Chemistry - unit 5 - section 2: transitional metals

what is transitional metal

a d-block element that can form at least one stable ion with a partially filled (incomplete subshell)

how many electrons can d-block hold

10 electrons

which two element is a exception to the first row of d -block elements

scandium and zinc as they don’t form a stable ion with a partially filled d-subshell

how do electrons fill the shell of the 8 transitional elements

first up fill up singly in an unoccupied orbital then double up. As the electrons repel each other

transitional metals box notations

the common exception in 3d box notations

chromium and copper - an electron from the 4s orbital moves into the 3sd orbital to create a more stable half full or full subshell

why is scandium not a transitional metal

scandium forms only 1 stable ion of Sc3+

s3+ has an empty d - subshell, as it is not partially filled it is not a transitional metal

why is zinc not a transitional metal

zinc only forms only 1 stable ion of zn2+

zn2+ has a full d - subshell. as it is not partially filled it is not a transition element

how to check the electron configuration

add all the numbers in the electron configuration of an element and compare answer with the atomic number

the electron configuration for Fe3+

properties of transitional metals

variable oxidation states because the electrons sits in4s and 3d