1. WHAT DO ALL THESE THINGS HAVE IN COMMON?

2. Oxidation and Reduction+1 -1
2Na0 + Cl202NaCl O I L
Oxidation is loss of electrons or…
xidation s
osing
Na01e- + Na+1
(Half reaction)
Na is oxidized.

3. R I G 2Na0 + Cl202NaCl Cl0 + 1e-Cl-1 eduction s aining
Oxidation and Reduction +1 -1
2Na0 + Cl202NaCl R I G
Reduction is gain of electrons or…
eduction s
aining
Cl0 + 1e-Cl-1
(Half reaction)
Cl is reduced.

4. LEO says GER

5. 2Na0 + Cl202Na+1Cl-1 Secret Agent Man Cl Na R.A. O.A.
Here’s a little trick
Secret Agent Man
OIL
RIG
Oxidizing agent (O.A.) causes a particle to lose e- (by gaining e- itself)
Reducing agent (R.A.) causes another particle to gain e- (by losing e- itself) Cl Na
Particle
Oxidized
Particle
Reduced
R.A.
O.A.
2Na0 + Cl202Na+1Cl-1

6. 2Na0 + Cl202Na+1Cl-1
The particle oxidized and the particle reduced are
ALWAYS on the same side of the equation!
AND the oxidizing agent and reducing agent
are ALWAYS on the same side of the equation
OIL
RIG

7. So happy togetherrrrrr!
Oxidation and reduction always occur together

8. Ca + S Ca S Practice +2 -2 Ca S Ca S OIL RIG R.A. O.A. Then identify:+2 -2
OIL
RIG
Ca + S Ca S
R.A.
O.A.
1. Assign charges.
2. Particle oxidized ____ 3. Particle reduced ____
4. Oxidizing agent _____ 5. Reducing agent ____
Then identify: Ca
OIL S
RIG Ca
R.A. S
O.A.

9. Mg + Cl2 Mg Cl2 Practice -1 +2 Mg Cl Mg Cl OIL RIG R.A. O.A.
RIG +2
Mg + Cl2 Mg Cl2
R.A.
O.A.
Assign charges.
2. Particle oxidized ____ 3. Particle reduced ____
4. Oxidizing agent _____ 5. Reducing agent ____
Then identify: Mg
OIL Cl
RIG Mg
R.A. Cl
O.A.

10. Mg Cl2 Oxidation States -1 +2
Oxidation states indicates how many e- are gained, lost, or shared.
Oxidation states
Mg Cl2 +2 -1

11. Rules for Naming Oxidation States
1. In their compounds, the metals of Group 1A always have an oxidation number of +1, the charge on their ions
2. The oxidation number of fluorine (F) is - 1 when it is in a compound. +1 -1
NaBr
GIVE RULES SHEET AND RULES W.S.
HAVE THEM WORK ON RULES W.S. IN CLASS USING RULES AS REFERENCE
GO OVER W.S. QUICKLY
GO THROUGH RULES; STAR #1, #2, #5, #7 BECAUSE THEY ARE AN ALWAYS.
GIVE “OXIDATION STATES” WORKSHEET FOR HOMEWORK…START IN CLASS +1 -1
CuF

12. Rules for Naming Oxidation States
3. The oxidation number of a monatomic ion is equal to its charge.
Fe+3….Oxidation # = +3

13. Rules for Naming Oxidation States
4. The sum of the oxidation numbers of all the atoms in the formula of a compound is equal to zero.
5. In their compounds, the metals of group 2A always have an oxidation number of +2, the charge on their ions. +1 -2
K2Se
+1(2) + -2 = 0
= 0
K will always be +1 because it is in group 1 +2 -2
CaS
= 0

14. Rules for Naming Oxidation States
6. In compounds, the oxidation number of oxygen is almost always -2. (Exception: peroxides such as H2O2 or Na2O2 where oxidation number is -1 +1 -1 +1 -1
Na2O2
H2O2
2(+1) + 2(-1) = 0
= 0
2(+1) + 2(-1) = 0
= 0

15. Rules for Naming Oxidation States
7. The oxidation number of an atom of a free element is zero.
8. Hydrogen has an oxidation number of +1 in all compounds, except the metal hydrides, like LiH or CaH2, where oxidation number is -1.
Na Br20
HF KH +1 -1
Metal hydride

16. Rules for Naming Oxidation States
9. In combinations involving nonmetals, the oxidation number of the less electronegative element is positive and of the more electronegative element is negative. +2 -3 +4 -2
SO2
Fe3P2
+4 + 2(-2) = 0
= 0
3(+2) + 2(-3) = 0
= 0

17. Rules for Naming Oxidation States
10. The algebraic sum of the oxidation numbers of the atoms of a polyatomic ion is equal to its charge. -2 ( )
= the whole ion (S & 3 O’s) have a
charge of -2
SO3 -2
SO3 ( ) +4 -2
___ + -6 = -2 +4

18. Polyatomic Ions
Some covalently bonded groups of atoms act like single atoms in forming ions.
These charged groups of covalently bonded atoms are called radicals or polyatomic ions.
SULFITE: SO AMMONIUM: NH4+1
SULFATE: SO HYDRONIUM: H3O+1
CHLORITE: ClO HYDROXIDE: OH-1
CHLORATE: ClO CYANIDE: CN-1
CHROMATE: CrO PHOSPHATE: PO4-3

19. Practice: assign oxidation states (numbers).+2 -2 +1 -1
NaCl
MgS Al
ZnO H2
CrF2
+2 -2 = 0
+1 -1 = 0 +2 -2
1-3 on ws
+2 -2 = 0 +2 -1
+2 + 2(-1) = 0
+2 -2 = 0

20. Practice: Assign oxidation states (charges).+3 -2 +1 -1
Fe2O3
K2O2
NO2
HBr
SrH2
MnBr2
= 0
= 0 +2 -1 +1 -1
*Metal hydride
*peroxide
= 0
Do 7
= 0 +2 -1 +4 -2
= 0
= 0

21. Practice: assign oxidation states (charges).-2 +1 -2 +3
(OH) -1
(Cr2O4)-2
-2 + ___ = -1 +1
____ + 4 (-2) = -2
___ + -8 = -2 +6
2(___) + -8 = -2 +3 +2 -2
PRACTICE!
(S2O3)-2
___ + 3 (-2) = -2
___ + -6 = -2 +4
2(___) + -6 = -2 +2

22. Practice: assign oxidation states (charges).+1 +6 -2 ?
H2SO4
1(2) + 1x + 4(-2) = 0
2 + 1x + -8 = 0
1x + -6 = 0
Number 4 on sheet
1x = +6
x = +6
= 0
= 0

23. Practice: assign oxidation states (charges).+1 +7 -2
1(+1) + 1x + 4(-2) = 0
HClO4
K2Cr2O7
1 + 1x -8 = 0
= 0
1x = +7
x = +7 +1 +6 -2
2(+1) + 2x + 7(-2) = 0
PRACTICE!
= 0
2 + 2x -14 = 0
2x = +12
x = +6

24. Writing a Formula Al+3 S-2 Al2+3S3-2 = Al2S3 Rb+1 N-3 = Rb3+1N-3 Rb3N1
Write down elements with their oxidation numbers.
*More electronegative is written last.
Al+3 S-2
Al2+3S3-2 =
Al2S3
2(+3) + 3(-2)
+6 -6 = 0
Rb+1 N-3 =
Rb3+1N-3
Rb3N1
3(+1) + 1 (-3)
+3 -3 = 0

25. Polyatomic Ions in Compounds
Potassium + chlorite
Calcium + chromate
Magnesium + hydroxide
K+1 & (ClO2)-1 = KClO2
+1 -1 = 0
Ca+2 & (CrO4)-2 = CaCrO4
+2 -2 = 0
Mg+2 & (OH)-1 = Mg(OH)2
*Leave polyatomic in parenthesis!
+2 + 2(-1) = 0

26. Writing Chemical Formulas
Li+1I-1
LiI
Li and I
K and P
Rb and C
Li and Cr2O7-2
K+1P-3
K3P
PRACTICE
Rb+1C-4
Rb4C
Li+1(Cr2O7)-2
Li2Cr2O7

27. CHEMICAL REACTIONS & EQUATIONS

28. Chemical Reactions

29. Chemical Reactions
Process in which one or more substances are converted into new substances with different physical and chemical properties
For example, a yellow solid precipitate, lead iodide (PbI2), forms from the mixture of two clear liquids, potassium iodide (KI) and lead nitrate (Pb(NO3)2).

30. Word Equation
Hydrogen + Oxygen
Water + Energy
Reactants
Products

31. Balanced Formula Equations2
H2 (g) + O2 (g) 1 2
H2O (l)
Why?
To give a quantitative, as well as qualitative information.

32. 2H2 (g) + 1O2 (g)
2H2O (l)
2 Molecules Water
2 Molecules H + 1 molecule O +
2 Moles H2 + 1 Mole O2
2 Moles Water
4 g
32 g +
36 g

33. Rules for Balancing Equations
1. Write correct formulas for all reactants and products.
Use the symbols for elements: Iron = Fe
Don’t forget diatomic elements travel in pairs!
H2, N2, O2, F2, Cl2, Br2, I2

34. Rules for Balancing Equations
2. Obey the LAW OF CONSERVATION OF MASS.
Same number of each kind of atom on both sides of the equation.
25g +
25g +
50 g
50 g +
150 g ?g

35. How to Balance an Equation
3. To balance atoms of reactants and products, change ONLY the coefficients.
4. Do NOT change the chemical formula to balance numbers of atoms.
Numbers IN FRONT of the formulas
NOTE: Subscripts are lower numbers in formula
4 Al2O3
Coefficient
Subscripts

36. How to Balance an Equation cont.
5. Check your work by counting atoms of each element.
6. Check to see that the coefficients are in the lowest whole number ratio.
2H2O (l)
2H2 (g) + 1O2 (g)
4 Hydrogen
4 Hydrogen
2 Oxygen
2 Oxygen

37. Practice Balancing These Equations2 1 2
Ca O2
CaO
1 Ca
1 Ca
2 O
1 O
*Hint: Start by making the uneven side even.
2 O
2 O
1 Ca
2 Ca
2 Ca
2 Ca
2 O
2 O
2 Ca, 2 O
2 Ca, 2 O

38. Practice 1 1 2 2 CH4 + O2 CO2 + H2O 2 O 3 O 4 O 4 O 1 C 1 C 4 H 4 H
*Hint: Start with the element that is split up: Oxygen.
Then, make uneven side even.
2 O
3 O
4 O
4 O
1 C
1 C
4 H
4 H
1 C, 4 H, 4 O
1 C, 4 H, 4 O

39. Practice 2 Fe + Cl2 FeCl3 2 1 3 1 Fe 1 Fe 2 Cl 3 Cl 6 Cl 6 Cl 1 Fe

40. Practice 2 1 HgO Hg + O2 2 1 2 3 3 Al + MnO Al2O3 + Mn 2 Al, 3 Mn, 3 O
Br NaI
NaBr I2
2 Br, 2 Na, 2 I
2 Br, 2 Na, 2 I
Do these on own 2 1
HgO
Hg O2 2
2 Hg, 2 O
2 Hg, 2 O

41. Coefficients Must Be in Lowest WHOLE Number!2 4 2 1 2
21/2 5 1
C2H O2
CO H2O
What number can you multiply 21/2 by to get
the smallest whole number? 2!
So, multiply the whole equation by 2 to get a properly
balanced equation.
4 C, 4 H, 10 O
4 C, 4 H, 10 O

42. You try. Multiply by 2! 8 C, 2O H, 26 O 8 C, 2O H, 26 O 4 1 2 13 8
61/2 10
C4H O2
CO H2O 5
Multiply by 2!
8 C, 2O H, 26 O
8 C, 2O H, 26 O

43. Classification of Chemical Reactions
1. Synthesis
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Combustion (burning)

44. A B AB Synthesis Examples: 1 Cu + O2 2 CuO 1 H2CO3 CO2 + H2O
Two reactants combine to form a single product (compound). A B AB
One Product
Examples: 1 2
Cu O2
CuO 1
H2CO3
CO H2O

45. AB A B Decomposition Examples: 2 3 KClO3 KCl + O2 1 2 H2O2 H2O + O2
One reactant breaks down to form two or more products. AB A B
One Reactant
Examples: 2 3
KClO3
KCl O2 1 2
H2O2
H2O O2

46. A BC AC B Single Replacement Examples: 2 1 Mg + HCl MgCl2 + H2 2 1
One element replaces another from a compound A BC AC B
Examples: 2 1
Mg + HCl
MgCl H2 2 1
Cl KI
KCl I2

47. Double Replacement (ionic)
Ions in a solution combine to form a product that leaves the scene of the reaction AB CD AD CB
Example:
AgNO3 (aq) + NaCl (aq)
AgCl (s) + NaNO3 (aq)

48. More on Double Replacement
Precipitate (s), gas (g) or water (H2O) will form
AgNO3 (aq) + NaCl (aq)
AgCl (s) + NaNO3 (aq)
Actual reaction:
AgCl
Ag+1 + Cl-1
Don’t dwell (do it in depth later)
Spectator Ions:
Na+1 & NO3-1

49. What happens when you put
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens when you put
AgNO3 and NaCl in water?

50. NaCl
AgNO3

51. NaCl
AgNO3

52. AgNO3
NaCl

53. AgNO3
NaCl

54. AgNO3
NaCl

55. AgNO3
NaCl

56. AgNO3
NaCl

57. Ag NO3
Na Cl

58. Ag+
NO3-
Na+
Cl-

59. Ag+
NO3-
Na+
Cl-

60. Ag+
NO3-
Cl-
Na+

61. NO3-
Ag+
Na+
Cl-

62. NO3-
Na+
Ag+
Cl-

63. NO3-
Na+
Ag+
Cl-

64. NO3-
Na+
Cl-
Ag+

65. Na+
NO3-
Cl-
Ag+

66. Na+
NO3-
Cl-
Ag+

67. Na+
NO3-
Ag+
Cl-

68. Na+
NO3-
Ag+
Cl-

69. Na+
NO3-
Ag+
Cl-

70. Na+
NO3-
Ag+
Cl-

71. NO3-
Na+
AgCl

72. Na+
NO3-
AgCl

73. Na+
NO3-
AgCl

74. Na+
NO3-
AgCl(s)
precipitate
AgCl

75. Na+
NO3-
AgCl(s)
precipitate
AgCl

76. Na+
NO3-
AgCl

77. NO3-
Na+
AgCl

78. NO3-
Na+
AgCl

79. Na+
NO3-
AgCl

80. Na+
NO3-
AgCl

81. Na+
NO3-
AgCl

82. Na+
NO3-
AgCl

83. Na+
NO3-
AgCl

84. Na+
NO3-
AgCl

85. AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
AgNO3
AgNO3
NaCl

86. AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
AgNO3
AgNO3
NaCl

87. AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
AgNO3
AgNO3
NaCl

88. AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
NaCl
NaCl
NaCl
AgNO3
AgNO3
AgNO3
AgNO3
NaCl
Ag+
Na+
NO3-
Cl-

89. AgNO3
NaCl
NaCl
NaCl
AgNO3
NaCl
AgNO3
Ag+
Na+
NO3-
Cl-
Ag+
Cl-
NO3-
Na+
Na+
Ag+
NO3-
Cl-
AgCl

90. Ag+
Na+
NO3-
Cl-
Cl-
Cl-
Na+
Ag+
NO3-
NO3-
Ag+
Na+
NO3-
Ag+
Cl-
Na+
NO3-
Cl-
NO3-
Na+
Cl-
Na+
Ag+
Ag+
Cl-
Ag+
Cl-
Cl-
Ag+
Ag+
AgCl
AgCl
AgCl

91. Ag+
NO3-
Cl-
Ag+
NO3-
Na+
Ag+
Cl-
NO3-
Na+
NO3-
Ag+
Cl-
NO3-
NO3-
Na+
Cl-
Na+
Na+
Cl-
Ag+
Ag+
Na+
NO3-
Cl-
NO3-
Na+
Na+
Na+
Cl-
Ag+
AgCl
AgCl
AgCl
AgCl

92. Ag+
NO3-
Cl-
NO3-
Na+
NO3-
NO3-
Na+
Ag+
NO3-
NO3-
Cl-
Na+
Na+
Na+
Cl-
Ag+
Ag+
NO3-
Cl-
Na+
Na+
Na+
NO3-
Na+

93. NO3-
NO3-
Na+
NO3-
NO3-
Na+
NO3-
NO3-
Na+
Na+
Na+
Cl-
Ag+
Ag+
NO3-
Cl-
Na+
Na+
Na+
NO3-
Na+

94. NO3-
NO3-
Na+
NO3-
NO3-
Na+
NO3-
NO3-
Na+
Na+
Na+
Cl-
Ag+
Ag+
NO3-
Cl-
Na+
Na+
Na+
NO3-
Na+

95. NO3-
Na+
Na+
NO3-
Na+
NO3-
NO3-
NO3-
Na+
Na+
Na+
NO3-
NO3-
Na+
NO3-
Na+
Na+

96. NO3- Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+
AgCl(s)

97. NO3- Na+ Na+ NO3- Na+ NO3- NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ NO3-
AgCl(s)

98. NO3- Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+
AgCl(s)

99. Combustion (burning) Produces light and heat CxHy+ O2 CO2 + H2O
Balance C 1st, then H, then O (because it splits up) 3 1
C3H O2 5
CO H2O 4 1 2
C2H2+ O2 2 4
CO H2O 2 1
2.5 5

100. Classification of Equations
SYNTHESIS AB A B Ca S
CaS
DECOMPOSITION AB A B
2HgO
2Hg O2

101. Classification of Equations
SINGLE
REPLACEMENT AB C A BC
2KCl
Br2
Cl2
2KBr
DOUBLE
REPLACEMENT AB CD AD CB
CaSO4
BaCl2
CaCl2
BaSO4

102. Putting it all together
1. Assign the charges.
2. Write the correct formulas.
3. Balance the equation.
4. Identify the type of reaction.
BEFORE this they balance equation sheet (see star) then go back and ID type of equation
Iron (II) sulfide + Hydrochloric acid
Iron (II) chloride + Hydrogen sulfide

103. 1. Write the ions and element symbols
Iron (II) sulfide + Hydrochloric acid
Iron (II) chloride + Hydrogen sulfide
Fe+2S-2
+ HCl
Fe+2Cl-1
+ H+1S-2

104. 2. Rewrite the correct formula.
Fe+2S-2 + HCl
Fe+2Cl-1 + H+1S-2
FeS
+ HCl
FeCl2
+ H2S

105. 4. Identify the type of reaction.
3. Balance the equation. 1
FeS + HCl
FeCl H2S 2 1 1
4. Identify the type of reaction.
Insist on them writing oxidation states BEFORE formula.
Double Replacement!

106. Try this one. Ca0 + HCl Ca+2Cl-1 + H20 1 + HCl Ca CaCl2 + H2 2 1 1
1. Assign the charges.
2. Rewrite the correct formulas.
3. Balance the equation.
4. Identify the type of reaction.
Calcium + Hydrochloric acid
Calcium chloride+ Hydrogen
Ca0
+ HCl
Ca+2Cl-1
+ H20 1
+ HCl Ca
CaCl2 H2 2 1 1
Single Replacement!

107. Try this one. Zn+2 (OH)-1 Zn+2O-2 + H2O Zn(OH)2 ZnO + H2O 1 1 1
1. Assign the charges.
2. Rewrite the correct formulas.
3. Balance the equation.
4. Identify the type of reaction.
Zinc hydroxide
Zinc oxide+ water
Zn+2
(OH)-1
Zn+2O-2
+ H2O
Zn(OH)2
ZnO H2O 1 1 1
Maybe stop here and go on own with worksheet (depend on how they handle it).
Decomposition!

108. Try this one. N20 + O20 N+2O-2 1 N2 + O2 NO 1 2 Synthesis! Nitrogen
1. Assign the charges.
2. Rewrite the correct formulas.
3. Balance the equation.
4. Identify the type of reaction.
Nitrogen
Nitrogen oxide
+ Oxygen
N20
+ O20
N+2O-2 1
N O2 NO 1 2
Synthesis!

109. Activity Series of the Elements: Table LLi Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H2 Sb Bi Cu Hg Ag Pt Au
Nonmetals F2 Cl2 Br2 I2
Replaces H
from acids
Replaces H
from water
Most Active
Most Active
Least Active
Least Active
Metals replace metals or H
Nonmetals replace nonmetals
*REPLACE FROM OWN COLUMN

110. Making Predictions: Single Replacement Rxn
1. Assign the charges and predict products.
2. Rewrite correct formulas.
3. Use activity series to tell if rxn occurs and why.
4. Balance equation.
Pepsi commercial
Aluminum + Nickel (II) chloride ?

111. 1. Assign the charges and predict products.
Aluminum + Nickel (II) chloride ?
Al0
+ Ni+2Cl-1
Al+3Cl-1
+ Ni0
2. Rewrite correct formulas. Al
+ NiCl2
AlCl3
+ Ni

112. 3. Use the activity series to tell if the rxn occurs and why.
Yes, Al is more active than Ni. 2 Al
NiCl2 3 2
AlCl3 Ni 3
4. Balance equation.

113. Now try this one. Ca0 + Co+3(NO3)-1 Ca+2(NO3)-1 + Co0 3 3 Ca(NO3)2 Ca
1. Assign the charges (for compounds) and predict products.
2. Rewrite correct formulas.
3. Use activity series to tell if rxn occurs and why.
4. Balance equation.
Calcium + Cobalt (III) nitrate ?
Ca0
+ Co+3(NO3)-1
Ca+2(NO3)-1
+ Co0 3 3
Ca(NO3)2 Ca Co 2
+ Co(NO3)3 2
Yes, Ca is more active than Co.

114. Now try this one. Br20 + Rb+1I-1 Rb+1Br-1 + I20 2 1 2 RbBr + I2 1 Br2
1. Assign the charges (for compounds) and predict products.
2. Rewrite correct formulas.
3. Use activity series to tell if rxn occurs and why.
4. Balance equation.
Bromine + Rubidium Iodide ?
Br20
+ Rb+1I-1
Rb+1Br-1
+ I20 2 1 2
RbBr I2 1
Br2
RbI
Yes, Br is more active than I.

115. Making Predictions: Double Replacement Rxn
Double Replacements will only complete when one or more of these events occur:
1. Water forms (H2O)
2. A gas forms (g)
3. A precipitate (s) forms
Do “Chapter 9 Double Replacement Reactions” first two together, rest on own.

116. Let’s try a couple Does the reaction occur? Does the reaction occur?
Ba(OH)2 (aq) + H2SO4(aq)
BaSO4(aq) + H2O(l)
Does the reaction occur?
YES; water is formed.
What are the spectator ions?
(The ions not involved in forming water, gas, or precipitate)
Ba+2 & SO4-2
Ca3(PO4)2(aq) + NaNO3(aq)
Na3(PO4)2(aq) + CaNO3(aq)
Does the reaction occur?
No; no water, gas or
precipitate is formed.

117. Potassium chromate + copper(II) hydroxide
1. Assign the charges and predict products.
Rewrite correct formulas and look up states of products on Table C.
K+1 (CrO4)-2
+ Cu+2(OH)-1
Cu+2(CrO4)-2
+ K+1(OH)-1
K2 (CrO4)
+ Cu(OH)2
Cu(CrO4)
(s)
+ K(OH)
(aq)
insoluble
on Table C
soluble
on Table C

118. Does a precipitate (s) form? 1 2
Potassium chromate + copper(II) hydroxide
3. Balance equation.
4. Does reaction occur?
Does water form?
Does a gas (g) form?
Does a precipitate (s) form? 1 2
K2CrO Cu(OH)2
CuCrO4 (s) KOH (aq) NO
Do “Double Replacement Reactions” predicting
Then single and double replacement reactions predicting NO
YES! THE RXN OCCURS!