states that in the ground state of an atom or ion, electrons fill subshells of the lowest available energy, then they fill subshells of higher energy

A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms

The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion

In atomic theory and quantum mechanics, an atomic orbital is a mathematical function describing the location and wave-like behavior of an electron in an atom.

Hund's rule of maximum multiplicity is a rule based on observation of atomic spectra, which is used to predict the ground state of an atom or molecule with one or more open electronic shells.

an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

Lewis electron dot structures, are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.

Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions.

Molecular geometry is the three-dimensional arrangement of the atoms that constitute a molecule.

The octet rule is a chemical rule of thumb that reflects the theory that main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas

The oxidation state, sometimes referred to as oxidation number, describes the degree of oxidation of an atom in a chemical compound.

Pauliexclusion principle

the assertion that no two fermions can have the same quantum number.

Valence shell electron pair repulsion theory, or VSEPR theory, is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.

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vocab unit 3

Term	Definition
Aufbau Principle	states that in the ground state of an atom or ion, electrons fill subshells of the lowest available energy, then they fill subshells of higher energy
Covanlent bond	A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms
Electron Affinity	The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion
Electron Orbitals	In atomic theory and quantum mechanics, an atomic orbital is a mathematical function describing the location and wave-like behavior of an electron in an atom.
Hund's rule	Hund's rule of maximum multiplicity is a rule based on observation of atomic spectra, which is used to predict the ground state of an atom or molecule with one or more open electronic shells.
Ion	an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
Lewis dot structure	Lewis electron dot structures, are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
Metallic bond	Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions.
Molecular geometry	Molecular geometry is the three-dimensional arrangement of the atoms that constitute a molecule.
Octet rule	The octet rule is a chemical rule of thumb that reflects the theory that main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas
Oxidation number	The oxidation state, sometimes referred to as oxidation number, describes the degree of oxidation of an atom in a chemical compound.
Pauliexclusion principle	the assertion that no two fermions can have the same quantum number.
VSEPR theory	Valence shell electron pair repulsion theory, or VSEPR theory, is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.

Created by: jg373064

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