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Salt Analysis and d-block elements

Total questions: 100

Worksheet time: 51mins

Name
Class
Date
1.

Which block of elements are known as transition elements?

a)

p-block

b)

s-block

c)

d-block

d)

f-block

2.

Which one of the following is diamagnetic ion?

a)

Co2+

b)

Ni2+

c)

Cu2+

d)

Zn2+

3.

Colour of transition metal ions are due to absorption of some wavelength. This results in

a)

d-s transition

b)

s-s transition

c)

s-t/transition

d)

d-d transition

4.

Which of the following pairs of ions have the same electronic configuration?

a)

Cu2+, Cr2+

b)

Fe3+, Mn2+

c)

Co3+, Ni3+

d)

Sc3+, Cr3+

5.

Lanthanoid contraction is due to increase in

a)

atomic number

b)

effective nuclear charge

c)

atomic radius

d)

valence electrons

6.

Which of the following has magnetic moment value of 5.9 BM ?

a)

Fe2+

b)

Fe3+

c)

Ni2+

d)

Cu2+

7.

Which of the following are d-block elements but not regarded as transition elements?

a)

Cu, Ag, Au

b)

Zn, Cd, Hg

c)

Fe, Co, Ni

d)

Ru, Rh, Pd

8.

Transition elements form alloys easily because they have

a)

Same atomic number

b)

Same electronic configuration

c)

Nearly same atomic size

d)

None of the above

9.

Which one of the following characteristics of the transition metals is associated with higher catalytic activity?

a)

High enthalpy of atomisation

b)

Paramagnetic behaviour

c)

Colour of hydrate ions

d)

Variable oxidation states

10.

The property which is not characteristic of transition metals is

a)

variable oxidation states.

b)

tendency to form complexes.

c)

formation of coloured compounds.

d)

natural radioactivity.

11.

Transition elements shows variable oxidation states .

a)

True

b)

False

12.

Oxidation state of first transition series elements are related to their.....

a)

melting point and boiling point

b)

Reactivity and Size of their atoms

c)

electronic configuration

d)

Ionisation energy and Heat of sublimation

13.

Transition elements show variable oxidation states because……….

a)

the energy difference between (n-1)d and ns orbital is very large and the electrons from both these orbitals are used for bonding

b)

the energy difference between (n-1)d and ns orbital is very large and the electrons from both these orbitals are not used for bonding

c)

the energy difference between (n-1)d and ns orbital is very small and the electrons from both these orbitals are not used for bonding

d)

the energy difference between (n-1)d and ns orbital is very small and the electrons from both these orbitals are used for bonding

14.

The stable oxidation state of scandium is...

a)

+1

b)

+2

c)

+3

d)

+4

15.

From scandium to manganese the lower Oxidation state is given by ……..

a)

the number of electrons in the outer (n-1)d subshell

b)

the number of electrons in the outer s- subshell

c)

The sum of outer s and d electrons

d)

None of these

16.

From scandium to manganese the higher Oxidation state is given by ……..

a)

the number of electrons in the outer (n-1)d subshell

b)

the number of electrons in the outer s- subshell

c)

The sum of outer s and d electrons

d)

None of these

17.

Transition elements have a tendency to remain Noble for unreactive because…..

a)

they have variable oxidation states

b)

their melting point, ionization energy and heat of sublimation remains constant throughout the series

c)

they have low melting point, ionization energy and heat of sublimation

d)

they have high melting point, ionization energy and heat of sublimation

18.

The reactivity of transition elements goes on….

a)

decreasing across the series

b)

increasing across the series

c)

remains constant throughout the series

d)

none of these

19.

The colour of a transition metal ions is due to….

a)

Their high ionization energy

b)

Their low reactivity

c)

High melting point and boiling point

d)

d-d electron excitation

20.

The transition metal ions which have completely filled d-orbitals are ……..

a)

Coloured

b)

Colourless

c)

Both coloured and colourless

d)

None of these

21.

Second Transition Series is also called as …

a)

3d series

b)

4d series

c)

5d series

d)

6d series

22.

Second Transition Series consist of elements from …

a)

Scandium to Zinc

b)

Yttrium to Cadmium

c)

Yttrium to Palladium

d)

Hafnium to Mercury

23.

Atomic Number of Yttrium is ….

a)

19

b)

29

c)

39

d)

48

24.

Atomic Number of Cadmium is…

a)

49

b)

38

c)

39

d)

48

25.

Electronic Configuration of Niobium is ….

a)

[Kr] 5s2 4d3

b)

[Kr] 5s1 4d4

c)

[Kr] 5s0 4d5

d)

[Kr] 5s2 4d2

26.

Electronic Configuration of Molybdenum is ….

a)

[Kr] 5s2 4d4

b)

[Kr] 5s1 4d5

c)

[Kr] 5s2 4d5

d)

[Kr] 5s2 4d3

27.

1. Electronic Configuration of Palladium is ….

a)

[Kr] 5s2 4d8

b)

[Kr] 5s1 4d9

c)

[Kr] 5s0 4d10

d)

[Kr] 5s1 4d10

28.

Electronic Configuration of Silver is ….

a)

[Kr] 5s1 4d10

b)

[Kr] 5s2 4d9

c)

[Kr] 5s0 4d10

d)

[Kr] 5s2 4d10

29.

Atomic Number of Palladium is…

a)

45

b)

46

c)

47

d)

48

30.

Third Transition series is also called as …

a)

3d series

b)

4d series

c)

5d series

d)

6d series

31.

Third transition series consist of elements Lanthanum and from…….

a)

Scandium to Zinc

b)

Yttrium to Cadmium

c)

Hafnium to Mercury

d)

Yttrium to Mercury

32.

Atomic Number of Lanthanum is…

a)

56

b)

57

c)

58

d)

59

33.

Atomic Number of Mercury is…

a)

56

b)

72

c)

78

d)

80

34.

Atomic Number of Hafnium is…

a)

72

b)

71

c)

73

d)

80

35.

Electronic Configuration of Lanthanum is ….

a)

54[Xe] 6s2 5d1 4f 0

b)

54[Xe] 6s1 5d2 4f 0

c)

54[Xe] 6s0 5d3 4f 0

d)

54[Xe] 6s1 5d1 4f 1

36.

Electronic Configuration of Hafnium is …

a)

54[Xe] 6s2 5d1 4f 14

b)

54[Xe] 6s1 5d3 4f 14

c)

54[Xe] 6s2 5d2 4f0

d)

54[Xe] 6s2 5d2 4f 14

37.

What are typical oxidation state for Sc?

a)

-3

b)

+3

c)

-1

d)

+1

38.

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

a)

3p

b)

3s

c)

3d

d)

4s

39.
One metal that is liquid at room temperature is
a)
magnesium
b)
manganese
c)
mercury
d)
sodium
40.
If violet region is absorbed, what is the color that we see. Refer to color wheel
a)
Violet
b)
Orange
c)
Blue
d)
Yellow
41.
The name for Cr2S:
a)
Chromium (I) sulfide
b)
Chromium sulfide (I)
c)
Chromium (II) sulfide
d)
Chromium  sulfide (II)
42.
Which of the following is NOT a transition metal?
a)
Iron
b)
Gold
c)
Titanium
d)
Radium
43.
What colour is a compound that contains Fe3+?
a)
Brown solid
b)
Green solid
c)
Red solid
d)
Blue solid
44.
Which compound contains Cu2+?
a)
Compound A - blue solid
b)
Compound B - brown solid
c)
Compound C - green solid
d)
Compound D - white solid
45.
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
46.

Transition elements show variable oxidation state due to

a)

small size

b)

unpaired electron

c)

incomplete d orbital

d)

none of these

47.
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
48.
Why transition elements form complexes
a)
vacant d orbital
b)
smaller size
c)
higher charge on cation
d)
all of the above
49.

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

50.
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
51.

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

52.

Transition metal form interstial compounds due to

a)

void present in crystal lattice

b)

small size

c)

d-d transition

d)

all of these

53.
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
54.

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.

55.

Which of the following elements belong to actinoid-:

a)

Cerium

b)

Lutetium

c)

Thorium

d)

Lanthanum

56.

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

a)

3

b)

4

c)

5

d)

6

57.

d-d transition is possible only in-:

a)

Cu+1

b)

Cu+2

c)

Zn+2

d)

Zn

58.
Which of the following steps is NOT part of qualitative analysis?
a)
Cation tests
b)
Heat tests
c)
Melting point test
d)
Solubility
59.
Which of the following salts will produce a brown gas on heating?
a)
Lead(II) bromide
b)
Ammonium nitrate
c)
Potassium nitrate
d)
Zinc nitrate
60.
A solution X when added into sodium carbonate solution turns limewater cloudy. which of the following is solution X?
a)
Aqueous ammonia solution
b)
Calcium hydroxide solution
c)
Vinegar
d)
Magnesium nitrate solution
61.

Which of the following is insoluble?

a)

silver chloride

b)

zinc chloride

c)

potassium chloride

d)

ammonium chloride

62.

Which method is used to prepare lead (II) chloride?

a)

Pb(NO3)2(aq) + NaCl (aq) --->

b)

PbSO4(s)+ NaCl (aq) --->

c)

PbCO3(s) + NaCl (aq) --->

63.

Bryan wants to prepare silver chloride in the science laboratory. Which of the following reactants should he use?

a)

silver + hydrochloric acid

b)

silver hydroxide + hydrochloric acid

c)

silver nitrate + potassium chloride

d)

silver + chlorine gas

64.

Suzy wants to prepare potassium sulphate by reacting an acid with potassium hydroxide. Name the acid used in this experiment.

a)

hydrochloric acid

b)

nitric acid

c)

sulphuric acid

65.

In order to obtain a soluble salt from a solution, which of the following methods should be used

a)

filtration

b)

crystallization

c)

distillation

d)

fractional distillation

66.
Titration method is used to prepare salts from...
a)
Acid + Metal
b)
Acid + Alkali
c)
Base + Ammonium Salt
d)
Two Aqueous Solutions
67.

What is the colour of hydrated Copper (II) sulphate?

a)

White

b)

Blue

c)

Pink

d)

Brown

68.

Complete the following equation


Metal Carbonate + acid -->

a)

Salt + hydrogen

b)

Salt + water

c)

Salt + carbon dioxide

d)

Salt + carbon dioxide + water

69.
How do you test for oxygen gas?
a)
Makes a squeaky pop with a lit splint
b)
Relights a glowing splint
c)
Bleaches damp litmus paper
d)
Turns limewater milky
70.
How do you test for Chlorine gas?
a)
Bleaches damp litmus paper
b)
Makes a squeaky pop with a lit splint
c)
Relights a glowing splint
d)
Turns limewater milky
71.
All of the following salts are soluble except...
a)
Lead(II) nitrate
b)
Sodium carbonate
c)
Magnesium chloride
d)
Barium sulphate
72.

A solid is insoluble in water but dissolves in aqueous alkali without evolution of a gas. What could the solid be?

a)

Copper (II) carbonate

b)

Copper(II) hydroxide

c)

Zinc carbonate

d)

Zinc hydroxide

73.

What gas is formed when ammonium chloride is warmed with aqueous sodium hydroxide?

a)

Ammonia

b)

Chlorine

c)

Oxygen

d)

Hydrogen

74.

Which gas changes damp litmus paper from red to blue?

a)

Ammonia

b)

Carbon dioxide

c)

Chlorine

d)

Hydrogen

75.

In both experiments, a precipitate was obtained which dissolved in an excess of the added reagent. What could X contain?

a)

Copper (II) nitrate

b)

Iron(II) nitrate

c)

Iron(III) nitrate

d)

Zinc nitrate

76.

Which ion, in aqueous solution, forms a white precipitate when dilute sulfuric acid is added?

a)

Ag+

b)

Ba2+

c)

Cu2+

d)

Fe2+

77.

A metallic ion in aqueous solution produces

(i) white precipitate with aqueous sodium hydroxide, soluble in excess to produce a colourless solution.

(ii) white precipitate with aqueous sodium hydroxide, soluble in excess to produce a colourless solution.

What is the metallic ion?

a)

Al3+

b)

Ca2+

c)

K+

d)

Zn2+

78.

Aqueous sodium hydroxide reacts with a metal ion producing a coloured precipitate. This precipitate changes colour on standing. What is the ion present?

a)

Al3+

b)

Cu2+

c)

Fe2+

d)

Fe3+

79.

After acidification with dilute nitric acid, a colourless solution of X reacts with aqueous silver nitrate to give a white precipitate. What could X be?

a)

Calcium iodide

b)

Copper(II) chloride

c)

Lead(II) iodide

d)

Sodium chloride

80.

A salt is dissolved in water. The results of two separate tests on it are shown in the table.

  1. white precipitate which dissolved when excess aqueous ammonia is added.
  2. white precipitate is formed when dilute nitric acid and aqueous barium nitrate is added to the salt solution. What is the salt?
a)

Aluminium chloride

b)

Aluminium sulfate

c)

Zinc chloride

d)

Zinc sulfate

81.

A pale green solution X gives a green precipitate with excess aqueous sodium hydroxide. An alkaline gas is only given off when the mixture is warmed with aluminium powder. What ions foes X contain?

a)

Ammonium and copper(II)

b)

Ammonium and iron(II)

c)

Nitrate and copper(II)

d)

Iron(II) and nitrate

82.

Aluminium sulfate is used in water treatment. Aqueous aluminium sulfate is acidic. The options shows the pH and cation test using excess aqueous ammonia on four different samples of treated water. To which sample had an excess of aluminium sulfate been added?

a)

3, white precipitate

b)

3, no visible change

c)

7, no visible change

d)

11, white precipitate

83.

Aluminium sulfate is used in water treatment. Aqueous aluminium sulfate is acidic. The options shows the pH and cation test using excess aqueous ammonia on four different samples of treated water. To which sample had an excess of aluminium sulfate been added?

a)

3, white precipitate

b)

3, no visible change

c)

7, no visible change

d)

11, white precipitate

84.

What gas is formed when ammonium chloride is warmed with aqueous sodium hydroxide?

a)

Ammonia

b)

Chlorine

c)

Oxygen

d)

Hydrogen

85.

Isomerism that arises out of the difference in spatial arrangement of atoms or groups about the doubly bonded carbon atoms are called?

a)

Structural Isomerism

b)

Stereoisomerism

c)

Geometrical Isomerism

d)

Optical Isomerism

86.

Which among the following does not exhibit geometric isomerism?

a)

1-hexene

b)

2-hexene

c)

3-hexene

d)

4-hexene

87.

Which statement best defines chain isomerism?

a)

Existance of chemical compounds with same molecular formula

b)

Different ways the same number of carbons are connected which is either straight or branched

c)

Have mirror image of each other

d)

Similar chemical properties with different physical properties such as solubility

88.

How to determine that a molecule exhibit cis-trans isomerism?

a)

Restricted rotation in a carbon-carbon single bond of alkenes

b)

Each carbon of a site of restricted rotation has 2 different atoms or groups attached to it

c)

Exist in cyclic compouds only

d)

Similar chemical properties

89.

Which of the following molecules exhibit geometrical isomerism?

a)

CH2=CHCH3

b)

C6H5CH=CHC6H5

c)

(CH3)2C=CHCH3

d)

CH3CH2N=OH

90.

Isomerism exhibited by acetic acid and methyl formate is

a)

position

b)

chain

c)

functional

d)

metamerism

91.

Can enantiomer rotates plane-polarised light?

a)

Yes in all situations

b)

No because it is optically active

c)

Yes but it can only rotate the polarised light in opposite direction

d)

No due to its restricted rotation of carbon-carbon double bond

92.

1. CFT views the interaction between metal ions and ligands in complexes in terms of electrostatic _______________ and ____________________.

a)

attraction, repulsion

b)

positive, negative

c)

cation, anion

93.

Which orbital is very important in CFT?

a)

orbital p

b)

orbital s

c)

orbital d

94.

The sum of coordination number and oxidation number of the metal M in the complex [M(en)2 C2O4] Cl are

a)

6

b)

7

c)

8

d)

9

95.

In the complex [E(en)2(C2O4)]NO2 (where (en) is ethylenediamine) _______are the coordination number and the oxidation state of the element ‘E’ respectively.

a)

6 and 2

b)

2 and 2

c)

4 and 3

d)

6 and 3

96.

A complex compound in which the oxidation number of a metal is zero is

a)

K4 [Fe (CN)6]

b)

K3 [Fe (CN)6]

c)

[Ni (CO)4]

d)

[Pl (NH3 )4]Cl2

97.

A ligand can also be regarded as

a)

Lewis acid

b)

Bronsted base

c)

Lewis base

d)

Bronsted acid

98.

Which one is a cationic complex?

a)

K3[Fe(CN)6]

b)

Na2[Ni(EDTA)]

c)

[Co(en)2Cl2]Cl

d)

K3[Fe(CN)5NO]

99.

Which one is a neutral ligand?

a)

H2O

b)

NH3

c)

CO

d)

All of these

100.

Complexes having bidentate ligands are known as

a)

co-ordination sphere

b)

chelates

c)

central metal atom or ion

d)

complex ion

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