Ionization Energy and Electronic Configurations

This set of flashcards covers key concepts related to ionization energy, electronic configurations, and trends in the periodic table.

Discrete Energy Levels

The specific levels of energy that electrons occupy in an atom, as suggested by emission spectra.

Ionization Energy

The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions under standard conditions.

Lyman Series

A set of spectral lines corresponding to transitions of electrons in hydrogen from higher energy levels down to the first energy level.

Planck's Constant (h)

A constant used to describe the sizes of quanta; its value is approximately $6.63 imes 10^{-34} ext{ J s}$.

Successive Ionization Energies

The energies required to remove electrons one at a time from a gaseous atom or ion, which provide information about the electronic structure.

Shielding Effect

The phenomenon where inner electron shells reduce the effective nuclear charge felt by outer electrons, leading to lower ionization energy.

Electronic Configuration

The distribution of electrons in an atom's orbitals, described using quantum numbers.

Electrons in Orbitals

Regions of space around the nucleus where there is a high probability of finding an electron.

First Ionization Energy Trend Across a Period

Ionization energy generally increases across a period due to increased nuclear charge and consistent shielding.

Factors Influencing Ionization Energies

1. Nuclear charge increases; 2. Distance of outer electrons from the nucleus; 3. Shielding effect of inner electrons.

Pauli Exclusion Principle

No two electrons in an atom can have the same set of quantum numbers; therefore, only two electrons may occupy the same orbital with opposite spins.

Orbital Shape of s Orbital

s Orbitals are spherical and non-directional, meaning the probability of finding an electron is the same in all directions at a given distance from the nucleus.

p Subshell Orbitals

p Orbitals are dumbbell-shaped and directional, with three mutually perpendicular orbitals in each p subshell.

Aufbau Principle

Electrons fill the lowest energy orbitals first before occupying higher energy orbitals.

Hydrogen Ionization Energy

Calculated as $1308 ext{ kJ mol}^{-1}$, representing the energy needed to remove an electron from a hydrogen atom.

Noble Gases Ionization Energy Feature

Noble gases have extremely high first ionization energies due to their stable electron configuration.

Chemical Properties Periodicity

The recurring trends in properties of elements across different periods due to their electronic configurations.

Half-Filled Stability

The increased stability of atoms with half-filled subshells, which is due to symmetrical electron distribution.