Unit 10 Notes - Solon City Schools

General Chemistry
Unit 10
 Naming review
 Chemical Reaction/Equations
 Balancing
 Word Equations
 Translating to sentences
You should be able to:
1. Count atoms in a given chemical formula, based on subscripts and coefficients.
2. Use coefficients to properly balance a chemical equation.
3. Express chemical equations into formula, word, and sentence form.
1
Refresher on Ionic Naming
(metal and nonmetal)
I II III IV V VI VII VIII IX X
Formula to name:
1. Convert metal symbol to a name using the periodic table
If it is Sn or Pb or it is a D-Block metal (except Scandium family (+3) , Ag (+1) Zn (+2),
Cd (+2))
It will need a roman numeral
To get the roman numeral, uncriss cross the subscripts and make them
superscripts.
PbBr2
Pb Br2
Pb2+ Br(Bromine is 1- from the periodic table)
Check the negative charge…is it correct?? If yes, then so is the metal. Convert
the number the metal has to a roman numeral and put it after the metal’s name.
so in the above example the metal would be Lead (II)
Another example:
SnSO4
SO4 is a polyatomic (look on the blue sheet) so it looks like Sn is + and SO4 is –
since they are in a one to one ratio
BUT from the blue sheet we see the charge of SO4 is 2- which means Sn must be 2+
Tin (II)
2. Convert the anion to a name
a. If it is a single element, it is named after an element on the periodic table.
Make sure the name ends with – IDE
(IDE—I’d check the table)
b. If it is a polyatomic ion – check the blue sheet.
If it matches the one on the blue sheet exactly – it will end in ATE
If it has one more oxygen then the one on the sheet….PER…ATE
If it has one less oxygen then the sheet ---ITE
If it has 2 less oxygens then the sheet… HYPO…ITE
2
More examples:
1. BaCO3
2. Fe2O3
3. CrN
4. Cu3(PO5)2
Name to formula:
1. Convert the metal to its symbol
You need its charge (it will be a positive superscript)
If it has a roman numeral – that is the charge – it is positive
If it doesn’t have a roman numeral you have to get it from the periodic table
2. Convert the nonmetal to its symbol (it will be a negative superscript)
If it is a single element from the periodic table – use the oxidation pattern
If it is a polyatomic, the charge will be on the blue sheet
3. To get the balanced formula you must criss cross
If the subscripts can be simplified…you must do that!
Ex: Iron (III) bromate
= Fe3+ BrO3- =
Fe3+ BrO3-
=
Fe(BrO3)3
More examples:
1. Titanium (II) oxide
2. Scandium chlorite
3. .Tin (IV) fluoride
4. Silver hypophosphite
3
Ionic Naming Worksheet
Chemical name
Ions
1
Ag+ (IO)-
2
Sb3+ (PO4)3-
3
Be2+ (ClO4)-
4
Sn4+ I-
5
Zn2+ Br-
6
Au+ (SO5)2-
7
Magnesium Perbromate
8
Copper (I) Sulfite
9
Calcium Carbonate
10
Chromium (II) Sulfide
11
Strontium Phosphite
12
Sodium Phosphide
Ionic Formula
4
Refresher on Covalent Naming
(2 nonmetals)
mono di tri tetra penta hexa hepta octa nona deca
Formula to Name:
1. Name the first nonmetal as it appears on the periodic table.
Put a prefix counter in front of it to tell how many of them there are (see above).
If there is only one…do not use the term mono – just use the element name
2. Name the second nonmetal
a. if it is an element from the periodic table it will end in -IDE
b. if it is a polyatomic it will end in ate, per ate, ite or hypo ite
Put a prefix counter in front of it to tell how many of them there are.
If there is only one – you must use the term mono !
Examples:
1. SF6
2. O2Cl5
3. H2O
4. N(SO4)3
Name to Formula:
1. Turn the first element name into a symbol
a. If there is a prefix in front of it - convert it into a subscript after the element symbol
b. If there is not a prefix, assume there is one of that element
2. Turn the second element into a symbol
a. Take the prefix in front of it and convert it into a subscript after the element symbol
Examples:
1. Silicon trioxide
2. Phosphorous pentafluoride
3. Dinitrogen hexasulfide
4. Trichlorine heptaiodide
5
Ionic and Covalent compounds
Elements
Ionic or
Covalent
Ions
Chemical
Formula
Name of Compound
4 Phosphorus +
10 Oxygens
CS2
Calcium + Chlorine
Iron (III) + Bromine
Na2O
Potassium + Sulfur
Si3N4
Triantimony pentasulfide
Fe2(SO4)3
Strontium Chloride
CuOH
Nitrogen Dioxide
N2O
6
Tin (IV) + Fluorine
Cl2O7
Phosphorus Triodide
CCl4
Beryllium + Nitrate
Silicon monocarbide
RbClO3
Al2O3
1 Carbon + 1 Oxygen
7
What's wrong on the right hand side of the arrow?
1. Trisilicon Pentoxide →
2. FeSO4 →
Correct =
Iron (II) Sulfide
3. Cr(NO3)3 →
4. P2Cl5 →
S3O5
Chromium Nitrate
Correct =
Diphosphide Pentoxide
Correct =
5. Copper (I) Oxide
→
CuO2
Correct =
6. Dinitrogen Tetrasulfide → (NO3)2 (SO4)
7. Barium Phosphate →
8. CaBr2 →
9. SO →
Correct =
Be3(PO4)2
Correct =
Calcium (II) Bromide
Correct =
Sulfur Oxide
Correct =
Tin Oxide
Correct =
10. SnO →
11. Hexanitrogen Dichloride →
12. NiC →
Correct =
N2Cl6
Nickel (II) Carbide
13. Zinc Fluoride →
Correct =
ZnFl2
14. Cobalt (II) Phosphide →
Correct =
Correct =
Co3(PO4)2
Correct =
8
15. AgOH →
Silver hydrate
Correct =
9
10
11
Balancing Practice Problems
1.
___Na + ___MgF2
→
___NaF + ___Mg
2.
___Mg + ___HCl
→
___MgCl2 + ___H2
3.
___Cl2 + ___KI
→
___KCl + ___I2
4.
___NaCl
5.
___Na + ___O2
6.
___Na + ___HCl
→
___Na + ___Cl2
→
→
___Na2O
___H2 + ___NaCl
12
7.
___K + ___Cl2
→
___KCl
Challenges:
___C7H6O2 + ___O2 →
___CO2 + ___H2O →
___CO2 + ___H2O
___C3H8 + ___O2
13
Balance each of the following equations:
1. ___ Zn + ___HCl  ___ ZnCl2 + ___ H2
2. ___Sb + ___ O2  ___ Sb4O6
3. ___H3AsO4  ___ As2O5 + ___ H2O
4. ___N2O5 + ___H2O  ___HNO3
5. ___Fe2O3 + ___ C  ___CO + ___ Fe
6. ___Al4C3 + ___ H2O  ___CH4 + ___ Al(OH)3
7. ___Si2H3 + ___ O2  ___ SiO2 + ___ H2O
8. ___Na2O2 + ___ H2O  ___NaOH + ___O2
9. ___Ca3(PO4)2 + ___ H2SO4  ___CaSO4 + ___H3PO4
14
10. ___PCl5 + ___ H2O  ___H3PO4 + ___ HCl
11. ___NH4NO3  ___ N2O + ___ H2O
12. ___BaCl2 + ___Al2(SO4)3  ___BaSO4 + ___AlCl3
13. ___C6H6 + ___ O2  ___CO2 + ___ H2O
14. ___As + ___NaOH  ___Na3AsO3 + ___ H2
15. ___Ca10F2(PO4)6 + ___H2SO4  ___Ca(H2PO4)2 +
___CaSO4 + ___HF
15
One last balancing worksheet
1. ___Na2S + ____CaCl2
____NaCl + ____CaS
2. ___Mg3N2 + ____H2O
____MgO + ____NH3
3. ___Al + ____O2
____Al2O3
4. ___Sr(NO3)2 + ____Al2(CO3)3
5. ___C4H10 + ____O2
6. ___P4O10 + ____H2O
7. ___Al + ____Fe3O4
8. ___KClO3
____SrCO3 + ____Al(NO3)3
____CO2 + ____H2O
____H3PO4
____Al2O3 + ____Fe
____KCl + ____KClO4
16
Converting chemical equations to word equations
1. ____Na2SO4 + ____BaCl2
____BaSO4 + ____NaCl
2. ____ZnS + ____O2
____ZnO + ____SO2
3. ____NH3 + ____O2
____NO + ____H2O
4. ____Al + ____Br2
____AlBr3
5. ____Mg3N2 + ____HCl
6. ____GaCl3 + ____F2
____MgCl2 + ____NH3
____GaF3 + ____Cl2
7. ____Na2SO4 + ____Pb(NO3)2
8. ____FeCl3 + ____Na2CO3
9. ____CaCl2 + ____Na3PO4
10.
____S8 + ____F2
11.
____Zn + ____HCl
12.
____Mg + ____CuI2
____NaNO3 + ____PbSO4
____Fe2(CO3)3 + ____NaCl
____NaCl + ____Ca3(PO4)2
____SF6
____ZnCl2 + ____H2
____MgI2 + ____Cu
17
Converting word equations into chemical equations (I)
1. Magnesium Sulfate + Calcium Chloride
2. Beryllium Sulfide + Oxygen
3. Potassium Bromide + Chlorine
Calcium Sulfate + Magnesium Chloride
Beryllium Oxide + Sulfur Dioxide
Potassium Chloride + Bromine
4. Calciuim Phosphate + Dihydrogen Monosulfate
Calcium Sulfate + Trihydrogen Monophosphate
5. Aluminum Chloride + Iodine
6. Iron + Dihydrogen Monosulfate
Aluminum Iodide + Chlorine
Iron (II) Sulfate + Sulfur Dioxide +
Dihydrogen Monoxide
7. Phosphorous Pentachloride + Dihydrogen Monoxide
Trihydrogen Phosphate +
Hydrogen Chloride
8. Aluminum Sulfide + Dihydrogen Monoxide
Aluminum Hydroxide +
Dihydrogen Monosulfide
18
Converting word equations into chemical equations (II)
1. Aluminum Bromide + Chlorine
2.
Zinc + Lead (II) Nitrate
Aluminum Chloride + Bromine
Zinc (II) Nitrate + Lead
3. Hydrogen + Carbon Monoxide
4. Sodium + Hydrofluoric acid
5. Copper + sulfuric acid
Dihydrogen Monoxide + Carbon
Sodium Fluoride + Hydrogen
Copper (II) Sulfate + Dihydrogen Monoxide + Sulfur Dioxide
6. Potassium Carbonate + Calcium Chloride
7. Iron (III) Oxide + Carbon Monoxide
Calcium Carbonate + Potassium Chloride
Iron + Carbon Dioxide
8. Aluminum Oxide + Dihydrogen Monoxide
Aluminum Hydroxide
9. Hydrochloric acid + Calcium Carbonate
Calcium Chloride + Dihydrogen Monoxide
+ Carbon Dioxide
10. Strontium Iodide + Lead(II) Phosphate
11. Magnesium + Nitrogen
Strontium Phosphate + Lead (II) Iodide
Magnesium Nitride
12. Sodium Hydroxide + Hydrogen Chloride
Sodium Chloride + Dihydrogen Monoxide
19
Translate the following sentences into a formula equation.
1. Solid sulfur trioxide and dihydrogen monoxide combine to make sulfuric acid.
2. Aqueous lead (II) nitrate and aqueous sodium iodide react to make solid lead (II) iodide
and aqueous sodium nitrate.
3. Aqueous calcium fluoride and sulfuric acid react to form solid calcium sulfate and
hydrofluoric acid.
4. Solid calcium carbonate will come apart when heated to produce solid calcium oxide and
carbon dioxide.
5. Aqueous aluminum sulfate and aqueous magnesium hydroxide will react to form solid
aluminum hydroxide and aqueous magnesium sulfate.
6. Copper metal and aqueous silver nitrate react to form silver metal and aqueous copper (II)
nitrate.
20
Write a balanced chemical reaction for each of the reactions described below:
1. Barium metal and aqueous hydrochloric acid react to produce solid barium chloride and
hydrogen gas.
2. Using heat, aqueous nitric acid reacts with solid magnesium hydroxide to make aqueous
magnesium nitrate and liquid dihydrogen monoxide.
3. Solid Aluminum carbide reacts with dihydrogen monoxide in the liquid form at 450.0 oC
to yield carbon tetrahydride gas and aluminum hydroxide solid.
4. Lead (II) acetate in the solid form and aqueous hydrosulfuric acid react to form solid
Lead (II) sulfide and liquid acetic acid.
21
Write out these reactions in word form and sentence form :
1. H2 (g) + Cl2 (g)  2HCl (aq)
2. 2Al (s) + Fe2O3 (aq) 
Al2O3 (aq) + 2Fe (s)

3. 8Pb (s) + S8

8PbS (s)
550 oC
4. PbSO4 (aq) + FeCl2 (aq)

PbCl2 (s) + FeSO4 (aq)
22

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