ionic character

Moderators: Chem_Mod, Chem_Admin

Emely Reyna 1F
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

ionic character

Postby Emely Reyna 1F » Sun May 20, 2018 10:22 pm

One of the UA's workshop worksheets included a question that asked to determine which compound has greater ionic character, I was a bit confused on what to do for this question, does it mean which bond is ionic bond is stronger?

Danielle Sumilang - 1F
Posts: 31
Joined: Fri Apr 06, 2018 11:05 am

Re: ionic character

Postby Danielle Sumilang - 1F » Sun May 20, 2018 10:24 pm

Hello!

You're pretty much right. If a compound has a greater ionic character, then the ionic bond between the two elements is stronger than the elements in the other compound. A larger ionic character is caused by a great difference in electronegativity. One element in the compound is more electronegative than the other element.

Vivian Gonzalez 1A
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am

Re: ionic character

Postby Vivian Gonzalez 1A » Sun May 20, 2018 10:27 pm

I am also confused as to what the term covalent character means or is referring to. Can someone please explain?

Emely Reyna 1F
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

Re: ionic character

Postby Emely Reyna 1F » Sun May 20, 2018 10:27 pm

Thank you! This was really helpful!!! How would I be able to determine which element of the compound is more electronegative?

Emely Reyna 1F
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

Re: ionic character

Postby Emely Reyna 1F » Sun May 20, 2018 10:30 pm

Vivian Gonzalez 1A wrote:I am also confused as to what the term covalent character means or is referring to. Can someone please explain?



I think covalent character means the same thing as ionic character. One compound would have a greater covalent character if the difference in electronegativity is greater

Danielle Sumilang - 1F
Posts: 31
Joined: Fri Apr 06, 2018 11:05 am

Re: ionic character

Postby Danielle Sumilang - 1F » Sun May 20, 2018 10:32 pm

Emely Reyna 1F wrote:Thank you! This was really helpful!!! How would I be able to determine which element of the compound is more electronegative?


Hello!

You can determine if the element is more electronegative by using the periodic table trends we learned before the midterm. Electronegativity increases as you move from left to right in a row and from bottom to the top in a period.

Alicia Beebe
Posts: 37
Joined: Fri Apr 06, 2018 11:01 am

Re: ionic character

Postby Alicia Beebe » Sun May 20, 2018 10:35 pm

So every ionic bond has some covalent character. The bigger difference in electronegativity will always result in more ionic character, because the one with greater electronegativity will pull on the electrons so much that they will hardly be shared at all. As far as finding electronegativity, it increases as you go up and to the right on the periodic table, with F, O, N, Cl being the most electronegative, and specifically F having the highest electronegativity. There are quantitative values, but electronegativity is used more for comparison than anything else from what I understand

Ashley Martinez 1G
Posts: 26
Joined: Fri Apr 06, 2018 11:03 am

Re: ionic character

Postby Ashley Martinez 1G » Sun May 20, 2018 10:41 pm

The textbook mentions that an electronegative difference of ~2 means ionic character and electronegative differences smaller than ~1.5 are regarded as covalent. It then goes on to say there's a few exceptions to these guidelines. How do we determine these exceptions? Is it something we memorize? Thanks!

Chem_Mod
Posts: 18401
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: ionic character

Postby Chem_Mod » Mon May 21, 2018 11:38 pm

Covalent refers to "sharing" of electrons. In an ionic bond, the electron is primarily associated with one atom while the other lacks the electron.

BriannaParrington-1B
Posts: 29
Joined: Fri Apr 06, 2018 11:04 am

Re: ionic character

Postby BriannaParrington-1B » Tue May 22, 2018 4:40 pm

If the trend of electronegativity is highest to the upper right of the periodic table, does that mean that electronegativity is the least in the bottom left corner of the periodic table? Is there a specific trend we are supposed to know besides the highest electronegativity being in the upper right of the periodic table such as fluorine, chlorine, etc.?

Erin Li 1K
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am

Re: ionic character

Postby Erin Li 1K » Wed May 23, 2018 1:18 am

greater ionic character means greater difference in electronegativity


Return to “Ionic & Covalent Bonds”

Who is online

Users browsing this forum: No registered users and 0 guests