Ionization Energies and Electronic Configurations

These flashcards cover key concepts from the lecture on ionization energies and electronic configurations, providing definitions and explanations.

Ionization Energy

The energy required to remove an electron from a gaseous atom.

Electron Configuration

The distribution of electrons in an atom’s orbitals.

Discrete Energy Levels

The specific energy levels that electrons occupy within an atom.

Emission Spectrum

The spectrum of light released from excited atoms as they return to lower energy states.

Planck’s Constant (h)

A physical constant used to describe the sizes of quanta in quantum mechanics, approximately $6.63 imes 10^{-34} ext{ J s}$.

Lyman Series

A series of spectral lines corresponding to transitions from higher energy levels to the ground state in hydrogen.

Ground State

The lowest energy state of an atom, where electrons occupy the lowest available energy levels.

Shielding Effect

The phenomenon where inner electrons shield outer electrons from the full effect of the nucleus's positive charge.

Successive Ionization Energies

The energies required to remove additional electrons from an atom after the first ionization.

Convergence Limit

The point at which energy levels become infinitely close together, often related to the ionization energy of an atom.

First Ionization Energy of Calcium

The energy required to remove one electron from a neutral calcium atom.

Second Ionization Energy of Nitrogen

The energy needed to remove the second electron from a positively charged nitrogen ion.

Atomic Radius

The size of an atom, typically measured from the nucleus to the outer boundary of the surrounding cloud of electrons.

Nuclear Charge

The total charge of the nucleus, determined by the number of protons.

Electron Shielding

The reduction of effective nuclear charge on the electron cloud, due to repulsion by inner-shell electrons.

Trend in Ionization Energies Across a Period

Ionization energy generally increases as you move from left to right across a period in the periodic table.

Trend in Ionization Energies Down a Group

Ionization energy generally decreases as you move down a group in the periodic table.

Hund's Rule

Electrons will occupy degenerate orbitals singly before pairing up.

Pauli Exclusion Principle

No two electrons in an atom can share the same set of quantum numbers.

S Orbital

An orbital with a spherical shape that can hold a maximum of two electrons.

P Orbital

An orbital with a dumbbell shape that can hold a maximum of six electrons (three p orbitals).

D Orbital

An orbital that can hold a maximum of ten electrons, with more complex shapes.

Successive Ionization Energy Data

Values that reflect the energy required to remove electrons in succession, helping identify element groups.

Outer Electron Shells

The electron shells that are farthest from the nucleus, which contain the outermost electrons.

Core Electrons

Electrons located in the inner shells of an atom, not involved in bonding.

Relative Stability of Electron Configurations

The concept that certain configurations, especially filled and half-filled subshells, have lower energy and greater stability.

Electrostatic Attraction

The force that holds the electrons in atoms due to the attraction between negatively charged electrons and positively charged protons.

Electron Excitation

The process of an electron absorbing energy and moving to a higher energy level.

Ionization Reaction

A chemical reaction in which an electron is removed from an atom or molecule.

Cation Formation

The process of ion formation when an atom loses one or more electrons.

Anion Formation

The process of ion formation when an atom gains one or more electrons.

Group of the Periodic Table

A column in the periodic table containing elements with similar properties.

Period of the Periodic Table

A row in the periodic table where properties change gradually across.

Quantum Mechanical Model

The current model of atomic structure that incorporates wave-particle duality.

Unstable Electron State

A state where electrons are in higher energy levels but cannot remain there indefinitely.

Probability Distribution of Electrons

The likelihood of finding an electron in a particular region around the nucleus.

Schrodinger's Equation

A mathematical equation that describes the wave function of a quantum system.

Factors Influencing Ionization Energies

Includes atomic size, nuclear charge, and electron shielding.

Transition between Energy Levels

Movement of electrons between different energy levels corresponding to energy absorption or emission.

Plank-Einstein Theory

Relates energy to frequency via the equations $E = hf$, where $E$ is energy, $h$ is Planck's constant, and $f$ is frequency.

Franck-Condon Principle

Explains the intensities of spectral lines as a result of vibrational transitions.

Photon

A quantum of electromagnetic radiation, which can eject electrons from atoms.

Spectroscopy

The study of the interaction between light and matter.

Comparative Ionization Energy Data

Useful for drawing conclusions about atomic structure and reactivity.

Chemical Properties of Elements

The behaviors and characteristics of elements that determine how they react with other substances.

Ytterbium Ionization Energy

A specific measured value for ionization energy relevant in analyzing electronic configurations.

Notable Electron Configurations

Highlight electron configurations of key elements that illustrate principles of stability and reactivity.

Bonding Electrons

Electrons that are involved in forming chemical bonds between atoms.