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Periodic Table
Arrangement of elements by increasing atomic number.
Dobereiner's Triads
Groups of three elements with similar properties.
Law of Octaves
Element properties repeat every eighth element.
Mendeleev's Periodic Table
Elements arranged by increasing mass, showing periodicity.
Modern Periodic Table
Elements arranged by increasing atomic number.
Periods
Horizontal rows in the periodic table.
Groups
Vertical columns containing similar elements.
Electron Configuration
Distribution of electrons in an atom's orbitals.
Ground State
Lowest energy state of an electron.
Schrödinger's Equation
Describes electron behavior in atoms.
Electron Spin
Fundamental property indicating electron orientation.
Spin Quantum Number
Fourth quantum number indicating electron spin direction.
Pauli Exclusion Principle
No two electrons can have identical quantum numbers.
Orbital Diagrams
Visual representation of electron distribution in orbitals.
Degenerate Orbitals
Orbitals with the same energy level.
Effective Nuclear Charge
Net attraction an electron feels from the nucleus.
Shielding Effect
Reduction of nuclear charge felt by outer electrons.
Penetration
Ability of an electron to approach the nucleus.
Radial Distribution Function
Describes electron probability density around the nucleus.
Multi-electron Atoms
Atoms with more than one electron.
Quantum Numbers
Set of numbers describing electron states.
Charge Interaction
Forces between charged particles in an atom.
Energy Sublevels
Different energy levels within principal energy shells.
Aufbau Principle
Electrons fill orbitals from lowest to highest energy.
Pauli Exclusion Principle
No more than two electrons per orbital.
Hund's Rule
Electrons occupy unfilled orbitals before pairing.
Condensed Electronic Configuration
Uses noble gas notation for electron arrangement.
Valence Electrons
Electrons in the outermost energy level.
Core Electrons
Electrons not in the outermost energy level.
Anomalous Electron Configurations
Unexpected electron arrangements in certain elements.
Cation
Positively charged ion formed by losing electrons.
Anion
Negatively charged ion formed by gaining electrons.
Atomic Radius
Average distance between atomic nuclei in a molecule.
Effective Nuclear Charge (Zeff)
Charge experienced by an electron from the nucleus.
Paramagnetic
Atoms with unpaired electrons, attracted to magnets.
Diamagnetic
Atoms with all paired electrons, not attracted to magnets.
Periodic Table Blocks
Divided into s, p, d, and f sublevels.
Group Number
Indicates number of valence electrons in main-group elements.
Row Number
Indicates highest principal quantum number of elements.
Sodium Electron Configuration
1s2 2s2 2p6 3s1 or [Ne]3s1.
Ion Formation
Atoms gain or lose electrons to achieve stability.
Magnetic Properties
Determined by the presence of unpaired electrons.
Periodic Trend in Atomic Radius
Increases down a group, decreases across a period.
Electron Configuration of Ions
Ions mimic noble gas configurations for stability.
Electron Configuration and Reactivity
Valence electrons dictate chemical behavior of elements.
Zeff
Effective nuclear charge experienced by electrons.
s (shielding constant)
Represents electron shielding from nuclear charge.
Ionic radius
Size of an ion compared to its atom.
Cation radius
Smaller than corresponding neutral atom radius.
Anion radius
Larger than corresponding neutral atom radius.
Isoelectronic ions
Ions with the same number of electrons.
Ionization energy (IE)
Energy required to remove an electron from an atom.
First Ionization Energy
Energy to remove the first electron from neutral atom.
Second Ionization Energy
Energy to remove the second electron from an ion.
Trends in IE
IE decreases down a group, increases across a period.
Electron Affinity (EA)
Energy change when an electron is added to an atom.
Positive EA
Indicates energy is released when gaining an electron.
Negative EA
Indicates energy is absorbed when gaining an electron.
Trends in EA
No definite trend across periodic table groups.
Metallic Character
Tendency of an element to lose electrons.
Effective nuclear charge
Net positive charge experienced by valence electrons.
Successive Ionization Energies
Energy increases with each successive electron removal.
Periodic trend in ionic radii
Ion size increases down a group.
First IE exceptions
Notable deviations in ionization energy trends.
Electron pairing
Occurs when adding electrons to orbitals.
Atomic size arrangement
Order elements by decreasing atomic size.
Comparing ionic sizes
List ions by increasing ionic size.
