CHEM 1211: Exam 3
100 Cards in this Set
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Strong Acids
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A strong acid is an acid that ionizes completely in an aqueous solution by losing one proton, according to the equationHCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4
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Weak Acids
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A weak acid is an acid that dissociates incompletely. HF, CH3COOH, HCN, H3PO4, HNO2, H2CO3, H2SO3, (COOH)2
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Strong Bases
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Hydroxides of Group IA metals and the heavier metals of Group IIALiOH, NaOH, KOHm RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
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Weak Bases
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Covalent substances that are soluble in, but that ionize only slightly in, watermost common: ammonia- NH3
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Inorganic Acids(solubility)
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soluble
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Group IA(solubility)
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soluble
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ammonium ion(solubility)
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NH4; soluble
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Common Nitrates(solubility)
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NO3; soluble
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Common Acetates(solubility)
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CH3COO; soluble
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Common Chlorates(solubility)
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ClO3; soluble
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Common Perchlorates(solubility)
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ClO4; soluble
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Chlorides(solubility)
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soluble except for AgCl, Hg2Cl2, and PbCl2
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Bromides(solubility)
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soluble except for AgBr, Hg2Br2, and PbBr2moderately soluble: HgBr2
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Iodides(solubility)
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similar to bromides and chlorides; many heavy-metal iodides are insoluble
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Fluorides(solubility)
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soluble except MgF2, CaF2, SrF2, BaF2 and PbF2
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Sulfates(solubility)
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soluble except for PbSO4, BaSO4, and HgSO4moderately soluble: CaSO4, SrSO4, and Ag2SO4
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Common Metal Hydroxides(solubility)
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insoluble except those of the Group IA metals and the heavier members of the Group IIA metals beginning with Ca(OH)2
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Carbonates(solubility)
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insoluble in water except those of the Group IA metals moderately soluble: MgCO3
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Phosphates(solubility)
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insoluble in water except those of the Group IA metals
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Aresenates(solubility)
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insoluble in water except those of the Group IA metals
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NH4(solubility)
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moderately soluble
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Sulfides(solubility)
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insoluble in water except for those of the Group IA metals and Group IIA metals
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Binary Compounds(naming)
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A metal cation that exhibits only one oxidation state and a nonmetal anion- metal is named first and then the nonmetal with -ide at the end
A metal cation that exhibits more than one oxidation state with a nonmetal anion- metal, roman numeral, nonmetal with -ide at the end
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Pseudobinary Ionic Compounds(naming)
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consist of polyatomic ions that behave as simple binary ionic compounds
OH, CN, NH4
uses binary ionic naming system
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Binary Molecular Compounds(naming)
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2 nonmetals bonded together
name the first element then the second with a prefix: mono-, di, tri-, tetra-, penta-, hexa, hepta-, octa-, nona-, deca-
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Binary Acids(naming)
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hydrogen and a nonmetal are bonded
starts with hydrogen then the nonmetal ending in -ide
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AB2
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no lone pairs on A
linear electronic geometry and molecular sp hybridization nonpolar
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AB3
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no lone pairs on A
trigonal planar electronic and molecular geometry sp2 nonpolar
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AB4
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no lone pairs on A
tetrahedral electronic and molecular geometry sp3 nonpolar
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AB3U
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one lone pair on A
tetrahedral electronic geometry trigonal pyramidal sp3 polar
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AB2U2
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two lone pairs on A
tetrahedral electronic geometry angular, bent, or v-shaped sp3 polar
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ABU3
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three lone pairs on A
tetrahedral electronic geometry linear sp3 polar
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AB5
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trigonal bipyramidal electronic geometry and molecular
nonpolar sp3d
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AB4U, AB3U2, AB2U3
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one lone pair- seesaw
two lone pairs- T-shape three lone pairs- linear tringonal bipyramidal electronic geometry polar sp3d
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AB6, AB5U, AB4U2
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octahedral electronic geometry
square planar AB5U- square pyramidal AB6- octahedral sp3d2 nonpolar
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ternary acids and their salts
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contain three elements: hydrogen, oxygen, and another nonmetal
an -ic acid
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boric acid
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H3BO3
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carbonic acid
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H2CO3
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silicic acid
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H4SiO4
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nitric acid
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HNO3
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phosphoric acid
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H3PO4
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arsenic acid
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H3AsO4
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sulfuric acid
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H2SO4
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selenic acid
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H2SeO4
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telluric acid
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H6TeO6
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chloric acid
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HClO3
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bromic acid
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HBrO3
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iodic acid
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HIO3
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ternary acids indicating the higher oxidation state
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(stem)ic acid
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ternary acids indicating the lower oxidation state
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(stem)ous acid
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anions of -ous acids
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have -ite suffixes
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anions of -ic acids
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have -ate suffixes
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nitrous acid
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HNO2
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nitric acid
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HNO3
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sulfurous acid
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H2SO3
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sulfuric acid
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H2SO4
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chlorous acid
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HClO2
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chloric acid
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HClO3
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sodium nitrite
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NaNO2
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sodium nitrate
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NaNO3
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sodium sulfite
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Na2SO3
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sodium sulfate
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Na2SO4
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sodium chlorite
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NaClO2
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sodium chlorate
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NaClO3
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hypo-
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indicates the lowest oxidation state when there are two ternary acids of a central nonmetal
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per-
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highest oxidation state when there are more than two ternary acids of a central nonmetal
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hypochlorous acid
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HClO
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chlorous acid
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HClO2
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chloric acid
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HClO3
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perchloric acid
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HClO4
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sodium hypochlorite
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NaClO
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sodium chlorite
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NaClO2
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sodium chlorate
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NaClO3
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sodium perchlorate
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NaClO4
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ternary salts
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compounds that result from replacing the hydrogen in ternary acid with another ion
contain the cation of a base and the anion of an acid
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sodium hydrogen carbonate
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NaHCO3
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potassium hydrogen sulfate
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KHSO4
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potassium dihydrogen phosphate
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KH2PO4
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potassium hydrogen phosphate
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KHPO4
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oxidation-reduction reactions
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aka redox are "energy producing reactions"
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oxidation
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algebraic increase in oxidation number
process in which electrons are lsot
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reduction
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an algebraic decrease in oxidation number
process in which elctrons are gained
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oxidizing agents
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substances that gain electrons and oxidize other substances
always reduced
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reducing agents
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substance that lose electrons and reduce other substances
are always oxidized
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combination reactions
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involve the cobination of two substances to form a compound
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metal + nonmetal --->
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combination reaction
produces a binary ionic compound
2Na + Cl2 ---> 2NaCl
2Al + 3Br2 ----> 2AlBr3
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nonmetal + nonmetal --->
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combination reaction
produce covalent binary compound
P4 + 5O2 ---> P4O10
P4 + 6Cl2 ---> 4PCl3
2As + 3Cl2 --->2AsCl3
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compound + compound --->
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combination reaction
produces a compound
NH3 + HCl ---> NH4Cl
Li2O + SO3 ---> Li2SO4
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compound---> element +element
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decomposition reaction
2N2O ---> 2N2 + O2
CaCl2 ---> Ca + Cl2
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compound ---> compound + element
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decomposition reaction
2H2O2 ---> 2H2O + O2
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diproportion reaction
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when the same element is oxidized and reduced
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compound ---> compound + compound
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decomposition reaction
NH4HCO3 ---> NH3 + H2O + CO2
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displacement reactions
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occur when one element displaces another element from a compound
redox reactions in which the more active metal displaces the less active metal of hydrogen from a compound in aqueous solution
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more active metal + salt of less active metal --->
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displacement reaction
produces less active metal + salt of more active metal
2AgNO3 + Cu ---> Cu(NO3)2 + 2Ag
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active metal + nonoxidizing acid --->
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displacement reaction
produces hydrogen + salt of acid
2Al +3H2SO4 --->Al2(SO4)3 + 3H2
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active nonmetal + salt of less active nonmetal --->
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displacement reaction
produces less active nonmetal + salt of more active nonmetal
Cl2 + 2NaI ----> I2 + 2NaCl
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metathesis reactions
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occur when two ionic aqueous solutions are mixed and the ions switch partners
AX + BY ---> AY + BX
sometimes called "double displacement" reactions
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neutralization reactions
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type of metathesis reaction
the reaction of an acid with a metal hydroxide base produces salt and water
HBr + KOH ---> KBr + H2O
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precipitation reactions
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metathesis reactions
insoluble compound is formed as a product
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gas-formation reactions
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there is a formation of an insoluble or slightly soluble gas when there are no gaseous reactants
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Study Guide: Formulas