| 41. | Such bonds occur between two atoms with moderately different electronegativities and give rise to dipole-dipole interactions.
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| 42. | The electronegativity difference between the two atoms in these bonds is 0.3 to 1.7.
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| 43. | Elements in the same group tend to show patterns in atomic radius, ionization energy, and electronegativity.
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| 44. | Gallium and germanium have higher electronegativities than aluminium and silicon respectively because of the d-block contraction.
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| 45. | The above cases seem to demonstrate that the size of the chlorine is less important than its electronegativity.
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| 46. | Bonds to fluorine have considerable ionic character, a result of its small atomic radius and large electronegativity.
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| 47. | See also the elements'electronegativity difference for a ( perhaps outdated ) way to determine bonding types.
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| 48. | In more complex compounds, there is additional error since electronegativity depends on the molecular environment of an atom.
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| 49. | Elements in the same period show trends in atomic radius, ionization energy, electron affinity, and electronegativity.
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| 50. | This absorption is strengthened because these bonds are highly polar due to the extreme electronegativity of the fluorine atom.
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