QQuestionChemistry
QuestionChemistry
The electronic configuration of an element is 1s^2 2s^2
2p^6 3s^2 3p^6 3d^8 4s^2. What is its group?
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Analyze the Electronic Configuration
The given electronic configuration is $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{8} 4s^{2}
Step 3:: Identify the Valence Electrons
- Total valence electrons: $$4s^{2} + 3d^{8} = 2 + 8 = 10$$ electrons
- The valence electrons are those in the outermost shell - In this case, the valence electrons are in the 4s and 3d orbitals
Step 4:: Determine the Group
- For transition metals, the group is determined by the total number of valence electrons - This element has 10 valence electrons - This corresponds to Group 10 in the periodic table
Step 5:: Verify the Element
- Group 10 elements include Nickel (Ni), Palladium (Pd), and Platinum (Pt) - The electronic configuration matches Nickel (Ni)
Final Answer
The element belongs to Group 10 of the periodic table.
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