Final answer:
A bond formed between a dx²-y² orbital and a px orbital approaching along the x-axis would likely be a π (pi) bond, although without additional context, the formation of a double bond cannot be definitively concluded.
Step-by-step explanation:
When considering the type of bond formed between orbitals, it's essential to look at the orbital symmetries and their overlapping pattern. In this case, the bonding involves the dx²-y² orbital and a px orbital approaching along the x-axis.
Types of Molecular Orbitals
The dx²-y² orbital has four lobes lying in the xy plane along the axes and the px orbital also lies along the x-axis. This arrangement allows for effective sidewise overlap between these orbitals, but since the approach is directly along the x-axis, which suitably aligns with one of the lobes of the dx²-y² orbital, a π (pi) bond may form. In textbooks, formations of pi bonds are often depicted with adjacent p orbitals combining along planes that are parallel but not along the internuclear axis, which is characteristic of pi bonding.
However, without more context regarding the molecular geometry and electronic effects, the question's constraints are insufficient to definitively conclude that a double bond will form, though it's possible if another p orbital (for example, py) from the same atom could approach the dx²-y² region in a suitable orientation for bonding.