Handouts

Notes 24
1/24/12 -- Full Handout

IS9 23 notes
11/16/11 --

IS9 23 notes

I. Chemical Changes  (23.1/721-5)

 

 

A. Chemical Reactions

1. Change one or more substances into new substances

 

2. Reactant + reactant = product

3. Reactant = product + product

B. Conservation of Mass

•           Mass remains constant in a chemical reaction.

•           Mass is neither created, nor destroyed.

C. Chemical Equations

•          Chemical symbols (Mg, O)

•          Chemical formulas (MgO)

 

3. Coefficients – numbers of each element or molecule on each side of the reaction

4. Subscripts – small, lower numbers showing the number of atoms in each molecule in it’s formula

II.  Chemical Equations (23.2/726-9)

A. Overview:

•    Mg  + O2           MgO + Energy

•    Magnesium + Oxygen = Magnesium Oxide

•    Balanced:

     2 Mg  + O2        2 MgO + Energy

 

B. Balanced: Same # of atoms of each element in the reactants as in the products

C. Balancing Chemical Equations

1. Same # of atoms on each side of equation:

Step one

2. Mg + O2        MgO

     Mg 1           Mg 1

     O 2             O  1

Step two

2. Mg + O2        2 MgO

     Mg  1           Mg 2

     O 2             O 2

Step three

2. 2 Mg + O2        2 MgO

      Mg 2                                              Mg 2

       O 2                         O 2

 

•            Samples:

Li + H2O à LiOH + H2

Fe + O2 à FeO

Fe + Cl2 à FeCl3

 

4. AM p728  (Ignore the “aq” & “s”. )

III. Classifying Chemical Reactions

(23.3/730-3)

A. Synthesis

•           2 or more simple substances react to form a new more complex substance

•            2 Na + Cl2          2 NaCl

B. Decomposition

•           A complex substance breaks down into 2 or more simpler substances.

•             2 H2O           2 H2 + O2

C. Single-Replacement

•            An uncombined element replaces an element that is part of a compound.

•             2 Na + 2H20               2 NaOH + H2

•            Each Na replaced one H

D. Double-Replacement

•           Different atoms in two compounds replace each other.

•             MgCO3 + 2 HCl           MgCl2 + H2CO3

IV. Reaction Rates & Energy

(23.4/774-740)

A. Energy Exchanges

•           Bonds use and release energy

•           Activation energy – energy needed to start a reaction

B.  Exergonic Reactions

•           Energy is released (usually in the form of heat and/or light)

  • Exothermic - releases heat

•           Ex. burning of methane gas

•           Draw diagram, p 738

C.  Energonic Reactions

•           Energy is absorbed (usually heat or light)

  • Endothermic - absorbs heat

•           Ex. instant ice packs

•           Draw diagram, p 736

D. Kinetics

•   – study of reaction rates (how quickly reactants turn into products)

effected by:

temperature

pH

concentration

agitation (stirring)

surface

pressure

catalyst/inhibitors

 1 more check book...

Full Handout

Class Rules 2011-2012
8/31/11 --

 Integrated Science (IS9) & OGT

Mrs. Massie        August 2011

Full Handout

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