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Questions and Answers
What does the Pauli exclusion principle imply about electrons in an atom?
Which statement best describes Hund's rule?
According to the Aufbau principle, how does electron filling occur?
What characteristic is true for the d-block elements in terms of electron configuration?
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Which statement correctly describes electron shielding among d-block elements?
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Which statement accurately describes the order of filling of orbitals for transition metals?
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Why are Cr and Cu's electron configurations considered exceptions?
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When comparing atomic radii, how do d-block elements generally behave?
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What typically occurs to ionization energy as one moves across the d-block elements?
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What is the primary impact of electron-electron repulsions in the context of transition metals' electron configurations?
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Which atomic property is affected by electron configurations in d-block elements?
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In which circumstance does the Aufbau Principle fail for transition metals?
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Which of the following correctly describes the atomic radius trend among transition metals?
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What is the relationship between the first ionisation energy and the removal of valence electrons?
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Which element has the highest electronegativity according to the Pauling scale?
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What is the general trend of electronegativity across the transition metal series?
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How is electron affinity generally characterized for EA1?
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Which of the following statements about EA2 is correct?
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What trend is generally observed in the atomic radius of transition metals?
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What factor contributes to the increased ionisation energy after removing valence electrons?
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What is a characteristic of d-block elements regarding their electron configuration?
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Which of these elements exhibits an increase in electronegativity down the group?
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What is the expected trend of ionisation energy from magnesium (Mg) to aluminium (Al)?
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What is the primary determining factor for the order of electron addition in orbital filling?
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In the context of electron configuration, what does the notation [Ar] represent?
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Which statement correctly describes Hund's rule?
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How does the atomic radius trend across the d-block elements?
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What is the effect of electron shielding on ionization energy within d-block elements?
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For nickel (Ni), what is the correct full electron configuration?
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What does the term 'noble gas configuration' refer to in electron configurations?
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How does the general configuration of d-block elements typically appear?
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What is the importance of the principle quantum number (n) in determining an element's electron configuration?
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Which principle states that no two electrons in an atom can have the same set of quantum numbers?
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What effect does electron shielding have on the ionization energy of transition metals?
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Which electronic configuration correctly represents a transition metal in the d-block?
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What characteristic of d-orbitals contributes to the exceptional properties of transition metals?
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Which statement accurately describes the atomic radius trend in transition metals?
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What general trend is observed in the ionization energy of transition metals as you move from left to right across the d-block?
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Which quantum number represents the shape of d-orbitals in transition metals?
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Why do transition metals often form colored compounds?
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Which factor primarily influences the variation of atomic radius in transition metals?
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Which of the following correctly matches a property with transition metals?
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In terms of electron configuration, which statement is true for transition metals?
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Study Notes
Orbital Filling and Electronic Configuration
- Hund's rule states that electrons will singly occupy orbitals within a degenerate set before pairing up.
- The Pauli Exclusion Principle states that no two electrons in an atom can have the same four quantum numbers.
- The Aufbau principle states that electrons fill orbitals in order of increasing energy, starting with the lowest energy level.
d-Orbitals
- d-Orbitals are directional and have two nodal planes.
- d-Orbitals are five-fold degenerate, meaning they all have the same energy.
- d-orbitals have a sign change that does not occur through the center.
Electronic Configuration of Transition Metals
- The electronic configuration of transition metals is determined by the order of orbital filling, which is not always consistent with the Aufbau principle.
- It is important to note the exceptions to the Aufbau principle for transition metals.
Electronic Configuration Exceptions
- The electronic configurations of Cr ([Ar]3d54s1) and Cu ([Ar]3d104s1) are exceptions to the Aufbau principle, as the half-filled and fully-filled d-orbitals are more stable.
- The stability of half-filled and fully-filled d-orbitals is not always observed, as tungsten (W) follows the Aufbau principle.
- The electronic configuration of transition metals is influenced by the relative energies of the nd and (n+1)s orbitals, as well as electron-electron repulsion.
Simplified Electronic Configuration
- The electronic configuration of a transition metal can be simplified using the noble gas notation. For example, the electronic configuration of nickel (Ni) is [Ar]4s2, 3d8.
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Description
Test your understanding of orbital filling and electronic configuration principles, including Hund's rule, the Pauli Exclusion Principle, and the Aufbau principle. This quiz also covers specifics related to d-orbitals and the electronic configurations of transition metals, including notable exceptions in configurations. Challenge your knowledge on these essential concepts in chemistry!