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Questions and Answers

What is the most significant achievement in the 19th century related to chemistry?

The most significant achievement in the 19th century related to chemistry was Dmitri Mendeleev's work on the periodic classification of elements.

The energy of an electron in an Xp orbital is greater than an electron in an Xs orbital.

True (A)

What is the symbol for the screening constant?

σ

What is the definition of ionization energy?

<p>The minimum energy (kJ/mol) required to remove an electron from a gaseous atom in its ground state. (A)</p> Signup and view all the answers

How does the radius of a cation compare to the radius of its neutral atom?

<p>The radius of a cation is smaller than the radius of its neutral atom.</p> Signup and view all the answers

What factors determine ionization energy?

<p>All of the above (E)</p> Signup and view all the answers

How does the first ionization energy change going down a group in the periodic table?

<p>Decreases</p> Signup and view all the answers

Which of these has the highest electron affinity?

<p>F (B)</p> Signup and view all the answers

What is the general trend in electron affinity across a period?

<p>Increases</p> Signup and view all the answers

Which of the following elements has an electron configuration ending in ns²?

<p>Magnesium (C)</p> Signup and view all the answers

Describe the general trend in atomic size going across a period?

<p>Decreases</p> Signup and view all the answers

Describe the general trend in atomic size going down a group?

<p>Increases</p> Signup and view all the answers

In the ground state of the atom, electrons will occupy the lowest energy orbital first, and only fill the higher energy orbitals when no lower energy orbitals are left.

<p>True (A)</p> Signup and view all the answers

Match the following terms with their corresponding physical property:

<p>Ionization Energy = The energy required to remove an electron from a gaseous atom Electron Affinity = The energy change when an electron is added to an atom in the gaseous state Atomic Radius = Half the distance between the nuclei of two identical atoms bonded together Effective Nuclear Charge = Strength of the attractive force between the nucleus and valence electrons Shielding Effect = The effect of inner electrons on the attraction of outer electrons by the nucleus</p> Signup and view all the answers

Flashcards

Periodic Classification of Elements

Organization of elements based on their properties and atomic structure.

Electron Configuration

Arrangement of electrons in atomic orbitals.

Effective Nuclear Charge (Zeff)

Net positive charge experienced by valence electrons.

Atomic Radius

Half the distance between nuclei of two bonded atoms.

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Ionization Energy (IE)

Energy needed to remove an electron from an atom.

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Electron Affinity (EA)

Energy change when an atom gains an electron.

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Representative Elements

Groups 1A - 7A; have incomplete s or p subshells.

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Noble Gases

Group 8A (except He); have completely filled p subshells.

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Transition Elements

Groups 3B - 8B; have incomplete d subshells.

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f-block elements

Lanthanides and Actinides; have incomplete f subshells.

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Ground State electron configuration

Arrangement of electrons in an atom's lowest energy levels.

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Aufbau Principle

Electrons fill the lowest energy levels first.

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Hund's Rule

Electrons singly fill degenerate orbitals before pairing.

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Pauli Exclusion Principle

No two electrons can have the same four quantum numbers.

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Cations

Positively charged ions, formed by losing electrons.

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Anions

Negatively charged ions, formed by gaining electrons.

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Isoelectronic Species

Atoms or ions with the same electron configuration.

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Shielding Effect

Inner electrons reduce the nuclear charge experienced by outer electrons.

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Atomic Size Trend (Group)

Atomic size increases down a group due to increasing energy levels.

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Atomic Size Trend (Period)

Atomic size decreases across a period due to increasing effective nuclear charge.

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Ionic Radius

Size of an ion.

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Ionic Size Trend (Anions)

Anions are larger than their corresponding neutral atoms.

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Ionic Size Trend (Cations)

Cations are smaller than their corresponding neutral atoms.

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Ionization Energy

Energy required to remove an electron from an atom or ion.

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Electron Affinity

Energy change when an atom gains an electron.

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Study Notes

Inorganic Chemistry - The Chemistry of the Elements

  • Chapter Outline: Understand the periodic classification of elements and their electron configurations, and identify periodic variations in physical properties (effective nuclear charge, atomic/ionic radii, ionization energy, electron affinity).

Introduction

  • Early Development: Historical context of the periodic table, mentioning significant contributions throughout history (1735-1843, 1843-1886, 1894-1918 etc.). Highlight Dmitri Mendeleev's crucial work in classifying elements based on their properties.

Periodic Classification of the Elements

  • Organization: Elements arranged in a periodic table based on their atomic structure and properties.
  • Electron Configurations: Electron arrangement within the outermost subshells (ns, np), determining similar chemical behaviours of elements within groups. The provided data gives examples of electron configurations.
  • Ground State Electron Configurations: The electron arrangement of atoms in their lowest energy state.

Classification of the Elements

  • Representative Elements (Groups 1A-7A): Main group elements with incompletely filled s or p subshells.
  • Noble Gases (Group 8A): Completely filled p subshells, inert nature due to stable electron configurations.
  • Transition Metals (Groups 3B-8B): D-block elements with incompletely filled d subshells, forming cations with these subshells.
  • Lanthanides and Actinides: F-block elements, characterized by incompletely filled f subshells.

Ground State Electronic Configurations

  • Aufbau Principle: Filling of atomic orbitals with electrons, starting from the lowest energy levels first. This concept relates to Hund's rules and Pauli exclusion principle.

Cations and Anions of Representative Elements

  • Formation: Cations (positive ions) form when atoms lose electrons, attaining a stable noble gas configuration. Anions (negative ions) result from electron gain to achieve the same configuration.
  • Isoelectronic Species: Atoms and ions with identical electron configurations (e.g., Na+, Mg2+, F-, O2- all isoelectronic with Ne).
  • Atomic Size: Generally increases down a group (more energy levels, greater distance from the nucleus) and decreases across a period (increasing nuclear charge). Diatomic molecule distance is a measurable quantity reflecting this.
  • Ionic Radii: Anions are larger than their neutral atoms, and cations are smaller respectively. Electron-proton attraction and electron-electron repulsion are key factors influencing this trend.
  • Shielding Effect: Outer electrons are shielded from the full positive charge of the nucleus by inner electrons. This shielding effect affects atomic properties.

Effective Nuclear Charge (Zeff)

  • Definition: Positive charge felt by an electron, reduced by shielding from inner electrons. Increases across a period.

Ionization Energy

  • Definition: Energy needed to remove an electron from a gaseous atom. Increases across a period. Decreases down a group (higher energy levels are further from the nucleus).
  • Exceptions: Half-filled and filled orbitals lead to lower ionization energies due to stability.

Electron Affinity

  • Definition: Energy change when a gaseous atom gains an electron to form an anion. Increases generally across a period (greater attraction to nucleus). Decreases down a group. Exceptions exist due to orbital stability.

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