Final answer:
The number of bonds transition metals form is determined by their oxidation state, with transitions between ionic and covalent character depending on whether the oxidation state is low or high.
Step-by-step explanation:
The number of bonds transition metals can make is primarily dictated by their oxidation state. Transition metals are known for having multiple oxidation states which implies that they can exhibit a variety of chemical behaviors in bonding. For example, a transition metal in a lower oxidation state typically forms more ionic compounds, while in a higher oxidation state, it tends to form more covalent compounds or polyatomic ions. This is because the electronegativity of transition metals can vary with their oxidation states, so when transition metals are in very high oxidation states, their electronegativity values may become close to that of oxygen, leading to covalent bonding in oxides.
To determine the number of bonds a transition metal will form, we should look at the specific compound and identify the metal's oxidation state, which requires knowledge of electron configuration and the rules for oxidation states. Commonly observed oxidation states are a result of the metal losing electrons from both s and d orbitals; specifically, the 4s electrons are lost first.