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(i) Write the electronic configuration of the following ions:(a) He+ (b) Mg2+ (c) O2− (d) S2−(ii) What are the atomic numbers of elements whose outermost electrons are represented by:(a) 3s2 (b) 2p5 and (c) 2s1(iii) which atoms are indicated by the following configurations?(a) [He]2s2 (b) [Ne]3s23p5 (c) [Ar]4s23d5 |
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Answer» (a) He+∶ Number of electrons = 2 − 1 = 1 \(\therefore\) Electronic configuration = 1s1 (b) Mg2+:Number of electrons = 12 − 2 = 10 \(\therefore\) Electronic configuration = 2,8, = 1s2 , 2s2 , 2p6 (c) O2−:Number or electrons = 8 + 2 = 10 \(\therefore\) Electronic Configuration = 2, 8 = 1s2 , 2s22p6 (d) S2−∶ Number of electrons = 16 + 2 = 18 \(\therefore\) Electronic of Configuration = 2, 8, 8 = 1s2 , 2s22p6 , 3s23p6 (ii) (a) 3s2 , Atomic number of elements = 12 (b) For 2p5 , Atomic number of elements = 9 (c) For 2s1 , Atomic number of elements = 3 (iii)
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