 | Term | Definition |
| |
covalent bond |
A chemical bond formed between two atoms by sharing a pair of electrons. |
| |
dipole |
a molecule that is electrically asymmetrical, causing it to be oppositely charged at two points. |
| |
electronegativity |
the relative attraction that an atom has for a pair of shared electrons in a covalent bond. |
| |
ionic bond |
the chemical bond between a positively charged ion and a negatively charged ion. |
| |
ionization energy |
the energy required to move an electron from an atom, an ion, or a molecule. |
| |
Lewis structure |
a method of indicating the covalent bonds between atoms in a molecule or an ion such that a pair of electrons (:) represents the valence electrons forming the covalent bond. |
| |
linear structure |
in the VSEPR model, an arrangement where the pairs of electrons are arranged 180 degrees apart for maximum separation. |
| |
nonpolar covalent bond |
a covalent bond between two atoms with the same electronegativity value; thus, the electrons are shared equally between the two atoms. |
| |
polar covalent bond |
a covalent bond between two atoms with differing electronegativity values, resulting in unequal sharing of bonding electrons. |
| |
resonance structure |
a molecule or ion that has multiple Lewis structures. |
| |
tetrahedral structure |
an arrangement of the VSEPR model where four pairs of electrons are placed 109.5 degrees apart to form a tetrahedron. |
| |
trigonal planar |
an arrangement of atoms in the VSEPR model where the three pairs of electrons are placed 120 degrees apart on a flat plane. |
