D and F Block

Why Zn,Cd,Hg are not transition metals?

Fully filled d orbital

General electronic configuration of d block elements

(n-1)d1-10ns1-2

Energy difference between (n-1)d and ns2 is

Little

Why D block elements show variable oxidation state?

Due to partially filled d orbital

D block elements have similarity

Across the period

Silver atom has completely filled d orbitals (4d10) in its ground state.
How can you say that it is a transition element?

It can show variable oxidation state and form complexes

What elements have more than one structure at room temp?

Zn,Cd,Hg,Mn

Zn,Cd,Hg are also called

Soft metals

Melting point curve has a maxima at mid of the series indicating that

1 electron in d orbital is more favourable for interatomic interactions

What does high enthalpy of atomisation mean?

High boiling point

Why frequent metal-metal bonding occurs in heavy transition metals?

High enthalpies of atomisation

What is Lanthanoid contraction?

The decrease in atomic radii because of filling of electrons in 4f orbital before 5d orbital.

What is a consequence of lanthanoid contraction?

The second and the third series have similar radii and properties

Shielding order in orbitals(high to low)

spdf

Enthalpy of atomisation is maximum for which element in 3d series?

Vanadium

Enthalpy of atomisation is minimum for which element in 3d series?

Zinc

Why transition metals have high enthalpy of atomisation?

Due to unpaired electrons they have strong interatomic interaction and hence stronger bonding

Why Zinc has the lowest enthalpy of atomisation?

No unpaired electrons

The first ionisation enthalpy order of 3d series doesn’t follow a smooth trend because

Removing one electron changes the way the other electrons are arranged

Why is it difficult to obtain os greater than 2 for Cu,Zn,Ni

Due to high enthalpies of ionisation

Which 3d element exhibits the max no. of os?

Manganese

Which os state of titanium is most stable?

4

What is the reason for variable os?

Incomplete filling of d-orbitals

In p block the lower oxidation states are favoured by

Heavier metals

Why lower os are favored by heavier metals in p-block?

Due to inert pair effect

A transition element that doesn’t exhibit variable oxidation states

Scandium

What is the reason for the inability of Cu to generate H2 from acids?

Positive electrode potential

What is the reason for +ve electrode potential of Cu?

Low hydration enthalpy compared to the energy required to transform Cu(s) to Cu2+(aq)

Beyond Mn no metal has a trihalide except?

Fe n Co

Why F is able to stabilise the highest oxidation state in CoF3?

Due to higher lattice energy

What accounts for F’s stability in higher covalent compounds?

Higher bond enthalpy

Fluorides are instable in

Lower os

Cu(1) compounds are unstable and undergo

Disproportionation

Which is more stable Cu+ or Cu2+?

Cu2+

Why Cu2+ is more stable than Cu+?

Negative hydration enthalpy

Stability to stabilise higher os is more for

Oxygen

Does Mn2O7 have an Mn-O-Mn bridge?

Yes

In Mn2O7 each Mn is surrounded by an O by what formation

Tetrahedral

Mn3O4 is a mixed oxide of

Mno,Mno2

In +3 state what are the elements that are strong oxidising agents

Manganese and Cobalt

In +2 state what elements are strong reducing agents?

Titanium,Vanadium and Chromium

What is the reason for the irregularity in the trend of electrode potential?

Irregular variation of ionisation enthalpies and sublimation enthalpies

Except which metal the members of the 3d series are more reactive

Copper

The general trend in less negative electrode potential is due to

Increase in sum of first and second ionisation enthalpy

What substances are repelled by a magnetic field?

Diamagnetic

What substances are attracted by a magnetic field?

Paramagnetic

Colour of Ti3+

Purple

Colour of V4+

Blue

Colour of V3+

Green

Colour of V2+

Violet

Colour of Cr3+

Violet

Colour of Mn3+

Violet

Colour of Cr2+

Blue

Colour of Mn2+

Pink

Colour of Fe3+

Yellow

Colour of T