Chemistry Terminology: Bonding

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Can you name the Chemistry Terminology of Bonding by definition?

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Description of TermTerm
The amount of energy necessary to break a bond. This energy is a measure of how hard it is to break a bond.
A negatively charged ion.
A measure of the ability of an atom to attract electrons to itself.
A nonbonding pair of electrons.
The difference between the number of bonding electron pairs an the number of antibonding electron pairs in a molecule.
Eight electrons. For atoms other than H, the valence shell is filled with eight electrons. A filled valence gives the molecule a noble gas configuration and renders it stable.
The charge on an atom in a molecule.
A mathematical formula whose consequence is that negatively and positively charged particles attract each other and similarly charged species repel each other.
The orbitals with the highest occupied principle quantum number.
A positively charged ion.
A regularly repeating three-dimensional array of atoms, molecules, or ions.
An electron configuration with a full valence shell.
A bond that results from a sharing of electrons between nuclei.
The process by which atomic orbitals are combined to produce a new set of orbitals suitable for use in a discussion of bonding in polynuclear atoms.
Discussed in Molecular Orbital Theory, Heading , such diagrams show the relative energy and the parentage of molecular orbitals from atomic orbitals.
One of several Lewis structures whose average represents an accurate depiction of the molecule not properly represented by one simple Lewis structure.
Description of TermTerm
A chemical species containing a covalent bond.
The three dimensional structure and orientation of the atoms, bonds, and lone pairs in a molecule.
A description of bonding that combines atomic orbitals from each bondedatom to produce a set of molecular orbitals.
A molecular orbital that results from an out-of-phase overlap of atomic orbitals to produce an orbital that is higher in energy than either of its parent molecular orbitals.
A charged species created by the gain or loss of an electron from an atom or neutral molecule.
A measure of how well two orbitals constructively interfere with one another.
A theory used to predict bonding geometries that states that electron pairs will be distributed about the central atom to minimize electron pair repulsions.
A molecular orbital that results from an in-phase overlap of atomic orbitals that has a lower energy than either of its parent atomic orbitals.
A description of a covalent bond whereby electrons are represented by dots and a bond is represented by placing a line between the two atoms in that bond.
The direction and magnitude of the charge separation in a bond.
A combination of atomic orbitals in molecular orbital theory that provides an orbital description of a molecule analogous to the atomic orbital description of atoms.
An electron configuration with a partially filled valence shell.
That which holds together atoms in molecules and ions in lattices.
A bond that results from electrostatic attraction between oppositely charged ions. The cation is positively charged, while the anion is negatively charged.
The distance between bonded nuclei.

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