Question

Name the following compounds: (a) \(\mathrm{KClO},(\mathrm{b}) \mathrm{Ag}_{2} \mathrm{CO}_{3},\) (c) \(\mathrm{HNO}_{2}\) (d) \(\mathrm{KMnO}_{4},\) (e) \(\mathrm{CsClO}_{3},(\mathrm{f}) \mathrm{KNH}_{4} \mathrm{SO}_{4}\) (g) FeO, (h) \(\mathrm{Fe}_{2} \mathrm{O}_{3},\) (i) \(\mathrm{TiCl}_{4},(\mathrm{j}) \mathrm{NaH},(\mathrm{k}) \mathrm{Li}_{3} \mathrm{~N},\) (I) \(\mathrm{Na}_{2} \mathrm{O},(\mathrm{m}) \mathrm{Na}_{2} \mathrm{O}_{2}\)

Short answer

(a) Potassium Hypochlorite, (b) Silver Carbonate, (c) Nitrous Acid, (d) Potassium Permanganate, (e) Cesium Chlorate, (f) Potassium Ammonium Sulfate, (g) Iron(II) Oxide, (h) Iron(III) Oxide, (i) Titanium(IV) Chloride, (j) Sodium Hydride, (k) Lithium Nitride, (l) Sodium Oxide, (m) Sodium Peroxide.

Step-by-step solution

Identify Compound Components for (a)

The compound \( \text{KClO} \) consists of potassium (K) and the chlorate ion (ClO). We'll name it 'Potassium Hypochlorite' since \( \text{ClO}^- \) is known as the hypochlorite ion.

Identify Compound Components for (b)

The compound \( \text{Ag}_{2}\text{CO}_{3} \) consists of silver (Ag) and the carbonate ion (CO)\(_3\). Thus, it is named 'Silver Carbonate' as \( \text{CO}_{3}^{2-} \) represents the carbonate ion.

Identify Compound Components for (c)

The compound \( \text{HNO}_{2} \) contains hydrogen (H) and the nitrite ion (NO)\(_2\). It is named 'Nitrous Acid', since \( \text{HNO}_{2} \) is the acid form where \( \text{NO}_{2}^{-} \) is the nitrite ion.

Identify Compound Components for (d)

The compound \( \text{KMnO}_{4} \) includes potassium (K) and the permanganate ion (MnO)\(_4\). The name is 'Potassium Permanganate' because MnO\(_4^\text{-}\) is known as the permanganate ion.

Identify Compound Components for (e)

The compound \( \text{CsClO}_{3} \) has cesium (Cs) and the chlorate ion (ClO)\(_3\). Therefore, it is called 'Cesium Chlorate', as ClO\(_3^-\) is the chlorate ion.

Identify Compound Components for (f)

The compound \( \text{KNH}_{4} \text{SO}_{4} \) contains potassium (K), ammonium ion (NH)\(_4^+\), and the sulfate ion (SO)\(_4^2^-\). It is named 'Potassium Ammonium Sulfate' since NH\(_4^+\) is the ammonium ion and \( \text{SO}_{4}^{2-} \) is the sulfate ion.

Identify Compound Components for (g)

The compound \( \text{FeO} \) consists of iron (Fe) and oxygen (O), and since iron has a charge of 2+ in this compound, the oxide ion has a charge of 2-. Therefore, it is 'Iron(II) Oxide'.

Identify Compound Components for (h)

The compound \( \text{Fe}_{2} \text{O}_{3} \) consists of iron (Fe) and oxygen (O). Iron has a charge of 3+ in this compound making it 'Iron(III) Oxide', as each Fe\(^{3+}\) pairs with O\(^{2-}\) in a 2:3 ratio.

Identify Compound Components for (i)

The compound \( \text{TiCl}_{4} \) includes titanium (Ti) and chlorine (Cl). Since titanium is in the 4+ oxidation state here, it is 'Titanium(IV) Chloride'.

Identify Compound Components for (j)

The compound \( \text{NaH} \) contains sodium (Na) and hydrogen (H). It is 'Sodium Hydride' because \( \text{H}^- \) represents the hydride ion.

Identify Compound Components for (k)

The compound \( \text{Li}_{3} \text{N} \) includes lithium (Li) and nitrogen (N). The name is 'Lithium Nitride', resulting from the nitride ion N\(^{3-}\) combining with Li\(^+\).

Identify Compound Components for (l)

The compound \( \text{Na}_{2} \text{O} \) consists of sodium (Na) and oxygen (O). It is called 'Sodium Oxide', reflecting the oxide ion O\(^{2-}\).

Identify Compound Components for (m)

The compound \( \text{Na}_{2} \text{O}_{2} \) includes sodium (Na) and the peroxide ion (O)\(_2^{2-}\). Thus, it is named 'Sodium Peroxide'.

Key concepts

Chemical Nomenclature

Chemical nomenclature refers to the systematic naming of chemical compounds, which ensures a standardization important for global communication. It is governed primarily by the International Union of Pure and Applied Chemistry (IUPAC) rules. Depending on the type of compound, different naming protocols are followed:

• Binary Ionic Compounds: These are typically named by first stating the metal (cation) followed by the non-metal (anion) with an "-ide" suffix.
• Polyatomic Compounds: Here, rather than changing the suffix of the anion, the whole common name of the polyatomic ion is retained.
• Transition Metals: For compounds containing transition metals, the oxidation state of the metal is included in the name, using Roman numerals in parentheses.

Understanding these basic rules helps in accurately determining the name of a given compound.

Ionic Compounds

Ionic compounds are formed when metals transfer electrons to non-metals, resulting in cations and anions that are held together by strong electrostatic forces. These compounds often form crystalline solids and have high melting and boiling points.

• Formation of Ionic Compounds: Typically involves a metal losing electrons to become a positively charged cation, while a non-metal gains those electrons to form a negatively charged anion.
• Properties: Ionic compounds tend to be soluble in water and conduct electricity when in a liquid state or dissolved in water, thanks to the mobility of ions.
• Examples: Familiar everyday ionic compounds include sodium chloride (NaCl), commonly known as table salt.

Recognizing the nature and properties of ionic compounds is key to understanding their behavior in various chemical contexts.

Polyatomic Ions

Polyatomic ions are charged entities composed of two or more atoms covalently bonded, but they behave as a single ion when forming compounds. These ions add complexity to the nomenclature and chemical behavior of ionic compounds.

• Common Polyatomic Ions: Examples include sulfate (SO extsubscript{4} extsuperscript{2-}), nitrate (NO extsubscript{3} extsuperscript{-}), and ammonium (NH extsubscript{4} extsuperscript{+}).
• Naming Compounds with Polyatomic Ions: The name of the cation comes first, followed by the name of the polyatomic ion, preserving its full name rather than altering the ending.
• Chemical Reactions: Polyatomic ions often participate in chemical reactions as entire units, which means they maintain their internal connectivity and charge throughout reactions.

Knowing how to work with polyatomic ions is crucial for mastering chemical nomenclature and reactivity.

Oxidation States

An oxidation state, sometimes referred to as oxidation number, indicates the degree of oxidation of an atom within a compound. It is a hypothetical charge that an atom would have if all bonds to atoms of different elements were fully ionic.

• Determining Oxidation States: Use rules such as assigning oxygen a state of -2, hydrogen +1, and their sums in compounds equalling the total charge of the molecule.
• Purpose: Helps in understanding redox reactions, where electrons are transferred between species leading to oxidation and reduction.
• Notation in Nomenclature: Especially vital for transition metals, where a specific oxidation state must be indicated to distinguish between multiple potential forms, such as Iron(II) and Iron(III).

Mastering oxidation states is an essential skill for predicting the outcome of chemical reactions and for accurately naming compounds.