Homework Answers
a) lithium has only two orbits. So, it's valence electron which is in 2s orbital is very very close to the nucleus. Sodium has 3 orbits. Though the effective nuclear charge increases in sodium, the valence electron which is in the 3s orbital, is at a very large distance. So, sodium has lower first-ionization energy.
b) The valence electrons in nitrogen are in half-filled 2p orbital. Being half-filled, the electrons in the orbital are more stable than that in oxygen because there is no such case in case of oxygen. So, the first ionization energy of oxygen is lower than that of nitrogen.
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3. Explain each of the following observations. (a) Sodium has a lower first-ionization energy than lithium....
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(2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy...
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In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
(2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy of nitrogen?
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