Question

1. a student needs to predict the properties of element y, which is located in group 16, period 3. using the periodic table as a model, which set of predictions is most accurate? y will be a metal, solid at room temperature, with 6 valence electrons, forming y²⁻ ions. y will be a nonmetal, solid at room temperature, with 6 valence electrons, forming y²⁻ ions. y will be a metalloid, liquid at room temperature, with 16 valence electrons, forming y²⁻ ions. y will be a nonmetal, gas at room temperature, with 3 valence electrons, forming y³⁻ ions.

Explanation:

Step1: Analyze group - 16 elements

Elements in Group 16 (also called chalcogens) are mostly non - metals. Oxygen is a gas, sulfur and selenium are solids at room temperature. The general electron configuration of Group 16 elements gives them 6 valence electrons. Non - metals in this group tend to gain 2 electrons to form anions with a charge of - 2.

Step2: Evaluate each option

• Option 1: Elements in Group 16 are not metals. So this option is incorrect.
• Option 2: Non - metal, solid at room temperature (like sulfur and selenium), 6 valence electrons and forms $Y^{2 - }$ ions (by gaining 2 electrons to achieve a stable octet) is correct.
• Option 3: Group 16 elements are not metalloids (except polonium but it's a special case and not liquid at room temperature), and they do not have 16 valence electrons. So this option is incorrect.
• Option 4: Group 16 elements are not gases with 3 valence electrons. So this option is incorrect.

Answer:

Y will be a nonmetal, solid at room temperature, with 6 valence electrons, forming $Y^{2 - }$ ions.