CEM 141 Final Exam pt 3 (Real Exam 3, Mock
Exam 3, PP Lecture 26-35)
- ANS-Hybrid orbitals
# of hybrid orbitals coming out - ANS-the # atomic orbitals going in = ???
1. draw lewis structure
2. determine electron pair geometry
3. determine molecular shape
4. determine the bond polarities
5. add up the bond polarities
6. figure out molecular polarity - ANS-to determine molecular polarity:
120 degrees - ANS-trigonal planar bond angle
180 degrees - ANS-linear bond angle
2 - ANS-in MO Theory, each orbital can contain up to ____ electrons
2 because the London dispersion forces are stronger because the molecule is larger, so more
energy is required to overcome them - ANS-Which do you predict to have a higher boiling point
and why?
1. CH3OH
2.CH3CH2CH2OH
2 electrons - ANS-in MO theory, each bond is made up of how many electrons?
2 electrons - ANS-in VB theory, each bond is made up of how many electrons?
2+ - ANS-transition metals always form a ____ ion
3D - ANS-What info is missing from a Lewis Structure?
3rd network of strong bonds; you would have to break bonds to disrupt a crystal - ANS-what
makes diamond hard?
4 bonds to 4 identical carbons - ANS-in diamond, each carbon forms how many bonds to how
many carbons?
, a filled s orbital and two half-filled p orbitals - ANS-in diamond, the electrons are in what
orbitals?
a metal and a nonmetal - ANS-simple ionic compounds contain:
abnormal, irregular, departing from the usual - ANS-anomalous
an equal # of molecular orbitals - ANS-in the Molecular Orbital Theory, atomic orbitals combine
to form:
An extended network of boron and nitrogen atoms held together by covalent bonds -
ANS-Boron nitride is the second hardest substance known (after diamond) It has a very high
melting point, but does not conduct electricity. What types of bonding do you think are present in
boron?
anions - ANS-non-metals form (cations/anions)
anomalous - ANS-properties of water are:
are the same - ANS-if there are no lone pairs in a molecule, the electron geometry and
molecular shape:
as "sticks" - ANS-how are bonds often shown in the valence bond theory?
atomic orbitals overlap to form bonds - ANS-Valence Bond Theory
attracts its own valence electrons strongly AND attracts electrons from other atoms in bonds -
ANS-an atom that has a high effective nuclear charge...
b/c it can absorb and emit photons (just like metals) - ANS-why is graphite shiny?
b/c of the 4 hydrogen bonds around each water molecule - ANS-why does ice take up a
hexagonal crystal form?
between molecules - ANS-where are hydrogen bonding interactions present? (between/within
molecules)
bonding between C has to be broken - ANS-to melt/decompose diamond, what has to happen?
C atom has 4 valence electrons in different types of orbitals - ANS-How can carbon form 4
identical bonds in diamond?
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