Chemistry Chapter 5 Flashcards
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Chemistry Chapter 5 Flashcards

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Questions and Answers

What are energy levels?

The fixed energies an electron can have are called energy levels.

What does quantum refer to in energy?

  • The amount of energy required to move an electron between energy levels (correct)
  • The mass of an electron
  • The speed of light
  • The size of an atom
  • 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?

    <p>It describes the probability of finding an electron at various locations around the nucleus.</p> Signup and view all the answers

    What did Bohr propose about electron orbits?

    <p>He proposed that an electron is found only in specific circular paths or orbits around the nucleus.</p> Signup and view all the answers

    What does the quantum mechanical model determine?

    <p>It determines the allowed energies an electron can have and the probability of finding an electron in various locations.</p> Signup and view all the answers

    What does each energy sub level correspond to?

    <p>Each energy sub level corresponds to one or more orbitals of different shapes.</p> Signup and view all the answers

    What is electron configuration?

    <p>The arrangement of electrons in various orbitals around the nuclei of atoms.</p> Signup and view all the answers

    What does the Aufbau Principle state?

    <p>Electrons occupy the orbitals of lowest energy first.</p> Signup and view all the answers

    What does the Pauli Exclusion Principle state?

    <p>An atomic orbital may describe at most two electrons.</p> Signup and view all the answers

    What does spin refer to in quantum mechanics?

    <p>Spin is a quantum mechanical property of electrons, indicating their direction of rotation.</p> Signup and view all the answers

    What does Hund's Rule state?

    <p>Electrons occupy orbitals of the same energy to maximize the number of electrons with the same spin direction.</p> Signup and view all the answers

    What are the exponents used in electron configuration for s, p, d, and f orbitals?

    <p>s:2, p:6, d:10, f:14.</p> Signup and view all the answers

    How are electron configurations represented in order?

    <p>They are represented in a diagonal order starting from 1s to 7p.</p> Signup and view all the answers

    What is amplitude in terms of wave properties?

    <p>Amplitude is the wave's height from zero to the crest.</p> Signup and view all the answers

    What does wavelength represent, and how is it denoted?

    <p>Wavelength is represented by λ and is the distance between the crests of waves.</p> Signup and view all the answers

    What does frequency represent, and how is it denoted?

    <p>Frequency is represented by ν and is the number of wave cycles to pass a given point per unit of time.</p> Signup and view all the answers

    What are hertz?

    <p>Units of frequency equal to cycles per second.</p> Signup and view all the answers

    What is included in electromagnetic radiation?

    <p>Radio waves, microwaves, infrared waves, visible light, ultraviolet waves, x-rays, and gamma rays.</p> Signup and view all the answers

    What happens to sunlight when it passes through a prism?

    <p>It separates into a spectrum of colors.</p> Signup and view all the answers

    What does the atomic emission spectrum consist of?

    <p>The wavelengths of spectral lines characteristic of the element.</p> Signup and view all the answers

    What is Planck's constant and its value?

    <p>Planck's constant is a value of 6.626 x $10^{-34}$.</p> Signup and view all the answers

    What is the photoelectric effect?

    <p>Electrons are ejected when light shines on a metal.</p> Signup and view all the answers

    What are photons?

    <p>Light quanta.</p> Signup and view all the answers

    What is the ground state of an atom?

    <p>When the electron has the lowest possible energy.</p> Signup and view all the answers

    What does the Heisenberg Uncertainty Principle state?

    <p>It states that it is impossible to know both the velocity and the position of a particle simultaneously.</p> Signup and view all the answers

    What happens when atoms absorb energy?

    <p>Their electrons move to higher energy levels.</p> Signup and view all the answers

    How does light relate to the photoelectric effect?

    <p>Einstein proposed that light could be described as quanta of energy behaving like particles.</p> Signup and view all the answers

    What is the relationship between emitted light frequency and electron energy change?

    <p>The light emitted has a frequency directly proportional to the energy change of the electron.</p> Signup and view all the answers

    How do classical mechanics and quantum mechanics differ?

    <p>Classical mechanics describes the motion of large bodies, while quantum mechanics describes subatomic particles and atoms as waves.</p> Signup and view all the answers

    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.

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    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.

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