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Unit 3: Bonding
Chemistry
Term | Definition |
---|---|
Electron configuration | The arrangement of electrons in an 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 structural formula in which electrons are represented by dots; dots 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 | Describes a molecule in which the positive and the negative charges are separated |
Nonpolar | A nonpolar molecule is one whose charge distribution is spherically symmetric when averaged over time |
Bent | 2 atoms bonded to central atom & 1 lone pairs of electron(s) |
Tetrahedral | 4 atoms bonded to central atom & 0 lone pairs of electron(s) |
Trigonal Planar | 3 atoms bonded to central atom & 1 lone pairs of electron(s) |
Linar | 2 atoms bonded to central atom & 0 lone pairs of electron(s) |
Valence Electrons | An electron that is found in the outermost shell of an atom and that determines the 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 |