Draw all geometrical and linkage isomers of square planar \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{SCN})_{2}\)

Imagine a square with each corner holding tightly to an important corner piece. In chemistry, this image becomes very real in what we call a square planar complex. At the heart of the square sits a central metal atom, think of it as the king of its castle, surrounded on all sides by four loyal subjects, the ligands. Picture the game of checkers, the pieces are placed flat with one directly across from another. This flat arrangement is key because it creates different possibilities for how the molecules can arrange themselves.
In the example of Pt(NH3)2(SCN)2, platinum (Pt) is our king, and it has two types of ligands: the ammonia (NH3) and the thiocyanate (SCN). Thanks to the square planar structure, these ligands can sit next to each other in different patterns which leads to fascinating variations called isomers. This variety is not just for show; the different arrangements can lead to differences in chemical reactions and properties, making the understanding of square planar complexes an exciting area in the realm of coordination chemistry.

Within the kingdom of square planar complexes, the arrangement of the ligands can tell a story of two cities: 'Cis' and 'Trans'. These are the two major neighborhoods where our ligand citizens can live. Let's explore the bustling streets of cis and trans isomers.
In the cis configuration, two of the same ligands are next-door neighbors; they live side by side. In our case, the two NH3 ligands are adjacent, like two houses on the same block. This coziness affects how they interact with their surroundings, potentially making the entire molecule react in a certain way.
On the flip side, in the trans arrangement, the same ligands live across town from each other. Our NH3 friends are now at diagonal corners, staring across the square at one another. This separation could lead to a less congested interaction and different chemical behaviors. The personalities of 'Cisville' and 'Transtown' can greatly influence reactions, which is why understanding their unique layouts is a cornerstone for chemists crafting reactions or synthesizing new materials.

Stepping into the world of chemistry is akin to diving into a vibrant social scene where certain molecules, known as ambidentate ligands, are the life of the party. These are the social butterflies that can interact with the metal center through not one, but two different atoms.
Picture a friend who can shake your hand with either their left or right hand; that's what ambidentate ligands can do in the coordination chemistry universe. A classic example of such a ligand is the SCN- ion from our Pt(NH3)2(SCN)2 complex. It can attach to the central metal atom either through the sulfur (S) or the nitrogen (N) atom, effectively changing its 'handshake'.
Depending on which 'hand' the ligand uses to hold onto the metal, the properties of the resulting complex can change dramatically. This chameleon-like behavior can make ambidentate ligands tricky to predict but incredibly valuable for creating a diverse set of compounds with a wide range of applications, from catalysis to pharmaceuticals. These ligands teach us the importance of flexibility and adaptability in chemistry.