chem

• ideal gas=small, nonpolar
• lower average velocity=lower temp
• buffer capacity depends on the number of moles present
• smaller ions have a larger lattice energy
• greater molar mass= greater LDFs
• linear=2 bonding pairs
• trigonal planar=3 bonding pairs
• tetrahedral=4 bonding pairs
• trigonal bipyramidal= 5 bonding pairs
• octahedral= 6 bonding pairs
• electron deficient elements: Be (2) B(3)
• Expanded octets: P(5) S(6)
• molecules with the lowest charge and highest molar mass will plate out the greatest mass of metal
• when a current is run through water, it will both reduce into hydrogen gas and oxidize into oxygen gas
• standard reduction potential of ions must be greater than the metal's SRP for a reaction to occur
• if Q=K, the cell is at equilibrium and has zero voltage
• the best indicator changes color at the equivalence point of the titration.
• more ions in solution=greater conductivity
• all single bonds are sigma bonds, additional bonds are pi bonds
• as long as temp remains constant, so does K.
• an element that is more electronegative will have the negative partial charge
• HCl is strong
• HBr is strong
• HI is strong
• HClO4 is strong
• HNO3 is strong
• H2SO4 is strong
• HF is weak
• HC2H3O2 is weak
• HNO2 is weak
• HOCl is weak
• HCO2H is weak
• HCN is weak
• H2SO3 is weak
• H2CO3 is weak
• as [HA] decreases, percent ionization increases, [H3O+] decreases, pH increases
• Dilution with water causes the value of Q to become less than Ka. This causes a shift in the equilibrium with a net conversion from reactants to products. As a result, the percent ionization of the acid increases.
• common ion effect: if the salt that is being dissolved shares an ion with the solution it is being dissolved in, less of that salt will dissolve.
• saturated- solute dissolves until it is unable to dissolve, leaving undissolved substances at bottom.
• unsaturated- completely dissolves, no remaining substances.