Ionic Character  [ENDORSED]

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yasminea 3L
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Joined: Wed Sep 21, 2016 2:56 pm

Ionic Character

Postby yasminea 3L » Thu Oct 27, 2016 6:45 pm

For each pair, determine which compound has bonds with greater ionic character. a) PH₃ or NH₃; b) SO₂ or NO₂; c) SF₆ or IF₅.

Matthew_Vargas_2G
Posts: 18
Joined: Fri Jul 22, 2016 3:00 am

Re: Ionic Character

Postby Matthew_Vargas_2G » Thu Oct 27, 2016 6:51 pm

For each pair, determine which compound has bonds with greater ionic character. a) PH₃ or NH₃; b) SO₂ or NO₂; c) SF₆ or IF₅.

In this case, since each one shares a similar set of atoms (i.e. H3 and 02 and F6) you would look at the placement of the other atom on the periodic table. The larger the size of the compound, the less ionic characteristics it will have because it will be less soluble. In other words, the electronegativity and atomic radius will affect the ionic character for these compounds. Between P and N for a, N has a smaller atomic radius and a higher electronegativity, which gives this compound a greater ionic character. Following this thought process, you can answer the other questions :) just remember that electronegativity is going to the right and up and atomic radius increases going to the left and down of the periodic table!
Last edited by Matthew_Vargas_2G on Thu Oct 27, 2016 6:58 pm, edited 1 time in total.

Alicia_Miller_3F
Posts: 10
Joined: Wed Sep 21, 2016 2:58 pm

Re: Ionic Character  [ENDORSED]

Postby Alicia_Miller_3F » Thu Oct 27, 2016 6:54 pm

Hi,
Look at the difference in how far each atom in the pairs are placed from each other and the pair in which the atoms are farther from each other, the ionic character will be greater due to a greater difference in electronegativity. For example, the electronegativity difference between P and H is greater than the difference between N and H so PH3 would have greater ionic character. You can look up specific values for electronegativity if the atoms are too close to tell. Also, keep in mind that electronegativity increases as you move toward the top right of the period table and decreases as you move toward the bottom left of the table.
Hope this helped! (:


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