Physics Chapter 2: Atomic Structure Quiz
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Questions and Answers

What is the relative mass of a proton in atomic mass units (amu)?

  • 1.007276 (correct)
  • 0
  • 1.008665
  • 5.485799 x 10^-4

    • Isotopes of an element have the same number of protons but different numbers of electrons.

    False

    What is the charge of an electron?

    -1.602 x 10^-19 C

    The atomic number (Z) of an element equals the number of ______ in the nucleus of its atoms.

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

    Match each particle with its corresponding charge:

    <p>Proton = +1 Neutron = 0 Electron = -1</p> Signup and view all the answers

    Which of the following statements is true regarding the mass number?

    <p>It includes both protons and neutrons.</p> Signup and view all the answers

    All naturally occurring carbon atoms have the same mass number.

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

    The mass number (A) of carbon with six protons and six neutrons is ______.

    <p>12</p> Signup and view all the answers

    Which of the following equations correctly represents the relationship between wave speed, wavelength, and frequency?

    <p>$c = vλ$</p> Signup and view all the answers

    Electromagnetic waves travel at different speeds in a vacuum compared to in air.

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

    What is the speed of light in a vacuum in meters per second?

    <p>3.00 × 10^8</p> Signup and view all the answers

    The energy emitted or absorbed in discrete quantities is referred to as a ___.

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

    What type of radiation primarily reaches the Earth from the Sun?

    <p>Visible and ultraviolet radiation</p> Signup and view all the answers

    Match the type of radiation to its common use:

    <p>Infrared radiation = Transmits heat energy from glowing coals Microwave radiation = Heats food quickly Visible light = Colors seen in rainbows Ultraviolet radiation = Energy from the Sun</p> Signup and view all the answers

    What was the frequency of the radio wave emitted by Ethiopian National Radio in kHz?

    <p>2400</p> Signup and view all the answers

    According to Planck's proposal, energy is emitted in ___ quantities.

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

    What law proposed by Dalton describes the relationship between masses of elements that combine chemically?

    <p>Law of multiple proportions</p> Signup and view all the answers

    The photoelectric effect occurs when electrons are emitted from a metal surface due to electromagnetic radiation of any energy level.

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

    Name the three principal types of radiation emitted by radioactive substances.

    <p>Alpha particles, beta particles, gamma rays</p> Signup and view all the answers

    Bohr's theory explains that the electron in a hydrogen atom can only occupy specific ___ levels.

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

    Match the following terms with their definitions:

    <p>Photon = A particle of electromagnetic radiation with energy hν Emission spectrum = The spectrum associated with the emission of light from an atom Nuclear atom = An atom with a tiny, dense nucleus surrounded by electrons Photoelectric effect = The emission of electrons from a metal surface when struck by light</p> Signup and view all the answers

    Which series in the hydrogen spectrum includes transitions to the n = 2 level?

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

    The emission spectrum of hydrogen only includes ultraviolet wavelengths.

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

    What does the Bohr Model primarily explain?

    <p>Quantized energy states for electrons in a hydrogen atom.</p> Signup and view all the answers

    The transition from n = 4 to n = 1 in a hydrogen atom emits a photon in the __________ spectrum.

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

    Match the following series in atomic hydrogen emission spectrum with their corresponding spectrum region:

    <p>Lyman = Ultraviolet Balmer = Visible and ultraviolet Paschen = Infrared Brackett = Infrared</p> Signup and view all the answers

    What factor increases as an electron transitions from a higher to a lower energy level in a hydrogen atom?

    <p>Energy of the emitted photon</p> Signup and view all the answers

    The Bohr Model accurately predicts the atomic spectra of all elements.

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

    What is one limitation of the Bohr Model regarding spectral lines?

    <p>It does not explain the splitting of spectral lines in a magnetic field.</p> Signup and view all the answers

    What does the periodic law state?

    <p>Certain physical and chemical properties repeat at regular intervals.</p> Signup and view all the answers

    The electron configuration of an element can help determine its group in the periodic table.

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

    What is a 'group' in the context of the periodic table?

    <p>A group refers to a vertical column of elements with similar properties.</p> Signup and view all the answers

    The first-row transition metal with atomic number 24 is __________.

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

    Which transition element is known for having a unique electron configuration due to a half-filled d-subshell?

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

    Match the following transition metals with their atomic numbers:

    <p>Iron = 26 Titanium = 22 Nickel = 28 Vanadium = 23</p> Signup and view all the answers

    There are no exceptions to the Aufabu principle among transition metals.

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

    The electron configuration of Nickel can be represented as __________.

    <p>[Ar] 3d^8 4s^2</p> Signup and view all the answers

    What does the letter 'd' represent in the subshell notation 4d?

    <p>Type of orbital</p> Signup and view all the answers

    The value of ℓ can only be equal to or greater than the principal quantum number n.

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

    What is the maximum number of electrons that can occupy a subshell with ℓ = 1?

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

    The magnetic quantum number (mℓ) can take values from _____ to _____ including 0.

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

    Match the principal quantum numbers with their allowed angular momentum quantum numbers (ℓ):

    <p>n = 1 = ℓ = 0 n = 2 = ℓ = 0, 1 n = 3 = ℓ = 0, 1, 2 n = 4 = ℓ = 0, 1, 2, 3</p> Signup and view all the answers

    Which of the following statements is true regarding the electron spin quantum number (ms)?

    <p>It can be +½ or -½.</p> Signup and view all the answers

    For every set of n, ℓ, and mℓ values, an atomic orbital can accommodate more than two electrons.

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

    List the possible values of mℓ when ℓ = 2.

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

    Study Notes

    Atomic Structure and Periodic Properties of the Elements

    • This unit covers the historical development of atomic models, experimental observations by scientists, subatomic particles, electromagnetic radiation, atomic spectra, Bohr models, quantum mechanical models, and periodic trends.
    • The unit will also cover scientific inquiry skills.
    • Early Greek philosophers debated the composition of matter. Democritus proposed the concept of atoms as indivisible particles.
    • John Dalton developed an atomic theory based on experimental evidence.
    • Dalton's postulates included: matter is made of atoms; atoms of an element are identical; atoms of different elements have different masses; atoms combine in simple whole number ratios to form compounds; and atoms are neither created nor destroyed during chemical reactions.
    • Dalton's theory led to the development of the law of conservation of mass and the law of definite proportions.
    • Dalton's theory was modified due to further scientific discoveries (the existence of isotopes and subatomic particles for example).
    • The modern atomic theory and postulates are discussed.
    • Key experiments leading to the discovery of the electron, nucleus, and neutron: cathode ray experiments, the oil drop experiment, and alpha particle scattering experiments.
    • Specific discoveries and contributions by scientists like Thomson, Millikan, and Rutherford are mentioned.
    • Atomic spectra are discussed: how atoms emit light when excited, how line spectra are discrete, and the connection to quantized energy levels.
    • The Bohr model of the hydrogen atom is reviewed, highlighting its contributions and limitations including the postulates of quantized energy levels, circular orbits, and fixed angular momentum.
      - Calculation examples that involve these equations are included.
    • The quantum mechanical model of the atom is explained, describing the quantum mechanical description of atoms.
    • The roles of quantum numbers (n, l, ml, ms) and their significance in determining energy levels and orbital shapes are addressed.
    • Specific orbital shapes of s, p, and d orbitals are discussed.
    • Electronic configurations and orbital diagrams explaining the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
    • Periodic trends are discussed within the context of the periodic table.
    • How the electron configuration of an element is related to its position in the periodic table is explained. - How to write electron configurations for elements in the periodic table.
    • The concepts of atomic radius, ionization energy, electron affinity, electronegativity, and metallic character. Trends in these properties across periods and down groups are analyzed.
    • The advantages of the periodic classification of elements are highlighted.

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    Description

    Test your knowledge on atomic structure and properties with this quiz. Questions cover topics like protons, electrons, isotopes, and the speed of light. It's perfect for students studying physics and understanding fundamental concepts in atomic theory.

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