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quiz 1 in chemistry
front 1 Choose the paramagnetic species from below. O2⁻ Zn Ca Cd2⁺ Nb3⁺ | back 1 Nb3⁺ |
front 2 Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error? n = 1, l = 0, ml =0 n = 3, l = 0, ml =0 n = 3, l =3 , ml = -2 n = 2, l = 1 , ml = -1 n = 4, l = 2, ml =0 | back 2 n = 3, l =3 , ml = -2 |
front 3 Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. n = 4, l = 4, ml =0 n = 3, l = 1, ml = -2 n = 4, l = 0, ml =-1 n = 5, l = 3, ml =-3 n = 3, l = 2, ml =+3 | back 3 n = 5, l = 3, ml =-3 |
front 4 Give the ground state electron configuration for Se. [Ar]4s23d10 [Ar]4s24d104p4 [Ar]3d104p4 [Ar]4s23d104p6 [Ar]4s23d104p4 | back 4 [Ar]4s23d104p4 |
front 5 Give the ground state electron configuration for Sr. [Kr]5s25d105p2 [Kr]5s24d105p2 [Kr]5s24d2 [Kr]5s2 [Kr]5s24d10 | back 5 [Kr]5s2 |
front 6 Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom. n = 4, l = 1, ml = 1, ms = -1/2 n = 5, l = 1, ml =1 , ms = -1/2 n = 5, l = 1, ml = 0, ms = +1/2 n = 5, l = 0, ml = 0, ms = -1/2 n = 4, l = 1, ml = -1, ms = +1/2 | back 6 n = 5, l = 0, ml = 0, ms = -1/2 |
front 7 How many different values of ml are possible in the 3d sublevel? 5 1 3 7 2 | back 7 5 |
front 8 How many different values of ml are possible in the 4f sublevel? 5 2 3 1 7 | back 8 7 |
front 9 How many of the following elements have 1 unpaired electron in the
ground state? Answers: 2 1 4 3 | back 9 3 |
front 10 How many sublevels are contained in the second shell (n=2) of a given atom? 3 1 4 9 2 | back 10 2 |
front 11 How many unpaired electrons are present in the ground state Kr atom? 3 2 0 5 1 | back 11 0 |
front 12 How many valence electrons does an atom of S have? 6 3 2 1 4 | back 12 6 |
front 13 Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1. Ga Al In B | back 13 Ga |
front 14 Identify the location of the visible range of light. between microwave and radio between gamma ray and ultraviolet between x-ray and gamma ray between x-ray and ultraviolet between ultraviolet and infrared | back 14 between ultraviolet and infrared |
front 15 In which orbital below would an electron (on average) be farthest from the nucleus?: 2p 3s 3d 4f 1s | back 15 4f |
front 16 Place the following elements in order of increasing atomic
radius. Ba < Cl < P P < Cl < Ba Ba < P < Cl Cl < P < Ba Cl < Ba < P | back 16 Cl < P < Ba |
front 17 Place the following in order of increasing radius. Rb⁺ < Br⁻ < Na⁺ Br⁻ < Rb⁺ < Na⁺ Rb⁺ < Na⁺ < Br⁻ Br⁻ < Na⁺ < Rb⁺ Na⁺ < Br⁻ < Rb+ | back 17 Na⁺ < Br⁻ < Rb+ |
front 18 Place the following types of electromagnetic radiation in order of
increasing frequency. microwaves < visible light < X-rays visible light < X-rays < microwaves X-rays < microwaves < visible light microwaves < X-rays < visible light X-rays < visible light < microwaves | back 18 microwaves < visible light < X-rays |
front 19  Refer to the figure. Place the following in order of increasing
IE1. As < N < F N < As < F F < N < As F < N < As As < F < N | back 19 As < N < F |
front 20 What are the possible orbitals for n = 3? s, p, d s, p, d, f s, p s | back 20 s, p, d |
front 21 When filling degenerate orbitals, electrons fill them singly at first, with parallel spins. This is know as Aufbau principle Hund's rule Heisenberg uncertainty principle Pauli's exclusion principle | back 21 Hund's rule |
front 22 Which of the following occur as the wavelength of a photon increases? the energy increases the frequency decreases Planck's constant decreases the speed decreases None of the above occur as the wavelength of a photon increases. | back 22 the frequency decreases |
front 23 Which of the following quantum numbers describes the shape of an orbital? magnetic quantum number principal quantum number Schrödinger quantum number spin quantum number angular momentum quantum number | back 23 angular momentum quantum number |
front 24 Which of the following statements is TRUE? An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. Two electrons in the same orbital can have the same spin. It is possible for two electrons in the same atom to have identical values for all four quantum numbers. None of the above are true. | back 24 An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. |
front 25 Which of the following types of electromagnetic radiation has the shortest wavelength? green yellow violet blue orange | back 25 violet |
front 26 Which of the following visible colors of light has the highest frequency? orange red green yellow blue | back 26 blue |
front 27 Which reaction below represents the second ionization of Sr? Sr⁺(g) + e⁻ → Sr(g) Sr(g) → Sr⁺(g) + e⁻ Sr2⁺(g) + e⁻ → Sr⁺(g) Sr⁺(g) → Sr2⁺(g) + e⁻ Sr⁻(g) + e⁻ → Sr2⁻(g) | back 27 Sr⁺(g) → Sr2⁺(g) + e⁻ |
front 28 Which reaction below represents the second electron affinity of S? S2⁻(g) → S⁻(g) + e⁻ S⁻(g) → S(g) + e⁻ S⁻(g) + e⁻ → S2⁻(g) S(g) → S⁺(g) + e⁻ S(g) + e⁻ → S⁻(g) | back 28 S⁻(g) + e⁻ → S2⁻(g) |
front 29 Write out the orbital diagram that represents the ground state of As. How many unpaired electrons are there? 0 3 2 1 4 | back 29 3 |