Steps to Writing Reactions Some steps for doing reactions 1. Identify the type of reaction 1. Predict the product(s) of the reaction 2. Write the correct.

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Presentation transcript:

Steps to Writing Reactions Some steps for doing reactions 1. Identify the type of reaction 1. Predict the product(s) of the reaction 2. Write the correct formula of the compounds 1. Balance the equation

Seven Diatomic elementsSeven Diatomic elements Have No Fear Of Ice Cold Beer! For example, Oxygen is O 2 as an element. H 2, N 2, F 2, O 2, I 2, Cl 2, Br 2 Memorize this list!

Notation used to show physical state of substances: (s) solid, such as metals (l) liquid, like water! (g) gas, like hydrogen (aq) aqueous, dissolved in water Memorize these!

Single replacement reactions

Single Replacement Reactions Single Replacement Reactions occur when one element replaces another in a compound. A metal can replace a metal (the positive ions trade places) OR a nonmetal can replace a nonmetal (the negative ion trades). element + compound element + compound A + BY AY + B (if A is a metal) OR X + BY BX + Y (if X is a nonmetal) (remember the cation always goes first!)

Activity Series:

Single Replacement Reactions

Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zn (s) + HCl (aq) ZnCl 2(aq) + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction 2

Single Replacement Reactions Sodium bromide solid reacts with chlorine gas NaBr (aq) + Cl 2(g) NaCl (aq) + Br 2(l) Note that chlorine replaces bromine in the compound Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq) Copper DOES NOT reaction with aqueous aluminum nitrate. Copper is below aluminum on the activity series. Cu (s) + Al(NO 3 ) 3(aq) 22 No Reaction

Alkali metals and alkaline earth metals: Most react with acid solutions to produce a salt and hydrogen gas. Ex: Mg (s) + HCl (aq) MgCl 2 + H 2(g) You try: Li (s) + H 2 SO 4(aq) Memorize the following acids: hydrochloric acid HCl Sulfuric acid H 2 SO 4 Nitric acid HNO 3 Phosphoric acid H 3 PO 4

Alkali metals and alkaline earth metals Many of them are active metals that react with water and produce a base and hydrogen gas: Ex: 2 Li (s) + 2 H2O (l) 2 LiOH (aq) + H 2(g) Hint: Water is HOH! You try: Ca (s) + HOH (l)

Alkali Metals and Alkaline Earth metals Active metals replace the metallic ions in solution to produce a salt and the other metal. Ex: Mg (s) + CuCl 2(aq) MgCl 2(aq) + Cu (s) Your turn: Mg (s) + ZnCl 2(aq)

Halogens: More active halogens replace less active halides in single replacement reactions. F > Cl > Br > I (The same order as the periodic table) Example: MgBr 2(s) + Cl 2(g) MgCl 2(s) + Br 2(l) Try: NaBr (s) + I 2(g) NO REACTION!

Practice 1. Mg (s) + H 2 SO 4(aq) 1. Au (s) + HCl (aq) 1. Zn (s) + CuSO 4(aq) 2. Cl 2(aq) + CaBr 2(aq) 1. Fe (s) + HNO 3(aq) 1. Na (s) + H 2 O (l)

Answers: Check your work! 1. Mg (s) + H 2 SO 4(aq) MgSO 4(aq) + H 2(g) 1. Au (s) + HCl (aq) No reaction 1. Zn (s) + CuSO 4(aq) Cu (s) + ZnSO 4(aq) 2. Cl 2(aq) + CaBr 2(aq) Br 2(aq) + CaCl 2(aq) 1. Fe (s) + 2 HNO 3(aq) H 2(g) + Fe(NO 3)2(aq) 1. 2 Na (s) + 2 H 2 O (l) 2 NaOH (aq) + H 2(g)

More practice – answers on the next slide. 1. Al (s) + H 2 SO 4(aq) 1. Ca (s) + HCl (aq) 1. Cu (s) + ZnSO 4(aq) 2. F 2(aq) + LiBr (aq) 1. Mg (s) + HNO 3(aq) 1. Ca (s) + H 2 O (l) 1. Cl 2(aq) + AlBr 3(aq)

1. 2Al (s) + 3 H 2 SO 4(aq) 2 H 2 (g) + Al 2 (SO 4 ) 3(aq) 1. Ca (s) + 2 HCl (aq) CaCl2(aq) + H 2(g) 1. Cu (s) + ZnSO 4(aq) no reaction 2. F 2(aq) + LiBr (aq) LiF (aq) + Br 2(aq) 1. Mg (s) +2 HNO 3(aq) Mg(NO 3 ) 2(aq) + H 2(g) 1. Ca (s) + 2 H 2 O (l) Ca(OH) 2(aq) + H 2(g) 1. Cl 2(aq) + AlBr 3(aq) AlCl 3(s) + Br2 (aq)