2.  A process by which one or more substances are changed into one or more different substances. Reactants  Products

3. NaHCO 3(s) + HCl (aq)  NaCl (aq) + H2O (l) + CO 2(g)  Yield sign (s) Solid (l) Liquid (g) Gas (aq) aqueous (dissolved in water)

4.  Nitrogen gas and oxygen gas react to produce dinitrogen pentoxide.  2 N 2 (g) + 5 O 2 (g)  2 N 2 O 5

5.  Potassium reacts with water to form potassium hydroxide and hydrogen gas.  2 K + 2 H 2 O  2 KOH + H 2(g)

6.  Synthesis (Combination)  Decomposition  Single Displacement (Single Replacement)  Double Displacement (Double Replacement) ◦ Neutralization  Combustion

7.  Also known as Combination  Two substances (usually elements) comvine to form a new compound.  A + B  AB  2 Ca(s) + O 2 (g )  2 CaO(s)

8.  A compound breaks into its component parts  AB  A + B  2 NaCl  2 Na(s) + Cl 2 (g)

9.  Also known as Single Replacement  An element replaces an anion or a cation of a compound.  A + BC  B + AC  A + BC  C + BA  Mg(s) + H 2 SO 4 (aq)  MgSO 4 (aq) + H 2 (g)

10.  Also known as Double Replacement  Cations from two compounds exchange partners  AB + CD  AD + CB  BaCl 2 (aq) + Na 2 SO 4 (aq)  BaSO 4 (g) 2 NaCl(g)

11.  An acid and a base react to form a salt and water. ◦ Cation from base pairs with anion from acid to form a salt. ◦ Hydroxide from base pairs with hydrogen from acid to form water.  This is also a Double Displacement (Replacement)  HX + YOH  H 2 O + YX  HCl(aq) + NaOH(aq)  H 2 O(l) + NaCl(aq)

12.  Also known as oxidation ◦ Oxygen is a reactant ◦ Products always contain carbon dioxide and water ◦ Typically produces heat  C x H y O z + O 2  CO 2 + H 2 O  CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(g )

14.  Will nickel replace hydrogen from water? ◦ NO  Will lithium replace hydrogen from water? ◦ YES  Will lead replace hydrogen from steam? ◦ NO  Will magnesium replace hydrogen from steam? ◦ YES  Will silver replace hydrogen from acids? ◦ NO  Will sodium react with oxygen to form oxides? ◦ YES

15.  Will potassium replace zinc within a compound? ◦ YES  Will lead replace aluminum within a compound? ◦ NO  Will gold replace lithium within a compound? ◦ NO  Will iron replace copper within a compound? ◦ YES

16.  Using what you know about types of reactions and the activity series, you can predict products for a reaction.  Ex: ◦ Li + AgNO 3  ◦ Na + MgSO 4  LiNO 3 + Ag Mg + Na 2 SO 4

17.  Barium chloride reacts with silver nitrate ◦ Type of reaction: Double Displacement ◦ BaCl 2 + Cu(NO 3 ) 2  Ba(NO 3 ) 2 + CuCl 2  Aluminum oxide decomposes ◦ Type of reaction: Decomposition ◦ Al 2 O 3  Al + O 2 ◦ 2 Al 2 O 3  4 Al + 3 O 2

18.  If compounds are soluble, they have the ability to dissolve.  If they dissolve, they dissociate or “break apart” into their ions.  Ex: ◦ NaCl  Na +1 + Cl -1 ◦ BaF 2  Ba +2 + 2 F -1

19.  2 AgNO3 + H 2 S  Ag 2 S + 2 HNO 3  Q: How many moles of Ag 2 S will be produced from 3.5 moles of AgNO 3 ?  What happens if grams is involved? ◦ Use Molar Mass! 1.75 mol Ag 2 S

20. Q: How many grams of Ag 2 S will be produced from 3.5 moles of AgNO 3 ? A balanced chemical equation tells the mole:mole ratio between different compounds in the equation.

21.  If you are given information about one substance and asked about a different substance, it is a stoichiometry problem.

22.  What is the mass of Mg(OH) 2 that will react with 1.20g of HCl? Mg(OH) 2 + HCl  MgCl 2 + H 2 O 2 2 0.956g Mg(OH) 2