Chemistry Chapter 7 Flashcards

Chemical Formulas and Compounds

• Chemical Formula: Represents the relative number of atoms of each kind in a chemical compound.
• Molecular Formula: Specifies the number of atoms of each element in a single molecule of the compound.

Types of Compounds

• Ionic Compound: Formed from a lattice of positively and negatively charged ions due to mutual electrostatic attraction.
• Formulas Unit: Indicates the simplest ratio of a compound's positive ions (cations) to negative ions (anions).
• Monatomic Ions: Ions created from a single atom, acting as building blocks for compounds.
• Binary Compounds: Compounds consisting of just two different elements, representing a fundamental type of chemical combination.

Nomenclature and Naming Systems

• Nomenclature: The naming convention for binary ionic compounds, combining cation and anion names, with cations named first.
• Stock System of Nomenclature: Utilizes oxidation numbers, with Roman numerals indicating an ion's charge, shown in parentheses after the metal's name.
• Old System for Naming Binary Molecules: Employs prefixes (mono, di, tri, etc.) to denote the number of each element; the second element's name ends in -ide.

Classes of Chemical Compounds

• Hydrocarbons: Molecular compounds that consist only of carbon and hydrogen atoms.
• Oxyanions: Polyatomic ions that contain oxygen, often integral in various chemical reactions.
• Acid: A class of compounds that usually refers to their aqueous solutions with specific properties, distinct from the pure compound.
• Binary Acids: Composed of two elements, typically hydrogen and one halogen (e.g., fluorine, chlorine).
• Oxyacids: Contain hydrogen, oxygen, and another element, often a nonmetal.

Additional Concepts

• Salt: An ionic compound formed from the reaction of an acid, generating a cation, and an anion from the acid.
• Oxidation Numbers/States: Indicate the degree of oxidation of an atom in a compound, essential for understanding electron transfer in reactions.
• Molecular Mass: The mass of a molecule, integral for calculations in stoichiometry.
• Formula Mass: Measured in amu, equal to the molar mass for a given compound.
• Molar Mass: Expressed in g/mol, numerically the same as formula mass, important for converting between mass and moles.
• Percentage Composition: Represents the mass percentage of each element present in a compound, useful for analysis.
• Empirical Formula: Shows the smallest whole-number mole ratio of the elements in a compound, possibly differing from the correct molecular formula.
• Molecular Formula: The actual formula that defines the composition of a molecular compound, revealing the true number of atoms involved.

Test your knowledge of chemical formulas and compounds with these flashcards from Chapter 7. Each card provides definitions essential for understanding the composition of various chemical substances. Perfect for students looking to reinforce their chemistry learning!