Vocabulary Week 17!!
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reactants
products
synthesis
decomposition
combustion
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shibboleth
propitiate
chortle
unremitting
inure
Remember…
• Nuclear reactions
• Chemical reactions
involve changes
involve changes with
with atom’s
atoms’ electrons
nucleus
• Reactants
–Starting
substances in a
reaction
–Arrow points away
from reactants
+
• Products
–Substances
formed during a
reaction
–Arrow points to
products

Chemical Reactions
Types
1. Synthesis
2. Decomposition
3. Single
displacement
4. Double
displacement
5. Combustion
Synthesis
• Two or more substances react to produce
one product
A + B  AB
2Na + Cl2  2NaCl
Decomposition
• Single reactant breaks down into two or more
products
AB  A + B
2 NaN3 → 2 Na + 3 N2
Sodium azide decomposes
into nitrogen gas and is
used in air bags.
Single Displacement
• Atoms of one element replace the atoms of
another element in a compound
A + BX  AX + B
Mg + 2HCl  MgCl2 + H2
Tums is used to neutralize
stomach acid
Double Displacement
• Exchange of positive ions between substances
AX + BY  BX + AY
CaCO3 + H2SO3  H2CO3 + CaSO4
Double
Replacement
• Marble can
become
eroded by
acid rain.
Calcium
sulfate, a
product,
leaves a white
coating on the
statue.
Combustion
• Oxygen combines with a substance and
releases energy (and usually products include
carbon dioxide and water)
A + O2  CO2 + H2O + bi-products
C8H18 + O2  CO2 + H2O + energy
Type of
Reaction
Example
Synthesis
A + B  AB
Decomposition
AB  A + B
Single Replacement
A + BX  AX + B
Double Replacement
AX + BY  AY + BX
Combustion
A + O2  CO2 + H2O + products
Changes in Matter
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Evidence of chemical reaction:
1.
2.
3.
4.
5.
6.
Gas is produced
Color Change
Change in smell
Formation of solid—precipitate
Light is produced
Temperature change
-exothermic
-endothermic
• Some reactions occur in water
• When a solid substance is
dissolved in water it is an
aqueous solution (aq)
Reactivity Series
• Helps determine if a reaction
will occur
• If the single element is higher
on the list  yes a reaction will
occur
• If the single element is lower
on the list  NO REACTION
A + BX  AX + B
Al + PbNO3 
Most Active
Lithium
Rubidium
Potassium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Iron
Nickel
Tin
Lead
Copper
Silver
Platinum
Gold
1. Al (s) + PbNO3 (aq) 
2. Cu (s) + MgSO4 
3. Al (s) + SnPO4(aq) 
4. Zn (s) + K3PO4(aq) 
5. Fe (aq) + KCl (aq) 
6. Mg (s) + NaNO3 (aq) 
7. Zn (s) + CuCl2 (aq) 
8. Na (s) + Au(OH)2 (l) 
9. Zn (s) + Cu(NO3)2 (aq) 
10. Fe (s) + Ni(ClO3)2 (aq) 
11. Au (s) + CaSO4 (aq) 
12. Mg (s) + LiBr (aq) 
13. Ni (s) + CaSO4 (aq) 
14. Al (s) + KClO2 (aq) 
15. Mn (s) + Na3PO4 (l) 
16. Al (s) + Sn(NO3)2 (aq) 
17. Ag (s) + PbCl4 (aq) 
18. Zn (aq) + FeI3 (aq) 
19. K (s) + Cu(ClO3)2(aq) 
20. Pb (s) + Au3(PO4)2 (aq) 
Law of Conservation of Mass
• Mass/matter can not be created nor destroyed
• Atoms you start with (reactants) must still be
there when you end (products)
• This is called balancing the equation
• Mass Reactants = Mass Products
Mg + 2HCl  MgCl2 + H2
• Big numbers = Coefficients
–can change
• Small numbers = Subscripts
–DO NOT CHANGE, if you
change you no longer have the
same substance
Steps to balancing equations
1. Write formulas for all compounds (sometimes
it is given)
2. Separate Reactants and products by a line
3. Count how many atoms of each element are
present on the reactant and the product side
(element inventory)
4. Change coefficients so that element inventory
is balanced
5. Simplify coefficients
6. Check work
Al
+
C3H8 +

O2
O2

Al2O3
CO2 +
H2O
KNO3

O2 +
CS2 
KNO2
+
CO2
O2
+ SO2
Cu +
Cu
+
H2O 
Cl2
CuO

+
CuCl2
H2
Al(NO3)3+ NaOH  Al(OH)3 + NaNO
Fe + H2SO4 
Fe2(SO4)3 +
H2
KOH +
Al
+
HBr 
KBr +

Al2S3
S8
H2O
Al(OH)3 +
H2CO3
Al2(CO3)3 + H2O
Al(OH)3 +
HBr 
AlBr3 +
H2O
Vocab Week 18!
Last one this semester!
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single displacement
double displacement
reactivity series
precipitate
aqueous
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obsequious
moribund
winnow
flaccid
rife
Na +
NaNO3 
Li
AlCl3 
+
Na2O +
LiCl +
Al
N2
NH3
FeS2
+
+
HCl 
O2

NH4Cl
Fe2O3
+
SO2
sodium hydroxide 
sodium oxide + water
sodium reacts with water to produce sodium
hydroxide and hydrogen gas
carbon tetrahydride reacts with oxygen to
produce carbon dioxide and water
chlorine + sodium iodide
chloride + iodine

sodium
hydrogen chlorite
water

chlorine (III) oxide +
ammonium phosphate + barium hydroxide 
ammonium hydroxide + barium phosphate
Type of
Reaction
Example
Synthesis
A + B  AB
Decomposition
AB  A + B
Single Replacement
A + BX  AX + B
Double Replacement
AX + BY  AY + BX
Combustion
A + O2  CO2 + H2O + products
1. Ba (s) + O2(g)  BaO2 (s)
2. HNO3 (aq) + LiOH(aq)  LiNO3(aq) + H2O(l)
3. 2Sb(s) + 3 I2 (g)  2SbI3 (g)
4. C3H8 + O2(g)  CO2 (g) + H2O(g)
5. H3PO4(aq)+ LiOH (aq)  Li3PO4(aq) + H2O(l)
6. Fe(s) + CuSO4 (aq)  FeSO4(aq) + Cu(s)
7. CS2 (g) + O2(g)  CO2 (g) + S2(s)