obeying the octet rule? If not, indicate which atom or atoms violate the octet rule and why it is OK.

Give the formulas for the following compounds: (a) Ammonium acetate (b) Ammonium carbonate (c) Iron(II) nitrate (d) Ferric hydroxide (e) Calcium hypochlorite
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