Question

Give the systematic names for the formulas or the formulas for the names: (a) tin(IV) chloride; (b) FeBr \(_{3}\); (c) cuprous bromide; (d) \(\mathrm{Mn}_{2} \mathrm{O}_{3}\).

Short answer

a) SnCl_{4}, b) Iron(III) bromide, c) CuBr, d) Manganese(III) oxide

Step-by-step solution

Analyze the name 'tin(IV) chloride'

The name 'tin(IV) chloride' indicates the cation is tin with a charge of +4. Tin with a +4 charge is written as Sn^{4+}. The chloride anion has a charge of -1, written as Cl^{-}. To balance the charges, four chloride anions are needed. The formula is SnCl_{4}.

Determine the name for FeBr_{3}

Fe indicates iron, and Br is bromine. FeBr_{3} implies iron is in the +3 oxidation state to balance three bromides, each with a charge of -1. Thus, the name is iron(III) bromide.

Analyze the name 'cuprous bromide'

The term 'cuprous' indicates copper(I), which means copper has a +1 charge (Cu^{+}). Bromide has a charge of -1, written as Br^{-}. The formula reflecting a 1:1 ratio is CuBr.

Determine the name for Mn_{2}O_{3}

Mn indicates manganese, and O is oxygen. The formula Mn_{2}O_{3} suggests each manganese cation has a +3 charge to balance three oxide ions, each having a charge of -2. Thus, the name is manganese(III) oxide.

Key concepts

ionic compounds

Ionic compounds are chemical compounds composed of positively and negatively charged ions. These ions are held together by strong electrostatic forces, often referred to as ionic bonds.

In an ionic compound, the total positive charge of the cations equals the total negative charge of the anions, resulting in a neutral overall charge.

Common examples of ionic compounds include table salt (NaCl) and magnesium oxide (MgO).

• To write the formula of an ionic compound, always balance the charges of the cations and anions.
• For example, in tin(IV) chloride (SnCl₄), the tin ion (Sn⁴⁺) and four chloride ions (Cl^-) balance each other out, resulting in the formula SnCl₄.

oxidation states

Oxidation states (or oxidation numbers) indicate the degree of oxidation of an atom in a molecule. These are important for understanding the transfer of electrons in chemical reactions.

In simple terms, the oxidation state tells you how many electrons an atom has gained or lost compared to its neutral state.
For example:

• In FeBr₃, iron has an oxidation state of +3 because it has lost three electrons and each bromide ion (Br^-) has gained one electron.
• In Mn₂O₃, each manganese atom has an oxidation state of +3 to balance the -2 charge of each oxygen atom.

When naming compounds containing elements with variable oxidation states, use Roman numerals to indicate the specific state, as in iron(III) bromide for FeBr₃.

chemical formulas

Chemical formulas represent the types and numbers of atoms in a compound. For ionic compounds, these formulas are determined by balancing the positive and negative charges of the involved ions.

Key points to consider:

• Identify the cation and anion and their charges.
• Balance the total positive and negative charges.
• Write the cation first, followed by the anion.

For example, in cuprous bromide (CuBr), copper (Cu⁺) and bromide (Br^-) balance each other with a 1:1 ratio. Similarly, in Mn₂O₃, two manganese ions (Mn³⁺) balance three oxide ions (O^2-), resulting in the formula Mn₂O₃. Understanding chemical formulas helps in writing and interpreting chemical equations accurately.

transition metals

Transition metals are elements found in the middle of the periodic table, specifically in groups 3-12. They are known for their ability to form compounds with various oxidation states.

Characteristics of transition metals include:

• Multiple oxidation states, which allow for a variety of compounds.
• The ability to form colored compounds.
• Good conductors of electricity and heat.

For instance, iron (Fe) can have oxidation states such as +2 and +3, and manganese (Mn) can have states like +2, +3, +4, +6, and +7. This versatility makes transition metals essential in many chemical reactions and industrial applications.

In systematic naming, Roman numerals are used to indicate the specific oxidation state of the transition metal. As seen in the examples, iron(III) bromide (FeBr₃) and manganese(III) oxide (Mn₂O₃) clearly denote the oxidation states of the metals involved.