Vocabulary Week 17!!
• reactants
• products
• synthesis
• decomposition
• combustion
• shibboleth
• propitiate
• chortle
• unremitting
• inure
Remember…• Chemical reactions
involve changes with atoms’ electrons
• Nuclear reactions involve changes with atom’s 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 + B2 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 + H2Tums is used to neutralize stomach acid
Double Displacement• Exchange of positive ions between substances
AX + BY BX + AYCaCO3 + 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
• Evidence of chemical reaction:1. Gas is produced2. Color Change3. Change in smell4. Formation of solid—precipitate5. Light is produced6. 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
Most ActiveLithium
RubidiumPotassiumCalciumSodium
MagnesiumAluminum
ManganeseZincIron
NickelTin
LeadCopperSilver
PlatinumGold A + BX AX + B
Al + PbNO3
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 equations1. 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 + O2 Al2O3
C3H8 + O2 CO2 + H2O
KNO3 KNO2 + O2
O2 + CS2 CO2 + SO2
Cu + H2O CuO + H2
Cu + Cl2 CuCl2
Al(NO3)3+ NaOH Al(OH)3 + NaNO3
Fe + H2SO4 Fe2(SO4)3 + H2
KOH + HBr KBr + H2O
Al + S8 Al2S3
Al(OH)3 + H2CO3 Al2(CO3)3 + H2O
Al(OH)3 + HBr AlBr3 + H2O
Vocab Week 18!Last one this semester!
• single displacement
• double displacement
• reactivity series
• precipitate
• aqueous
• obsequious
• moribund
• winnow
• flaccid
• rife
Na + NaNO3 Na2O + N2
Li + AlCl3 LiCl + Al
NH3 + HCl NH4Cl
FeS2 + O2 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 sodium chloride + iodine
hydrogen chlorite chlorine (III) oxide + water
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)