Question

- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions: Please answer each fill in the blank with the best answer. 1. The energy required to remove an electron from a gaseous atom is called the T ilas_energy. 2. When an electron is removed the atom gets a 3. The energy required to remove a second electrons is called the charge. energy. 4. It always requirest i -- to remove a second electron. 5. The energy required to remove an electron is always much, much greater if the atom is isoelectronic with a _before the electron is removed. 6. The ionization energy of the elements will _ as you move down a group on the Periodic Table. 7. This is because the electrons are attracted to the nucleus as they get further away from the nucleus. 8. The ionization energy of the elements will as you move from left to right across a period on the Periodic Table. 9. This is because the electrons are all the same distance from the nucleus in the same period, but the elements have protons as you move from left to right across the Periodic Table. 10. Circle the element in each of the following pairs with the greater (1) ionization energy c) cesium or lead a) lithium or boron d) sodium or argon b) magnesium or strontium 11. Arrange the following elements in order of increasing ionization energy: a) Sr, Be, Mg c) Na, Al, s b) Bi, Cs, Ba e increase between the 1st and 2nd ionization energies for the 12. Why is there a very large increase between the 1st and 2nd jonization elements in group 1?

Answer 1

- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wish #4 > Application! Directions: Please answer each fill in the blank with the best answer. 1. The energy required to remove an electron from a gaseous atom is called the Lonas energy. 2. When an electron is removed the atom gets a positive charge. 3. The energy required to remove a second electrons is called the Second lonization energy. energy 4. It always requires more energy to remove a second electron. 5. The energy required to remove an electron is always much, much greater if the atom isoelectronic with a noble gas before the electron is removed. 6. The ionization energy of the elements will decrease as you move down a group on the Periodic Table. 7. This is because the electrons are less attracted to the nucleus as they get further away from the nucleus. increase as you move from left 8. The ionization energy of the elements will to right across a period on the Periodic Table. 9. This is because the electrons are all the same distance from the nucleus in the same period, but the elements have more protons as you move from left to right across the Periodic Table. 10. Circle the element in each of the following pairs with the greater (1M) ionization energy a) lithium or boron c) cesium orlead d) sodium or (argon b) magnesium or strontium 11. Arrange the following elements in order of increasing ionization energy: a) Sr, Be, Mg Sr<Mg<Be c) Na, Al, S Na<Al<S b) Bi, Cs, Ba Cs<Ba<Bi 12. Why is there a very large increase between the 1 a very large increase between the 1 and 2ne ionization energies for the elemeFor the group 1 elements, after the removal of first electron, the resulting ion becomes isoelectronic with a noble gas. So the element always wants to be stable by the removal of 1st electron and attain a noble gas configuration. Now after the removal of first electron, as the noble gases has the highest ionization energy, the 2nd electron removal requires a lot of energy and thus a very large difference between 1st and 2nd ionization energies for group 1 elements.
The first electron removal from Group 1 elements are always easy and requires very low energy for ionization. That is the reason you see $Na^{+}$ but never $Na^{2+}$ because the second electron removal is very much an unfavorable task!