WorksheetsAP Chem Unit 10 Mock Exam
Total questions: 30
Worksheet time: 45mins
Of the following molecules, which has the smallest dipole moment?
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N2
CH4
HBr
NO
•It melts at 320° Celsius
•It does not conduct electricity as a solid.
•It conducts electricity in an aqueous solution.
C6H12O6(s)
NaOH(s)
Cdiamond(s)
Cu(s)
Sigma AND Pi bonding occurs in each which of the following?
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CO32-
NH4+
O2
CH2O
Which of the following best helps to explain why the value of ΔH° for the dissolving of CaF2 in water is positive?
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Ca2+ ions have very strong ion-dipole interactions with water molecules in the solution, illustrated in Step 3.
Ca2+ ions have very strong ion-ion interactions with F- ions in the crystal lattice, illustrated in Step 2.
H2O molecules have strong dipole-dipole interactions known as hydrogen bonding, illustrated in Step 1.
Which of the following steps in the solution process is the value of ΔH° for that step positive?
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Step 1
Step 2
Step 3
For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily?
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SO2
SO3
I3-
H2O
Organize the bond angles in H2O, NH3, and CH4. Explain.
H2O < NH3 < CH4
Unshared pairs of electrons repel more strongly than bonded pairs.
H2O < NH3 < CH4
The hybridization of the central atom decreases with decreased core charge.
CH4 < NH3 < H2O
The hybridization of the central atom increases with increased core charge.
CH4 < NH3 < H2O
Bonded pairs of electrons repel more strongly than unshared pairs.
Consider the molecule below. Determine the molecular geometry at each of the 2 labeled atoms.
1 = tetrahedral
2 = bent
1 = tetrahedral
2 = tetrahedral
1 = trigonal planar
2 = bent
1 = trigonal planar
2 = tetrahedral
I2 is more polarizable than H2 and, thus, have stronger London dispersion forces.
I2 is less polarizable than H2 and, thus, have weaker London dispersion forces.
I2 has a smaller permanent dipole than H2 and, thus, have weaker dipole-dipole forces.
I2 has a larger permanent dipole than H2 and, thus, have stronger dipole-dipole forces.
How do the molecular geometries and polarities of the two molecules compare?
CO2 is linear and non-polar.
H2O is bent and polar.
CO2 is linear and polar.
H2O is bent and non-polar.
CO2 is linear and polar.
H2O is linear and polar.
CO2 is bent and polar.
H2O is bent and polar.
Consider the following ionic compounds BaO NaCl KCl MgO Order from lowest to highest melting point:
KCl < NaCl < BaO < MgO
KCl < NaCl < MgO < BaO
MgO < BaO < KCl < NaCl
NaCl < MgO < KCl < BaO
H2O
BP=100°C
CH3OH
BP=64.96°C
CH3CH2OH
BP=78.5°C
CH3CH2–O–CH2CH3
BP=4.5°C
B with single bonds.
In the reaction,
NO + O3 → NO2 + O2
the N atom in the NO molecule must strike a terminal O atom in the O3 molecule. Which of the diagrams below would most likely result in the formation of the products?
NO CALCULATOR:)
For the reaction
2A + B → products
use the experimental data provided to determine the rate law.
rate = k [A] [B]
rate = k [A]
rate = k [A] [B]0
rate = k [A]2
A 50.0mL sample of an acid, HA, of unknown molarity is titrated, and the pH of the resulting solution is measured with a pH meter and graphed as a function of the volume of 0.100M NaOH added. Based on the data, which of the following is the approximate molar concentration of the unknown acid, HA?
0.0800M
0.125M
0.800M
0.0125M
Giant molecules, such as diamonds, in which each atom forms strong covalent bonds with all of its neighboring atoms lends what characteristics to covalent network substances?
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Shared electrons.
Low melting points.
Very hard substances.
Poor conductivity.
Transfer of electrons to form ions.
Which of the following would make a strong electrolyte when dissolved in water?
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CH3COCH3
NaNO3
C6H12O6
HCl
Identify all types of intermolecular attractive forces present in pyridine.
London Dispersion Forces
Dipole-Dipole Attractions
Hydrogen Bonding Attractions
Ion-Dipole Attractions
Identify all types of intermolecular attractive forces present in benzene.
London Dispersion Forces
Dipole-Dipole Attractions
Hydrogen Bonding Attractions
Ion-Dipole Attractions
Solubility of Pyridine in Water at 25oC
54.5g per 100mL of water
Solubility of Benzene in Water at 25oC
0.00452g per 100mL of water
Explain the solubility difference between pyridine and benzene in water.
The intermolecular forces between molecules of pyridine and water must be STRONGER than the intermolecular forces between molecules of benzene of water because pyridine is MORE soluble than benzene in water.
The intermolecular forces between molecules of pyridine and water must be STRONGER than the intermolecular forces between molecules of benzene of water because pyridine is LESS soluble than benzene in water.
The intermolecular forces between molecules of pyridine and water must be WEAKER than the intermolecular forces between molecules of benzene of water because pyridine is MORE soluble than benzene in water.
The intermolecular forces between molecules of pyridine and water must be WEAKER than the intermolecular forces between molecules of benzene of water because pyridine is LESS soluble than benzene in water.
What is the strongest type of intermolecular or intramolecular attractive force that must be overcome for the decomposition of ammonia, NH3?
2NH3(g) → N2(g) + 3H2(g)
Hydrogen Bonding Attractions
Dipole-Dipole Attractions
London Dispersion Forces Attractions
Covalent Bonds
Ion-Dipole Attractions
What is the strongest type of intermolecular or intramolecular attractive force that must be overcome for the vaporization of ammonia, NH3?
NH3(l) → NH3(g)
Hydrogen Bonding Attractions
Dipole-Dipole Attractions
London Dispersion Forces Attractions
Covalent Bonds
Ion-Dipole Attractions
