6th 6 Weeks Review

March 18, 2018 | Author: Brady Zhou | Category: Intermolecular Force, Chemical Equilibrium, Ion, Properties Of Water, Chemical Reactions


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Birenbaum6th 6 weeks review CH 11............................................................................................................................................................................... 2 CH 13 and 14 .................................................................................................................................................................. 5 CH 15 .............................................................................................................................................................................. 6 1 they all have 2 electrons in their valence shell ns2np5. electrons with his electron configuration are nonmetals.elements with this electron configuration are expected to form -1 anions. the noble gases exists as monoatomic gaseous atoms Cr3+=[Ar]3d3 Br5+=4f145d10 2 .2 cannot have the same spin Hund¶s rule.The effective nuclear charge acting on an electron is larger than the actual nuclear charge A tin atom has 50 electrons.violation last three boxes does not have one in all three Elements that readily conduct electricity are elements with low ionization energies Electron affinity measures how easily an atom gains an electron False. more reactive than Magnesium. elements with this electron configuration from acidic oxides Alkali metals tend to be more reactive than alkaline earth metals because alkali metals have lower ionization energies All of the following are ionic compounds except: SiO2 Hydrogen doesn¶t belong to any family In nature. smaller radius than Barium H2 is always produced when an active metal reacts with water Oxides of the active metals combine with water to form metal hydroxides Oxides of most non-metals combine with base to form water and a salt The reaction of a metal and a nonmetal produces a salt Atomic radius increases as we move down and left The atomic radius of main group of elements increase down a group because the principle quantum number of each valence orbitals increases First ionization of aluminum: Al(g) --> Al+(g)+ eSecond ionization of phosphorous: P+(g)--> P2+(g)+ eChlorine is more apt to exist as an anion than is sodium because chlorine has a greater electron affinity CO2 is the most acidic (out of some) Transition metal within a period differ mainly in the number of d electrons Not true about alkali metals.Birenbaum Ch7 y y y y y y y y y y y y y y y y y y y y y y y y y y y y Pauli Exclusion principle. Electrons in the 5p sub-shell experience the lowest effective nuclear charge The first ionization energies of elements increase as you go from left to right across the period and increases from top to bottom True.Halogens have the most negative electron affinities Sr.reacts with Cl to from SrCl2. The strongest interparticle attraction is between solids and the weakest interparticle attraction is between gasses. In liquids. What is the strongest intermolecular force in I2? London dispersion 11. Which substance has the highest boiling point? C2I6 C2H6 C2F6 C2Br6 C2Cl6 6. the atoms become more separated and they have less attraction for one another 4. 14. 18. What is the predominate intermolecular force in C12H26? London dispersion forces 17. The shape of a meniscus is determined by the relative magnitude of cohesive forces in the liquid and adhesive forces between the liquid and the container. 3. What is the predominate intermolecular force in (CH3) NH2? Hydrogen bonding 15. What is the strongest intermolecular force in CBr4? London dispersion forces 7. regardless of polarity are polarizable. 5. Crystalline solids have highly ordered structures 2. What is the intermolecular force between Na+ and H2O? Ion dipole 13.Birenbaum CH 11 1. What intermolecular force does hydrogen bonding fall under? Dipole 9. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. 3 . Which of the following is correct? All of them Viscosity increases with decreasing temperature Viscosity increases with increasing molecular weight Viscosity increases with increasing intermolecular forces 19. but not strong enough to keep molecules from moving past one another. As a solid element melts. What is the force responsible for ice being less dense than water? Hydrogen bonding 12. Large molecules. the attractive intermolecular forces are strong enough to keep molecules relatively close. Polarizability is the ease at which the change distribution in a molecule can be distorted by an external electric Field 10. Which should have the highest critical temperature? CBr4 Ch4 CCl4 H2 CF4 9.dipole attraction? XEF4 BCl3 AsH3 Co2 Cl2 3. Large intermolecular forces are manifested by which of the following? All of them High heat of fusion and vaporization Low vapor pressure High boiling point High critical temperature and pressure 30. How high a liquid will rise up a narrow tube as a result of capillary action depends on the magnitude of cohesive forces in the liquid and adhesive forces between the liquid and the tube. Which of the following exhibits dipole. 11. The property responsible for the ³beading up ³of water is surface tension. 7. What is the vapor pressure at the normal boiling point? 1atm 22. Covalent networks have a low melting point. The critical pressure is the pressure above which a substance is a liquid at all temperatures. Vapor pressure increases as molecular weight increases. 8. 10. softness. Which substance only has London dispersion forces as its intermolecular force? H2S CH4 CH3OH NH3 HCl 2. A volatile substance is one that readily evaporates. 12.Birenbaum 21. Wihixh of the following substances has the highest boiling point? H2O CH4 NH3 CO2 Kr 4. 23. and gravity 6. Some things take longer to cook at high altitudes than low altitudes because water boils at a lower temperature at higher altitudes than at lower altitudes. 33. What types of intermolecular forces exist between HI and H2S? Dispersion forces and dipole-dipole 5. Molecular solids consist of atoms or molecules held together by intermolecular forces. low electrical conduction False Additional questions from the quiz 1. The critical temperature is the temperature above which a gas can not be liquefied 4 . Freezing is an exothermic process. The distribution of water in octane (C8H18) is prevented by hydrogen bonding 12. As concentration of a solution increases freezing point decreases and vapor pressure decreases 3.Birenbaum CH 13 and 14 1. in . 5 . 8. A colloid is not a homogeneous mixture 4. In a saturated solution.100 moles of solution which of the following has the lowest vapor pressure? Al (ClO4)3 KCLO4 Ca (ClO4)2 NaCl sucrose 2. Increasing the temperature of a reaction leads to an increase in the reaction because more molecules more frequently and with greater force 17. Adding a nonvolatile solute to a solution decreases vapor pressure. A+B yields C+D (fast) B+D yields X (slow) D is the intermediate 5. 10. and collision energy. the crystallization rate=the rate of dissolution 15. Emulsifying agents are hydrophobic and hydrophilic. The phrases ³like dissolves in like´ refers to the fact that polar solvents and dissolve in polar solutes and nonpoar solvents dissolve in nonpolar solutes 14. Molality varies with temperature. 13. and the collision orientation. What is the most soluble in CCl4? C10H22 H2O NH3 CH3CH2OH NaCl 6. 11. A catalyst can increase the rate of the reaction by providing an alternate pathway to lower activation energy. The activated complex is the species that exists at the maximum point on the curve 18. The addition of a catalyst will lower activation energy. 7. 9. The rate of the reaction depends on the collision frequency. The unit of molality is moles/ kg 16. The formation of a solution in an endothermic process can be spontaneous by an increase in disorder. The equilibrium constant expression depends on the stochiometry of the reaction 5.4 kJ Le Chatelier s principle predicts that adding N2 (g) to the system at equilibrium will result in a decrease of the concentration of H2 (g) 6. the rates of the forward and reverse reactions are equal 2. Le Chatelier¶s principle states that if a system at equilibrium is disturbed. At equilibrium. What will the change the value of the equilibrium constant? Changing temperature 4. In an exothermic equilibrium reaction increasing the reaction temperature favors the formation of reactants True 3. 2NH3 (g) N2 (g) +3H2 (g) H =+92.Birenbaum CH 15 1. 2SO2 (g) +O2 (g) 2SO3 (g) H =-99 kJ Le Chatelier s principle predicts that increasing the temperature will decrease the partial pressure of SO3 (g) ***Most questions are in CH15 quiz*** 1. the equilibrium will shift to minimize the disturbance. effectively removing it and shifting the equilibrium to the right False 2. Q is the same as the Keq when Q=Keq 6. 2CO2 (g) 2CO (g) +O2 (g) H =-514kJ Le Chatelier s principle predicts that adding O2 (g) to the reaction will increase the partial pressure of CO2 (g) at equilibrium 7. 6 . Which of the following is correct concerning the Haber process? It is the process used for the synthesis of ammonia 3. At constant temperature reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles in the system False 4. The effect of a catalyst on a chemical reaction is to react with the product. True 5. The effect of a catalyst is to increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture.
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