The F- And D- Block Elements - Introduction To Enthalpy Of Atomization Of D & F Elements

The f- and d- block elements - Introduction to Enthalpy of Atomization of d & f elements

Slide 1

The f-block and d-block elements are also known as transition elements.
They are located in the middle of the periodic table.
The transition elements have partially filled d or f orbitals.
These elements show a variety of chemical properties due to their partially filled orbitals.

Slide 2

Enthalpy of atomization is the enthalpy change that occurs when one mole of a substance in the gaseous state is formed from its atoms in the gaseous state.
The enthalpy of atomization for d and f block elements is significant due to the involvement of the partially filled d or f orbitals.

Slide 3

Enthalpy of atomization is a measure of the strength of the metallic bond.
The stronger the metallic bond, the higher the enthalpy of atomization.
In the case of d and f block elements, the presence of partially filled orbitals strengthens the metallic bond.

Slide 4

The enthalpy of atomization for d-block elements is generally high.
This is because the d orbitals are closer to the nucleus and experience a higher effective nuclear charge.
As a result, the d electrons are strongly held by the nucleus, leading to a higher enthalpy of atomization.

Slide 5

The f-block elements, also known as the lanthanides and actinides, have the highest enthalpy of atomization.
This is due to the presence of f orbitals, which are even closer to the nucleus and experience an even higher effective nuclear charge.

Slide 6

The lanthanides are called inner transition elements because their f orbitals are located inside the d orbitals.
The actinides are also inner transition elements but have f orbitals located below the d orbitals.

Slide 7

The enthalpy of atomization for f-block elements is affected by the shielding effect.
The f orbitals provide poor shielding due to their shape, which results in a higher effective nuclear charge experienced by the outermost electrons.
Therefore, the enthalpy of atomization for f-block elements is higher compared to d-block elements.

Slide 8

The d block elements show periodic trends in their enthalpy of atomization.
Generally, the enthalpy of atomization increases across a period and decreases down a group.
This trend can be attributed to changes in effective nuclear charge and atomic size.

Slide 9

The enthalpy of atomization can be affected by the electronic configuration of the transition element.
Elements with half-filled or completely filled orbitals tend to have higher enthalpies of atomization due to increased stability.

Slide 10

In conclusion, the enthalpy of atomization for d and f block elements is higher compared to other elements due to the involvement of partially filled d or f orbitals.
This leads to stronger metallic bonds and higher effective nuclear charges, resulting in higher enthalpy values.

Slide 11

The enthalpy of atomization is an important concept in understanding the properties of d and f block elements.
It helps explain their high melting and boiling points, as well as their ability to form stable complexes.
The enthalpy of atomization is also useful in predicting the reactivity of these elements.

Slide 12

The enthalpy of atomization can be calculated using Hess’s Law.
It involves breaking the element into individual atoms and then calculating the energy required for this process.
The enthalpy of atomization is equal to the sum of the enthalpy changes for each step in the process.

Slide 13

The enthalpy of atomization can be determined experimentally using calorimetry.
This involves measuring the heat released or absorbed during the atomization process.
The enthalpy change can then be calculated using the equation q = mcΔT.

Slide 14

The enthalpy of atomization is affected by various factors such as atomic size, electron configuration, and bond strength.
Atomic size plays a role in determining the distance between the nucleus and the outermost electrons, which affects the strength of the metallic bond.

Slide 15

The electron configuration of d and f block elements also influences the enthalpy of atomization.
Elements with more stable electron configurations, such as half-filled or fully filled orbitals, have higher enthalpy values.
This is due to the increased stability and stronger metallic bonds.

Slide 16

The bond strength in d and f block elements is determined by factors such as effective nuclear charge and electron-electron repulsion.
The higher the effective nuclear charge, the stronger the bond and the higher the enthalpy of atomization.
Electron-electron repulsion also affects the bond strength, with less repulsion leading to stronger bonds.

Slide 17

The enthalpy of atomization can be used to explain the reactivity of d and f block elements.
Elements with higher enthalpy values are generally less reactive because it requires more energy to break their metallic bonds.
This is why many d and f block elements are known for their stability and resistance to corrosion.

Slide 18

The enthalpy of atomization is also important in understanding the formation of complexes.
Transition elements have a high enthalpy of atomization, allowing them to form stable coordination complexes with ligands.
The enthalpy change during complex formation can be calculated using the enthalpy of atomization.

Slide 19

The enthalpy of atomization plays a role in the industrial processes involving d and f block elements.
For example, the enthalpy of atomization is important in the production of metals through the reduction of their oxides.
It is also useful in the design of catalysts for chemical reactions.

Slide 20

In summary, the enthalpy of atomization is a measure of the strength of the metallic bond in d and f block elements.
It is affected by factors such as atomic size, electron configuration, and bond strength.
The enthalpy of atomization helps explain the properties and reactivity of these elements, as well as their ability to form stable complexes.

Slide 21

Atomic Size: The distance between the nucleus and the outermost electrons affects the strength of metallic bonds. Smaller atomic size leads to stronger bonds.
Electron Configuration: Half-filled or completely filled orbitals provide increased stability and result in higher enthalpy values.
Bond Strength: Factors such as effective nuclear charge and electron-electron repulsion influence the bond strength and, consequently, the enthalpy of atomization.
Reactivity: Elements with higher enthalpy values are generally less reactive due to the energy required to break their metallic bonds.
Complex Formation: The high enthalpy of atomization allows d and f block elements to form stable coordination complexes with ligands.

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Slide 22

Industrial Applications: The enthalpy of atomization is important in processes such as the reduction of metal oxides to produce metals and in the design of catalysts for chemical reactions.
Stability: D and f block elements are known for their stability and resistance to corrosion, partly due to their high enthalpy values.
Heat of Atomization Calculation: Hess’s Law can be used to calculate the enthalpy of atomization by breaking the element into individual atoms and calculating the energy required.
Calorimetry: Experimental methods, such as calorimetry, can be used to determine the enthalpy change during the atomization process.
Enthalpy Change Equation: The equation q = mcΔT can be used to calculate the enthalpy change, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

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Slide 23

Electron Configurations of D Block Elements: The electron configurations of d block elements can be written using the (n-1)d electron configuration.
Electron Configurations of F Block Elements: The electron configurations of f block elements can be written using the (n-2)f14(n-1)d electron configuration.
Lanthanides and Actinides: The lanthanides and actinides are inner transition elements with f orbitals located inside or below the d orbitals, respectively.
Shielding Effect: The shape of f orbitals provides poor shielding, resulting in higher effective nuclear charge and higher enthalpy of atomization.
Periodic Trends: The enthalpy of atomization generally increases across a period and decreases down a group in the periodic table.

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Slide 24

Example: Iron (Fe) has an electron configuration of [Ar] 4s2 3d6.
Example: Cerium (Ce) has an electron configuration of [Xe] 6s2 4f1 5d1.
Example: Neodymium (Nd) has an electron configuration of [Xe] 6s2 4f4.
Example: Uranium (U) has an electron configuration of [Rn] 7s2 5f3 6d1.
Example: Platinum (Pt) has an electron configuration of [Xe] 6s1 4f14 5d9.

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Slide 25

Example: Chromium (Cr) has an enthalpy of atomization of 449 kJ/mol due to its stable half-filled 3d orbital with electron configuration [Ar] 3d5 4s1.
Example: Silver (Ag) has an enthalpy of atomization of 280 kJ/mol because of its stable completely filled 4d orbital with electron configuration [Kr] 4d10 5s1.
Example: Mercury (Hg) has an enthalpy of atomization of 60.9 kJ/mol due to its unstable partially filled 5d orbital with electron configuration [Xe] 6s2 5d10.
Example: Gadolinium (Gd) has an enthalpy of atomization of 420 kJ/mol because of its stable half-filled 4f orbital with electron configuration [Xe] 6s2 4f7 5d1.
Example: Curium (Cm) has an enthalpy of atomization of 425 kJ/mol due to its stable half-filled 5f orbital with electron configuration [Rn] 7s2 5f7 6d1.

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Slide 26

Example: The enthalpy of atomization of copper (Cu) is 337 kJ/mol because of its high effective nuclear charge and strong metallic bonds.
Example: The enthalpy of atomization of zinc (Zn) is 118 kJ/mol due to its stable completely filled 3d orbital and strong metallic bonds.
Example: The enthalpy of atomization of gold (Au) is 334 kJ/mol because of its high effective nuclear charge and strong metallic bonds.
Example: The enthalpy of atomization of nickel (Ni) is 428 kJ/mol due to its high effective nuclear charge and strong metallic bonds.
Example: The enthalpy of atomization of tin (Sn) is 305 kJ/mol because of its high effective nuclear charge and strong metallic bonds.

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Slide 27

Example: The high enthalpy of atomization of d and f block elements leads to their high melting and boiling points.
Example: The enthalpy of atomization of d block elements contributes to their ability to form stable complexes with ligands.
Example: The enthalpy of atomization of transition metals is crucial in the production of metals through the reduction of their oxides.
Example: The enthalpy of atomization of d block elements is important in the design of catalysts for chemical reactions.
Example: The high enthalpy values of f block elements play a role in their stability and resistance to corrosion.

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Slide 28

Example: Iron (Fe) has a high enthalpy of atomization, which contributes to its stability and resistance to corrosion.
Example: Lanthanum (La) has a high enthalpy of atomization, making it useful in the production of high-quality steel.
Example: Uranium (U) has a high enthalpy of atomization, which allows it to be used as a fuel in nuclear reactors.
Example: Platinum (Pt) has a high enthalpy of atomization, making it valuable in catalytic converters.
Example: Gadolinium (Gd) has a high enthalpy of atomization, making it useful in magnetic resonance imaging (MRI) contrast agents.

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Slide 29

Example: The enthalpy change during the atomization of iron can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Example: The enthalpy of atomization of copper can be determined experimentally using calorimetry by measuring the heat released or absorbed during the process.
Example: The enthalpy change during the atomization of silver can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Example: The enthalpy of atomization of gold can be determined experimentally using calorimetry by measuring the heat released or absorbed during the process.
Example: The enthalpy change during the atomization of nickel can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

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Slide 30

Example: The enthalpy change during the atomization of tin can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Example: The enthalpy of atomization of cerium can be determined experimentally using calorimetry by measuring the heat released or absorbed during the process.
Example: The enthalpy change during the atomization of neodymium can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Example: The enthalpy of atomization of uranium can be determined experimentally using calorimetry by measuring the heat released or absorbed during the process.
Example: The enthalpy change during the atomization of platinum can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.