acids - substances that ionize to form hydrogen ions
- aka proton donors (H+ is essentially just a proton)
- monoprotic acids - donate 1 hydrogen ion per molecule (ex. HCl, HNO3)
- diprotic acids - donate 2 hydrogen ions per molecule (ex. H2SO4); ionization occurs in 2 steps
bases - substances that accept hydrogen ions, produce hydroxide ions in reactions
- ex. NaOH, KOH, Ca(OH)2
- doesn't necessarily have to contain hydroxide ions
- must accept hydrogen ion
strength of acids/bases
- strong electrolyte = strong acid/base
- weak electrolyte = weak acid/base
- reactivity - depends on the actions of both the cation/anion, not just strength of acid/base
- strong acids - HCl, HBr, HI, HClO3, HNO3, H2SO4
- strong bases - group 1A/2A metal hydroxides
- molecular compounds that aren't acids/bases are nonelectrolytes
neutralization reactions - mixing an acidic and base solution
- product has none of the characteristics of the reactants
- salt - ionic compound whose cation comes from a base and whose anion comes from an acid
- neutralization reaction between an acid and metal hydroxide produces water and a salt
- sulfate/carbonate combine w/ hydrogen ions to form gas
oxidation-reduction (redox) reactions - involve transfer of electrons between reactants
- oxidation - loss of electrons in a substance
- reduction - gain of electrons in a substance
- in reactions, 1 reactant loses an electron and another reaction gains an electron
- oxidation/reduction come together
oxidation number - aka oxidation state; actual chargeof the atom as a monoatomic ion
- oxidation >> increase in oxidation number
- reduction >> decrease in oxidation number
- equals 0 when atom is in its elemental form
- equals charge for all monoatomic ions
- usually negative for all nonmetals
- sum of all oxidation numbers in a neutral compound equals 0
displacement reaction - ion in a solution gets replaced through oxidation of an element
- A + BX >> AX + B
- metals undergo displacement reactions w/ acids to form salts and hydrogen gas
- net ionic reaction shows a change in oxidation states
activity series - list of metals arranged in order of decreasing oxidation
- oxidation causes metals to be eaten away
- active metals - metals at the top of the list; alkali/alkaline earth metals; reacts most readily to form compounds
- noble metals - metals at the bottom of the list; 8B/1B metals
- any metal can be oxidized by elements below it on the list
- only metals above hydrogen in the activity series can react w/ acids to form H2
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