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This means both Ti and Sc form stable ions with an electronic configuration of 3s2 3p6. This means Sc and Ti lose 3 and 4 electrons respectively hence forming the Sc3+ and the Ti4+ ions.
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Scandium Sc 1s2 2s2 2p6 3s2 3p6 3d1 4s2
Titanium Ti 1s2 2s2 2p6 3s2 3p6 3d2 4s2
Vanadium V 1s2 2s2 2p6 3s2 3p6 3d3 4s2
Chromium Cr 1s2 2s2 2p6 3s2 3p6 3d5 4s1
Manganese Mn 1s2 2s2 2p6 3s2 3p6 3d5 4s2
Iron Fe 1s2 2s2 2p6 3s2 3p6 3d6 4s2
Cobalt Co 1s2 2s2 2p6 3s2 3p6 3d7 4s2
Nickel Ni 1s2 2s2 2p6 3s2 3p6 3d8 4s2
Copper Cu 1s2 2s2 2p6 3s2 3p6 3d10 4s1
Zinc Zn 1s2 2s2 2p6 3s2 3p6 3d10 4s2
As Chromium and Copper are in the fourth period we would expect it to follow the same pattern as the other elements in the same periods as in the 4s sub shell is filled first rather than the 3d sub shell...
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