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| Mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together;Atoms are usually less stable by themselves than combined with other atoms |
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| Chemical bonding resulting from the attractions of cations and anions; In pure ionic bonding, atoms give up electrons completely to other atoms, which accept them completely to form ions which attract one another |
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| Results from sharing of electrons between two atoms; A pure covalent bond results in the electrons being “owned” equally by two atoms, both have equal electronegativities. |
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| electrons shared unequally |
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| electrons shared between atoms equally |
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| Bond type depending on electronegativity difference: 0-0.3, greater than 0.3-1.7, >1.7 |
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| nonpolar covalent, polar covalent, ionic |
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| neutral group of atoms held together by covalent bonds |
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| How does a covalent bond form? |
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| As the atoms near each other, the nuclei are attracted to each other which decreases the potential energy. But the nuclei will repel each other and so will the electrons, this increases potential energy. Ultimately the attractive forces are dominant resulting in a decrease of potential energy at which point a distance is reached where the repulsion between the like charges equals the attraction of the opposite charges |
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| what is the distance called where a covalent bonds's atoms are close enough where the repulsion between like charges equals the attraction of opposite charges. |
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| energy required to break a chemical bod and form neutral isolated atoms |
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| chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has 8 electrons in its highest occupied energy level. |
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exceptions to octet rule:
hydrogen
beryllium
boron
aluminum
atoms of elements in groups 15, 16, 17, and 18 except N, O, and F |
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2 electrion
4 electrons
6 elections
6 electrons
can form expanded octets; more than 8 electrons |
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| Which element are more apt to have multiple bonds? |
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| how to calculate formal charge |
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| # valence electrons-# of bonds around atom-lone pair electrons around atom |
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