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Questions and Answers
What are energy levels?
What are energy levels?
The fixed energies an electron can have are called energy levels.
What does quantum refer to in energy?
What does quantum refer to in energy?
What is the quantum mechanical model?
What is the quantum mechanical model?
A modern description of electrons in atoms derived from the solutions to the Schrodinger equation.
What does an atomic orbital describe?
What does an atomic orbital describe?
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What did Bohr propose about electron orbits?
What did Bohr propose about electron orbits?
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What does the quantum mechanical model determine?
What does the quantum mechanical model determine?
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What does each energy sub level correspond to?
What does each energy sub level correspond to?
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What is electron configuration?
What is electron configuration?
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What does the Aufbau Principle state?
What does the Aufbau Principle state?
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What does the Pauli Exclusion Principle state?
What does the Pauli Exclusion Principle state?
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What does spin refer to in quantum mechanics?
What does spin refer to in quantum mechanics?
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What does Hund's Rule state?
What does Hund's Rule state?
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What are the exponents used in electron configuration for s, p, d, and f orbitals?
What are the exponents used in electron configuration for s, p, d, and f orbitals?
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How are electron configurations represented in order?
How are electron configurations represented in order?
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What is amplitude in terms of wave properties?
What is amplitude in terms of wave properties?
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What does wavelength represent, and how is it denoted?
What does wavelength represent, and how is it denoted?
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What does frequency represent, and how is it denoted?
What does frequency represent, and how is it denoted?
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What are hertz?
What are hertz?
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What is included in electromagnetic radiation?
What is included in electromagnetic radiation?
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What happens to sunlight when it passes through a prism?
What happens to sunlight when it passes through a prism?
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What does the atomic emission spectrum consist of?
What does the atomic emission spectrum consist of?
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What is Planck's constant and its value?
What is Planck's constant and its value?
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What is the photoelectric effect?
What is the photoelectric effect?
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What are photons?
What are photons?
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What is the ground state of an atom?
What is the ground state of an atom?
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What does the Heisenberg Uncertainty Principle state?
What does the Heisenberg Uncertainty Principle state?
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What happens when atoms absorb energy?
What happens when atoms absorb energy?
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How does light relate to the photoelectric effect?
How does light relate to the photoelectric effect?
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What is the relationship between emitted light frequency and electron energy change?
What is the relationship between emitted light frequency and electron energy change?
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How do classical mechanics and quantum mechanics differ?
How do classical mechanics and quantum mechanics differ?
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Study Notes
Energy Levels and Quantum Concepts
- Energy levels refer to the distinct fixed energies an electron can possess.
- Quantum denotes the minimal energy needed to relocate an electron between energy levels, indicating that electron energy is quantized.
Quantum Mechanical Model
- Represents a modern understanding of electron behavior in atoms, derived from the Schrodinger equation.
Atomic Orbitals
- Define the likelihood of an electron's position around the atomic nucleus, influencing electron arrangement.
Bohr Model and Quantum Mechanics
- Proposed that electrons occupy specific circular orbits around the nucleus.
- The quantum mechanical model establishes possible energies for electrons and predicts their spatial distribution around nuclei.
Electron Configuration Principles
- Aufbau Principle: Electrons fill the lowest energy orbitals first.
- Pauli Exclusion Principle: Each atomic orbital can accommodate a maximum of two electrons.
- Hund's Rule: Electrons fill degenerate orbitals singly before pairing to maximize unpaired spins.
Electron Configuration and Notation
- Orbital capacities: s (2), p (6), d (10), f (14).
- Follows a diagonal order for filling: 1s, 2s 2p, 3s 3p 3d, etc.
Wave Properties
- Amplitude: Refers to the height of a wave from the centerline to its crest.
- Wavelength (λ): Distance between successive wave crests.
- Frequency (ν): Number of wave cycles that pass a point per unit time, expressed in Hertz (Hz), where 1 Hz equals one cycle per second.
Electromagnetic Radiation and Spectrum
- Encompasses various forms such as radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays.
- Spectrum: Produced when different wavelengths from sunlight are separated through a prism.
Atomic Emission Spectrum
- Characteristic wavelengths of spectral lines for each element contribute to its atomic emission spectrum.
Planck's Constant and Energy Changes
- Planck's constant is valued at 6.626 × 10⁻³⁴.
- The energy of a quantum can be calculated using the formula E = hv, where h represents Planck's constant and v denotes frequency.
- Minor energy changes relate to low-frequency radiation; major changes pertain to high-frequency radiation.
Photoelectric Effect and Photons
- Occurs when electrons are emitted from metals upon exposure to light.
- Photons are defined as discrete packets of light energy.
Ground State and Energy Absorption
- Ground state indicates the lowest energy state of an atom.
- Absorption of energy results in electron elevation to higher energy levels; light emission occurs when electrons revert to lower levels.
Heisenberg Uncertainty Principle
- States that simultaneous knowledge of a particle's position and velocity is fundamentally impossible.
Classical vs. Quantum Mechanics
- Classical mechanics effectively explains motion for larger objects, while quantum mechanics describes the behavior of subatomic particles and atoms as waves.
Studying That Suits You
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Description
Test your understanding of key concepts in Chemistry Chapter 5 with these flashcards. Focused on energy levels, quantum mechanics, and the modern model of atoms, this quiz will help reinforce your learning and comprehension of essential terms and principles.