Question

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. a) Lithium has higher ionization energy than sodium. b) Fluorine has higher ionization energy than boron. c) Oxygen has lower ionization energy than nitrogen. 3. ELECTRON AFFINITY. The electron affinity is the energy change occurring when an electron is added to an isolated atom. Values generally become more negative (exothermic) from left to right across rows and less negative for elements lower in columns of the table. Both trends have many exceptions. Explain why: a) The electron affinity is more negative for fluorine than for oxygen. b) The electron affinity is less negative for sodium than for lithium. c) The electron affinity is less negative for nitrogen than for carbon.

Answer 1

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