MT-CHM1-LEC-Lesson-3-Energy-1.0

RECALL OF PAST LESSON

Periodic Table

  • Definition: Tabular arrangement of chemical elements.

  • Organization: Based on atomic number, electron configuration, and recurring chemical properties.

  • Purpose: Systematic way to categorize and understand fundamental building blocks of matter.

Atomic Number and Structure

  • Atomic Number: Unique identifier for each element, representing the number of protons in the nucleus.

  • Groups and Periods:

    • Groups: Vertical columns sharing similar properties.

    • Periods: Horizontal rows detailing trends and relationships among elements.

Chemical Properties

  • Valence Electrons: Elements in the same group behave similarly due to similar valence electron counts.

  • Metallic vs Non-Metallic Properties:

    • Metals: Lustrous, good conductors, tend to lose electrons.

    • Non-metals: Lack metallic properties, often gain electrons in reactions.

Metallic and Non-Metallic Properties

  • Classification: Metals, non-metals, and metalloids based on chemical/physical characteristics.

  • Trends: Atomic size, ionization energy, electronegativity, and reactivity reflect trends across groups and periods.

Major Groups in Periodic Table

  • Main Groups: Alkali metals, alkaline earth metals, halogens, noble gases (Groups 1, 2, 13-18).

  • Transition Metals: Found in the d-block, known for multiple oxidation states and complex compound formation.

  • Lanthanides and Actinides: F-block elements located below the main table, notable for their unique properties.

Historical Development

  • Mendeleev's Periodic Law: Fundamentally arranged elements to predict properties of undiscovered elements.

ENERGY

Definition

  • Energy is the part of the universe capable of doing work.

Classification of Energy

  • Kinetic Energy:

    • Associated with motion; includes thermal energy linked to atom/molecule motion.

    • More thermal energy increases kinetic energy.

  • Potential Energy:

    • Stored energy based on the position within a system.

    • Includes chemical energy stored in bonds.

  • Sound Energy:

    • Produced through vibrations; travels as waves needing a medium (e.g., air, water).

    • Examples include voice, musical instruments, etc.

  • Radiant Energy:

    • Combination of heat and light energy; travels in waves.

    • Found in light bulbs, sunlight, etc.

  • Electrical Energy:

    • Produced by the movement of electrons.

    • Powers devices like TVs, radios, and household appliances.

  • Atomic Energy:

    • Generated from splitting atoms; releases significant energy.

    • Examples include nuclear power and atomic bombs.

  • Mechanical Energy:

    • Visible movement energy; associated with moving objects.

    • Includes machines and kinetic activities.

Transformation of Energy

  • Defined as changing energy from one form to another, a fundamental principle in energy studies.

CONSERVATION AND MEASUREMENT OF ENERGY

Conservation of Energy

  • Law: No energy is created or destroyed during transformations; total energy remains constant.

Measurement of Energy

  • Caloric Measurement:

    • 1 calorie: energy needed to raise 1g of water by 1°C.

    • 1 kcal = 1000 calories.

    • 1 calorie = 4.184 Joules.

    • Important in nutrition (1 Cal = 1 kcal).

SUMMARY

  • Energy plays a crucial role in both inorganic and organic chemistry.

  • Energy changes during chemical reactions are fundamental for understanding molecular behavior and predicting chemical interactions.

REFERENCES

  • Stoker, H. Stephen (2013). Biological Chemistry(6th Ed). USA: Cengage Learning.

  • Bettelheim (2019). Introduction to General Organic, and Biochemistry(11th edition). Cengage Learning.