AP Summer Assignment
Chapters 1-3 AP Exam Questions Worksheet
Part I: Multiple Choice
Directions: Answer the following questions by placing the letter of your choice on a separate sheet of paper to be handed in with your work packet
1. Which of the following properties generally decreases across the periodic table from sodium to chlorine?
a. First ionization energy
b. Atomic mass
c. Electronegativity
d. Maximum value of oxidation number
e. Atomic mass
2. The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following?
a. Na has a greater density at standard conditions than Ne
b. Na has lower first ionization energy than Ne.
c. Na has a higher melting point than Ne
d. Na has a higher neutron to proton ratio than Ne
e. Na has fewer naturally occurring isotopes than Ne
3. Which of the following characteristics is common to elemental sulfur chlorine, nitrogen, and carbon?
a. They are gaseous elements at room temperature
b. They have oxides that are acid anhydrides
c. They have perceptible color at room temperature
d. They form ionic oxides
e. They react readily with hydrogen at room temperature
4. A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of….
a. Cu c. Fe e. Zn
b. Mn d. Ni
5. A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made.
Mass of metal = 19.611 grams
Volume of water before addition of metal = 12.4 milliliters
Volume of water after addition of metal = 14.9 milliliters
The density of the metal, when correctly rounding using sig. figs, should be reported as:
a. 7.8444 grams per mL d. 7.8 grams per mL
b. 7.844 grams per mL e. 8 grams per mL
c. 7.84 grams per mL
6. Which of the following techniques is most appropriate for the recovery of solid KNO3 from an aqueous solution of KNO3?
a. Paper chromatography
b. Filtration
c. Titration
d. Electrolysis
e. Evaporation to dryness
7. A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following could the solid be?
a. CaCO3 d. AgCl
b. BaSO4 e. Zn(OH)2
c. Pb(NO3)2
8. Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does not liberate heat when water is added to it?
a. KNO3 d. H2SO4
b. NaOH e. Na
c. CaO
9. When a solution of sodium chloride is vaporized in a flame, the color of the flame is:
a. Blue d. violet
b. Yellow e. white
c. Green
10. All of the halogens in their elemental form at 25oC and 1 atm are
a. Conductors of electricity
b. Diatomic molecules
c. Odorless
d. Colorless
e. Gases
11. Which of the following represents an acceptable laboratory practice?
a. Placing a hot object on a balance pan
b. Using distilled water for the final rinse of a buret before filling it with standardized solution
c. Adding a weighted quantity of solid acid to a titration flask wet with distilled water
d. Using 10 mL of standard strength phenolphthalein indicator solution for titration of 25 mL of acid solution
e. Diluting a solution in a volumetric flask to its final concentration with hot water
12. Which of the following substances is LEAST soluble in water?
a. (NH4)2SO4
b. KMnO4
c. BaCO3
d. Zn(NO3)2
e. Na3PO4
13. Consider the element indium, atomic number 49, atomic mass 114.8g. The nucleus of an atom of indium 112 contains.
a. 49 protons, 63 neutrons, 49 electrons
b. 49 protons, 49 neutrons
c. 49 protons, 49 alpha particles
d. 49 protons, 63 neutrons
e. 49 protons, 112 neutrons
14. How many grams of potassium are in 21.9 g of K2CrO7?
a. 3.54 g
b. 1.120 g
c. 7.07 g
d. 78.2 g
e. 43.8 g
15. Suppose you are given the percent mass of the elements in a compound and you wish to determine the empirical formula. Which of the following is true?
a. You must convert percent by mass to relative numbers of atoms
b. You must assume exactly 100.0 g of the compound
c. You must divide all of the percent by mass numbers by the smallest percent by mass
d. You cannot solve for the empirical formula without the molar mass
e. At least two of the above is true
Part II: Short Answer and Problems
Directions: Show all work and solve the following problems
1. The postulates of the Bohr model of the hydrogen atom can be stated as follows:
I. The electron can exist only in discrete states each with a different energy
II. The electron can exist only in certain circular orbits
III. Radiation is emitted by the atom only when an electron makes a transition from a state of higher energy to one of lower energy
a. State whether each of the postulates is currently considered to be correct, according to the wave mechanical model description of the hydrogen atom
b. Give the wave mechanical description that has replaced one of the postulates now considered to be incorrect
2. Use the details of modern atomic theory to explain each of the following experimental observations
a. Within a family such as the alkali metals, the ionic radius increases as the atomic number increases
b. The radius of the chlorine atom is smaller than the radius of the chloride ion, Cal-
c. The first ionization energy of aluminum is lower than the first ionization energy of magnesium (Mg = 7.6, Al = 6.0)
d. For magnesium the difference between the second and third ionization energies is much larger than the difference between the first and second ionization energies (Ionization energies for Mg 1st = 7.6, 2nd = 14, 3rd = 80)
3. Account for each of the following in terms of principles of atomic structure, including the number, properties, and arrangements of subatomic particles.
a. The second ionization energy of sodium is about three times greater than the second ionization energy of magnesium
b. The difference between the atomic radii of Na and K is relatively large compared to the difference between the atomic radii of Rb and Cs
c. A sample of nickel chloride is attracted into a magnetic field, whereas a sample of solid zinc chloride is not
d. Phosphorous forms the fluorides PF3, and PF5, whereas nitrogen only forms NF3.
4. The empirical formula of styrene is CH; its molar mass is 104.1 g/mol. What is the molecular formula of styrene?
5. Adipic acid contains 49.32%C, 43.84%O, and 6.85% H by mass. What is the empirical formula?
6. A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is X? (Choices are: He, C, F, S, or none of these)