Transcript Do Now

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
Introduction
• Matter – anything that takes up space and
has mass
• All matter is composed of atoms
• Atoms – smallest particle of matter that still
has chemical properties
• Element – one atom
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 numbertells 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
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.
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?
Get with your Electron Partner!
1. Draw atoms for the following elements.
•
•
•
Neon
Boron
Lithium
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
Radioactive Isotopes
• What is an isotope again?
• 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.
Radioactive Isotopes
• Ex. Radioactive Isotopes are used to help
doctors diagnose disease and locate certain
types of cancers
What happens if there are
different number of ______ than
a normal atom?
•
Neutrons?
•
More protons than electrons?
•
More electrons than protons?
“Happy” Atoms
• Atoms need to have the right number of
electrons around them (happy)
• Ions- an atom that has lost or gained one or
more electrons and carries a charge.
• Ions can lose or gain electrons to be neutral
Na
+
Cl
How many electrons does each of
the following want to be “happy”.
• 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 happy?
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
Do Now
• Take a few minutes to study for your
quiz.
• Pen or pencil is fine.
• I’ll be handing back tests, quizzes,
and other papers. Look through
them. If you have any questions,
please ask.
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
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
• Look at the compounds below: list
how many molecules, how many of
each atom, how many total atoms.
• 2(NH₄)₂Cr₂O₇
• Pb(NO₃)₂
• 4Al₂(CO₃)₃
•
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 Bond
• Some atoms tend to donate or accept electrons
more easily than other atoms.
– Ex. Metals (D) and Non Metals (A)
Van Der Waals Interactions
 When molecules come close together, the
attractive forces between slightly positive and
negative regions pull on the molecules and
hold them together.
 The strength of the attraction depends on the
size of the molecule, its shape, and its ability
to attract electrons.
Do Now
• What are the 2 main types of bonds?
• What happens with electrons in each type of bond?
• What is a compound?
• What bond are these compounds?
–
–
–
–
–
–
CH₄
Fe₂O₃
KNO₃
I₂
C₄
H₂O
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)
Balancing Equations
• The law of conservation of mass states
matter cannot be created or destroyed
• The number and types of atoms must be the
SAME on both sides of the equations
Ex. ___ H2 + ___O2  ___H2O
H= ____
O= ____
H= ____
O= ____
Neutron Partners!!
Balance the following equations:
1. ___H2 + O2 ---- > ___H2O
2. ___Zn + ___HCl --- > ___ZnCl2 + ____H2
3. ___SiO2 + ___HF--- > ___SiF4 + ___H2O
4. ___K + ___Br2 ----> ___KBr
5. ___Al + ___FeO ---- > ___Al2O3 + ___Fe
Do Now
• What happens during a chemical
reaction?
• What are the components of a chemical
reaction.
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 with
your Proton Partner
1. Combustion reactions of fuels
2. melting ice cubes
3. Nuclear Bomb
4. a candle flame
5. cooking an egg
DEMO
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.
• https://www.youtube.com/watch?v=r1ryDV
gx0zw
Enzymes Continued
• Anything that changes the shape of the
active site stops the enzyme from
working.
• Ways to denature an enzyme:
– pH
– Temperature
Quick!
• Label the parts of the reaction:
Do Now
• What are acid and bases?
• What foods do you know of are
acidic?
• What foods are basic?
• Why is it important to know the pH of
a substance?
Objectives
• SWBAT:
– Identify substances as an acid, base, or
neutral
– Draw a pH scale and place substances
according to it’s pH value
– Explain what happens during a
neutralization reaction
– Explain and describe the difference
between various mixtures.
6.3 Solutions
• Solution = A Liquid mixture in which the solute
dissolved in a solvent.
• Ex. Hot Chocolate (Water and Coco Powder)
• Solute- Substance that is dissolved in solvent.
– Ex. Coco Powder
• Solvent- Substance that the solute dissolved in.
– Ex. Water
• How do things dissolve?
– Polar Covalent Bond: Slight Positive and negative
charges
• Ex. H2O
– Non-Polar: Do not dissolve in water
• Ex. Lipids and Fats
Mixtures
What is the difference?
Mixtures
• Homogeneous – Has a uniform
composition throughout (a.k.a solutions)
– Ex: Air
• Heterogenous- components remain
distinct.
– Ex: Fruit Loops
Acids and Bases
• pH- Measure of concentration of hydrogen ions in a solution
• Acids- Release Hydrogen Ions (H+). Tastes Sour.
– Ex: HCl
• Bases- Release Hydroxide Ions (OH-). Taste Bitter. (a.k.a
Alkaline)
– Ex: NaOH
• Neutral – Number of H+ = Number of OH+
pH Paper: Indicates the number of H+ ions by means of a number
value.
• Litmus Paper:
– Red:
• Stays red in a Acid
• Turns Blue in a Base
– Blue:
• Stays Blue in Base
• Turns Red in Acid
Buffers
• Buffers are mixtures that can react with
acids or bases to keep the pH within a
particular range.
– (We want to keep our body fluids at a pH
of 6.5-7.5. Why do you think that is?)
Neutralization Reactions
• When an acid and a base react to
form water and a salt. It’s
“Neutralized”
NaOH + HCl ---- H2O + NaCl
- “Salt” positive/negative ion.
Na+
OH-
H+
Cl-
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.
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.
• Are also called Polymers – molecules made from repeating units of
identical (or nearly identical)
compounds linked together by covalent
bonds.
Carbohydrates
• Broken down into sources of energy
– Ex. Glucose!
• Ratio of carbon : hydrogen : oxygen of 1:2:1
• (CH2O)n
• N= # of CH2 in a chain
*Where there is a corner
there is a carbon!*
Carbohydrates
Simple Carbs:
• Monosaccharide- Values of n ranging from three to
seven (simple sugar)
Ex. Glucose (n=6)
• Disaccharide - Two monosaccharides joined together
Ex. Lactose
Complex Carbs:
• Polysaccharide- many monosaccharides joined
together
Ex. Glycogen (energy storage in muscle or liver)
Disaccharide
Monosaccharide
Polysaccharide
Lipids
• Fats, Oils, and Waxes
• Made mostly of C and H
• Used for energy storage and insulation
• 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)
– More unhealthy
• Unsaturated Fats – Double bonds between the carbons
– Liquid at room temperature (typically)
– More Healthy
*But what is the worst type of fat?!
Click me
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
Do Now
• What are carbs broken down into?
• What does this provide?
• If this compound isn’t used, what is
it stored as?
• Where is it stored?
• What are the purpose of lipids?
• Difference between Unsaturated
and Saturated fats?
• What are HDL and LDL?
Proteins
• Made of small carbon compounds called amino acids
• There are 20 types of amino acids.
• We produce 10 of the 20!
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
*Involved in nearly every function of your body!
Nucleic Acids
• Store and transmit genetic information.
• Nucleic acids are made of smaller
repeating subunits called nucleotides
• composed of carbon, nitrogen, oxygen,
phosphorus, and hydrogen atoms.
Three types of Nucleic Acids
• DNA
• RNA
• ATP
Do Now
Please hand in your Enzyme Web Quests
into the bin!
Then Answer:
– What monomers make up proteins?
• What part of their structure make each one
different?
– Why are proteins so important?
– What is the purpose of nucleic acids?
• What are the three types?
Yay Lab!!
Do Now
• Please grab 5 colored pencils
• Then answer:
– What kind of information can be found
on a nutritional label on food products?
Food Labels
• Ingredients are listed in descending
order.
– First 2-3 listed, are the main ingredients.
– 1st ingredient makes up the largest
portion.
• Manufacturers are required to list the
amount of saturated and trans fats.
– Voluntarily can put the amount of
unsaturated fats.
40 Calories is LOW
100 Calories is MODERATE
400+ Calories is HIGH
Finding Total Calories
• 1g Fat = 9 cal
• 1g Carbs= 4 cal
• 1g Protein= 4 cal
– *FDA allows about 20% discrepancy on
food labels.
Calories from Fat
• 1g Fat = 9 cal
– *Calories from fat are rounded to the
nearest 10 calorie increment.
• % of calories from fat:
Calorie from fat
Total Calorie
100%
% Daily Value
Amount Given
Recommended Amount
100%
– *No % DV for protein because it is not a
concern.
– *No % DV for Trans fats, but suggested
amount is less than 1%
– *Have yet to come up with a % DV for
sugar.
Biological Molecule Video!!
• https://www.youtube.com/watch?v=H
8WJ2KENlK0