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test_III_blue - Name: Class: Date: CHEM 1211 Test III...

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Unformatted text preview: Name: Class: Date: CHEM 1211 Test III Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following statements is CORRECT? - If a reaction occurs at constant pressure, w = AE. . If a reaction occurs at constant pressure, q = AH. c. If a reaction occurs at constant pressure, q = AE. d. If a reaction occurs at constant volume, AE > AH. e. If a reaction occurs at constant volume, w = AE. 2. The thermochemical equation for the combustion of hexane is shown below. C6H14(g) + 19/2 02(g) —) 6 C02(g) + 7 H20(g) AH" = —4l63 1:] What is the enthalpy change for the combustion of 2.50 g (Isl-1.4? -121kJ . -1.66x103kJ c. -1.04x104kJ d. _-1.43x105kJ e. -3.59><105kJ 3; A chemical reaction in a bomb calorimeter evolves 5.17 k] of heat. If the heat capacity of the calorimeter is 1.08 kJ!°C, what is the temperature change of the calorimeter? a. 0.209%: b.‘ 409°C @ 439°C . 5.58 °c e. 5.25 °C 4. Which of the following chemical equations does not correspond to a standard molar enthalpy of formation? a. Ca(s) + 0(3) + 3/2 02(g) ‘—) CaC03(s) V b. C(s) + 1/2 02(g) —+ C0(g) 0- Hzlg) + 1" 2 02%) —> H200) d- N2(g) + 2 02(3) '9 N204lg) song) + 1/2 org) —> song) 5. The Schrodinger wave equation a. calculates the position and momentum of an electron at any given time. (19 can be solved to determine the probability of finding an electron in a region of space. c. proves that energy is equal to mass times the speed of light squared. d. incorrectly predicts circular orbits of electrons around nuclei. 6. is used to calculate the velocity of an electron. Name: 1]): A 6. Which of the following statements is INCORRECT? The location and the energy of an electron in an atom can be simultaneously known with little or no uncertainty. _ b. The energies of an atom's electrons are quantized. 0. Quantum numbers define the energy states and the orbitals available to an electron. d. The behavior of an atom‘s electrons can be described by standing waves. e. Electrons have both wave and particle properties. 7. Whattype oforbital is designated n = 3, I= 2, m; = -1? a. 35 b. 3;? 3d . 2f e. 2d __H_ 8. What shell contains a total of 9 orbitals? a. n=1 b. n=2 ® n= 3 (1. n=4 e. n= 5 _ 9. Which f th following sets of quantum numbers refers to a 4p orbital? a. n=1,l=1,m;=- b. n=1,l=2,m;=- ' (9 n=4,l=1,m;=0 d. n=4,l=2,m;=-1 e. n=4,l=3,m;=+2 10. Which of the following properties is associated with the value of the I quantum number? ' a. the number of electrons in an orbital I b. the size of an orbital c. the orientation in space of an orbital d. _ the energy of an orbital the shape of an orbital 11. Which of the following diagrams represent p—orbitals? we a. (Donly @ (monly 0- (HD0111)! d- (IV)0nly e. (I) and (II) Name: -- r 1]): A 12. The Pauli exclusion principle states that _ no two electrons in an atom can have the same four quantum numbers. I electrons can have either :t% spins. c. _ electrons with opposing spins are attracted to each other. d. no two electrons in an atom can have the same spin. e. atoms with no unpaired electrons are diamagnetic. 13. What is the maximum number of electrons that can occupy the n = 5 shell? a. 5 7 b. 10 c. 14 d. 25 so 14. Which of the following elements is an s—block element? a. C b. Cd Cs . Cl e. Cf _ 15. Which of the following atoms is diamagnetic? a. Rb I b. C c. F (1. Cu Sr 16. Which element has the electron configuration 1522s22p53523p4? a. Mg ®' 3 c. S] d. Se e. Ga 17. Hund‘s rule states that the most stable arrangement of electrons (for a ground state electron configuration) a. has a filled valence shell of electrons. b. has two electrons per orbital, each with identical spins. c. ' has m; values greater than or equal to zero. has the maximum number of unpaired electrons, all with the same spin. c. has two electrons per orbital, each with opposing spins. 18. Place the following atoms in order of increasing atomic radii: Se, 0, S, and As. 0 < s< Se < As . o < s '< As > Se 0. As «.1 Se <'S < 0 d. Se<As<S<O e. S<As<O<Se ID:A 19. Rank K, Li, and Cs in order of increasing first ionization energy. a. K < Cs < Li Cs < K < Li c. Cs < Li < K d. Li < Cs < K e. Li < K < Cs __ 20. A silicon atom has _ valence electrons. a. 0 b. 2 (g 4 d. 6 e. 10 _ 21. What is the total number of valence electrons in a carbonate ion? a. 20 b. 22 24 . 26 e. 30 ____ 22. If two or more species have the same number of electrons resulting in similar Lewis structures, they are said to be . ‘ - a. neutral b. resonant structures c. symmetric isoelectronic 7 e. covalent 23. How many lone-pair electrons are on the carbon atom in C02? .‘1’ c. 2 (i. 3 e. 4 . 24. Which of the following elements is most likely to form a molecular structure that disobeys the octet rule? r a. Ne ' b. C Ci)? Cl 25. Use VSEPR theory to predict the molecular geometry of H30“. trigonal-pyramidal . trigonal-planar c. bent d. T-shaped e linear Test III - A (10 points) Determine the enthalpy change for the following reaction: Using the following data: P4(s) + 10C12(g) 9 4PC15(s) AH°=-1774;0kJ m L/ (PC13(1) + C12(g) -) PC15(s) AH°=-123.8kJ F}, r mm; ——-?‘+ PCES— #7794 0k? ‘4 (PCP;- -=7 9(03 r COS “q (#223 gig?) W R, H0le Apply .6/774016' films-H HPaS + q oz; +495“. 2K3- RH- »gwu WHMW’CPZHPQ, #973316— (5 points) Give the grounds state electron configurations for the following atoms: Arsenic (As) 7 /.s"'.'251 210‘ 35:03P" 5’57“ Eloy/03 0} [Ar] 75‘3" 7,05 Rubidimn (Rb) D (a 25‘35‘ 3301' 35‘ 3/05 ’73; 3"! 551 g [Kr-j 55‘ (10 points) Give the Lewis structure for the following molecules or ions: NH: H . N ' AW )3 SF6 : \\i (5% 1:: IF3 1E! 51% z 15 ...
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test_III_blue - Name: Class: Date: CHEM 1211 Test III...

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