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Questions and Answers
What distinguishes d-block elements from other elements?
What distinguishes d-block elements from other elements?
- The last electron enters the p-orbitals of the penultimate shell.
- The last electron enters the d-orbitals of the penultimate shell. (correct)
- The last electron enters the s-orbitals of the outermost shell.
- They always have completely filled d-orbitals.
Which statement accurately describes a transition element?
Which statement accurately describes a transition element?
- An element with a completely filled d-orbital in its ground state.
- An element with a partially filled p-orbital in its ground state.
- An element that only exhibits one oxidation state.
- An element with a partially filled d-orbital in its ground state or most stable oxidation state. (correct)
Where are d-block elements located in the periodic table?
Where are d-block elements located in the periodic table?
- At the bottom, separate from the main body of the table.
- In the middle, between the s-block and p-block elements. (correct)
- On the far right side of the periodic table.
- Between the alkali metals and alkaline earth metals.
What is the general electronic configuration of d-block elements?
What is the general electronic configuration of d-block elements?
Which subshell is filled first, 'ns' or '(n-1)d', and why?
Which subshell is filled first, 'ns' or '(n-1)d', and why?
Which of the following series represents the 3d transition series?
Which of the following series represents the 3d transition series?
The second transition series consists of how many elements?
The second transition series consists of how many elements?
Which elements have a single electron in the 4s-orbital, differing from the expected electron configuration?
Which elements have a single electron in the 4s-orbital, differing from the expected electron configuration?
Why do Cr and Cu have a single electron in their 4s orbitals?
Why do Cr and Cu have a single electron in their 4s orbitals?
Which electronic configuration represents the chromium atom?
Which electronic configuration represents the chromium atom?
How does atomic radii generally behave across a period in the d-block elements?
How does atomic radii generally behave across a period in the d-block elements?
What factor contributes to the near similarity in atomic radii of second and third transition series elements?
What factor contributes to the near similarity in atomic radii of second and third transition series elements?
How do ionic radii generally compare to atomic radii for transition metals?
How do ionic radii generally compare to atomic radii for transition metals?
Which property contributes to the metallic behavior of transition elements?
Which property contributes to the metallic behavior of transition elements?
What factor most directly influences the melting points of transition metals?
What factor most directly influences the melting points of transition metals?
Which element has the highest melting point?
Which element has the highest melting point?
How do first ionization enthalpies generally change across a transition series?
How do first ionization enthalpies generally change across a transition series?
Why are the first ionization enthalpies of Zn, Cd, and Hg high?
Why are the first ionization enthalpies of Zn, Cd, and Hg high?
What is the primary reason for transition elements exhibiting variable oxidation states?
What is the primary reason for transition elements exhibiting variable oxidation states?
What explains the relative stabilities of different oxidation states in transition elements?
What explains the relative stabilities of different oxidation states in transition elements?
Which statement is correct regarding metallic character and oxidation state in d-block element compounds?
Which statement is correct regarding metallic character and oxidation state in d-block element compounds?
What is the relationship between ionization enthalpy and the stability of a compound formed by a transition metal?
What is the relationship between ionization enthalpy and the stability of a compound formed by a transition metal?
What accounts for the variations in the M2+/M standard electrode potentials among transition metals?
What accounts for the variations in the M2+/M standard electrode potentials among transition metals?
What unique property does copper exhibit in its standard electrode potential series?
What unique property does copper exhibit in its standard electrode potential series?
Why is there a growing trend towards less negative E° values along the series in the M2+/M Standard Electrode Potentials?
Why is there a growing trend towards less negative E° values along the series in the M2+/M Standard Electrode Potentials?
Which of the following dictates catalytic properties in transition elements?
Which of the following dictates catalytic properties in transition elements?
What is the role of surface area in the catalytic activity of transition elements?
What is the role of surface area in the catalytic activity of transition elements?
What is the relationship between unpaired electrons and magnetism?
What is the relationship between unpaired electrons and magnetism?
Which formula is used to calculate magnetic moment in transition element series is the orbital angular magnetic moment is insignificant?
Which formula is used to calculate magnetic moment in transition element series is the orbital angular magnetic moment is insignificant?
What is the nature of the magnetic property of interstitial compounds?
What is the nature of the magnetic property of interstitial compounds?
How much is the atomic radii different to form alloys?
How much is the atomic radii different to form alloys?
What is the relationship between oxidation state and acidity?
What is the relationship between oxidation state and acidity?
Which of the following equations is correct for the conversion of sodium chromate into sodium dichromate?
Which of the following equations is correct for the conversion of sodium chromate into sodium dichromate?
What happens when an alkali is added to an orange red solution of dichromate?
What happens when an alkali is added to an orange red solution of dichromate?
Potassium dichromate acts as a powerful oxidising agent with dil. sulphuric acid, what molecules are furnished?
Potassium dichromate acts as a powerful oxidising agent with dil. sulphuric acid, what molecules are furnished?
What is used to test whether a driver has consumed alcohol or not?
What is used to test whether a driver has consumed alcohol or not?
Large scale, potassium permanganate is prepared from the mineral pyrolusite.
Large scale, potassium permanganate is prepared from the mineral pyrolusite.
In strongly alkaline solution, what ion is produced?
In strongly alkaline solution, what ion is produced?
What term is referred to for Alkaline KMnO used for ?
What term is referred to for Alkaline KMnO used for ?
In first transition elements series the orbital contribution is quenched by the:
In first transition elements series the orbital contribution is quenched by the:
Flashcards
What are d-block elements?
What are d-block elements?
Elements where the last differentiating electron enters the (n-1) d orbitals.
What is (n-1) d1-10, ns0-2?
What is (n-1) d1-10, ns0-2?
The general electronic configuration of d-block elements.
Where do d-block items lie?
Where do d-block items lie?
Elements located in the middle of the periodic table.
What is the 1st Transition series?
What is the 1st Transition series?
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Why Cr and Cu exceptions?
Why Cr and Cu exceptions?
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What is Oxidation State?
What is Oxidation State?
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Variable oxidation states?
Variable oxidation states?
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Oxidation state calculation
Oxidation state calculation
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How Oxidation States vary?
How Oxidation States vary?
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Bonding Change?
Bonding Change?
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Important electron Configuration?
Important electron Configuration?
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Chemical reactivity
Chemical reactivity
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What affects Electrode size?
What affects Electrode size?
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Standard Electrode Potentials (Eº) and chemical reactivity.
Standard Electrode Potentials (Eº) and chemical reactivity.
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Transition metal Oxides?
Transition metal Oxides?
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Oxides properties?
Oxides properties?
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Property of Transition metal
Property of Transition metal
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Key Properties?
Key Properties?
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Define Interstitial Compounds.
Define Interstitial Compounds.
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What is Alloy formation about?
What is Alloy formation about?
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What does Magnetic Behavior help with ?
What does Magnetic Behavior help with ?
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what are Complex compounds?
what are Complex compounds?
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Thermodynamic Stability?
Thermodynamic Stability?
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What are uses of MnO4?
What are uses of MnO4?
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Oxidation of metals:
Oxidation of metals:
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State and why ?
State and why ?
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Electronic configuration is important in?
Electronic configuration is important in?
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What does the Contraction Lead too
What does the Contraction Lead too
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Atomic Numbers?
Atomic Numbers?
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Series of Oxidation States
Series of Oxidation States
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What occurs or is there an effect in Actinides atoms.
What occurs or is there an effect in Actinides atoms.
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Study Notes
d & f Block Elements
- Elements where the last differentiating electron enters the d-orbitals of the penultimate shell ((n-1)d) are d-block elements
- A transition element can be defined as an element with partially filled d-orbitals in its ground state or most stable oxidation state
- Copper(I) has a configuration of 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹ and Copper(II) is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹
Properties of d-Block Elements
- These elements show properties intermediate between s-block and p-block elements
- They exhibit a transition in properties from electropositive (s-block) to less electropositive (p-block) elements, hence called transition elements
Position in the Periodic Table
- d-block elements are located between the s-block and p-block elements in the middle of the periodic table
Electronic Configuration
- As atomic number increases in d-block elements, the d-orbitals of the penultimate shell ((n-1)d) get gradually filled
- The general electronic configuration of d-block elements is (n-1)d¹⁻¹⁰ ns⁰⁻²
- Four series exist based on which d-orbitals are filled: 3d, 4d, 5d, and 6d subshells, each with ten elements
- The (n-1)d subshell energy is slightly greater than the ns subshell, so the ns orbital fills first
The d series can be shown as follows
- First (3d) Transition Series (Sc–Zn)
- Second (4d) Transition Series (Y-Cd)
- Third (5d) Transition Series (La–Hg)
- Fourth (6d) Transition Series
Exceptional Electronic Configurations
- Chromium (Z=24) and copper (Z=29) configurations are exceptions
- Chromium and copper have a single electron in the 4s-orbital, unlike other elements
- Additional stability is gained by having either half-filled (5 electrons) or completely filled (10 electrons) d-sublevels
- Chromium achieves a 3d⁵ 4s¹ configuration, while copper attains a 3d¹⁰ 4s¹ configuration
- This relies on exchange energy
Atomic Radii Trends
- Transition metals have atomic radii in-between those of s- and p-block elements
- Generally, the atomic radii of d-block elements in a series decrease with increasing atomic number, but the decrease is small after midway
- Atomic radius decreases as the nuclear charge increases and d-electron shielding is small
- After midway, added d-electrons screen the outermost electrons, increasing the screening effect
- This effect counterbalances the increased nuclear charge, and atomic radii remain practically the same after chromium
- At the end of a period, a slight increase in atomic radii occurs
Explanations for Atomic Radii
- Near the series end, increased electron-electron repulsions in the orbitals overcome attractive forces, expanding the electron cloud
- Atomic radii increase down the group, with second series elements larger than the first
- Lanthanide contraction causes the second and third transition series atomic radii to be nearly identical
Ionic Radii Details
- Ionic radii follow the same trends as atomic radii
- Transition metals exhibit different ionic radii in different oxidation states
- Transition metal ionic radii are smaller than representative element radii of the same period
Metallic Properties of Transition Elements
- Except for liquid mercury, all transition elements exhibit typical metallic structures
- Transition elements are ductile and have high melting points, boiling points, thermal/electrical conductivity, and tensile strength
- Transition elements have relatively low ionization energies and form metallic bonds due to having one or two electrons in the outermost ns¹ or ns² energy level
- The stronger the metallic bonding, the greater the number of unpaired d electrons due to overlapping of unpaired electrons between metal atoms
Melting Point Facts
- Transition metals generally have high melting points due to the presence of unpaired e-
- Melting points increase and reach a maximum at Cr. Fe and higher series reach max after Cr.
- Melting points decrease W has the highest melting point
- Hg has the lowest melting point
- In the 3d series Mn has the lowest melting point
Ionization Enthalpy Information
- First ionization enthalpies of d-block elements lie between s-block and p-block elements
- D-block elements are higher than s-block elements and are lesser than those of p-block elements
- Ionization enthalpy generally increases along a series, though some irregularities
- Increasing ionization enthalpies result from increased nuclear charge, contracting the atom and complicating electron removal
- Differences in ionization enthalpies between consecutive d-block elements of same series are very much less than those of consecutive s-block or p-block elements
Explanations of Ionization Enthalpies
- Added d electrons in the (n-1) or penultimate shell provide a screening effect, shielding outer s electrons from nuclear attraction
- Opposing effects arise from rising nuclear charge and added d electrons
- Fully-filled configurations result in very high ionization enthalpies for Zn, Cd, and Hg due to the valence (n-1) d¹⁰ ns²
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Description
Explanation of d & f block elements, their position in the periodic table, and electronic configuration. Transition elements have partially filled d-orbitals. These elements show properties intermediate between s-block and p-block elements.
