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Questions and Answers
What is the electronic configuration of Chromium?
What is the electronic configuration of Chromium?
- [Ar]3d⁵4s¹ (correct)
- [Ar]3d⁶4s²
- [Ar]3d¹⁰4s¹
- [Ar]3d⁴4s²
Why is Copper not considered to have the same electronic configuration as other d-block elements?
Why is Copper not considered to have the same electronic configuration as other d-block elements?
- It has a configuration of [Ar]3d⁹4s².
- It does not exhibit oxidation states.
- It has a configuration of [Ar]3d¹⁰4s¹. (correct)
- It has a completely filled 4s orbital.
Which statement accurately describes why Zn is not classified as a transition metal?
Which statement accurately describes why Zn is not classified as a transition metal?
- It does not exhibit variable oxidation states.
- It has completely filled d-orbitals in its oxidation states. (correct)
- It belongs to the f-block elements.
- It has partially filled d-orbitals.
What characteristic do Ag and Au share that qualifies them as transition metals?
What characteristic do Ag and Au share that qualifies them as transition metals?
On what ground is Scandium classified as a transition element?
On what ground is Scandium classified as a transition element?
Which of the following is true regarding the exceptional electronic configurations of d-block elements?
Which of the following is true regarding the exceptional electronic configurations of d-block elements?
What property allows transition metals to exhibit a range of oxidation states?
What property allows transition metals to exhibit a range of oxidation states?
Which of the following elements is NOT considered a transition metal?
Which of the following elements is NOT considered a transition metal?
What causes the color of transition metal ions?
What causes the color of transition metal ions?
Why are Cu(I) salts colorless?
Why are Cu(I) salts colorless?
Which ion is colored among Sc3+, Zn2+, and Cr3+?
Which ion is colored among Sc3+, Zn2+, and Cr3+?
What makes transition metals effective catalysts?
What makes transition metals effective catalysts?
Why are zinc salts colorless?
Why are zinc salts colorless?
Which feature primarily contributes to the formation of complex compounds by transition metals?
Which feature primarily contributes to the formation of complex compounds by transition metals?
What characteristic of Cu(II) salts contributes to their color?
What characteristic of Cu(II) salts contributes to their color?
Which of the following statements about transition metals is correct?
Which of the following statements about transition metals is correct?
Why is Cu+ considered diamagnetic?
Why is Cu+ considered diamagnetic?
Why does Vanadium have a relatively low E°(M³⁺ / M²⁺) value?
Why does Vanadium have a relatively low E°(M³⁺ / M²⁺) value?
What is the magnetic moment of Sc3+?
What is the magnetic moment of Sc3+?
Which statement is true regarding Cu2+?
Which statement is true regarding Cu2+?
What accounts for the high stability of Mn²⁺ compared to other ions?
What accounts for the high stability of Mn²⁺ compared to other ions?
Using the formula, what is n for Mn2+?
Using the formula, what is n for Mn2+?
How can the stability of cations be related to their standard electrode potential?
How can the stability of cations be related to their standard electrode potential?
Which factor contributes to the increasing oxidizing power in VO₂⁺ < Cr₂O₇²⁻ < MnO₄⁻?
Which factor contributes to the increasing oxidizing power in VO₂⁺ < Cr₂O₇²⁻ < MnO₄⁻?
What is the calculation for the number of unpaired electrons in Ti3+?
What is the calculation for the number of unpaired electrons in Ti3+?
Why is Cr²⁺ considered a strong reducing agent?
Why is Cr²⁺ considered a strong reducing agent?
If n > 5, how do you calculate the number of unpaired electrons?
If n > 5, how do you calculate the number of unpaired electrons?
What makes copper (I) compounds unstable in aqueous solutions?
What makes copper (I) compounds unstable in aqueous solutions?
What is the magnetic moment of a divalent ion with atomic number 25?
What is the magnetic moment of a divalent ion with atomic number 25?
Why are Sc3+ salts considered diamagnetic?
Why are Sc3+ salts considered diamagnetic?
Which of the following elements are considered diamagnetic?
Which of the following elements are considered diamagnetic?
What is the cause of paramagnetism in transition metals?
What is the cause of paramagnetism in transition metals?
Which of the following correctly describes d-block elements?
Which of the following correctly describes d-block elements?
What characteristic defines transition elements?
What characteristic defines transition elements?
Where are d-block elements located in the periodic table?
Where are d-block elements located in the periodic table?
Which group numbers do d-block elements occupy?
Which group numbers do d-block elements occupy?
What is the general electronic configuration for d-block elements?
What is the general electronic configuration for d-block elements?
How many series of d-block elements are known?
How many series of d-block elements are known?
What is the valence shell electronic configuration of the 3d series of elements?
What is the valence shell electronic configuration of the 3d series of elements?
Which series belongs to the second transition series?
Which series belongs to the second transition series?
What is the primary reason for the maximum melting and boiling points of transition metals found at the middle of each series?
What is the primary reason for the maximum melting and boiling points of transition metals found at the middle of each series?
Which element has the lowest melting point among the transition metals?
Which element has the lowest melting point among the transition metals?
Why do Mn, Tc, and Re have lower melting points despite having more unpaired electrons?
Why do Mn, Tc, and Re have lower melting points despite having more unpaired electrons?
Regarding the enthalpy of atomization, which statement is correct?
Regarding the enthalpy of atomization, which statement is correct?
What trend is observed in atomic radius across a transition series?
What trend is observed in atomic radius across a transition series?
How do ionization enthalpies change across a transition series?
How do ionization enthalpies change across a transition series?
Which of the following pairs correctly identifies the relationship between atomic and ionic radii in transition metals?
Which of the following pairs correctly identifies the relationship between atomic and ionic radii in transition metals?
What explains the increase of density in transition metals along a period?
What explains the increase of density in transition metals along a period?
What is the reason for the higher second ionization enthalpy of copper compared to zinc?
What is the reason for the higher second ionization enthalpy of copper compared to zinc?
During which process does manganese form a half-filled d configuration?
During which process does manganese form a half-filled d configuration?
Which of the following elements shows the maximum oxidation state of +7 in the 3d series?
Which of the following elements shows the maximum oxidation state of +7 in the 3d series?
Which statement best describes the variable oxidation states of transition metals?
Which statement best describes the variable oxidation states of transition metals?
How does the second ionization enthalpy of manganese compare to that of iron?
How does the second ionization enthalpy of manganese compare to that of iron?
What happens to the oxidation state of transition elements as the atomic number increases up to manganese in the 3d series?
What happens to the oxidation state of transition elements as the atomic number increases up to manganese in the 3d series?
What configuration does copper achieve after the first ionization?
What configuration does copper achieve after the first ionization?
Which two elements have a third ionization enthalpy that is considered very high?
Which two elements have a third ionization enthalpy that is considered very high?
Which element in the 3d series exhibits the highest oxidation state?
Which element in the 3d series exhibits the highest oxidation state?
What is the reason that +2 oxidation state is the most common for 3d series transition metals?
What is the reason that +2 oxidation state is the most common for 3d series transition metals?
Which of the following is known to be a stronger reducing agent?
Which of the following is known to be a stronger reducing agent?
Which compound is expected to show more covalent character?
Which compound is expected to show more covalent character?
In which oxidation state is chromium more acidic, CrO or CrO₃?
In which oxidation state is chromium more acidic, CrO or CrO₃?
Which transition element does not exhibit variable oxidation states?
Which transition element does not exhibit variable oxidation states?
What is the significance of the E°(M²⁺/M) value for copper being positive?
What is the significance of the E°(M²⁺/M) value for copper being positive?
Which 3d series transition metal has the largest number of oxidation states?
Which 3d series transition metal has the largest number of oxidation states?
What is the nature of oxides formed by all transition metals except scandium?
What is the nature of oxides formed by all transition metals except scandium?
Which of the following oxides is classified as amphoteric?
Which of the following oxides is classified as amphoteric?
What is the primary ore from which potassium dichromate is manufactured?
What is the primary ore from which potassium dichromate is manufactured?
What does the reaction of V2O5 with acids produce?
What does the reaction of V2O5 with acids produce?
Which of these is NOT a use of potassium dichromate?
Which of these is NOT a use of potassium dichromate?
Which of the following statements about amphoteric oxides is true?
Which of the following statements about amphoteric oxides is true?
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Study Notes
Electronic Configuration of 3d Series Elements
- Scandium (Sc): Atomic number 21, electronic configuration [Ar]3d¹4s².
- Titanium (Ti): Atomic number 22, electronic configuration [Ar]3d²4s².
- Vanadium (V): Atomic number 23, electronic configuration [Ar]3d³4s².
- Chromium (Cr): Atomic number 24, unique configuration [Ar]3d⁵4s¹ due to stability of half-filled orbitals.
- Manganese (Mn): Atomic number 25, electronic configuration [Ar]3d⁵4s².
- Iron (Fe): Atomic number 26, electronic configuration [Ar]3d⁶4s².
- Cobalt (Co): Atomic number 27, electronic configuration [Ar]3d⁷4s².
- Nickel (Ni): Atomic number 28, electronic configuration [Ar]3d⁸4s².
- Copper (Cu): Atomic number 29, unique configuration [Ar]3d¹⁰4s¹ due to stability of fully filled orbitals.
- Zinc (Zn): Atomic number 30, electronic configuration [Ar]3d¹⁰4s².
Exceptional Electronic Configurations
- Some d-block elements show exceptions due to the energy difference between ns and (n-1)d orbitals.
- Half-filled (d⁵) and completely filled (d¹⁰) configurations provide extra stability.
- Cu and Cr have unique configurations to exploit this stability.
Transition Elements
- Zn, Cd, and Hg are not transition elements because they have completely filled d-orbitals in their common oxidation states.
- Cu, Ag, and Au are considered transition elements since they possess partially filled d-orbitals in oxidation states.
- Scandium (Sc) is a transition element due to partially filled d-orbitals, while Zn is not, as it has a completely filled d-orbital.
Magnetic Properties
- Transition metals are often paramagnetic, possessing unpaired electrons in d-orbitals.
- Diamagnetic substances lack unpaired electrons and are not attracted to magnets.
- Magnetic moment can be calculated using the formula (μ = \sqrt{n(n+2)}) where (n) is the number of unpaired electrons.
Coloration of Transition Metal Ions
- Color arises from unpaired d-electrons undergoing d-d transitions, absorbing visible light.
- Cu²⁺ ions absorb red and emit blue, showcasing complementary colors.
- Zn²⁺ salts are colorless due to lacking unpaired electrons.
Catalytic Properties
- Transition metals and their compounds act as catalysts due to multiple oxidation states, large surface area, and the presence of unpaired d-orbitals.
- Example: Vanadium pentoxide is used as a catalyst in the manufacturing of sulfuric acid.
Oxidation States of Transition Elements
- Variable oxidation states result from the loss of inner (n-1)d and outer ns electrons.
- Manganese exhibits the highest oxidation state (+7), while zinc typically shows +2.
- The stability of oxidation states can be explained through standard electrode potentials.
Characteristics of Transition Metal Compounds
- Transition metals form a variety of complex compounds due to their small ionic size and high polarizing power.
- The presence of vacant d-orbitals allows for effective bond formation.
Properties Trends Among Transition Metals
- Melting and boiling points are generally highest in the middle of transition series due to optimal metallic bonding from unpaired electrons.
- Ionization enthalpies generally increase across the period, influenced by effective nuclear charge and electron configurations.
- Atomic and ionic radii decrease with increasing atomic number, although patterns may vary slightly among specific elements.
Summary of Oxides and Oxoanions
- Transition metals mainly form ionic and basic oxides, while higher oxidation states exhibit covalent and acidic properties.
- Certain oxides show amphoteric characteristics and can react both as acids and bases.
Notable Transition Element Compounds
- Potassium dichromate (K₂Cr₂O₇) is used widely, especially in the leather industry, and is obtained from chromite ore.
General Observations
- Transition metals generally display a wide range of oxidation states and complex formation abilities, maintaining unique properties that differentiate them from main group elements.
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