AP Chemistry: Atomic Structure
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AP Chemistry: Atomic Structure

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Questions and Answers

What is the net positive charge experienced by an electron in an atom?

  • Effective nuclear charge (Zeff) (correct)
  • Neutron number
  • Electron number
  • Proton number
  • What is the trend in atomic radius across a period?

  • Remains constant
  • Increases from left to right
  • Increases down a group
  • Decreases from left to right (correct)
  • What is the energy required to remove an electron from an atom?

  • Electron affinity
  • Electronegativity
  • Ionization energy (correct)
  • Electrolysis energy
  • Which block of the periodic table includes the transition metals?

    <p>d-block</p> Signup and view all the answers

    What is the ability of an atom to attract electrons in a covalent bond?

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

    What is the result of the increase in effective nuclear charge (Zeff) across a period?

    <p>Decrease in atomic radius</p> Signup and view all the answers

    What is the trend in ionization energy down a group?

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

    What is the unit of measurement for energy in chemistry?

    <p>Joules (J)</p> Signup and view all the answers

    What technique is used to measure the energy of electrons emitted from an atom?

    <p>Photoelectron spectroscopy (PES)</p> Signup and view all the answers

    What is the trend in electronegativity across a period?

    <p>Increases from left to right</p> Signup and view all the answers

    Study Notes

    Atomic Structure

    • Atomic structure consists of protons, neutrons, and electrons
    • Protons and neutrons are found in the nucleus, while electrons orbit around it
    • Electrons are arranged in energy levels or shells, with each shell having a specific capacity

    Effective Nuclear Charge

    • Effective nuclear charge (Zeff) is the net positive charge experienced by an electron in an atom
    • Zeff is the result of the attractive force between the nucleus and electrons, and the repulsive force between electrons
    • Zeff increases from left to right across a period, and decreases down a group
    • Atomic radius decreases from left to right across a period, and increases down a group
    • This is due to the increase in Zeff, which pulls electrons closer to the nucleus
    • Atomic radius is measured in picometers (pm)

    Ionization Energy

    • Ionization energy (IE) is the energy required to remove an electron from an atom
    • IE increases from left to right across a period, and decreases down a group
    • This is due to the increase in Zeff, which makes it harder to remove an electron

    Periodic Table Blocks

    • The periodic table is divided into blocks based on the last orbital filled
    • The blocks are:
      • s-block (alkali metals and alkaline earth metals)
      • p-block (nonmetals and metalloids)
      • d-block (transition metals)
      • f-block (lanthanides and actinides)

    Electronegativity

    • Electronegativity is the ability of an atom to attract electrons in a covalent bond
    • Electronegativity increases from left to right across a period, and decreases down a group
    • Electronegativity is measured using the Pauling scale, with higher values indicating greater electronegativity

    Force of Energy

    • Not a specific topic in AP Chemistry, but energy is a fundamental concept in chemistry
    • Energy is the ability to do work, and is measured in units such as joules (J)

    Photoelectron Spectroscopy

    • Photoelectron spectroscopy (PES) is a technique used to measure the energy of electrons emitted from an atom
    • PES involves bombarding atoms with high-energy radiation, causing electrons to be emitted
    • The energy of the emitted electrons is measured, providing information about the atomic orbitals and electron binding energies

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    Test your knowledge of atomic structure, including effective nuclear charge, atomic radius trends, ionization energy, periodic table blocks, electronegativity, and more.

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