Chemistry 111 Study Sheet Answers
Test 2 (Chapters 9-11, and Sections 2.7-2.9)
1. K2SO4 has Ionic bonding. What state would it be in at room
sp3, tetrahedral,
4bonds (4sigma)
temperature? Solid
2. Determine the hybridization, electron arrangement, and the
number of sigma(σ) and pi(π) bonds for the indicated atoms.
3. What does VSEPR stand for?
H
H C
H
sp, linear, 3 bonds
(1 sigma, 2 pi) sp, linear, 4 bonds
(2 sigma, 2 pi)
C
sp, linear, 4 bonds
(2 sigma, 2 pi)
H
N
O
C
sp2, trigonal planar,
2 bonds (1sigma, 1pi)
C H
sp2, trigonal planar,
4 bonds (3sigma, 1pi)
Valence Shell Electron Pair Repulsion Theory
4. Define the following: molecular structure (the geometric arrangement of atoms connected to a central atom),
bond distance (the distance between the nuclei of two bonded atoms), and bond angle (the angle between
two of an atoms bonds)
5. The following molecular structures correspond to: a) how many regions of electron density (groups of electrons) and b) what bond
angles? octahedral a) 6; b) 90°, tetrahedral a) 4; b) 109.5°, trigonal bipyramidal a) 5; b) 120° and 90°, linear a)
2; b) 180°, and trigonal planar a) 3; b) 120°.
6. What constitutes a region of electron density? One group of electrons is a single bond, a double bond, a triple
bond, or a lone pair.
7. Which of the following causes the most electron repulsions? single, double, or triple bonds or lone pairs of electrons
8. What type of compounds are attracted to an electric field? polar molecules
9. Which of the following compounds are polar: NH3, H2O, CCl4, SF6.
10. What is valence bond theory? Please see textbook.
11. What type of overlap gives the maximum possible p orbital overlap? Head on sigma bonding (not side-to-side pi
bonding)
12. What is a sigma (σ) (the region of orbital overlap lies on an imaginary line connecting the nuclei; head on
overlap) and a pi (π) bond (the region of orbital overlap does not lie on an imaginary line connecting the
nuclei; side-to-side overlap)?
13. What do single (1sigma), double (1sigma and 1 pi), and triple bonds (1sigma and 2 pi) consist of in terms of sigma and
pi bonds?
14. F (T/F) sp hybrid orbitals are bigger than sp3 hybrid orbitals.
15. All hybrid orbitals on a hybridized atom are of equal or unequal energy?
16. 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 linear sp, SO2 bent sp2, IF4- square planar sp3d2,
CH4 tetrahedral sp3, C2H4 trigonal planar sp2, C2H2 linear sp, ClF3 trigonal planar sp3d.
Drawings available on reserve in library.
17. What electronic structures correspond to the following hybridizations? sp (linear), sp2 (trigonal planar), sp3
(tetrahedral), sp3d2 (octahedral), sp3d (trigonal bipyramidal)?
18. Polyatomic ions are held together with covalent bonds, but combine with metal cations to form ionic compounds.
19. Predict the charge on the monoatomic ions formed from the following atoms: Te 2-, Cs 1+, Si 4-, F 1-, Na 1+.
20. What did the colorful compounds that we looked at in lab have in common? transition metals
ferrous chloride FeCl2, potassium bisulfate KHSO4,
21. Write the formula for:
diphosphorus pentoxide P2O5,
lead(II) oxide PbO, silicon dioxide SiO2, barium hydride BaH2.
22. Name the following compounds: N2O4 dinitrogen tetroxide, Fe(OH)3 iron(III) hydroxide, K2O potassium oxide,
KHSO4 potassium bisulfate, NH4Cl ammonium chloride, KClO2 potassium chlorite, KClO4 potassium
perchlorate, KClO potassium hypochlorite, KClO3 potassium chlorate, PbCrO4 lead(II) chromate,
Ba3(PO3)2 barium phosphite, KMnO4 potassium permanganate, K2S potassium sulfide, AuPO4 (gold has
2 possible charges but was not on your list).
23. Give the formula for the following compounds: ammonium phosphate (NH4)3PO4, sodium acetate NaC2H3O2, iron(III)
bromide FeBr4, sulfur trioxide SO3, copper(II) nitrate Cu(NO3)2, phosphorous pentachloride PCl5, nitrogen dioxide
NO2.
24.
anions→
cations↓
Na
1
S
Cl
C2H3O2
SO4
NO2
PO4
Na2S
NaCl
NaC2H3O2
Na2SO4
NaNO2
Na3PO4
CaCl2
Ca(C2H3O2)2
CaSO4
Ca(NO2)2
Ca3(PO4)2
Ca(OH)2
3 Al(C2H3O2)3
Al2(SO4)3
Al(NO2)3
AlPO4
Al(OH)3
H2SO4
HNO2
H3PO4
H2O
CuNO2
Cu3PO4
CuOH
Ca
CaS
Al
Al2S3
AlCl3
H
H2S
HCl
HC2H3O2
Cu+1
Cu2S
CuCl
CuC2H3O2
Cu2SO4
Cu+2
CuS
CuCl2
Cu(C2H3O2)2
CuSO4
2
4
5
Cu(NO2)2
6 Cu3(PO4)2
1. sodium sulfide; 2. calcium chloride; 3. aluminum acetate; 4. sulfuric acid;
5. copper(I) nitrite; 6. copper(II) phosphate; 7. sodium hydroxide
25. Identify the cation and anion and their charge for each of the following compounds.
NH41+ Cl– ; Co2+
S2- ; Ba2+
O22– (peroxide) ; Cs1+ CN1–
;
Sn2+
SO32–
OH
7 NaOH
Cu(OH)2