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Chapter 8: Problem 23

Give the names and formulas of two oxides of carbon.

Short Answer

Expert verified
The oxides are Carbon dioxide (\( \text{CO}_2 \)) and Carbon monoxide (\( \text{CO} \)).

Step by step solution

01

Understanding the Problem

The task is to identify and write down the names and chemical formulas of two different oxides of carbon. Oxides are compounds formed by the combination of oxygen with another element, in this case, carbon.
02

Determine the First Oxide

The most common oxide of carbon is carbon dioxide. It forms when carbon combusts in the presence of excess oxygen or during respiration. The chemical formula for carbon dioxide is \( \text{CO}_2 \).
03

Determine the Second Oxide

Another oxide of carbon is carbon monoxide, which forms when carbon burns in limited oxygen. This compound is often a byproduct of incomplete combustion. The chemical formula for carbon monoxide is \( \text{CO} \).
04

Conclusion

We have identified two oxides of carbon: Carbon dioxide with the formula \( \text{CO}_2 \) and carbon monoxide with the formula \( \text{CO} \).

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Key Concepts

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

Carbon Dioxide
Carbon dioxide is one of the most significant gases in Earth's atmosphere. This molecule, with the chemical formula \( \text{CO}_2 \), consists of one carbon atom covalently double bonded to two oxygen atoms. It plays a crucial role in Earth's carbon cycle and is vital for photosynthesis in plants. Additionally, carbon dioxide is a greenhouse gas, trapping heat in the atmosphere, which impacts global climate patterns.
In our everyday life, carbon dioxide is released during the breathing process and during the combustion of fossil fuels.
  • Carbon dioxide's chemical formula, \( \text{CO}_2 \), indicates its composition.
  • A key characteristic of this compound is its ability to dissolve in water forming carbonic acid, which contributes to the acidity of natural water bodies.
Understanding carbon dioxide's properties and its environmental impact is essential for addressing climate change.
Carbon Monoxide
Carbon monoxide is an odorless, colorless gas with the chemical formula \( \text{CO} \). It is composed of one carbon atom and one oxygen atom, linked by a triple covalent bond. Produced during the incomplete combustion of carbon-containing fuels, carbon monoxide is a dangerous pollutant.
Due to its ability to bind with hemoglobin in red blood cells, carbon monoxide can impede the transport of oxygen in the blood, leading to serious health risks such as carbon monoxide poisoning.
  • Its formula, \( \text{CO} \), signifies the unique bonding between its atoms.
  • Sources of carbon monoxide include vehicles, generators, and other appliances that burn fossil fuels.
Awareness and proper ventilation can prevent the dangers associated with this toxic gas.
Chemical Formulas
Chemical formulas serve as a shorthand way to represent chemical substances. In the case of carbon oxides, the formulas \( \text{CO}_2 \) and \( \text{CO} \) tell us the number and types of atoms in each compound.
These formulas not only indicate how many atoms of each element are present but also reveal the ratio of these atoms.
  • \( \text{CO}_2 \) means one carbon atom bonded to two oxygen atoms.
  • \( \text{CO} \) means one carbon atom bonded to one oxygen atom.
Chemical formulas provide a quick reference for understanding the structure and characteristics of compounds, which is essential in studying chemistry.
Oxidation States
The concept of oxidation states helps to describe the distribution of electrons among the atoms in a molecule. For carbon and its oxides, oxidation states can reveal how electrons are shared between carbon and oxygen.
In carbon dioxide \( \text{CO}_2 \), carbon is in a +4 oxidation state because it forms four bonds with oxygen, an element that typically has a -2 oxidation state. On the other hand, in carbon monoxide \( \text{CO} \), carbon holds a +2 oxidation state due to its dual combination of electrons with one oxygen atom.
  • Oxidation states help in determining the electron transfer during reactions.
  • They also assist in understanding the redox characteristics of a compound.
Learning about oxidation states can deepen our understanding of chemical reactions and the nature of compounds.

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Most popular questions from this chapter

The ground-state electron configuration of an atom is \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\). What is the valence-shell configuration of the atom in the same group, but in Period 5 ?

Theelectron affinity of the lutetium atom (element 71\()\) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using \(X\) rays). In this experiment, a beam of lutetium negative ions, \(\mathrm{Lu}^{-},\) was prepared and irradiated with a laser beam having a wavelength at \(1064 \mathrm{nm}\). The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of \(0.825 \mathrm{eV}\), what is the electron affinity of lutetium?

Write the orbital diagram for the ground state of the selenium atom. Give all orbitals.

As we noted at the beginning of Section \(8.2,\) an atom has an infinite number of electron configurations, including not just the ground state but excited states as well. The following are excited states of neutral atoms. Identify the element and write the ground-state electron configuration for that atom. a .\(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1} 4 p^{1}\) b. \(1 s^{1} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\) c. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{1}\) d. \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{2} 3 p^{1}\) e. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9} 4 s^{2} 4 p^{5}\)

A metallic element reacts vigorously with water, evolving hydrogen gas. An excited atom of this element has its outer electron in the \(3 p\) orbital. When this electron drops to its ground state in the \(3 s\) orbital, light is emitted of wavelength \(589 \mathrm{nm}\). What is the identity of the element? Explain how you arrived at your answer. What is the color of the emitted light?
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