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d Block elements

Total questions: 60

Worksheet time: 30mins

Name
Class
Date
1.

What are typical oxidation state for Sc?

a)

-3

b)

+3

c)

-1

d)

+1

2.

Electron configuration for Sc is

a)

[Ar]4s23d1

b)

[Ar]4s13d1

c)

[Ar]4s13d2

d)

none of these

3.

Diamagnetism is shown when electrons are spin-paired

a)

Right

b)

Wrong

4.

d-block elements loses first elecrton(s) from...---subshell.

a)

3p

b)

3s

c)

3d

d)

4s

5.

What are typical oxidation state for Fe?

a)

+1

b)

+2

c)

+3

d)

+4

6.
One metal that is liquid at room temperature is
a)
magnesium
b)
manganese
c)
mercury
d)
sodium
7.
Which is a chemical property of metals
a)
Thermal conductivity
b)
Corrosion
c)
Electrical Conductivity
d)
Magnetism
8.
If violet region is absorbed, what is the color that we see. Refer to color wheel
a)
Violet
b)
Orange
c)
Blue
d)
Yellow
9.
If red/orange region is absorbed, what is the color that we see. Refer to color wheel
a)
Red
b)
Orange
c)
Blue
d)
Yellow
10.
3d orbitals are degenerate. What does it means?
a)
All 3d orbitals are in same order
b)
All 3d orbitals have different electron arrangement
c)
All 3d orbitals are in the same energy level
d)
All 3d orbitals have the same shape
11.
Ti3+ solution in the presence of water, is violet in color. Why?
a)
Presence of water ligands cause color formation
b)
Electron can be excited
c)
Wavelength of light can be absorbed
d)
Presence of water ligand cause the splitting the 3d orbitals
12.
Sc3+ solution in the presence of water is colorless. Why?
a)
Presence of ligands cause the splitting of 3d orbital.
b)
There is no splitting of 3d orbitals
c)
There is no electrons to be excited
d)
Energy level is too high for electron to reach
13.
Zn2+ solution in the presence of water is colorless. Why?
a)
Presence of ligands cause the splitting of 3d orbital.
b)
There is no splitting of 3d orbitals
c)
There is no electrons to be excited
d)
3d orbitals are fully filled and no electrons can be excited
14.
The name for Cr2S:
a)
Chromium (I) sulfide
b)
Chromium sulfide (I)
c)
Chromium (II) sulfide
d)
Chromium  sulfide (II)
15.
What is the correct formula for chromate ion?
a)
Cr2O7²⁻
b)
ClO₂⁻
c)
CrO₄²⁻
d)
HCO₃⁻
16.
Which of the following is NOT a transition metal?
a)
Iron
b)
Gold
c)
Titanium
d)
Radium
17.
What colour is a compound that contains Fe3+?
a)
Brown solid
b)
Green solid
c)
Red solid
d)
Blue solid
18.
Which compound contains Cu2+?
a)
Compound A - blue solid
b)
Compound B - brown solid
c)
Compound C - green solid
d)
Compound D - white solid
19.
The elements in Groups 3 through 12 are called ____________________ metals.  
They include: copper, nickel, gold, silver, iron
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
20.
What colour is a compound that contains Fe2+?
a)
Brown solid
b)
Green solid
c)
Red solid
d)
Blue solid
21.

Transition elements show variable oxidation state due to

a)

small size

b)

unpaired electron

c)

incomplete d orbital

d)

none of these

22.
why does transition metal form alloys with other transition metals?
a)
due to similar ionic size
b)
due to incomplete d orbital
c)
variable oxidation  state
d)
none
23.
Why transition elements form complexes
a)
vacant d orbital
b)
smaller size
c)
higher charge on cation
d)
all of the above
24.

Transition metals in many compounds acts as good catalyst due to

a)

complete d orbital

b)

unpaired electron

c)

large surface area

d)

none of these

25.
Transition metal form coloured complexes due to
a)
incomplete d orbital
b)
d-d transition
c)
absorption of radiation in visible region
d)
all the above
26.

Transition metal and its compound show paramagnetic behaviour due to presence of

a)

paired electron

b)

unpaired electrom

c)

coloured compound

d)

none of the above

27.
Melting point of transition metals are high
a)
due to strong ionic bond
b)
due to strong covalent bond
c)
due to  strong metallic bond
d)
due to strong H-bond
28.

Transition metal form interstial compounds due to

a)

void present in crystal lattice

b)

small size

c)

d-d transition

d)

all of these

29.
These elements are separated from the main part of the periodic table.  They are in the top row of this section.
a)
Lanthanides
b)
Actinides
c)
Alkali Metals
d)
Alkaline Earth Metals
30.

Cu2+ solution in the presence of water is blue. Why?

a)

Splitting of 3d orbital and electron can be easily excited

b)

Blue light is aborbed to excite elec to higher energy level

c)

Blue light is emitted when elec move to lower energy level

d)

3d orbital are partially filled and electrons can be excited

31.

Why is zinc not considered a transition metal?

a)

Zinc is not a transition metal because it gains two 4s electrons to give a 2+ion with full d subshell levels.

b)

Zinc is not a transition metal because it loses four 4s electrons to give a 4+ion with full d subshell levels.

c)

Zinc is not a transition metal because it loses two 4s electrons to give a 2+ion with full d subshell levels.

d)

Zinc is not a transition metal because it gains two 4d electrons to give a 2+ion with full d subshell levels.

32.

Density of transition metals is greater than the density of the Group 1 and 2 metals.

a)

True

b)

false

33.

The most common oxidation state of lanthanoids is-:

a)

+4

b)

+3

c)

+6

d)

+2

34.

Which of the following elements belong to actinoid-:

a)

Cerium

b)

Lutetium

c)

Thorium

d)

Lanthanum

35.

Which element among the lanthanoids has the smallest atomic radius ?

a)

Ce

b)

Lu

c)

Eu

d)

Gd

36.

Lanthanoids are placed in -:

a)

3rd group and 7th period

b)

3rd group and 6th period

c)

4rd group and 7th period

d)

4rd group and 5th period

37.

The general electronic configuration [Rn]5f1-14 6d0-1 7s2 is of -:

a)

Lanthanoids

b)

Actinoids

c)

s- block elements

d)

d-block elements

38.

The number of unpaired d electrons retained in Fe+2 (Z= 26) ion is -:

a)

3

b)

4

c)

5

d)

6

39.

d-d transition is possible only in-:

a)

Cu+1

b)

Cu+2

c)

Zn+2

d)

Zn

40.

The general electronic configuration [Xn]4f1-14 5d0-1 6s2 is of-:

a)

Lanthanoids

b)

Actinoids

c)

s- block elements

d)

d-block elements

41.

Which of the following transition elements is used as a catalyst in Haber’s process?

a)

Fe

b)

Ni

c)

Ti

d)

V

42.

Which of the following is the least basic in nature-

a)

La(OH)3

b)

Ce(OH)3

c)

Yb(OH)3

d)

Lu(OH)3

43.

Which of the following compounds is expected to be coloured?

a)

AgNO3

b)

CuSO4

c)

ZnCl2

d)

CuCl

44.

The general electronic configuration of transition elements is-:

a)

(n-1)d1-10 ns1-2

b)

(n-1)d10 ns1

c)

(n-1)d10 ns2

d)

(n-1)d5 ns1

45.

•Which of the following ion is diamagnetic in nature?

a)

Fe+3

b)

Sc +3

c)

Cr+2

d)

Cu+2

46.

Highest magnetic moment is shown by the ion-:

a)

Cr+3

b)

Fe+3

c)

Co+3

d)

V+2

47.

The most stable oxidation state of Ti is-:

a)

+5

b)

+2

c)

+3

d)

+4

48.

Which of the following are true about transition elements?

a)

Form coloured ions or compounds

b)

Show catalytic properties

c)

Appear as shiny grey solid

d)

Could form at least one stable simple ion with partially filled d-orbitals.

49.

X is a suitable material used to build aircraft jet engines because it has a low density and high resistance to corrosion. X is

a)

carbon fibre

b)

chromium

c)

titanium

d)

tin

50.

A transition metal is a...

a)

metal that forms multiple stable ions with a full d sub-level

b)

metal that forms one stable ion with a partially-filled d sub-level

c)

metal that forms one or more stable ions with a partially-filled sub-level

d)

metal that forms one stable ion with a full d sub-level

51.

Which is the correct electronic configuration for Fe2+?

a)

[Ar] 4s2 3d6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d 6

c)

[Ar] 3d6

d)

1s2 2s2 2p5 3s2 3p6 3d 6

52.

Why is zinc not considered a transition metal?

a)

Zinc is not a transition metal because it gains two 4s electrons to give a 2+ion with full d subshell levels.

b)

Zinc is not a transition metal because it loses four 4s electrons to give a 4+ion with full d subshell levels.

c)

Zinc is not a transition metal because it loses two 4s electrons to give a 2+ion with full d subshell levels.

d)

Zinc is not a transition metal because it gains two 4d electrons to give a 2+ion with full d subshell levels.

53.

Which of the following properties about transition elements is incorrect?

a)

Transition metals have variable oxidation state.

b)

They are the only elements that can form coloured ions in aqueous solution.

c)

Transition elements are good catalyst.

d)

They are the only elements that can form complexes.

54.

Cobalt has a proton number of 27. Choose the correct electronic configuration for Co4+.

a)

[Ar]3d34s2

b)

[Ar]3d7

c)

[Ar]3d74s2

d)

[Ar]3d5

55.

Which of the transition elements exhibit highest oxidation state?

a)

Manganese

b)

Vanadium

c)

Iron

d)

Chromium

56.

Gemstones such as diamonds, rubies, emeralds, and sapphires have different colours. Why?

a)

This is because gemstones contain ions or compounds of the metal elements

b)

This is because gemstones contain ions or compounds of the metallic elements

c)

This is because gemstones contain ions or compounds of the non-metal elements

d)

This is because gemstones contain ions or compounds of the transition elements

57.

What is the elctronic configuration of Cu2+

a)

[Ar] 3d10 4s1

b)

[Ar] 3d9 4s2

c)

[Ar] 3d9 4s0

d)

[Ar] 3d8 4s1

58.

Ni3+ cation has (a)   unpaired electrons

59.

The maximum oxidation state of chromium in its aqueous solution and compound is

(a)  

60.

The melting points of transition elements are above 1000 °\degree C because

(a)  

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