Transition elements
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Describe d-block elements
-found in the middle of the periodic table -some elements are transition metals
what is a transition element?
d-block element that can form at least one stable ion with a partially filled (incomplete) d-subshell
d-subshell can hold up to how many electrons?
10
How does chromium and copper behave differently in electron configuration compared to other transition elements in period 4?
An electron from the 4s orbital moves into the 3d orbital to create a more stable half full (Cr) or full 3d sub-shell respectively (Cu)
Why is scandium not a transition element?
-scandium forms ion Sc3+ -Sc3+ has an empty d-subshell. As it is not partially filled, it is not a transition element
Why is zinc not a transition element?
-Zinc forms ion Zn2+ -Zn2+ has a full d-subshell. As it is not partially filled, it is not a transition element.
How do transition metals lose electrons in a specific way to form ions?
lose from 4s first then 3d
What are the properties of transition metals?
-variable oxidation states -form coloured ions in solution -good catalysts
Why do transition metals have variable oxidation states?
because the electrons sit in the 4s and 3d energy levels which are very close. As a result, electrons are gained and lost using a similar amount of energy when they form ions
V 2+ colour?
violet
V 3+ colour?
green
VO 2+ colour?
blue
Cr 3+ colour?
green
Cr2O7 2- colour?
orange
Mn2+ colour?
pale pink
MnO4 2- colour?
green
MnO4- colour?
purple
Fe2+ colour?
pale green
Fe3+ colour?
yellow
Co2+ colour?
pink
Ni2+ colour?
green
Cu2+ colour?
blue
Ti2+ colour?
violet
Ti3+ colour?
purple