Explanation:
This atom is on the almost extreme right of the 2nd period of the periodic table (except for the stable element on the extreme right). This means it has the highest mass number of the unstable elements of the period. It thus attracts its electron clouds more strongly that the elements to the left of the period . This means it can gain an atom easily ( this is what is called electronegativity – tendency to attract an electron) than is can lose an electron. In addition, it only needs to acquire one electron to achieve a stable electron configuration (8) in its valence shell.
Due to these, it is hard for the atoms to lose an electron which is why it has a high ionization energy- the energy required to lose an electron.
Learn More:
For more on electronegativity and ionization energy check out;
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First let us determine the electronic configuration of
Bromine (Br). This is written as:
Br = [Ar] 3d10 4s2 4p5
Then we must recall that the greatest effective nuclear
charge (also referred to as shielding) greatly increases as distance of the
orbital to the nucleus also increases. So therefore the electron in the
farthest shell will experience the greatest nuclear charge hence the answer is:
<span>4p orbital</span>
Answer:
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Explanation:
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