Question

For the simple reaction \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\) list the types of bonds that must be broken and the types of bonds that must form for the chemical reaction to take place.

Short answer

For the reaction \( 2 \mathrm{CO}(g) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g) \), the bonds that must be broken are the triple bond in CO molecules (one sigma and two pi bonds between C and O atoms) and the double bond in O2 molecules (one sigma and one pi bond between O atoms). The bonds that must be formed are the double bonds in CO2 molecules (one sigma bond and one pi bond between the C atom and each O atom).

Step-by-step solution

Identify the reactants and products of the reaction

The given reaction is: \( 2 \mathrm{CO}(g) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g) \). Here, the reactants are Carbon Monoxide (CO) and Oxygen (O2) molecules, and the product formed is Carbon Dioxide (CO2) molecules.

Determine the types of bonds in the reactants

In the reactants, we have: 1. Carbon Monoxide (CO) molecule: Carbon Monoxide contains a triple bond between the Carbon (C) and Oxygen (O) atoms, which consists of one sigma bond and two pi bonds. 2. Oxygen (O2) molecule: Oxygen molecule contains a double bond between the two Oxygen (O) atoms, which consists of one sigma bond and one pi bond.

Determine the types of bonds in the product

The product is Carbon Dioxide (CO2) molecule: In Carbon Dioxide, there are two double bonds. Each double bond is between the Carbon (C) atom and an Oxygen (O) atom, and each double bond consists of one sigma bond and one pi bond.

List the types of bonds that must be broken

In order for the reaction to take place, the following bonds in the reactants must be broken: 1. The triple bond in CO: One sigma bond and two pi bonds between C and O atoms must be broken in both CO molecules. 2. The double bond in O2: One sigma bond and one pi bond between the two O atoms must be broken.

List the types of bonds that must be formed

As the product of the reaction is CO2, the following bonds must be formed: 1. Two double bonds in each CO2 molecule: One sigma bond and one pi bond between the C atom and each O atom must be formed. In summary, for the reaction \( 2 \mathrm{CO}(g) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g) \) to take place, the triple bond in CO molecules and the double bond in O2 molecule must be broken. Meanwhile, the double bonds in CO2 molecules must be formed.

Key concepts

Types of Chemical Bonds

Understanding the types of chemical bonds is fundamental to comprehending how chemical reactions occur. Essentially, chemical bonds are the attractive forces that hold atoms together in molecules. There are three primary types of chemical bonds: ionic, covalent, and metallic.

• Ionic bonds form between metals and non-metals where one atom donates electrons to another, leading to the formation of ions that attract each other due to their opposite charges.
• Covalent bonds occur between non-metal atoms where electrons are shared between atoms. This category also includes polar covalent bonds with unequal sharing leading to slight charges on atoms, and the nonpolar where electrons are shared equally.
• Metallic bonds are found in metals, where electrons form a 'sea' that is free-flowing around positively charged metal ions.

In the exercise example, the reaction involves breaking and forming of covalent bonds. Carbon monoxide (CO) has a triple bond—comprised of one sigma and two pi bonds—while oxygen (O2) has a double bond, with one sigma and one pi bond. These are examples of covalent bonds. In reactions, energy is needed to break these bonds, and energy is released when new bonds form.

Chemical Reactions

Chemical reactions involve the transformation of substances through the breaking of old bonds and the formation of new ones. The substances at the beginning are called reactants, and the resulting substances are called products. Reactions can be characterized by changes such as the release or absorption of energy, production of gas, formation of a precipitate, or color change.

There are several types of chemical reactions:

• Synthesis reactions, where simpler substances combine to form more complex molecules.
• Decomposition reactions, which involve a compound breaking down into simpler substances.
• Single replacement reactions, where an element in a compound is replaced by another element.
• Double replacement reactions, involving the exchange of components between two compounds.
• Combustion reactions, where a substance combines with oxygen, releasing energy as light and heat.

The exercise provided illustrates a synthesis reaction where carbon monoxide and oxygen combine to form carbon dioxide. Here, the bonds in the reactants are broken, and new bonds are formed to create the product.

Chemical Equation Balancing

Balancing chemical equations is a critical skill in chemistry that ensures the law of conservation of mass is upheld. This law states that matter cannot be created or destroyed in a chemical reaction. Hence, the number of atoms for each element must be the same on both sides of the equation.

To balance an equation, one must adjust the coefficients—the numbers in front of the compounds or elements in the reaction—to make sure that the same number of atoms of each element is present on both sides. Steps in balancing a chemical equation typically include:

• Determine the number of atoms of each element in the reactants and products.
• Adjust coefficients to get the same number of atoms on both sides.
• Start with the most complex molecule or the element that appears least frequently.
• Double-check that all elements are balanced, and make sure that the smallest set of whole numbers is used.

Referring to our exercise, the chemical equation is already balanced as written:
\(2 \text{ CO}(g) + \text{ O}_{2}(g) \rightarrow 2 \text{ CO}_{2}(g)\formatting-correct\).\formatting-correct\ This equation shows that two molecules of carbon monoxide react with one molecule of oxygen to produce two molecules of carbon dioxide, and it follows that there is an equal number of carbon and oxygen atoms on both sides of the equation.