What is the charge on the lowest energy/most stable ions of K, Sc, S and Br?
K is +1
Sc is +3
S is -2 and Br is -1
To determine the charge on the lowest energy/most stable ions of K (potassium), Sc (scandium), S (sulfur), and Br (bromine), you need to consider the electronic configurations of these elements.
1. K (Potassium):
To find the charge on the lowest energy ion, you observe the elements' position in the periodic table. Potassium (K) is in Group 1, which means it has one valence electron. Group 1 elements typically lose one electron to achieve a stable electron configuration. Therefore, the charge of the lowest energy/most stable ion of potassium is +1.
2. Sc (Scandium):
Scandium (Sc) is located in Group 3 of the periodic table. Elements in this group can have different charges depending on the specific compound or situation. Since scandium has three valence electrons, it can lose all three electrons to form a +3 ion, which is the most stable ion for scandium.
3. S (Sulfur):
Sulfur (S) is located in Group 16 of the periodic table. Group 16 elements typically gain two electrons to achieve a stable electron configuration. Therefore, the charge of the most stable ion of sulfur is -2.
4. Br (Bromine):
Bromine (Br) is located in Group 17 of the periodic table. Group 17 elements typically gain one electron to achieve a stable electron configuration. Therefore, the charge of the most stable ion of bromine is -1.
In summary:
- The most stable ion of potassium (K) has a charge of +1.
- The most stable ion of scandium (Sc) has a charge of +3.
- The most stable ion of sulfur (S) has a charge of -2.
- The most stable ion of bromine (Br) has a charge of -1.