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Agenda
• Atoms and the Periodic
table Jeopardy
• Notes: Chemical
Equations and Reactions
• Molecular models
• Model and Change Quiz
tomorrow

Bell Work
• Draw both the Bohr
model and the Lewis dot
model of the following:
–
–
–
–
–

Aluminum
Carbon
Arsenic
Argon
helium
Chemical Equations and
Reactions
April 2, 2013
Objectives
1. Explain the difference between
elemental and chemical formula
2. Recognize all the parts of a chemical
equation
3. Describe how compounds are different
than the materials that compose it
4. Balance Chemical Equations
Chemical Bonding
The attraction between two atoms that
holds them together
Chemical changes occur because of breaking and
rearrangement

Chemical change = chemical reaction
Chemical Equation
To show chemical reactions we use
chemical equations

C + O2 --> CO2
4 Al (s) + 3 O2 (g) ---> 2 Al2O3 (s)
Parts of Chemical Equation
Elemental formula: how atoms are
bounded together in an element



Li
O2 , N2 , S8
Chemical formula: representation
of a compound, when atoms of
different elements bond to each other


NaCl, NH3 , CO2
Subscript:
represents how
many of a
particular atom
Coefficient:
represents how
many of a
particular element
or molecule
(s) represents solid
(l) represents liquid
(g) represents gas
(aq) represents aqueous
How many atoms?
C + O2 --> CO2

4 Al (s) + 3 O2 (g) ---> 2 Al2O3 (s)
Chemical Equation
Reactants --> Products
C + O2 --> CO2
when reading an equation Arrow = yields
Law of Conservation of Mass
Matter is neither created nor destroyed
during a chemical reaction
Therefore all chemical equations must be
balanced; equal atoms of each element on
each side
Balancing equation rules
You may change the coefficients in front
You may NOT change the subscripts
Changing the subscript changes the
compound
Steps of balancing
1. Write the correct formulas for the
equation. Once written do not change
the formula’s
2. Find the number of atoms on the left side
of each element and compare it against
the number of atoms of the same
elements on the right side
4. Check your answer to see if:

The numbers of atoms on both
sides of the equation are now
balanced.
 The coefficients are in the lowest
possible whole number ratios.
(reduced)
Helpful hints
Take one element at a time working left to
right,
Leave H for next to last and O last
IF everything balances except for O, and
there is no way to balance O with a whole
number, double all the coefficients and try
again.
Balancing Equations
___ H2(g) + ___ O2(g) ---> ___ H2O(l)
One of the oxygen atoms
binds with two of the
hydrogen atoms
Done Activities
Which equations are balanced?
Balance the ones that aren’t
a.Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
b. Al(s) + Br2(l)  Al2Br6(s)
c. HgO(s)  Hg(l) + O2(g)
___ Al(s) + ___ Br2(l) ---> ___ Al2Br6(s)
____C3H8(g) + _____ O2(g) ---->
_____CO2(g) + _____ H2O(g)
____B4H10(g) + _____ O2(g) ---->
_____B2O3(g) + _____ H2O(g)

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Chemical reactions

  • 1. Agenda • Atoms and the Periodic table Jeopardy • Notes: Chemical Equations and Reactions • Molecular models • Model and Change Quiz tomorrow Bell Work • Draw both the Bohr model and the Lewis dot model of the following: – – – – – Aluminum Carbon Arsenic Argon helium
  • 3. Objectives 1. Explain the difference between elemental and chemical formula 2. Recognize all the parts of a chemical equation 3. Describe how compounds are different than the materials that compose it 4. Balance Chemical Equations
  • 4. Chemical Bonding The attraction between two atoms that holds them together Chemical changes occur because of breaking and rearrangement Chemical change = chemical reaction
  • 5. Chemical Equation To show chemical reactions we use chemical equations C + O2 --> CO2 4 Al (s) + 3 O2 (g) ---> 2 Al2O3 (s)
  • 6. Parts of Chemical Equation Elemental formula: how atoms are bounded together in an element   Li O2 , N2 , S8
  • 7. Chemical formula: representation of a compound, when atoms of different elements bond to each other  NaCl, NH3 , CO2
  • 8. Subscript: represents how many of a particular atom Coefficient: represents how many of a particular element or molecule
  • 9. (s) represents solid (l) represents liquid (g) represents gas (aq) represents aqueous
  • 10. How many atoms? C + O2 --> CO2 4 Al (s) + 3 O2 (g) ---> 2 Al2O3 (s)
  • 11. Chemical Equation Reactants --> Products C + O2 --> CO2 when reading an equation Arrow = yields
  • 12. Law of Conservation of Mass Matter is neither created nor destroyed during a chemical reaction Therefore all chemical equations must be balanced; equal atoms of each element on each side
  • 13. Balancing equation rules You may change the coefficients in front You may NOT change the subscripts Changing the subscript changes the compound
  • 14. Steps of balancing 1. Write the correct formulas for the equation. Once written do not change the formula’s 2. Find the number of atoms on the left side of each element and compare it against the number of atoms of the same elements on the right side
  • 15. 4. Check your answer to see if:  The numbers of atoms on both sides of the equation are now balanced.  The coefficients are in the lowest possible whole number ratios. (reduced)
  • 16. Helpful hints Take one element at a time working left to right, Leave H for next to last and O last IF everything balances except for O, and there is no way to balance O with a whole number, double all the coefficients and try again.
  • 17. Balancing Equations ___ H2(g) + ___ O2(g) ---> ___ H2O(l) One of the oxygen atoms binds with two of the hydrogen atoms
  • 18. Done Activities Which equations are balanced? Balance the ones that aren’t a.Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) b. Al(s) + Br2(l)  Al2Br6(s) c. HgO(s)  Hg(l) + O2(g)
  • 19. ___ Al(s) + ___ Br2(l) ---> ___ Al2Br6(s)
  • 20. ____C3H8(g) + _____ O2(g) ----> _____CO2(g) + _____ H2O(g) ____B4H10(g) + _____ O2(g) ----> _____B2O3(g) + _____ H2O(g)