the complete photoelectron spectrum of an element is given above. which labeled peak corresponds to the 1s…

the complete photoelectron spectrum of an element is given above. which labeled peak corresponds to the 1s electrons and why?\na peak x, because 1s electrons are the easiest to remove from the atom.\nb peak x, because 1s electrons have the strongest attractions to the nucleus.\nc peak y, because electrons in the 1s sublevel are the farthest from the nucleus.

the complete photoelectron spectrum of an element is given above. which labeled peak corresponds to the 1s electrons and why?\na peak x, because 1s electrons are the easiest to remove from the atom.\nb peak x, because 1s electrons have the strongest attractions to the nucleus.\nc peak y, because electrons in the 1s sublevel are the farthest from the nucleus.

Answer

Brief Explanations:

In a photoelectron spectrum, the binding energy is related to the attraction of electrons to the nucleus. 1s electrons are in the innermost shell, closest to the nucleus. According to Coulomb's law ((F = k\frac{q_1q_2}{r^{2}}), where (q_1) and (q_2) are charges, (r) is the distance), the closer the electrons (smaller (r)) to the positively - charged nucleus ((q_1) is the nuclear charge, (q_2) is the electron charge), the stronger the electrostatic attraction. A higher binding energy means more energy is required to remove the electron. Since 1s electrons are closest to the nucleus (strongest attraction), they have the highest binding energy. Looking at the spectrum, peak X has a higher binding energy than peak Y.

Answer:

B. Peak X, because 1s electrons have the strongest attractions to the nucleus.