2. Properties of Water
1. abundant
Water is the most _________
inorganic compound for living
organisms because most cellular
activity takes place in water.
2. Water is a _________ bonded
covalently
compound.
3. Properties of Water
3) expands
Water __________ when it
____________ causing ice to be
freezes
less dense than liquid water, so
lakes freeze from the top down.
4.
5. Properties of Water
4) absorb
Water can _____________ a lot
of _________ without changing
heat
temperature.
6. Properties of Water
5. polar
Water is a ________ molecule,
meaning there is a greater chance of
finding shared electrons orbiting
oxygen
around the __________ atom than
hydrogen
the __________ atoms.
a) Oxygen has ______ protons in its
8
nucleus and thus has a much
stronger
_________ attraction for electrons than
1
does hydrogen with only ______ proton
in its nucleus.
7. Properties of Water
b) This uneven sharing gives oxygen
negative
a slight __________ charge, while
positive
hydrogen has a slight _________
charge.
9. Properties of Water
c) The positively charged H of one molecule
is attracted to the negatively charged O
of another water molecule, forming a
hydrogen bond
_______________. Hydrogen bonds are
__________ than ionic or covalent
weaker
bonds.
O(-) Hydrogen
H(+) H(+) Bond
O(-)
H(+) H(+)
15. Properties of Water
6) mixture
A __________ is a material
composed of two or more
elements or compounds that are
physically
_____________ mixed together
chemically
but not ________________
mixed together.
a) Water can form 2 mixtures.
16. Properties of Water
i. Water as a solution
1) universal solvent
Water is the “_______________”,
or a substance in which the solute
dissolves.
2) Water’s ___________ gives it the
polarity
ability to dissolve both ionic
compounds and other polar
sugar
molecules, such as _________
salt
and ___________.
19. Properties of Water
ii. Water can also be
involved in
suspensions
____________, which
are mixtures of water
and non-dissolved
material.
7) Blood can be both a
solution
___________ and a
suspension
_____________.
20. Acids, Bases and the
pH Scale
1) When an ionic
compound, such
as NaCl forms a
solution with
water
________, the
compounds
break apart and
form ions.
21. Acids, Bases and the
pH Scale
2) Water
sometimes
breaks apart
into ions as
well, at a rate
of 1 in 550
million
molecules of
water.
22. 3) When solutions contain ______
equal
amounts of OH- and H+, they are
considered _________.
neutral
23. Acids, Bases and the
pH Scale
3) When solutions contain more
______ than OH-, they are
H+
considered _________.
acidic
4) When solutions contain more
OH- than H+, they are
______
basic
considered _________.
26. Acids, Bases and the
pH Scale
5)We use a scale to represent the
a) pH scale
“p” stands for ____________.
b) potential
“H” stands for ____________.
hydrogen
27. Acids, Bases and the
pH Scale
The numbers on this
scale stand for a
negative power of 10.
For example, a pH of 5
would mean that there The pH
are 1 x 10-5 H+ ions in Scale
the solution.
Therefore, as you move
up on the pH scale, the
number of H+ ions in
solution inversely goes
down.
28. pH Example
pH 9 = 1 x 10-9 = .000000001
pH 5 = 1 x 10-5 = .00001
pH 4 = 1 x 10-4 = 10x
.0001
pH 3 = 1 x 10-3 = .001
pH 2 = 1 x 10-2 =
.01
pH 1 = 1 x 10-1 =
.1
32. Acids, Bases and the
pH Scale
6) Buffers acids
_________ are weak ______ or
______ that react with strong
bases
acids and bases to prevent a
change in pH.
7) Most cellular fluids must remain
at _________ or chemical
6.5-7.5
reactions will be affected.
33. Ben’s Bad Day -
Revisited
Lactic acid build- up (pH goes down)
H+ + HCO3- H2CO3 H2O + CO2
exhale
