Do Now!! ?

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Do Now!! ?

• What is an atom?
• Why do we have a periodic table?
• What information can we find in a periodic table?

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Chapter 6

• Biochemistry

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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.

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Atoms

• Smallest particle of matter that still has
  chemical properties
• Matter anything that takes up space and has mass
• Contain 3 parts
• Protons positively charged, contain mass of 1
• Location
• Neutrons no charge, contain mass of 1
• Location
• Electrons Outside nucleus, negatively charged,
  insignificant mass
• Location

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Atoms make up Elements

• A pure substance that cant 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.

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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.
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Periodic Table Information

• Atomic number- tells us the of protons (as well
  as electrons)
• Symbol- unique for each element.
• Atomic Mass- of protons neutrons

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• C

12.02
How would you determine the number of neutrons
in an atom??
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So

• What makes atoms different?
• How is carbon different from oxygen?
• Different numbers of protons!!

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Think-Pair-Share

• List the number of protons, neutrons, and
  electrons for the following
• Mg
• Ca
• Fe
• Cl

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Do Now!! ? Complete the chart
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Do Now!! ?
Complete the missing information and include the
number of protons, neutrons, and electrons.
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Do Now!! ?

• List the number of protons, neutrons and
  electrons for the following
• H
• P
• K
• Ni
• Ar

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Objectives

• To practice drawing different atoms.
• To review parts of the atom by completing a
  worksheet activity.

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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

Valence electrons electrons on outermost shell
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Lets Draw Oxygen!

• How many protons, neutrons and electrons does an
  atom of oxygen have?
• How many valence electrons are there?

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Practice

• Lets draw
• 1. He
• 2. Na
• 3. S
• 4. C
• 5. Cl

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Do Now!! ?
Please complete the table below!
Acid Base
s on pH scale
Release_____ in water
Litmus paper is _____ in its presence
Examples
What is a neutralization reaction? What are the
reactants? Products?
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Do Now!! ?

• Lets draw
• 1. Ar
• 2. Al
• 3. Na
• 4. Ne
• 5. Mg

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Objectives

• To discuss isotopes and relate their research to
  the medical field
• To determine the number of protons, neutrons and
  electrons of ions
• To identify types of bonds

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What is wrong with this picture?
Carbon -atomic symbol C -atomic
6 -atomic mass 12.02
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Isotopes

• Isotopes contain the same of protons and
  electrons as the element, but a different number
  of neutrons.
• Ex Carbon-14
• Contains 6 protons (still carbon)
• Also contains 8 neutrons, instead of 6

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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.

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Radioactive Isotopes

• Ex Radioactive isotopes are used to help doctors
  diagnose disease and locate certain types of
  cancer.

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What happens if there are different number of
______ than a normal atom?

• Neutrons?
• More protons than electrons?
• More electrons than protons?

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Happy Atoms

• Atoms need to have the right number of electrons
  around them (happy)
• Ions- charged atom or groups of atoms
• Ions can lose or gain electrons
• Lose form positive ions
• Gain form negative ions

Na
Cl
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How many electrons does each of the following
want to be happy?

• Oxygen
• Carbon
• Hydrogen
• Nitrogen

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Lets Practice!

• List the number of protons, neutrons and
  electrons in each ion
• O-
• Na
• N3-
• Cl-
• F
• Are any of these atoms happy?

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Do Now!! ?

• Think-Pair-Share
• - If an ion is positively charged, does it gain
  or lose electrons?
• - Negatively charged?
• - How many electrons does O3- have?

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Objectives

• Identify protons, neutrons and electrons in ions.
• Identify compounds.
• Determine what information can be received from a
  chemical formula.

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Do Now!! ?

• Identify the element and then state if it is a
  normal atom, an isotope, or an ion.

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Objectives

• Practice identifying components of ions by
  completing a worksheet
• Identify compounds.
• Determine what information can be received from a
  chemical formula.
• Compare and contrast ionic bonding vs. covalent
  bonding.
• Explain what Vanderwalls interactions are.

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Molecules and Compounds

• Molecule Forms when two or more atoms form
  chemical bonds
• Compound A pure substance formed when 2 or more
  different elements combine
• Always formed using a specific ratio
• Ex fuel in cars (hydrocarbons)

• Chemically and physically different from the
  elements that make them up
• Must be broken down CHEMICALLY, not physically

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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, 1 oxygen atom

O
H
H
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Lets try some examples

• For the following examples list the total number
  of atoms for each element and how many of each
  molecule.
• C6H12O6
• 3CH4
• 5CO2
• 3O3
• 4HCl

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Do Now!! ?

• For the following examples list the total number
  of atoms for each element and how many of each
  molecule.
• 2H2SO4
• 4HNO3
• 5MgCl2
• NaOH
• 4C6H8O7

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Objectives

• Compare and contrast ionic bonding vs. covalent
  bonding.
• Explain what Vanderwalls interactions are.
• Explain what a chemical reaction is.
• Identify reactants and products in a reaction.
• Balance an equation.

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How do compounds stay together?

• Bonds!
• 2 most common types
• Covalent- atoms share electrons
• Ionic- atoms gain or lose electrons to bond

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Covalent Bonding

• 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)
• Ex H2O

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Ionic Bond

• Some atoms tend to donate or accept electrons
  more easily than other atoms.
• Ex. Metals (D) and Non Metals (A)

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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.

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Do Now!! ?

• Please take out your ion worksheet!

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Objectives

• To define chemical reaction
• To differentiate between endothermic and
  exothermic reactions
• To illustrate types of reactions in a lab
  activity

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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

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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

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Energy in Reactions

• The activation energy - minimum amount of energy
  needed for reactants to turn into products

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Types of Reactions

• Exothermic- releases heat energy
• The energy of the product is LOWER than the
  energy of the reactants.

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Types of Reactions (cont.)

• Endothermic - absorbs heat energy
• The energy of the products is HIGHER than the
  energy of the reactants.

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Demo time!! ?
Endothermic or Exothermic??
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Do Now!! ?

• Glucose and oxygen react to form carbon dioxide
  and water.
• Identify
• Products
• Reactants
• Is this a balanced equation?

ATP (energy)
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Objectives

• To balance equations.
• To identify types of reactions.
• To explain how an enzyme works.
• To determine the difference between a solute and
  a solvent.

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Do Now!! ?

• Determine whether or not the following are
  Exothermic or Endothermic reactions
• 1. Combustion reactions of fuels
• 2. melting ice cubes
• 3. Nuclear Bomb
• 4. a candle flame
• 5. cooking an egg
• 6. Photosynthesis

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Objectives

• To identify types of reactions.
• To explain how an enzyme works.
• To determine the difference between a solute and
  a solvent.
• To list the properties of water.

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What you should know about enzymes!!
Type of Enzyme Substrate Product
Lipase Protein Amino Acid
Protease Fats Fatty Acid
Carbohydrase Carbohydrates Glucose
Lactase Lactose Glucose
Amylase Carbohydrates Glucose
Pepsin Protein Amino Acid

• Specialized proteins that act as catalysts
• Aka they speed up reactions!
• Usually end in ase
• NOT consumed in the reaction
• They are reused!!

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What do they do?

• Lower the activation energy needed!!

• Activation energy barrier is like a wall between
  two parts of a pond.
• If an enzyme lowers the wall, more frogs have
  enough energy to reach the other side.

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How do they work?

• A substrate fits in the active site of an enzyme
• Specific to one kind of substrate
• Lock and key
• This forms an enzyme substrate complex.
• Will then break or form bonds.

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Denaturing Enzymes

• Enzymes have specific optimal conditions
• Temperature
• pH
• If those conditions change, enzyme is permanently
  damaged
• Denatured!
• Cannot do its job

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Do Now!! ?

• What is the purpose of an enzyme?
• What was the enzyme used in your liver lab?
• What is a substrate?
• What was the substrate in your liver lab??

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Objectives

• To identify types of reactions.
• To explain how an enzyme works.
• To determine the difference between a solute and
  a solvent.
• To list the properties of water.

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How do they work?

• http//www.youtube.com/watch?vXTUm-75-PL4

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6.3 Solutions

• Solution Mixture of a solute dissolved in a
  solvent (ex iced tea!)
• How do things dissolve?
• Polar Covalent Bond Slight positive and negative
  charges
• Ex. H2O (universal solvent!) and NaCl (salt)
• Non-polar Do not dissolve in water
• Ex. Lipids and Fats

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Mixtures

• Solute- substance that is dissolved
• Solvent- substance that the solute dissolved in.
• Ex. Hot chocolate (Water and Coco Powder)

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Mixtures

• Homogeneous

• Heterogeneous

What is the difference?
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Mixtures

• Homogeneous- has a uniform composition throughout
  (a.k.a solutions).
• Heterogeneous- components remain distinct.

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Buffers

• What happens to enzymes in a strong pH?
• Buffers are mixtures that can react with acids or
  bases to keep the pH within a particular range
• Ex Keep body fluids at a pH of 6.5-7.5
• Ex Hemoglobin

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6.4 Macromolecules of Life

• Organic Chemistry The study of organic
  compounds
• The element carbon is a component of almost all
  biological molecules (organic)
• Inorganic no carbon

C arbon H ydrogen N itrogen O xygen P hosphorus S
ulfur
Six most abundant elements of life!!
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Molecules

• Macromolecules -
• large molecules formed by joining smaller organic
  molecules together.
• Are also called Polymers
• made from repeating units of identical (or nearly
  identical) compounds (monomers)

Polymer
monomer
monomer
monomer
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Do Now!! ?

• Determine whether the following substances are
  heterogeneous or homogenous
• Chicken noodle soup
• Black coffee
• Jello
• Jello fruit salad
• Cole Slaw
• Whole milk
• Chipotle Burritos

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Do Now!! ?

• Label the parts of the reaction below

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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.

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Carbohydrates

• Sources of energy
• Ratio of carbon hydrogen oxygen of 121
• (CH2O)n
• n of CH2O in a chain
• Ex glucose (C6H12O6)

Glucose



Where theres a corner theres a carbon!


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Identify the Carbohydrates!

• 1) C6H12O6
• 2) CH3
• 3) C4H2O2
• 4) C24H48O24

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Carbohydrates (cont.)

• Monosaccharide- values of n ranging from three to
  seven (simple sugar)
• ex glucose (n 6)
• Disaccharide - Two monosaccharides joined
  together
• ex lactose
• Polysaccharide- many monosaccharides joined
  together
• ex glycogen (energy storage in muscle)

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Disaccharide (lactose)
Monosaccharide (glucose)
Polysaccharide (glycogen)
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Do Now!! ? (P. 5)

• What are the four macromolecules?
• What are some differences between simple and
  complex carbohydrates?
• Which of the following are carbohydrates?
• CH2O
• C6HO6
• C12H24O12
• C6H12O5

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Lipids

• Fats, oils and waxes
• Made mostly of C and H
• Triglycerides
• Used for energy storage and insulation
• Fat solid at room temperature
• Oil Liquid at room temperature

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Lipids (cont.)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

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Proteins

• Made of small carbon compounds called amino acids

• Atoms contain carbon, nitrogen, oxygen, hydrogen,
  and sometimes sulfur.

Central Carbon
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Proteins in the Body

• Involved in nearly every function of your body.
• structural -
• hair, collagen, muscle, skin etc. made of
  proteins
• enzymes
• speed up chemical reactions

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Nucleic Acids

• Store and transmit genetic information.
• Made of smaller repeating subunits called
  nucleotides
• Composed of carbon, nitrogen, oxygen, phosphorus,
  and hydrogen atoms.

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Think Pair ShareLets Try These
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Think Pair - Share

• Try THESE!

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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

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Do Now Please complete the table! ?
Chemical/ Symbol Atomic Number Atomic Mass Bonds Formed
Carbon C 6 12 4
Hydrogen H 1 1 1
Nitrogen N 7 14 3
Oxygen O 8 16 2
Phosphorus - P 15 31 5
Sulfur - S 16 32 2
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Lets Review

• Carbon has _____ electrons in its outermost
  energy level.
• One carbon atom can form _____ covalent bonds
  with other atoms.
• Bonds enable carbon atoms to bond to each other
  variety of important organic compounds.

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Do Now!! ?

• What are the four macromolecules of life?
• What are some examples of saturated and
  unsaturated fats?
• What is a trans fat?

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Objectives

• To explain how the body uses fats and proteins.
• To compare and contrast saturated vs. unsaturated
  fats.
• To discuss proteins and nucleic acids.

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Acids and Bases

• Acids- Releases hydrogen ions.
• Bases- Releases hydroxide ions.
• pH- measure of concentration of hydrogen ions in
  a solution.