Types of chemical reactions
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| Electrolytes | are substances whose aqueous solutions conduct electric current.
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| non electrolytes | do not conduct electricity.
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| 3 major classes of solutes are strong electrolytes: | Strong acids
Strong bases
Most soluble salts
These compounds are completely or nearly completely ionized (or dissociated) in dilute aq solutions, so they are strong electrolytes.
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| a substance that produces H+ in aq solution
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| A base is a substance that | produces OH- ions in aq solution.
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| a compound that contains a cation (other than H+) and an anion (other than OH- or O2-)
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| Strong acids | ionize (separate into H+ and stable anions) completely or nearly completely in dilute aq solutions.
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| Examples of strong acids | HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HNO3 nitric acid
H2SO4 sulfuric acid
HClO3 chloric acid
HClO4 perchloric acid
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| Ionize only slightly (usually less than 5%) in dilute aq solution, so that’s why they are weak (less H+).
Have reversible reactions
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| examples of weak acids | HF hydrofluoric acid
CH3COOH acetic acid (vinegar)
HCN hydrocyanic acid
HNO2 nitrous acid
H2CO3 carbonic acid (soda water)
H2SO3 sulfurous acid
H3PO4 phosphoric acid
(COOH)2 oxalic acid
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| are soluble in water and are dissociated completely in dilute aq solution. Ionize 100% in H2O
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| Common strong bases | LiOH lithium hydroxide
NaOH sodium hydroxide
KOH potassium hydroxide
RbOH rubidium hydroxide
CsOH cesium hydroxide
Ca(OH)2 calcium hydroxide
Sr(OH)2 strontium hydroxide
Ba(OH)2 barium hydroxide
All hydroxides of IA and IIA metals.
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| not very basic.
Cu(OH)2 copper (II) hydroxide
Fe(OH)2 iron (II) hydroxide
Fe(OH)3 iron (III) hydroxide
Zn(OH)2 zinc (II) hydroxide
Mg(OH)2 magnesium hydroxide
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| weak bases | covalent compounds that ionize slightly in water.
Ammonia is most common weak base
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| Solubility Guidelines for Compounds in Aqueous Solutions | Common inorganic acids and low-molecular-weight organic acids are water soluble.
All common compounds of the Group IA metal ions and the ammonium ion are water soluble.
Li+, Na+, K+, Rb+, Cs+, and NH4+
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| Solubility Guidelines for Compounds in Aqueous Solutions continued | Common nitrates, acetates, chlorates, and perchlorates are water soluble.
NO3-, CH3COO-, ClO3-, and ClO4-
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| Solubility Guidelines for Compounds in Aqueous Solutions continued | Common chlorides are water soluble.
Exceptions – AgCl, Hg2Cl2, & PbCl2
Common bromides and iodides behave similarly to chlorides.
Common fluorides are water soluble.
Exceptions – MgF2, CaF2, SrF2, BaF2, and PbF2
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| Solubility Guidelines for Compounds in Aqueous Solutions continued | Common sulfates are water soluble.
Exceptions – PbSO4, BaSO4, & HgSO4
Moderately soluble – CaSO4, SrSO4, & Ag2SO4
Common metal hydroxides are water insoluble.
Exceptions – LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
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| Common carbonates, phosphates, and arsenates are water insoluble.
CO32-, PO43-, & AsO43-
Exceptions- IA metals and NH4+
Moderately soluble – MgCO3
Common sulfides are water insoluble.
Exceptions – IA metals and NH4+ plus IIA metals
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| Solubility | The higher the charges are the more strongly the anion and cation attract one another and the less soluble the salt is likely to be.
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| Size of ions also matters: the smaller ions are able to get closer to one another and thus increase the ionic attractive force. Larger anions with low neg charges almost always give soluble salts (nitrates, perchlorates)
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| Reactions in Aqueous Solution | Symbolic representation of what is happening at the laboratory and molecular levels in aqueous solutions.
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| three ways to write reactions in aqueous solutions | Molecular equation/formula unit equations
Show all reactants & products in molecular or ionic form
Total ionic equation
Show the ions & molecules as they exist in solution
Net ionic equation: shows ions that participate in reaction removes spectator
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| Spectator ions | do not participate in the reaction. They are the ones that appear in the same form on both sides of the total ionic equation
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| Binary compounds | made of two elements.
metal + nonmetal = ionic compound
nonmetal + nonmetal = covalent compound
Name the more metallic element first.
Name the less metallic element second.
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| Binary Ionic Compounds | are made of a metal cation and a nonmetal anion.
Cation named first
Anion named second
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| Metals exhibiting multiple oxidation states are most of the transition metals, metals in groups III (not Al), IV, & V
Old method: add “ic” for higher oxidation state “ous” for lower
Modern method: Roman numerals in () to indicate metal’s oxidation sta
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| Pseudobinary ionic compounds | There are three polyatomic ions that commonly form binary ionic compounds.
OH- hydroxide
CN- cyanide
NH4+ ammonium
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| Binary Acids | binary compounds w/ hydrogen & nonmetal
Usually gases @ room temp
Nomenclature for gaseous compounds: hydrogen (stem)ide.
When the compounds are dissolved in water they form acidic solutions.
Nomenclature for the acidic solutions is
hydro (stem)ic a
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| Binary covalent molecular compounds composed of two nonmetals other than hydrogen | Nomenclature must include prefixes that specify the number of atoms of each element in the compound.
Use the minimum number of prefixes necessary to specify the compound.
Frequently drop the prefix mono-.
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| Ternary Acids and Their Salts | are made of three elements
H, O, & a nonmetal
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| naming Ternary Acids and Their Salts | 2 of the compounds are chosen as the basis for the nomenclature system.
Higher oxidation state for nonmetal is named (stem)ic acid.
Lower oxidation state named (stem)ous acid
Salts: Anions of -ic make “ate” salts.
Anions of -ous acids make “ite” salts
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| There are two other possible acid and salt combinations. | Acids that have a higher oxidation state than the “ic” acid are given the prefix “per”.
These acids and salts will have one more O atom than the “ic” acid.
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| Acids that have a lower oxidation state than the “ous” acid are given the prefix “hypo”.
These acids and salts will have one less O atom than the “ous” acid.
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