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

In summary, the general trend for ionization energy on the periodic table is to increase from left to right and decrease from top to bottom. The correct order for the given elements, from largest to smallest, is Ne, F, P, Be. It should be noted that comparing P to Be is difficult as their positions on the periodic table do not provide a clear trend. Overall, this is a poorly designed problem.
  • #1
phrygian
80
0

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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  • #2
IMHO that's just a bad problem.
 
  • #3
i agree. its a really bad problem
 

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

1. What is ionization energy?

Ionization energy is the amount of energy required to remove an electron from an atom or molecule, resulting in the formation of an ion. It is an important measure of an atom's tendency to gain or lose electrons.

2. How is ionization energy measured?

Ionization energy is typically measured in units of kilojoules per mole (kJ/mol) or electron volts (eV). It can be experimentally determined through various techniques, such as photoelectron spectroscopy or mass spectrometry.

3. Which factor determines the ionization energy of an atom?

The ionization energy of an atom is primarily determined by the number of protons in its nucleus, also known as its atomic number. As the number of protons increases, so does the ionization energy.

4. How does the size of an atom affect its ionization energy?

Generally, the smaller the atom, the higher its ionization energy. This is because smaller atoms have a stronger hold on their electrons due to a higher nuclear charge, making it more difficult to remove an electron.

5. How do the ionization energies of Ne, F, P, and Be compare?

Based on their atomic numbers, the ionization energies of these elements follow the trend of increasing from Be to Ne, with Ne having the highest ionization energy. This is because Ne has the most protons and therefore the strongest hold on its electrons. Additionally, F has a slightly higher ionization energy than P due to its smaller size.

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