chapter 6 the chemistry of life. atoms and their interactions
TRANSCRIPT
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Chapter 6The Chemistry of Life
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Atoms and their interactions
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Elements• An element is a substance that can’t be
broken down into simpler chemical substances – 90 elements occur naturally– 25 are essential to living organisms (table 6.1)– 4 elements make up 96% of the mass of a
human• Carbon (C) Hydrogen (H) Nitrogen (N) Oxygen (O)
• Trace elements are present in living things in small amounts and play a vital role in maintaining healthy cells in organisms– Plants absorb them through their roots– Animals get them through food they eat
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Atoms: The building blocks of Elements
• An atom is the smallest particle of an element that has the characteristics of that element
• An atom has a specific structure– Nucleus– Electron energy levels (orbitals)
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Protons
Neutrons
Electron Energy Levels (orbitals)
Nucleus
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When electrons fill in energy levels they fill in a specific order.
First orbital = 2 electronsSecond orbital = 8 electronsThird orbital = 18 electronsFourth orbital = 32 electrons
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Isotopes of an Element
• An atom of the same element that has a different number of neutrons but same amount of protons and electrons
– Carbon-12 (12C)– Carbon-14 (14C)
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Compounds
• – a substance that is composed of atoms of two or more different elements that are chemically combined.– H2O
– H2SO4
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Molecule – a group of atoms held together by covalent bonds and having no overall charge
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Bonding
• Covalent – chemical bond formed when two atoms combine by sharing electrons
• Can form between atoms of the same element or atoms of different elements
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• Ionic – chemical bond formed by the attractive forces between two ions of opposite charge
• Compounds formed by ionic bonds are ionic compounds or salts, like NaCl or table salt.
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Non-Polar Covalent Bonds
• Electrons are shared equally– A covalent bond between two
atoms of the same element is always non-polar
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Polar Covalent Bonds
• Electrons are not shared equally by the two atoms
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Polar Covalent Molecule• Formed from polar covalent bonds.• Uneven distribution of charge• Each molecule has a positive end
and a negative end
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Chemical Reactions
• Metabolism – all the chemical reactions that occur within an organism
• Chemical Equations – represent chemical reactions – Use symbols and formulas to
represent each element
NaOH + HCl → NaCl + H2O
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Mixtures
• – a combination of substances in which individual components maintain their properties
– Sand & sugar mixed together
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Acid • – substance that forms
Hydrogen ions (H+) in water– pH below 7– HCl when dissolved in water
forms H+ ions and Cl- ions
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Base
• – substance that forms hydroxide ions (OH-) in water– pH above 7– NaOH when dissolved in
water forms Na+ ions and OH- ions
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Solutions
• – a mixture in which one or more substances (solute) are distributed evenly in another substance (solvent)
– Sugar in water
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• Solute – substance to be dissolved
• Solvent – substance doing the dissolving
Sugar & WaterSugar = Solute Water =
Solvent
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6.2 Water and Diffusion
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• Water is a polar molecule; therefore, water molecules bond
• The bond formed by negative and positive ends of polar molecules are called Hydrogen Bonds
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• Water – resists change in temperature– requires more heat to increase its
temperature– helps maintain a steady
environment when conditions fluctuate
– important to cellular functions; it helps cells maintain an optimum environment
– Expands as it freezes– Helps form soil by freezing in
cracks of rocks and breaking them apart
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Diffusion
• Diffusion – movement of particles from where there is a high concentration to where there is a low concentration
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• 3 things affect rate of diffusion– Concentration
•More concentrated the substances, the more rapidly diffusion occurs
– Temperature•Higher temperature = faster
diffusion (molecules moving faster)
– Pressure•Higher pressure = faster
diffusion
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• Dynamic Equilibrium – continuous movement but no overall concentration change
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6.3 Life Substances
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The Role of Carbon in Organisms
• Carbon– Forms strong, stable,
chemical bonds– 4 bonding sites– Bonds 4 times for stability– Forms chains of almost
unlimited length– They can form closed chains,
rings, or branch wildly
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• Isomer – compounds that have the same molecular formula but different 3-D structure
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Molecular Chains
• Polymer – a large molecule formed when many smaller molecules bond together– Formed by condensation– Broken apart by hydrolysis
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Carbohydrates
• Organic compound composed of carbon, hydrogen, and oxygen– Simple carbs – simple sugar
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Structure of Carbohydrates• Monosaccharide – simplest carb• Disaccharide – two
monosaccharides bonded together– Bonding of glucose and
fructose together makes sucrose (table sugar)
• Polysaccharide – largest carbohydrate molecules– Composed of many
monosaccharide subunits•Starch•cellulose
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Structure of Lipids• Large proportion of C-H
bonds • Commonly called fats and
oils• Insoluble in water • Cells use for energy
storage, insulation, and protective coatings
• Major components of membranes
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Structure of proteins• Large polymer composed of
amino acids– There are 20 common amino
acids that make thousands of proteins
– Amino acids bond to one another via a peptide bond
– The number and order of amino acids in protein chains determine what protein it is
• Proteins come in large variety of shapes and sizes
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Structure of Nucleic Acids• A complex macromolecule
that stores cellular information; it contains instructions used to form all of an organism’s enzymes and structural proteins– DNA– RNA
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THE END