Chemistry Acids Quiz

Acids

• Acids are covalent compounds that ionize in water.
• They contain hydrogen ions (H⁺) that dissociate in water.
• The general formula for an acid's ionization is: Acid → H⁺ + anion
• Hydrogen ions are responsible for the acidic properties.

Binary Acids

• Contain only two elements (no oxygen).
• Names begin with "hydro" and end with "-ic" acid.
• Example: HCl (Hydrochloric acid)

Tertiary Acids

• Contain three or more elements, including oxygen.
• Two types:
  • "ic" acids: derived from polyatomic anions with "-ate" endings. Example: H₂SO₄ (Sulfuric acid), derived from the sulfate ion (SO₄²⁻).
  • "ous" acids: derived from polyatomic anions with "-ite" endings. Example: H₂SO₃ (Sulfurous acid), derived from the sulfite ion (SO₃²⁻).

Important Examples of Acids

• Nitric acid (HNO₃): derived from nitrate ion (NO₃⁻)
• Nitrous acid (HNO₂): derived from nitrite ion (NO₂⁻)
• Acetic acid (CH₃COOH or HC₂H₃O₂): derived from acetate ion (C₂H₃O₂⁻)
• Phosphoric acid (H₃PO₄): derived from phosphate ion (PO₄³⁻)
• Phosphorous acid (H₃PO₃): derived from phosphite ion (PO₃³⁻)
• Carbonic acid (H₂CO₃): derived from carbonate ion (CO₃²⁻)

Molecular Compounds

• Made of two or more nonmetal elements.
• Often exist as molecules.
• Examples: H₂O, CO₂, H₂SO₄, CH₄

Properties of Molecular Compounds

• Typically have low melting and boiling points.
• Generally exist as liquids or gases at room temperature.
• Atoms share electrons to achieve a full valence shell (no ions involved).

Covalent Bonding

• Atoms share electrons to achieve a full valence shell.
• The sharing of electrons forms the covalent bond.

Electronegativity

• A measure of an element's ability to attract electrons in a chemical bond.
• Atoms of the same element share electrons equally (non-polar bonds).
• Atoms of different elements share electrons unequally (polar bonds).
• The element with higher electronegativity attracts electrons more strongly, creating partial charges in the bond.

Polar Bonds and Water

• Water's polar O-H bonds contribute to its unique properties (e.g., expansion upon freezing, high boiling point).

Molecular Geometry

• Electron pairs arrange themselves around a central atom to maximize distance.
• The basic shape is a tetrahedron (central atom with 4 electron pairs).
• Lone electron pairs affect the shape of molecules.

Naming Chemical Compounds

• Ionic compounds: Metal-nonmetal (ide)
• Ionic compounds: Metal-polyatomic ion
• Ionic compounds: Transition metal (Roman numeral) nonmetal or polyatomic ion
• Covalent compounds: Use prefix system (e.g., mono-, di-, tri-, etc.) to indicate the number of atoms of each element. Use "ide" ending for second element. Omit "mono-" if only one atom of the first element.
• Acids: If starts with hydrogen, determine if it is a binary acid (hydro- + base name + -ic acid) or a ternary acid (base name + -ic or -ous acid depending on the anion ending with "-ate" or "-ite").

###Naming Covalent Compounds(Examples)

• Cl₂O₈: Dichlorine octoxide
• Si₃N₄: Trisilicon tetranitride
• CO: Carbon monoxide

Distinguishing Between Ionic and Covalent Compounds

• Use the rules and examples to identify whether a compound is ionic or covalent from its formula. Understand the differences in their structure and bonding to accurately classify.

Test your knowledge on the properties and types of acids. This quiz covers both binary and tertiary acids, as well as important examples and their formulas. Assess your understanding of acid ionization and nomenclature.