WOuld you expect each of the following atoms to gain or lose electrons when forming ions? What ion is most likely in each case?
a. Na
b. Sr
c. P
d. Ba
Elements on the left hand side of the periodic table are likely to lose electrons. Elements on the right side of the periodic table are likely to gain electrons.
To determine whether an atom will gain or lose electrons when forming ions, we need to look at its position in the periodic table and its valence electron configuration.
a. Na (Sodium):
Sodium, with an atomic number of 11, is located in Group 1 of the periodic table. It has one valence electron in its outermost energy level. To achieve a stable electron configuration like that of a noble gas (in this case, neon), sodium will lose this one valence electron when forming an ion. Therefore, it is likely to form a Na+ ion (cation).
b. Sr (Strontium):
Strontium, with an atomic number of 38, is located in Group 2 of the periodic table. It has two valence electrons in its outermost energy level. To achieve a stable electron configuration like that of a noble gas (in this case, krypton), strontium will lose these two valence electrons when forming an ion. Therefore, it is likely to form an Sr2+ ion (cation).
c. P (Phosphorus):
Phosphorus, with an atomic number of 15, is located in Group 15 of the periodic table. It has five valence electrons in its outermost energy level. To achieve a stable electron configuration like that of a noble gas (in this case, argon), phosphorus will gain three electrons when forming an ion. Therefore, it is likely to form a P3- ion (anion).
d. Ba (Barium):
Barium, with an atomic number of 56, is located in Group 2 of the periodic table. It has two valence electrons in its outermost energy level. To achieve a stable electron configuration like that of a noble gas (in this case, xenon), barium will typically lose these two valence electrons when forming an ion. Therefore, it is likely to form a Ba2+ ion (cation).
Remember, the tendency to gain or lose electrons is based on the concept of achieving a stable electron configuration to attain a lower energy state and greater stability.