General Chem
General Chem
General Chem
General Chem
General Chem
100
Intramolecular bonds
What is ionic, covalent, metallic
100
IMF types in order of strength
What is network, hydrogen, dip dip, london disperson
100
London dispersion forces
What is seen in neutral nonpolar molecules. more electrons stronger the force. temporary dipoles. gases at room temp
100
Phase change covalent bond
What is intermolecular forces break
100
Phase change ionic bond
What is intramolecular forces break
200
Lewis dot structure
What is 1. count valence 2. adjust charge add eletron if negative and take away if pos 3. draw skeletal structure, the least electronegative is central 4. add electrons to surronding until each has complete outer shell. 5. add remaining to the central 6. look at central a) if it is complete you done b) if has fewer than eight remove a pair from an outer. C) if it is in the 3 period it can have 8-12 eletrons.
200
Resonance forms
What is draw the double bond every way possible and draw ⇌. strength is between single and double bond since they are happening at the same time.
200
Equilibrium
What is a dynamic, reversible state in which the forward rate is equal to the reverse rate
200
Reaction quotient (Q)
What is reaction quotient (Q) at initial, Q=[products]/[reactants]
200
Equilibrium constant (K)
What is at equilibrium, K=[products]/[reactions]
300
Comparing Q to K
What is 1. QK, shifts left
300
Le Chatelier's principle
What is Systems at equilibrium respond to disturbances by partially countering the effect of the disturbance
300
Strong acids
What is HCl, HBri, HI, HClO₄, H₂SO₄, HNO₃
300
Strong bases
What is strong bases group I and group II hydroxides
300
Neutral
What is pH = pOH = 7 @ 25°C
400
Weak acid
What is does not completely dissociate in water; includes carboxylic acids and conjugate acids
400
Weak base
What is does not completely dissociate in water; includes ammonia, amines and pyridines, and conjugate bases
400
Half equivalence point
What is [HA] = [A⁻] and pH = pKa
400
Equivalence point
What is moles of titrant and moles of titrate are equal (MaVa=MbVb) and pH rapidly changes
400
Solubility rules
What is All sodium, potassium, ammonium, and nitrate salts are soluble in water
500
Common ion effect
What is salt is less soluble in a solution that has an ion in common with the salt
500
Gibbs free energy
What is delta g = -RT lnK
500
Arrhenius A/B definition
What is -Acid- substance that ionizes in water and produces H+ ions -ex. HCl→H⁺+Cl⁻ -Base- substance that ionizes in water and produces OH- ions -ex. NaOH→Na⁺+OH⁻
500
Bronsted-Lowry A/B definition
What is -Acid- substance that is capable of donating a proton (H+ ion) -Base- substance that is capable of accecpting a proton Reaction: NH₃ + H₂O ↔ NH₄⁺ + OH⁻ Bronsted-Lowry Acid: H₂O and NH₄⁺ Bronsted-Lowry Base: NH₃ and OH⁻ Conjugate Pair: NH₄⁺ and NH₃, H₂O and OH⁻
500
Lewis A/B definition
What is -Base- electron pair donor -Acid- electron pair accecptor -All Bronsted-Lowry bases are Lewis bases and all Bronsted-Lowry acids are Lewis acids -ex. NH₃ + BCl₃ → H₃NBCl₃ where NH₃ is Lewis base and BCl₃ is the Lewis acid, accecpting the electron pair.
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