Questions and Answers
What represents the d-block elements in the periodic table?
Which of the following elements is classified as a transition metal?
What are the two series of inner transition metals called?
Which oxidation state is commonly stable among transition metals?
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Which of the following compounds contains chromium and is often used in laboratories?
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What type of energy sources do the inner transition elements, Th, Pa, and U, represent?
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Which orbital is progressively filled in the f-block elements?
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What is the significance of electrode potential values in d- and f-block elements?
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What is the enthalpy of atomisation for zinc?
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Which statement is true regarding the ionisation enthalpy of transition elements?
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Why do 3d electrons effectively shield 4s electrons from increasing nuclear charge?
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What is the trend in atomic radii as we move from Scandium to Zinc?
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What is a notable characteristic of the first ionisation enthalpy of the 3d series metals?
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What is the primary reason for the irregular trend in first ionisation enthalpy among 3d series metals?
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Which transition element has the highest first ionisation enthalpy in the 3d series?
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What is true about the ionisation enthalpies of the first three elements in the transition series?
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What is formed when manganese (II) ions are oxidised by peroxodisulphate?
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Which of the following statements about potassium permanganate is true?
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Why is the manganate ion considered paramagnetic?
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Which of the following is a property of permanganate ion?
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What does acidified permanganate solution oxidise iron(II) ions to?
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What happens to starch when it reacts with permanganate in an acidified solution?
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How are manganate and permanganate ions geometrically characterized?
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Which of the following reactions involves permanganate as an oxidizing agent?
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Which transition metal has the highest third ionisation enthalpy based on the content?
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What does the term 'dominant term' refer to in the context of ionisation enthalpies?
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Which oxidation state is identified as the lowest common oxidation state for transition metals mentioned?
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Why does Zinc (Zn) have a correspondingly low ionisation enthalpy?
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Which transition metals have third ionisation enthalpies indicating difficulty obtaining higher oxidation states?
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What characteristic do nearly all transition elements exhibit?
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What does the trend in third ionisation enthalpies reflect?
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What complexity affects the prediction of oxidation states from ionisation enthalpies?
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Which of the following elements does not exhibit typical metallic structures at normal temperatures?
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What is a notable feature of transition metals regarding oxidation states?
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Which lattice structures are observed for Chromium (Cr)?
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What is the typical characteristic of transition metals in terms of conductivity?
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Which of the following transition metals displays a hexagonal close packed (hcp) structure?
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Which of the following elements has a body-centered cubic (bcc) structure among the listed?
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Which transition element is known to be an exception in exhibiting typical metallic properties?
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What does 'ccp' stand for in the context of lattice structures?
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Study Notes
Overview of d- and f-Block Elements
- d-block elements (transition metals) are located in groups 3-12 of the periodic table.
- f-block elements (inner transition metals) consist of lanthanides and actinides, found at the bottom of the periodic table.
- Key transition elements include iron (Fe), copper (Cu), silver (Ag), and gold (Au), pivotal in human civilization.
- Lanthanides (4f) span from cerium (Ce) to lutetium (Lu), while actinides (5f) range from thorium (Th) to lawrencium (Lr).
Properties of Transition Elements
- Transition metals exhibit typical metallic characteristics: high tensile strength, ductility, malleability, and good thermal/electrical conductivity.
- Exceptions to typical structures include zinc (Zn), cadmium (Cd), mercury (Hg), and manganese (Mn), which do not exhibit standard metallic structures.
Lattice Structures
- Various typical metallic lattice structures include:
- Body-Centered Cubic (bcc): Sc, Cr, Mo, and W.
- Face-Centered Cubic (ccp): Ni, Cu, and Ag.
- Hexagonal Close Packed (hcp): Ti, Co, and Ru.
Enthalpy of Atomisation
- Transition metals have higher enthalpies of atomisation due to numerous unpaired electrons leading to stronger interatomic interactions.
- Zinc has the lowest enthalpy of atomisation in the 3d series, indicating weaker bonding compared to others.
Ionisation Enthalpy Trends
- Ionisation enthalpies generally increase across the series due to increasing nuclear charge.
- Variations in ionisation enthalpy are less steep than in non-transition elements.
- The removal of electrons affects the relative energies of 4s and 3d orbitals, influencing ionisation values.
Oxidation States
- Transition metals exhibit a wide range of oxidation states; this diversity is essential for their chemical reactivity.
- Common oxidation states for first-row transition metals include +1, +2, +3, +4, +5, and +6.
Compounds and Reactions of Transition Metals
- Manganese can exhibit variable oxidation states, such as transitioning from Mn(II) to Mn(VI).
- Potassium permanganate (KMnO4) exhibits intense color and is used in various oxidation reactions:
- It oxidises oxalates to carbon dioxide, iron(II) to iron(III), and nitrites to nitrates.
Molecular Structure and Properties
- The manganate ion (MnO4^2-) is tetrahedral and paramagnetic due to an unpaired electron, while permanganate (MnO4^-) is diamagnetic with no unpaired electrons.
- Potassium permanganate is poorly soluble in water but decomposes upon heating.
Summary of Reactions Involving Permanganate
- Acidified permanganate solutions participate in redox reactions:
- Oxidation of oxalate: COO^- → 5 CO2 + 10 e^-
- Oxidation of Fe(II): Fe^2+ → Fe^3+ + e^-
- The balancing of reductant half-reactions is crucial for writing complete redox reactions.
These notes encapsulate the fundamental aspects and properties of d- and f-block elements and highlight their significance in chemistry.
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Description
This quiz focuses on the positions and properties of d- and f-block elements in the periodic table. You will test your knowledge about transition metals like iron, copper, silver, and gold. Prepare to explore these essential chemical families in depth.