Tin(IV) Hydroxide and Ionic Compounds

The video tutorial explains how to write the formula for Tin(IV) Hydroxide. It begins by identifying the element symbol for tin (Sn) and its charge as a transition metal (4+). The hydroxide ion (OH-) is introduced, and the need to balance the charges in the ionic compound is discussed. By using four hydroxide ions, the charges are balanced to achieve a net charge of zero, resulting in the formula Sn(OH)4. The video concludes with a summary of the process.

What is the element symbol for tin as found on the periodic table?

• Te

• Pb

• Sn

• Ti

What is the charge of the tin ion in Tin(IV) Hydroxide?

• 4+

• 3+

• 2+

• 1+

What is the charge of the hydroxide ion?

• 2-

• 2+

• 1-

• 1+

Why do the charges in an ionic compound need to balance?

• To ensure the compound is stable

• To make the compound more reactive

• To change the compound's color

• To increase the compound's mass

How many hydroxide ions are needed to balance the charge of one tin ion in Tin(IV) Hydroxide?

• Four

• Two

• Five

• Three

What is the correct formula for Tin(IV) Hydroxide?

• Sn(OH)3

• SnO2

• Sn(OH)2

• Sn(OH)4