Pemantapan kimia kimia kimia aka bogorusu

Nnnn

1. General C hemistry “CHEMICAL REACTION”

2. Reaksi kimia Reaksi kimia = perubahan kimia (chemical change) Chemical Change: “A change which changes the chemical identity of the substance and creates one or more new substances“

3. Logam natrium bereaksi dengan air, menghasilkan gas hidrogen . Na + H 2 O  NaOH + H 2 ( belum setara ) Logam natrium bereaksi dengan air, menghasilkan gas hidrogen .

4. Larutan kalium iodida direaksikan dengan larutan timbel (II) nitrat . m enghasilkan endapan berwarna kuning

5. Negative Electrode Positive Electrode 2H 2 O 2H 2 + O 2

6. Chemical Equations Concise representations of chemical reactions

7. Anatomy of a Chemical Equation CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g )

8. Reactants appear on the left side of the equation. CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g ) Anatomy of a Chemical Equation

9. Products appear on the right side of the equation. Anatomy of a Chemical Equation CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g )

10. The states of the reactants and products are written in parentheses to the right of each compound Anatomy of a Chemical Equation CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g )

11. Coefficients are inserted to balance the equation. Anatomy of a Chemical Equation CH 4 ( g ) + 2 O 2 ( g ) CO 2 ( g ) + 2 H 2 O ( g )

12. Subscripts and Coefficients Give Different Information Subscripts tell the number of atoms of each element in a molecule

13. Subscripts and Coefficients Give Different Information Subscripts tell the number of atoms of each element in a molecule Coefficients tell the number of molecules

14. Reaksi kimia Reaksi redoks Reaksi non redoks BIL ANGAN OKS IDASI = ‘ Muatan ’ asumsi = elektron ikatan dibagi berdasarkan elektronegativitas H H ada perubahan biloks tidak ada perubahan biloks

15. H Cl +1 –1 reaksi redoks : reduksi oksidasi kenaikan biloks melepas elektron penurunan biloks menerima elektron reduktor : mereduksi = teroksidasi oksidator : mengoksidasi = tereduksi

16. LEO the lion says GER! GER! Contoh reaksi redoks : Zn + Cu 2+  Zn 2+ + Cu MnO 4  + S 2  MnO 2 + S IO 3  + HSO 3   I  + SO 4 2 ose lectrons xidation L E O ain lectrons eduction G E R

17. Asam – basa ( penetralan ) Pembentukan gas Pembentukan endapan Reaksi non redoks : NaOH + HCl  NaCl + H 2 O (l) AgNO 3 + KCl  AgCl (s) + KNO 3 Na 2 CO 3 + HCl 2 NaCl + H 2 O + CO 2 (g)

18. Manakah yg termasuk reaksi redoks dan non redoks KOH + H 3 PO 4  K 3 PO 4 + H 2 O CH 4 + Br 2  CBr 4 + HBr Pb ( NO 3 ) 2 + Na 2 SO 4  PbSO 4 + 2NaNO 3

19. REAKSI NON REDOKS

20. The Reaction of K 2 CrO 4 ( aq ) and Ba (NO 3 ) 2 ( aq )

21. Regular balanced equation or molecular equation: K 2 CrO 4( aq ) + Ba (NO 3 ) 2( aq )  BaCrO 4(s) + 2KNO 3( aq ) Complete ionic equation: 2K + ( aq ) + CrO 4 2- ( aq ) + Ba 2+ ( aq ) + 2NO 3 - ( aq )  BaCrO 4(s) + 2K + ( aq ) + 2NO 3 - ( aq ) Net ionic equation: (Ions participate in reaction) Ba 2+ ( aq ) + CrO 4 2- ( aq )  BaCrO 4(s)

22. MgCl 2 + 2AgNO 3  2AgCl + Mg( NO 3 ) 2

23. Write complete ionic and net ionic equations for each of the following molecular equations 2HClO 4 ( aq ) + Ca (OH) 2 ( aq )  Ca ( ClO 4 ) 2 ( aq ) + 2H 2 O ( l ) HC 2 H 3 O 2 ( aq ) + NaOH ( aq )  NaC 2 H 3 O 2 ( aq ) + H 2 O( l ) 2HNO 3 ( aq ) + Mg(OH) 2 ( s )  2H 2 O ( l ) + Mg( NO 3 ) 2 ( aq ) Pb ( NO 3 ) 2 ( aq ) + Na 2 SO 4 ( aq )  PbSO 4 ( s ) + 2NaNO 3 ( aq )

24. Write the molecular equation and the net ionic equation for each of the following aqueous reactions. If no reaction occurs, indicate this. a. FeSO 4 + NaCl  b. Na 2 CO 3 + MgBr 2  c. MgSO 4 + NaOH  d. NiCl 2 + NaBr  e. AgNO 3 + NaI  f. Ba( NO 3 ) 2 + K 2 SO 4  g . Mg( NO 3 ) 2 + K 2 SO 4  h . CaCl 2 + Al( NO 3 ) 3 

25. Acid–Base Reactions with Gas Formation

26. Na 2 CO 3 ( aq ) + 2HCl ( aq )  2NaCl ( aq ) + H 2 CO 3 ( aq ) Na 2 CO 3 ( aq ) + 2HCl ( aq )  2NaCl ( aq ) + H 2 O( l ) + CO 2 ( g ) Acid–Base Reactions with Gas Formation

27. Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. a. NaOH + HNO 3  b. HCl + Ba(OH) 2  c. HC 2 H 3 O 2 + Ca (OH) 2  d. NH 3 + HNO 3  e. Al(OH) 3 + HCl  f. HBr + Sr (OH) 2  g . Ba(OH) 2 + HC 2 H 3 O 2  h . HNO 3 + KOH 

28. REAKSI REDOKS

29. Balancing Redox Reactions MnO 4 - ( aq ) + Fe 2+ ( aq ) Acid Fe 3+ ( aq ) + Mn 2+ ( aq ) Half reactions: MnO 4 -  Mn 2+ (reduction) Fe 2+  Fe 3+ (oxidation) Balance half reactions: MnO 4 -  Mn 2+ Manganese is balanced Balance oxygen by adding 4H 2 O to the right side of the equation

30. c. Balance hydrogen by adding 8H + to the left side 8H + ( aq ) + MnO 4 - ( aq )  Mn 2+ ( aq ) + 4H 2 O Equalize the charge by adding electrons 5e - + 8H + ( aq ) + MnO 4 - ( aq )  Mn 2+ ( aq ) + 4H 2 O (l) Fe 2+ ( aq )  Fe 3+ ( aq ) + e - x 5 5 Fe 2+ ( aq )  5 Fe 3+ ( aq ) + 5e - Add half reactions : 5 Fe 2+ ( aq ) + MnO - 4( aq ) + 8H + ( aq )  5 Fe 3+ ( aq ) + Mn 2+ ( aq ) + 4H 2 O (l) Check that elements and charges are balanced.

31. Balancing Redox Reactions ClO - + CrO 2 -  Cl - + CrO 4 2- (basic solution) +1 +3 -1 +6 First half reaction: ClO - +2e -  Cl - ClO - + 2e -  Cl - + H 2 O ClO - + 2e - +2H +  Cl - + H 2 O Second half reaction: CrO 2 -  CrO 4 2- CrO 2 -  CrO 4 2- + 3e - CrO 2 - + 2H 2 O  CrO 4 2- + 3e - CrO 2 - + 2H 2 O  CrO 4 2- + 3e - + 4H +

32. Multiply first half reaction by 3 and second half reaction by 2 then add two half reactions. 3ClO - + 6e - + 6H +  3 Cl - + 3H 2 O 2CrO 2 - + 4H 2 O  2 CrO 4 2- + 6e - + 8H + 3ClO - + 2CrO 2 - + H 2 O  3 Cl - + 2 CrO 4 2- + 2H + Add OH - to both sides to remove H + 3ClO - + 2CrO 2 - + H 2 O + 2OH -  3 Cl - + 2 CrO 4 2- + 2H + + 2OH - 3ClO - + 2CrO 2 - + H 2 O + 2OH -  3 Cl - + 2 CrO 4 2- + 2 H 2 O 3ClO - + 2CrO 2 - + 2OH -  3 Cl - + 2 CrO 4 2- + H 2 O

33. Balancing redox reaction Fe(OH) 2 + H 2 O 2  Fe(OH) 3 + H 2 O in acid solution Al + NO 3   Al(OH) 4  + NH 3 ClO  + Mn(OH) 2  MnO 2 + Cl  MnO 4  + H 2 C 2 O 4  Mn 2+ + CO 2 in basic solution Cr 2 O 7 2  + H 2 C=O  HCOOH + Cr 3+ N 2 H 4 + Cu(OH) 2  N 2 + Cu

34. 5 Reaction Types Synthesis Decomposition Combustion Single Replacement Double Replacement

35. Synthesis Reactions Two substances react to form a single product. X + Y XY

36. 2 Mg ( s ) + O 2 ( g )  2 MgO ( s )

37. Decomposition Reactions A single reactant decomposes or breaks down into two or more products. A B + C (decomposition of a metal chlorate or metal carbonate are the most common)

38. Two Types of Combustion Reactions Incomplete combustion: C x H y + O 2 CO + H 2 Complete Combustion: C x H y + O 2 CO 2 + H 2 O

39. Examples: CH 4 ( g ) + 2 O 2 ( g )  CO 2 ( g ) + 2 H 2 O ( g ) C 3 H 8 ( g ) + 5 O 2 ( g )  3 CO 2 ( g ) + 4 H 2 O ( g )

40. Two Types of Single Replacement Reactions Single Replacement of a Halogen: Z 2 + AX AZ + X 2 Single Replacement of a Metal: M + AX MX + A

41. Fe (s) + CuSO 4 ( aq )  Fe SO 4 ( aq ) + Cu (s )

42. Double Replacement Reactions A reaction in which the cations and anions of both reactants switch partners. AX + DZ AZ + DX