Final answer:
To determine which atoms form ionic bonds, metals on the left of the periodic table become cations and nonmetals on the right become anions. Mg, In, Cs, Pb, Co, Ca, Na, Al, Sn, Cd are likely to form positive ions, while P, I, Cl, O, Br, N, F, S are likely to form negative ions. P would form a 3- ion, while Mg and Al would form 2+ and 3+ ions, respectively.
Step-by-step explanation:
To determine which atoms are likely to form ionic bonds, we look to the periodic table and consider the general trend for ion formation based on their position. Metals, typically found on the left side of the periodic table, will tend to lose electrons to form positively charged ions or cations. Nonmetals, found on the right side of the periodic table, will gain electrons to form negatively charged ions or anions.
In the list provided:
- Mg, In, Cs, Pb, and Co, which are metals, would be expected to form positive ions.
- P, I, Cl, O, which are nonmetals, would be expected to form negative ions.
For instance:
- Phosphorus (P) would likely form a 3- anion (P3-).
- Magnesium (Mg) would typically form a 2+ cation (Mg2+).
- Aluminum (Al) would form a 3+ cation (Al3+).
Similarly, for the second list:
- Br, N, F, S, which are nonmetals, would probably form negative ions.
- Ca, Na, Al, Sn, Cd, as metals, would form positive ions.
Predicting Ion Charge
- The monatomic ion of phosphorus (P) in a binary ionic compound would have a charge of 3-.
- For magnesium (Mg) and aluminum (Al), the monatomic ions would carry charges of 2+ and 3+, respectively.
It's important to note that the predictive power of the periodic table is crucial in understanding ionic bond formation.