9. justify why the number of valence electrons stays the same within a group using electron configurations…

9. justify why the number of valence electrons stays the same within a group using electron configurations. i need a hint groups or families have similar properties and a play a key role in determining these properties. once an atom has a b, additional electrons are placed in a higher energy level.

9. justify why the number of valence electrons stays the same within a group using electron configurations. i need a hint groups or families have similar properties and a play a key role in determining these properties. once an atom has a b, additional electrons are placed in a higher energy level.

Answer

Answer:

Elements in the same group have the same number of valence - shell electrons because as you move down a group, the principal quantum number (n) of the outermost shell increases, but the number of electrons in the outermost shell (valence electrons) remains the same. For example, all elements in Group 1 (alkali metals) have an electron - configuration ending in (ns^1), where (n) represents the principal energy level. As you go from lithium ((1s^22s^1)) to sodium ((1s^22s^22p^63s^1)) to potassium ((1s^22s^22p^63s^23p^64s^1)), the outermost electron is in an (s) orbital and there is 1 valence electron. The additional electrons are placed in higher energy levels, but the number of valence electrons remains constant for elements within the same group.