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What does the depth of the PE well tell you?
Tells you how strong the attraction between the two atoms are; and how much energy would be needed to get out of the well TERM 2
Non-polar bonds
DEFINITION 2 electrons are shared equally TERM 3
Polar bonds
DEFINITION 3 Electrons are shred unequally which results in a dipole TERM 4
Ionic Bond
DEFINITION 4 electrostatic attraction between two charred ions (not really an ionic bond) Ionic lattice forms Force of attraction - constant (q+q-/r^2) PE = constant (q+q-/r) large charge difference = stronger attraction larger ions - smaller attraction TERM 5
What's the same between intermolecular
forces and bonds?
DEFINITION 5 force of electrostatic attraction has to overcome energy release energy when formed
What is different between intermolecular
forces and bonds?
Bonds = attraction between electrons from one atom and protons of another atom IM = attraction between one dipole to another Bonds = when bonds break new SPECIES are formed IM = when SAME SPECIES (usually phase change) TERM 7
Types of IM's?
DEFINITION 7 LDF's = temporary fluctuating dipoles, non-polar molecules only force present, in all substances Dipole-Dipole = stronger than LDF's, in polar substances Hydrogen Bonds = stronger than LDF's and dipole-dipole, H is bonded to O,N,F; interactions with other molecules are stronger TERM 8
Enthalpy
DEFINITION 8 Change in H heat absorbed or released during a reaction under constant pressure Endothermic = energy absorbed = surrounding gets cold (Delta H is +) Exothermic = energy released = surrounding gets warm (Delta H is -) TERM 9
Entropy
DEFINITION 9 number of possible arrangements in a given state more number of possible arrangements = higher probability of that state S=klogW (W=# arrangements) Is temperature and surrounding dependent TERM 10
2nd Law of Thermodynamics
DEFINITION 10 for any change the total entropy of the universe must INCREASE! total S = change in S (system) + change in S (surroundings)
