7 Matching Annotations
- Nov 2017
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chem.libretexts.org chem.libretexts.org
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Example 9.3.1
Can you do some practices problems during lecture?
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chem.libretexts.org chem.libretexts.org
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A bond in which the electronegativity of B (χB) is greater than the electronegativity of A (χA), for example, is indicated with the partial negative charge on the more electronegative atom: lesselectronegativeAδ+−moreelectronegativeBδ−(8.4.1)(8.4.1)lesselectronegativemoreelectronegativeA−Bδ+δ− \begin{matrix} _{less\; electronegative}& & _{more\; electronegative}\\ A\; \; &-& B\; \; \; \; \\ ^{\delta ^{+}} & & ^{\delta ^{-}} \end{matrix} \tag{8.4.1}
This doesn't necessarily mean that the atoms themselves are positive or negative, right? This is only related to their electronegativity (0-4)? So, A could be X=2.2 and B could be X=2.4 and A would be positive because it has a lower electronegativity?
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Bond polarity and ionic character increase with an increasing difference in electronegativity.
Is the way we determine bond polarity similar to the way we determine electronegativity (simply by looking at the periodic table)?
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Both of these are properties of the isolated atom.
Would the properties be different for an atom that was not isolated?
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Recall that a lowercase Greek delta (δδ\delta) is used to indicate that a bonded atom possesses a partial positive charge, indicated by δ+δ+\delta^+, or a partial negative charge, indicated by δ−δ−\delta^-,
why are the charges partial?
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Q=μr=1.109D(3.3356×10−30C⋅m1D)(1127.8pm)(1pm10−12m)=2.901×10−20C
can we go over this in detail in class?
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