Considering the atomic number and position in the periodic table, arrange the following elements in the increasing order of metallic character: Si, Be, Mg, Na, P.
P < Si < Be < Mg < Na
Explanation
Metallic character increases down a group and decreases along a period as we move from left to right.
In the given elements, P and Si belong to the 3rd period. Moving from left to right, the metallic character decreases, making P less metallic than Si.
Be and Mg belong to Group 2. Since metallic character increases down a group, Mg is more metallic than Be. Na is in Group 1 and is located to the left of Mg in the 3rd period, making it the most metallic among all the given elements.
Therefore, the increasing order of metallic character is: P < Si < Be < Mg < Na.
Solution Steps
Step 1: Recall the periodic trend: metallic character increases down a group and decreases from left to right across a period.
Step 2: Compare elements in the same period (P and Si in the 3rd period): P is to the right of Si, so P is less metallic (P < Si).
Step 3: Compare elements in the same group (Be and Mg in Group 2): Mg is below Be, so Mg is more metallic (Be < Mg).
Step 4: Compare positions across the table: Na is in Group 1, left of Mg in the 3rd period, making it the most metallic. Combine all comparisons to get the final order: P < Si < Be < Mg < Na.