Chemistry: Naming Compounds and Ions

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Questions and Answers

What suffix designation is used for the higher oxidation state in the classical nomenclature system?

-ic (correct)

-ide

-ous

-ate

Which of the following is true regarding the Roman numeral notation in the IUPAC system?

It is used exclusively for polyatomic ions.

It always precedes the elemental name.

It indicates the oxidation number of multivalent cations. (correct)

Only Latin names are allowed in this system.

How are oxyacids named according to the type of polyatomic ion they contain?

They use '-ic' for ions ending in -ate. (correct)

They do not utilize any suffix but simply list the ions.

They follow the pattern of -ous acid for -ate ions.

They always include the suffix '-ide'.

In the case of compounds containing hydrogen, when is hydrogen listed first in the compound name?

When hydrogen has a lower electronegativity. Signup and view all the answers

Which of the following correctly represents a multivalent cation?

Fe2+ represents iron with oxidation state 2. Signup and view all the answers

What is the correct name for the compound HCl in aqueous solution?

Hydrochloric Acid Signup and view all the answers

What is the characteristic of hydrated compounds?

They incorporate water into their crystal structure. Signup and view all the answers

Which of the following represents the naming convention for a compound with a polyatomic ion?

May use parentheses if charge changes. Signup and view all the answers

What is the correct name for the compound CoCl2 · 2 H2O?

Cobalt(II) chloride dihydrate Signup and view all the answers

In the combustion reaction of C2H6, what are the products formed?

Carbon dioxide and water Signup and view all the answers

Which of the following is a characteristic of a synthesis reaction?

Two or more reactants combine to form one product Signup and view all the answers

What is a key feature of special decomposition reactions involving metal hydroxides?

They result in a metal oxide and water Signup and view all the answers

What is the balanced form of the decomposition reaction for MgCO3?

MgCO3(s) -> MgO(s) + CO2(g) Signup and view all the answers

Which reaction type is characterized by a single metal or non-metal combining with a molecule?

Single displacement Signup and view all the answers

How should you represent an unbalanced equation?

Skeleton equation Signup and view all the answers

When a non-metal oxide reacts with water, what type of product is expected?

Acid Signup and view all the answers

Study Notes

Naming Compounds

Ionic Compounds: Use the names of the cation and anion.
Polar Covalent Compounds: Use prefixes to indicate the number of atoms of each element.
Pure Covalent Compounds: Use prefixes to indicate the number of atoms of each element, except if the first element is only one atom then "mono" is omitted.

Multivalent Cations

Multivalent cations are elements that can form more than one stable positive ion.
Common examples:
- Iron (Fe): Fe²⁺ (ferrous) or Fe³⁺ (ferric)
- Copper (Cu): Cu⁺ (cuprous) or Cu²⁺ (cupric)
- Lead (Pb): Pb²⁺ (plumbous) or Pb⁴⁺ (plumbic)

Classical Naming System

Uses suffixes "-ic" (higher oxidation state) or "-ous" (lower oxidation state) for Latin names of multivalent cations.
Example:
- FeCl₃: Ferric Chloride
- FeCl₂: Ferrous Chloride

IUPAC Naming System

Uses Roman numerals to indicate the oxidation state of multivalent cations.
Does not use Latin names.
Example:
- FeCl₃: Iron (III) Chloride
- FeCl₂: Iron (II) Chloride

Polyatomic Ions

Treated as monatomic ions with brackets and oxidation number.
Most common polyatomic ions end in "-ate".
Examples:
- PO₄^3-: Phosphate
- SO₄^2-: Sulfate
- CO₃^2-: Carbonate
- NO₃^-: Nitrate

Prefixes for Polyatomic Ions

Hypo___ite: Two fewer Oxygen atoms than the base form
___ite: One fewer Oxygen atom than the base form
___ate: Base form
Per___ate: One more Oxygen atom than the base form
Examples:
- Hypochlorite (ClO^-)
- Chlorite (ClO₂^-)
- Chlorate (ClO₃^-)
- Perchlorate (ClO₄^-)

Compounds Containing Hydrogen

If Hydrogen has a lower electronegativity than the other element, it is written first. E.g. HCl (Hydrogen Chloride)
If Hydrogen has a higher electronegativity than the other element, it is written last and ends in "-ide". E.g. LiH (Lithium Hydride)

Haloacids

Compounds containing Hydrogen with a halide ion (F, Cl, Br, I).
Named as "Hydrogen _-ide", e.g. Hydrogen Bromide.
In aqueous solution, they become acids called "Hydro_ic Acid", e.g. Hydrochloric Acid.
Example:
- HCl (Hydrogen Chloride)
- HCl(aq) (Hydrochloric Acid)

Oxyacids

Acids containing oxygen.
Named as "Hydrogen (name of polyatomic ion)".
Example: H₂SO₄ (Hydrogen Sulfate)
Named as "Hypo___ous Acid", "___ous Acid", "___ic Acid", "Per___ic Acid".
Example:
- Hypochlorous Acid (HClO(aq))
- Nitrous Acid (HNO₂(aq))
- Sulfuric Acid (H₂SO₄(aq))
- Perchloric Acid (HClO₄(aq))

Hydrated Compounds

Ionic compounds that incorporate water molecules into their crystal structure.
Named by adding "hydrate" after the name of the compound.
Example: CoCl₂ · 2H₂O (Cobalt (II) Chloride Dihydrate)

Types of Reactions

Combustion: A hydrocarbon molecule reacts with oxygen to produce carbon dioxide, water, and energy.
Synthesis: Two or more reactants combine to form a larger product.
Decomposition: A product splits into two or more reactants.
Single Displacement: A single metal or non-metal combines with a molecule.

Combustion

In complete combustion, enough oxygen is present to produce CO₂ and H₂O.
Incomplete combustion occurs when there is not enough oxygen, resulting in products like carbon and carbon monoxide.

Synthesis

Also called a formation reaction.
Example:
- C(s) + O₂(g) → CO₂(g)
- 2Na(s) + Cl₂(g) → 2NaCl(aq)

Special Synthesis

Non-metal oxides (e.g. CO₂) with water form acids.
- CO₂(g) + H₂O(l) → H₂CO₃(aq)
Metal oxides (e.g Li₂O) with water form bases.
- Li₂O(s) + H₂O(l) → 2LiOH(aq) + H₂

Decomposition

Binary Decomposition: A compound breaks down into its elements.
- 2NaCl(aq) → 2Na + Cl₂
Metal Nitrate Decomposition: Decomposes into metal nitrite and oxygen gas.
- 2NaNO₃(s) → 2NaNO₂(s) + O₂(g)
Metal Carbonate Decomposition: Decomposes into metal oxide and carbon dioxide.
- MgCO₃(s) → MgO(s) + CO₂(g)
Metal Hydroxide Decomposition: Decomposes into metal oxide and water.
- 2LiOH → Li₂O + H₂O

Special Decomposition

Metal hydroxides decompose into metal oxides and water.
- 2NaOH(s) → Na₂O(s) + H₂O(l)
Acids decompose into non-metal oxides and water.
- H₂CO₃(aq) → CO₂(g) + H₂O(l)

Important Notes

(s) = Solid
(g) = Gas
(l) = Liquid
(aq) = Aqueous solution
N.R = No reaction
Unbalanced equations are called skeleton equations.
Acids contain hydrogen and look like HF(aq).
Bases contain hydroxide and look like KOH(aq).

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Description

This quiz covers the essential rules for naming ionic, polar covalent, and pure covalent compounds. Additionally, it explores the nomenclature of multivalent cations and the differences between classical and IUPAC naming systems. Test your understanding of chemical nomenclature in this informative quiz.