Question

Name each of the following compounds: a. \(\mathrm{CsF}\) b. b. \(\mathrm{Li}_{3} \mathrm{N}\) c. \(\mathrm{Ag}_{2} \mathrm{S}\) d. \(\mathrm{MnO}_{2}\) e. \(\mathrm{TiO}_{2}\) f. \(\mathrm{Sr}_{3} \mathrm{P}_{2}\)

Short answer

a. Cesium Fluoride b. Lithium Nitride c. Silver Sulfide d. Manganese(IV) Oxide e. Titanium(IV) Oxide f. Strontium Phosphide

Step-by-step solution

a. Naming CsF

Cs is Cesium and F is Fluorine. In an ionic compound, the metal (Cesium) is written first, followed by the non-metal (Fluorine). The non-metal's name gets slightly modified by adding the suffix "-ide," resulting in Fluoride. So, the compound's name is Cesium Fluoride.

b. Naming Li3N

Li is Lithium and N is Nitrogen. Following the same rules as above, the compound is named Lithium Nitride.

c. Naming Ag2S

Ag is Silver and S is Sulfur. Silver is a transition metal that typically forms a +1 ion, so there is no need to mention its charge. Thus, the compound is named Silver Sulfide.

d. Naming MnO2

Mn is Manganese and O is Oxygen. As Manganese is a transition metal, we must indicate the charge, or oxidation number, with a Roman numeral. Since each Oxygen atom has a charge of -2 and there are two Oxygen atoms, the Manganese must have a +4 charge. The compound is named Manganese(IV) Oxide.

e. Naming TiO2

Ti is Titanium and O is Oxygen. Titanium is also a transition metal, so we must indicate its charge. In this case, the two Oxygen atoms have a combined charge of -4, so the Titanium must have a +4 charge. The compound is named Titanium(IV) Oxide.

f. Naming Sr3P2

Sr is Strontium and P is Phosphorus. Here, Strontium is the metal and Phosphorus is the non-metal. The name of the non-metal element Phosphorus becomes Phosphide. The compound is named Strontium Phosphide.

Key concepts

Ionic Bonding

Ionic bonding is a type of chemical bond where there is a transfer of electrons from one atom to another. This process creates ions, which are atoms or molecules that carry a net electric charge. In an ionic bond, one atom will lose one or more electrons and become a positively charged ion, while another atom will gain those electrons and become a negatively charged ion. The attractive force between these oppositely charged ions results in a stable ionic compound. Ionic bonds usually form between metals and non-metals. Metals tend to lose electrons due to their low electronegativity, while non-metals tend to gain electrons because of their high electronegativity.

Common examples of ionic compounds include sodium chloride ( ext{NaCl}), potassium iodide ( ext{KI}), and the ones mentioned in the exercise like cesium fluoride ( ext{CsF}) and lithium nitride ( ext{Li}_{3} ext{N}). Such compounds are typically crystalline and have high melting and boiling points. Because ionic compounds are formed from charged ions, they can conduct electricity when dissolved in water or melted into a liquid.

Chemical Nomenclature

Chemical nomenclature is the set of rules used for naming chemical substances. Understanding these rules is crucial for writing and interpreting chemical formulas and names.

The basic rule for naming ionic compounds is to state the name of the positive ion (the cation), followed by the name of the negative ion (the anion). For monatomic ions, the cation retains its elemental name, while the anion's name is modified to end with the suffix "-ide." For example, in cesium fluoride ( ext{CsF}), cesium retains its name, and fluorine becomes fluoride.

• For polyatomic ions, different naming conventions apply, often based on the ion's overall charge and composition.
• Compounds involving transition metals require you to specify the metal's charge in the compound's name using Roman numerals.
• For example, in manganese(IV) oxide ( ext{MnO}_{2}), the charge of manganese is indicated as +4.

These rules ensure clarity and precision when communicating chemical compositions and reactions, making understanding the naming conventions essential for students and professionals in chemistry.

Transition Metals

Transition metals are elements found in the middle of the periodic table, in groups 3 through 12. They are characterized by having d-orbitals that are being filled with electrons. Because of their electron configurations, transition metals can have various oxidation states, which means they can lose different numbers of electrons. This property makes them versatile and widely used in different chemical reactions.

When naming compounds that include transition metals, it's important to indicate the oxidation number of the metal. This is done using Roman numerals in parentheses right after the metal's name. For example, in titanium dioxide ( ext{TiO}_{2}), titanium has an oxidation state of +4, thus the compound is called titanium(IV) oxide.

Unlike other metals, transition metals often form brightly colored compounds. They are also excellent conductors of electricity and heat, which is why they are commonly used in industrial processes, electronics, and catalysis. Knowing their oxidation states and how to properly name transition metal compounds is an essential skill in chemistry, especially in the context of understanding reactions and equations.