Ranking the Ionization Energy of Ne, F, P, and Be

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SUMMARY

The discussion focuses on ranking the first ionization energies of Neon (Ne), Fluorine (F), Phosphorus (P), and Beryllium (Be). The established order from largest to smallest ionization energy is Neon, Fluorine, Phosphorus, and Beryllium. The general trend indicates that ionization energy increases from left to right across the periodic table and decreases from top to bottom. Participants express frustration over the difficulty of comparing Phosphorus to Beryllium due to their positions in the periodic table.

PREREQUISITES
  • Understanding of periodic table trends
  • Knowledge of ionization energy concepts
  • Familiarity with atomic structure
  • Basic chemistry terminology
NEXT STEPS
  • Research the periodic trends in ionization energy
  • Study the factors affecting ionization energy
  • Learn about exceptions to periodic trends
  • Explore the concept of electron affinity
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Chemistry students, educators, and anyone interested in understanding atomic properties and periodic trends in ionization energy.

phrygian
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Homework Statement



Rewrite each of the following lists from largest to smallest value of each property:

First Ionization Energy Be, P, Ne, F


Homework Equations



Our book says the general trend for ionization energy on the periodic table is to increase from left to right and decrease from top to bottom.

The key says the answer is Ne, F, P, Be.

The Attempt at a Solution



With the trends you can find that the energy for Ne is greater than for F which is greater than for Be. For P we can only see that it is less than N because it is located under N on the periodic table. How can P be compared to Be? Is there a way to approach this or was this just a bad problem?
 
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IMHO that's just a bad problem.
 
i agree. its a really bad problem
 

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