Test 2 Review
Name:
Question 1. Draw the electron dot formulas for the following:
a) NCl2H (N is central atom)
b)N2O (1 N is central atom)
c) For the compounds in question #5, give the number of electron groups, the electronic geometry
and the molecular shape of the molecules.
Compound
Electron
Groups
Electron
Molecular
Group
Shape
Arrangement
SCl2H
N2O
Question 2. Write the molecular formula for the following names:
a) Lead (IV) Sulfide
b) Molybdenum (V) Phosphate
c) Barium Phosphide
d) Ruthenium (III) sulfide
e) Dinitrogen oxide
f) Nitrogen disulfide
Question 3. Name the following covalent compounds:
a) P2O5
b) F3S5
Question 4. The combustion of natural gas, CH4 is very important in energy production:
a) What is the balanced chemical equation for the combustion of natural gas?
b) If 15.5g of CH4 and 55.2g of O2 are burned, what is the limiting reactant?
c) How much water is produced(in grams)?
d) What is the percent yield if only 28.5g of H2O are collected?
Question 5. Consider the reaction:
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
a) What type of reaction is it?
b) What species is being reduced and what is being oxidized?
Question 6. Consider the Molecule VO(H2PO4)2:
a) What is its Molar Mass?
b) How many moles are in 234.5g of it?
c) How many moles are 8.36x1022 molecules?
d) How many H atoms are in 1 molecule of it?
e) How many O atoms are in 7.35 moles?
Question 7. Write the Balanced Formulas for the following Anions and Cations:
S2Sr2+
Mo4+
Cr6+
Na+
CO32Fe3+
P3-
F-
Question 8. What is the pressure (in mmHg) of a gas that occupies 1.345x108μL, has a temperature of
67.3◦C and contains 1.76 moles of N2?
Question 9. At standard temperature and pressure (STP), how many moles of N2 occupy 5.83x10-3ML?
Question 10. A container of Xe gas at -23◦C occupies 3.45L at a pressure of 2.45atm. What volume (in L)
does it occupy at 72◦C at a pressure of 657mmHg?
Multiple Choice
Question#11 How many moles of oxygen can be produced from one mole of KClO3 in the reaction:
2KClO3→2KCl + 3O2?
a) 1 mol
b) 1.5 mol
c) 2 mol
d) 3 mol
Question#12 The number of C atoms in 0.500 mole of C is_______.
a) 2.50 × 1023 C atoms
b) 3.01 × 1023 C atoms
c) 5.01 × 1023 C atoms
d) 6.00 × 1023 C atoms
Question#13 How many moles of O atoms are there in 2 moles of glucose: (C6H12O6)?
a) 2 moles
b) 24 moles
c) 6 moles
d) 12 moles
Question#14 What is the molar mass of S3 if the molar mass of sulfur is 32.0?
a) 64 g
b) 32 g
c) 96 g
d) 10.7 g
Question#15 What is the percent yield if 50 g of CO2 were collected and 200g were expected?
a) 50%
b) 25%
c) 75%
d) 100%
Question#16 Which of the following reactions can be classified as decomposition?
a) CuCO3 (s) → CuO (s) + CO2 (g)
b) 4Fe (s) + 3O2 (g) → 2Fe2O3 (s)
c) Mg (s) + 2AgNO3 (aq) → Mg(NO3)2 (aq) + 2Ag (s)
d) NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (l)
Question#17 What is the correct name of the ionic metal compound: AuCl3?
a) gold chloride
b) gold trichloride
c) gold (III) chloride
d) gold (III) trichloride
Question#18 What is the name of the covalent compound: S3Cl5?
a) Sulfur chloride
b) Sulfur hexachloride
c) Trisulfur chloride
d) Trisulfur pentachloride
Question#19 What is the correct formula for Chromium (VI) hydroxide?
a) Cr(OH)3
b) Cr(OH)6
c) CrOH6
d) Cr6OH
Question#20 How many electrons were lost by Pb in Lead (IV) chloride?
a) 4
b) 5
c) 0
d) 6
Gas Law Equations:
P1V1=P2V2
V1=V2
T1 T2
P1 = P2
T1 T2
V1 = V2
n1 n2
P1V1=P2V2
T1 T2
PV=nRT where R=0.0821(L●atm)/(mole●K) or,
R=62.4 (L●mmHg)/(mole●K)