w7- pdf

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What does the Pauli exclusion principle imply about electrons in an atom?

Electrons can occupy the same orbital if they have different spin states.

Electrons must possess unique sets of quantum numbers to avoid pairing. (correct)

Electrons have the ability to share orbitals if they are in different energy levels.

All electrons will occupy the lowest energy orbitals regardless of quantum numbers.

Which statement best describes Hund's rule?

Electrons fill orbitals in pairs before filling singly.

Electrons in degenerate orbitals must be in pairs with opposite spins.

Electrons fill available orbitals in order of decreasing energy.

Each orbital in a degenerate set must be singly occupied before any pairing occurs. (correct)

According to the Aufbau principle, how does electron filling occur?

Electrons fill the lowest available energy levels first. (correct)

Electrons fill orbitals from highest to lowest energy first.

Electrons occupy higher energy orbitals before lower ones.

Electrons can fill any orbital irrespective of energy levels.

What characteristic is true for the d-block elements in terms of electron configuration?

They have partially filled d-orbitals in their ground state configurations. Signup and view all the answers

Which statement correctly describes electron shielding among d-block elements?

Core electrons effectively shield valence electrons in d-block elements. Signup and view all the answers

Which statement accurately describes the order of filling of orbitals for transition metals?

nd orbitals are filled before the (n+1)s orbital generally for transition metals. Signup and view all the answers

Why are Cr and Cu's electron configurations considered exceptions?

Their configurations demonstrate how the half or fully filled concept does not apply uniformly. Signup and view all the answers

When comparing atomic radii, how do d-block elements generally behave?

They exhibit a consistent decrease in atomic radius across a period. Signup and view all the answers

What typically occurs to ionization energy as one moves across the d-block elements?

Ionization energy progressively increases. Signup and view all the answers

What is the primary impact of electron-electron repulsions in the context of transition metals' electron configurations?

They allow the (n+1)s orbital to be filled before the nd orbitals in certain cases. Signup and view all the answers

Which atomic property is affected by electron configurations in d-block elements?

The stability of oxidation states is influenced by their electron configurations. Signup and view all the answers

In which circumstance does the Aufbau Principle fail for transition metals?

Due to the repulsive interactions in the respective orbitals. Signup and view all the answers

Which of the following correctly describes the atomic radius trend among transition metals?

The atomic radius decreases and then increases within the d-block. Signup and view all the answers

What is the relationship between the first ionisation energy and the removal of valence electrons?

Ionisation energy increases drastically after removing valence electrons. Signup and view all the answers

Which element has the highest electronegativity according to the Pauling scale?

Fluorine (F) Signup and view all the answers

What is the general trend of electronegativity across the transition metal series?

Increases across the series and decreases down the group. Signup and view all the answers

How is electron affinity generally characterized for EA1?

It is mostly negative. Signup and view all the answers

Which of the following statements about EA2 is correct?

It is always positive. Signup and view all the answers

What trend is generally observed in the atomic radius of transition metals?

It increases down the group and decreases across the series. Signup and view all the answers

What factor contributes to the increased ionisation energy after removing valence electrons?

The decrease in electron shielding. Signup and view all the answers

What is a characteristic of d-block elements regarding their electron configuration?

They have partially filled d orbitals. Signup and view all the answers

Which of these elements exhibits an increase in electronegativity down the group?

Rhenium (Re) Signup and view all the answers

What is the expected trend of ionisation energy from magnesium (Mg) to aluminium (Al)?

It decreases. Signup and view all the answers

What is the primary determining factor for the order of electron addition in orbital filling?

The sum of the principal quantum number (n) and angular quantum number (l). Signup and view all the answers

In the context of electron configuration, what does the notation [Ar] represent?

A simplified representation of the full electron configuration for elements after argon. Signup and view all the answers

Which statement correctly describes Hund's rule?

Every orbital in a subshell must have one electron before any orbital gets a second electron. Signup and view all the answers

How does the atomic radius trend across the d-block elements?

It consistently decreases from left to right across the row. Signup and view all the answers

What is the effect of electron shielding on ionization energy within d-block elements?

Increased shielding leads to decreased ionization energy. Signup and view all the answers

For nickel (Ni), what is the correct full electron configuration?

1s2 2s2 2p6 3s2 3p6 4s2 3d8 Signup and view all the answers

What does the term 'noble gas configuration' refer to in electron configurations?

An electron arrangement exhibiting full outer subshells, leading to chemical inertness. Signup and view all the answers

How does the general configuration of d-block elements typically appear?

Noble gas core followed by (n-1)d and ns electrons. Signup and view all the answers

What is the importance of the principle quantum number (n) in determining an element's electron configuration?

It indicates the energy level and size of the orbital. Signup and view all the answers

Which principle states that no two electrons in an atom can have the same set of quantum numbers?

Pauli exclusion principle Signup and view all the answers

What effect does electron shielding have on the ionization energy of transition metals?

It decreases the ionization energy by reducing the effective nuclear charge experienced by outer electrons. Signup and view all the answers

Which electronic configuration correctly represents a transition metal in the d-block?

[Xe] 6s² 4f¹⁴ 5d⁹ Signup and view all the answers

What characteristic of d-orbitals contributes to the exceptional properties of transition metals?

They are five-fold degenerate and directional, enabling complex bonding. Signup and view all the answers

Which statement accurately describes the atomic radius trend in transition metals?

The atomic radius tends to decrease across the period due to increasing nuclear charge. Signup and view all the answers

What general trend is observed in the ionization energy of transition metals as you move from left to right across the d-block?

Ionization energy increases due to increasing nuclear attraction on valence electrons. Signup and view all the answers

Which quantum number represents the shape of d-orbitals in transition metals?

Azimuthal quantum number (l) Signup and view all the answers

Why do transition metals often form colored compounds?

The presence of d-electrons allows for transitions that absorb certain wavelengths. Signup and view all the answers

Which factor primarily influences the variation of atomic radius in transition metals?

The amount of electron shielding from inner shells. Signup and view all the answers

Which of the following correctly matches a property with transition metals?

Transition metals typically exhibit variable oxidation states. Signup and view all the answers

In terms of electron configuration, which statement is true for transition metals?

They can have variable numbers of d-electrons during ionization. Signup and view all the answers

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.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

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!