Unit 6 Flashcards
What is the VSEPR theory?
valence shell electron pair repulsion
electrons don’t want to be next to each other
what does the VSEPR theory determine
the shape of an atom/molecule
when the central atom has unshared electrons, the angles between bonding pairs will be ______ than when all central atom’s electrons are shared
smaller
What are electron domains?
the bonding regions which determine the shape
which elements are ok with more than 8 valence electrons?
row 3 and below
which elements are ok with less than 8 valence electrons?
B and Be
double, single, and triple bonds only count as ___ region
1
several atomic orbitals mix to form the same total number of equivalent hybrid orbitals whatever you mix you need to get the same number back out
orbital hybridization
linear, trigonal planar, tetrahedral, trygonal bipyramidal, and octahedral are all what?
types of hybridization
Name, draw electron dot structure, find shape, and hybridization of the following
NBr3
CO2
BF3
what makes a molecule nonpolar?
The molecules shape has no lone pairs or if it does it’s either square planar or linear.
What are inTRAmolecular forces? And draw a picture of it
attractive forces that occur inside the molecule.
What are inTERmolecular forces? And draw a picture of it
attractive forces between two molecules
What determines the boiling and melting points of a molecular compounds?
inTERmolecular bond
Rank these from strong to weak molecular force
liquids, solids, and gases
solids, liquids, gases
The two weakest attractions between molecules are collectively called______. These two forces are _________ _____ and _________ _____.
Vander Waals
dispersion forces
dipole interactions
REMEMBER TO PUT BRACKETS ON CHARGED LEWIS DOT STRUCTURES
Draw an example of dispersion forces
Would a hydrogen molecule with dispersion force or Neon molecule with dispersion force have a stronger pull and higher boiling point
Neon because it has more valence electrons
If an atom or molecule has electrons then they are engaging in _______________.
dispersion
draw a picture of dipole interactions using H and Cl
draw a picture of hydrogen bonding and an example of something that’s not
List the substances BaCl2, H2, CO, HF, and Ne in order of increasing boiling points
H2 Ne CO HF BaCl2
What are the steps to organizing substances in order of increasing boiling points
find an ionic compound (metal paired with non-metal)
Hydrogen bonding
Dipole (polar bond)
Dispersion (more number of electrons= higher boiling point)
