Inorganic Chemistry: Associated Course - 1 (AC-1) Syllabus Review

This set of vocabulary flashcards provides definitions for the major concepts, theories, and laws outlined in the Inorganic Chemistry (AC-1) syllabus for Semester-I, covering basic concepts, atomic structure, periodicity, and chemical bonding.

Mole concept

A fundamental concept in chemistry used for expressing the amount of a substance, involving laws of chemical combination and stoichiometry.

Strength of Solution

A measure of the amount of solute in a given amount of solvent or solution, typically expressed as Normality, Molarity, or Molality.

Bohr's theory

A theory describing the atomic structure and atomic spectrum of the hydrogen atom, including its specific limitations.

de' Broglie equation

An equation in wave mechanics that relates the wave nature of matter to its momentum.

Heisenberg's Uncertainty Principle

A principle in quantum mechanics stating that it is impossible to simultaneously determine the exact position and momentum of a particle.

Schrodinger's wave equation

A fundamental equation in wave mechanics used to describe the behavior and energy levels of electrons in an atom.

$\psi$ and $\psi^2$

Variables in Schrodinger's wave equation where $\psi$ represents the wave function and $\psi^2$ represents the probability density of finding an electron.

Pauli's Exclusion Principle

A principle stating that no two electrons in an atom can have the same set of four quantum numbers.

Hund's rule of maximum multiplicity

A rule stating that for a given electron configuration, the lowest energy term is the one with the greatest value of spin multiplicity.

Aufbau principle

A rule used to determine the electron configuration of an atom, subject to specific limitations and used to describe the variation of orbital energy with atomic number.

Slater rules

A set of rules used to calculate the effective nuclear charge and the shielding or screening effect in an atom.

Ionization enthalpy

The energy required to remove an electron from a gaseous atom; involves successive enthalpies and various factors that affect ionization energy.

Electron gain enthalpy

The energy change that occurs when an electron is added to a neutral gaseous atom, including its trends across the periodic table.

Sanderson electron density ratio

A specific ratio used in the discussion of electronegativity, partial charge, and hybridization.

Radius ratio rule

A rule used to predict the coordination number and structure of ionic crystals based on the sizes of the ions, including its limitations.

Born - Lande equation

An equation derived to provide an expression for the lattice energy of an ionic crystal.

Mandelung constant

A geometric factor used in the calculation of lattice energy for ionic crystals.

Born-Haber cycle

A cycle used to analyze the energetics of ionic compounds and calculate lattice energy.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A theory used to predict the shapes of simple molecules and ions based on the lone and bond pairs of electrons.

Valence Bond theory (VBT)

An approach to chemical bonding involving the Heitler London approach and the hybridization of $s$, $p$, and $d$ atomic orbitals.

Bent Rule

A rule used in hybridization and chemical bonding to explain the shapes of hybrid orbitals and resonance energy.

Molecular orbital theory (MOT)

A theory describing the electronic structure of molecules using molecular orbital diagrams for homonuclear and heteronuclear diatomic and polyatomic molecules.

Fajan's rules

Rules describing the covalent character in ionic compounds based on polarizing power and polarizability.

Dipole moment

A measure used to determine the ionic character in covalent compounds and bond moments.