Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
UNIT 3
Electrons and bonding
| Term | Definition |
|---|---|
| AUFBAC Principle | The aufbau principle, from the German Aufbauprinzip, also called the aufbau rule, states that in the ground state of an atom or ion, electrons fill sub shells of the lowest available energy, then they fill sub . |
| Covalent Bond | A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs, and the stable balance of attractive and repulsive forces between atoms, when they share electro |
| 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. This function can be used to calculate the probability of finding any electron of an atom in any |
| 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 | Ions are charged atoms, meaning a neutral atom has lost or gained electrons giving the atom an electric charge. Gaining electrons makes the atom negatively charged, and losing electrons makes the atom positively charged. |
| Lewis dot structure | Lewis structures, also known as Lewis dot formulas, Lewis dot structures, electron dot structures, or 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 t |
| 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. It may be described as the sharing of free electrons among a structure of positively charged |
| Molecular geometry | Molecular geometry is the three-dimensional arrangement of the atoms that constitute a molecule. It includes the general shape of the molecule as well as bond lengths, bond angles, torsional angles and any other geometrical parameters that determine the p |
| 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 # | The oxidation state, sometimes referred to as oxidation number, describes the degree of oxidation of an atom in a chemical compound. |
| Pauli exclusion principle | The Pauli exclusion principle says that no two electrons can have the same set of quantum numbers; that is, no two electrons can be in the same state. This exclusion limits the number of electrons in atomic shells and subshells. Each value of n correspond |
| 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:
Oa459702
Popular Chemistry sets