How to determine the value of electronegativity

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SUMMARY

This discussion focuses on determining the electronegativity of elements from different periods and groups in the periodic table, specifically comparing an atom from Period 4, Group 7 with an atom from Period 3, Group 5. It is established that electronegativity generally decreases down a group due to increased atomic radius and electron shielding, which weakens the effective nuclear charge. However, the discussion notes that electronegativity trends can behave unusually in d-block elements, where it may increase down the periods. Clarification is provided that the comparison should be made between Period 4 and Period 5 rather than Period 3 and 4.

PREREQUISITES
  • Understanding of periodic trends in electronegativity
  • Familiarity with atomic structure and effective nuclear charge
  • Knowledge of the periodic table layout, specifically groups and periods
  • Basic chemistry concepts related to d-block elements
NEXT STEPS
  • Research the trends in electronegativity across different groups and periods in the periodic table
  • Study the concept of effective nuclear charge and its impact on atomic properties
  • Explore the unique properties of d-block elements and their electronegativity trends
  • Examine case studies of specific elements to understand exceptions in electronegativity trends
USEFUL FOR

Chemistry students, educators, and professionals seeking to deepen their understanding of electronegativity trends and atomic properties in the periodic table.

kenny1999
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for an atom that is an element in Period 4 , Group 7

to compare with another atom of element in Period 3, Group 5

Without looking at the Periodic table or electronegativity values, how can I

determine which one of these two atom is more electronegative?

(While Period 4, Group 7 has more number of outermost electrons but it has a larger atomic radius)

Can anyone good at Chemistry explain? Thank you very much!
 
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Well period 4 elements will be way bigger than period 3 elements and as a result their effective nuclear charge is a lot weaker because their nuclei are shielded way more (due to the greater number of electrons surrounding the nuclei). Thats why electronegativity usually decreases as you move down periods. Group 5 and 7 are d block metals and they start at period 4 so you're question doesn't make sense. Let's say its period 4 and 5 instead of 3 and 4. Electronegativity trends get a bit abnormal in the d block and it often increases as you move down periods. I don't know why that is.
 

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