Metallic, Ionic or Covalent Bonds
Lewis Structures
Intermolecular Forces
Polar or Non-Polar?
Molecular Geometry
100
electrons are shared
covalent
100
What is wrong with Lewis dot structure "B"?
Each hydrogen has too many bonds.
100
intermolecular forces are the forces _______ molecules
100
The bond between sodium and chlorine in NaCl
Polar
100
What is the molecular geometry of a molecule of Br2?
linear
200
luster and ductility
metallic
200
What is wrong with Lewis dot structure "F"?
Oxygen does not have an octet.
200
Which is is the strongest IMF: dipole-dipole, H-bonding, or London Dispersion forces?
dipole-dipole
200
The molecule H2O
Polar
200
What molecular geometry is demonstrated in the following image?
trigonal pyramidal (3 atoms, 1 lone pair)
300
high melting and boiling points
ionic
300
Methanol is an alcohol that can be used to produce acetic acid found in vinegar. Draw the Lewis dot structure for methanol (CH3OH).
300
Which is the weakest intermolecular force: dipole-dipole, H-bonding, or London Dispersion forces?
London Dispersion forces
300
The bond between Carbon and Oxygen in CO2
Polar
300
Which compound below has a molecular geometry that is tetrahedral?
SiO2 BF3 HCl CCl4
CCl4
400
nonconductors in the solid, molten, and dissolved state
covalent
400
Ammonia is a substance used in creating fertilizers to use on farms. Draw the Lewis structure for ammonia (NH3).
400
Hydrogen bonding occurs between molecules with bonds between Hydrogen and what three other atoms?
Nitrogen, Oxygen, Fluorine (NOF)
400
The molecule NH3
Polar!
400
What is the molecular geometry of SO3. Draw the Lewis dot structure to help you!
trigonal planar (3 atoms, 0 lone pairs)
500
electrons delocalized
metallic
500
Phosphate is a polyatomic ion present in bones, genes, teeth. Draw the Lewis structure for phosphate (PO43-).
500
London Dispersion forces come from the random motion of...
electrons
500
The molecule CO2
Non-polar.
500
Why do we say that the polarity of a tetrahedral molecule "depends"?
The polarity depends on what surrounds the central atom.
If all of the surroundings atoms are the same, the dipoles cancel, and the molecule is nonpolar (symmetrical).
If the surrounding atoms are different, the dipoles do NOT cancel, and the molecule is polar (asymmetrical).
