Why is the first ionization of aluminum less than the first ionization of magnesium? Select all that apply. a) The last valence electron of aluminum begins the occupation of the 3p subshell. b) The last valence electron of magnesium ends the occupation of the 3s subshell. c) The statement is incorrect because the general trend left to right in a row is for the effective nuclear charge to increase. d) The 3s electrons shield the 3p electrons from the nuclear charge.

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Q: 3) Which of the following is isoelectronic with Mg? Ar, K*, S² or Ne s2-

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Q: QUESTION 4 For which of the elements below is there a large increase in the 4th ionization energy…

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Q: 2) Define the Pauli Exclusion Principle and contrast it to the Pauli Principle

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Q: Which atom would have the largest effective nuclear charge for its valence electrons? a) Si b) S…

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Q: Write the electron configuration and draw the orbital diagrams of the following elements  a) C2+…

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Q: Explain why the first ionization energy of sodium (Na) is significantly less than that of neon (Ne).

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Q: Why is the first ionization of aluminum less than the first ionization of magnesium? Select all that…

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Q: Define Ionization Energy?

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