Was doing some past paper questions and i’m not sure why B is the answer not C, please help. Which shows the configuration of an atom of a transition metal?: A [Ar] 4s2,3d0 B [Ar] 4s2,3d8 C [Ar] 4s2, 3d10 D [Ar] 4s2, 3d10, 4p1
Was doing some past paper questions and i’m not sure why B is the answer not C, please help. Which shows the configuration of an atom of a transition metal?: A [Ar] 4s2,3d0 B [Ar] 4s2,3d8 C [Ar] 4s2, 3d10 D [Ar] 4s2, 3d10, 4p1
So you have 2 definitions I will write for you d block element - atom whose highest energy orbital is a d orbital Transition element - d block element that can form at least one ion with a partially filled d subshell. For this reason, Zinc and Scandium are not considered transition elements For writing the electron configurations, remember Cu and Cr are your exceptions, needing a full d subshell and half d subshell respectively. So has a 4S1. These are the only exceptions for the transistion elements For example, Cu is [Ar]4s1,3d10 Cu1+ is [Ar]3d10 Cu2+ is [Ar]3d9 It has formed at least one ion with a partially filled d subshell A - highest energy is s orbital, not a d block element D - highest energy is p orbital, not a d block element C - is Zinc, which is a d block element, but not a transition metal