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Chemical Equation • A representation of a chemical reaction: C2H5OH + 3O2 2CO2 + 3H2O reactants products Chemical Equation C2H5OH + 3O2 2CO2 + 3H2O The equation is balanced. 1 mole of ethanol reacts with 3 moles of oxygen to produce 2 moles of carbon dioxide and 3 moles of water Molecular representation of a rxn Molecular rep of a rxn Which of the following correctly describes the balanced chemical equation given below? There may be more than one true statement. 4Al + 3O2 2Al2O3 I. For every 4 atoms of aluminum that react with 6 atoms of oxygen, 2 molecules of aluminum oxide are produced. II. For every 4 moles of aluminum that react with 3 moles of oxygen, 2 moles of aluminum oxide are produced. III. For every 4 grams of aluminum that react with 3 grams of oxygen, 2 grams of aluminum oxide are produced. Rules for Balancing Reactions • For each element, the number of atoms on the reactant side must equal the number of atoms on the product side. • The subscripts cannot change. Only coefficients can be changed. • The coefficients must be whole numbers. • The coefficients must be simplified (divided down) as much as possible. Which of the following correctly balance the chemical equation given below? There may be more than one correct balanced equation. CaO + C CaC2 + CO2 I. II. III. IV. CaO2 + 3C CaC2 + CO2 2CaO + 5C 2CaC2 + CO2 CaO + (2.5)C CaC2 + (0.5)CO2 4CaO + 10C 4CaC2 + 2CO2 Which of the following statements are true concerning balanced chemical equations? There may be more than one true statement. I. The number of molecules is conserved. II. The coefficients tell you how much of each substance you have. III. Atoms are neither created nor destroyed. IV. The coefficients indicate the mass ratios of the substances used. V. The sum of the coefficients on the reactant side equals the sum of the coefficients on the product side. 1. CH4 + 2. SiO2 + 3. K + 4. C2H6 + 5. NH3 + O2 CO2 + H2O HF SiF4 + H2O H2O H2 + KOH O2 CO2 + H2O O2 NO + H2O 1. H2SO4 2. Fe(CN)3 + 3. K3PO4 + + Ca(OH)2 MgCl2 H2O CaSO4 FeCl3 H3PO4 + H2O + Mg(CN)2 + KOH Reaction Symbols • (s) solid • (l) liquid • (g) gas • (aq) aqueous = dissolved in water • △ heat added (put over arrow) Diatomic Molecules • Remember which atoms make diatomic molecules: – H2 and N2, O2, F2 Cl2 Br2 I2 -This is only when they are by themselves! -When other atoms are by themselves they don’t have any subscripts, for example iron is just Fe Write the balance chemical equation for the following: 1) Hydrogen gas is ignited and burns, combining with oxygen to form water vapor. 2) Silver oxide is decomposed by strong heating into silver metal and oxygen gas. 3) Methanol (CH3OH) is synthesized from carbon monoxide gas and hydrogen gas. 4) If iron (III) oxide is heated strongly in a stream of carbon monoxide gas, it produces elemental iron and carbon dioxide gas. Classifying Reactions 8 different types of reactions: 1. Precipitation reactions (aq) + (aq) (s) + (aq) or (l) AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) 2. Acid-base reactions --OH + H-- salt + H2O(l) NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) 3. Oxidation-reduction reactions uncombined element on one side is combined on the other side Fe2O3(s) + Al(s) Fe(l) + Al2O3(s) 4. Synthesis – one product N2 + O2 2NO 5. Decomposition – one reactant 2H2O 2H2 + O2 6. Combustion – O2 is a reactant, O adds to each element If C and H, then CO2 + H2O are the products CH4 + 2O2 CO2 + 2H2O Another way to classify: 7. Double displacement – “doubles” on both sides AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) 8. Single displacement – a “single” and a “double” on both sides Fe2O3(s) + Al(s) Fe(l) + Al2O3(s) Precipitation Reactions • Form a solid (s) on product side • Must have only (aq) on reactant side • The solid formed is NOT a strong electrolyte Pb(NO3)2(aq) + 2NaI(aq) PbI2(s) + 2NaNO3(aq) • Is the product a solid????? – Will NOT be solid if: •It contains a group I metal •It contains NH4+ •It contains NO3- Complete and balance the precipitation reactions: a) LiOH(aq) + MgS(aq) b) PbCl2(aq) + KBr(aq) Identify the precipitate (solid) in each case! Acid-Base Reactions • Also called neutralization reactions • Acids: they have H’s at the front, e.g. H2SO4 – Their function is to give their H’s away • Bases: they have OH’s at the end, e.g. Ba(OH)2 – Their function is to take the acids H’s and combine with their OH’s to make H2O • Strong bases are always aq, never solid: – Group I with OH •LiOH •NaOH •KOH •RbOH •CsOH - Certain Group II with OH - Ca(OH)2 - Sr(OH)2 - Ba(OH)2 Equations that show the dissociation: Strong acids -dissociate completely in water to produce H+ ions. HCl H+ + ClH2SO4 2H+ + SO42Strong bases - dissociate completely in water to produce OH ions. NaOH Na+ + OHBa(OH)2 Ba2+ + 2OH- Acid-Base Reactions • Always produce water and salt Salt = metal from base and leftovers from acid HNO3(aq) + KOH(aq) H2SO4(aq) + LiOH(aq) H3PO4(aq) + Ca(OH)2(aq) QUESTION In the balanced equation for the neutralization of sodium hydroxide with sulfuric acid, the products are: a) b) c) d) e) NaSO4 + H2O NaSO3 + 2H2O 2NaSO4 + H2O Na2S + 2H2O Na2SO4 + 2H2O ANSWER e) Na2SO4 + 2H2O Give the acid base reaction that will produce the following salts: a) K2SO4 b) CsNO3 • Sr(OH)2 + H3PO4 Redox Reactions • Oxidation-reduction (redox) – The oxidation number (charge) changes from reactant side to product side – Is a transfer of electrons – Element is alone on one side, but combined with other element(s) on the other side 2Mg + O2 2MgO H2O(l) H2(g) + O2(g) QUESTION Give the reaction type for each of the following reactions: Pb(NO3)2(aq) + 2NaI(aq) PbI2(s) +2Na(NO3)(aq) Na(s) + LiCl(aq) Li(s) + NaCl(aq) HClO3(aq) + KOH(aq) KClO3(aq) + H2O(l) ANSWER precipitation, redox, acid-base 3 more Reaction Types • Synthesis – one product N2 + O2 2NO • Decomposition – one reactant 2H2O 2H2 + O2 • Combustion – O2 is a reactant, CO2 + H2O are the products CH4 + 2O2 CO2 + 2H2O Another way to classify: – Double displacement AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) – Single displacement Fe2O3(s) + Al(s) Fe(l) + Al2O3(s) 1. CH4 + 2. SiO2 + O2 CO2 + H2O HF SiF4 + H2O H2 3. K + H2O 4. Fe + O2 5. NH3 + O2 + KOH Fe2O3 NO + H2O 1. H2SO4 2. Fe(CN)3 + 3. K3PO4 + + 4. CaCO3 Ca(OH)2 MgCl2 H2O CaO + CO2 CaSO4 FeCl3 H3PO4 + H2O + Mg(CN)2 + KOH Electrolytes Strong – break up into + and – in water NaCl Na+ + ClWeak – only a few molecules break up in water vinegar solution Non - no molecules break up in water sugar solution Strong Electrolytes • Compounds containing a group 1 metal • Compounds containing NH4+ • Compounds containing NO3• Strong acids • Strong bases The 7 Strong Acids • HCl • HBr • HI • HNO3 • H2SO4 • HClO4 • HClO3 The 8 Strong Bases • LiOH • NaOH • KOH • RbOH • CsOH • Ba(OH)2 • Sr(OH)2 • Ca(OH)2 Describing Reactions in Solution 1. Molecular equation (reactants and products as compounds) AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) 2. Complete ionic equation (all strong electrolytes shown as ions) Ag+ + NO3 + Na+ + Cl AgCl(s) + Na+ + NO3 Describing Reactions in Solution (continued) 3. Net ionic equation (show only components that actually react) Ag+ + Cl AgCl(s) Na+ and NO3 are spectator ions. Write the balanced net ionic equation for the following reaction: Pb(NO3)2(aq) + H2SO4(aq) PbSO4(s) + HNO3(aq) Give the molecular equation for Ni(NO3)2 + NaOH Give the net ionic equation for Ni(NO3)2 + NaOH Give the complete ionic equation for Ni(NO3)2 + NaOH What were the spectator ions in that equation?