Why Does Ionization Energy Increase Going Down A Group Class 11 ...

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AnswerQuestion Answers for Class 12Class 12 BiologyClass 12 ChemistryClass 12 EnglishClass 12 MathsClass 12 PhysicsClass 12 Social ScienceClass 12 Business StudiesClass 12 EconomicsQuestion Answers for Class 11Class 11 EconomicsClass 11 Computer ScienceClass 11 BiologyClass 11 ChemistryClass 11 EnglishClass 11 MathsClass 11 PhysicsClass 11 Social ScienceClass 11 AccountancyClass 11 Business StudiesQuestion Answers for Class 10Class 10 ScienceClass 10 EnglishClass 10 MathsClass 10 Social ScienceClass 10 General KnowledgeQuestion Answers for Class 9Class 9 General KnowledgeClass 9 ScienceClass 9 EnglishClass 9 MathsClass 9 Social ScienceQuestion Answers for Class 8Class 8 ScienceClass 8 EnglishClass 8 MathsClass 8 Social ScienceQuestion Answers for Class 7Class 7 ScienceClass 7 EnglishClass 7 MathsClass 7 Social ScienceQuestion Answers for Class 6Class 6 ScienceClass 6 EnglishClass 6 MathsClass 6 Social ScienceQuestion Answers for Class 5Class 5 ScienceClass 5 EnglishClass 5 MathsClass 5 Social ScienceQuestion Answers for Class 4Class 4 ScienceClass 4 EnglishClass 4 MathsWhy does ionization energy increase going down a group but decreases going across a period?AnswerVerified500.4k+ viewsHint: Let’s first discuss what ionization energy is. Ionization energy is the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule. Ionization energy exhibits periodicity on the periodic table. The general trend is for ionization energy to increase moving from left to right across an element period. Moving left to right across a period, atomic radius decreases, so electrons are more attracted to the nucleus.Complete answer: Ionization energy increases across a period because the number of protons increases. This means that there is an increase in nuclear charge so there'll be more attraction.While there is more attraction, one should know that distance from the nucleus and shielding effect remains reasonably constant. This is because all the valence electrons are in the same principal quantum shell.So the increase in nuclear charge increases attraction and makes the removal of an electron require more energy, while distance from the nucleus and shielding effect remains reasonably constant.Going down a group, the ionization energy decreases. This is due to the shielding or screen effect of the outer electrons from the nucleus and so the attraction is weaker and they are more easily removed.Note: There are however some exceptions across every period where the ionization energy drops between an atom of group $ A $ and group $ 3 $ and between group $ 5 $ and group $ 6 $ . The first drop is due to a slight increase in distance from the nucleus as the outer electron occupies a new subshell slightly further away from the nucleus. The second drop is due to spin pair repulsion which is due to the presence of two electrons in the same p orbital. This makes it require less energy to remove.Recently Updated PagesMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for SuccessMaster Class 11 Chemistry: Engaging Questions & Answers for SuccessMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for SuccessMaster Class 11 Chemistry: Engaging Questions & Answers for Success

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