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AP Chemistry chapter 4

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Section 1

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Types of Equations

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Chemistry Science

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Mar 14, 2020

Cards (19)

Section 1

(19 cards)

Types of Equations

Front

Molecular equation - shows the complete chemical formulas of reactants and products Complete ionic equation - shows all soluble strong electrolytes as ions (split the aqueous compounds) Net ionic equation - shows reaction after spectator ions are eliminated

Back

Molarity

Front

Molarity (M) = moles of solute / liters of solution

Back

Bases

Front

Bases - accept ionizable hydrogen (proton acceptor). Bases taste bitter and feel slippery. Bases often contain hydroxide or amines (-NH2). Other aqueous anions can also attract protons to form insoluble compounds or gases and function as bases. Ammonia (NH3) is a common base

Back

Oxidation number rules

Front

Elements in their elemental form have an oxidation number of 0. The oxidation number of a monatomic ion is the same as its charge. Oxygen has an oxidation number of -2, except in the peroxide ion (O2 2- ) in which it has an oxidation number of -1. Hydrogen is -1 when bonded to a metal, +1 when bonded to a nonmetal. Fluorine always has an oxidation number of -1. The other halogens have an oxidation number of -1 when they are negative; they can have positive oxidation numbers, however, most notably in oxyanions. The sum of the oxidation numbers in a neutral compound is 0. The sum of the oxidation numbers in a polyatomic ion is the charge on the ion.

Back

Dilution

Front

M1V1=M2V2

Back

TItration

Front

- analytical technique used to determine the unknown concentration of a solution by reacting it with a solution of known concentration (called a standard solution). Can be an acid-base neutralization, redox, or any other type of reaction. Equivalence point - point at which the moles of the unknown substance completely react with the moles of the standard solution. End point - point at which the indicator changes color and is designed to occur as closely as possible to the equivalence point

Back

Oxidation-reduction reactions

Front

Leo Ger OIL RIG Oxidation: loss of e ; ox # increases Reduction: gain of e ; ox # decreases example: Fe 2+ + 2e Fe(s) (reduction)

Back

Electrolytes

Front

- Ionic compounds are strong electrolytes (single arrow for dissociation reaction) - Most molecule compounds (not molecular acids) are nonelectrolytes - Strong molecular acids are strong electrolytes (single arrow) - Weak bases are weak electrolytes (double arrow)

Back

Seven strong acids

Front

Hydrochloric acid, HCl Hydrobromic acid, HBr Hydroiodic acid, HI Chloric acid, HClO3 Perchloric acid, HClO4 Nitric acid, HNO3 Sulfuric acid, H2SO4

Back

Half reaction method

Front

determine oxidation & reduction write two separate half-reactions balance all atoms except H & O balance O's (add H2O's) balance H's (add H+'s) add e 's to more positive side balance e's between half-reactions combine half-reactions

Back

Writing net ionic equations

Front

(i) Write balanced molecular equation. (ii) Separate all aqueous strong electrolytes into ions. (iii) Cancel spectator ions.

Back

Solubility rules

Front

- All compounds containing alkali metal cations and ammonium ion are soluble - All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble. - All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+ - All sulfates are soluble except those containing Hg2+, Pb2+, Ca2+, Sr2+, or Ba2+ - All hydroxides are insoluble except compounds compounds of the alkali metals Ca2+, Sr2+, Ba2+ - All compounds containing PO4^2-, S^2-, CO3^2-, and SO3^2- ions are insoluble except those containing alkali metals or NH4+

Back

Eight strong bases

Front

Group1 hydroxides o LiOH, NaOH, KOH, RbOH, CsOH Heavy group 2 hydroxides o Ca(OH)2, Sr(OH)2, Ba(OH)2

Back

Metathesis Reactions

Front

- Use formulas to determine ions present. - Write formulas of product by switching cations and anions (use charge to find new formulas) - Balance

Back

Neutralization reactions

Front

- When acidic and basic hydroxide solutions mix the result is water and a salt (ionic compound formed from a cation from an base and an anion from an acid)

Back

Acids

Front

contain ionizable hydrogen (proton donor). Acid formulas usually start with a hydrogen or contain -COOH. Acids have a sour taste and burn. Monoprotic - 1 ionizable hydrogen o HCl o CH3COOH, the hydrogen in the carboxyl group (COOH) is ionizable Diprotic - 2 ionizable hydrogens o H2SO4 o Only the first ionizable hydrogen in H2SO4 ionizes completely. Triprotic - 3 ionizable acids o H3PO4

Back

Common Precipitates

Front

Hydroxides, carbonates, phosphates, and chromates (except with ammonium and group 1)

Back

Gas forming acid-base reactions

Front

carbonates (and hydrogen carbonates) H2O and CO2 + salt Sulfites (SO3) H2O and SO2 + salt Sulfides H2S + salt Nitrites (NO2) NO + NO2 + salt

Back

Solution Stoichiometry

Front

- Moles (mole ratio) are the common link that connect all substances in chemical reactions. How do you get from substance A to substance B? o Mole ratio from the coefficients in the balanced equation How do you get to (and from) moles? o Liters - use molarity o Grams - use molar mass o Molarity - use volume in liters

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