Transcript Chemistry review ppt edited

Chemical Basis for
Life Chapter
2
Why do we need
Chemistry in A and P?
• Your human body is a highly
organized and ever changing
collection of chemicals.
• There is also a very specific amount
of each of these chemicals in your
body.
What do you think might
happen if any of these
chemicals are out of balance?
Any change in any of the chemicals in
your body can have drastic affects on
your health and could even cause death.


For example: if you have too little iron
in your body this can lead to a disease
known as anemia.
 On the flip side, if you
have too much iron you
have hemochromatosiswhich can eventually
destroy your heart
pancreas and liver.


Matter is anything that takes up space
and has mass.
Matter is made of atoms, which are the
smallest particles of an element that
still have all the properties of an
element.

States of Matter
◦Solid
◦Liquid
◦Gas


All matter is composed of substances
called ELEMENTS.
Elements are what you find on the
periodic table. Can anyone name any
Elements?
What do you think are some of
the major elements found in
the human body?
Living organisms require about 20 elements (There
are 92 elements in nature and 19 made)
Oxygen, Carbon, Hydrogen, and Nitrogen make up
more than 95% of the human body.
The other elements include: calcium, phosphorus,
potassium, sulfur, chlorine, sodium, magnesium and
many other trace elements (meaning they have a very
small amount: iron, zinc, copper, etc)
 Smallest
 Made
amount of an element
up of 3 subatomic particles
◦ Neutrons (o) = neutral/no charge
◦ Protons (+) = positive charge
◦ Electrons (-) = negative charge


Protons and
Neutrons are found
in the nucleus of the
atom.
Electrons are in
motion in the space
around the nucleus.
# E- = # P+
Why is this important and what
does it have to do with anatomy?
The positive charge from the Proton and the
Negative charge from the electron balance
out the charge of the atom.
These charges are what eventually aid in
forming combinations of atoms- or chemical
compounds …for example: water is made
from Hydrogen and Oxygen.
1 tell 2 what you think would happen to
the charge of the atom if it were to
loose an electron.




Proton (+) = the guy
Electron (-) = the girl
Neutron (o) = the wing man
The electron is attracted to it’s opposite
charge (the proton +) so it remains in orbit
around the nucleus, but it plays “hard to get”
by maintaining a velocity that is fast enough
that it’s never pulled into the nucleus. The
neutron is there to support the nucleus but it
never gets involved.
 STOP
POINT! 
 Atomic
structure hand out
What would the electron distribution for Calcium with an atomic
number of 20 be? How does this reflect to the Matterville analogy?
Nucleus
What would the electron distribution for Neon with an atomic number
of 10 be?
Nucleus
Chemical compounds are formed by chemical bonds.
Atoms either lose electrons, gain electrons or share
their electrons in order to form a bond with other
atoms in your body.
Atoms that lose or gain and electron are called ions
(it is now chemically charged…the charges don’t
balance)
Example: Na+Cl*Na loses an electron
*Cl gains an electron (they
exchange electrons)
The opposite charges
attract and form a bond
called an ionic bond
2 ask 1 why do you think Na has a
tendency to lose an e- where Cl
have a tendency to gain an e-?
Covalent bonds form when atoms
share their electrons instead of
exchanging them.
Example:
Carbon molecule:
•H and O form a covalent
bond that creates the molecule
water.
•This molecule has + and –
poles!
•These charges cause the
water molecules to bind
loosely to each other. This
loose binding is known as a
Hydrogen bond ( Hydrogen
bond because Hydrogen is
involved) (cross out #1 in
notes)
• Hydrogen bonds are weak bonds.
• What do you think that means?
• They can break apart easily.
• How would this be helpful in the body?
• Many systems require water so the
molecules need to be able to break apart
easily for easy transport. Cross out C and
write this.



STOP POINT!
IN SMALL GROUPS provide a visual
demonstration/skit of your assigned
Chemical Bond. This will count toward class
participation points.
Hydrogen bonds, Ionic Bonds, Covalent
bonds.

Chemical Reaction – a
process that changes one
set of chemicals into
another.
◦ Involves the breaking and
forming of new bonds. Quantity
remains the same.
•
•
•
1+1=2
1+1 2
If this represented a
chemical reaction, then
1=reactants and 2 =
product
The reactants “react” to form
the product.
Synthesis/Anabolic Reaction:
when two or more atoms
bond to form a more complex
structure.
Example: fixing worn or
damaged tissues requires a build
up of smaller molecules coming
together to make a larger
molecule.
A+B
AB
Decomposition/catabolic
reaction: When a bond
holding atoms together
breaks and produces a
simpler molecule.
Example: Is needed for foods
to be digested and energy to be
released for your body to use.
AB
A+B
All reactions need energy to occur.
 Activation Energy – refers to the energy
needed to get the reaction started
For example, you must apply force when
striking a match to get the fire to start.
 Rollercoaster example

•
•
Notice the different energy
levels between the reactants
and products.
Example: photosynthesis –
reactants of water and CO2
and energy from the sun
(activation energy) creates
products of Glucose and O2.
•
•
Notice the different energy
levels between the reactants
and products.
Example: combustion
reactions of fuels.
• 1 ask 2 “do you
think Exothermic
reactions are
anabolic or catabolic
and why?”


Name 2 Endothermic reactions and 2
exothermic
What type of bonds form water?
Catalysts

Catalyst - a substance that lowers a
reactions activation energy
◦ In other words, speeds up the reaction.
Enzymes
Biological Catalysts are
called Enzymes.

They speed up chemical
reactions in the cells. However
they are not essential, for the
reactions can occur on their
own

Enzymes
•The names of enzymes typically end in “-ase”
•For example: protease splits proteins into its
monomers - amino acids.
•What do you think carbohydrase does?
•Splits carbohydrates (polysaccarides) into its
monomers - monosaccarides.
•Also used for: protein synthesis, synthesis
of RNA and DNA, etc.
 STOP
POINT!
 Chemical
Reactions Review
worksheet.
Inorganic and Organic
Compounds
• The atoms and molecules that form compounds can
either be inorganic or organic.
• What is the difference?
• Inorganic are substances that can dissolve in water or
react with water to release electrolytes.
• Why might these be necessary for your body?
• Organic are substances that contain carbon,
hydrogen and oxygen and do not dissolve in
water.
• Why might these be important?
Organic Compounds
found in the body
••
Carbohydrates
••
Lipids
••
Nucleic Acids
••
Proteins
What are these?
Carbohydrates
What do you think the importance of
Carbohydrates are?
1.Provide energy that your cells
and body need.
2. Help build cell structures.
Carbohydrates
Examples:
1. Sugars- Monosaccharides such as Glucose,
Fructose, and Galactose
2.Disaccharides- Which contains two
monosaccharides. Such as: sucrose
3. Polysaccharides- many monosaccharides
combined together like a chain. Such as: Starch,
glycogen
LIPIDS

Glycerol + 3 Fatty Acids = Lipid
1 Glycerol
3 Fatty Acid
Chains
 Carbon, Hydrogen, & Oxygen
LIPIDS
FUNCTION
Lipids functions are:
1.Help in long term energy storage
2.Protection and Insulation
3.Membrane structure
4.Acting as a chemical messenger
LIPIDS
FORM
Lipids can be:
1.Fats
2.Steroids
3.Phospholipids
How do you think
the form relates
to the function?
Which type of
lipid is
responsible for
what function?
Proteins
Proteins Functions are:
1.Help in structure of bones and muscle
2.Regulate cell processes and chemical reactions
3.Help transport substances in and out of the cell.
4.Help fight against foreign substances
Protein Forms include:
1.Enzymes
2.Hormones
3.Antibodies
4.Structural proteins
Proteins
Which forms go with
which functions?
Nucleic Acids
Nucleic Acid Functions:
1.Form genes- store genetic info and transmit
genetic information
2.Help aid in protein synthesis.
Nucleic Acid Forms:
1.DNA
2.RNA
What are the four essential
organic compounds found
in living things?
What is the difference
between inorganic and
organic compounds in the
body?
Compound
inorganic
Primary
Compounds
organic


What do some people drink Gatorade while
they exercise?
Give three examples of carbohydrates
Stop Point:
Organic Compounds
Foldable



Characteristics of Living Things Group activity
At your tables brainstorm a list of things that
organisms (living things) must do to be
considered living. (5 minutes)
Volunteer a spokes person to come write
what you came up with on the board.
 Brainstorming:
1.Growth: change in size
2.Respiration: Obtaining oxygen, releasing
energy from food and storing it in ATP,
removing carbon dioxide
3.Digestion: breakdown of food into nutrients
4.Absorption: movement of substances
through membranes into body fluids
5.Movement: change in body position or of body
part, internal movement
6. Responsiveness: Reaction to change inside
or outside body
7. Reproduction: production of new organisms
(not required for individual survival) and cells
8. Circulation: movement of substances in
body fluids
9. Excretion: removal of waste products
10. Maintaining homeostasis: regulates its
internal environment and tends to maintain a
stable, constant condition
Brainstorm in your groups what you
think your body needs to live.
Hint: without it you will die- only those
that are necessary- not that would be
helpful.





Water: provides environment for chemical
reactions, transports substances, maintains
body temp. (carries heat)
Pressure atmospheric pressure forces air
into lungs, hydrostatic pressure moves blood
Food provides body with nutrients
Heat higher the heat the faster chemical
reactions occur in body
Oxygen helps release energy from glucose
(energy is then stored in ATP)
 Sleep