Transition vs d-block elements

Watch
This discussion is closed.
qqqwwweee
Badges: 2
Rep:
?
#1
Report Thread starter 15 years ago
#1
Just want to check whether the definitions I learnt are right.

d-block elements are those having outer electrons in d orbitals which are in the process of being filled.
Transition elements are d-block elements forming one or more stable ions which have incompletely filled d-orbitals.
Are they correct?

So, Zinc is neither a d-block nor transition element?
Are all transition elements d-block elements?
Can anyone suggest some examples of d-block elements which are not transition element? Is Scandium a transition element?
0
MadNatSci
Badges: 12
Rep:
?
#2
Report 15 years ago
#2
(Original post by keisiuho)
Just want to check whether the definitions I learnt are right.

d-block elements are those having outer electrons in d orbitals which are in the process of being filled.
Transition elements are d-block elements forming one or more stable ions which have incompletely filled d-orbitals.
Are they correct?

So, Zinc is neither a d-block nor transition element?
Are all transition elements d-block elements?
Can anyone suggest some examples of d-block elements which are not transition element? Is Scandium a transition element?

Zinc is a d-block element, in the last d-block column, but not a transition metal. Scandium is not a transition element, no. Silver is also a bit anomalous, but I'm still not sure why exactly it only forms one ion...
0
ianaf18
Badges: 0
#3
Report 15 years ago
#3
d-block element = an element which has at least one bonding electron in its d shell.
e.g scandium and zinc

Transition elemnet = an elment which forms one or more ions with a partially filled d subshell and are stable under normal conditions.
0
qqqwwweee
Badges: 2
Rep:
?
#4
Report Thread starter 15 years ago
#4
(Original post by ianaf18)
d-block element = an element which has at least one bonding electron in its d shell.
e.g scandium and zinc
Why does Zinc have bonding electrons in its d shell? It is fully filled.
0
ResidentEvil
Badges: 1
Rep:
?
#5
Report 15 years ago
#5
so is Zinc^(2+) a transition element then? or Sc^(3+)? or are these ions and not elements that they wont be classed as transitional elements?
0
crana
Badges:
#6
Report 15 years ago
#6
(Original post by ResidentEvil)
so is Zinc^(2+) a transition element then? or Sc^(3+)? or are these ions and not elements that they wont be classed as transitional elements?
no - even these ions still have full d-shells. eg the electronic structure of Zn (outermost shells) is 3d10 4s2

so when it becomes Zn 2+ it still has a full dshell as it only loses the outer s electrons.

I don't think Sc actually forms Sc 3+ although I may be wrong.

regarding the 2nd part of your question, a transition element is one that has an incomplete d shell in one of its oxidation states (i think?) so even if the element has a fll d shell, if it forms an ion with an incomplete d
shell it still counts as transition.

But this is why for e.g. Cu(I) compounds are usually colourless but Cu(2) compounds usually coloured (coloured compounds being a common feature of transition metals) - only the Cu(2) has an incomplete d shell

rosei
0
hornblower
Badges: 0
Rep:
?
#7
Report 15 years ago
#7
A d block element is an element where the highest occupied energy level is a d orbital.

A transition element is an element that forms at least one stable ion with a partially filled d shell.
0
X
new posts
Back
to top
Latest
My Feed

See more of what you like on
The Student Room

You can personalise what you see on TSR. Tell us a little about yourself to get started.

Personalise

If you do not get the A-level grades you want this summer, what is your likely next step?

Take autumn exams (125)
46.64%
Take exams next summer (39)
14.55%
Change uni choice through clearing (68)
25.37%
Apply to uni next year instead (24)
8.96%
I'm not applying to university (12)
4.48%

Watched Threads

View All