Atomic Structure: Subatomic Particles and Atomic Models
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Questions and Answers

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

  • 1 amu (correct)
  • 0.00055 amu
  • 2 amu
  • 5 amu
  • According to the Rutherford Model, what is the charge of the nucleus?

  • Variable charge
  • Positively charged (correct)
  • Neutrally charged
  • Negatively charged
  • What is the purpose of the atomic number (Z)?

  • To determine the number of neutrons
  • To determine the number of protons (correct)
  • To determine the number of electrons
  • To determine the mass number
  • What is the shape of a p-orbital?

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

    In the Bohr Model, what happens when an electron gains energy?

    <p>It jumps to a higher energy level</p> Signup and view all the answers

    What is the term for the regions where electrons are likely to be found?

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

    What determines the chemical properties of an element?

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

    Which of the following principles states that electrons occupy the lowest available energy level?

    <p>Aufbau principle</p> Signup and view all the answers

    What is the shape of an s-orbital?

    <p>Spherical shape</p> Signup and view all the answers

    What is the term for the arrangement of electrons in energy levels?

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

    What happens to the atomic radius as you move from left to right across a period?

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

    Which of the following trends is observed in the periodic table?

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

    Study Notes

    Atomic Structure

    Subatomic Particles

    • Proton: Positively charged, found in the nucleus, mass = 1 amu (atomic mass unit)
    • Neutron: No charge, found in the nucleus, mass = 1 amu
    • Electron: Negatively charged, found in energy levels, mass = 0.00055 amu

    Atomic Models

    • Rutherford Model (1911): Nucleus with electrons orbiting around it
      • Positively charged nucleus with negatively charged electrons
    • Bohr Model (1913): Energy levels with electrons jumping between them
      • Electrons occupy specific energy levels (shells) around the nucleus

    Atomic Structure Notation

    • Atomic Number (Z): Number of protons in an atom's nucleus
    • Mass Number (A): Sum of protons and neutrons in an atom's nucleus
    • Electron Configuration: Arrangement of electrons in energy levels
      • Notation: 1s² 2s² 2p⁶ (example)

    Energy Levels (Shells)

    • Principal Energy Levels (n): 1, 2, 3, ... (distance from nucleus increases)
    • Subshells (l): s, p, d, f (shapes of orbitals)
    • Orbitals: Regions where electrons are likely to be found
      • s-orbitals: spherical shape
      • p-orbitals: dumbbell shape
      • d-orbitals: four-leaf clover shape
      • f-orbitals: complex shape

    Atomic Structure

    Subatomic Particles

    • A proton has a positive charge and is found in the nucleus with a mass of 1 atomic mass unit (amu).
    • A neutron has no charge and is found in the nucleus with a mass of 1 amu.
    • An electron has a negative charge and is found in energy levels with a mass of 0.00055 amu.

    Atomic Models

    Rutherford Model (1911)

    • The nucleus is positively charged, and electrons orbit around it.
    • The model consists of a positively charged nucleus with negatively charged electrons.

    Bohr Model (1913)

    • Electrons occupy specific energy levels (shells) around the nucleus.
    • Electrons jump between energy levels, and each energy level has a specific capacity.

    Atomic Structure Notation

    • The atomic number (Z) is the number of protons in an atom's nucleus.
    • The mass number (A) is the sum of protons and neutrons in an atom's nucleus.
    • Electron configuration is the arrangement of electrons in energy levels.
    • Electron configuration notation is used to describe the arrangement, such as 1s² 2s² 2p⁶.

    Energy Levels (Shells)

    • Principal energy levels (n) are numbered from 1, 2, 3, and so on, with increasing distance from the nucleus.
    • Subshells (l) are classified as s, p, d, and f, and they have different shapes of orbitals.
    • Orbitals are regions where electrons are likely to be found, with different shapes:
      • s-orbitals are spherical in shape.
      • p-orbitals have a dumbbell shape.
      • d-orbitals have a four-leaf clover shape.
      • f-orbitals have a complex shape.

    Atomic Structure

    Subatomic Particles

    • Protons have a positive charge and are found in the nucleus, determining the element through their atomic number.
    • Neutrons have no charge and are found in the nucleus, contributing to the atomic mass along with protons.
    • Electrons have a negative charge and are found in energy levels outside the nucleus, with their number equal to the number of protons in a neutral atom.

    Energy Levels (Shells)

    • Electron configuration refers to the arrangement of electrons in energy levels.
    • The valence shell is the outermost energy level, determining the chemical properties of an atom.
    • The Aufbau principle states that electrons occupy the lowest available energy level.
    • Pauli's Exclusion Principle states that each electron has a unique set of quantum numbers.

    Atomic Orbitals

    • s orbitals have a spherical shape, with one orbital per energy level.
    • p orbitals have a dumbbell shape, with three orbitals per energy level (x, y, z).
    • d orbitals have a complex shape, with five orbitals per energy level.
    • f orbitals have a complex shape, with seven orbitals per energy level.

    Electron Configuration Notation

    • Shorthand notation represents the number of electrons in each orbital (e.g., 1s² 2s² 2p⁶).
    • Block notation groups orbitals (s, p, d, f) with the number of electrons in each.
    • Atomic radius decreases from left to right across a period and increases from top to bottom in a group.
    • Electronegativity increases from left to right across a period and decreases from top to bottom in a group.
    • Ionization energy increases from left to right across a period and decreases from top to bottom in a group.

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    Description

    Learn about the basic structure of an atom, including protons, neutrons, and electrons, and explore the Rutherford and Bohr models of atomic structure.

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