Questions: Arrange the following elements in order of increasing (1 = smallest, 4 = largest) atomic radius: Ge, N, P, Si. N Ge P Si

Transcript text: Arrange the following elements in order of increasing (1 = smallest, 4 = largest) atomic radius: $\mathrm{Ge}, \mathrm{N}, \mathrm{P}, \mathrm{Si}$. $\square$ N $\square$ Ge $\square$ P $\square$ Si

Solution

Solution Steps

Step 1: Understanding Atomic Radius Trends

The atomic radius generally increases as you move down a group in the periodic table because additional electron shells are added. Conversely, the atomic radius decreases as you move across a period from left to right due to the increasing nuclear charge, which pulls the electrons closer to the nucleus.

Step 2: Identify the Position of Elements

Nitrogen (N) is in Group 15, Period 2.
Phosphorus (P) is in Group 15, Period 3.
Silicon (Si) is in Group 14, Period 3.
Germanium (Ge) is in Group 14, Period 4.

Step 3: Arrange Elements by Atomic Radius

Nitrogen (N): Being in Period 2, it has the smallest atomic radius among the given elements.
Silicon (Si): In Period 3, it has a larger atomic radius than nitrogen.
Phosphorus (P): Also in Period 3, but in the same group as nitrogen, it has a slightly larger atomic radius than silicon.
Germanium (Ge): In Period 4, it has the largest atomic radius among the given elements.