Matter and Energy

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Matter and Energy
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Matter

• Matter is anything that has mass and takes up
  space.
• All matter is composed of small particles called
  Atoms.
• Atoms are the basic building blocks that you can
  not see.

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Atoms and Their Structure

• Atoms are composed of even smaller parts
• Protons (p) positively charged
• Electrons (e-) negatively charged
• Neutrons (n) no charge.
• Protons and Neutrons are located in the nucleus
  of an atom.
• Electrons move rapidly around outside of the
  nucleus.

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Atoms and Their Structure
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Atoms and Their Structure

• In an uncombined atom, the number of protons
  equals the number of electrons giving the atom no
  charge.
• The region of space that electrons occupy while
  moving around the nucleus is known as the
  electron cloud.

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Electron Energy Levels

• Energy Levels are the different regions around
  the nucleus in which the e- travel.
• The first level holds a max of 2 e-.
• The 2nd and 3rd levels hold a max of eight.

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Elements

• Elements are substances that are composed of only
  one type of atom.
• Helium (H), Oxygen (O), Iron (Fe), etc.
• Elements differ in the the number of protons in
  their nucleus.
• All atoms of the same element have the same
  number of protons but the number of neutrons can
  be different. These are called Isotopes.

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Molecules

• Atoms combine in such a way that their outer
  energy level is filled.
• When the atoms share e-, their bond is covalent.
• Ex. Hydrogen gas H-H, Oxygen gas O-O
• A combination of two or more atoms combined by a
  covalent bond is called a molecule.

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Compounds

• A Compound is a substance composed of different
  kinds of atoms covalently bonded together.
• When atoms combine with one another, each new
  substance formed has a definite composition.

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Examples of Compounds

• Ammonia NH3
• Glucose C6H12O6
• Octane C8H18
• Table Salt NaCl
• Water H20
• Carbon Dioxide CO2

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Ions

• When atoms loose or gain e- they have a charge.
  The charged atom is called an ion.

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Ions

• Atoms that lose electrons become positive ions.
• Atoms that gain electrons become negative ions.
• The force of attraction between the two ions is
  called an ionic bond.
• Compounds formed this way are called ionic
  compounds.

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Ions

• In an ionic compound, the negative and positive
  charges must balance out so the net charge is
  zero.
• Na Cl ? Na Cl- ? NaCl
• Sodium Chlorine Sodium ion
  Chloride ion salt

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Symbols and Formulas

• A symbol is a one or two letter representation of
  an element.
• First letter is a capital.
• Second is lowercase.
• A group of symbols called a chemical formula
  shows the number and kind of each atom in a
  compound.
• Numbers in front of a formula apply to the entire
  formula.

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Symbols and Formulas

• H20?
• 2 Hydrogen and 1 Oxygen
• CO2?
• 1 Carbon and 2 Oxygen
• 5H2O?
• 10 Hydrogen and 5 Oxygen

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Solutions

• Solutions are homogeneous substances with
  different compositions.
• Homogeneous means the same throughout.

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Solutions

• Solutions are composed of two parts
• Solute gets dissolved.
• Solvent does the dissolving.
• Ex. When you put sugar in coffee, which
  substance is which?
• Coffee solvent, sugar - solute

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Solutions

• Ionic compounds undergo disassociation in
  solutions, meaning that the ions separate.

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Acids and Bases

• Sometimes water molecules disassociate to form 2
  ions.
• Hydroxide ion ? OH-
• Hydrogen ion ? H
• Solutions with an equal number of these ions are
  neutral.
• Solutions with more H are called Acids.
• Solutions with more OH- are called Bases.

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Acids and Bases

• A pH scale measures the relative concentration
  of ions in acids and bases.
• The scale measures from 0 14
• 7 is neutral
• lt 7 is an acid.
• gt 7 is a base.

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Changes in Matter
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Properties of Matter

• Properties are the characteristics scientists
  use to describe matter.
• Physical properties describes features of a
  substance.
• Chemical properties describe how matter will
  react with other matter.

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Properties of Matter

• A physical change is a changing of physical
  properties.
• A chemical change, involves the breaking of bonds
  and rearrangement of atoms or molecules.
• Ex. Iron, with O turns to rust.
• Ex. Copper with O turns blue.
• Ex. Wood burning in a fire.
• A chemical reaction the making of new
  substances with different properties the original
  components.

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Chemical Equations

• A Chemical Equation is a statement that describes
  a chemical reaction with symbols and formulas.
• Reactants substance that enter into the
  reaction.
• Products substances that are made in the
  reaction.

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Chemical Equations

• During a chemical reaction, mass can neither be
  created nor destroyed, this is called the Law of
  Conservation of Mass.
• Equations MUST be balanced to follow that law.
• The same number of atoms must be on each side.

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Biological Chemistry
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CARBONATE DEMO

• Need dry egg shell, sea shell, bit of chalk,
  antacid tablet, vinegar, test tubes, magnifying
  glass.
• How do you know a chemical change has happened?
• Which samples came from living things?
• CO2 is a major contributor to green house
  effects. What would happen if all CO2 producing
  organisms died off?

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Organic Compounds

• Organic compounds are ones that contain carbon.
• Carbon can form bonds with other atoms, including
  itself, to make chains.
• The bonds can be single, double or triple.

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Structural Formulas

• Structural Formulas show the arrangement of the
  atoms in space.
• The number of lines correspond to the type of
  bond. (sing, dbl, trp.)
• C-C is a single bond
• CC is a double bond
• CC is a triple bond

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Structural Formulas

• Compounds that have the same simple formula but
  different structural formulas are called isomers.

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Organic Compounds

• There are four main organic, C,H, and O
  containing compounds.
• They are
• Carbohydrates (sugars)
• Lipids (fats)
• Proteins
• Nucleic Acids (DNA/RNA)

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Carbohydrates

• Carbohydrates are composed of C,H, and O in a
  ratio of 2 Hydrogens to 1 Oxygen.
• They are the main source of energy.

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Carbohydrates

• There are three types of Carbs
• Monosaccharides (fructose fruit sugar)
• Disaccharides (Lactose milk sugar)
• Polysaccharides (starch hamburger bun)

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Carbohydrates

• Monosaccharides these are the building blocks
  of the other two types.
• They are the simplest sugars.
• They all share the same simple formula of
  C6H12O6.
• Glucose
• Galactose
• Fructose

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Carbohydrates

• Disaccharides are composed of two
  monosaccharides.
• They share the same simple formula of C12H24O12.
• Sucrose
• Maltose

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Carbohydrates

• Polysaccharides These are the complex
  carbohydrates composed of many monosaccharides.
• Starch
• Cellulose
• Glycogen

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Lipids

• Lipids are the energy storage molecules also
  compose of C, H, and O.
• Unlike carbs, the number of Hs are far greater
  than the number of Os.
• C57H110O6

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Lipids

• Lipids include fats, waxes and oils.
• All fats are made from two types of molecules.
• Fatty acids
• Glycerol
• Although fatty acids are different, they all
  contain the same group of atoms called a carboxyl
  group.
• ( -COOH)

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Lipids

• Fatty acids are represented in structural
  formulas as the letter R.
• Fatty acids in which the carbon atoms are linked
  by single covalent bonds are called saturated
  fats.
• Fatty acids that have atoms linked but one or
  more double covalent bonds are called unsaturated
  fats.

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Proteins

• Proteins are the largest group of organic
  materials.
• They are not usually used by organisms as energy
  sources.
• Some are used to build living material (muscle)
• Others carry out chemical reactions, fight
  diseases, or transport materials in and out of
  cells.

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Proteins

• Proteins also contain C, H, and O as well as
  Nitrogen (N) and Sulfur (S).
• They are made up of hundreds or thousands of
  simpler compounds called amino acids.

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Proteins

• There are 20 different amino acids.

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Amino Acids

• All contain a single carbon, connected to a
  carboxyl group (-COOH), a H atom, and an amino
  group (-NH2)

• When amino acids bond together they are known as
  peptides.

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Proteins

• Two peptides linked together are called
  dipeptides.
• Many peptides linked together are called
  polypeptides.
• Just like the letters of the alphabet can be
  arranged to form different words, the 20 amino
  acids can form an endless variety of polypeptides
  with different properties.

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Proteins

• A protein molecule may consist of more than one
  polypeptide.
• Proteins have a three dimensional shape that is
  crucial to their function.

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Nucleic Acids

• Nucleic Acids are the most complex of all
  biological molecules.
• They include DNA and RNA and contain the codes
  that control an organisms basic appearance and
  behavior.

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Nucleic Acids

• DNA (Deoxyribonucleic acid) and RNA (Ribonucleic
  acid) control the cells activities.
• DNA forms the genetic codes.
• RNA works to carry out the instructions of that
  code.

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Reactions of Biological Compounds

• Recall a monosaccharide was C6H12O6, yet a
  disaccharide is C12H22O11.
• Whats missing?
• Where did it go?
• What is it?

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Reactions of Biological Compounds

• There are two types of reactions among biological
  reactions
• Condensation reactions
• Hydrolosis

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Condensation Reactions

• When mixing two monosaccharides together, a
  molecule of water has to be removed in order to
  join the two sugars together.
• This process of removing a H2O is called a
  condensation reaction.

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Hydrolysis

• Large molecules are converted into smaller ones
  by a process that is the reverse of condensation.
  
• Hydrolysis is the addition of water.
• This process is important because large molecules
  must be broken down into simpler one before they
  can be used by cells.

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Energy

• Energy is the ability to do work.
• There are two types of energy
• Kinetic
• Potential
• Potential Energy is the energy of position, or
  stored energy.
• Kinetic Energy is the energy of motion.

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Energy

• Survival of organisms depends on chemical energy
  stored in energy rich molecules.
• When a reaction occurs, bonds break, energy is
  released, and stored energy (potential) is
  converted to usable energy (kinetic).
• The energy is used by cells to do biological work.

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Conservation of Energy

• When energy is transformed, it does not
  disappear.
• The Law of Conservation of Energy states that
  energy is neither created nor destroyed.

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Activation Energy

• The minimum amount of energy required to start a
  chemical reaction is called Activation Energy.
• A piece of wood wont just catch on fire, you
  need a match to provide enough heat to activate
  the reaction.
• A ball on the top of stairs needs a nudge to
  start rolling down the stairs.

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Enzymes

• The reactions of living organisms can not always
  depend on heat as a source of activation energy
• The heat required would be too high, damaging
  cells.
• Heat would be far to random of a source it
  could trigger too many reactions at once.

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Enzymes

• Cells contain enzymes, proteins that lower the
  activation energy required and allow reactions to
  occur at the normal temperature of cells.
• Enzymes are specific, guiding only one type of
  reaction.
• They are not permanently changed or used up so a
  given enzyme can be used over and over again.

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Enzymes

• Reactants in cellular reactions are called
  substrates.
• Most enzymes are named by adding ase to the name
  of the substrate in which the enzyme is
  controlling.
• E.x. the enzyme that helps convert Maltose to
  Glucose is called Matase.

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Induced Fit Model

• When an enzyme and a substrate join, the shape of
  the enzyme changes a little for a better fit the
  enzyme acts as a flexible key.
• For example.

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Example Reaction
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Example Reaction
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Example Reaction