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Unit 3: Bonding
Term | Definition |
---|---|
Electron configuration | The arrangement of electrons in an atom |
Covalent bond | A bond formed when atoms shared 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 structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent 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 | A covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom |
nonpolar | A covalent bond in which bonding electrons are equally attracted to both bonded atoms |
bent | 2 atoms are bonded to the central atom and there are 1 to 2 lone pairs |
tetrahedral | There are 4 atoms that are bonded to the central atom and 0 lone pairs |
trigonal planar | 3 atoms that are bonded to the central atom and 0 lone pairs |
linear | 2 atoms that are bonded to the central atom and 0 lone pairs |
valence electrons | An electron that is found in the outermost shell of an atom and that determines the atomĀ“s chemical properties |
formula unit | The simplest collection of atoms from which an ionic compoundĀ“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 |