Identify the block and group that corresponds to the following generalized electron configuration and indicate the number of unpaired electrons in this group: [noble gas] ns2 (n-1)d10 np4.1 pointd-block, Group 12 and zero unpaired electronsp-block, Group 14 and two unpaired electronsp-block, Group 16 and two unpaired electronss-block, Group 2 and zero unpaired electrons
Question
Identify the block and group that corresponds to the following generalized electron configuration and indicate the number of unpaired electrons in this group: [noble gas] ns2 (n-1)d10 np4.1 pointd-block, Group 12 and zero unpaired electronsp-block, Group 14 and two unpaired electronsp-block, Group 16 and two unpaired electronss-block, Group 2 and zero unpaired electrons
Solution
The correct answer is p-block, Group 16 and two unpaired electrons.
Here's the step-by-step reasoning:
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The electron configuration given is [noble gas] ns2 (n-1)d10 np4. This means that the last electrons are in the p orbital.
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In the periodic table, the blocks are determined by the type of orbital being filled. Since the last electrons are in the p orbital, this element is in the p-block.
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The group number in the periodic table corresponds to the number of valence electrons. The ns2 and np4 in the electron configuration indicate that there are a total of 6 valence electrons. Therefore, this element is in Group 16.
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The number of unpaired electrons is determined by the number of electrons in the outermost orbital that are not paired. In this case, the np4 indicates that there are 4 electrons in the p orbital, 2 of which are unpaired (since each orbital can hold up to 2 electrons, and the p orbital has 3 sub-orbitals, allowing for a total of 6 electrons). Therefore, there are two unpaired electrons.
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