Final answer:
The common charges of tin ions are 2+ and 4+, which occur by losing electrons from its p and s orbitals, respectively. Zirconium commonly forms a 4+ ion as it loses four valence electrons from the s and d orbitals, aiming for a more stable noble gas electron configuration.
Step-by-step explanation:
Predicting the common charges of the ions of tin involves understanding its position on the periodic table and its electron configuration. Tin (Sn) has two common ions: Sn2+ and Sn4+. For the Sn2+ ion, tin loses the two electrons in its p orbital, resulting in the electron configuration [Kr]4d105s2. For the Sn4+ ion, tin loses two additional electrons from the s orbital, resulting in [Kr]4d10. When it comes to zirconium (Zr), the highest possible charge is typically 4+, as it loses its four valence electrons (two from the s orbital and two from the d orbital), resulting in [Kr]4d2.
The reasoning is based on the concept that ions tend to form in ways that lead to a complete octet (eight electrons) in their outermost shell, thus achieving a more stable noble gas electron configuration. Transition metals like tin and zirconium often have more than one common ion and can lose different numbers of d electrons after the s electrons are lost to form various positively charged ions.