2. The ionization energy of an element is defined as the amount of energy required to remove an electron from an individual atom. The following table gives the ionization energy (in units of kilojoules per mole) for five metals, listed in alphabetical order. Locate each of these metals on the periodic table and arrange them in order of rows and columns as in the periodic table. (a) Describe the periodic trend in the ionization energy of elements within a group. (b) Describe the periodic trend in the ionization energy of elements across a period.
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This is because as you move down a group, the number of energy levels (shells) increases, meaning the outermost electrons are further from the nucleus and are therefore less tightly bound to the nucleus. This makes it easier to remove an electron, thus requiring Show more…
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14. State the relationship between atomic number and first ionization energy as the elements in Group 1. As the atomic number increases, the ionization energy in Group 1 decreases. Explain. 15. The radius of a lithium atom is 130 picometers, and the radius of a fluorine atom is 60 picometers. Describe the general trend in atomic radius as each element in Period 2 is considered in order from left to right: The atomic radius in Period 2 decreases. Explain. Describe the general trend in electronegativity as each element in Period 2 is considered in order from left to right. The electronegativity across Period 2 increases. Explain.
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Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium $(738 \mathrm{kJ} / \mathrm{mol})$ and aluminum $(578 \mathrm{kJ} / \mathrm{mol}) .$ Explain this observation. (b) Explain why the ionization energy of phosphorus $(1012 \mathrm{kJ} / \mathrm{mol})$ is greater than that of sulfur $(1000 \mathrm{kJ} / \mathrm{mol})$ when the general trend in ionization energies in a period would predict the opposite.
The successive ionization energy values for an element $\mathrm{X}$ are given below: (a) 1st ionization energy $=410 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (b) 2 nd ionization energy $=820 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (c) 3 rd ionization energy $=1100 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (d) 4 th ionization energy $=1500 \mathrm{~kJ} \mathrm{~mol}^{-1}$ (e) 5 th ionization energy $=3200 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Find out the number of valence electron for the atom, $\mathrm{X} .$ (a) 4 (b) 3 (c) 5 (d) 2
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