1. Unit 7 Chemical Reactions

2. Physical Vs. Chemical Change Physical changes= changes in form (phase), but not the identity of the substance ex: H 2 O (s)  H 2 O (l) (* Starts as H 2 O and ends as H 2 O) Chemical Change = Covalent/ ionic bonds break between reactants, producing new products. ex: H 2 O (l)  H 2 (g) + O 2 (g)

3. Bonds: Chemical Vs. Physical Physical Change Strong bonds (covalent) between atoms break & recombine in new combinations Weak bonds (hydrogen) break between molecules Chemical Change

4. Indicators of a Chemical Rxn 1)Light/ heat are produced 2)Color Change 3)Formation of a precipitate (solid) 4)Production of a gas

5. Importance of a Chemical Equation Ex: HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l) Symbols used in Chemical Equations (s) = solid (l) = liquid (g) = gas (aq) = aqueous, a.k.a. dissolved in water → = yields/ results ↔ = reversible reaction = Reactions are heated There are many more symbols used too! ReactantsProducts  It’s a chemical sentence describing a chemical or physical change

6. The charcoal used in a grill is basically carbon. The carbon reacts with oxygen to yield carbon dioxide. C + O 2  CO 2,

7. Naming & Formula Writing for Ionic and Covalent compounds Pgs 203-215

8. Writing & Naming Ionic Formulas 1)Write the charges above the symbols for the ions 2) “Swap & Drop” the charges 3) Formula = MgCl 2 Name: Magnesium Chloride (first element’s name + second element’s name with ending changed to “ide” Mg 1 2+ Cl 2 -1 (use periodic table to determine the charge or reference sheet on back of table) ex: Mg 2+ Cl -1 (Write the cation first)

9. Dealing with Transition Metals Many transition metals form more than one ion (see reference sheet on back of periodic table for this information) Fe 2+ = iron (II) Fe 3+ = iron (III) ex: Fe 2+ & Cl -1 = FeCl 2 Name= Iron (II) chloride Ex: Fe +3 & Cl -1 = FeCl 3 Name: Iron (III) chloride

10. Formulas & Naming (w/ Polyatomic Ions) Show formula for: Al bonded with SO 4 Al +3 SO 4 -2 Formula = Al 2 (SO 4 ) 3 Name: Aluminum sulfate (SO 4 ) = polyatomic ion -acts as an ion, but has more than one atom

11. Formula Writing & Naming Covalently Bonded Substances PrefixMeaning mono1 di2 tri3 tetra4 penta5 hexa6 hepta7 octa8 nona9 deca10 Prefixes used in Covalently bonded molecules

12. Naming Rules Example: N 2 O 5 dinitrogen pentoxide Less electronegative element first –Use prefix if more than one atom More electronegative element second –Prefix of the number of atoms Drop (o) or (a) at end of prefix if element name begins with a vowel –Root name –Ending –ide

13. Summary: Naming/ formulas NOTES: Type IType IIaType IIbType IIc Who’s Bonding?2 non-metalsMetal + non-metal Transition metal + non-metal Metal (usually) + Polyatomic Ion Example of formula & name N 2 O 3 Dinitrogen trioxide CaCl 2 Calcium chloride CuBr 2 Copper (II) Bromide Ca(NO 3 ) 2 Calcium Nitrate Name 1 st element? Prefix (except if only one) + full name Full Name Full name + roman numeral Full name + roman numeral (if need) Name the 2 nd element?Prefix + -ide ending + -ide endingRoot + -ide ending Name polyatomic based on back of periodic table Special rules for this type? Use pre-fixes: 1: mono- 2: di- 3: tri- 4: tetra 5: penta 6: hexa- 7:hepta- 8: octa- 9:nona- 10: deca- “Swap & Drop” -Write Ion charges -Swap & drop the numbers - Write as a formula: Ca Cl 2 - Same as Ia, except: - Transitional metals can have more than one cation EX: Cu 1+ or Cu 2+ (See back of Periodic Table to know) - Use roman numerals to indicate the cation - Same as Ia & Ib except: -Some groups of elements form “polyatomic ions” -NO 3 = nitrate -The whole unit has a charge: (NO 3 ) 1-

14. Diatomic Molecules Some elements are never found as a single atom, they bond with themselves. Here is the list of the 7 diatomic molecules: H 2, N 2, O 2 (the ”gens”) F 2, Cl 2, Br 2, I 2 (the aka halo”gens”) Ex: hydrogen reacts with oxygen to produce water Formula: H 2 + O 2  H 2 O (notice it’s not H + O  H 2 O)

15. Types of Chemical Reactions

16. There are 5 types of chemical reactions : 1.Synthesis reactions 2.Decomposition reactions 3.Single replacement reactions 4.Double replacement reactions 5.Combustion reactions You need to be able to identify the type of reaction and predict the product(s)

17. Synthesis A + B  AB Ex: 4Fe + 3O 2  2Fe 2 O 3

18. Decomposition AB  A + B Example: CaCO 3  Ca + CO 3

19. Single Replacement A + BC  AC + B Example: Mg + 2HCl  MgCl 2 + H 2

20. Double Replacement AB + CD  AD + CB Example: Pb(NO 3 ) 2 + 2 KI  PbI 2 + 2 KNO 3

21. Combustion Reactions C x H y + O 2  CO 2 + H 2 O + Energy Example: CH 4 + 2O 2  CO 2 + 2H 2 O + Energy

22. Balancing Chemical Equations

23. Law of Conservation of Matter Matter can not be created or destroyed during chemical reactions “what goes in must come out”

24. Law of Conservation of Matter # of atoms that go in a chemical reaction MUST come out” Unbalanced EX: C 6 H 12 O 6 + O 2  CO 2 + H 2 O 6 C’s go in & only 1 C comes out (H’s and O’s don’t add up either!) Not possible!  We balance chemical equations to adhere to the Law of conservation of matter. EX: C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O (now it’s balanced) -

25. Balancing Equations (Coefficients vs Subscripts) When balancing, you can only add coefficients in front of the compounds (NEVER change the subscripts) 3H 2 0 Coefficient (3) tells the number of molecules Subscript (2) tells the number of atoms of each element What this says: 3 molecules of water 6 atoms of hydrogen 3 atoms of oxygen Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or sharing for covalent)

26. Steps to balancing chemical equations: 1)Balance one element at a time. Working left to right, find the number of atoms for each element on the left side and compare those against the number of the atoms of the same element on the right side. Helpful hint: Never start by balancing the H’s or O’s. Save H for next to last and O until last. 2)Place coefficients in front of formulas so that the left side has the same number of atoms as the right side. Helpful hint: Polyatomic ions that appear on both sides of the equation should be balanced as independent units 3) Double check your math to make sure you’ve balanced everything correctly.

27. Balancing Equations Ex 1: ___ H 2 O(l) ---> ___ H 2 (g) + ___ O 2 (g) 22 Ex 2: __C 2 H 4 (g) + __ O 2 (g)  __CO 2 (g) + __H 2 O(g) 222 Ex 3: ___ Al(s) + ___ Br 2 (l) ---> ___ Al 2 Br 3 (s) 32 4 Ex 4: __ ZnCl 2 + __Fe 2 (SO 4 ) 3  __ FeCl 3 + __ZnSO 4 3 32 Ex 5: __ Ca + __H 2 O  __ Ca(OH) 2 + __H 2 2 Ex 6: CH 4 O + O 2  CO 2 + H 2 O

28. Predicting Products & Will Reaction Work?

29. Steps to Predicting Products 1.Identify the type of reaction 2.Write down all the atoms and their charges below the problem (do not write down subscripts unless it’s a polyatomic ion. Subscripts change from reactants side to products side) 3.Predict the product (s) using the type of reaction as a model and write the products with the charges. 4.Do swap and drop to find formulas of products (Don’t forget about the diatomic elements! For example, Oxygen is O 2 as an element.) 5.Balance it

30. Synthesis A + B  AB Example: Fe + O 2  -Write charges for each reactant: Fe +3 O 2- -Write product, swap and drop: Fe 2 O 3 -Balanced equation: 4Fe + 3O 2  2Fe 2 O 3

31. Decomposition AB  A + B Example: CaCO 3  -Break up the reactant into the 2 ions that make it up: Ca 2+ CO 3 2- -Write them as products -Balance equation: CaCO 3  Ca + CO 3

32. Single Replacement A + BX  AX + B Example: Mg + HCl  -Write the charges for each ion Mg +2 H + Cl - -If there is a lone cation, swap it with the cation in the compound. MgCl 2 -If there is a lone anion, swap it with the anion in the compound -Write the new lone cation or anion H 2 (diatomic) -Balance the equation Mg + 2HCl  MgCl 2 + H 2 Hint: When H 2 O splits into ions, it splits into H + and OH - (not H+ and O -2 !!)

33. Double Replacement Example: Pb(NO 3 ) 2 + KI  Pb +2 NO 3 -1 + K + I -  #2 switch partners so that + and – are together #1 Write the charges for each ion (not the subscript unless it’s a polyatomic) #3 Swap and drop to get correct formulas for products: PbI 2 KNO 3 AX + BY  AY + BX #4 Write as products and balance equation Pb 2+ I -1 + K +1 NO 3 -1 Example: Pb(NO 3 ) 2 + 2 KI  PbI 2 + 2 KNO 3

34. Combustion C x H y + O 2  CO 2 + H 2 O + Energy Example: CH 4 + O 2  -The reactants are always a carbon, hydrogen compound and oxygen -The products are always carbon dioxide, water and energy -Balance equation CH 4 + 2O 2  CO 2 + 2H 2 O + Energy

35. Predicting Products Practice Zinc metal reacts with aqueous hydrochloric acid Zn (s) + 2 HCl (aq)  ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) Note that fluorine replaces chlorine in the compound

36. Will a Reaction Occur? 3 reactions ALWAYS work: –Combustion, Synthesis, and Decomposition Single replacement & Double replacement reactions do not always work. - You need more information for each type of reaction to know for sure if a reaction will take place. Just because a reaction works out on paper, does not mean it would actually happen in a test tube.

37. Single replacement reactions and the Activity Series  You need the Activity Series chart to determine if a single replacement reaction will occur Ex #1 : Will this reaction happen? Mg + HCl  ???? Mg must be able to replace H… can it?  Find Mg and H on the chart  Mg is higher (Stronger) than H (weaker) and so Mg replaces H.  YES, Reaction will occur * Elements on top can replace all those below in a reaction Mg + 2HCl  MgCl 2 + H 2

38. Single Replacement Reactions Practice Problems Will this reaction occur? Mg + NaCl  ??? Mg is trying to kick out Na… can it? -Na is higher on the chart than Mg so Na will not be kicked out by Mg. We write: Mg + NaCl  NO REACTION

39. Will Double Replacement Reactions Occur? YES, if at least one of the products is a solid (aka precipitate). (or H 2 O) AX + BY  AY (s) + BX (s) YES AX + BY  AY (s) + BX (aq ) YES AX + BY  AY (aq) + BX (aq) NO  You need a “Solubility Table” to know what state the products will be in.  Use solubility rules: Soluble – dissolved in water (aq) Insoluble - a solid precipitate (s)

40. Solubility Table The study of quantities of materials consumed and produced in chemical reactions.

41. Double Displacement Practice Problems Will this Reaction Occur? Pb(NO 3 ) 2 + 2KI  PbI 2 + 2KNO 3 Need to look up products on the chart to determine if either of them is a solid –PbI 2 = solid (insoluble) –KNO 3 = aqueous Answer: Pb(NO 3 ) 2 (aq) + 2KI (aq)  PbI 2 (s) + 2KNO 3 (aq) Reaction will occur because 1 solid in products

42. Reversible Reactions Ex: H 2 O + CO 2 H 2 CO 3 Symbol for a reversible reaction Reversible reactions can proceed in both the forward and reverse directions Equilibrium= When the forward and the reverse reactions occur at the same rate

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