Hydrogen Bonding
SURFACE TENSION
Hydrogen Bonding results





the hydrogen
- ex. the water droplets below and the water
strider above are all caused by water’s surface
tension
COHESION


Water is a polar molecule
Water is attracted to itself by hydrogen
bonds
ADHESION


Occurs when water is attracted to other materials
The water below is attracted to the glass of the
graduated cylinder
LOW VAPOR PRESSURE

Vapor pressure- pressure produced when vapor particles
above a liquid in a sealed container collide with the container
walls.

The tendency of water molecules to escape liquid form is low
HIGH HEAT OF VAPORIZATION
LOW SOLID DENSITY
-liquid water can absorb a large amount of
heat before completely turning into a gas
because hydrogen bonds resist individual
water molecules from breaking away
water molecules are
closer together and
free to move
water molecules are far apart
and in a fixed position
Density
Mass
=
Volume
UNIVERSAL SOLVENT


- many
 water can
Covalent Compounds
(2 or more nonmetals)
Ionic Compounds
(metal and nonmetal)
Polar
Non– polar
Define the following terms
solventsolute–
solubilitysolution
miscible–
immiscible-
solute
solvent
―Like dissolves like‖

-
dissolves in
-ex. fats, oils, waxes (non-polar) will not dissolve in water (polar), but will dissolve in
gasoline (non-polar)
dissolves in
SOLVATION (dissociation)


Process that
During solvation
- The waxy cuticle on this leaf is non polar
and the water droplets are polar therefore
the water is repelled from the leaf
1) TEMPERATURE

kinetic energy
- the amount
ex. sugar dissolves quickly in warm coffee
-

carbonated beverages— soft drinks, like Dr. Pepper or Sprite, have carbon dioxide dissolved
in them
ex. All soft drinks lose carbonation if not kept cold.
-
Solid solute breaks up
faster if particles have
a higher kinetic energy
(moving faster).
2) PRESSURE
Solid solutes are _________soluble at ___________
Gas solutes are ______ ______ under ______ pressure
and _____soluble under _______ pressure


Gas particles move faster
as temperature increases
allowing them to leave
solution.
Henry’s Law
The amount of gas dissolved
in solution is directly
proportional to the pressure
of the gas over the solution
3) PARTICLE SIZE

The smaller
- sugar granules dissolve faster than sugar cubes
less surface
area
more surface
area
4) agitation of solution
(Stirring/shaking)
Solid & Liquid Gas Anybody ever open a bottle of soda after it was shaken?
Gas vs. Solid Solubility
Temp ↑
Temp ↓
Pressure ↑
Pressure ↓
Particle Size ↑
Particle Size ↓
Agitation ↑
Agitation ↓
Gas
Solid
SOLUBILITY RULES
Alkali Ions (Li, Na, K, etc)
Hydrogen (H+)
Ammonium Ion (NH4+)
All Nitrate NO3- ions
All Acetate CH3COO or
C2H3O2
Soluble
Soluble
Soluble
Soluble
Soluble
Chlorate, ClO3-1, and Perchlorate, ClO4-1
Soluble
Chloride, Cl-
Bromide, Br
Iodide, I-
-
Fluoride, F
Sulfate,
SO4-2
Sulfide, S-2
Hydroxide, OHPhosphate, PO4-3
Chromate, CrO4-2
Oxalate, C2O4-2
Carbonate, CO3-2
Sulfite, SO3-2
Ag, Pb+2, Hg2+2, Cu+,Fe+3—>
Insoluble (low solubility)
All Other Positive ion—>
Soluble
Mg+2, Ca+2, Sr+2, Ba+2, Pb+2-->
Insoluble
All Other Positive ions-->
Soluble
Ba+2, Sr+2,Pb+2-->
Insoluble
All Other Positive ions-->
Soluble
Alkali Ions, H+, NH4+, Be+2-->
Soluble
Mg+2,Ca+2,Sr+2, Ba+2-->
Soluble
All Other Positive ions-->
Insoluble
Alkali Ions, NH4+,Sr+2, Ba+2-->
Soluble
All Other Positive ions-->
Insoluble
Alkali Ions, H+, NH4+-->
Soluble
All Other Positive ions-->
Insoluble
unsaturated saturated supersaturated -
Crystallization occurs when
supersaturated solutions
cool down
- this flask of water would
become saturated when all of
the space between the water molecules is taken up by a
solute.
heating up the water
would cause the molecules
to spread out providing
more room for a solute than
is normally there
(supersaturated)
-
Used to determine
saturated
unsaturated
supersaturated
add solvent
High
Molarity
Low
Molarity
add solute
Concentrated solution- _______amount of solute, _____ amount
of solvent (ex. very sweet kool-aid)
Moles of solute
Molarity =
Liters of solution
Dilute solution- ___amount of solute, ____ amount
of solvent
(ex. watered down kool-aid)
What is the molarity of a solution of
HCl if 3 moles of HCl is dissolved in
2.5 liters of water?
How many moles of NaCl are present
in 200 mL of a 3 M solution of salt water?
If 20 grams of KCl is dissolved in 5
liters of water what is the molarity of
the solution?
How would you make a 1 M solution
of NaCl?
2
1
Stock solution
Dilute solution
Dilution Formula
MsVs
Stock solution
=
MdVd
Dilute solution
1) How many milliliters of a 5 M NaCl stock solution are needed to make 200 mL of a 0.171 M NaCl solution?
2) What volume should 100 mL of a 12 M HCl stock solution be diluted to in order to make a solution of 3 M HCl?
3) If you need 1 L of a 1 M NaOH solution, how many milliliters of a 10 M stock solution should you dilute?
Dissociation
ionic
compound

covalent
compound
Electrolytes are ionic compounds - this includes acids, bases, and salts
Strong Elecrolytes
Acids
HCl
HBr
HI
HNO3
H2SO4
HClO4
Bases
NaOH
KOH
Mg(OH)2
NH3 +
Salts
KCl
MgSO4
KClO3
CaCl2
H2O
HCl
+
H2 O
KCl
+ H2 O
NH4+ + OHH3O+ +
Cl-
H2O + K+ + Cl-
Changes in the physical properties of a mixture not based on the identity of the solute but based on the number of particles in a solution. Ionic compounds have a greater effect because they break up into more particles through dissociation.
NaCl (salt) breaks up into Na+1 and Cl-1 when put into water, but sugar does not dissociate.
Vapor pressure decreases – slows down evaporation
Boiling Point increases –
raises temperature at which solvent boils (Ex: Adding salt to pasta)
Freezing Point decreases – lowers temperature at which solvent freezes (Ex: (Adding salt to icy roads)