Which of the following shows a correct relationship between first ionization energies of the given atoms? view available hint(s) which of the following shows a correct relationship between first ionization energies of the given atoms? ga > ge ne > f li > be xe > ne

Option (b) is the correct answer.

Explanation:

The energy required to remove the most loosely bound electron from a neutral gaseous atom is known as ionization energy.

So, when there is increase in atomic size of the atom there is less force of attraction between the nucleus and the valence electrons of the atom.  

Hence, it is easy to remove the most loosely bound electron. Therefore, with increase in size there will occur a decrease in ionization energy of atom.

And, when we move across a period then there occurs a decrease in size of atom. Hence, ionization energy across a period increases.

Out of the given options neon is smaller is size that fluorine atom. So, ionization energy of neon is more than the ionization energy of fluorine atom.

Thus, we can conclude that Ne > F shows a correct relationship between first ionization energies of the given atoms.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

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