Transcript Entire

Do Now
• What is an atom?
• Why do we have a periodic table?
• What information can we find in a periodic
table?
Chapter 6
Biochemistry
Objectives
• To define an atom.
• To determine the make-up of an atom.
• To list different elements that can be found
on Earth.
• To explain what type of information can be
gathered from the periodic table.
Brain-Based Learning
Name __________________
Neutron
Proton
Electron
Atoms
• Building blocks of matter
• Contain 3 parts
+
-
– Protons: positively charged, contain mass
– Neutrons: no charge, contain mass
– Electrons: negatively charged, insignificant
mass
Atoms make up Elements
• a pure substance that can’t be broken
down into other substances by physical or
chemical means.
• Made up of only 1 type of atom
• Contain a unique name and symbol.
Periodic Table of Elements
• Periods: horizontal
rows
• Groups: vertical
columns
– elements in the same
group have similar
chemical and physical
properties.
**Organized based on the # of protons in the nucleus of an atom.**
Periodic Table Information
• Atomic number- tells
us the # of protons
(and electrons)
• Symbol- unique for
each element.
• Atomic Mass- # of
protons and neutrons
6
C
12.02
Practice Problems
4
9.01
C
12.02
7
N
Ne
20
Complete the missing information
and include the number of protons,
neutrons, and electrons.
Neutron Partners…
• List the number of protons, neutrons, and
electrons for the following…
– Mg
– Ca
– Fe
– Cl
Drawing an atom…
• Things to remember!
– Proton # = Electron #
– Protons and Neutrons are in the nucleus and
add up to the atomic mass.
– Electrons are arranged in energy levels
•
•
•
•
1st energy level holds 2 electrons
2nd energy level holds 8
3rd energy level holds 8
Etc.
Lets Draw Oxygen!
• What is the atomic number of oxygen?
Do Now
• Answer the following
based on the picture
to the right…
–
–
–
–
Name of Element
# of Protons
# of Neutrons
# of Electrons
19
K
39.10
Objectives
• Draw an atom.
• Define isotopes.
• Identify different types of common
compounds.
• Compare and contrast the two types of
bonds.
Get with your Electron Partner!
1. Draw atoms for the following elements.
•
•
•
•
Neon
Boron
Lithium
Oxygen
What is wrong with this picture?
Carbon
-atomic symbol “C”
-atomic # 6
-atomic mass 12.02
Isotopes
• Isotopes contain the same # of protons as
the element, but a different number of
neutrons.
– Ex: Carbon-14
• Contains 6 protons (still carbon)
• Also contains 8 neutrons, instead of 6
**What else will be different other than the number of protons and
neutrons?**
Radioactive Isotopes
• Changing the # of neutrons changes the
stability of the atom, causes decay in the
nucleus or causes it to break apart.
– Ex: Carbon-14 is used in carbon-dating. We
can tell how old something is by how much
carbon is left.
What happens if there are different
number of ______ than a normal
atom?
•
•
•
Protons and Neutrons?
More protons than electrons?
More electrons than protons?
Neutral Atoms
• Atoms need to have the right number of
electrons around them (neutral)
• Ions- charged atom or groups of atoms
• Ions can lose or gain electrons to be
neutral
Na
+
Cl
How many electrons does each of
the following want to be “neutral”.
•
•
•
•
Oxygen
Carbon
Hydrogen
Nitrogen
Neutron Partners!
• List the number of protons, electrons, and
neutrons in each ion
– O– Na+
– N3-
• Are any of these atoms neutral?
Do Now
• Identify the element and then state if it is a
normal atom, an isotope, or an ion.
Objectives
• Identify compounds.
• Determine what information can be gotten
from a chemical formula.
• Compare and contrast ionic bonding vs.
covalent bonding.
• Explain what “Vanderwalls interactions”
are.
Compounds
• A pure substance formed when 2 or more
elements combine.
– Always formed using a specific ratio
• Ex: 2 molecules of Hydrogen + 1 molecule of
Oxygen will give us water (H2O)
– Chemically and physically different from the
elements that make them up.
– Must be broken down CHEMICALLY, not
physically
Chemical Formulas
• The number before the formula states how
many molecules
• Ex. 4 H2O = 4 water molecules
• The subscript number states how many of
that type of atom
• Ex. H2O = 2 hydrogen atoms
Let’s try some examples (neutron
partners)
For the following examples list the total
number of atoms for each element and
how many of each molecule.
1. C6H12O6
2. 3CH4
3. 5CO2
4. 3O3
5. 4HCl
Do Now
• Take out your homework from last night!
• Determine the # of molecules, # of atoms
for each element, and then the total
number of atoms for the following
compounds…
– 6H2O4
– 3CO2
– NaCl2
Objectives
• Understand how elements are held
together.
• Explain the components of a reaction.
How do compounds stay together?
•
Bonds!
– 2 most common types
1. Covalent- atoms share electrons
2. Ionic- atoms gain or lose electrons to bond
Covalent Bonding
Molecule: compound held together by covalent
bonds.
• Carbon (C) – form 4 bonds (another 4 e)
• Hydrogen (H) – form one bond (1 e)
• Nitrogen (N) – form 3 bonds (3 e)
• Oxygen (O) – form 2 bonds (2 e)
• H2O
O
H
H
Ionic Bonding
Ionic Bond
• Some atoms tend to donate or accept
electrons more easily than other atoms.
– Ex. Metals (D) and Non Metals (A)
Review!
• How many protons, neutrons, and
electrons are in O2-?
• An acid releases ____ ions in solution and
a base releases ____ ions in solution.
• Using the formula 3C6H12O6, how many
atoms of oxygen are present?
Quiz on the info up till now!
On the quiz…
• Parts of an atom
– Protons, neutrons, electrons
• Drawing- neutral atoms, ions, isotopes
• Compounds- what are they?
• Bonds
– Covalent and Ionic, what are they?
– How many bonds can elements make (according to
their valence electrons)
• Chemical formulas
– Determine molecule #, atom #, total atom #
Do Now
• What happens during a chemical reaction?
• What are the components of a chemical
reaction.
• Write an example of a chemical reaction
we have worked with in one of our labs.
Objectives
• To identify reactants and products in a
chemical reaction.
• To compare and contrast exothermic vs.
endothermic reactions.
• Explain how enzymes work
6.2 Chemical Reactions
• A chemical reaction -atoms or groups of
atoms are reorganized into different
substances.
• Chemical Reactions:
– Production of heat or light,
– Formation of a gas, liquid, or solid
Parts of a Reaction
Reaction- Molecules breaking or coming
together
Reactants- What goes in the reaction
Products- What comes out of the reaction
Ex: Na+ +
Cl- =
NaCl
Think – Pair - Share
 Glucose and oxygen react to form carbon
dioxide and water.
 Identify:
 Products
 Reactants
 Is this a chemical equation? Why?
+ ATP
(energy)
Energy in Reactions
• The activation energy - minimum amount
of energy needed for reactants to turn into
products
Types of Reactions
• Exothermic- released heat energy.
 The energy of the product is lower than the
energy of the reactants.
Types of Reactions
• Endothermic - absorbed heat energy.
– The energy of the products is higher than the
energy of the reactants.
Think – Pair - Share
• Determine whether or not the following are
Exothermic or Endothermic reactions:
• (Neutron Partner)
• 1. Combustion reactions of fuels
• 2. melting ice cubes
• 3. Nuclear Bomb
• 4. a candle flame
• 5. cooking an egg
Review
• What were the reactants in your liver lab?
• What were the products?
• What type of reaction was it? (endothermic
or exothermic)
• Give an example of an endothermic
reaction (not the example I gave)
What you should know about
enzymes!
-Specialized proteins that act as “catalyst”
(speeds up a reaction)
- Usually end in “ase”
-Not consumed in the reaction
What do they do?
How do they work?
• A substrate fits in the active site of an enzyme.
• This forms an enzyme substrate complex.
• They then break or form bonds.
Active
Site
Maltase
(Enzyme)
HOH
Maltose
(substrate)
HOH
Buffers
• What happens to enzymes in a strong pH?
(think about our lab!)
• Buffers are mixtures that can react with
acids or bases to keep the pH within a
particular range. (Remember
homeostasis? We want to keep our body
fluids at a pH of 6.5-7.5)
Chemistry in Biology
Do Now
Objectives
• List the 4 macromolecules of life.
• Identify the 3 different types of
carbohydrates.
• Explain the importance of carbs in the
body.
• Explain why low-carb diets can be harmful.
Review
• What is the purpose of an enzyme?
• What are the components of a solution?
Give an example.
• What are the 2 properties of water we
talked about?
• What are the 2 types of mixtures? Give an
example of each.
6.4 Macromolecules of Life
• Organic Chemistry - The element carbon
is a component of almost all biological
molecules. (Inorganic= no carbon)
Let’s Review
• Carbon has _____ electrons in its
outermost energy level.
• One carbon atom can form _____ covalent
bonds with other atoms.
Molecules
• Macromolecules – large molecules formed by joining smaller
organic molecules together.
• Polymers – molecules made from repeating units of
identical (or nearly identical) compounds
linked together by covalent bonds.
Carbohydrates
• Monosaccharide- ranging from three to
seven (simple sugar)
• Disaccharide - Two monosaccharides
joined together
• Polysaccharide- many monosaccharides
joined together
Carbohydrates
• Ratio of carbon : hydrogen : oxygen of
1:2:1
• (CH2O)n
Identify which molecules are
carbohydrates…
•
•
•
•
1) C6H12O6
2) CH3
3) C4H2O2
4) C24H36O24
•
•
•
•
Classify the following as mono, di,
or poly – saccaride
1. C6H12O6
2.
3. C12H24O12
4.
Article & Questions
• Get with your proton partner and join
another pair of proton partners! Read the
article and answer the questions.
Whatever you do not finish will be
homework.
Do Now
• Take out your carbohydrate article!
• What are carbs used for?
• Give an example of a simple carb and a
complex carb.
Objectives
• To explain how the body uses fats and
proteins.
• To compare and contrast saturated vs.
unsaturated fats.
• To understand the two types of
cholesterol.
Lets learn about FAT!!
• http://www.youtube.com/watch?v=2S1mQ
YO0g68
Lipids
• Made mostly of C and H
• Triglyceride
– Fat – solid at room temperature
– Oil – Liquid at room temperature
Saturated vs. Unsaturated
• Saturated Fats – Only Single bonds between the
carbons
– Solid at room temperature
(typically)
• Unsaturated Fats – Double bonds between the carbons
– Liquid at room temperature
(typically)
Click me
Types of Lipids
Saturated fats
Structural
differences
Unsaturated fats
all single bonds (one some double bonds (2
shared pair of
shared pairs of
electrons)
electrons)
Phase of matter solid fats
liquid fats
source
come from animals
come from vegetables
health
Less healthy
More healthy
Purpose
energy storage and insulation
So… people have a problem
with….
• Hydrogenated Oils
• Trans fats
• What are they?
• Why do they have a problem?
• TRANS FATS ARTICLE WITH
PARTNERS
Cholesterol
HDL
LDL
name
High density
lipoproteins
low density lipo
proteins
function
transport cholesterol
from the body to transport cholesterol
the liver for
from the liver to
breakdown and
the body
disposal
Health
good cholesterol
Purpose
strengthens cell membranes
bad cholesterol
Proteins
• Made of small carbon compounds called
amino acids
Central Carbon
Atoms that make up Amino Acids:
 carbon, nitrogen, oxygen, hydrogen, and
sometimes sulfur.
 Amino acids are connected together
through a PEPTIDE BOND.
Proteins in the Body
• structural – hair, collagen, muscle etc
• enzymes –
– speed up chemical reactions
Nucleic Acids
• complex macromolecules that store and
transmit genetic information.
• Nucleic acids are made of smaller
repeating subunits called nucleotides
• composed of carbon, nitrogen, oxygen,
phosphorus, and hydrogen atoms.
Think – Pair – Share
Let’s Try These
Think – Pair - Share
• Try THESE!