Bond Polarity
Lewis to 3D
Water
Gases
100
Definition of an Ionic bond (include types of elements that do this)
Non-metals steal electrons from metals, creating oppositely charged ions that stick together.
100
Draw the lewis structure, including any partial charges, and determine the 3d shape.
Te2
Linear, non-polar double bond with 2 lps on each
100
Describe how you would draw a hydrogen bond
Dotted line connecting a positive charge on one molecule and a negative charge on the other
200
Definition of a polar covalent bond (include types of elements that do this)
Non-metals share an electron unevenly, resulting in partial charges based on differences in electronegativity.
200
Draw the lewis structure, including any partial charges, and determine the 3d shape.
CAtF3
tetrahedral, all single bonds, At partial plus, Fs partial negative, polar molecule
200
In general, what would you expect to be true about a hydrophilic molecule
Polar or ionic, that is anything with charge
200
If temperature is constant, what happens to the pressure in a container if the volume of the container increases.
Pressure goes down (creates a vacuum)
Think pulling a syringe back
300
Definition of a hydrogen bond
Atoms ability to attract an electron
300
Draw the lewis structure, including any partial charges, and determine the 3d shape.
SbAtH2
trigonal pyramidal, Sb central with 1 lp, no partial charges, non-polar
300
In general, what would you expect to be true about a hydrophobic molecule
All covalent bonds, Non-polar molecules, no charges
300
What happens to the temperature of a gas in a container if the pressure is increased
Temp goes up
Compressing causes more molecular movement/collisions between molecules
400
Which would you expect to have a larger atomic radius Zr or Te, and why?
Zr, same row but farther to the left, has same number of shells but fewer protons, electrons are less attracted to nucleus (lower electronegativity).
400
Draw the lewis structure, including any partial charges, and determine the 3d shape.
SiS2
linear, 2 double bonds, S partial negative, Si partial plus, non-polar (symetrical)
400
Which would you expect to have a higher boiling point,
CH4 or H2O, and WHY
CH4 molecules are symmetrical/non polar, can’t hydrogen bond with each other the way water does, makes it easier for them to evaporate
400
500
Which would you expect to have a larger atomic radius Po or Se, and why?
Po, same column, lower down, more shells, valence electrons farther from nucleus and have more repulsive electron shells between them and protons, less access/lesser attraction to protons (lower EN)
500
Draw the lewis structure, including any partial charges, and determine the 3d shape.
SnPoH2
trigonal planar, Sn central Po double bonded, no partial charges.
500
