An element with the ground-state electron configuration 1s2 2s2 2p2 belongs to which group__________________?
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Answer: B. Group IV-A
Explanation
The given ground-state electron configuration ends with two electrons in the second p orbital. Adding the valence electrons in the second shell yields a total of four valence electrons. Having four valence electrons places this specific element directly into Group IV-A of the table. Electron configuration describes the distribution of electrons of an atom across atomic orbitals. Valence electrons occupy the outermost principal energy level and determine chemical reactivity. Group numbers in the main-block periodic table typically correspond to the number of valence electrons.
Carbon is the element with this configuration and forms the structural backbone of all organic chemistry. Semiconductor manufacturing relies heavily on Group IV-A elements like silicon and germanium. Determining electron configurations helps chemists predict bonding behavior and molecular geometry. Group II-A elements possess two valence electrons in their outermost s orbital, not four. Group VII-A elements have seven valence electrons and end in p5 electron configurations. Group VI-A elements have six valence electrons and end in p4 electron configurations.
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