Chapter+6+Resources

1) Guide to Reading Chapter 6 Chemical Reactions – Part 1   Answer in complete sentences. =  2) Chapter 6 NOTES  =
 * 1) Why do we need to balance equations?
 * 2) Once the formulas of reactants and products are known, how do you adjust the number of atoms needed to follow the “Law of Conservation of Mass?”
 * 3) Explain the difference between the use of a coefficient and a subscript.
 * 4) How is the state of each compound in a chemical equation indicated?
 * 5) What substances must always be written as diatomic molecules?

Chemical Reactions
= Evidence of Chemical Change  = == o   Atoms of reactants are rearranged to bond with different atoms. == == o   What evidence of chemical reactions have you observed? Physical States == == o   Use symbols to indicate the physical states of reactants and products:  ==

 o  States are written after the chemical formulas.
= Atom INVENTORY  =

 o  The element symbols do not change  –  Why not?
== o   The total number of atoms in the reactants must match the number of atoms in the products. == == o   The total mass of all reactants is the same as the total mass of all products. ==

= Law of Conservation of Matter  = == o   Atoms are neither created nor destroyed in a chemical reaction. ==

= Words to Formula  =

== o   Once the formulas are written correctly, you may not change the subscripts. == = Writing Formulas  =

 o  Learn the 7 diatomic elements.
== o   Look for clues about the states of matter in the word problem. == = COEFFICIENTS  = == o   Make a list of all of the atoms in reactants and count the total atoms present. ==

 o  Compare the count to those atoms present in the products.
== o   Now adjust the reactants and products by trying COEFFICIENTS. == = H2 (g) + O2 (g) H2O(l)  = = Chlorine gas is bubbled into an aqueous solution of potassium bromide to produce bromine and aqueous potassium chloride. =

3) Chapter 6 Homework problems # 33 & 37