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Chemistry 201/211 Worksheet 6 1.) a.) b.) c.) Fall 2004 November 11 Give the symbol of the element In Group 14 that has the smallest atomic radius In Period 3 that has the highest ionization energy In Group 16 that has the lowest electronegativity Oregon State University C Ar Po 2.) Circle any true statement. A 3p orbital... a.) can have an electron with a quantum number of l=2 no, p implies l=1 b.) can hold a maximum of 6 electrons yes, (2l+1) ml values times 2 () = 6ec.) can have an electron with a quantum number m l = -2 no, ml ranges from –l to +l d.) can have a maximum of 3 unpaired electrons for an atom in the ground state yes, there can be six electrons total in a p sublevel, if there are only three, they will be arranged so that their spin is maximized () 3.) The first two quantum numbers (n,l) of the highest energy electron of scandium in the ground state are a.) 3,0 b.) 3,1 c.) 3,2 d.) 4,0 e.) 4,1 Scandium is the first d (l=2) element in the periodic table. Being the first d, the minimum n is 3. 4.) Which of these statements are true? a.) Electrons have wave properties True b.) Infrared radiation corresponds to higher energy radiation than visible light False The wavelength of infrared radiation is longer than visible light and E=hc/. c.) Atoms emit light only at discrete, well-defined frequencies. True d.) The Pauli exclusion principle requires that only two electrons occupy a given orbital False. Six electrons can occupy a p orbital, 10 can be in a d orbital, etc… 5.) Consider an iron, Fe, atom. a.) Write its unexcited ground state electron configuration. 1s22s22p63s23p64s23d6 b.) Write its orbital diagram () () ()()() () ()()() () ()()()()() 1s2 2s2 2p6 3s2 3p6 4s2 3d6 2+ c.) Write the abbreviated ground state configuration for Fe [Ar]3d6 d.) Compare the size of Fe with Fe2+; compare the size of Fe2+ and Fe3+ Fe>Fe2+ Fe2+>Fe3+ e.) What is the value of the highest n in the ground state? 4 f.) What is the value of the highest l 2 6.) Based on their positions in the periodic table, select the atom with the larger first ionization energy from each of the following pairs: a.) B, Cl b.) N, P c.) Hf, Cs d.) O, N e.) Ga, Ge 7.) What is the trend in first ionization energies as you proceed across the fourth period from K to Kr? How does this compare with the trend in atomic sizes? The first ionization energy increases as we go across the fourth period and the atomic size decreases. 8.) Which of the following groups of elements is arranged in order of increasing electronegativity? a.) Si<Al<Br<Cl b.) Na<K<Ca<Ba c.) P<S<O<F d.) K<Rb<Cs<F e.) N<P<S<Cl 9.) Which of the following is expected to have the largest radius a.) K+ b.) Ca2+ c.) S2d.) Cle.) They are all the same 10.) Write the Lewis dot structure of carbon suboxide (C3O2, three central carbons flanked by two oxygen atoms). What would you predict its molecular geometry to be? C3O2 is linear 11.) Draw the Lewis structures for the following compounds. Also indicate the molecular geometry. a.) NH3 b.) H2S c.) PCl4+ d.) CO325.) CH3Cl 12.) Benzene (C6H6) consists of a six-member ring of carbon atoms with one hydrogen bonded to each carbon. Write Lewis structures for benzene, including resonance structures. 13.) Which one of the following species would have a Lewis structure most like that of SO2? a.) CO2 b.) NO2 c.) NO2+ d.) NO2e.) SiO2 How many unshared electron pairs (lone pairs) are in a molecule of SO2? 2 What is its molecular geometry? bent 14.) The Lewis structure represents… a.) NO2 b.) NO2- c.) NO2+ d.) both NO2- and NO2+ e.) NO2, NO2- and NO2+ There are 18 e- that are used in this Lewis structure (3 bonds * 2 = 6e- + 12 lone pair e-). Nitrogen has 5 e- and oxygen has 6 e- that total to 17e-. Therefore, an extra electron was needed making an overall negative one charge.