Uncertainty in Measurement (Section)
Round each of the following numbers to four significant figures and express the result in standard exponential notation: (a) 102.53070, (b) 656.980, (c) 0.008543210,
(d) 0.000257870, (e) -0.0357202.
WEEK TWO NOTES (PART 2) Atomic Shells and Classical Models of Chemical Bonding Covalent bonds – electrons shared somewhat equally between 2 atoms making the bond Ionic bonds – 1 or more electrons is completely transferred from 1 atom to another Polar covalent bonds – partial transfer of charge from 1 atom to another Electronegativity – tendency of an atom to attract atoms from other atoms; decides if a bond is either covalent, ionic or polar covalent. Lewis dot diagrams show the # of valence electrons associated with each atom in a molecule + shows bonding VSEPR – valence shell electron pair repulsion theory o Electrons will be as far apart as possible Representations of Molecules Molecule – co