Chapter 7: Problem 112
Write chemical formulas for oxides of nitrogen with the following oxidation numbers: +1,+2,+3,+4,+5 . (Hint: There are two oxides of nitrogen with a +4 oxidation number.)
Short Answer
Expert verified
+1: N2O, +2: NO, +3: N2O3, +4: NO2 & N2O4, +5: N2O5.
Step by step solution
Over 22 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemical Formulas
Chemical formulas are representations of molecules using letters and numbers. They show which elements are present and how many atoms of each element are in a compound. The formula provides a concise way to convey information about a molecule's composition. For example, in the formula \(NO_2\), 'N' stands for nitrogen and 'O' stands for oxygen, while the numbers indicate the count of oxygen atoms combined with one nitrogen atom.
These formulas are essential in understanding chemical reactions and properties. By knowing a compound's formula, you can predict how it will react and what it will produce. It also helps identify the proportions of elements within the compound, which is critical for calculations in chemical equations.
These formulas are essential in understanding chemical reactions and properties. By knowing a compound's formula, you can predict how it will react and what it will produce. It also helps identify the proportions of elements within the compound, which is critical for calculations in chemical equations.
Oxides of Nitrogen
Oxides of nitrogen are chemical compounds composed of nitrogen and oxygen. Their chemical formulas vary depending on the oxidation state of the nitrogen atom. These compounds are significant in various chemical processes and have diverse applications.
Understanding these oxides helps predict their interactions in the environment and their effects on health and technology.
- Dinitrogen monoxide (\(N_2O\)), with a +1 oxidation number, is commonly known as laughing gas.
- Nitrogen monoxide (NO) features nitrogen in a +2 oxidation state and is a crucial molecule in biological signaling.
- Dinitrogen trioxide (\(N_2O_3\)) represents nitrogen in a +3 oxidation state and is less stable, typically existing under low-temperature conditions.
- The +4 oxidation state of nitrogen can produce nitrogen dioxide (NO2), a brown gas involved in air pollution, or dinitrogen tetroxide (\(N_2O_4\)), which is commonly used as a rocket propellant.
- Dinitrogen pentoxide (\(N_2O_5\)), where nitrogen exhibits a +5 oxidation number, is used in producing explosives and some organic compounds.
Understanding these oxides helps predict their interactions in the environment and their effects on health and technology.
Nitrogen Oxidation Numbers
Oxidation numbers, or states, reflect the charge of a nitrogen atom within a molecule based on electron distribution. In a compound, they help determine how atoms share electrons. The oxidation number of nitrogen varies from -3 to +5, based on its tendency to lose or gain electrons.
For oxides of nitrogen:
Grasping these numbers is vital for predicting how nitrogen compounds will form and interact with other elements.
For oxides of nitrogen:
- +1 oxidation number in \(N_2O\) indicates a slightly higher oxidation state leading to lesser electron sharing compared to elemental nitrogen.
- +2 in NO suggests that nitrogen shares electrons more equally with oxygen.
- +3 in \(N_2O_3\) indicates even lesser electron density around nitrogen showing a significant oxidation.
- +4 in NO2 or \(N_2O_4\) shows a strong tendency of nitrogen atoms to lose electrons while bonding with oxygen.
- +5 in \(N_2O_5\) reflects nitrogen's maximum oxidation state, meaning it shares more of its electrons with highly electronegative oxygen atoms.
Grasping these numbers is vital for predicting how nitrogen compounds will form and interact with other elements.
Chemical Compounds
Chemical compounds consist of two or more elements chemically bonded together, resulting in distinct molecules. They have fixed ratios and specific arrangements, which dictate their properties and chemical behavior.
Nitrogen oxides are an example of a class of compounds where nitrogen forms bonds with oxygen. Each compound demonstrates different properties due to varying nitrogen oxidation numbers. These differences affect their reactivity, stability, and applications.
For example:
Understanding chemical compounds and their formation is crucial in the study of chemistry, as it enables us to manipulate materials for desired outcomes such as medicine, environmental management, and industrial applications.
Nitrogen oxides are an example of a class of compounds where nitrogen forms bonds with oxygen. Each compound demonstrates different properties due to varying nitrogen oxidation numbers. These differences affect their reactivity, stability, and applications.
For example:
- \(N_2O\) is used medically for pain relief due to its anesthetic properties.
- NO, as a free radical, plays a role in various physiological processes but also contributes to atmospheric reactions.
- \(N_2O_3\) and NO2 are less stable but important in the formation of nitrate salts.
Understanding chemical compounds and their formation is crucial in the study of chemistry, as it enables us to manipulate materials for desired outcomes such as medicine, environmental management, and industrial applications.
