Ionic Characters

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Ionic Characters

Postby Anthony_Imperial_1G » Mon Oct 24, 2016 6:28 pm

When subtracting electronegativities of a molecule, do you take into account a subscript of an element?
For example, H2S. Would I need to multiply the electronegativity of hydrogen by two before subtracting it from sulfur, or do I just subtract the two without multiplying them.

Posts: 21
Joined: Wed Sep 21, 2016 2:58 pm

Re: Ionic Characters

Postby Rachel_Smith_3D » Mon Oct 24, 2016 6:31 pm

Subtract without multiplying. The bond type is not influenced by the number of bonds.

Kaitlin_Ryan_ 3K
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Re: Ionic Characters

Postby Kaitlin_Ryan_ 3K » Wed Oct 26, 2016 2:15 pm

How is ionic character determined?

Brian Huynh 3D
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Joined: Wed Sep 21, 2016 2:58 pm

Re: Ionic Characters

Postby Brian Huynh 3D » Wed Oct 26, 2016 2:37 pm

One factor that can help determine iconic character is the difference in electronegativity between two atoms. The greater the difference in electronegativity, the greater the charge difference and greater ionic character of the covalent bond. Typically a electronegative charge difference of > 2 indicate it is an ionic bond and < 1.5 signify covalent bonds.

Ruiz Samantha 2C
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Joined: Wed Sep 21, 2016 2:58 pm

Re: Ionic Characters

Postby Ruiz Samantha 2C » Wed Oct 26, 2016 6:20 pm

Fluorine is the most electronegative with 4.0. An easy way to remember this is by knowing that F will always be 4.0, subtracting .5 on the left it will be Oxygen with (3.5), subtract .5 on the left and it will be Nitrogen (3.0), subtract .5 and it will be followed by Carbon with (2.5), subtract .5 and it will be Boron with (2.0).

Jocelyn Sandoval 3B
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Joined: Wed Sep 21, 2016 2:59 pm

Re: Ionic Characters

Postby Jocelyn Sandoval 3B » Wed Oct 26, 2016 7:25 pm

Also, you can determine the ionic character of a molecule by looking at the periodic table. The farther away the elements are, the greater the ionic character and vice versa for covalent character; the closer the elements, the greater the ionic character.

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