Ch.2- Basic Chemistry

Subdecks (2)

Cards (213)

  • Matter
    -Anything that has mass and takes up space(weight)
    - Solids, Liquids, and Gasses
    - Physical & Chemical changes
  • Energy
    the ability to do work
  • Kinetic energy

    when energy is actually doing work
  • Potential Energy (PE)

    When energy is inactive or stored
  • Forms of Energy
    chemical, electrical, mechanical, radiant
  • Chemical energy

    stored in bonds of chemical substances
  • Electrical energy

    results from the movement of charged particles-ions
  • Mechanical energy

    directly involved in moving matter- muscles
  • Radiant energy

    travels in waves- the electromagnetic spectrum including x-rays, infrared, light, radio, and UV rays
  • Fundamental units of matter
    can't be broken down into smaller units
  • 96% of the body is made from 4 elements
    Carbon (C), Oxygen (O), Hydrogen (H), Nitrogen (N)
  • Atoms
    building blocks of elements
  • Inside the nucleus
    protons and neutrons
  • Outside the nucleus
    electrons
  • Atomic number

    equal to the number of protons that the atoms contain - also equals the number of electrons
  • Atomic Mass Number (amu)

    Sum of protons and neutrons
  • Isotopes
    -Have the same number of protons and electrons, but the same atomic number
    - Vary in number of neutrons so different atomic masses
  • Atomic weight

    -close to mass number of most abundant isotope
    -atomic weight reflects natural isotope variation
  • Radioisotopes
    -Heavy isotope
    - Tends to be unstable
    - Decomposes to move stable isotope
  • Radioactivity
    - process of spontaneous atomic decay
    - releases particles (alpha, beta, and gamma rays)
  • Molecule
    2 or more atoms combined chemically
  • Compound
    2 or more DIFFERENT atoms combined chemically
  • Chemical Reactions

    Occurs when atoms combine or dissociate from other atoms
  • In chemical reactions, atoms are
    -united by chemical bonds
    -dissociated from other atoms when chemical bonds are broken
  • Electrons
    -Negatively charged particles
    - occupy energy levels called electron levels or shells
    - closest to the nucleus and most strongly attracted
  • Each shell has distinct properties
    -The number of electrons has an upper limit
    -Shells closest to the nucleus fill first
  • Bonding
    Involves interactions between electrons in the outer shell(Valence shell)
  • Full valence shells do not form

    bonds
  • Inert elements
    have complete valence shells and are stable
  • Rules of 8s
    Step 1: Shell 1 has 2
    Step 2: Shell 2 has 10 electrons
    Step 3: Shell 3 has 18 electrons
  • Reactive Elements

    -valence shells are not full and are unstable
    -tend to gain, lose, or share electrons
    -allows for bond formation, which produces stable valence
  • Ionic bonds

    form when electrons are completely transferred from one atom to another
  • Ions
    -charged particles
    - either donate or accept electrons
  • Anions
    negatively charged ions (accept electrons)
  • Cations
    positively charged ions (donate electrons)
  • Opposites attract so stick together

    most form salts
  • Covalent Bonds

    -atoms become stable through shared electrons
    - Single covalent bonds share one electron
    - Double covalent bonds share two electrons
  • Covalent bonded molecules
    -some are non-polar: electrically neutral as a molecule
    -some are polar: have a positive and negative side
  • Polar molecules orient themselves toward other
    polar or charged particles
  • Hydrogen bonds

    -weak chemical bonds
    -hydrogen is attracted to the negative portion of polar molecule
    -provides attraction between molecules