Honors Chemistry Chapter 7-8 Take-home Quiz Name ____________________________________ Period _____ Date ____________ 1)_____ Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves A) radio waves > microwaves > ultraviolet light B) ultraviolet light > microwaves > radio waves C) radio waves > ultraviolet light > microwaves D) ultraviolet light > radio waves > microwaves E) microwaves > radio waves > ultraviolet light 2)_____ How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy? A) 3.37 × 1019 photons D) 4.03 × 1028 photons 30 B) 3.06 × 10 photons E) 2.48 × 1025 photons C) 1.80 × 1024 photons 3)_____ Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s. A) 1.99 × 10-10 m D) 5.52 × 10-9 m -10 B) 5.03 × 10 m E) 2.76 × 10-9 m C) 1.81 × 10-10 m 4)_____ Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon. A) n = 1 to n = 2 D) n = 6 to n = 3 B) n = 2 to n = 3 E) n = 3 to n = 1 C) n = 4 to n = 5 5)_____ What are the possible orbitals for n = 3? A) s, p, d B) s, p, d, f C) s D) s, p E) p, d, f 6)_____ Which of the following statements is TRUE? A) We can sometimes know the exact location and speed of an electron at the same time. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. E) All of the above are true. 7)______ No two electrons can have the same four quantum numbers is known as the a. Pauli exclusion principle c. Aufbau principle b. Hund's rule d. Heisenberg uncertainty principle 8)______ Only two electrons, with opposing spins, are allowed in each orbital is known as the a. Pauli exclusion principle c. Aufbau principle b. Hund's rule d. Heisenberg uncertainty principle 9)______ When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as a. Pauli exclusion principle b. Hund's rule c. Aufbau principle d. Heisenberg uncertainty principle 10)______ Choose the orbital diagram that represents the ground state of N. A) C) B) D) E) 11)______ Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. 1 2 1 b. n = 3, l = 0, ml = 1, ms = 2 1 c. n = 3, l = 2, ml =1 , ms = + 2 a. n = 3, l = 1, ml = 1, ms = + 1 2 1 e. n = 3, l =2 , ml = 1, ms = 2 d. n = 2, l = 1, ml = 1, ms = - 12)______ Which of the following statements is TRUE? A) 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. B) 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. C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. D) Two electrons in the same orbital can have the same spin. E) None of the above are true. 13)______ Give the number of core electrons for O. A) 0 B) 1 C) 2 D) 3 E) 4 14)______ How many valence electrons do the alkali earth metals possess? A) 1 D) 6 B) 2 E) 8 C) 7 15)______ The complete electron configuration of gallium, element 31, is __________. A) 1s22s22p103s21s22s22p103s2 3p104s23d3 B) 1s22s22p63s23p63d104s24p1 C) 1s42s42p63s43p64s43d3 D) 1s42s42p103s43p9 E) 1s42s42p83s43p84s3 16)______ The condensed electron configuration of silicon, element 14, is __________. A) [He]2s42p6 D) [He]2s4 B) [Ne]2p10 E) [He]2s62p2 2 2 C) [Ne]3s 3p 17)______ What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals? A) ns1 C) 1s22s1 B) ns2 D) 1s22s2 18)______ Place the following elements in order of increasing atomic radius. P Ba Cl A) Ba < P < Cl D) Cl < Ba < P B) P < Cl < Ba E) Ba < Cl < P C) Cl < P < Ba 19)______ What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200 A) Si D) Cl B) S E) Mg C) P 20)______ Choose the paramagnetic species from below. a. Ca d. Zn 2+ 3+ b. O e. Nb 2+ c. Cd 21)______ Which ionization process requires the most energy? a. W(g) → W+(g) + ec. W2+(g) → W 3+(g) + eb. W+(g) → W 2+(g) + ed. W3+(g) → W 4+(g) + e- 22)______ Calculate the energy change associated with the transition from n=4 to n=1 in the hydrogen atom. 23)______ Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 4 and the atom emits a photon of light with a wavelength of 486 nm. 24)______ Why does the size of the transition elements stay roughly the same as you move across a period? 25)______ Define paramagnetic. 26)______ Below is a list of successive ionization energies (in kJ/mol) for a period 3 element. Identify the element and explain how you came to that conclusion. IE2 = 2250 IE3 = 3360 IE4= 4560 IE5= 7010 IE6= 8500 IE7 = 27,100 27)______ Why is the first ionization energy of sulfur smaller than the first ionization energy of phosphorus? 28)______ Define electron affinity.