2024-09-16T20:09:19+03:00[Europe/Moscow] en true <p>Atomic <strong>mass unit (amu)</strong></p>, <p>Atomic<strong> number</strong></p>, <p>Mass <strong>number</strong></p>, <p>Atomic <strong>mass</strong></p>, <p>How do you find the <strong>atomic mass</strong> of an element</p>, <p>How do you read a mass spectrometry graph</p>, <p>Pure substance vs. mixture </p>, <p>Pure element vs. compound </p>, <p>Heterogeneous vs. homogeneous mixture</p>, <p>What is a mole and what does it measure</p>, <p><strong>Molar</strong> mass (what is it equal to)</p>, <p>Mole (amount) ⇌ grams (weight)</p>, <p>Law of conservation of mass</p>, <p>In <strong>isotope notation</strong> the ___ is on the bottom, and the ___ is on the top representing the different ___</p> flashcards

Chapter 1 - Atomic theory

Atomic structure Atomic mass The mole Matter classification

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  • Atomic mass unit (amu)

    The mass of one singular proton or neutron

  • Atomic number

    The number of protons in an atom (top of element card)

  • Mass number

    The sum of protons and neutrons in an atom combined

  • Atomic mass

    The average mass of an atom based on its abundance of isotopes

    - Is = to molar mass

  • How do you find the atomic mass of an element

    ∑n(fraction of isotope n that makes up the element) x (amu mass of that isotope n)

  • How do you read a mass spectrometry graph

    x-axis: The position of each peak indicates the mass of the isotope

    y-axis: The height of each peak indicates the relative abundance of the isotope

  • Pure substance vs. mixture

    Pure substance = only 1 type of atom or molecule

    Mixture = 2 or more pure substances mixed together

  • Pure element vs. compound

    Pure element = A pure substance that cannot be further simplified (individual oxygen and hydrogen atoms)

    Compound = A pure substance with only 1 type of molecule (water only contains water molecules made of oxygen and hydrogen)

  • Heterogeneous vs. homogeneous mixture

    Heterogeneous = molecules are distinct from each other

    Homogeneous = molecules mix together evenly (dissolving)

  • What is a mole and what does it measure

    - A mole is a measure of amount

    - 1 mole of anything has 6.022x1023 units

  • Molar mass (what is it equal to)

    molar mass is the mass (weight) of 1 mole of atoms of a given element

    - Molar mass in g = atomic mass

  • Mole (amount) ⇌ grams (weight)

    # of Particles/atoms ⇋ (1 mole ÷ 6.022x1023) ⇋ (molar mass in g ÷ 1 mole) ⇋ mass in g

  • Law of conservation of mass

    The total mass of reactants consumed is = to the total mass of products formed

  • In isotope notation the ___ is on the bottom, and the ___ is on the top representing the different ___

    - atomic number (# of protons)

    - Mass number (# of protons and neutrons combined)

    - The different number of neutrons that isotopes of the same element can have (This is the only number that changes in standard notation)