The Chemistry of Life Why are we studying chemistry? Chemistry is the foundation of Biology.
Basic Chemistry Review AP Biology. Why are we studying chemistry????
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Transcript of Basic Chemistry Review AP Biology. Why are we studying chemistry????
Basic Basic ChemistryChemistry
ReviewReviewAP BiologyAP Biology
Why are we studying chemistry????
2. Atoms combine by chemical bonding to form molecules
1. Matter consists of chemical elements in pure form and in combinations called compounds
3. Weak chemical bonds play important roles in the chemistry of life
4. A molecule’s biological function is related to its shape
5. Chemical reactions result from making and breaking chemical bonds
Main IdeasMain Ideas
Naturally Occurring Elements in the Human Body
Structure of an Structure of an AtomsAtoms
• Protons• Neutrons• Electrons -Found in
energy levels
NucleusNucleus
Each Energy Level Can Hold Each Energy Level Can Hold A Certain Numbers of A Certain Numbers of
Electrons!Electrons!Only Only TWO TWO on on the the first first levellevel!!
Different atoms have different Different atoms have different numbers of electrons!numbers of electrons!
Eight Eight on on the the 22ndnd and and 3rd 3rd levelslevels!!
Each Energy Level Can Hold Each Energy Level Can Hold A Certain Numbers of A Certain Numbers of
Electrons!Electrons!
Electrons can move from one energy level to another
• Atomic Atomic NumberNumber
• Number of Number of ProtonsProtons
1
1
•Atomic MassAtomic Mass
•Sum of Sum of Protons & Protons & NeutronsNeutrons
Periodic Table
IsotopesIsotopes are atoms that have the same number of protons and differ only in the
number of neutrons.
Most isotopes are stable but radioactive isotopes are unstable and break down into more stable forms by emitting particles and
energy (radiation). Radiation can be detected, so radioactive isotopes are useful as labels in scientific
research and medical diagnostic procedures.
• Radioactive isotopes are used to diagnose medical disorders. (C-11, F-18, O-15)– Radioactive tracers can be used with imaging
instruments to monitor chemical processes in the body.
atoms can gain or lose electronsatoms can gain or lose electrons
Cation
Anion
3P
3P3P
3P
3P
3P
atoms can gain or lose electronsatoms can gain or lose electrons
Ionization: requires energy
Why do atoms lose and gain electrons?
To become more stable.
Stability=full outer energy level
Why do Atoms Form Compounds?
•Stability.•What makes an atom stable?
•Full outer energy level.•Eight.
How can atoms become stable?
•Gain or lose electrons.•Share electrons.
•A Chemical Bond holds atoms together in a compound.
•Two basic typesTwo basic types:
•Ionic•Covalent
Ionic Bonding
Transfer of
electrons
from one
atom to
another
atom.
Occurs between
metals and nonmetals.Remember: Atoms need a full
outer energy level to be stable.
Bonding occurs with the valence electrons.
Occurs between metals and nonmetals.
Metals are electron donors.
Non-metals are electron accepters.
Called compounds.
OPPOSITS ATTRACT!
Ionic
Bondin
g
Covalent Bonding
The
sharing of
electrons
between
atoms.
Occurs between nonmetal
s and nonmetal
s.Called
Molecules.
Hydrogen and Fluorine
Hydrogen and Chlorine
Single, Double, Triple
Unequal Sharing
δ+
Polar
δ_
Polar covalent bonds in a water molecule
Covalent Bonds• The attraction of electrons to an atom
is called electronegativity. • The more electronegative an atom,
the more a shared electron is pulled towards its nucleus.
• If two atoms are of the same element or of the same electronegativity, the pull of the electron is equal and the bond is a NONPOLAR covalent bond.
•POLAR covalent bonds form when one atom is more electronegative than another; thus, the electron is pulled closer to the atom with the high + charge…forming poles.
Hydrogen BondingHydrogen BondingWeak attraction between hydrogen and an electronegative atom such as oxygen and nitrogen taking part in a polar covalent bond.
A hydrogen bond
Hydrogen Hydrogen bonds in bonds in protein protein
structurestructure
Hydrogen Hydrogen bonds in DNA bonds in DNA
structurestructure
Chemical Reactions and Energy
• All chemical reactions release or absorb energy.– Heat, light, sound
• Chemical reactions are the making and breaking or bonds.
Chemical EquationsChemical Equations--show chem. rxnsshow chem. rxns..
2H2H22 + O + O22 2H 2H22OO Reactants:Reactants: substances that undergo substances that undergo
chemical reactions.chemical reactions. Products:Products: substance formed by chemical substance formed by chemical
reactions. reactions. Coefficient:Coefficient: shows the # of mol of each shows the # of mol of each
substancesubstance Subscript:Subscript: the # of atoms of each element in the # of atoms of each element in
the moleculethe molecule Ex. 2HEx. 2H22OO Ex #2: CEx #2: C1212HH2222OO1111
1. Exergonic
• Chemical reactions that releases energy are called exergonic.– Glow sticks
• If heat is released, it is called exothermic.
2. Endergonic
• Chemical reactions that require energy are called endergonic.
• Ex: Cold Packs• If heat is absorbed, it is called
endothermic
Oxidation-Reduction Rxns• Transfer electrons from one reactant to another• Loss of electrons – oxidation• Gain of electrons – reduction
Ex. Xe- + Y X + Ye-
(X is the electron donor, so reducing agent;
Y is the electron acceptor, so oxidizing agent.)
Catalysts and InhibitorsSome reactions proceed slowly.
•They can be sped up by a catalysts.– Catalysts are not used up in the reaction.– EX: enzymes (biological catalysts)
Some reactions proceed to fast.•They can be slowed down by
inhibitors.– EX: Preservatives in food
Photo- synthesi
s: a solar-
powered rearrangement
of matter