Final answer:
The charge of the ion for each atom is predicted based on its group number and whether it's a metal or nonmetal.
- Si14 will lose 4 electrons and form Si4+.
- -As33 will gain 3 electrons and form As3-.
- -Mg12 will lose 2 electrons and form Mg2+.
- -Rb37 will lose 1 electron and form Rb+.
- -F9 will gain 1 electron and form F-.
- -Ge32 will lose 4 electrons and form Ge4+.
- -Sn50 will lose 4 electrons and form Sn4+.
Step-by-step explanation:
To predict the charge of the ion formed from each atom, we consider the atom's position in the periodic table and whether it tends to lose or gain electrons to achieve a noble gas electron configuration. The charge of an ion typically depends on whether the element is a metal or a nonmetal and its group number.
- Si (Silicon - Group 14): Usually forms a 4+ cation.
- As (Arsenic - Group 15): Usually forms a 3- anion.
- Mg (Magnesium - Group 2): Usually forms a 2+ cation.
- Rb (Rubidium - Group 1): Usually forms a 1+ cation.
- F (Fluorine - Group 17): Usually forms a 1- anion.
- Ge (Germanium - Group 14): Usually forms a 4+ cation.
- Sn (Tin - Group 14): Can form either a 2+ or 4+ cation, depending on the compound.
Nonmetals and metalloids like As and F usually form anions, and the charge can be determined by subtracting 18 from their group number. Metals like Si, Mg, Rb, Ge, and Sn typically form cations, and for Group 1 and Group 2 elements, the charges are +1 and +2, respectively. Group 14 elements tend to form +4 cations, although Sn can vary.