Question

State how each of the following is used in naming inorganic compounds: ide, ous, ic, hypo, per, ite, ate, Roman numerals.

Short answer

'-ide' is used for anions, '-ous' and '-ic' for acids/salts with lower and higher oxidation states, 'hypo-' and 'per-' for even lower and higher oxidation states, '-ite' and '-ate' for salts/oxyanions with lower and higher oxidation states, and Roman numerals indicate the oxidation state of metals in compounds with multiple oxidation states.

Step-by-step solution

Understanding 'ide'

The suffix '-ide' is used to name simple anions and monatomic ions (ions consisting of only one atom). For example, Cl- is called chloride, and O2- is called oxide.

Understanding 'ous' and 'ic'

The suffixes '-ous' and '-ic' are used in the naming of inorganic acids and their corresponding salts to indicate the oxidation state of the nonmetal in the acid. 'Ous' indicates a lower oxidation state, while 'ic' indicates a higher oxidation state. For example, H2SO3 is sulfurous acid and H2SO4 is sulfuric acid.

Understanding 'hypo' and 'per'

The prefixes 'hypo-' and 'per-' are used with '-ous' and '-ic' to indicate even lower or higher oxidation states, respectively. For example, HClO is hypochlorous acid, and HClO4 is perchloric acid.

Understanding 'ite' and 'ate'

The suffixes '-ite' and '-ate' are used to name the salts and oxyanions of elements. The '-ite' indicates a lower oxidation state than '-ate'. For example, NO2- is nitrite and NO3- is nitrate.

Understanding Roman numerals

Roman numerals are used in the names of coordination compounds and to indicate the oxidation number of the metal when the metal can exist in more than one oxidation state. For example, FeCl2 is iron(II) chloride and FeCl3 is iron(III) chloride.

Key concepts

Chemical Nomenclature

Chemical Nomenclature involves a systematic process for naming chemical compounds and is crucial for clear communication in the field of chemistry. Understanding the suffix 'ide' is the first step - it's usually used for simple, negatively charged ions (anions). Monatomic anions like Cl- (chloride) and O2- (oxide) are examples.
In naming molecular compounds, we use prefixes to indicate the number of atoms present. This is common in covalent compounds, for instance, CO is carbon monoxide while CO2 is carbon dioxide.
It is also important to know the difference between binary compounds (like NaCl, sodium chloride) and more complex compounds like KNO3 (potassium nitrate), where a metal is bonded to an oxyanion. Grasping these basics can significantly simplify the naming process for students.

Oxidation States

Understanding oxidation states is key when dealing with inorganic compounds. This concept refers to the effective charge of an element when electrons are assumed to be either completely gained or lost, determined by a set of rules.
The suffixes '-ous' and '-ic' signify different oxidation states: 'ous' indicating a lower oxidation state (for example, in ferrous Fe²⁺, compared to ferric Fe³⁺, which is 'ic') and 'ic' indicating a higher oxidation state. In the case of transition metals that exhibit multiple oxidation states, Roman numerals come into play: FeCl₂ is named iron(II) chloride because iron is in the +2 oxidation state, while FeCl₃ is named iron(III) chloride for the +3 oxidation state.

Inorganic Acids and Salts

Inorganic Acids and their salts follow distinctive naming conventions. Prefixes like 'hypo-' and 'per-' along with suffixes '-ous' and '-ic' are crucial for these names. The pattern here is based on the amount of oxygen in the acid: 'hypo-' signifying the least, and 'per-' the most.
For example, HClO (hypochlorous acid) has less oxygen than HClO₂ (chlorous acid), which has lower oxygen content than HClO₃ (chloric acid), and the most oxygen is found in HClO₄ (perchloric acid). Identifying these patterns helps to infer both the name and the formula of the acids and salts in question. Moreover, the corresponding salts for these acids end in '-ite' or '-ate' depending on whether the acid they derive from ends with '-ous' or '-ic', respectively.

Oxyanions

Oxyanions are negatively charged polyatomic ions that include oxygen. The names for these ions end with '-ite' for a lower oxidation state, or '-ate' for a higher one. For instance, SO₃^2- is known as sulfite and SO₄^2- as sulfate, pointing out the difference in oxygen content.
In these cases, the 'ite' suffix indicates one less oxygen atom than 'ate'. Recognizing and memorizing common oxyanions like nitrite (NO₂^-) and nitrate (NO₃^-), and their respective oxidation states can greatly enhance a student’s ability to name compounds containing these ions.