Atomic Orbitals and Electron Configurations
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Questions and Answers

What happens to energy as wavelength increases?

  • Energy increases.
  • Energy becomes unpredictable.
  • Energy remains constant.
  • Energy decreases. (correct)
  • Which type of radiation has the shortest wavelengths?

  • Gamma rays (correct)
  • Visible light
  • Radio waves
  • Microwaves
  • What defines a line spectrum?

  • It represents thermal radiation.
  • It shows a blend of colors.
  • It contains continuous light.
  • It has only discrete lines. (correct)
  • Which of the following statements about frequency is true?

    <p>Frequency determines the color of visible light.</p> Signup and view all the answers

    What portion of the electromagnetic spectrum does visible light occupy?

    <p>A very small portion.</p> Signup and view all the answers

    How is the electromagnetic spectrum generally arranged?

    <p>By frequency from low to high.</p> Signup and view all the answers

    Which statement correctly describes the relationship between wavelength and frequency?

    <p>As wavelength increases, frequency decreases.</p> Signup and view all the answers

    What role do emission spectra play in atomic models?

    <p>They provide insights into the arrangement of electrons.</p> Signup and view all the answers

    Which orbital designation is NOT considered legitimate?

    <p>1p</p> Signup and view all the answers

    What does an electron configuration denote?

    <p>The arrangement of electrons in an atom's orbitals</p> Signup and view all the answers

    What is indicated by the superscript in an electron configuration?

    <p>The number of electrons in the sublevel</p> Signup and view all the answers

    In an orbital diagram, how are paired electrons represented?

    <p>With an arrow pointed up and another arrow pointed down</p> Signup and view all the answers

    What is the primary purpose of quantum mechanics (QM) in relation to atomic orbitals?

    <p>To predict the probability of finding an electron in a specific region.</p> Signup and view all the answers

    Which of the following shapes is correctly associated with the f orbitals?

    <p>Complex and multi-lobed</p> Signup and view all the answers

    How many sublevels are present in the principal energy level when n = 3?

    <p>4 sublevels.</p> Signup and view all the answers

    Which of the following statements about electron spin is accurate?

    <p>Electrons spin like tops on a vertical axis with two possible directions</p> Signup and view all the answers

    Which of the following statements about atomic orbitals is true?

    <p>An atomic orbital can contain a maximum of two electrons.</p> Signup and view all the answers

    Which of the following best describes orbital energy levels?

    <p>They dictate the arrangement of electrons in orbitals</p> Signup and view all the answers

    Which sublevel can be occupied at the principal quantum number n=3?

    <p>All of the above</p> Signup and view all the answers

    Which sublevel corresponds to the principal quantum number n = 2?

    <p>s and p.</p> Signup and view all the answers

    What does an electron density map represent?

    <p>The probability of finding electrons within certain regions of an atom.</p> Signup and view all the answers

    What did Niels Bohr utilize to conceive his atomic model?

    <p>The line spectrum of hydrogen</p> Signup and view all the answers

    What is the lowest energy level of an electron in a hydrogen atom according to the Bohr model?

    <p>n = 1</p> Signup and view all the answers

    What occurs when a hydrogen atom absorbs energy?

    <p>An electron moves to a higher-energy orbit</p> Signup and view all the answers

    What is the main limitation of the Bohr model when it comes to multiple electron atoms?

    <p>It only accounts for electrons in circular orbits</p> Signup and view all the answers

    What does the quantum mechanical model define instead of specific electron locations?

    <p>Regions of space called orbitals</p> Signup and view all the answers

    Which characteristic of orbitals differentiates the quantum mechanical model from the Bohr model?

    <p>Orbitals can have various shapes</p> Signup and view all the answers

    What happens when an electron relaxes back to a lower-energy orbit?

    <p>It releases a photon of light</p> Signup and view all the answers

    What quantum mechanical concept conflicts with the idea of fixed electron orbits?

    <p>Probabilistic electron distributions</p> Signup and view all the answers

    What type of ion is formed when an atom loses one or more electrons?

    <p>A cation</p> Signup and view all the answers

    Which trend is observed for an atom regarding electron loss and gain across a period in the periodic table?

    <p>Atoms at the far right gain electrons most easily.</p> Signup and view all the answers

    What is the term used for atoms that achieve a noble gas electron configuration?

    <p>Isoelectronic</p> Signup and view all the answers

    What charge does an atom acquire when it gains one or more electrons?

    <p>Negative</p> Signup and view all the answers

    Which of the following correctly identifies an atom maintaining equal numbers of protons and electrons?

    <p>A neutral atom</p> Signup and view all the answers

    In terms of charge, how does an atom become a cation?

    <p>By losing electrons</p> Signup and view all the answers

    Which process is primarily involved in an atom achieving isoelectronic status?

    <p>Electron transfer</p> Signup and view all the answers

    What can be predicted about the ions formed by main-group elements according to the content?

    <p>They will lose or gain electrons to achieve noble gas configurations.</p> Signup and view all the answers

    Study Notes

    Atomic Orbitals

    • The shapes of f orbitals are highly complex.
    • Atomic orbital energy levels are more complex for multi-electron atoms.
    • The sub-level designation 1p is not a legitimate designation because the principal quantum number, n, cannot be equal to 1 for a p sub-level.
    • Sub-Level Designation 2s, 3f, and 4p are legitimate.

    Electron Configurations

    • The behavior of an atom depends on its electron configuration, which describes the specific arrangement of electrons within the atom's orbitals.
    • Electron configurations are written as a series of numbers and letters indicating occupied energy sublevels, with the superscript indicating the number of electrons in the sublevel.

    Orbital Diagrams

    • An orbital diagram uses a square box to represent each orbital, which is labelled with the n value and s, p, d, or f designation.
    • Orbital diagrams also use arrows to represent each electron.
    • The first electron in an orbital is usually represented with an arrow pointing upward. The second electron in an orbital must point downward.

    Nature of Light

    • Wavelength (λ) is the distance between identical points on consecutive waves, such as the distance between two crests.
    • Frequency (ν) is the number of waves that pass through a particular point in one second.
    • As wavelength increases, energy decreases, and as frequency increases, energy increases.
    • The electromagnetic spectrum arranges all types of electromagnetic radiation (light), from gamma rays, which have the shortest wavelengths, to radio waves, which have the longest wavelengths.
    • Line Spectra are emission spectra that are not continuous, but contain only discrete lines.
    • The line spectra of elements are critical to developing our understanding of atomic models.

    The Bohr Atom

    • Photons, tiny discrete packets of light, were used by Danish physicist Niels Bohr to create a model of the atom, which is now known as the Bohr atom, in conjunction with the line spectrum of hydrogen.
    • The concentric circular paths around the nucleus in Bohr's model are called orbits, and each orbit is at a specific energy level designated by a quantum number, n.
    • The electron in the hydrogen atom resides at the lowest possible energy level (n = 1), called the ground state.
    • The Bohr model explained the observed line spectra of hydrogen but failed to explain the spectra of any other elements.

    Quantum Mechanical Model

    • The quantum mechanical (QM) model replaced the Bohr model.
    • The QM model does not define the location of an electron, instead, it defines a region of space called an orbital where an electron is most likely to be found.
    • QM orbitals vary in shape, as opposed to Bohr's orbits, which were all circular and only varied in size.

    Electron Density Map

    • Probability density maps for electrons can be calculated using the mathematics of QM, creating a visual representation called an atomic orbital.
    • The number of energy sublevels in each principal energy level, n, is equal to the principal quantum number.
    • The number of orbitals contained in each sublevel is equal to 2l + 1.
    • Each orbital can contain a maximum of two electrons.
    • Elements in the same group (column) of the periodic table have the same number of valence electrons.
    • Valence electrons are the electrons in the outermost shell of an atom.

    Ions

    • An ion is an atom in which the number of electrons is not equal to the number of protons.
    • Cations are atoms that have lost one or more electrons and become positively charged.
    • Anions are atoms that have gained one or more electrons and become negatively charged.
    • Atoms of main-group elements will lose or gain electrons to achieve a noble gas electron configuration - This is referred to as being isoelectronic.
    • The loss or gain of electrons allows predictions of the ion's charge.

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    Description

    This quiz explores the concepts of atomic orbitals, electron configurations, and orbital diagrams. You will learn about the legitimacy of sub-level designations and how to interpret electron arrangements within atoms. Test your understanding of these fundamental principles in atomic structure.

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