Physical and Chemical Properties of Matter

This page delves deeper into the properties of matter, distinguishing between physical and chemical properties. Understanding these properties is crucial for solving stoichiometry problems and answers.

Definition: Physical properties are observed without changing the identity and composition of the substance.

Examples of physical properties include color, odor, density, melting point, boiling point, and hardness.

Definition: Chemical properties describe how a substance may change or react to form other substances.

Chemical properties include flammability, corrosiveness, and reactivity with acids.

The page also introduces intensive and extensive properties:

• Intensive properties are independent of the amount of substance present $e.g., temperature, melting point$
• Extensive properties depend on the amount of sample $e.g., mass, volume$

Highlight: Understanding the difference between physical and chemical changes is essential for stoichiometric calculations.

The text explains dissociation and introduces the concept of electrolytes, which is important for understanding reactions in aqueous solutions.

Vocabulary: An electrolyte dissociates into ions when dissolved in water.

This information is crucial for performing stoichiometric calculations with chemical formulas and equations involving ionic compounds.

Classification of Matter and Measurement Units

This page provides a comprehensive overview of the classification of matter and introduces important measurement units used in general chemistry stoichiometry calculations.

The classification of matter is presented in a hierarchical structure:

1. Matter
2. Mixture $Heterogeneous or Homogeneous$ or Pure Substance
3. Element or Compound

Example: Water $H₂O$ is an example of a pure substance that is a compound.

The page introduces important prefixes used in the metric system, which are essential for stoichiometric calculations:

• Kilo $10³$, Mega $10⁶$, Giga $10⁹$, Tera $10¹²$, Peta $10¹⁵$
• Deci $10⁻¹$, Centi $10⁻²$, Milli $10⁻³$, Micro $10⁻⁶$, Nano $10⁻⁹$

Highlight: Understanding unit conversions is crucial for solving stoichiometry problems and answers.

The text also covers temperature conversions between Kelvin, Celsius, and Fahrenheit scales, which are often used in stoichiometric calculations.

Example: K = °C + 273.15

Lastly, the page introduces the concept of significant figures, which is essential for reporting results accurately in stoichiometric calculations worksheets.

Nomenclature and Polyatomic Ions

This page focuses on chemical nomenclature and introduces important polyatomic ions, which are crucial for writing and balancing chemical equations in stoichiometric calculations.

The text provides prefixes for naming compounds with multiple atoms:

• Mono $1$, Di $2$, Tri $3$, Tetra $4$, Penta $5$
• Hexa $6$, Hepta $7$, Octa $8$, Nona $9$, Deca $10$

Vocabulary: Polyatomic ions are charged species composed of two or more atoms bonded together.

The page lists several common polyatomic ions, including:

• NH₄⁺ $Ammonium$
• NO₃⁻ $Nitrate$
• SO₄²⁻ $Sulfate$
• PO₄³⁻ $Phosphate$
• C₂H₃O₂⁻ $Acetate$

Highlight: Familiarity with polyatomic ions is essential for writing correct chemical formulas in stoichiometric calculations.

The text also mentions elements that occur naturally as diatomic molecules, such as hydrogen $H₂$, nitrogen $N₂$, oxygen $O₂$, and the halogens $F₂, Cl₂, Br₂, I₂$.

Understanding these concepts is crucial for performing stoichiometric calculations with chemical formulas and equations.

Chemical Equations and Reactions

This page introduces the basics of chemical equations and different types of chemical reactions, which are fundamental to stoichiometric calculations.

Definition: A subscript in a chemical formula indicates the number of atoms of an element in a molecule or formula unit.

Definition: A coefficient in a chemical equation indicates the number of molecules or formula units of a substance.

The text covers three main types of chemical reactions:

1. Combination reaction: A + B → C
2. Decomposition reaction: C → A + B
3. Combustion reaction: Hydrocarbons reacting with oxygen in air

Highlight: Understanding these reaction types is crucial for balancing equations and performing stoichiometric calculations.

The page also introduces the concepts of formula weight and molecular weight:

• Formula Weight: Sum of atomic weights for atoms in a formula unit
• Molecular Weight: Sum of atomic weights in a molecule

Example: For AB₂, if A has an atomic weight of 1 amu and B has an atomic weight of 2 amu, the formula weight would be 1 + $2 × 2$ = 5 amu.

Lastly, the text mentions percent composition, which is the percentage of mass of a compound contributed by each element. This concept is essential for solving various stoichiometry problems and answers.

Introduction to Matter and Its Properties

This page introduces fundamental concepts in general chemistry, focusing on the properties and classification of matter. It provides essential definitions and explanations that form the basis for stoichiometric calculations.

Definition: Matter is anything that has mass and occupies space.

The page covers various properties of matter, including:

• Composition: Types of atoms and their relative proportions in a sample
• Pure substances: Matter with distinct properties and consistent composition
• Elements: Substances that cannot be decomposed into simpler substances
• Compounds: Substances composed of two or more elements

Highlight: The Law of Constant Composition states that the elemental composition of a compound is always the same.

The text also explains the difference between heterogeneous and homogeneous mixtures, which is crucial for understanding stoichiometry problems and answers.

Vocabulary: Molecules are larger units in which two or more atoms are joined together.

Lastly, the page introduces the concepts of accuracy and precision in measurements, which are essential for performing accurate stoichiometric calculations with chemical formulas and equations.