Download ap chemistry review – multiple choice

AP CHEMISTRY REVIEW – MULTIPLE CHOICE
Questions 1-4 refer to the following types of energy
(a) Activation Energy
(b) Free Energy
(c) Ionization Energy
(d) Kinetic Energy
(e) Lattice Energy
1. The energy required to convert a ground-state atom in the gas phase to a positive gaseous ion.
2. The energy change that occurs in the conversion of an ionic solid to widely spaced gaseous ions.
3. The energy in a chemical or physical change that is available to do useful work,
4. The energy required to form the transition state in a chemical reaction.
Questions 5-8 refer to atoms for which the occupied atomic orbitals are shown below:
(a) 1s ___
(b) 1s 
(c) 1s 
(d) 1s 
(e) [Ar] 4s
2s
2s
2s
2s



 2p 

_____
 2p 


3d 




5. Represents an element that is chemically unreactive.
6. Represents an atom in an excited state.
7. Represents an atom that has 4 valence electrons.
8. Represents an atom of a transition metal.
Questions 9-12 refer to the following descriptions of bonding in different types of solitds.
(a) Lattice of positive and negative ions held together by electrostatic forces.
(b) Closely packed lattice with delocalized electrons throughout.
(c) Strong single covalent bonds with weak intermolecular forces.
(d) Strong multiple covalent bonds (including pi bonds) with weak intermolecular forces.
(e) Macromolecules held together by strong polar bonds
9.
Cesium chloride, CsCl (s)
10. Gold, Au (s)
11. Carbon Dioxide, CO2 (s)
12. Methane, CH4 (s)
Questions 13-14 refer to the following elements
(a) Lithium
(b) Nickel
(c) Bromine
(d) Uranium
(e) Fluorine
13. Is a gas in its standard state at 298 K.
14. Reacts with water to form a strong base.
Questions 15-18 refer to the following
(a) Heisenbery uncertainty principle
(b) Pauli exclusion principle
(c) Hund’s rule (principle of maximum multiplicity)
(d) Shielding effect
(e) Wave nature of matter
15. Can be used to predict that a gaseous carbon atom in it ground state is paramagnetic
16. Explains the experimental phenomenon of electron diffraction.
17. Indicates than an atomic orbital can hold no more than 2 electrons.
18. Predicts it is impossible to determine simultaneously the exact position and the exact velocity of an electron.
Questions 19-21
(a) Ne
(b) Li
(c) Al
(d) Cl
(e) Ca
19. Which of the following elements above is most commonly found as a negatively charged ion?
20. Which of the elements above has the same electron structure as Mg2+
21. Which of the elements above is found as a diatomic gas in its uncombined state?
Questions 22-25
(a) H2O
(b) NH3
(c) CH4
(d) HF
(e) NH222. This molecule is nonpolar
23. This molecule does NOT exhibit sp3 hybridization.
24. The molecule has a trigonal pyramidal shape.
25. This substance does not exhibit any hydrogen bonding.
Questions 26-29 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all
concentrations are 1 M.
(a)
(b)
(c)
(d)
(e)
NH3 and NH4Cl
H3PO4 and NaH2PO4
HCl and NaCl
NaOH and NH3
NH3 and HC2H3O2 (acetic acid)
26. The solution with the lowest pH
27. The most nearly neutral solution
28. A buffer at a pH > 8
29. A buffer with a pH < 6