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Chemistry > D BLOCK > Flashcards

D BLOCK Flashcards

1
Q

What groups in the periodic table make up the d-block?

A

Groups 3-12.

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2
Q

Which orbitals are progressively filled in the d-block elements?

A

The d orbitals.

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3
Q

How many long periods are there in the periodic table where the d-block elements are found?

A

Four long periods.

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4
Q

What does the f-block of the periodic table consist of?

A

Elements in which the 4f and 5f orbitals are progressively filled.

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5
Q

Where is the f-block placed in the periodic table?

A

In a separate panel at the bottom of the periodic table.

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6
Q

What is another name for d-block elements?

A

Transition metals.

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7
Q

What is another name for f-block elements?

A

Inner transition metals.

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8
Q

How many series of transition metals are there?

A

Four series: 3d, 4d, 5d, and 6d.

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9
Q

What elements make up the 3d series of transition metals?

A

Scandium (Sc) to Zinc (Zn).

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10
Q

What elements make up the 4d series of transition metals?

A

Yttrium (Y) to Cadmium (Cd).

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11
Q

Which elements are part of the 5d series of transition metals?

A

Lanthanum (La) and Hafnium (Hf) to Mercury (Hg).

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12
Q

What elements are included in the 6d series of transition metals?

A

Actinium (Ac) and elements from Rutherfordium (Rf) to Copernicium (Cn).

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13
Q

What are the two series of inner transition metals called?

A

Lanthanoids (4f series) and Actinoids (5f series).

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14
Q

What elements are included in the 4f series?

A

Cerium (Ce) to Lutetium (Lu).

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15
Q

What elements are included in the 5f series?

A

Thorium (Th) to Lawrencium (Lr).

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16
Q

Why were transition metals originally named so?

A

Because their chemical properties were transitional between those of s- and p-block elements.

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17
Q

How does IUPAC define transition metals?

A

Metals with incomplete d subshells either in their neutral atoms or in their ions.

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18
Q

Why are zinc (Zn), cadmium (Cd), and mercury (Hg) not regarded as transition metals?

A

They have a full d¹⁰ configuration in their ground state and common oxidation states.

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19
Q

Why are the chemistries of Zn, Cd, and Hg studied along with transition metals?

A

They are the end members of the 3d, 4d, and 5d transition series, respectively.

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20
Q

What makes transition elements different from other elements?

A

The presence of partly filled d or f orbitals in their atoms.

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21
Q

Can the usual theory of valence for non-transition elements be applied to transition elements?

A

Yes, the usual theory of valence can be successfully applied to transition elements as well.

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22
Q

Which precious metals belong to the transition metals series?

A

Silver, gold, and platinum.

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23
Q

Which industrially important metals are part of the transition metals series?

A

Iron, copper, and titanium.

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24
Q

Where is the d-block located in the periodic table?

A

In the large middle section, flanked between the s- and p-blocks.

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25
Q

Which orbitals receive electrons in d-block elements?

A

The d-orbitals of the penultimate energy level.

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26
Q

How many rows of transition metals are there, and what are they?

A

Four rows: 3d, 4d, 5d, and 6d.

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27
Q

What is the general electronic configuration of the outer orbitals in d-block elements?

A

(n-1)d^1-10 ns^1-2, except for palladium (Pd), which has 4d^10 5s^0.

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28
Q

What does (n-1) represent in the electronic configuration of d-block elements?

A

It represents the inner d orbitals, which may have 1 to 10 electrons.

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29
Q

How many electrons can the outermost ns orbital of d-block elements have?

A

One or two electrons.

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30
Q

Why are there exceptions to the general electronic configuration in d-block elements?

A

Because of the small energy difference between (n-1)d and ns orbitals, and the extra stability of half-filled and completely filled orbitals.

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31
Q

What is the electronic configuration of chromium (Cr) in the 3d series?

A

3d^5 4s^1 instead of 3d^4 4s^2.

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32
Q

Why does chromium (Cr) have an unusual electronic configuration?

A

The energy gap between the 3d and 4s orbitals is small, and the half-filled 3d^5 configuration is more stable.

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33
Q

What is the electronic configuration of copper (Cu) in the 3d series?

A

3d^10 4s^1 instead of 3d^9 4s^2.

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34
Q

Why does copper (Cu) have an unusual electronic configuration?

A

The completely filled 3d^10 configuration is more stable than 3d^9 4s^2.

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35
Q

What is the general electronic configuration of Zn, Cd, Hg, and Cn?

A

(n-1)d^10 ns^2.

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36
Q

Why are Zn, Cd, Hg, and Cn not considered transition elements?

A

Their orbitals are completely filled in both the ground state and their common oxidation states.

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37
Q

Why do the d orbitals of transition elements influence their surroundings more than s and p orbitals?

A

Because the d orbitals protrude to the periphery of an atom more than s and p orbitals.

38
Q

What similarities do ions with a given d^n configuration (n = 1–9) exhibit?

A

They have similar magnetic and electronic properties.

39
Q

What characteristic properties do transition elements exhibit due to partly filled d orbitals?

A
  1. Display of a variety of oxidation states. 2. Formation of colored ions. 3. Ability to form complexes with a variety of ligands.
40
Q

What other properties do transition metals and their compounds exhibit?

A

Catalytic property and paramagnetic behavior.

41
Q

Do transition elements show more similarities within a row or a group?

A

They show greater similarities in a horizontal row compared to non-transition elements, though some group similarities also exist.

42
Q

What typical metallic properties do nearly all transition elements display?

A

High tensile strength, ductility, malleability, high thermal and electrical conductivity, and metallic lustre.

43
Q

Which transition elements are exceptions to having typical metallic structures at normal temperatures?

A

Zinc (Zn), Cadmium (Cd), Mercury (Hg), and Manganese (Mn).

44
Q

Are transition metals generally hard or soft?

A

Transition metals (except Zn, Cd, and Hg) are very hard.

45
Q

What is the volatility of transition metals?

A

Transition metals (except Zn, Cd, and Hg) have low volatility.

46
Q

How do the melting and boiling points of transition metals compare to other metals?

A

Transition metals have high melting and boiling points.

47
Q

What series do the melting points of transition metals in Fig. 8.1 belong to?

A

The 3d, 4d, and 5d series.

48
Q

Why do transition metals have high melting points?

A

Due to the involvement of a greater number of electrons from (n-1)d in addition to the ns electrons in interatomic metallic bonding.

49
Q

In a row of transition metals, when do melting points reach a maximum?

A

At a d^5 configuration, except for anomalous values of Mn and Tc.

50
Q

How do the melting points of transition metals change as the atomic number increases?

A

They fall regularly as the atomic number increases.

51
Q

Why do transition metals have high enthalpies of atomisation?

A

Due to strong interatomic interactions, particularly when one unpaired electron per d orbital is present.

52
Q

What does the maxima in enthalpies of atomisation at the middle of each transition series indicate?

A

It indicates that one unpaired electron per d orbital is particularly favorable for strong interatomic interaction.

53
Q

How does the number of valence electrons affect bonding in transition metals?

A

Greater the number of valence electrons, stronger is the resultant bonding.

54
Q

How does the enthalpy of atomisation influence the standard electrode potential of a metal?

A

Metals with very high enthalpy of atomisation tend to be noble in their reactions.

55
Q

What property is associated with metals that have very high enthalpy of atomisation?

A

They tend to have very high boiling points and are more noble in their reactions.

56
Q

What relationship exists between boiling point and enthalpy of atomisation for transition metals?

A

A very high boiling point corresponds to very high enthalpy of atomisation.

57
Q

Why are metals with high enthalpy of atomisation considered noble in reactions?

A

Because strong interatomic interactions make them less reactive under standard conditions.

58
Q

How do the enthalpies of atomisation compare between the first, second, and third series of transition metals?

A

The metals of the second and third series have greater enthalpies of atomisation than the corresponding elements of the first series.

59
Q

What is a consequence of higher enthalpies of atomisation in second and third series transition metals?

A

It leads to more frequent metal–metal bonding in compounds of the heavy transition metals.

60
Q

Why do second and third series transition metals exhibit more metal-metal bonding in their compounds?

A

Because they have greater enthalpies of atomisation, which strengthens interatomic interactions.

61
Q

What happens to the radius of ions with the same charge in a series as atomic number increases?

A

The radius decreases progressively with increasing atomic number.

62
Q

Why does the radius of ions decrease as atomic number increases?

A

Each added electron enters a d orbital, and the d electron shielding is ineffective, increasing net attraction to the nucleus.

63
Q

What is the effect of a d electron on shielding?

A

The shielding effect of a d electron is not very effective.

64
Q

How does ineffective shielding by d electrons affect ionic radius?

A

It increases the net electrostatic attraction between the nucleus and outermost electron, causing the ionic radius to decrease.

65
Q

Is the trend of decreasing radius with increasing atomic number also observed in atomic radii?

A

Yes, the same trend is observed in the atomic radii of a given series.

66
Q

How does the variation in atomic sizes within a series compare to variations between series?

A

The variation within a series is quite small, but differences are more significant when comparing between series.

67
Q

How do atomic sizes change from the first (3d) to the second (4d) series?

A

There is an increase in atomic sizes from the first (3d) to the second (4d) series.

68
Q

How do atomic radii of the third (5d) series compare to the second (4d) series?

A

The atomic radii of the third (5d) series are virtually the same as the second (4d) series.

69
Q

What phenomenon explains the lack of size increase from the second to third series?

A

Lanthanoid contraction, caused by the filling of 4f orbitals, reduces the expected increase in size.

70
Q

Why does the filling of 4f orbitals affect atomic radii?

A

The 4f orbitals have poor shielding, leading to a stronger nuclear attraction and smaller atomic sizes.

71
Q

What is the primary cause of Lanthanoid contraction?

A

The poor shielding effect of 4f orbitals, which increases the effective nuclear charge experienced by outer electrons.

72
Q

How does Lanthanoid contraction affect periodic trends of elements?

A

It reduces the expected increase in atomic and ionic radii down the group in the periodic table.

73
Q

What is the impact of Lanthanoid contraction on chemical properties?

A

It makes the 5d series elements similar in size to the 4d series, affecting their chemistry and reducing variations across periods.

74
Q

Why do 4f orbitals have poor shielding effects?

A

The 4f orbitals are more diffused and do not effectively shield the nuclear charge from the outermost electrons.

75
Q

What is one observable consequence of Lanthanoid contraction in transition metals?

A

Transition metals in the 5d series have radii almost identical to their 4d counterparts.

76
Q

How does Lanthanoid contraction influence the separation of Lanthanides?

A

The small differences in ionic radii among Lanthanides make their chemical separation challenging.

77
Q

What is the net result of Lanthanoid contraction on the second and third d series?

A

The second (4d) and third (5d) d series exhibit similar radii (e.g., Zr 160 pm, Hf 159 pm) and have much more similar physical and chemical properties than expected based on usual family relationships.

78
Q

Why do Zr (4d) and Hf (5d) have nearly identical radii?

A

Due to Lanthanoid contraction, the poor shielding of 4f electrons reduces the size of Hf, making its radius (159 pm) almost identical to Zr (160 pm).

79
Q

How does Lanthanoid contraction affect the similarity in chemical properties between 4d and 5d elements?

A

The similar radii of 4d and 5d elements result in comparable chemical reactivity and bonding, making them behave similarly.

80
Q

Which property of d-block elements is most influenced by Lanthanoid contraction?

A

Atomic and ionic radii are most influenced, leading to similarities between elements in the 4d and 5d series.

81
Q

What is one industrial implication of Lanthanoid contraction?

A

The similarity in radii and properties of 4d and 5d elements, such as Zr and Hf, makes their separation during extraction processes challenging.

82
Q

How does Lanthanoid contraction affect the trend in ionization energies?

A

The increase in effective nuclear charge due to poor shielding by 4f electrons leads to higher ionization energies for Lanthanides and their subsequent elements.

83
Q

How does Lanthanoid contraction influence hardness and melting points?

A

Smaller atomic radii result in stronger metallic bonding, increasing hardness and melting points.

84
Q

What is the primary factor responsible for Lanthanoid contraction?

A

The imperfect shielding of one 4f electron by another within the same orbital set.

85
Q

How does the shielding effect of 4f electrons compare to that of d electrons?

A

The shielding of 4f electrons is less effective than the shielding of d electrons.

86
Q

What happens to the size of the 4f orbitals as nuclear charge increases?

A

The size of the 4f orbitals decreases fairly regularly as the nuclear charge increases along the series.

87
Q

How is Lanthanoid contraction similar to trends in ordinary transition series?

A

Both are caused by imperfect shielding of electrons within the same orbital set, leading to a decrease in atomic and ionic size with increasing nuclear charge.

88
Q

How does the decrease in metallic radius and increase in atomic mass affect the density of elements?

A

The decrease in metallic radius and increase in atomic mass results in a general increase in the density of these elements.

89
Q

How does the density change from titanium (Z = 22) to copper (Z = 29)?

A

There is a significant increase in the density from titanium (Z = 22) to copper (Z = 29).

90
Q

What causes the density increase in transition metals from titanium to copper?

A

The decrease in metallic radius and the increase in atomic mass contribute to the overall increase in density.

91
Q

Why do the transition elements exhibit higher enthalpies of
atomisation?
[intext]

A

Because of large number of unpaired electrons in their atoms they
have stronger interatomic interaction and hence stronger bonding
between atoms resulting in higher enthalpies of atomisation.

92
Q

In the series Sc (Z = 21) to Zn (Z = 30), the enthalpy of atomisation
of zinc is the lowest, i.e., 126 kJ mol–1. Why?
[Intext]

A

In the formation of metallic bonds, no eletrons from 3d-orbitals are involved
in case of zinc, while in all other metals of the 3d series, electrons from
the d-orbitals are always involved in the formation of metallic bonds

Chemistry (10 decks)

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