Memorized:
1. Which formula represents strontium phosphate?
A. SrPO4
B. Sr3PO8
C. Sr2(PO4)3
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D. Sr3(PO4)2
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3. Which one of the following is correct?
A. KClO3, potassium perchlorate
B. Al2(SO3)2, aluminum sulfate
E. Na2Cr2O7, sodium dichromate
Periodic Table without names
Unit 4
Dimensional analysis
2. In a methane (CH4) molecule, the angle between the two hydrogen atoms is:
A. 109.5
B. 120
C. 90
D. 180
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Provided:"
Coverage:
Electron Domain & Molecular Geometry including
bond angles) Hybridizations
Polyatomic ions
Electronegativity Trend
Practice Test
E. none
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C. CuO, copper oxide
D. MgPO4, magnesium phosphate
4. Which of the following is NOT a correct chemical formula?
A. SrBr2
B. Ca2O3
C. Mg3N2
5. Which one of the following does not exhibit resonance?
A. SO2
B. SO3
C. HI
D. Na2S
D. CO32-
6. Which of the following names is correct for the compound SnCl4?
A. tin (II) chloride
C. tin(IV) chloride
B. tin tetrachloride
D. tin chloride
E. AlI3
E. NO3-
E. tin (II) tetrachloride
7. For resonance forms of a molecule or ion, ______.
A. one always corresponds to the observed structure
B. all the resonance structures are observed in various proportions
C. the observed structure is a blend of the resonance forms
D. the same atoms need not be bonded to each other in all resonance forms
E. there cannot be more than two resonance structures for a given species
8. What is the maximum number of double bonds that carbon can form?
A. 4
B. 1
C. 0
D. 2
E. 3
9. The ICl4- has _____ valence electrons.
A. 34
B. 35
D. 28
E. 8
10. In PF3, the central phosphorus has
A. 2, 2
B. 1, 3
C. 36
nonbonding and
bonding electron pairs.
C. 3, 1
D. 1, 2
11. Resonance structures differ by __________.
A. number and placement of electrons
B. number of electrons only
E. placement of electrons only
12. What electrons are shown in the Lewis structure for CH4?
A. carbon’s electrons, only
B. both carbon and hydrogen’s electrons
E. 3, 3
C. placement of atoms only
D. number of atoms only
C. hydrogen’s electron’s only
D. both carbon and hydrogen’s valence electrons
13. Which substance would consist of positive ions immersed in a “sea” of mobile electrons?
A. sulfur
B. nitrogen
C. calcium
D. chlorine
14. The hybridization around the Xe in the molecule XeF4 is
A. sp3d2, square planar
B. sp3d, seesaw
and the shape is
:
C. sp3d, linear D. sp3d2, T-shaped
15. A pi (Π) bond :
A. comes from electrons in unhybridized atomic orbitals
B. has electron density between the bonding nuclei
C. is responsible for all covalent bonds
D. all of the above
16. The correct chemical formula for iron(II) sulfide is
A. FeS
B. Fe2S3
C. FeSO4
D. Fe2(SO4)3
17. Which type of bonding is found in all molecular substances?
A. covalent bonding
B. ionic bonding
C. hydrogen bonding
D. metallic bonding
18. What is the electronic geometry for 6 regions of high electron density on a central atom?
A. octahedral
B. square planar
C. trigonal bipyramidal
D. tetrahedral
E. trigonal planar
19. The phosphorus pentachloride molecule is nonpolar and contains no lone (unshared) electron pairs on the
phosphorus atom. What are all of the possible Cl-P-Cl bond angles?
A. 120°
B. 180°
C. 109.5°
D. 90°, 120°, and 180°
E. 90° and 180°
20. What is the chemical formula for iron(III) oxide?
A. FeO
B. Fe2O3
21. How many different elements are in K2SO4?
A. 4
B. 7
C. Fe3O
C. 3
D. Fe3O2
D. 6
22. Which of the following statements about the valence bond theory is false?
A. For an atom to share more than 8 electrons it must hybridize d orbitals.
B. To make 4 single bonds, an atom will make 4 sp3 hybrid orbitals.
C. The number of hybrid orbitals formed equals the number of high electron density regions.
D. Trigonal planar molecules use sp2 hybrid orbitals
E. Atoms that do not complete their octet use either sp3d or sp3d2 hybrid orbitals.
23. Which of the following molecules has 120° bond angles?
A. BF4B. CF4
C. H2O
D. BI3
24. Choose the species that is incorrectly matched with the electronic geometry about the central atom.
Molecule
Electronic Geometry
A.
CF4
tetrahedral
B.
BeBr2
linear
C.
H2O
tetrahedral
D.
NH3
tetrahedral
E.
PF3
pyramidal
25. Which molecule is incorrectly matched with the molecular geometry?
Molecule
Molecular Geometry
A
octahedral
SF6
B.
trigonal pyramidal
AsH3
C.
trigonal planar
BCl3
D.
AsF5
trigonal bipyramidal
E.
linear
H 2S
E. NH4+
26. Which species is incorrectly matched with the hybridization at the central atom?
Species
Hybridization at Central Atom
A.
sp2
SO2
B.
sp3
CF4
C.
sp3d2
PF5
D.
SeO42sp3
E.
HCN
sp
27. While BF3, ICl3, and PF3 all have the same number of atoms, they have different molecular geometries. Using the
VSEPR theory to support your answer, explain the differences in their geometries and bond angles.
28. The Lewis structure for TeCl4 has four bonding pairs and one lone pair. There are two possible positions for this
molecule’s lone pair, but only one is correct. Draw each possible structure (with the correct geometry) then explain
which is the correct one, and why.
29. Consider C2H3OH, as pictured to the right.
A. Name the molecular geometry and hybridization for both the first Carbon and the Oxygen in the molecule.
C: __________________________,
O: __________________________,
_____________
_____________
B. Draw a hybridization diagram for C2H3OH. Be sure to label all orbitals—hybridized or unhybridized. In addition,
label all bonds as sigma or pi bonds.
30. Predict (a) the approximate bond angle, (b) the molecular geometry. Write your answers near the corresponding labels
(1 to 5) in the drawings. (Note: the lone pairs on the F atoms are omitted.)
H
H
N
1
F
S
F
F
Br
4
C
N
F
F
F
2
F
3
C
N
5
F
F
C
H
C
C
N
O
H
N
H
31. For each of the molecules below fill in the indicated items in the chart. The central atoms are underlined.
Molecule
(1) SO2
(2) HBF2
(3) XeF4
(4) CH2Cl2
(5) NF3
(a) No. of
valence e - ‘s
(b) Lewis
structure
(c) Approximate
bond angle(s)
(d) Geometry
name
32. For each of the molecules below fill in the indicated items in the chart. The central atoms are underlined.
Molecule or
Ion
(a) No. of
valence e - ‘s
(b) Lewis
structure
(c)
Approximate
bond angle(s)
(d) Geometry
name
(1) OF2
(2) H2CO
(3) NO2+
(4) BF3
(5) SbF5
33. Draw Lewis structures for the following compounds. Determine molecular geometry, bond angles, hybridization, and
number of sigma/ pi bonds.
A. HOCl
C. H2S
B. PF3
D. TeF6
F. CH3-
E. CF3Cl
G. BF3
H. NO2
34. Name each of the following chemical compounds and determine their formula weights:
AgNO3
PbSO4
N 2O 3
CoCl2 . 4 H2O
HCl
NH3
PBr3
B 2F6
Sn(CO3)2
H2SO3
35. Write the formulas of each of the following chemical compounds and determine their formula weights.
lithium acetate
copper (I) oxide
ammonium phosphate
vanadium (V) cyanide
nitrogen tribromide
iron (II) fluoride tetrahydrate
sulfur hexachloride
platinum (IV) hydroxide
carbonic acid
magnesium acetate