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Molarity
Preparing a solution
Dilution
Solubility rules
Complete & Net Ionic Equations
Colligative properties
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Heat Flow
Energy diagrams
Thermochemical equations
Heating/ Cooling curves
Specific Heat Capacity
Calorimetry
Hess's Law
Enthalpies of formation
Bond enthalpies
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Collision Theory
Rate Comparisons
Integrated Rate Law
Differential Rate Law
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Equilibrium
Equilibrium Expression
ICE Tables
Calculating K
K vs Q
Le Chatelier's Principle
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Definitions
Conjugate Acids & Base Pairs
Autoionization of water
pH Scale
Strong Acids/ Bases
Ka and Kb
Buffer
Titrations
Indicators
pH salts
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Entropy
Gibb's Free Energy
G and Temperature
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Oxidation numbers
Half Reactions
Balancing Redox reactions
Voltaic cells
Cell potential (standard conditions)
Cell potential (non-standard)
Electrolysis
Quantitative Electrochemistry
Introduction to Light
Related Examples and Practice Problems
Additional Worked Out Examples/ Practice
Identifying classification types: Differentiation between elements, compounds or mixtures and homogeneous and heterogenous mixtures
Separation techniques: Selected and explaining limitation of appropriate separation
Relating Properties to Composition: Predicting classification based on descriptive properties
and more …
Topic Summary & Highlights
and Help Videos
Core Concept
The electromagnetic spectrum is a continuous range of all types of electromagnetic waves, each with a specific wavelength and energy. These waves travel through space at the speed of light and can be categorized based on their properties:
Wavelength (λ): The distance between two corresponding peaks (or troughs) in a wave. Longer wavelengths have lower energy, while shorter wavelengths have higher energy.
Frequency (ν): The number of wave cycles that pass a point in one second. Frequency and wavelength are inversely proportional (ν = c/λ, where c is the speed of light).
The Spectrum's Colorful Cast:
The electromagnetic spectrum is typically divided into seven major regions, each with unique properties and applications:
Radio Waves (Longest wavelength, lowest energy): Used for radio communication, broadcasting signals, and radar.
Microwaves: Employed in microwave ovens, wireless communication, and satellite technology.
Infrared Radiation (IR): Feels like warmth from the sun and has applications in night vision, remote controls, and spectroscopy (analyzing materials).
Visible Light: The portion of the spectrum our eyes can detect, responsible for vision and color perception.
Ultraviolet Radiation (UV): Causes sunburn, used in sterilization and fluorescent lights.
X-rays: High-energy radiation used in medical imaging and security scanners.
Gamma Rays (Shortest wavelength, highest energy): Most energetic form of radiation, used in cancer treatment and nuclear reactions.
Light: A Closer Look
As chemists, we're particularly interested in visible light and its interaction with molecules. Visible light is a tiny portion of the electromagnetic spectrum, with a range of wavelengths that our eyes can detect and interpret as different colors.
Color and Wavelength: The color we perceive depends on the wavelength of light. Red light has a longer wavelength than blue light.
Light and Matter
Light can interact with matter in various ways, influencing chemical reactions:
Absorption: When a molecule absorbs light, it gains energy and can be excited to a higher energy state. This absorbed light often falls within the ultraviolet or visible regions. Understanding absorption is crucial in spectroscopy, a technique used to identify and analyze molecules.
Emission: Excited molecules can return to their ground state by releasing energy as light. This emitted light can be of the same or different wavelength as the absorbed light, depending on the molecule.
Tips for Studying:
Use diagrams and visuals to represent the electromagnetic spectrum and different regions.
Practice converting between wavelength and frequency using the formula ν = c/λ.
Relate the color of light to its wavelength and energy.
Explore how light absorption and emission are used in various spectroscopic techniques.
