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Chemistry Chapter 6
| Term | Definition |
|---|---|
| chemical bond | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| why do most atoms chemically bond to each other? | most atoms are less stable existing by themselves than they are combined, by bonding with each other, atoms decrease in potential energy becoming more stable. |
| covalent | results from the sharing of electrons pairs between 2 atoms; forms molecules; Ex CO2, NH3 |
| Ionic | results from the electrical attraction between cations and anions; transfer of electrons between two atoms; forms formula units; Ex. AlP, KF, LiBr |
| metallic | results from the attraction between metal atoms and the surrounding sea of electrons; Ex foil, silver spoon |
| 0-0.3 electronegativity difference | the bond is non-polar covalent |
| 0.31-1.66 electronegativity difference | the bond is polar covalent |
| 1.67 or greater electronegativity difference | the bond is ionic |
| non-polar covalent bond | a covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in a balanced distribution of electrical charge; Ex. H2 and O2 |
| polar covalent bond | a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
| molecule | a molecule contains only non-metals and is covalently bonded |
| bond energy | the energy required to break a chemical bond is to form a neutral isolated atoms |
| bond length | the average distance between 2 bonded atoms |
| bond energies and bond lengths | the shorter the bond length the greater the bond energy |
| octet rule | when an atom has 8 valence electrons, this means its stable |
| electron sea model | electrons do not belong to any one atom but move freely about the metals network of empty atomic orbitas |
| why are most metals malleable and ductile but ionic crystals are not? | metallic bonding is the same in all directions throughout the solid due to the delocalized electrons |
| what determines the strength of a metallic bond? | metallic bond strength varies with the nuclear charge of the metal atoms. and, the number of electrons in the metals electron sea |
| why are metals good conductors? | the freedom of electrons to move in a network of metal atoms (the sea of electrons) |
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