Chemistry 111 Study Sheet
Test 2 (Chapters 9-11, 3, and Sections 2.7-2.9)
1. K2SO4 has ______ bonding. What state would it be in at room temperature? _____
3. Determine the hybridization, electron arrangement, and the number of sigma(σ) and pi(π) bonds for the indicated atoms.
4. What does VSEPR stand for?
5. Define the following: molecular structure, bond distance, and bond
angle.
6. The following molecular structures correspond to: a) how many
regions of electron density (groups of electrons) and b) what
bond angles? octahedral, tetrahedral, trigonal bipyramidal, linear, and trigonal planar.
7. What constitutes a region of electron density (group of electrons) for VSEPR theory?
8. Which of the following causes the most repulsions? single, double, or triple bonds or lone pairs of electrons
9. What type of compounds are attracted to an electric field?
10. Which of the following molecules are polar: NH3, H2O, CCl4, SF6.
11. What is valence bond theory?
12. What type of overlap gives the maximum possible p orbital overlap?
13. What is a sigma (σ) and a pi (π) bond?
14. What do single, double, and triple bonds consist of in terms of sigma and pi bonds?
15. _____(T/F) sp hybrid orbitals are bigger than sp3 hybrid orbitals.
16. All hybrid orbitals are of equal or unequal energy?
17. Identify the type of molecular structure and hybridization in each of the following compounds and sketch the hybrid and
unhybridized orbitals used in bonding. BeI2, SO2, IF4-, CH4, C2H4, C2H2, ClF3.
18. What electronic structures (shapes) correspond to the following hybridizations? sp, sp2, sp3, sp3d2, sp3d?
19. amu is an abbreviation for ________ .
20. What is the formula mass of NaOH? What is the mass of 2.7moles NaOH?
21. Find the formula mass of each of the following.
a. C5H12; b. Al(NO3)3
22. ________ molecules of NaH = 1 mole of NaH molecules.
23. ________ grams Be atoms = 1 mole of Be atoms
24. How many moles of Na2SO4 are in a 1.5 g sample of Na2SO4? How many moles of O atoms are in the same sample?
25. Calculate the % composition of C and H in CH4.
26. Determine the percent composition of C8H10O2.
27. What is the empirical formula for C9H12O3?
28. Determine the empirical formula for a compound with a percent composition of 45.0%C; 7.50%H; and 47.5%F.
29. Calculate the empirical formula of a polymer which is made of 59.9% C, 8.06% H, and 32.0 % O.
30. A 27.5 g sample of a compound containing carbon and hydrogen contains 5.5 g of hydrogen. The molecular mass of the
compound is approximately 30 amu. What are the empirical and molecular formulas?
31. Balance the following chemical equations.
a. KClO3
→
KCl +
O2
32. Balance the following equations:
b. Ca3(PO4)2
Na2S2O3 + I2 → NaI + Na2S4O6
+
C →
Ca3P2
+
CO
C3H6 + O2 → CO2 + H2O
HCl + Cr → CrCl2 + H2
33. List a) the product(s), and b) the reactant(s) in the equation:
KClO3
KCl +
→
O2
34. Given the balanced equation {2Al + 3H2SO4 → Al2(SO4)3 + 3H2} answer the following:
a) How many moles of Al2(SO4)3 can be produced by reacting 0.50mol H2SO4?
b) How many moles of Al2(SO4)3 can be produced by reacting 18g H2SO4?
c) How many grams of H2 can be produced by reacting 18g Al?
d) If 1.00mol Al is reacted with 1.25 mol H2SO4, which is the limiting reagent?
e) How many grams of H2 could be produced by the reaction in question d?
f) What is the limiting reagent if 54g Al is reacted with 98g H2SO4?
g) What is the percent yield if 87g of Al2(SO4)3 is produced by the reaction in question f?
35. 1.50 g of silicon and 1.50 g of nitrogen can be combined according to the following reaction:
Si + N2 → Si3N4
a. What is the limiting reagent? b) What is the theoretical yield of Si3N4?
36. What is the % yield of a reaction that converts 1000.0 g of C6H5CH3 to 1210.0 g of C6H5CO2H?
2 C6H5CH3 + 3 O2 → 2 C6H5CO2H + 2 H2O
37. Polyatomic ions are held together with
bonds, but combine with metal cations to form
compounds.
38. Predict the charge on the monoatomic ions formed from the following atoms: Te, Cs, Si, F, Na.
39. What did the colorful compounds that we looked at in lab have in common?
40. Write the formula for:
ferrous chloride, potassium bisulfate, diphosphorus pentoxide, lead(II) oxide, silicon dioxide, barium
hydride.
41. Name the following compounds: N2O4, Fe(OH)3, K2O, KHSO4, NH4Cl, KClO2, KClO4, KClO, KClO3, PbCrO4, Ba3(PO3)2,
KMnO4, K2S, AuPO4.
42. Give the formula for the following compounds: ammonium phosphate, sodium acetate, iron(III) bromide, sulfur trioxide,
copper(II) nitrate, phosphorous pentachloride, nitrogen dioxide.
43. Write the formula for the compound formed if the cation at the beginning of a row combines with the anion at the top of a column.
For nomenclature practice, name the compounds in the numbered boxes. (Note the example below.)
anions→
cations↓
S
Cl
C2H3O2
SO4
NO2
PO4
Na 1
OH
7
Ca
2
Ca(C2H3O2)2
Al
3
H
4
Cu+1
5
Cu+2
6
44. Identify the cation and anion and their charge for each of the following compounds.
NH4Cl
BaS
CoO2
CsCN
SnSO3