Reaction Types (P.99-117) 14%

Front 1

Chemical Reaction

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-defined as a process by which one or more substances are changed into one or more new substances.
Reactant ---> Product

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Synthesis Reaction (Type of Chemical Reaction) 1/6

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-a reaction in which two or more elements or compounds combine to form a single product.
-Ex: A+B--> C
-For example:
2Na+CL = 2NaCl

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Decomposition Reaction (Type of Chemical Reaction) 2/6

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-a reaction in which a single reactant , a compound, breaks into two or more parts.
-Ex: AB--> A + B
-For example:
2H(2)O-->2H+O

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Single Replacement or Displacement Reaction (Type of Chemical Reaction) 3/6

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-in this reaction, a more active element replaces a less active element in a compound.
-Ex: A+BC-->AC+B
-For example:
Cu+2AgNo-->2Ag+Cu(No)

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Double Replacement or Displacement Reaction (Type of Chemical Reaction) 4/6

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-in this reaction, two compounds react to form two new compounds. The formation of a molecular compound such as water, the formation of a gas, or the formation of a precipitate usually drives these reactions.
-Ex: AB+CD-->AD+CB
-For example:
Pb(No)+2KI-->2KNO+PbI

Front 6

Combustion Reaction (Type of Chemical Reaction) 5/6

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-in this type of reaction, often a hydrocarbon is burned in the presence of oxygen gas to form carbon dioxide (in a complete combustion) or carbon monoxide (in an incomplete combustion, due to a limited amount of oxygen).
-Ex: C(x)H(y)+O(2)
--->CO(2)+H(2)O(I)

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Hydrolysis Reaction (Type of Chemical Reaction) 6/6

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-A reaction that involves water.
-Ex: X(aq)+H(2)O(I)<-->HX(aq)+OH(aq)

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Net Ionic Equation

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-are equations that show only the soluble, strong electrolytes reacting (these are represented as ions) and omit the spectator ions, which go through the reaction unchanged.

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Net Ionic Equation Solubility Rules (p. 103):

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*1.) Most alkali metal compounds and NH(4) compounds are soluble.
2.) Cl, Br, I compounds are soluble, except when they contain Ag, Hg, or Pb.
3.) F compounds are soluble, except when they contain group 2A metals.
*4.) NO, CIO, CIO, and CHCOO compounds are soluble.
5.) SO compounds are soluble, except when they include Ca, Sr, Ba, Ag, Pb, or Hg.
6.) CO, PO, CO, CRO, S, OH, AND O compounds are insoluble.
7.) Group 2A metal oxides are classified as strong bases even though they are not very soluble.

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Rule about Common Reaction Types:

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-If an insolubel precipitate or gas an be formed ina areaction, it probably will be.
-Oxides (except group 1A) are insoluble, aned when reacted with water, they form either acids (nonmetal oxides) or bases (metal oxides).
-There are six strong acids that completely ionize: HCI, HBr, HI, HNO(3), H(2)SO(4), HCIO(4). All other acids are weak and are written together, as molecules.
-The strong bases that ionize are oxides and hydroxides of group 1A and 2A metals. All other oxides and hydroxides are considered weak and written together, as molecules.

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Conjugate Acid-Base Pairs

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-are compounds that differ by the presence of one proton, or H+. All acids have a conjugate base, which is formed when their proton has been donated; like-wise, all bases have a conjugate acid, formed after they have accepted a proton.

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Example Of Conjugate Acid-Base Pairs

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HX(aq)+H(2)O(I)<->X(aq)+H(3)O(aq)
-When the forward reaction occurs, HX donates a proton to water (so it acts as the base) to form hydronium. When the reaction occurs, the hydronium ion acts as the acid, donating a proton to the X. Together, HX and X are said to be conjugate acid-base pairs.

Front 13

Relative Strengths of Acids and Bases

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-Certain acids are stronger than other acids, and some bases are stronger than others. WHat this means is that some acids are better at donating a proton, and some bases are better proton acceptors. A STRONG acid or base dissociates or ionizes completely in aqueous solution. A WEAK acid or base does not completely ionize.

Front 14

Strong Acids

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-There are six acids that you'll need to memorize:
1. Hydrohalic acids: HCI, HBr, HI
2. Nitric Acid: HNO(3)
3. Sulfuric Acid: H(2)SO(4)
4. Perchloric Acid: HCIO(4)

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Strong Bases

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-Hydroxides (-OH), oxides of 1A and 2A metals (except Mg and Be), H-, and CH(3).

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Autoionization

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-in solution, a water molecule can even donate a proton to or accept a proton from another water molecule, and this process is called autoionization.

Front 17

Ion-Product Constant
1 x 10 (^-14)

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-At 25C, the value of K(w), which is known as the ION-PRODUCT CONSTANT, is 1x10(^-14).
-This means that the [H(3)O+]=[OH-] and each is equal to 1x10(-7). When the concentrations of H+ and OH- are equal in a solution, the solution is said to be neutral. In acidic solutions, the concentration of H+ is higher than that of OH-, and in basic solutions, the concentration of OH- is greater than that of H+.

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pH

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-The pH of a solution is calculated as the negative logarithm in base 10 of the hydronium ion concentration-it is an expression of the molar concentration of H+ ions in solution:
pH=-log[H+] or -log[H(3)O+]
-A solution like the equilibrium expression for water, which is neutral at standard temperature, would have a pH of:
pH=-log[1x10(-7)]=-(-7.00)=7.00
-If the solution contains more hydronium ions than this neutral solution ([H+]>1x10(-7)), the pH will be less than 7.00, and the solution will be acidic; if teh solution contains more hydroxide ions than this neutral solution ([OH-]>1x10(-7)), the pH will be greater than 7.00, and the solution will be basic.
-Similarly, the pOH of a solution is calculated as the negative logarithm in bas 10 of the hydroxide ion concentration:
pOH=-log[OH-]
-pH and pOH are related to each other by the equation:
pH+pOH=14
-Calculated the hydronium ion concentration of a solution:
[H(3)O+]=10(-pH)

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Question: Is the salt formed in this particular reaction: Neutral, Acidic, or Basic?
(What are the 3 Factors?)

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1.) Which acid reacted with which base to form this salt?
2.) Was the acid strong or weak?
3.) Was the base strong or weak?

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Redox and Electrochemistry: Oxidation-Reduction

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-reactions that involve the transfer of electrons b/w substances. They take place simultaneously, which makes sense b/c if one substance loses electrons, another must gain them. Many of the reactions we've encountered thus far fall into this category. For example, all single-replacement reactions are redox reactions.

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Electrochemistry (Oxidation-Reduction) 1/7

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-the study of the interchange of chemical and electrical energy.

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Oxidation (Oxidation-Reduction) 2/7

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-the loss of electrons. Since electrons are negative, this will appear as an increase in the charge (Zn loses two electons; its charge goes from 0 to +2). Metals are oxidized.

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Oxidizing Agent (OA) (Oxidation-Reduction) 3/7

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-the species that is reduced and thus causes oxidation.

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Reduction (Oxidation-Reduction) 4/7

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-the gain of electrons. When an element gains electrons, the charge on the element appears to decrease, so we say it has a reduction of charge (Cl gains one electron and goes from an oxidation number of 0 to -1). Nonmetals are reduced.

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Reducing Agent (RA) (Oxidation-Reduction) 5/7

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-the species that is oxidized and thus causes reduction.

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Oxidation Number (Oxidation-Reduction) 6/7

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-The assigned charge on an atom. You've been using these numbers to balance formulas.

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Half-Reaction (Oxidation-Reduction) 7/7

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-An equation that shows either oxidation or reduction alone.

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Redox Reaction

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-a reaction is considered a redox reaction if the oxidation numbers of the elements in teh reaction change in teh course of teh reaction. We can determine which elements undergo a change in oxidation state by keeping track of the oxidation numbers as the reaction progresses.

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Rules for Assigning Oxidation States

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1.) The oxidation state of an element is ZERO, including all elemental forms of the elements (e.g., N(2), P(4), S(8), O(3)).
2.) The oxidation state of a monatomic ion is the same as its charge.
3.) In compounds, fluorine is always assigned an oxidation state of -1.
4.) Oxygen is usually assigned an oxidation state of -2 in its covalent compounds. Exceptions to this rule include peroxides (compounds containing the O group), where each oxygen is assigned an oxidation state of -1, as in hydrogen peroxide (H(2)O(2)).
5.) Hydrogen is assigned an oxidation state of +1. Metal hydrides are an exception: in metal hydrides, H has an oxidation state of -1.
6.) The sum of the oxidation states must be zero for an electrically neutral compound.
7.) For a polyatomic ion, the sum of the oxidation states must equal the charge of teh ion.

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Standard Reduction Potential (E°)

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-The potential of a voltaic cell as a whole will depend on the half-cells that are involved. Each half-cell has a known potential, called its Standard Reduction Potential (E°). The cell potential is a measure of teh difference b/w the two electrode potentials, and the potential at each electrode is calculated as the potential for REDUCTION at the electrode.

Front 31

Electrolytic Cells

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-while voltaic celsl harness the energy from redox reactions, electrolytic cells can be used to drive nonspontaneous redox reactions, which are also called ELECTROLYSIS REACTIONS. Electrolytic cells are used to produce pure forms of an element; for example, they're used to seperate ores, in electroplating metals (such as applying gold to a less expensive metal), and to charge batteries (such as car batteries).
-These types of cells rely on a battery or any DC source-in other words, whereas the voltaic cell IS a battery, the electrolytic cell NEEDS a battery.
-Unlike voltaic cells, which are made up of two containers, electrolytic cells have just one container. However, like in voltaic cells, in electrolytic cells electrons still flow from the anode to the cathode.
-Diagram on p.117