Download Solvent Properties Of Water File - District 196 e

Why can we make so many
aqueous solutions?
• H2O is known as the “universal solvent”
because it can dissolve or be miscible with
most ionic and polar substances
***Remember the “Like” dissolves “like” rule
Ionic
• A compound that contains a cation (+)
and anion (-) formed through the
transferring of electrons.
• Water can dissolve many ionic
compounds because of its attraction to
the charges on the compound
(opposites attract)
• See solubility chart for exceptions:
Examples
• Water can make an aqueous solution
with:
NaCl
See how water breaks it apart with video link below:
https://www.youtube.com/watch?v=xdedxfhcpWo
Water cannot make an aqueous solution
with:
CaCO3
*forces are too strong to break apart (see
solubility chart)
Polar Bonding
• Between 2 nonmetals through the
unequal sharing of electrons
• Check electronegativities (.5> and <1.6)
• Draw dipoles toward the element with
greatest electronegative value to show
where electron distribution is the
greatest
Examples
• C --- O
• S ---Cl
Nonpolar Bonding
• Between 2 nonmetals through the equal
sharing of electrons
• Check electronegativities (<.5)
• No dipoles are needed
Examples
• C --- H
• I --- I
Polar Molecules
• A covalently bonded substance where
dipoles do not cancel because of the
unequal distribution of electrons
throughout the substance.
• Based on geometry/asymmetry of the
molecule.
• Most bent and trigonal pyramid
substances are polar
Examples
• H 2O
• NH3
Nonpolar Molecules
• A covalently bonded substance where
dipoles cancel because of the equal
distribution of electrons throughout the
substance.
• Based on geometry/symmetry of the
molecule.
Examples
• O2
• CH4
Ionic, Polar or Nonpolar?
• Ethanol C2H5OH
• Benzene C6H6
• Boron Trichloride BCl3
• Lithium Bromide LiBr
Examples
• Ethanol C2H5OH
• Boron Trichloride BCl3
• Benzene C6H6
• Lithium Bromide LiBr
Soluble In Water?
• Ethanol C2H5OH
• Benzene C6H6
• Boron Trichloride BCl3
• Lithium Bromide LiBr