Review sheet for AP Chemistry midterm
1. The formula of the precipitate from the reaction between Zinc Sulfate and Tin(II) Fluoride is
2. A sample of solution has a mixture of 0.01 M Aluminum Chloride and 0.05 M Magnesium
chloride, what is the molarity of Silver Chloride that is required to precipitate all the chloride
ions present in the solution is
4. 50 grams of Aluminum Sulfate is dissolved in 500 mL of water the particle concentration of
Aluminum and Sulfate ions are
6. If 4.2 grams of Magnesium carbonate produced only 1.5 grams of Carbondioxide, then what
is %purity of Magnesium carbonate.
8. Name the cations and anions whose aqueous solutions are always soluble.
9. What is volume of 0.05 Molar Sulfuric acid required to neutralize 20 mL of 0.1 Molar Sodium
Hydroxide.
13. Dichromate ion reacts with Nitrate ion in acid medium and form nitrate, Chromium(III) ion
and water. Write the ionic equation. What is the ion that is oxidized? What is the oxidation
state of Chromium in Dichromate ion? Balance the equation. In the above process 46 mL of
0.062 molar Dichromate was initially used to react with nitrate. The remaining
dichromate(excess) is determined by using 19.3 mL of 0.22M of Iron(II)nitrate and the reaction
is given as below.
6 Fe2+(aq) + Cr2O72-(aq) + 14 H+(aq)  2 Cr3+(aq) + 6 Fe3+(aq) + 7 H2O(l)
Calculate the moles of Dichromate reacted with nitrate ion, excess dichromate left.
19. how many atoms of each element are present in 1 mole of potash alum.
20. 3.42 grams of sucrose is dissolved in 100 mL solution, the molarity is
21. Potassium permanganate reacts with oxalic acid in acid medium to produce Carbondioxide,
how many moles of Carbondioxide are produced by the reaction of 40 mL of 0.4 M Potassium
permanganate and 100 mL 0.2 M Oxalic acid.
22. 1 Liter each of 2M Barium Chloride and 1M Potassium sulfate are mixed together, assuming
the volumes are additive. The contents of the final mixture and their molarities are
2. Give two examples of iso- electronic species
4. Why is the ionization energy of Potassium less than Argon, explain with atomic size and
effective nuclear charge.
5. Write the orbital notation electron configuration of a) Inert/Noble gas b)An element in Carbon
family c) excited state electron configuration of Hydrogen
6. Successive ionization energies of an element in K.Joules/mole are 590, 1145, 4912, 6491,8153
etc, then the element could be ________
7. Rutherford’s conclusions are
8. Paramagnetism in Nitrogen element is because it has three unpaired electrons, this
configuration of Nitrogen is in accordance with Aufbau/Pauli/Hund’s rule.
9. State all three above principles.
10. State Heisenberg uncertainty principle.
12. Calculate the wavelength/ Frequency and energy of 2nd line and Series limit in Balmer series.
13. Calculate the wavelength of proton moving at a speed of 70% of speed of light.
14. The 1st and 2nd ionization energy values in K.Joules/mole are given as follows. For Sodium
460 and 4562. For Magnesium are 738 and 1451. Explain why is the first ionization energy
Magnesium is higher than Sodium and Second Ionization energy of Sodium is higher than Mg.
19. Hydrogen molecule absorbs a photon of frequency of 3.00 × 1015 Hz. Calculate how much
energy is absorbed by Hydrogen in Joules. If the bond dissociation energy( energy required to
break the bond) of Hydrogen is 437 K. Joules/mole. Does this photon have enough energy to
break the bond. Justify your answer with calculations.
20. Is the energy required to remove an electron from 1s orbital of Sulfur and Chlorine same? Or
different? Explain.
21. The atomic radius and ionization energy of Magnesium are 79 pm and 737 K. Joules/mole,
then that of Sodium are
22. Compare the ionization energies of Neon and Fluorine. Justify your answer.
24. Arrange Be, N and F in the order of their atomic radius.
26. Write the excited state electron configuration of Sodium.
27. Why is 𝐶𝑙 − smaller than 𝑆 −2
1. The hybridization of Carbon atoms in Methane, Ethane, Ethene(Ethylene), Ethyne
(Acetelyne), Propene, Benzene, C2H4Cl2 C2H2Cl4 is and draw their Lewis Structures. Calculate
the number of sigma and pi bonds. Among Ethane, Ethene and Ethyne which C-C bond length
and C-C bond energy is maximum.
2. Give few examples of molecules that exhibit resonance and draw structures with the correct
geometries
3. Take few examples like CO2, SO2, BCl3, PCl3 of polar covalent bonds and find which one is
more polar. Justify. Also the draw their geometries, examine if the molecule has any net bond
moment. Justify.
4. Per VSEPR Theory write the examples of the molecules with different molecular geometries
starting at 2 electron pairs and all the way up to 7 electron pairs.
5. How will you know if the compound has ionic or covalent or both the bonds?
6. Give examples of molecules with square pyramidal geometry.
7. How is the solubility of ionic and covalent compounds determined? Give examples
8. Justify the geometries of Methane, Ammonia and water molecules and explain the bond
angles.
10. Write the geometries of all different types of hybridizations and give an example each.
11. Among NCl3, PCl3 and CHCl3, which molecules are planar? Draw their geometries.
12. Write different geometries in which all the bond angles are same and bond angles are
different. Give examples.
13. Write the Lewis structures of O3, Formate (𝐻𝐶𝑂2− ) and calculate their bond orders.
14. How is the bond dissocation and bond energies of reactants and products compared in
exothermic and endothermic reactions.
17. What is the hybridization, geometries, hybridizations and polarity of PCl3 PCl5
18. Draw the Lewis structures, hybridizations, geometries, number of sigma and pi bonds in
Acetic acid, acetate ion, CO2, HCN, SO3
20. Give two examples of compounds with both ionic and covalent bonds.
21. PCl5 exist, NCl5 does not exist. Justify.
26. Identify the hybridization of Carbon atoms in Ethanol(Ethyl alcohol) and Acetic
acid(ethanoic acid). Draw their Lewis structures. What are your observations on the bond length
of Acetate ion, justify your answer with the Lewis structures.
4. How does speed depend on pressure, temperature and nature of the gas?
5. Write the equation to calculate number of moles and density using pressure and temperature of
a gas? Work out an example from textbook or online?
6. 5 Liters of Carbon dioxide and 3 Liters of Helium at 1 atm pressure is introduced into 2 Liters
flask keeping the temperature constant. What is the new pressure of gases in the tank.
8. Under what conditions gases behave ideally?
9. How many moles of Sulfur trioxide is required to make 1 Liter of Oxygen at STP?
10. Calculate the pressure of 2 moles of an ideal gas at 250C, 740 mm pressure.
16.The mass of a sealed 1 liter rigid flask that contained dry air is 160 grams and with the unknown gas
without dry air is 165 grams. Both the air and the unknown gas were at 25.0 oC and 730. torr. Calculate
the mass, in grams, of the dry air that was in the sealed flask. (The density of dry air hypothetically is 1.g
L-1 at 25 oC and 730. torr.). Calculate the mass, in grams, of the sealed flask itself (i.e., if it had no air in
it). Calculate the mass, in grams, of the unknown gas that was added to the sealed flask. Calculate the
value of the molar mass of the unknown gas.
After the experiment was completed, the instructor informed the student that the unknown gas was
carbon dioxide (44.0 g mol-1). Calculate the percent error in the value of the molar mass calculated.
17. What are the temperature and pressure conditions for the ideal behavior of a real gas?
18. What is the effect of temperature of average kinetic energy and the average speed?
19. 32 grams of the sample of a gas has a pressure of 4 atm. At 273K, the gas could be
20. How does speed of the gas depends on its nature and temperature?
21. The pressure of a gas enclosed in 10 liter vessel is 3 atm. Calculate the pressure if the volume is
decreased to 5 liters.
22. The molar heat of vaporization of a gas with molar mass 16 is 8.2 k.J/mol, what is the energy
required to vaporize 64 g?
23. Why is the heat of vaporization greater than heat of fusion?
24. Why is the heat of vaporization of water greater than methane?
32. A solid – Liquid exist in equilibrium with each other, the temperature does not change on melting or
boiling, justify the constancy of the temperature.
33. Write the formula of all the compounds formed between Cl and F. Draw the Lewis structure of 𝐶𝑙𝐹3 .
What is the molecular shape of the above compound, justify on the basis of dipole moment. What
happens to the number of halogen atoms attached to Cl, Br and I as we move down the group.