Problem 72 - Chemistry

Question

Name each of the following compounds. Assume the acids are dissolved in water. a. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) g. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) b. \(\mathrm{NH}_{4} \mathrm{NO}_{2}\) h. \(\mathrm{Sr}_{3} \mathrm{~N}_{2}\) c. \(\mathrm{Co}_{2} \mathrm{~S}_{3}\) i. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{3}\right)_{3}\) d. ICl j. \(\mathrm{SnO}_{2}\) e. \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) k. \(\mathrm{Na}_{2} \mathrm{Cr} \mathrm{O}_{4}\) f. \(\mathrm{KClO}_{3}\) 1\. \(\mathrm{HClO}\)

Step-by-Step Solution

Answer

a. Acetic Acid b. Ammonium Nitrite c. Cobalt(III) Sulfide d. Iodine Monochloride e. Lead(II) Phosphate f. Potassium Chlorate g. Sulfuric Acid h. Strontium Nitride i. Aluminum Sulfite j. Tin(IV) Oxide k. Sodium Chromate l. Hypochlorous Acid

Step 1: Identify the type of compound

This is an acid dissolved in water, so it has an -ic ending and the prefix hydro-.

Step 2: Name the compound

Since the ion is acetate (C₂H₃O₂⁻), we name it as Acetic Acid. b. \(\mathrm{NH}_{4} \mathrm{NO}_{2}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

It is composed of ammonium ions (NH₄⁺) and nitrite ions (NO₂⁻), so we call it Ammonium Nitrite. c. \(\mathrm{Co}_{2} \mathrm{~S}_{3}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound is composed of cobalt (Co) and sulfide (S²⁻) ions. Since the subscript for Co is 2 and for S is 3, we name it Cobalt(III) Sulfide. d. ICl

Step 1: Identify the type of compound

This is a covalent compound.

Step 2: Name the compound

The compound is formed by iodine (I) and chlorine (Cl). It is called Iodine Monochloride. e. \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound is made of lead (Pb) and phosphate ions (PO₄³⁻). Since the subscript for Pb is 3, we call it Lead(II) Phosphate. f. \(\mathrm{KClO}_{3}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound consists of potassium (K⁺) and chlorate (ClO₃⁻) ions. It is called Potassium Chlorate. g. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Step 1: Identify the type of compound

The compound is an acid dissolved in water.

Step 2: Name the compound

Since the anion is sulfate (SO₄²⁻), we call it Sulfuric Acid. h. \(\mathrm{Sr}_{3} \mathrm{~N}_{2}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound is composed of strontium (Sr) and nitride (N³⁻) ions. It is called Strontium Nitride. i. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{3}\right)_{3}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound consists of aluminum (Al³⁺) and sulfite (SO₃²⁻) ions. It is called Aluminum Sulfite. j. \(\mathrm{SnO}_{2}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

This compound is composed of tin (Sn) and oxide (O²⁻) ions. Since the subscript for O is 2, we call it Tin(IV) Oxide. k. \(\mathrm{Na}_{2} \mathrm{Cr} \mathrm{O}_{4}\)

Step 1: Identify the type of compound

This is an ionic compound.

Step 2: Name the compound

The compound is composed of sodium (Na⁺) and chromate (CrO₄²⁻) ions. It is called Sodium Chromate. l. \(\mathrm{HClO}\)

Step 1: Identify the type of compound

The compound is an acid dissolved in water.

Step 2: Name the compound

Since the anion is hypochlorite (ClO⁻), we call it Hypochlorous Acid.

Key Concepts

Acids

Acids are special types of compounds that release hydrogen ions (H⁺) when dissolved in water. They usually have one or more hydrogen atoms that are bonded to a non-metallic element. The classic naming convention depends on the type of anion present in the acid.

• For oxyacids, the name is based on the anion. If the anion ends with -ate, the acid name ends with -ic (e.g., sulfate ightarrow sulfuric acid). If the anion ends with -ite, it changes to -ous (e.g., sulfite ightarrow sulfurous acid).
• For binary acids that don't contain oxygen, the prefix 'hydro-' is used, followed by the root name of the non-metal and the suffix -ic, such as hydrochloric acid for HCl.

Acids have different strengths based on their ability to dissociate and release hydrogen ions. A well-known strong acid is sulfuric acid ( H_{2} SO_{4}), while acetic acid ( HC_{2}H_{3}O_{2}) is a weaker acid.

Ionic Compounds

Ionic compounds are composed of positively charged ions called cations and negatively charged ions called anions. These ions bind together due to opposite electrical charges, creating a strong ionic bond.

• The formula of an ionic compound reflects the ratio between the cations and anions, ensuring an overall neutral charge.
• When naming these compounds, the cation name is written first, followed by the anion. Simple anions take the suffix -ide, like chloride for Cl⁻. If the anion is a polyatomic ion, its name remains unchanged, such as sulfate (SO₄²⁻) or nitrate (NO₃⁻).

Examples include Sodium chromate ( Na_{2}CrO_{4}) and Ammonium nitrite ( NH_{4}NO_{2}). The naming tells you that Sodium interacts with chromate ions, and ammonium combines with nitrite ions in the compound.

Covalent Compounds

Covalent compounds, or molecular compounds, occur when atoms share electrons instead of transferring them. This kind of bonding often involves non-metal elements forming molecules.

• The naming of covalent compounds uses prefixes to indicate the number of each element within a molecule. For example, the prefix mono- indicates one, di- for two, tri- for three, and so on.
• Names are given based on the number of atoms. If only one atom of the first element is present, the prefix mono- is usually omitted. For instance, carbon monoxide (CO) and sulfur hexafluoride ( SF_{6}) follow this scheme.

Iodine monochloride (ICl) is a suitable example. Iodine binds with one chlorine atom, making it a simple diatomic molecule.

Transition Metals

Transition metals are unique elements found in the central block of the periodic table. Known for their ability to form various oxidation states, they make compounds that can be challenging to name due to variable charges.

• In naming compounds containing transition metals, Roman numerals in parentheses indicate the metal's oxidation state. Cobalt(III) sulfide ( Co_{2} S_{3}) demonstrates this as cobalt adopts the +3 charge.
• Transition metals frequently form colorful compounds and have a capacity to act in catalysis and electronic applications owing to their versatile electron configurations.

An example is Tin(IV) oxide ( SnO_{2}), where tin exists in a +4 oxidation state. The numerals help clarify which form of the metal is present, which is crucial due to the variety of oxidation states they might exhibit.