Atomic Structure Review for Chemistry
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Questions and Answers

What is the correct electron configuration for the element Magnesium (Mg)?

  • 1s2 2s2 2p6 3s2 (correct)
  • 1s2 2s2 3s2
  • 1s2 2s2 2p6 3s1
  • 1s2 2s2 2p6 4s2

    • Which element is represented by the electron configuration 1s2 2s2 2p6 3s2 3p64s23d104p3?

  • Arsenic (As) (correct)
  • Selenium (Se)
  • Germanium (Ge)
  • Gallium (Ga)

    • In orbital notation, how many electrons can the 'd' subshell accommodate?

  • 14
  • 10 (correct)
  • 5
  • 2

    • What configuration error occurs when two 'p' electrons share the same orbital while others remain empty?

    <p>Hund's Rule is violated</p> Signup and view all the answers

    Which subshell must completely fill before any electrons occupy the 'p' subshell?

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

    What determines the mass number of an atom?

    <p>The sum of protons and neutrons</p> Signup and view all the answers

    Which particle has a negative charge?

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

    In an electrically neutral atom, how do the number of protons compare to the number of electrons?

    <p>Protons and electrons are equal</p> Signup and view all the answers

    What makes an atom an ion?

    <p>It has a net electrical charge due to unequal protons and electrons</p> Signup and view all the answers

    How do isotopes of the same element differ?

    <p>By the number of neutrons</p> Signup and view all the answers

    Which isotope of silicon has the greatest representation by percentage?

    <p>Si-28</p> Signup and view all the answers

    What is the charge of an atom with 8 protons and 10 electrons?

    <p>-2</p> Signup and view all the answers

    What is the average atomic mass of silicon given its isotopes' percentages?

    <p>28.09</p> Signup and view all the answers

    Which isotope of potassium is the most abundant?

    <p>K-39</p> Signup and view all the answers

    What happens to frequency when wavelength increases?

    <p>Frequency decreases</p> Signup and view all the answers

    Which transition emits light with the highest frequency?

    <p>n=6 to n=2</p> Signup and view all the answers

    How many total electrons can be held by the 4p sublevel?

    <p>6</p> Signup and view all the answers

    How does an electron move when it absorbs energy?

    <p>From lower energy level to higher energy level</p> Signup and view all the answers

    Which electron transition will absorb light with the highest energy?

    <p>n=6 to n=2</p> Signup and view all the answers

    What is the maximum number of electrons in one orbital of the 5d sublevel?

    <p>2</p> Signup and view all the answers

    Which sublevels are available in the 3rd energy level?

    <p>s, p, d</p> Signup and view all the answers

    Study Notes

    Atomic Structure Review

    • Subatomic Particles:
    • Protons: Small mass, positive charge, located in the nucleus.
    • Neutrons: Small mass, neutral charge, located in the nucleus.
    • Electrons: Small mass, negative charge, located in energy levels surrounding the nucleus.

    Determining Atomic Properties

    • Mass Number: Sum of protons and neutrons.
    • Charge: Difference between the number of protons and electrons.
    • Atomic Number: Number of protons in an atom.

    Atomic Structure Sketch

    • A sketch of an atom with 3 protons, 4 neutrons, and 2 electrons should be drawn, showing the nucleus with the protons and neutrons, and the electron cloud surrounding the nucleus.

    Atomic Table Completion

    • The table provides information about various elements including their symbol, atomic number, mass number, charge, proton count, neutron count, and electron count.
    • Examples: Magnesium-24 has 12 protons, 12 neutrons, and 12 electrons .
    • Oxygen-16 has 8 protons, 8 neutrons, and 8 electrons

    Ions Identification

    • Ions are atoms or molecules with a net electric charge.
    • Elements in the table with a charge indicating a difference between protons and electrons are ions
    • Examples: Oxygen (O-16) and Sodium (Na).

    Isotopes

    • Isotopes are atoms of the same element with different numbers of neutrons.
    • They share the same number of protons but differ in mass number.
    • Examples: Silicon-28, Silicon-29, and Silicon-30 are isotopes of silicon.

    Average Atomic Mass Calculation

    • The average atomic mass of an element is calculated by considering the abundance of each isotope.
    • Examples: Determine the average atomic mass of silicon given the percentage amounts and mass of each isotope.

    Determining the Most Abundant Isotope

    • An element's most abundant isotope will be the isotope that contributes most to the element's average atomic mass. (based on percentage abundance.

    Relationship Between Wavelength and Frequency

    • Wavelength and frequency are inversely related.
    • As one increases, the other decreases.

    Relationship Between Energy and Frequency

    • Energy and frequency are directly related.
    • As one increases, the other increases.

    Emission Spectra and Energy Levels

    • Electrons absorb energy and move to higher energy levels.
    • Electrons release energy and move to lower energy levels.
    • This energy change is often emitted as light with specific wavelengths (colors).

    Determining Electron Transitions

    • Electron transitions between energy levels determine the energy and frequency of emitted light.
    • Higher frequency transitions involve higher energy differences.

    Electron Configuration

    • Electron configurations describe how electrons are arranged in atoms. Sublevels within energy levels.
    • Sublevels (s,p,d,f) have orbitals that relate to electron numbers and the order filling.
    • Rules apply (e.g. Aufbau principle, Hund's rule)

    Orbital Notation

    • Orbital notations visualize electron distribution in atomic orbitals.

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    Description

    This quiz focuses on the fundamental concepts of atomic structure, including the characteristics of subatomic particles, the determination of atomic properties such as mass number and atomic number, and practical applications like sketching atoms and completing atomic tables. Test your understanding of these key concepts relevant to high school chemistry.

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