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Page 1

Title

HONORS CHEMISTRY Unit 1: Matter and Changes
NAME:

Page 2

Scientific Methodology

Definition: Method used by scientists for logical and systematic problem-solving.
Observation: Use of senses to obtain information.
- Types of Observations:
  - Qualitative: Descriptive qualities from senses.
  - Quantitative: Numerical data from observations.
Hypothesis: Proposed explanation testable through prediction
- Format: "If ____ then ____."
Experiment: Step-by-step procedure to test hypotheses.

Practice Questions

Qualitative observations: ______________________________
Quantitative observations: ____________________________
Variables:
- Independent Variable: Changed by the experimenter.
- Dependent Variable: Changes as a result of the independent variable.
- Controlled Variable: Kept constant throughout the experiment.

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Variables

Experiments involve three types of variables:
- Independent Variable: Intentionally manipulated.
- Dependent Variable: Outcomes based on independent variable changes.
- Controlled Variable: Variables kept constant to ensure valid results.

Practice Questions

Example 1: Changing ethanol volume in boiling point experiment.
- Independent Variable: ____________
- Dependent Variable: ____________
- Controlled Variables: ____________
Example 2: Mouthwash effectiveness experiment.
- Independent Variable: ____________
- Dependent Variable: ____________
- Controlled Variables: ____________

Practice Chemical Data

Mouthwash effectiveness measured by average bacterium per tooth
Variables in fish eggs hatching study setup with temperatures: 10℃, 20℃, 30℃, 40℃, and 50℃.

Page 4

Chemistry Fundamentals

Chemistry: Study of matter composition and changes.
Matter: Anything with mass and volume.
Chemical: Substance produced or used in chemistry.
- Common chemicals: water (H2O), methane (CH4).

Important Concepts

Chemical Formula: Indicates number and types of atoms.
- Example: H2O, CO2, NaCl.
Element: Simplest form of matter.
- Listed in the Periodic Table; examples include Carbon (C), Helium (He).
Subscript: Number indicating atoms, e.g., H2O means 2 hydrogen atoms.
Coefficient: Indicates how many molecules in a formula, e.g., in 3H2O, 3 is the coefficient.

Page 5

Element Symbols and Chemical Formulas

Need for Naming System: Common names lack chemical composition details.
Element Symbols: One, two, or three-letter codes representing elements (Capital Letter + lower case).
Examples:
- Copper: Cu, Argon: Ar, Lithium: Li.

Purpose of Element Symbols

Provides shorthand for elements in formulas.
Difference between element symbols and chemical formulas is that element symbols are single elements while formulas represent compounds.

Subscript Usage

Indicates quantity of each element in a compound.

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Composite Elements

Diatomic Elements: Composed of two atoms; found on the periodic table.
Examples include H2, O2, N2.
Tetratomic: Phosphorus as P4;
Octatomic: Sulfur as S8.

Practice: Write the chemical formula for the following elements.

Page 7

States of Matter

Matter: Anything with mass and volume.
Three Physical States:
- Solids, liquids, gases.
Solids: Fixed shape and volume.
- Example: Ice, iron.
Liquids: Fixed volume but take the shape of their container.
- Example: Water, oil.
Gases: No fixed shape or volume; fill containers.
- Example: Oxygen gas, air.

Page 8

Identifying States of Matter

Particle Level Drawings:
- Solid: Particles close in pattern.
- Liquid: Particles close but jumbled.
- Gas: Particles far apart.
Periodic Table: Colors indicate state:
- Black = solid, Blue = liquid, Red = gas.

Page 9

Atoms and Molecules

Atoms: Smallest units of elements.
Molecule: Two or more atoms bonded together.

Identifying Atoms and Molecules

Identifying: Use the periodic table to check if it has subscripts or multiple elements.
Practice distinguishing between atoms and molecules using examples.

Page 10

Diatomic and Polyatomic Elements

Diatomic Elements: H2, O2, N2, etc.
Polyatomic Elements: Phosphorus P4 and Sulfur S8.
Chemical Compound Formation:
- Example: Covalent compounds form with specific ratios determined by element properties.

Page 11

Pure Substances and Mixtures

Matter Categories: Pure substances and mixtures.
Pure Substances: Consistent chemical composition, such as elements and compounds.
Mixtures: Combinations of two or more substances, can vary in composition.
- Homogeneous Mixtures: Uniform compositions (saltwater).
- Heterogeneous Mixtures: Distinct parts visible (salad).

Page 12

Elements and Compounds

Element: Pure substance consisting of one type of atom.
Compound: Pure substance with two or more elements.

Practice Distinction Between Element and Compounds

Page 13

Separation Techniques

Mixture Separation: Homogeneous mixtures are harder to separate.
Filtration: Separates solids from liquids.
Distillation: Utilizes different boiling points.
Chromatography: Separates based on affability for mobile phases.

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Continued Separation Techniques

Sublimation: Solid to gas separation process.
Crystallization: Produces pure solid from solution.
Decantation: Transfers a liquid while leaving solids behind.
Centrifugation: Spins mixture to separate components based on density.

Page 15

Reading the Periodic Table

Structure: Columns (groups) and rows (periods).
Information in Each Box: Atomic number, symbol, name, mass.
Identity through Atomic Number: Unique to each element.

Page 16

Atomic Mass and Isotopes

Atomic Mass: Weighted average reflecting the number of isotopes and their masses.

Page 17

Reaction Terminology

Chemical Reactions: Involve reorganization of atoms, represented in chemical formulas.
Reactants vs Products: Substance before and after a reaction.

Page 18

Yield and State Symbols

Yield Symbol: Indicates the production/result of a reaction.
State Symbols: Represent physical state (solid, liquid, gas, aqueous).

Page 19

Physical and Chemical Properties

Properties: Characteristics observed/ measured without altering substances.

Page 20

Further Physical Properties Practice

Identifying properties as chemical (C) or physical (P).

Page 21

Physical and Chemical Changes

Types of Changes: Physical changes do not alter identity; chemical changes create new substances.
Recognizing Changes: Changes can be identified through observable events like color change or gas formation.