Term
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Definition
| the elements that are electron donors |
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Term
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Definition
| the elements that are electron acceptors |
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Term
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Definition
| the attractive forces between cations and anions; may result in ionic bonds |
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Term
| the type of chemical bond that occurs between elements of vastly different metal and nonmetal character |
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Definition
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Term
| the type of chemical bond that occurs between elements of similar metal and nonmetal character |
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Definition
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Term
| the covalent character of a bond depends on... |
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Definition
| the difference in the tendency of the atoms to attract electrons |
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Term
| when the covalent character of a bond increases |
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Definition
| when atoms become more equal in their electronegativity |
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Term
| is a bond ever 100% ionic? |
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Definition
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Term
| where the only 100% covalent bonds are |
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Definition
| between 2 atoms of the same element |
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Term
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Definition
| the ability of an atom in a molecule to attract electrons |
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Term
| elements w/ low EN act as... |
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Definition
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Term
| elements w/ high EN act as... |
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Definition
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Term
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Definition
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Term
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Definition
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Term
| the actual character of a bond formed between 2 elements is predicted by... |
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Definition
| the difference in their EN values |
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Term
| description of a bond between 2 elements with similar EN |
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Definition
| principally covalent with little ionic bond character |
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Term
| description of a bond between 2 elements with very different EN |
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Definition
| a bond whose ionic character is proportional to the magnitude of ΔEN |
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Term
| how to calculate % ionic character |
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Definition
| % ionic character = 100 x [1 - e(-0.25 x ΔEN2)]
developed by Linus Pauling to describe the nature of the chemical bond |
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Term
| values of ΔEN that are ionic |
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Definition
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Term
| values of ΔEN that are polar covalent |
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Definition
| those between 0.6 and 1.7 |
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Term
| why the polar covalent bond is polar |
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Definition
-the atom with the greater EN has a greater proportion of the shared electron density, becoming slightly negative
-the atom with the lesser EN has a lesser proportion of the shared electron density, becoming slightly positive
C—O, S—O, P—O, H—O |
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Term
| values of ΔEN that are nonpolar covalent |
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Definition
| less than approximately 0.7 |
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Term
| why the nonpolar covalent bond is nonpolar |
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Definition
| because the valence electrons reside almost completely with the more electronegative species, such as N—O |
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Term
| values of ΔEN that are pure covalent |
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Definition
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Term
| why the pure covalent bond is pure |
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Definition
| because the sharing of electrons is equal, such as in diatomic elements |
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Term
| the 2 most common bond types in soil minerals |
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Definition
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Term
| a bond, other than ionic and covalent, that occurs in minerals |
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Definition
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Term
| the strength of hydrogen bonds |
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Definition
| 1/20 the strength of the polar covalent bond in water molecules (about 23.3 kJ/mol vs. 492 kJ/mol) |
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Term
| where hydrogen bonds may occur |
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Definition
| between protons and O, F, N, and other electronegative atoms |
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Term
| the bond between adjacent aluminum hydroxide and silicate sheets in one unit in kaolinite |
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Definition
| principally ionic bonds having strong covalent character |
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Term
| the type of bond between adjacent units in kaolinite |
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Definition
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Term
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Definition
| attractive forces that can occur between neutral surfaces or molecules that are nonpolar |
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Term
| van der Walls bonding arises from... |
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Definition
| permanent or induced dipole interactions or from interactions that are caused by the dynamic polarization (also called dispersive forces) of neutral molecules |
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Term
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Definition
| van der waals forces that arise from the dynamic polarization of neutral molecules |
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Term
| some minerals in which van der Waals forces occur |
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Definition
| the clay minerals talc and pyrophyllite, where adjacent, neutrally charged sheets are held together by van der Walls forces |
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