Chemistry of Life Chapter 2.1. C 6 H 12 O 6 + 6O 2 CO 2 + H 2 O What elements are represented? ...
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Transcript of Chemistry of Life Chapter 2.1. C 6 H 12 O 6 + 6O 2 CO 2 + H 2 O What elements are represented? ...
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Chemistry of Life
Chapter 2.1
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C6H12O6 + 6O2 CO2 + H2O
What elements are represented?
What compounds are represented?
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How many atoms of each element are represented?
Is it balanced?Which scientific law do balanced chemical equations enforce?
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Atoms – The basic unit of matter. Composed of:Protons – positively charged particles in the nucleus of the atom
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Neutrons – particles with mass that have no charge; found in the nucleus of the atom
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Electrons – negatively charged particles moving around the nucleus in orbits.
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Atoms with equal numbers of protons and electrons are “neutral”
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Atoms with uneven numbers of electrons and protons = ion
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Atoms with more protons than electrons = cation (positive charge)
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Atoms with more electrons than protons = anion (negative charge)
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Elements – What is an Element?
One or more atoms Cannot be broken down or split
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Represented by a one or two letter symbol
ex. Na (sodium)
C (carbon)
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Atomic number = number of protons of an element.
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Atomic weight = number of protons plus number of neutrons. Ex: Carbon has 6 protons and 6 neutrons; atomic weight is 12
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Look at Carbon – CWhat is its atomic mass?
Can we tell how many electrons it has?
How? (hint – look at its atomic number)
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Isotope – Atoms of the same element that have different numbers of neutrons. Ex: Carbon can have 6, 7, or 8 neutrons
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Radioactive isotope – isotopes with unstable nuclei. Give off radiation
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Valence electronsThose electrons that orbit the outer energy level of an atom.
1st energy 2 electrons
2nd energy level 8 electrons
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Filled make the element more stable
Unfilled energy levels make the element more reactive with other elements.
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Compound – substance formed by the chemical combination of 2 or more elements. Ex: H2O, NaCl, HCl.
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Compound usually has different properties than the elements it is composed of
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Ex: H2O is a liquid composed of gaseous hydrogen and gaseous oxygen.
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Chemical bonds – forces that hold elements of a compound together.
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Forces are created by the interaction of each of the element’s valence electrons
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Ionic Bond – formed when one or more electrons are transferred from one atom to another.
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Ex: Sodium (Na) donates one electron to Chlorine (Cl) to form an ionic bond and make sodium chloride (NaCl – table salt)
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Covalent Bond – formed when one or more electrons are shared between elements. This type of bond between elements creates a molecule. Ex: H2O
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OH H
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Properties of Water
A common molecule with unique characteristics:
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Polar – due to the way the hydrogen atoms are arranged around the oxygen atom, water molecules have a (+) end and a (-) end = polar.
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OH H
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This electrical orientation causes water to be attracted to other charged elements and form hydration spheres around them. This keeps the elements from combining with other charged elements.
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Ex: salt placed in water dissolves. In other words, the sodium separates from chlorine & water molecules keep them apart. Water helps keep things dissolved = universal solvent
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Has a high heat capacity and heat of vaporization – water absorbs, transports, and releases a great deal of heat without changing its state (ice to water to vapor).
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That’s why, on a hot day, you just perspire and not evaporate. The water in your body stays liquid (and not turn into a vapor) while it is carrying the heat to the surface of your skin.
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Cohesive - sticks to itself; ex: beading water
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Adhesive - sticks to other things
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Highly reactive – virtually no chemical reactions occur in living systems without the presence of water
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It’s the major component of body lubricants (mucus), protective cushions (amniotic fluid and cerebrospinal fluid), and transport mediums (blood)
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SaltsIn living systems, salts are
compounds that dissolve in water and become electrolytes. Electrolytes conduct electricity in the body. Ex: Na, Ca, K, Cl are the major electrolytes. Gatorade has a concentration of these in it.
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ACIDSCompounds that give off
hydrogen ions (H+)in solution. Acids read below 7 on the pH scale. The more H+ given off, the lower the number on the pH scale.
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BasesCompounds that give
off hydroxide ions (OH-) in solution. Bases read above 7 on the pH scale. The more OH- given off, the higher the pH.
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BiochemistryThe Macromolecules of
Life
Chapter 2.3
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Organic ChemistryThe study of all compounds that
have bonds between carbon
atoms.
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Importance of Carbon
Carbon has 4 valence electrons
It tends to form covalent bonds with other carbon atoms
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In doing so, In doing so, carbon can carbon can form a variety form a variety of shapes…of shapes…
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…chains…
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…rings…
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…branches…
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…or combinations of chains, rings, and branches.
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Macromolecules
Carbon is able to form large and complex molecules called “macromolecules”
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Macromolecules are
made by “polymerization”
in which small compounds
(“monomers”) are put
together to make larger
compounds (called
“polymers”)
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There are 4 types of organic macro-molecules (organic polymers):
CarbohydratesLipidsProteinsNucleic Acids
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Carbohydrates “sugars”
Made of C, H, O in a 1:2:1 ratio; Ex: C6H12O6
Monomer is monosaccharide
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ExamplesGlucose-quick energyStarch-plant storageGlycogen- animal storageCellulose-structure in
plantsChitin-exoskeleton
crayfish
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Used as the main source of fuel and/or structural purposes
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Found in breads, Found in breads, cereals, pasta, potatoes, cereals, pasta, potatoes, corncorn
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Lipids: “fats”Made of mostly of C and H
Monomer is glycerol attached to fatty acids
OR
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Used to store energy, make cell membranes, waterproof coverings, chemical messengers
Examples: saturated fats, unsaturated fats, polyunsaturated fats, oils, waxes, cholesterol, steroids
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Contained in dairy Contained in dairy products, meats, some products, meats, some vegetablesvegetables
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Nucleic AcidsMade of C, H, O, N, PMonomers are nucleotides
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Used to store and transmit genetic information
Examples include DNA and RNA
Found in anything that contains cells
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ProteinsContains C, H, O, N, S, P
Monomers are amino acids
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Used to regulate chemical reactions and cell processes, form body structures, transport materials, or fight disease
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Examples include enzymes, antibodies, muscle tissue
Contained in meats, legumes, dairy products
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Enzymes – special types of proteins
Enzymes are proteins capable of increasing the rate of a reaction without being consumed in the process
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Types of reactions enzymes are involved in include:DigestionSynthesis of moleculesStorage and release of energy
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Enzymes have the ability to carry out reactions at lower temperatures that would normally require extremely high temperatures
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Activation Energy – the energy required to attach enzymes to substrates and cause a change
Substrate – the molecule undergoing a change; also called the reactant.
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Activation site – place on the enzyme where a specific substrate attaches
Reactant – in a chemical equation, it is on the left side; what is added together to form products
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Product – the end result of the enzyme-substrate reaction; found on the right side of a chemical equation
Optimum – the best conditions for a reaction to occur. In your body, optimum conditions are a pH of 7 and a temperature of 37oC
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Denature – to permanently change the shape of an enzyme due to pH or temperature extremes; can prevent the enzyme from functioning properly.
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Coenzyme – needs to be present in some enzymes to aid in the reaction. If it is missing the enzyme may not work; vitamins act as coenzymes.
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Inhibitors – things that prevent enzymes from working properlyCompetitive inhibitors – compete with the substrate for binding sites on the enzyme; slows down the reaction; ex: ethanol and isopropanol
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Noncompetitive inhibitors – irreversible binding to enzymes; stop the reaction permanently Ex: some heavy metals.