Lab Safety and Chapter Reviews

Midterm Review Sheet

• Homework Schedule:
  • Friday Night: Lab Safety and Chapter 1
  • Monday Night: Chapter 3 and Chapter 2
  • Tuesday Night: Chapter 4 and Chapter 5
  • Wednesday Night: Chapter 6 and Chapter 7

Lab Safety

• Safety Goggles: Essential for lab work to protect eyes.
• Eating, Drinking, Chewing: Prohibited in the lab for safety reasons.
• Spills: Proper procedures for clean-up must be followed.
• Glassware Breakage: Designated procedures for cleaning up broken glass.
• Reagent Bottles: Unused chemicals should not be returned.
• Acid Dilution: Specific procedures on proper acid dilution.
• Unattended Burners: Do not leave a lighted burner unattended.
• Organization: Maintain a clean and organized lab area.
• Hair and Jewelry: Secure loose hair and jewelry to prevent accidents.
• Safety Violation Scenario: Students should be able to describe a safety violation, and the correct course of action to take.

Chapter 1: Introduction to Chemistry

• Definition: Chemistry is the study of matter and its properties.
• Pure vs. Applied: Pure chemistry is focused on fundamental knowledge, while applied chemistry applies knowledge to solve problems.
• Reasons to Study Chemistry: Fundamental aspects of chemistry are vital in research and problem solving. Chemistry is related to several aspects in daily life.
• Macroscopic vs. Microscopic: Macroscopic refers to large-scale and visible objects, while microscopic refers to very small objects.
• Research Areas: Chemistry impacts various fields like medicine and materials science.
• Antoine-Laurent Lavoisier: Key figure in chemistry, contributed significantly.
• Scientific Method: Crucial steps in the scientific method must be followed.
• Independent vs. Dependent Variable: A distinction between independent and dependent variables is needed.
• Collaboration/Communication: Importance of teamwork and clear communication.

Chapter 3: Measurement, Unit Conversion, Dimensional Analysis, Significant Figures

• Accuracy vs. Precision: Accuracy refers to being close to the actual value. Precision refers to closeness of multiple measurements.
• Qualitative vs. Quantitative Observations: Qualitative observations are descriptive, while quantitative observations involve numbers.
• SI Units: Standard units of measurement for mass, length, time, temperature, and amount of a substance.
• Temperature Units: Celsius, Fahrenheit, and Kelvin.
• SI Prefixes: Prefixes for units of measurements for large and small values.
• Unit Conversions: Converting values between different units.
• Dimensional Analysis: Using units as a guide to solve problems.
• Significant Figures: Using the correct number of significant digits in calculations.
• Calculations (Sample): Calculations on significant figures, unit conversions, and dimensional analysis are vital to understand.

Chapter 2: Matter

• Definition of Matter: Physical substance in general, occupying space having rest mass and inertia.
• Compounds, Elements, and Atoms: Matter is composed of atoms, elements, and compounds.
• States of Matter: Solids, liquids, and gases.
• Physical vs. Chemical Changes/Properties: Students must be able to explain these differences.
• Reactants and Products: The substances that react and are produced are required.
• Chemical Reactions: Students are required to discuss signals for chemical reactions to occur.
• Extensive vs. Intensive Properties: Students need to differentiate extensive and intensive properties.
• Mixtures: Homogeneous and heterogeneous mixtures.
• Pure Substances: Students must be able to describe their characteristics.

Chapter 4: The Atom

• Democritus: Early atomic theory.
• Modern Atomic Concepts: Details on modern atomic structure including isotopes, ions, and their masses.
• Average atomic mass calculation: Students must be able to calculate the average atomic mass.
• Atomic Structure: Detailed information about subatomic particles are required.
• Symbols in Nuclear Notation: students should be able to read symbols and identify relevant information.

Chapter 5: Atomic Models and Electron Behaviour

• Atomic models:
  • Dalton
  • Thomson
  • Rutherford
  • Bohr
  • Schrodinger
• Quantum levels and Energy: Details about quantum energy levels are required.
• Atomic Orbitals: Students must know different types of orbitals (s, p, d, and f).
• Electron configurations: Students need to be able to write the electron configurations for different atoms.
• Wavelength, Frequency, Amplitude: Key definitions and relationships required.
• Relationship between wavelength and frequency: Students should be able to describe this relationship.

Chapter 6: The Periodic Table

• Mendeleev and Moseley: Contributions to the periodic table.
• Periodic Table Organization: Arrangement/Organization of the periodic table.
• Periods and Groups: Properties of elements based on location.
• Periodic Trends: Periodic trends of elements across periods and groups.
• Cations and Anions: Cations lose electrons, and anions gain electrons.
• Electron Affinity: Energy change when an electron is accepted.
• Key Groups: Identifying key groups on the periodic table.

Chapter 7: Ionic and Metallic Bonding

• Valence Electrons: Electrons involved in chemical bonding.
• Octet Rule: Atoms tend to gain, lose, or share electrons to achieve a stable outer electron configuration.
• Ionic Bonds: Bonds formed between ions.
• Ionic Compounds: Students should know characteristics of ionic compounds
• Metallic Bonds: Sea of electrons model used to describe metallic bonds.
• Alloys: Properties comparison to pure metals.

Prepare for your upcoming midterm with this comprehensive quiz covering lab safety protocols and key concepts from Chapters 1 to 7. Test your understanding of essential safety measures and relevant laboratory practices. This quiz will help reinforce your knowledge and ensure a successful performance in your upcoming evaluations.