- Oxygen < Carbon < Aluminum < Potassium
- Neon < Aluminum < Sulfur < Oxygen
- Fluorine has nine protons attracting 9 electrons which are much closer to the nucleus compared to Iodine. This results in smaller size of Fluorine than Iodine making it difficult to remove an electron from the atom.
- Because they have same number of electrons in the outer shell (valence electrons) which take part in chemical reaction.
- a. Decreases; b. Increases; c. Increases
- Atomic radius increases down the group on the periodic table. As we compare the elements down the group, the effective nuclear charge increases, but at the same time the outermost electrons are found in the shell that is farther away from the nucleus. Also the number of screening electrons increases. This results in reduced attraction between the nucleus and the outermost electrons.
- Ionization energy increases from left to right across the period. The atomic size becomes smaller from left to right. So it becomes harder to remove electron from the atom. Hence the energy required to do so (Ionization Energy) increases.
Parent Tip: Review the logic above to help your child master the concept of worksheet periodic table trends answer key.
