K and Ti both have d shells available for bonding. K is an alkali metal with an oxidation state of +1. K, otassum will form ionic bonds with the elements in Group 7 (halogens-salt makers).

Ti is a transion metal. Transition form coordination complexes. If you place transition metals in solution you can determine the corresponding oxidation states of the resulting ions. Transition metals have several oxidation states, but nonbonded transition metals only exhibit relatively low oxidation states. Many transition metals share the same oxidation states, and each row follows similar patterns.

Transition metals form coordination complexes....in solution this is often evidenced by highly colored solutions.

See this link:

http://en.wikipedia.org/wiki/TitaniumYes, Ti has what is called dsp hybridization/bonding. And yes all three orbitals participate in the bonding.

K: 1s

^{2}, 2s

^{2}, 2p

^{6} 3s

^{2 } 3p

^{6} 4s

^{2} or [Ar] 4s

^{2}Ti: 1s

^{2} 2s

^{2} 2p

^{6} 3s

^{2 } 3p

^{6 } 4s

^{2} 3d

^{2} or [Ar] 4s

^{2} 3d

^{2}Ti

^{+2}:[Ar]3d

^{2}Ti

^{+3}:[Ar]3d

^{1}For Ti we can write Ti: 1s

^{2} 2s

^{2} 2p

^{6} 3s

^{2} 3p

^{6} 3d

^{2} 4s

^{2} So for Ti we have 3s

^{2} 3p

^{6} 3d

^{2}Ti forms d

^{2}sp

^{3} Hybrids

These particular d

^{2}sp

^{3} hybrids are combinations of two 3d, the 3s, and three 3p functions.

The 3s : 3 is the energy level, S is the subshell, 1 orbital

The 3p: 3 is the energy, p is the subshell, 3 orbitals px, py, and pz

The 3d: 3 is the energy, d is the subshell, 5 orbitals d

_{yz}, d

_{xz}, d

_{xy}, d

_{x}_{2-y2}, and d

_{z}_{2.}In general:

S subshell has only 1 orbital.

The p subshell has 3 orbitals.

The d subshell has 5 orbitals.

The f subshell has 7 orbitals.

In Ti there are 2 electrons in the 3d shell.

Hence, the designation d

^{2}sp

^{3} Hybrids (TiCl-an octahedral complex)

For octahedral complexes: There are six d

^{2}sp

^{3} hybrid orbitals. They are arranged in an octahedral layout so that each has four other orbitals at 90° to it and one at 180°.

The following links should help you too:

http://faculty.colostate-pueblo.edu/linda.wilkes/111/3c.htmhttp://winter.group.shef.ac.uk/orbitron/AO-hybrids/d2sp3/index.htmlhttp://www.chem1.com/acad/webtext/chembond/cb09.htmlhttp://en.wikipedia.org/wiki/Titanium(III)_chloride