Module 5

    Cards (44)

    • Dalton's Atomic Theory - each element is made up of tiny particles called atoms
    • Dalton's Atomic Theory - the atoms of a given element are identical
    • Dalton's Atomic Theory - chemical reactions involve reorganization of the atoms, changes in the way they are bound together
    • Dalton's Atomic Theory - the atoms themselves are not changed in a chemical reaction, they will remain the same even the reaction is done
    • J.J Thomson's Atomic Theory - discovered the electron in his cathode ray tube
    • J.J Thomson's Atomic Theory - plum pudding model of the atom
    • Rutherford's Theory - used radon and some elements emits streams of positively charged particle through the gold foil experiment; atom is made up of mostly empty space and contained a positively charged nucleus
    • 2Oth century - the development of mass spectrophotometers lead to the discovery of neutrons
    • Elements - contains only 1 kind of atom
    • Compounds - contains 2 or more kind of atoms
    • Chemical bonds - attractive force that holds 2 atoms together in a more complex unit
    • chemical bonds - result of interaction between electrons found in the combining atoms
    • valence electron - an electron in the outermost electron shell of a representative element or noble-gas element
    • lewis symbol - a chemical symbol of an element surrounded by dots which are representation of the valence electrons present in atoms of the element
    • octet rule - states that it should have an eight electrons in a compound for it to be stable
    • ionic bond - formed through the transfer of one or more electrons from one atom or group of atoms to another atom or group of atoms
    • covalent bonds - formed through sharing of one or more pairs of electrons between 2 atoms
    • covalent compound - interaction between 2 or more non-metals
    • ionic compound - interaction between a metal and non-metal
    • Valence Shell Electron Pair Repulsion Theory (VSEPR) - model used to predict the shapes of compunds
    • Polar covalent bonds - having dipoles, a positive and a negative ends
    • non-polar covalent bonds - do not have positive or negative ends
    • Intermolecular forces of attraction (IMFA) - the attractive forces present between molecules
    • London dispersion forces- - weakest type of IMFA; present in all molecules; caused by fluctuations in the electron distribution within atoms or molecules
    • dipole-dipole forces - moderately strong type of IMFA; attractive forces between polar molecules; result of the electrical interactions among dipoles on neighboring molecules
    • hydrogen bonding - strongest type of IMFA; special type of dipole-dipole forces; attraction between hydrogen + any electronegative molecule
    • solubility - ability of a substance to dissolve in a given amount of solvent at a specified feature
    • Strong IMFA - results to a packed close together; exists as condensed phase (solid or liquid)
    • Weak IMFA - far from each other; exists as gas
    • Melting point - temperature at which the substance changes from solid to liquid; stronger IMFA, higher MP. This means greater amount of energy is needed to break the attractive forces between molecules
    • Boiling point - temperature at which the substance changes from liquid to gas
    • surface tension - tendency of a fluid to acquire the least possible surface area
    • Biomolecules - large organic compounds that are important to life's processes, such as respiration and metabolism
    • Proteins - macromolecules comprised of one or more long chains of amino acid residues joined together by peptide bonds
    • amino acids is the basic unit of proteins
    • transport proteins - carry small particles throughout the body
    • Carbohydrates - molecules that are composed of carbon, hydrogen, and oxygen
    • Monosaccharides - simple sugars (glucose)
    • Disaccharides - two monosaccharides bonded together (maltose, sucrose, lactose)
    • Polysaccharides - many monosaccharides bonded together (starch, glycogen, cellulose)
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