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Unit 3: Bonding
Term | Definition |
---|---|
Electron configuration | The arrangement of electrons in atom. |
Covalent bond | A bond formed when atoms share one or more pairs of electrons. |
Ionic bond | A force that attracts electrons from one atom to another, which transforms a neutral atom into an ion. |
Ion | An atom, radical, or molecule that has gained or lost one or more electrons and has a negative or positive charge. |
Lewis dot structure (electron-dot notation) | A structure formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represents pairs in covalent bonds. |
Octet rule | An atom will be most stable when surrounded by 8 electrons in the valence shell (outer most energy level) |
Metallic bond | A bond formed by the attraction between positively charged metal ions and the electrons around them. |
Conductivity | Material that is able to conduct electricity |
Polar | Describes a molecule in which the positive and negative charges are separated. |
Nonpolar | A covalent bond in which the bonding electrons are equally attracted to both bonded atoms. |
Bent | Two atoms bonded to central atom; One lone pair of electrons. |
Tetrahedral | Four atoms bonded to central atom. |
Trigonal Planar | Three atoms bonded to central atoms. |
Linar | Two atoms bonded to central atom . |
Valence electrons | An electron that is found in the outermost shell of an atom and that determines that atom's chemical properties. |
Formula unit | The simplest collection of atoms from which an ionic compound's formula can be written. |
Polyatomic ion | An ion made of two or more atoms. |
VSEPR theory | A theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other. |