Question

The maximum atomic radius exists for (1) \(\mathrm{Mg}\) (2) \(\mathrm{N}\) (3) Si (4) \(\mathrm{P}\)

Short answer

Magnesium (Mg)

Step-by-step solution

Understand Atomic Radius

The atomic radius is the distance from the nucleus of an atom to the outermost electron shell. It generally increases as you move down a group in the periodic table and decreases as you move across a period from left to right.

Identify the Periods and Groups

List the positions of each element in the periodic table:- \(\text{Mg (Magnesium)}\) is in Group 2, Period 3.- \(\text{N (Nitrogen)}\) is in Group 15, Period 2.- \(\text{Si (Silicon)}\) is in Group 14, Period 3.- \(\text{P (Phosphorus)}\) is in Group 15, Period 3.

Compare Across the Period

Elements in the same period should be compared from left to right. \(\text{Mg}\), \(\text{Si}\), and \(\text{P}\) are all in Period 3. Magnesium \(\text{Mg}\) is further to the left and typically has a larger atomic radius than \(\text{Si}\) and \(\text{P}\) due to fewer protons causing less attraction to the electrons.

Compare by Group

Moving down a group increases the atomic radius. However, since Nitrogen (Group 15, Period 2) is in an earlier period than Magnesium, its atomic radius will be smaller than Magnesium and the others in Period 3.

Conclusion

Based on their positions in the periodic table, \(\text{Mg}\) has the largest atomic radius among \(\text{Mg}\), \(\text{N}\), \(\text{Si}\), and \(\text{P}\).

Key concepts

atomic radius

The atomic radius is a fundamental concept in chemistry indicating the size of an atom. It is defined as the distance from the center of the nucleus to the outermost shell of an electron. When comparing atomic sizes, it's important to note that the atomic radius can be influenced by various factors.

The precise size of the atomic radius can offer insights into how atoms bond with each other and their reactivity. Here are key points about atomic radius:

• Measured typically in picometers (pm) or angstroms (Å)
• Varies depending on whether you're discussing covalent radius, ionic radius, or metallic radius
• Can be influenced by the type of electron orbitals involved

Overall, the atomic radius provides a useful picture of how large an atom is and how it may interact in different chemical contexts. Always keep in mind that atomic radius trends are predictable but can vary based on atomic structure and energy levels.

periodic table trends

Periodic table trends are patterns observed within the elements organized in the periodic table. One of the most significant trends is the change in atomic radius as one moves across periods or down groups.

As you progress from left to right across a period, the atomic radius generally decreases. This occurs because the number of protons in the nucleus increases, creating a stronger attraction to electrons, pulling them closer to the nucleus.

Conversely, moving down a group increases the atomic radius. This is due to the addition of electron shells, which outweighs the increased nuclear charge, resulting in atoms becoming larger. These trends help predict and explain chemical behavior and bonding properties of elements.

• Across a Period: Atomic radius decreases
• Down a Group: Atomic radius increases
• Helps in understanding reactivity and bonding characteristics

These trends are incredibly useful when understanding how elements will react with one another and predicting the properties of unknown or less-studied elements.

element comparison

When comparing elements, particularly their atomic radii, it's important to look at their positions within the periodic table and understand periodic trends.

Consider elements Magnesium (Mg), Nitrogen (N), Silicon (Si), and Phosphorus (P). Comparing their atomic radii involves checking their respective periods and groups and applying periodic trends:

• Magnesium (Mg): Group 2, Period 3 - Larger atomic radius as it is in the leftmost position in its period
• Nitrogen (N): Group 15, Period 2 - Smaller atomic radius due to being in a higher period
• Silicon (Si): Group 14, Period 3 - Smaller than Mg since it is further to the right
• Phosphorus (P): Group 15, Period 3 - Slightly larger than Si but smaller than Mg

By understanding the group and period positions, and how elements interact with periodic trends, one can determine that Magnesium (Mg) has the largest atomic radius among these elements. This doesn't just help with specific comparisons but aids in predictions across the periodic table.