a shorter, easier way to show chemical reactions, using symbols, not words, for the reactants and...
TRANSCRIPT
17-2 Describing Chemical Reactions
a shorter, easier way to show chemical
reactions, using symbols, not words, for the reactants and the
productshydrogen molecules react with oxygen molecules to form water molecules
H2 + O2 H2O
reactant + reactant “YIELDS” products
CHEMICAL EQUATION
Law of Conservation of Masstotal mass of reactants must equal total mass of products
matter is NOT destroyed or created in a chemical reaction
=
ELEMENTS – represented by a one or two-letter symbol (letter)
C Na HCOMPOUNDS– represented by a chemical formula
(word) which uses subscripts to show the ratio of elements in the
compound H2O2 CO2 C3H8OHOW MANY?
coefficient in front of the chemical formula tells “how many” atoms or molecules
3H2O2 4CO2 2C3H8O
Chemical Formulas & Counting Atoms
Balancing Chemical EquationsH + O H2O
• Continue adding coefficients to obtain the same number of atoms of each element on both sides of the equation(change coefficient, then change counts)
• Add the subscript “2” to all diatomics that are ALONE in the equation (N, O, F, Cl, Br, I, H)(note: only time a subscript can & must be changed)
• Count the number of atoms that are present in the basic equation and record
• Pick an element that is not balanced on both sides of the equation ( H & O last)
• Add a coefficient in front of the chemical formula to adjust the count and record the new values
Balancing Chemical EquationsMg + O MgO
• Continue adding coefficients to obtain the same number of atoms of each element on both sides of the equation(change coefficient, then change counts)
• Add the subscript “2” to all diatomics that are ALONE in the equation (N, O, F, Cl, Br, I, H)(note: only time a subscript can & must be changed)
• Count the number of atoms that are present in the basic equation and record
• Pick an element that is not balanced on both sides of the equation ( H & O last)
• Add a coefficient in front of the chemical formula to adjust the count and record the new values
C + Cl CCl4
Building Equations (basic equation is given)
Mg + O2 ------> MgO
C + Cl2 ------> CCl4
Building w/Marshmallows
Note: add like elements on the same side of the equation
Al + O2 Al2O3
SO2 + O2 SO3
Balancing Chemical Equations
• Continue adding coefficients to obtain the same number of atoms of each element on both sides of the equation(change coefficient, then change counts)
• Add the subscript “2” to all diatomics that are ALONE in the equation (N, O, F, Cl, Br, I, H)(note: only time a subscript can & must be changed)
• Count the number of atoms that are present in the basic equation and record
• Pick an element that is not balanced on both sides of the equation ( H & O last)
• Add a coefficient in front of the chemical formula to adjust the count and record the new values
Al + O Al2O3
SO2 + O SO3
Classifying Chemical EquationsSYNTHESIS – two or more substances combine to make a more complex substance
AB + C ABC (synthesize means to put together)
DECOMPOSTION - a complex substance breaks down into simpler substances
ABC AB + C (decompose means to break down)
REPLACEMENT – two elements in two different compounds trade places
AB + CD AC + BD (replace means to find a new partner)
Synthesis of Acid Rain2 SO2 + O2 + 2 H2O 2 H2SO4
Decomposition of Hydrogen Peroxide
Isolating Copper by Replacement
2 H2O2 2 H2O + O2
2 CuO + C 2 Cu + CO2
Synthesis, Decomposition, or Replacement