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Chemistry MSL Practical Style Review 1. What is the nuclear composition of uranium-235? A B C D 92 electrons + 143 protons 92 protons + 143 electrons 143 protons + 92 neutrons 92 protons + 143 neutrons 2. Which best describes the relationship between subatomic particles in any neutral atom? A B C D The number of protons equals the number of electrons. The number of protons equals the number of neutrons. The number of neutrons equals the number of electrons. The number of neutrons is greater than the number of protons. 3.What is the name of the compound PbO ? A B C D lead oxide lead(II) oxide lead oxide(II) lead(IV) oxide 4. What is the chemical formula for calcium nitrate? A B C D CaNO3 Ca(NO2)2 Ca(NO3)2 Ca3N2 5. Which is the correct formula for dinitrogen pentoxide? A B C D N4O NO2 N2O5 NO4 6. What is the pressure, in atmospheres, exerted by a 0.100-mol sample of oxygen in a 2.00-L container at 273C? A B C D 4.48 x10-1 atm 2.24 x 100 atm 1.12 x 103 atm 2.24 x103 atm 7. Based on the VSEPR theory, what is the molecular geometry of a molecule of PI3 ? A B C D linear tetrahedral trigonal planar trigonal pyramidal 8. Which substance listed in the table is a liquid at 27 C? I II III IV A B C D Melting Point 28C -10C 20C -90C Boiling Point 140C 25C 140C 14C I II III IV 9. The total pressure in a closed vessel containing N2, O2 and CO2 is 30 atm. If the partial pressure of N2 is 4 atm, and the partial pressure of O2 is 6 atm, what is the partial pressure of CO2? A B C D 20 atm 30 atm 40 atm 50 atm 10. What type of bonding is associated with compounds that have the following characteristics: •high melting points •conduct electricity in the molten state •solutions conduct electricity •normally crystalline solids at room temperature. A B C D covalent ionic hydrogen metallic 11. Consider this reaction: NH3 (g) + HCl (g) → NH4Cl (s) Which type of reaction does this equation represent? A B C D combustion decomposition single replacement synthesis 12. What products are formed when the metal potassium is added to water? A B C D K and H2O KOH and H2O K2O and H2 KOH and H2 13. What coefficients are required to balance this equation? _Fe2O3 _CO _Fe _CO2 A B C D 2, 6, 3, 6 1, 3, 2, 3 1, 1, 2, 2 1, 1, 2, 1 14. An aqueous solution of silver nitrate is added to an aqueous solution of iron (II) chloride. Which is the net ionic equation for the reaction that occurs? A B C D AgNO2 (aq) + FeCl (aq)→ AgCl (s) + FeNO2 (aq) 2AgNO3 (aq) + FeCl2 (aq)→2AgCl (s) + Fe(NO3)2 (aq) 2Ag+1 (aq) + NO3-1 (aq) + Fe+2 (aq) + Cl2 (g)→ 2AgCl (s) 2Ag+ (aq) + 2Cl- (aq)→ 2AgCl (s) 15. Consider this chemical equation: NH3 (aq) + HCl (aq) NH4+ (aq) + Cl- (aq) In this reaction, why is the ammonia considered a base? A B C D NH3 increases the hydronium ion concentration. NH3 decreases the hydroxide ion concentration. NH3 accepts a proton. NH3 donates a proton. 16. What is the pH of a solution of KOH with a hydroxide concentration of [OH] = 1 × 10−4 M? A B C D - 10 -4 4 10 17. In a titration experiment, if 30.0 mL of an HCl solution reacts with 24.6 mL of a 0.50-M NaOH solution, what is the concentration of the HCl solution? A B C D 0.41 M 0.61 M 1.5 M 370 M 18. For the reaction A+ (aq) + B- (aq) → AB (s) increasing the temperature increases the rate of the reaction. Which is the best explanation for this happening? A B C D The pressure increases, which in turn increases the production of products. The concentration of reactants increases with an increase in temperature. The average kinetic energy increases, so the likelihood of more effective collisions between ions increases. Systems are more stable at high temperatures. 19. Which is a unique characteristic of the bonding between metal atoms? A B C D Atoms require additional electrons to reach a stable octet. Atoms must give away electrons to reach a stable octet. Atoms share valence electrons only with neighboring atoms to reach a stable octet. Delocalized electrons move among many atoms creating a sea of electrons. 20. Consider this phase diagram: At what temperature does the normal boiling point occur? A B C D 45°C 60°C 100°C 110°C