ate readias is a result of two different ideas. The first idea is that as one mo
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ate readias is a result of two different ideas. The first idea is that as one moves down a period electrons to larger principal quantum numbers (n); therefore, the atom's radius is ing larger. The second always batling each other. The equation below helps us determine the effeetive pull exerted on a specifie electron by the nucleus. As one moves These two are nuclear charge, which is the across a only slightly. That as period, Z (nuclear charge) increases by 1 for each element, while the shielding increases means as you move across a period, the pull of the nucleus increases -Z-shielding Cations have a smaller radius than their corresponding neutral atom. Anions have a larger radius Jonization energy is defined as the energy required to ionize (remove an electron) a neutral atom than their corresponding neutral atom and corresponds to the following reaction equation. lonization energy tends to increase across a period and decrease down a group. There are also 2nd, 3d, and subsequent ionization energies. The 2nd jonization energy is the energy required to remove a second electron and corresponds to the following reaction. Electron affinity is defined as a measure of the energy change when an electron is added to a neutral atom to form a negative ion. Questions 7. Identify the atom with the larger atomic radius and explain why. a. b. Ca or K N or O 8. Circle the element in each pair that has the higher 1st ionization energy and explain why Ba or Cs Br or Kr a. b. 9. Identify the element in each pair that has the greater electron affinity and explain why. a. Cl or Br b. H or He 10, why would you think that the elements in group 1 have extremely high 2nd ?Onization energies?Explanation / Answer
1. a. K(potassium) has a larger atomic radius than Ca( Calcium). In the periodic table, as we move across a period the atomic radius decreases(because of effective nuclear charge) and when we move down a group it increases(because of addition of a new shell). K lies to the left of Ca in the periodic table hence atomic radius is bigger.
b. N has a bigger atomic radius as it lies to the left of O in the periodic table.
2. a . Cesium has lower first ionization energy than barium. Ionization energy increases across the period and Ba lies on the right of Cs in the 6th period.
b. Kr has higher ionization energy than Br because it lies on its right in the 4th period. Morever Kr is a noble gas and removing an electron from its stable octet electronic configuration requires alot of energy.
3. a . Electron affinity of Cl is higher than Br. Electron affinity decreases down the group.Cl is more electronegative than Br hence has higher affinity/ attachment towards its electrons.
b. Helium has zero electron affinity as it is a noble gas with stable octet electronic configuratoin. Hence H has higher electron affinity than Helium.
4. Elements in group 1 have the general electronic configuration of the form ns1 (n = Group number). Ionization energy equals the energy required to remove the valence electron from an atom. For second ionization energy, we have to remove an electron from an already positively charged ion (because we have already removed one electron from the atom after which it has developed +1 charge). After developing a positive charge the electrons are more strongly attached to the atom, making it very difficult to further remove an electron.
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