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CH103
Chemistry - Quantum Theory and Electronic Structure of Atoms
| Question | Answer |
|---|---|
| Electromagnetic Radiation | A form of energy that travels through space as waves and includes radio waves, visible light, X-rays, and gamma rays. |
| Wavelength (λ) | Distance between two identical points on a wave, such as crest to crest. Measured in meters (m) Longer wavelength = lower energy |
| Frequency (ν) | Number of waves passing a point each second. Measured in hertz (Hz) Higher frequency = higher energy |
| Speed of Light | c=λν where: c = 3.00 × 10⁸ m/s λ = wavelength ν = frequency |
| Electromagnetic Spectrum -- Order from lowest energy to highest energy: | 1)Radio waves 2)Microwaves 3)Infrared 4)Visible light 5)Ultraviolet 6)X-rays 7)Gamma rays |
| Visible Light Colors | Color - Wavelength Red(Longest), Orange, Yellow, Green, Blue, Indigo, Violet(Shortest) |
| Red = | lowest energy |
| Violet= | highest energy |
| Max Planck | Proposed that energy is emitted in packets called quanta. |
| Max Planck Energy equation: | E=hν where: E = energy h = Planck's constant ν = frequency |
| Planck's Constant | h=6.626×10−34J⋅s |
| Photon | A particle of light carrying a quantum of energy. (Higher frequency light has higher-energy photons) |
| As frequency increases: | Energy increases |
| As wavelength increases: | Energy decreases |
| Atomic Emission Spectrum | When excited electrons return to lower energy levels, they emit light. (Each element produces a unique spectrum) |
| Ground State | The lowest-energy state of an atom, where its electrons occupy the lowest available energy levels |
| Excited State | A higher-energy state of an atom that occurs when one or more electrons absorb energy and move to higher energy levels. |
| Bohr Model | Proposed: Electrons occupy fixed energy levels. Electrons move between energy levels by absorbing or releasing energy. |
| Energy Levels | n = 1, 2, 3, 4... where n is the principal quantum number. |
| Absorption | Electron moves: n=1→n=3n = 1 \rightarrow n = 3n=1→n=3 Energy absorbed. |
| Emission | Electron moves: n=3→n=1n = 3 \rightarrow n = 1n=3→n=1 Energy released. |
| Hydrogen Spectrum | Because electrons can only exist in certain energy levels, hydrogen emits only specific wavelengths of light. This produces a line spectrum. |
| Planck | Quantum theory |
| Einstein | Photoelectric effect |
| Bohr | Energy levels in atoms |
| Higher Frequency Means: | Higher energy, Shorter wavelength |
| Longer Wavelength Means: | Lower frequency, Lower energy |
| Red Light | Long wavelength, Low frequency, Low energy |
| Violet Light | Short wavelength, High frequency, High energy |
| State the speed of light. | 3.00×108 m/s |
| What equation relates wavelength and frequency? | c=λν where ccc = speed of light, λ\lambdaλ = wavelength, and ν\nuν = frequency. |
| Who developed quantum theory? | Max Planck. |
| What is Planck's equation? | E=hν where EEE = energy, hhh = Planck's constant, and ν\nuν = frequency. |
| What is the photoelectric effect? | The emission of electrons from a metal surface when light of sufficient energy shines on it. |
| What is the difference between a ground state and an excited state? | Ground state: Lowest-energy state of an atom. Excited state: Higher-energy state after the atom absorbs energy. |
| What happens when an electron falls from a higher to a lower energy level? | The electron releases energy as a photon (light). |
| What does the Bohr model propose? | Electrons occupy specific energy levels around the nucleus and can move between levels by absorbing or releasing energy. |
| Why does hydrogen produce a line spectrum? | Because its electron can occupy only certain allowed energy levels, so it emits only specific wavelengths of light when transitioning between those levels. |
| Quantum | The smallest discrete amount of energy that can be absorbed or emitted by matter. |
| Electromagnetic radiation = | energy traveling as waves |
| Wavelength= | distance between wave peaks |
| Frequency= | waves per second |
| Photon= | particle of light |
| Quantum = | smallest unit of energy |
| Ground state = | lowest-energy state |
| Excited state = | higher-energy state after absorbing energy |
Created by:
jsminnie118