presentation: chapters 2 - ap biology with mrs. haas · presentation: chapters 2 chemical context...
TRANSCRIPT
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Presentation: Chapters 2 Chemical Context of Life
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Atom Basics
Atomic Structure
Atomic mass vs. Atomic Weight
Isotopes- Radioactive tracers
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Intramolecular Forces
Bonding Forced WITHIN (Intra-) molecules
Covalent bonding- polar or non polar
Ionic bonding
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Covalent Bonding
Sharing electrons
May be polar or non polar
Based on electronegativity= pull on electrons (affinity for e-)
Nonpolar= Atoms have equal electronegativity
Electrons are shared equally
ex. carbon and hydrogen, diatomic molecules
Polar= One atom has higher electronegativity
Electrons closer to one atom, partially negative
ex: oxygen and hydrogen
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Examples
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Polar Covalent Bond- Water
Oxygen has greater electronegativity
Electrons are drawn closer
Oxygen is now partially negative and hydrogens are partially positive
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Polar Covalent Bonding
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Non-polar Covalent Bonding
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Ionic Bonding
Atoms gain (-) or lose (+) electrons to achieve a full outer (valence) shell
Oppositely charged ions (cation/anion) attract one another
A metal and a nonmetal
Usually forms a lattice pattern
Stronger than covalent bonding
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Intermolecular Forces (IMFs)
Bonding BETWEEN (Inter-) molecules
Hydrogen Bonding
Dipole-dipole
Van der Waals forces
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Hydrogen “Bond”/Interaction
Forms between two polar molecules
Hydrogen bonded to N, O, F the bonded to another polar molecule
Partial charges of one molecule are attracted to the opposite charges of another
Ex. water and ammonia
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Other IMFs
Van der Waals attractions
Weak IMFs caused by changing dipoles
Gecko Fingers