Sc 10
Mr. Bellman
Ch 4 B Pretest
Naming Compounds / Formula and Balancing Equations
Vocab: Be able to define these terms:
binary covalent compounds
balanced chemical equation
chemical reaction
skeleton equation
ionic compounds
chemical equation
conservation of mass
symbolic equation
(16 )
NAME____________________
Date______________Bk_____
polyatomic ion
reactants
coefficient
chemical formula
subscript
products
diatomic
multivalent
______________________1. The number in front of a chemical formula in a balanced chemical equation.
______________________2. The number after a chemical symbol that how many atoms are present in the molecule.
______________________3. The name given to compounds that have two non-metal elements sharing electrons to form a bond.
______________________4. An unbalanced chemical equation. An equation that only shows the reactant and product molecules.
______________________5. This term describes the fact that the mass of the reactants equals the mass of the products.
______________________6. Compounds made up of metals and non-metals.
______________________7. Elements, molecules or compounds found on the left side of the arrow in a chemical reaction.
______________________8. Ions that contain more than one atom in its formula.
______________________9. Elements that naturally occur as two atoms joined together with covalent bonds.
______________________10. Metals that can have more than one positive charge are called this.
Name the following compounds:
1. Ca3P2
___________________________
2. KNO3
___________________________
3. V(OH)5
___________________________
4. (NH4)3PO4
___________________________
5. Si2Br5
___________________________
6. CuS
___________________________
7. SnF4
___________________________
8. HCH3COO
___________________________ or __________________________
9. Mg(OH)2
___________________________
Give the formula for the following compounds:
1. hydrogen thiosulfate
___________________________
2. sodium nitride
___________________________
3. mercury ( II ) sulfide
___________________________
4. nitric acid
___________________________
(or hydrogen nitrate)
5. trinitrogen nonachloride
___________________________
6. osmium ( III ) iodide
___________________________
7. strontium bicarbonate
___________________________
8. tantalum huskyide
___________________________
9. gold ( III ) dichromate
___________________________
Balance the following reactions:
1. ____ K
+
____ N2
____ K3N
2. ___ Mg3P2
+
____ NaBr
____ MgBr2
3. ____ C3H8
+
____ O2
____ CO2
4.
____ C6H14 +
5. ____ Co(OH)3 +
+
+
____ Na3P
_____ H2O
____O2
_____ CO2
+
____ H2O
____ SrSO4
____ Sr(OH)2 + ____ Co2(SO4)3
6. cobalt reacts with chlorine to produce cobalt ( III ) chloride
skeleton
balanced
7. calcium nitrate plus potassium phosphate produces potassium nitrate and calcium phosphate
Skeleton
Balanced
8. sulfuric acid plus lead ( IV ) hydroxide produces lead ( IV ) sulfate and water
skeleton
balanced
Answers:
Vocab: 1. Coefficients 2. Subscripts 3. Binary covalent compounds 4. Skeleton equation 5. (law of ) conservation of mass
6. ionic compounds 7. Reactants 8. Polyatomic ions 9. Diatomic 10. Multivalent metals
Naming:
1. calcium phosphide
2. potassium nitrate 3. vanadium ( V ) hydroxide 4. ammonium phosphate 5. disilicon pentabromide
6. copper ( II ) sulfide
7. tin ( IV ) fluoride
8. hydrogen acetate or acetic acid
9. magnesium hydroxide
1. H2S2O3 2. Na3N
3. HgS
4. HNO3
5. N3Cl9
6. OsI3
7. Sr(HCO3)2 8. Ta3(OKM)5 9. Au2(Cr2O7)3
Balancing: showing coefficients only:
1. 6 1 2
2. 1 6 3 2
3. 1 5 3 4
4. 2 19 12 14
5. 2 3 3 1
Balancing word equations: showing final balanced equation (skeleton equation has no coefficients)
6. Skeleton: Co + Cl2
CoCl3
balanced
2 Co + 3 Cl2
2 CoCl3
7. Skeleton:
Balanced:
8. skeleton:
Balanced:
Ca(NO3)2 + K3PO4
KNO3
3 Ca(NO3)2 + 2 K3PO4
6 KNO3
H2SO4
Pb(SO4)2
+
Pb(SO4)2
+ 4 H2O (trick: write water as HOH to help balance)
4 H (OH)
2 H2SO4
+
Pb(OH)4
+
Pb(OH)4
+ Ca3(PO4)2
+ Ca3(PO4)2
H2O (trick: write water as HOH to help balance)