1. Chemical Reactions
Basic
Chemistry
i wonder why
Physical Science

2. In your lab notebook, please answer as best you can:
1. What are the horizontal rows of the Periodic Table called? What do the elements
in each row have in common?
• Elements in each “period” have the same number of occupied energy levels
(and some shared chemical and physical properties).
2. What are the vertical columns of the Periodic Table called? What do the
elements in each column have in common?
• Each “group” of elements has the same number of valence electrons.
3. Which class of elements contains mostly gasses and elements that are dull and
brittle?
• Nonmetals
4. What group(s) of elements are most likely to donate electrons (become cations)?
• Alkali Metals (group 1) and Alkaline Earth Metals (group 2)
4. What chemical properties to the Noble Gasses (group 18 elements) have?
• Full valence electron energy levels, very stable/unreactive (inert)
Bonus Question: How many elements are liquid at room temperature (72o
F)? Can
you name them?
Review
Quiz 5
Two: Mercury (Hg) & Bromine (Br)
* Gallium (Ga) and Caesium (Cs) are liquid at 85 degrees Farenheit

4. Reading The Periodic Table
- Review
• What is this and what does it tell you?
• the atomic number
• # of protons (& electrons)
• What is this number and what does tell you?
• the atomic mass (in amu's)
• Average weight of combined protons & neutrons
• Calculate the # of neutrons by subtracting the atomic number from
the rounded atomic mass
• What is this called?
• atomic symbol (abbreviation of element name)
• allows easier written chemical formulas
• H2O2, CO2, C6H12O6
• Describe an electron.
• Carries a negative charge.
• Very tiny - has virtually no mass.
• Orbits around the nucleus in energy levels.
Review

5. Chemical Bonding
- Ionic, Covalent, Metallic
Review

6. Electronegativity
- how strong an atom tends to pull on other electrons
Advanced
Topic

7. Electronegativity
• Electronegativity is a measure of how strong an atom tends to pull on
electrons of other nearby atoms.
• Highly electronegative elements tend to
form anions by stealing electrons
from atoms with very low
electronegativity.
Advanced
Topic

8. Chemical Reactions
• A chemical reaction occurs when two or more substances
interact to form new substances
• reactants: the substances that interact in a chemical reaction
• products: the new substances formed due to the chemical reaction
reactants products
• H2 + Cl2 2HCl 2H2 + O2 2H2O
reactants
product
• a diatomic molecule is a
molecule made of two atoms
hydrogen (g) + chlorine (g) hydrochloric acid (l) hydrogen (g) + oxygen (g) water (l)

9. Conservation of Mass & Energy
• Matter (made of atoms) cannot be created or destroyed.
• Law of Conservation of Mass
• During chemical reactions, changes will occur, but
• No atoms will ever cease to exist
• No atoms can ever come from nothing
• Atoms can only be rearranged into
different forms or substances
•Also true for energy
•Energy cannot be created or destroyed.
• Change forms (see picture)
• Move from one place to another

10. Evidence of a Chemical Change
• A chemical change may be indicated by:
• A new color forming
• Change in temperature (gets warmer or cooler)
• Bubbles or precipitate
• (evidence that a substance with a different state of matter is forming)
• Release of energy
• Sound, light, and/or heat
Review
Also

11. Experiment 5.2
Reaction Rates
(a.k.a. Kool Colors)
Observation:
• How do you know a reaction is finished?
•Name some fast/slow reactions you know about:
• FAST: explosions, fire, vinegar/baking soda
• SLOW: rusting, photosynthesis, decomposing food,
bread rising (yeast)
Conclusion:
• Did the color change (reaction) happen faster in cold,
room temp, or hot Koo-Aid? Why do you think that is?
• What patterns do you notice between different groups
(different flavors)?
• What differences in color change were there between
different flavors of Kool-Aid?

12. Balancing Chemical Equations
• What do you notice about reactants & products in
this reaction?
• Fe + Cl2 = FeCl3
• total # of iron atoms in the reactants: 1
• total # of chlorine atoms in reactants: 2
• To make it equal on both sides, coefficients are
added to balance the equation.
• 2 Fe + 3 Cl2 = 2 FeCl3
• Let's try another one:
• C6H12O6 + O2 = CO2 + H2O
ferric chloride
Advanced
Topic

13. Steps to Balancing an Equation
Step 1
Identify reactants & products and write their
chemical formulas on the appropriate sides of
the equation.
Step 2
Count the number of atoms of each element
on each side of the equation. (use a table to
keep track)
Step 3
Try coefficients that will balance the equation.
- Start with elements that appear only once
on each side of the equation.
- Never change the subscripts in a
chemical formula.
Step 4
Check to be sure you have the same number
of atoms of each element on both sides of the
equation.
• Example: Balance the equation that takes place when sodium
hydroxide reacts with sulfuric acid to form sodium sulfate and water.
Advanced
Topic

14. More Practice
• Balance the equation that takes place when methane gas reacts
with oxygen to form carbon dioxide and water.
Step 1: CH4 + O2 CO2 + H2O
Step 2:
Step 3: CH4 + 2 O2 CO2 + 2 H2O
Step 4:
Element Before After
C 1 1
H 4 2
O 2 3
Element Before After
C 1 1
H 4 4
O 4 4

15. Reaction Rates
• Collision Theory: substances cannot react unless their particles come
in contact with one another
• The more they collide, the more likely they'll react (faster rate)
• The slower the particles move, the less likely they'll collide and thus react
(slower rate)
Factors affecting the rate of reaction:
Concentration
• More reactants per volume increases the
number of particle collisions
Temperature
• Heat makes particles move faster
Surface Area
• A spread-out solid increases the chances
for liquid or gas to come in contact with it
Catalysts
• Lower the energy needed to get a reaction
started (activation energy)
Temperature & Surface Area Demo

16. Types of Chemical Reactions
• Synthesis: two or more substances combine to form a new substance
• A + B  AB
• examples: photosynthesis, formation of rust and table salt
• Decomposition: one substance breaks down into two or more simpler
substances
• AB  A + B
• examples: rotting leaves, electrolysis of water
• Combustion: a substance combines with
elemental oxygen and produces heat
• C 3H8 + 5 O2 3 CO2 + 4 H2O
• examples: burning wood, coal or gas, fireworks
• Displacement: an atom in a compound is replaced by a different atom
• A + BC  B + AC
• useful for separating a particular element from a compound
• examples: silver from silver nitrate Cu + 2 AgNO3  Cu(NO3)2 + 2 Ag
Single Displacement Example
Advanced
Topic