Chemistry Atomic Model Overview
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Chemistry Atomic Model Overview

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Questions and Answers

Who believed the universe was made of invisible units called atoms?

Democritus

Aristotle supported Democritus's theory about atoms.

False

What did Dalton's atomic theory propose?

  • Atoms of the same element are different.
  • Atoms can change into different elements.
  • Atoms are indivisible particles. (correct)
  • Atoms combine in simple ratios. (correct)

    • What concept did J.J. Thomson contribute to atomic theory?

    <p>Discovery of the electron</p> Signup and view all the answers

    What did Rutherford's gold foil experiment conclude?

    <p>The nucleus is small and dense.</p> Signup and view all the answers

    What did Niels Bohr propose about electron arrangement?

    <p>Electrons exist in distinct energy levels.</p> Signup and view all the answers

    According to Bohr's model, electrons can jump between levels with energy being ___ or ___.

    <p>added, released</p> Signup and view all the answers

    Who improved upon Bohr's findings by proposing the Quantum Mechanical Model?

    <p>Heisenberg and Schrödinger</p> Signup and view all the answers

    What does the Quantum Mechanical Model describe?

    <p>Electrons exist in 'clouds'.</p> Signup and view all the answers

    What does the Principal Quantum Number (n) refer to?

    <p>The principal energy levels</p> Signup and view all the answers

    The azimuthal quantum number (ℓ) can take on any integer value from 0 to n.

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

    How many electrons can one orbital hold?

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

    What are the four quantum numbers used to describe electrons in an atom?

    <p>n, ℓ, mℓ, ms</p> Signup and view all the answers

    The letters s, p, d, and f also represent the type of orbitals and correspond to the quantum number ℓ values of ___, ___, ___, and ___ respectively.

    <p>0, 1, 2, 3</p> Signup and view all the answers

    The 3d orbital has 6 available orbitals.

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

    What is the maximum number of electrons that can occupy the 2p subshell?

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

    Match the quantum number with its description:

    <p>n = Principal energy levels ℓ = Shape of the orbital mℓ = Orientation of the orbital ms = Spin of the electron</p> Signup and view all the answers

    What determines the shape of the orbital?

    <p>Azimuthal Quantum Number (ℓ)</p> Signup and view all the answers

    The orbital notation for oxygen is 1s2 2s2 2p______.

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

    Match the quantum numbers with their corresponding values:

    <p>n=1 = 1s n=2, l=0 = 2s n=2, l=1 = 2p n=3, l=2 = 3d</p> Signup and view all the answers

    Magnetic Quantum Number (mℓ) indicates the spin of the electron.

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

    What do the letters s, p, d, and f stand for in relation to orbital types?

    <p>Sharp, Principal, Diffuse, Fundamental</p> Signup and view all the answers

    What is the total number of orbitals found in the 3rd energy level?

    <p>5</p> Signup and view all the answers

    The quantum number 'l' indicates the shape of an electron's orbital.

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

    What is the value of 'ms' for an electron in the 1s orbital if it is spinning clockwise?

    <p>1/2</p> Signup and view all the answers

    What did Thomson use to discover the electron?

    <p>A cathode ray tube</p> Signup and view all the answers

    Rutherford concluded that atoms are mostly solid and have a dense structure.

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

    What particle did Rutherford identify as being located in the nucleus?

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

    Electrons orbit the nucleus similar to how planets orbit the _____?

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

    What was one of Rutherford's conclusions based on the Gold Foil Experiment?

    <p>Atoms have a small, dense nucleus.</p> Signup and view all the answers

    Electrons can only exist at certain fixed energy levels in Bohr's model.

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

    Match the following scientists with their discoveries:

    <p>Thomson = Discovered the electron Rutherford = Discovered the nucleus Bohr = Proposed electron energy levels Dalton = Atomic theory of matter</p> Signup and view all the answers

    What is the term for the amount of energy required to move an electron from one energy level to another?

    <p>Quantum of energy</p> Signup and view all the answers

    Which of the following statements accurately describes the quantum mechanical model?

    <p>It restricts the energy of electrons to certain values.</p> Signup and view all the answers

    The quantum mechanical model provides specific paths for electrons to follow around the nucleus.

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

    What determines the allowed energies an electron can have according to the quantum mechanical model?

    <p>Quantum mechanical model</p> Signup and view all the answers

    Each energy sublevel corresponds to one or more __________ of different shapes.

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

    What role do orbitals play in the quantum mechanical model?

    <p>They describe the shape and probability of finding electrons in a region.</p> Signup and view all the answers

    A quantum is the amount of energy needed for an electron to remain in the same energy level.

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

    Match the concepts with their definitions:

    <p>Energy level = The specific energies an electron can have Quantum = The amount of energy needed for an electron to transition between energy levels Orbital = The region where an electron is likely to be found</p> Signup and view all the answers

    The allowed energies of an electron can be described by its __________.

    <p>energy level</p> Signup and view all the answers

    What is the shape of the p subshell?

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

    Electrons in the same orbital can have the same spin quantum number.

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

    What is the value of the magnetic quantum number (mℓ) when ℓ equals 2?

    <p>-2, -1, 0, +1, +2</p> Signup and view all the answers

    The value of the spin quantum number (ms) can be either ___ or ___.

    <p>+½, -½</p> Signup and view all the answers

    Which orbital corresponds to the angular momentum quantum number ℓ=0?

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

    Match the subshell type with its corresponding angular momentum quantum number (ℓ):

    <p>s = 0 p = 1 d = 2 f = 3</p> Signup and view all the answers

    A half-filled subshell is paramagnetic.

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

    What is the principle that states no two electrons in the same atom can have identical quantum numbers?

    <p>Pauli exclusion principle</p> Signup and view all the answers

    Study Notes

    Atomic Theory Through the Ages

    • Democritus proposed that the universe was made of invisible units called atoms.

      -400 BC

      -took 2000 years to be proved right

    • Aristotle supported Democritus's theory about atoms.

    • Dalton's Atomic Theory proposed that all matter is made up of atoms, which are indivisible and indestructible particles.

    • "billiard ball model" was proposed by john dalton in 1804

    • john dalton (1766-1844)

      -wrote the first atomic theory

      -atoms can neither be destroyed nor be created

      -atoms of an element are identical

    • J.J. Thomson discovered the electron, a negatively charged particle, which he proposed were embedded in a positively charged sphere.

      -also used cathode ray experiment to discover the existence of the electron

    • discovery of the electron

      -1897, Thomson used a cathode ray tube to deduce the presence of a electron.

    • nuclear model - Ernest Rutherford's gold foil experiment concluded that atoms have a small, dense, positively charged nucleus at their center.

    • Niels Bohr proposed that electrons orbit the nucleus in specific energy levels or shells.

      -According to Bohr's model, electrons can jump between levels with energy being absorbed or emitted.

      -electrons revolve the nucleus (like planets in the solar system)

    • Erwin Schrödinger improved upon Bohr's findings by proposing the Quantum Mechanical Model.

      - The Quantum Mechanical Model describes electrons as existing in probability regions called orbitals, a more sophisticated model than Bohr's.

      - Principal Quantum Number (n) refers to the energy level of an electron, with higher numbers indicating higher energy levels.

      -The azimuthal quantum number (ℓ) can take on any integer value from 0 to n-1, with ℓ = 0, 1, 2, and 3 representing s, p, d, and f orbitals, respectively.

      - Each orbital can hold a maximum of two electrons.

    Quantum Numbers: Describing Electron Behavior

    • The four quantum numbers used to describe electrons in an atom are:
      • Principal Quantum Number (n): Describes the energy level of an electron
      • Azimuthal Quantum Number (ℓ): Describes the shape of an electron's orbital.
      • Magnetic Quantum Number (mℓ): Describes the orientation of an electron's orbital in space.
      • Spin Quantum Number (ms): Describes the spin of an electron, either spin up (+1/2) or spin down (-1/2)

    Orbital Types and Configurations

    • The letters s, p, d, and f also represent the type of orbitals and correspond to the quantum number ℓ values of 0, 1, 2, and 3, respectively.
    • The 3d orbital has 6 available orbitals.
    • The maximum number of electrons that can occupy the 2p subshell is 6.
    • The orbital notation for oxygen is 1s2 2s2 2p4.
    • The Magnetic Quantum Number (mℓ) indicates the orientation of the orbital in space.
    • The letters s, p, d, and f stand for sharp, principal, diffuse, and fundamental, respectively, which are historical terms related to the appearance of spectral lines.

    Electron Arrangement

    • The total number of orbitals found in the 3rd energy level is 9.
    • The value of ms for an electron in the 1s orbital if it is spinning clockwise is +1/2.
    • Thomson used a cathode ray tube to discover the electron.
    • Rutherford concluded that atoms are mostly empty space and have a dense nucleus.
    • Rutherford identified the proton as being located in the nucleus.
    • Electrons orbit the nucleus similar to how planets orbit the Sun.
    • One of Rutherford's conclusions based on the Gold Foil Experiment was that atoms have a positively charged center.

    Energy Levels and Quantum Mechanics

    • Bohr's model states that electrons can only exist at certain fixed energy levels.
    • The term for the amount of energy required to move an electron from one energy level to another is ionization energy.
    • The quantum mechanical model describes electrons as existing as probability waves within orbitals, rather than fixed orbits.
    • Allowed energies of an electron are determined by its principal quantum number (n) and the potential energy of the electron within the atom's electric field.
    • Each energy sublevel corresponds to one or more orbitals of different shapes.
    • Orbitals are probability regions where electrons are likely to be found, providing a more realistic representation of electrons' behavior.
    • Quantum is the amount of minimum energy an electron can absorb/release to transition between energy levels.

    Orbital Shape and Quantum Numbers

    • The allowed energies of an electron can be described by its principal quantum number (n).
    • The p subshell has a dumbbell shape.
    • The value of the magnetic quantum number (mℓ) when ℓ equals 2 is -2, -1, 0, 1, 2.
    • The value of the spin quantum number (ms) can be either +1/2 or -1/2.
    • The s orbital corresponds to the angular momentum quantum number ℓ = 0.
    • s, p, d, and f subshells correspond to ℓ values of 0, 1, 2, and 3, respectively.
    • Pauli Exclusion Principle states that no two electrons in the same atom can have identical quantum numbers.

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