Question

Locate the following elements on the periodic table, and write the formula of a compound that justifies each of your answers: (a) Two nonmetals that can form more than four bonds (b) Two nonmetals that form a maximum of four bonds (c) Two nonmetals that form oxides that are gases at \(25^{\circ} \mathrm{C}\) (d) A nonmetal that forms an oxide that is a solid at \(25^{\circ} \mathrm{C}\)

Short answer

Phosphorus, Sulfur, Carbon, Nitrogen, Carbon Dioxide, Nitrogen Dioxide, Sulfur Trioxide.

Step-by-step solution

Identify Nonmetals That Can Form More Than Four Bonds

Phosphorus (P) and Sulfur (S) are nonmetals that can form more than four bonds. Phosphorus forms \[\text{PCl}_5\](Sulfur's oxide is a gas at room temperature, so it is not chosen here despite its ability to form more bonds with different elements like in SF_6).

Check Nonmetals Up to Four Bonds

Carbon (C) and Nitrogen (N) are nonmetals that form a maximum of four bonds. Their typical compounds include: \[\text{CH}_4\] and \[\text{NH}_3\].

Find Oxides of Nonmetals Gaseous at Room Temperature

Carbon dioxide (\[\text{CO}_2\]) and Nitrogen dioxide (\[\text{NO}_2\]) are both gases at \(25^{\circ} \text{C}\). These oxides correspond to carbon and nitrogen respectively.

Locate a Solid Nonmetal Oxide

Sulfur (S) forms sulfur trioxide (\[\text{SO}_3\]), which is a solid at \(25^{\circ} \text{C}\). This satisfies the criteria for a nonmetal forming a solid oxide.

Key concepts

Nonmetals

Nonmetals are a group of elements on the periodic table characterized by their inability to conduct electricity well and their tendency to form covalent bonds by sharing electrons. Nonmetals are found on the right side of the periodic table, with some common examples including oxygen (O), nitrogen (N), sulfur (S), and phosphorus (P). These elements usually have high electronegativities and ionization energies, meaning they tend to attract electrons rather than give them away.
Nonmetals are crucial in forming various compounds, like water (\(H_2O\) and carbon dioxide (\(CO_2\). These elements often combine with metals to form ionic compounds or with each other, forming covalent or molecular compounds. Their ability to form multiple bonds is pivotal in chemistry and biology, enabling the formation of complex molecules like proteins and DNA.

Chemical Bonds

Chemical bonds are the connections between atoms that hold molecules together. These bonds are formed by the sharing or transfer of electrons between atoms. There are three main types of chemical bonds: ionic, covalent, and metallic.

• Ionic Bonds: Formed when electrons are transferred from one atom to another, resulting in the formation of oppositely charged ions. These ions attract each other, forming a bond. A classic example is sodium chloride (table salt, \(NaCl\)).
• Covalent Bonds: Formed when atoms share electrons. Nonmetals typically form covalent bonds with each other. An everyday example is water (\(H_2O\)).
• Metallic Bonds: A bond found in metallic elements, where electrons are shared and dispersed over a lattice of metal atoms.

Understanding the type of chemical bond in a compound helps predict its properties like melting point, conductivity, and solubility. Nonmetals mainly form covalent bonds, crucial for forming essential life compounds, like carbohydrates and amino acids.

Oxides

Oxides are compounds that consist of oxygen and another element. They are classified based on the nature of the element bonded to oxygen, giving us nonmetallic oxides and metallic oxides. Nonmetal oxides often form acidic solutions in water. Here's more detailed information on different oxides:

• Nonmetal Oxides: These include well-known gases like carbon dioxide (\(CO_2\)) and nitrogen dioxide (\(NO_2\)). At room temperature (\(25^{ ext{\circ}}C\)), these compounds are gaseous. They appear as products in combustion processes and are involved in the greenhouse effect.
• Metallic Oxides: Typically solid at room temperature and can form bases when dissolved in water. For example, magnesium oxide (\(MgO\)) reacts with water to form magnesium hydroxide.
• Solid Nonmetal Oxides: An example is sulfur trioxide (\(SO_3\)), which forms solid structures at room temperature.

Understanding oxides is vital in chemistry for predicting reactions and understanding environmental phenomena like acid rain.

Chemical Formulas

Chemical formulas represent the proportions of elements in a compound. They provide insight into the composition and structure of molecules, using symbols and numbers to indicate the type and number of atoms present.

• Empirical Formulas: The simplest whole-number ratio of atoms in a compound, like \(CH_2O\) for glucose.
• Molecular Formulas: Provide the exact number of each type of atom in a molecule, such as \(C_6H_{12}O_6\) for glucose.
• Structural Formulas: Illustrate the specific arrangement of atoms within a molecule. This gives insight into how atoms are bonded and connected.

Chemical formulas are essential in finding the molar mass of compounds, balancing chemical equations, and understanding reaction stoichiometry. They are a fundamental part of learning chemistry, allowing students to predict the nature and behavior of chemical substances.