a. I VSEPR, g e e. b. Valence-Space Electron-Part Reabsorption c. Valence-Shell Electron-Pair Recoil d. Valence-Shell Electron-Pair Repulsion e. Valence-Space Electron-Part Repulsion f. Who cares?
2. An atom with sp d hybridization is a member of the _________ electron geometry group.
a. Linear d. Trigonal Bipyramidal b. Trigonal planar e. Octahedral c. Tetrahedral f. Bent
3. There are ______ bonds and _______ bonds in the following molecule:
a. 14, 4 b. 4, 14 c. 13, 5 d. 5, 13 e. 13, 0
4. The forces within a molecule are called intramolecular forces, while forces between two molecules are called - _______________ forces.
5. Explain what London Dispersion Forces, Dipole-dipole forces, and Hydrogen Bonding are:
i. London Dispersion Forces
ii. Dipole-Dipole Forces
iii. Hydrogen Bonding
6. What is the strongest IMF present in a solution of C3H7FH? a. Ionic b. Hydrogen Bonding c. Dipole-Dipole d. London Dispersion
7. How many of the following molecules are nonpolar?
C2H4NH2, O2, SiH3F, C3H8O, O3, BeCl2, NaCl, COS
Answer key springaoao
O
) g
6
Every bond has 7 sigma bond , every other bond if it has
a b s z e a double or triple bond are pig .
4 3
intermolecular
weak intermolecular force , present in every molecule but most relevant in nonpolar molecules
Intermediate intermolecular force , found between polar molecules
strongest intermolecular force , H-FDN Bonded together
g o- intramolecular
HB NP , Dpp P
i
a. 5 b. 4 c. 3 d. 2 e. 1
8. Which of the following is true about London-dispersion forces? a. Intermolecular forces between nonpolar molecules caused by the
presence of permanent dipoles in the molecules. b. An attraction between regions of polar molecules that have partial
charges of opposite sign c. Intermolecular forces between nonpolar molecules caused by the
presence of temporary dipoles in the molecules. d. Intermolecular forces between a hydrogen atom bonded to a N, O,
or F atom. 9. Which of the following ranks the compounds from lowest to highest
boiling point? a. CH < CH O < CaCO < CH OCH b. CaCO < CH OCH < CH < CH O c. CH OCH < CH O < CaCO < CH d. CH < CH OCH < CH O < CaCO
10. The electron geometry of CH F is __________, and its molecular geometry is _______________.
a. Tetrahedral, tetrahedral b. Tetrahedral, bent c. Trigonal planar, trigonal pyramidal d. Linear, linear
11. The hybridization of NH is ____________. a. sp c. sp b. sp d. sp d
12. Which of the following will have the lowest boiling point? a. (NH4)Cl b. I2 c. MgS d. HOC6H6OH
13. Which of the following will have the highest boiling point? a. Cl2 b. PH3 c. NH3 d. CH3F
14. True or False: Water, the molecule that makes up approximately 60% of our body weight, is polar.
a. True b. False
H
0 HB f HB
O
15. Rank the following molecules based on strength of intermolecular forces (IMFs):
NH3, Fluorine monochloride, Strontium Sulfide, C6H6
a. SrS > NH3 > FCl > C6H6 b. SrS > FCl > NH3 > C6H6 c. NH3 > SrS > FCl > C6H6 d. NH3 > FCl > SrS > C6H6 e. C6H6 > FCl > NH3 > SrS f. C6H6 > FCl > SrS > NH3
16. What is the hybridization at the nitrogen and starred carbon in the following molecule?
a. Sp3, Sp3 b. Sp2, Sp2 c. Sp, Sp d. Sp3, Sp2 e. Sp2, Sp3 f. Sp2, Sp g. Sp, Sp2 h. Sp3, Sp i. Sp, Sp3
17. Using the structure above, what is the electron-pair geometry of the starred carbon?
a. Linear b. Trigonal planar c. Tetrahedral d. Trigonal pyramidal
18. What is the molecular geometry of the central atom in XeF4? a. Linear b. Trigonal Planar c. Tetrahedral d. Bent e. Square Planar f. Trigonal Pyramidal
19. _____________ is a bonding theory based on the mixing of atomic orbitals of similar shapes and energies to form molecular orbitals that belong to the molecule as a whole.
HB DD Ionic LDF
Ionic > HB > DD > LDF
0 111 n 2
He CIN : C O
O H
c o
• . -
Molecular Orbital theory
a. Valence bond theory b. Hybridization c. Molecular orbital Theory d. Atomic Theory e. Big Bang Theory
20. What is the molecular geometry of SeH ? a. Linear b. Trigonal Planar c. Tetrahedral d. Bent
21. Which of the following is a nonpolar molecule?
HF, CHCl , H O, C H
a. CHCl b. C H c. HF d. H O
22. Which would dissolve best in H2O? a.
23. The strongest intermolecular force that would occur between C13H27OH molecules is _________, and the molecules interact primarily by _________ IMFs. (LDF = London Dispersion Forces; HB = Hydrogen Bonding; DD = Dipole-Dipole forces)
a. LDF, DD b. LDF, HB c. DD, LDF d. HB, DD e. HB, LDF
24. In each of the following pairs of compounds, which compounds is likely to be more soluble in CCl ?
a. NaBr b. CS c. CH CH OH d. KOH e. CH F
25. Which of the following compound is likely to be most soluble in water? a. NaCl b. KI c. CHCl d. CH OCH e. MgO
26. Which of the following would mix with (dissolve in) benzene (C6H6)? a. CH3OH
O
se--6
0
Ionic TNP which means best one is a nonpolar molecule NP
, LDF
HB
Ionic
DD
O DD - Polar Np
b. HCN c. HI d. Br2
27. Which of the following has the lowest vapor pressure? a. CH3OH b. CH3CH2CH3 c. C2H2 d. HBr e. NO32-
28. True or False: Both nitrogens in N2O3 have a steric number of 3, and the same molecular geometry.
a. True b. False
29. How many resonance structures exist for S3 (that most correctly depict its structure)?
a. One b. Two c. Three d. Four
30. There is (are) _____ double bond(s) and a total of ____ lone pairs in O . a. One, two b. Two, two c. One, six d. Two six
Determine which intermolecular force is the strongest in each compound:
a. London-dispersion forces b. Dipole-Dipole Forces c. Hydrogen Bond
31. HCl 32. SiO2 33. CF4 34. CH3OH 35. Which of the following is the correct geometry shape of Bromine
Pentahydride?
a. Square pyramidal b. Octahedral c. Trigonal Pyramidal d. T-shaped
36. Which of the following is an example of an intramolecular force? a. London Dispersion Force b. Dipole-Dipole Force
-polar ,DD - DD
, Polar O - NP , LDF
O -HB strongest Ints , highest BP - lowest Vapor-LDF Pressure - LDF - DD - Np
=÷%÷?o-trigonal ManorBent
3@
33 . 34.
O
c. Hydrogen bond d. Covalent bond e. Ionic bond f. All of the above g. A, B, and C h. D and E
37. A beaker of pure CH NH a e f g IMF : a. LDF b. Dipole-dipole c. Hydrogen Bond d. A & B only e. B & C only f. All of the above g. Ionic Bond
38. The electron geometry of CH F is __________, and its molecular geometry is _________.
a. Linear, linear b. Tetrahedral, Trigonal Pyramidal c. Tetrahedral, Bent d. Tetrahedral, Tetrahedral e. Trigonal planar, Trigonal pyramidal f. Octahedral, Seesaw
39. H2O has an electron geometry (electron domain) of ________, and its molecular geometry is ________.
a. Tetrahedral, Tetrahedral b. Tetrahedral, Trigonal Pyramidal c. Tetrahedral, Bent d. Tetrahedral, Linear
41. How many sigma and Pi bonds are in C H ? a. 3 sigma bonds, 2 Pi bonds b. 3 sigma bonds, 1 Pi bond c. 2 sigma bonds, 2 Pi bonds d. 1 sigma bond, 0 Pi bond
O ⇐4
- N , - H Nts
2
30,2T