Atomic Structure Basics
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Atomic Structure Basics

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Questions and Answers

Which of the following subatomic particles has a negative charge?

  • Neutron
  • Nucleus
  • Electron (correct)
  • Proton
  • What is the maximum number of electrons that can be held in the first electron shell?

  • 2 (correct)
  • 4
  • 6
  • 8
  • Which type of chemical bond is formed by the transfer of electrons between atoms?

  • Nonpolar covalent bond
  • Ionic bond (correct)
  • Polar covalent bond
  • Covalent bond
  • What is the mass of a proton in atomic mass units (amu)?

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

    Which of the following electron configurations is an example of a correct notation?

    <p>1s2 2s2 2p6</p> Signup and view all the answers

    What is the primary characteristic of a hydrogen bond?

    <p>Polarity between bonded atoms</p> Signup and view all the answers

    Which of the following states of matter has a fixed shape and volume?

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

    What is the process of changing from a liquid to a gas?

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

    What is the unit of measurement that represents 6.022 x 10^23 particles?

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

    What is the formula that represents the simplest whole-number ratio of atoms in a compound?

    <p>Empirical Formula</p> Signup and view all the answers

    Study Notes

    Atomic Structure

    • Atomic Model: The modern atomic model consists of:
      • Protons (positive charge) in the nucleus
      • Neutrons (no charge) in the nucleus
      • Electrons (negative charge) in energy levels around the nucleus
    • Electron Configuration:
      • Electron shells (energy levels) have a maximum number of electrons
      • The first shell can hold up to 2 electrons, the second shell up to 8, and so on
      • Electron configuration notation: 1s2 2s2 2p6 (example)
    • Subatomic Particles:
      • Protons: positively charged, mass of 1 amu (atomic mass unit)
      • Neutrons: no charge, mass of 1 amu
      • Electrons: negatively charged, negligible mass

    Chemical Bonding

    • Types of Chemical Bonds:
      1. Ionic Bonds: Formed by the transfer of electrons between atoms
        • Cations (positively charged) and anions (negatively charged) attract each other
      2. Covalent Bonds: Formed by the sharing of electrons between atoms
        • Polar covalent bonds: unequal sharing of electrons, resulting in a partial charge
        • Nonpolar covalent bonds: equal sharing of electrons
      3. Hydrogen Bonds: Weak bonds between hydrogen and highly electronegative atoms (F, O, N)
    • Bond Properties:
      • Bond length: distance between the nuclei of two bonded atoms
      • Bond energy: energy required to break a bond
      • Bond polarity: difference in electronegativity between bonded atoms

    States of Matter

    • Solid:
      • Particles are closely packed and vibrate in place
      • Has a fixed shape and volume
    • Liquid:
      • Particles are close together but able to move past each other
      • Has a fixed volume but takes the shape of its container
    • Gas:
      • Particles are widely spaced and move freely
      • Has neither a fixed shape nor volume
    • Phase Changes:
      • Melting: solid to liquid
      • Freezing: liquid to solid
      • Vaporization: liquid to gas
      • Condensation: gas to liquid

    Stoichiometry

    • Mole: A unit of measurement, 6.022 x 10^23 particles (atoms, molecules, ions)
    • Molar Mass: The mass of one mole of a substance, in grams
    • Empirical Formula: The simplest whole-number ratio of atoms in a compound
    • Molecular Formula: The actual number of atoms in a molecule
    • Stoichiometric Calculations:
      • Moles of reactants to moles of products
      • Mass of reactants to mass of products
      • Limiting reagent: the reactant that determines the amount of product formed

    Atomic Structure

    • Atomic model consists of protons, neutrons, and electrons
    • Protons have a positive charge and neutrons have no charge, both are found in the nucleus
    • Electrons have a negative charge and are found in energy levels around the nucleus
    • Electron shells have a maximum number of electrons, with the first shell holding up to 2 electrons, the second shell up to 8, and so on
    • Electron configuration notation is used to describe the arrangement of electrons in an atom, for example, 1s2 2s2 2p6

    Subatomic Particles

    • Protons have a mass of 1 amu (atomic mass unit) and a positive charge
    • Neutrons have a mass of 1 amu and no charge
    • Electrons have a negligible mass and a negative charge

    Chemical Bonding

    • Chemical bonds are formed between atoms through the transfer or sharing of electrons
    • Ionic bonds are formed by the transfer of electrons, resulting in positively charged cations and negatively charged anions that attract each other
    • Covalent bonds are formed by the sharing of electrons between atoms, resulting in a molecule
    • Polar covalent bonds involve unequal sharing of electrons, resulting in a partial charge, while nonpolar covalent bonds involve equal sharing of electrons
    • Hydrogen bonds are weak bonds between hydrogen and highly electronegative atoms such as fluorine, oxygen, and nitrogen

    Bond Properties

    • Bond length is the distance between the nuclei of two bonded atoms
    • Bond energy is the energy required to break a bond
    • Bond polarity is the difference in electronegativity between bonded atoms

    States of Matter

    • In a solid, particles are closely packed and vibrate in place, having a fixed shape and volume
    • In a liquid, particles are close together but able to move past each other, having a fixed volume but taking the shape of its container
    • In a gas, particles are widely spaced and move freely, having neither a fixed shape nor volume
    • Phase changes occur when a substance changes from one state of matter to another, such as melting, freezing, vaporization, and condensation

    Stoichiometry

    • A mole is a unit of measurement, equal to 6.022 x 10^23 particles (atoms, molecules, or ions)
    • Molar mass is the mass of one mole of a substance, in grams
    • The empirical formula is the simplest whole-number ratio of atoms in a compound
    • The molecular formula is the actual number of atoms in a molecule
    • Stoichiometric calculations involve the mole ratio of reactants to products, and the mass ratio of reactants to products
    • The limiting reagent is the reactant that determines the amount of product formed

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    Description

    Learn about the modern atomic model, electron configuration, and subatomic particles. Test your knowledge of protons, neutrons, electrons, and energy levels.

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