5Apossible set of quantum numbers to describe an electron in a 5Bsubshell is (1)
ID: 554930 • Letter: 5
Question
5Apossible set of quantum numbers to describe an electron in a 5Bsubshell is (1)n=5,1 m:2. m,.+1 (2) n = 5. 1:3, mr . 0, m, . . ½ (3) n#5. e:0, me-o,ma..½ @n=s,1.mao. 6. The orbital diagram for a ground-state oxygen atom is 1s 2s 2p (1)A (2)B (3)C D 7. Which ground-state atom has an electron configuration described by the following orbital diagram? 5s 5p (1) antimony-.germaniumn 8. A ground-state atom of vanadium has 4d (3) indum (4) tin unpaired electrons and is blereyhet (1) one, diamagnetic three, paramagnetic (4) four, paramagnetic (2) two, diamagnetic 9. "No two electrons in an atom can have the same four quantum numbers" is a statement of 10. Which of the following elements has the smallest first ionization energy? (1) Hund's rle the Pauli exclusion principle (3) Bohr's equation (4) the de Broglie's relation (1)CI (2) Na (3) Be (4) K 11. In what row Krj5s 4do5p (1) row 4, group 4A (2) row 4, group 5A (3) row 5, group 4A (4) row 5, group 5A 12. How many valence electrons does a P atom have? (1)31 (2)8 (3)15 (4)5 13. How many electrons does an arsenic atom need to til its outermost s and p subshells? (1)8 (2)7 (3)5 (4)3 14. Which two electron configurations represent elements that would have similar chemical properties? (1) (2) and (4) () and (2) (3) (1) and (3) (4) (2) and (3) 15 How many electrons are in the 3d subshell of bromine? (1)0 (2)2 (3)10 (4) 18Explanation / Answer
10. OPTION 4. Among the other elements given, Na and K can attain a noble gas configuration if they expel one of their valence electrons making them possess low first ionization enthalpies. However, K has a shell more than Na and so, its effectively nuclear charge on a valence electron is much less than that of Na giving it the lowest first ionization enthalpy.
11. OPTION 4. The given electronic configuration points to an element with atomic number 51 which corresponds to antimony. Antimony is placed in row 5 and group 5A or 15.
12. OPTION 4. Phosphorous is in the same group as N. So like N it has a valence electron configuration of 3s2 3p3. Thus it has 5 valence electrons.
13. OPTION 4. Arsenic resides in the same group as N and P. So its valence electronic configuration will be ns2, np3. This makes the atom require 3 more electrons to fill its p-shell and thus attain an octet.
14. OPTION 1. Among the given electronic configurations, only 2 and 4 have an almost filled p-orbital with a single electron required. This would give both elements the tendency to abstract electrons from other atoms to attain a stable p6 configuration. In case of others, two electrons are required for p4 and 5 for d5 thus making their reactivities dissimilar.
15. OPTION 3. Bromine is a halogen with a characteristic p5 outer-electron configuration. Taking into account the fact that Br occurs after the first row transition metals, we can say that a 3d10, 4s2, 4p5 configuration exists for bromine.
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