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The Chemistry of Life
E. coli vs. E. coli
Atoms
• Submicroscopic units of matter
• Smallest unit of all physical material
Structure of Atoms
• Proton– In nucleus– Positive charge
• Neutron– In nucleus– No charge
• Electron– Surround nucleus– Negative charge
Atomic Mass
• Combined mass of protons & neutrons
• Electron mass is too small to matter
Atomic Mass = 14
Elements
• Made of a single kind of atom
• Type determined by its number of protons
7 Protons = Nitrogen
Atoms & Isotopes• Atoms
– protons = electrons– Electrically neutral
• Isotopes– Same number of protons,
different number of neutrons– Differ in atomic mass
Electrons• Could be found anywhere around nucleus
• Most likely location is its shell
Electrons• Shells correspond to energy levels
• Energy increases away from the nucleus
• Number of protons also increases energy
Molecules
• Combinations of atoms
– Same elements or different elements
– Methods atoms combine
• Share electrons
• Attract via opposing electron charges
Compounds
• Molecules with different atoms
• Methods of combining– Sharing electrons– Atoms lose & gain electrons
(Ions)
Chemical Formula
• Method to describe molecule composition
H2O = Water
2 Parts Hydrogen
1Part Oxygen
Factors that Influence Interaction Among Atoms
1. Tendency of electrons to occur in pairs
2. Tendency of atoms to balance charges
3. Tendency of outer shell to be full
(Octet Rule)
Octet Rule
• Refers to 8 as stable number of electrons in outer shell
• First energy level is exception (2 electrons)
• Atoms with unfilled shells tend to interact
Noble Gases
• Equal numbers of protons & electrons
• Outer energy shell full
• Do not readily react with other elements
Helium Neon
Argon Krypton
Xenon Radon
Chemical Bonds Form Molecules• Ways atoms can satisfy octet rule
– Gain electrons from other atoms– Lose electrons to other atoms– Share electrons with other atoms
Covalent Bonds
• Atoms share outer electrons
Ionic Bonds• One atom donates electron to other atom
Oxidation
• Process where addition of Oxygen, lose Hydrogen or lose electron
from element or compound
• Oxygen
– Strong electron receptor
– Most frequent receptor in biological systems
Reduction
• Process where an atom gains an electron
• Changes charge by -1
• Oxidation and reduction occur together
Called redox reactions
Diatomic Molecules
• Paired atoms that form a molecule
• Share electrons with covalent bond
H2 = Hydrogen Gas
O2 = Oxygen Gas
Cl2 = Chlorine Gas
N2 = Nitrogen Gas
Covalent Bond Strength
• Can be weak or strong
• Single bond (example Hydrogen gas)
• Double bond (example Oxygen gas)
• Triple bond (example Nitrogen gas)
Bonding in Carbon
• Can form four covalent bonds
• Can bond to more than one atom
• Basis for many biological molecules
Energy and Covalent Bonds
• Bonds act as storage place for energy
• Breaking bonds releases energy
• Allows organisms to store & use energy
Water
• Most abundant molecule in your body
• Vital to life
Frog Eggs in Water Environment
Chemical Properties of Water
• Hydrogen’s electrons usually near Oxygen
• Molecule has polarity (polar molecule)
Polarity of Water
• Allows it to attract other molecules
• Forms hydrogen bonds– Weak attraction– Easily made &
broken
Specific Heat
• Heat needed to raise or lower temperature
• Water has high specific heat
– Modulates temperature in living bodies
– As water absorbs heat, hydrogen bonds break
Water, Temperature & Hydrogen Bonds
Cohesion & Adhesion
• Cohesion– Hydrogen bonds make molecules “stick
together”– Aids water movement in plants
• Adhesion– Weak electrical attraction of molecules– Capillary action
Surface Tension
Cohesion of water molecules at its surface
Water as a Solvent
• Solution = homogeneous mixture of substances
• Solvent = substance in greatest amount
• Solute = dissolves in solvent
• Water is a powerful solvent
• Ions break away in presence of water
How Salt Dissolves in Water
Water &Nonpolar Molecules
• Nonpolar molecules– Do not form hydrogen bonds– Not dissolved in water
Oil is Hydrophobic
Ionized Water
• Water can Accept or donate protons
H2O OH- + H+
Acids & Bases
• Acid– Dissociates to form H+ ions in water– pH less than 7
• Base– Accepts H+ ions in water– pH greater than 7
pH scale
• Indicates concentration of H+ ions
• Neutral is at 7
• Determined by taking negative value of exponents of its H+ ions concentration
End Chapter 3