1A. The periodic trend for ionization energy states that typically ionization energy increases to the [left, right] across a period.

Complete the following sentence by selecting the appropriate choices.

1A. The periodic trend for ionization energy states that typically ionization energy increases to the [left, right] across a period. This is because as effective nuclear charge increases to the [right, left] across a period, the [valence electrons, core electrons] experience a stronger attraction to the [valence electrons, core electrons, nucleus] and therefore require more energy to be removed.

Complete the following statement for magnesium and aluminum.

1B. Contrary to the periodic trend, the first ionization energy of [magnesium, aluminum] is less than the first ionization energy of [magnesium aluminum].

1C. Which of the following statements bestexplains why these two elements do not follow the trend?

i) The first ionization energy of magnesium involves the removal of an electron from a filled s orbital while the first ionization energy of aluminum involves the removal of an electron from a partially filled p orbital. The removal of an electron from a partially filled orbital requires less energy than the removal of an electron from a filled orbital.

ii) The first ionization energy of magnesium involves the removal of a paired electron while the first ionization energy of aluminum involves the removal of an unpaired electron. The removal of an unpaired electron requires less energy than the removal of a paired electron.

iii) The first ionization energy of magnesium involves the removal of a 3s electron while the first ionization energy of aluminum involves the removal of a higher energy 3p electron. The electrons in the 3p orbitals are higher in energy and therefore require less energy to remove the electron.

Expert Solution

1A. The periodic trend for ionization energy states that typically ionization energy increases to the [right] across a period. This is because as effective nuclear charge increases to the [right] across a period, the [valence electrons] experience a stronger attraction to the [nucleus] and therefore require more energy to be removed.

1B. Contrary to the periodic trend, the first ionization energy of [aluminum] is less than the first ionization energy of [magnesium].

1C. Which of the following statements best explains why these two elements do not follow the trend?

i) The first ionization energy of magnesium involves the removal of an electron from a filled s orbital while the first ionization energy of aluminum involves the removal of an electron from a partially filled p orbital. The removal of an electron from a partially filled orbital requires less energy than the removal of an electron from a filled orbital. (Remember partially filled term is different from half filled (which is more stable).

queen_honey_blossom answered 2 years ago

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