Transcript Chapter 3

Chapter 3
Matter and Energy
Vocabulary
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Acid
Amino acid
Carbohydrate
Coenzyme
Covalent bond
Element
Enzyme
Ionic bond
Kinetic energy
Molecule
Polypeptide
Potential energy
solution
activation energy
bond
chemical formula
compound
electron cloud
energy level
ion
isomer
lipid
nucleic acid
polysaccharide
protein
Matter and Its
Combinations
• All matter is made up of
atoms.
• Protons (+ charge) and
neutrons (no charge)
are in the center.
• Electrons ( - charge)
are outside of the
nucleus in an electron
cloud.
• Click here!
Energy Levels
• Electrons travel around
the nucleus at different
energy levels. The farther
away from the nucleus an
electron is, the more
energy it has because it’s
farther away from the pull
of the positively charged
protons.
Atom Song
(3:28)
• The first energy
level closest to the
nucleus can hold
up to 2 electrons.
• 2nd level: up to 8
electrons.
• 3rd level: 18 e• 4th level: 32 e-
Elements
(2:05)
• Elements are substances composed of
only one kind of atom.
• The number of neutrons in any given
element are the same except in isotopes.
• Isotopes have different numbers of
neutrons and thus different masses then
the most common form of any given
element. Examples: C-12 and C-14 are
isotopes of carbon. One has a mass of
12 amu and the other a mass of 14 amu
because it has more neutrons.
Elements vs. Compounds
• Elements
• Compounds
• Carbon: C
• Methane: CH4
• Hydrogen: H
• Hydrogen molecule: H2
• Oxygen: O
• Oxygen molecule: O2
• Nitrogen: N
• Nitrogen molecule: N2
• Phosphorous: P
• Phosphate ion: PO4 3-
Covalent vs Ionic
bonding
• When atoms combine
chemically by sharing
electrons, they have
formed a covalent
bond.
• Ions are atoms that
have given up or
taken electrons.
Compounds that are
formed by ions (2:12) are
called ionic
compounds. (17:38)
Chemical equations
• Chemical equations use formulas to
describe chemical changes that take
place. Numbers of atoms before the
reaction and after the reaction must be
the same.
• Reactants  Products
• Hydrogen + Oxygen produces water
• H2 + O2  H2O (unbalanced equation)
• Balanced, this equation is:
• 2H2 + O2  2H2O
Balance these
equations:
• Zn + HCl  ZnCl2 + H2
• Mg + H2O  Mg(OH)2
• Mg(OH)2 + HCl  MgCl2 + H2O
• NaClO3  NaCl + O2
• CH4 + O2  CO2 + H2O
Solutions
• Solutions are homogeneous
mixtures that are the same
throughout, although they can have
varying amounts of dissolved
substances in them.
• So, why do some things dissolve in
water and others don’t?
• Potassium permanganate
dissolution demo 1. (click here)
• Demo 2 (click here)
(1:00)
(1:00)
Acids and Bases
Introduction to Acids/Bases (2:04)
pH Scale (2:42)
pH in the Chemistry of Nature (3:19)
3.2 Biological Chemistry
• Carbon compounds
– Structure
– Isomers
• Carbohydrates
– Monosaccharides, Disaccharides and
Polysaccharides
• Lipids
– Structure
• Proteins
– Structure
• Nucleic Acids
– Condensation Reactions
– Hydrolysis
Carbon Compounds
• Living organisms
as well as
substances like
fossil fuels are
made up of carbon
compounds.
Carbon has 4
valence electrons
that can form
single, double and
triple bonds.
Isomers
• Isomers are molecules that
have identical formulas but
different structural
arrangements.
• Both of the molecules →
have the formula C6H14 but
have different structures.
• These different shapes do
not constitute different
compounds. To get a
different compound the
bonding pattern of the
atoms would have to
change.
Branched chain isomers (4:36)
Carbohydrates
• Carbohydrates are organic
compounds made up of 1 part
carbon to 2 parts hydrogen and 1
part oxygen, or a 1:2:1 ratio.
• Glucose, galactose and fructose are
examples of simple sugars called
monosaccharides.
• Intro to carbohydrates
(2:00)
• Two simple sugars
can bond together
to form
disaccharides.
Sucrose (table
sugar), is made up
of glucose and
fructose bonded
together.
• Monosaccharides and
disaccharides (click here)
•
(2:16)
Complex Carbohydrates:
Polysaccharides ( click)
(4:32)
Glycogen
• Polysaccharides are
formed from long chains
of monosaccharides.
• An example is glycogen
which is made up of
glucose. The body can
store the glycogen and
then convert it back to
glucose when needed.
• Others include cellulose
and starch.
Assignment:
Using a Venn Diagram, compare and
contrast simple and complex
carbohydrates
Fats, Lipids and Fatty
Acids
• Fats and oils belong to
a class of organic
compounds called
lipids.
• Are fats good?
(3:07)
• Lipids and cholesterol (1:12)
• Fatty Acids
•
(2:45)
Proteins and Amino
Acids
(2:30)
• What is protein?
(3:05)
• Proteins are built
from chains of amino
acids. They have a
central carbon atom
bonded to a carboxyl
group, a hydrogen
atom and an amino
group.
• The bonds that form
proteins are called
peptide bonds. (2: 23)
Nucleic Acids
DNA Molecule
• Molecules that
control an
organism’s basic
appearance and
behavior are
called nucleic
acids.
• These include
deoxyribonucleic
acid (DNA) and
ribonucleic acid
(RNA).
Condensation Reaction
• Maltose is a large
disaccharide
formed from the
condensation
(water producing)
reaction between
two glucose
molecules.
• Amino acids from
the foods you eat
form proteins with
this type of
reaction.
Two glucose molecules react
to form maltose and water
Hydrolysis
• Hydrolysis (2:10)
occurs when the
addition of a water
molecule breaks
up a larger
molecule into
smaller molecules.
• A dipeptide +
water can yield
two amino acids
such as glycine
and alanine.
Formation of glucose and fructose
by adding a water molecule to sucrose
ENERGY!!!
• Potential and
Kinetic Energy
(2:07)
• Law of
Conservation of
Energy
(4:35)
Potential and Kinetic Energy
Activation energy/Enzymes
• Activation energy is the
smallest amount of
• Enzymes are proteins
energy it takes to start
that lower the
a chemical reaction.
activation energy
• Different reactions
needed for chemical
require different
reactions in cells.
amounts of energy.
Heat is a common form
of energy used to start
a chemical reaction,
but is not practical
when looking at
biochemical reactions
because too much heat
↑
would kill cells.
I am an enzyme, click on me! (1:37)
Enzymes/Substrates
• Enzymes are reusable and each has a
unique shape that determines its
chemical function.
• Substrates work with enzymes in
chemical reactions.
• Most enzymes are named by adding the
suffix –ase to the name of the substrate
reaction the enzyme controls. ie: the
enzyme that guides the conversion of
maltose to glucose is called maltase.
Substrates/Coenzymes
• Substrates attach themselves to enzymes, which
change shape slightly which lowers the activation
energy needed because the active site of the
enzyme will only fit together with a certain part of
the substrate.
• Coenzymes sometimes made from vitamin
molecules, are reusable, and needed in small
amounts. They are enzymes’ little helpers by
helping substrates bind or transferring atoms from
one substrate to another..
Micro Elements
(next 9 slides)
• Iron (Fe) Contained in hemoglobin and
myoglobin which are required for oxygen
transport.
• Anemia results from a lack of Fe.
• Enlarged liver, diabetes and cardiac
failure can be caused by too much iron.
• Hemochromatosis is a genetic disease
caused by excess iron absorption.
• Potassium (K) is a major electrolyte
of blood and extracellular fluid.
Maintains pH and osmotic balance.
• Chlorine (Cl) Major electrolyte of the
blood and intracellular/extracellular
fluid. Maintains pH and osmotic
balance.
• Sulfur(S) Part of essential amino
acids. Contained in vitamins,
thiamin and biotin. Part of
glutathione
and required for
detoxification.
• Copper (Cu) regulates Fe transport
and release from storage.
• Too much copper can cause liver
disease and is associated with the
genetic disorder, Wilson’s disease,
where excess copper affects the
brain, eyes and kidneys.
• Manganese (Mn) Needed for bone
formation and reproduction. Too
much causes poor Fe absorption.
Iodine: Produces thyroxine which
controls metabolic rate and
prevents goiter.
• Zinc (Zn)
• Selenium (Se)
important for
Deficiency esults
reproduction,
in oxidative
required for DNA
membrane
binding which
damage. In
regulate a variety
humans it causes
of activities. An
heart damage,
excess can cause
known as
anemia or reduced
Keshan’s Disease.
bone formation.
• Fluorine (F) Tooth
development and
protection.
• Strengthens
enamel to prevent
decay.
• Cobalt (Co) An
excess may cause
cardiac failure.
Macro elements—essential for
proteins and enzyme activity
• Calcium: Ca
Structure of bones
and teeth
• Phosphorous: P
• Structure of bones
and teeth,
required for ATP
production.
• Magnesium (Mg)
Bone structure,
too little results in
muscle spasms
and can lead to
Ca deficiency.
• Sodium (Na)
Major electrolyte
of blood and
extracellular fluid.
Maintains pH and
osmotic balance.
• Molybdenum (Mo) An
excess can cause
diarrhea and growth
reduction.
• Chromium (Cr) Helps
regulate sugar levels.
Deficiency may cause
hyperglycemia
(elevated blood
sugar) and
glucosuria. (sugar in
urine)