Download Semester 2 review questions

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Chemistry I: Semester Review Questions – The Mole and Stoichiometry
1. How many particles of CO2 are present in 245 g of CO2?
2. How many liters of oxygen gas at STP are required to react with 65.3 g of aluminum in the
production of aluminum oxide?
3. Copper reacts with silver nitrate to form silver and copper(II) nitrate. How many grams of
copper are required to react with 50.0 mL of 8.0M AgNO3?
4. A substance is found to be composed of 70.58% Carbon, 5.93% Hydrogen, and 23.49% Oxygen.
Find the empirical formula for the substance.
Empirical Formula ____________________
5. Given that the substance above has a molar mass of 204.24 g/mole, find the molecular formula of
the substance. Show your work.
Molecular formula:
6. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. How many liters
of 3.75 M HCl are needed to fully react with 165.53 g of zinc?
7. For ZnCl2, calculate the Percent Composition of each element.
Data Table: The Reaction between Tin(II) Nitrate and Aluminum
Mass of Empty Beaker
Mass of beaker and Tin (II) Nitrate
Trial 1
34.56 g
78.84 g
Mass of Aluminum metal
6.45 g
Mass of beaker and Tin (Sn) Metal after reaction
64.76 g
1. Balance the following Equation:
_____ Sn(NO3)2
+
_____ Al

_____ Al(NO3)3
+
_____ Sn
2. Determine the Mass of Aluminum metal and Tin(II) Nitrate used in this reaction.
3. Using the information from question (2) and the balanced equation, calculate the theoretical amount
of Tin (Sn) that should have been produced from this reaction. (hint: determine the limiting
reactant)
Theoretical yield =_________________________, Limiting reactant = ______________
4. Using the above data table, calculate the actual amount of Tin (Sn) produced from the reaction.
5. Using the information from questions 3 & 4, calculate the percent yield of Tin for the reaction.
Based on your answer to #3 (the limiting reactant), find out how much of the excess reactant should be
left at the end of the experiment.
Chemistry I: Semester Review Questions – Electron Configuration
NAME THE TERM DESCRIBED BY THE FOLLOWING DEFINITIONS:
1. A packet of light energy that carries a quantum of energy.
2. The state when all electrons of an atom are in the lowest possible energy levels.
3. When an electron jumps up to a higher energy level, the atom is in its ___.
4. The scientist who applied Einstein’s particle-wave theory to electrons.
5. The theory that it is impossible to know both the position and speed of an electron
simultaneously.
6. The theory that no two electrons in an atom can share the same 4 quantum numbers.
7. The theory that electrons fill the lowest energy orbitals first.
8. The theory that, within a sublevel, electrons prefer to occupy their own orbital.
9. A term describing the outermost electrons in an atom.
10. A positively charged ion is called a(n) ___. A negatively charged ion is called a(n) ___.
11. The most stable type of electron configuration.
12. A three-dimensional region in space where an electron is likely to exist.
DRAW ORBITAL DIAGRAMS (boxes) FOR THE FOLLOWING ELEMENTS AND GIVE THE
FOUR QUANTUM NUMBERS FOR THE LAST ELECTRON:
13. Mg
14. Si
15. Ti
WRITE LONGHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
16. N
17. K
18. Cr
WRITE SHORTHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
19. Sb
20. Bi
21. Tc
22. Ge
Chemistry I: Periodic Trends Semester Review Questions
Answer the following questions. (Correct any false statements).
1. ____________________ was a Russian chemist who arranged the known elements in vertical columns in order
of increasing mass and noticed a pattern in physical and chemical properties.
2. ____________________ was a British physicist who determined the atomic number (number of protons in the
nucleus)of the atoms of elements and then arranged the elements according to their atomic number.
3. _____(T/F) The modern periodic table arranges the elements in order of increasing atomic number.
4. ___________________ are the horizontal rows of the periodic table.
5. __________________ or ___________________ are the vertical columns of the periodic table.
6. _____(T/F) The elements in a period have similar chemical and physical properties.
7. _____(T/F) The characteristic properties of the elements in a group change from period to period.
8. Circle the element below that would most similar in chemical and physical properties as calcium:
potassium
iron (Fe)
bromine (Br)
beryllium
sodium
9. Underline the element above that would be most different from calcium.
10. Label the following diagram with s, p, d, and f and then match the characteristics listed below with the letters
s, p, d and f.
_____ contains the noble (inert) gases
_____ contains the alkali metals
_____ contains most of the nonmetals
_____ contains the transition metals
_____ contains the alkaline earth metals
_____ contains the lanthanide and actinide series (inner transition elements)
_____ Representative elements (2 blocks)
_____ group 1, 2 and helium
_____ 13, 14, 15, 16, 17 and 18
11. State the periodic law:
Answer the following questions by filling in the blank.
1. __________ Determine the number of valence electrons in the following element:
[Ne]3s23p2
2. __________ How many valence electrons does column 13 contain?
3. __________Determine the number of valence electrons in the following element:
[Ar]4s23d104p5
4. __________What is the valence electron configuration for any element in group 2?
5. __________ What energy level are Bromine’s valence electrons in?
6. Period:__________ Given the following configuration: [Ar]4s23d104p2; what period
and block is the last valence electron found in?
Block:___________
7. ___________The electron configuration for an element is: [Ar]4s23d104p5 What family
does it belong to?
Fill in the blank with the correct choice, (A, B, or C) from the given list.
A. Increase
B. Decrease
C. Stay the same
8_____ As you move left to right in a period, atomic size will…
9_____ As you move up a group, 1st ionization energy will…
10_____ As you move from Iodine to Fluorine, electronegativity will…
11_____ As you move from Scandium to Zinc, shielding will…
12_____ As you move down a group, atomic size will…
13_____ The size of a positive ion compared to the neutral atom will…
14_____ As you move from Sodium to Cesium, shielding will…
15_____ The size of a negative ion compared to the neutral atom will…
16_____ As you move from right to left in a period, 1st ionization energy will…
17_____ As you move left and down, electronegativity will…
Use the Ionization Energies listed in the data table below to answer the following questions.
Element
1st
2nd
3rd
4th
5th
6th
Xq
650
1320
2745
12756
----18__________ What is the value of the third ionization energy?
19__________ How many valence electrons does element Xq have?
Give the name for the following compounds
23. BaSO3
29. AgNO3
24. (NH4)3PO4
30. Fe2O3
25. MgSO4
31. HClO
26. CaO
32. N2O3
27. H3PO4
33. HF
28. MnO
34. NaHCO3
WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS:
35. hydrobromic acid
42. diphosphorus pentoxide
36. chromium(III) carbonate
43. sulfurous acid
37. magnesium sulfide
44. lead(II) nitrate
38. iodine trichloride
45. dihydrogen monoxide
39. lithium hydride
46. sodium oxalate
40. ammonium hydroxide
47. perchloric acid
41. calcium chloride
48. chlorous acid
Chemistry I: Covlent bonding Semester Review Questions
For each of the following molecules, draw the Lewis Diagram.
MOLECULE
1. OF2
2. CO32-
3. CI4
LEWIS DIAGRAM
Chemistry I: Gas law Semester Review Questions
FOR EACH OF THE FOLLOWING, NAME THE GAS LAW AND SOLVE THE PROBLEM:
1. Hydrogen is collected over water at 0.975 atm and 28C. What is the partial pressure of H2? Water
has a partial pressure of .0349 atm.
2. How many moles of chloroform, CHCl3, are required to fill a 253-mL flask at 100.0C and 940 torr?
3. You want the pressure inside a bottle to be 75.0 kPa at 23C. At what temperature in Celsius should
you seal the bottle when the pressure is 1.12 atm?
4. A diver’s lungs hold about 20.0 L of air underwater at a pressure of 875 mm Hg. Assuming he holds
his breath and his lungs don’t burst, what will be the volume of air in his lungs at standard pressure
on the water’s surface?
5. What pressure is required to compress a gas that occupies 6500 L at 25C and 1.0 atm to a volume of
40.0 L at 18C?
6. When a canning jar is sealed at 100C the pressure inside is 101.3 kPa. What is the pressure inside
the jar when it cools to room temperature, about 21C?
7. CO2 gas is collected over water at 100.3 kPa and 19C. Find the pressure of the dry gas. Water has
a partial pressure of 2.23 KPa.
8. What is the temperature of a 0.00893 mol sample of neon gas that has a volume of 302 mL and a
pressure of 0.941 atm?
9. A gas occupies 4.78 L at 78.1 kPa and 25C. What will the volume be at 0.975 atm and 15C?
10. A shampoo bottle contains 443 mL of air at 65C. What is its volume when it cools to 22C?
11. A balloon is filled with helium to a volume of 12.5 liters at 25C and 101 kPa. How many grams of
helium are in the balloon?
12. Three gases are inside a room. If the total pressure of the gases is 1.01 atm and Hydrogen has a
pressure of 0.25 atm, Nitrogen has a pressure of 0.45 atm, and Oxygen is the only other gas in the
container, what is the pressure of the oxygen in the container?
13. Ammonia and Nitrogen gases are placed in the same room. Which gas will diffuse faster and how
many times faster will it be then the other gas?
SOLVE THE FOLLOWING GAS STOICHIOMETRY PROBLEMS:
14. What volume of chlorine is required to produce 25.4 g of copper(II) chloride at 18C and 2.13 atm?
Cu + Cl2  CuCl2
15. At 778 mm Hg and 25C, how many grams of zinc are required to produce 25.2 liters of hydrogen
gas?
__Zn + __HCl  __ZnCl2 + __H2
16. If 5.45 g of potassium chlorate decompose, how many liters of oxygen gas are given off at 1.58 atm
and 32C?
2KClO3  2KCl + 3O2
17. When aluminum is burned in 15.0 L of oxygen at 97.3 kPa and 21C, how many grams of aluminum
oxide are formed?
4Al + 3O2  2Al2O3
18. If 12.8 g of CaCO3 decomposes at 38C and 0.96 atm, how many dm3 of CO2 are formed in addition
to CaO?
CaCO3  CaO + CO2
REMEMBER: 1cm 3 = 1 mL & 1 dm3 = 1 L
Laws:
P1V1 P2V2

T1
T2
Ptotal = P1 + P2 + …
PV = nRT
R = 0.0821
atm  L
mol  K
or R = 8.314
KPa  L
mol  K