Final answer:
The predominant type of bonding in titanium varies based on its oxidation state. In metallic titanium, the bonding is metallic, whereas in compounds like titanium (IV) oxide (rutile), the bonding is more covalent due to the similar electronegativities of titanium and oxygen.
Step-by-step explanation:
The predominant type of bonding in titanium (Ti) largely depends on its chemical context, especially the oxidation state of titanium. When we consider titanium in the form of titanium (IV) oxide, also known as rutile, we are looking at a type of crystal where titanium shows a +4 oxidation state. According to the information provided, oxides with higher oxidation states, like TiO₂, tend to have more covalent bonding because the electronegativity of titanium in this state is closer to that of oxygen, leading to a shared pair of electrons rather than a full transfer.
Additionally, titanium can also exhibit metallic bonding when it is in its metallic form, where electrons are delocalized in a 'sea' around positively charged metal ions. This allows metals to conduct electricity and heat, and provides them with their malleability and ductility. In contrast, titanium compounds in which titanium is in a lower oxidation state would have more ionic character, as the metal would have an electronegativity significantly lower than that of oxygen.
The rutile crystal illustrated by titanium dioxide (TiO₂) has a tetragonal structure with a coordination number of 6 for the Ti⁴⁺ ions, which stresses the significance of its covalent character. Lastly, titanum also forms compounds with halides, where it has significant covalent characteristics due to the likely high oxidation state of titanium, making the titanium-halogen bonds more covalent in nature.