Oh I know what electronegativity means and what polar means but how would you order the compounds from most to least covalent and most to least ionic without the use of google
Oh I know what electronegativity means and what polar means but how would you order the compounds from most to least covalent and most to least ionic without the use of google
It's not perfect but you can consider the difference in electronegativity between the two elements (assuming its a simple example!). The greater the difference the more ionic it is likely to be.
Oh I know what electronegativity means and what polar means but how would you order the compounds from most to least covalent and most to least ionic without the use of google
Is this for Gcse or Alevel chemistry? You should not be wortied about using google or youtube. They have some quality stuff that is sometimes better than your school of college notes! But to deal with your problem you first need to list the compound you are talking about and identify each element in them. Then look at the electropositivity and electronegativity of the elements. e.g Group 1 metals - very electropositive. group7 elements such as fluorine -very electronegative. So, for example, Na Fluoride very ionic compared to Iron chloride for example. What is your list?
Alevel chemistry. So I have these ionic compounds KF Na2O Al2O3 CrBr And then the covalent compounds are PH3 NO2 SiO2 and Br2 How would you know for each of the two groups of ionic and Covalent t compounds, how they’re ordered from strongest to weakest?
Alevel chemistry. So I have these ionic compounds KF Na2O Al2O3 CrBr And then the covalent compounds are PH3 NO2 SiO2 and Br2 How would you know for each of the two groups of ionic and Covalent t compounds, how they’re ordered from strongest to weakest?
Your full understanding of the strength of electrostatic attraction between atoms and also electron sharing and polarity makes this an easy task to complete. KF is the most ionic!
Your full understanding of the strength of electrostatic attraction between atoms and also electron sharing and polarity makes this an easy task to complete. KF is the most ionic!
But why? How do you order them? What do you look at? Do you add the electronegativities up? What do you do?
But why? How do you order them? What do you look at? Do you add the electronegativities up? What do you do?
Please don't listen to those who are telling you how "easy" it should be. We all struggle with something; they're patronising you.
For instance, with potassium fluoride, find the e- neg values of both K and F.
Then subtract the higher e- neg value from the lower e- neg value. Since the differences are very high, the compound will be ionic. It's ionic b/c it e- neg differenced are so large that fluorine can remove potassium's outer e-.
here's an excerpt from this website:
" Ionic bonding is shown at the point where the two elements have the largest difference in electronegativity, as in CsF. Covalent bonding is shown where the elements have low or no difference in electronegativity but a high average electronegativity, as in F2. Metallic bonding is shown where the elements have low or no difference in electronegativity and a low average electronegativity, as in Cs. These relationships can be used to predict the type of bonding likely to be exhibited by any compound based on the elements involved."
Please don't listen to those who are telling you how "easy" it should be. We all struggle with something; they're patronising you.
For instance, with potassium fluoride, find the e- neg values of both K and F.
Then subtract the higher e- neg value from the lower e- neg value. Since the differences are very high, the compound will be ionic. It's ionic b/c it e- neg differenced are so large that fluorine can remove potassium's outer e-.
here's an excerpt from this website:
" Ionic bonding is shown at the point where the two elements have the largest difference in electronegativity, as in CsF. Covalent bonding is shown where the elements have low or no difference in electronegativity but a high average electronegativity, as in F2. Metallic bonding is shown where the elements have low or no difference in electronegativity and a low average electronegativity, as in Cs. These relationships can be used to predict the type of bonding likely to be exhibited by any compound based on the elements involved."
Please don't listen to those who are telling you how "easy" it should be. We all struggle with something; they're patronising you.
For instance, with potassium fluoride, find the e- neg values of both K and F.
Then subtract the higher e- neg value from the lower e- neg value. Since the differences are very high, the compound will be ionic. It's ionic b/c it e- neg differenced are so large that fluorine can remove potassium's outer e-.
here's an excerpt from this website:
" Ionic bonding is shown at the point where the two elements have the largest difference in electronegativity, as in CsF. Covalent bonding is shown where the elements have low or no difference in electronegativity but a high average electronegativity, as in F2. Metallic bonding is shown where the elements have low or no difference in electronegativity and a low average electronegativity, as in Cs. These relationships can be used to predict the type of bonding likely to be exhibited by any compound based on the elements involved."
That's not how it works. You can't bonds on how covalent or ionic they are. They either are or aren't depending on the compound. Like say you have a chemical reaction of Sodium+Chlorine----->Sodium Chloride it's obviously an alkali metal+a halogen so a ionic bond. The ionic bond formed is no more ionic than say Potassium Fluoride or Lithium Bromide. The same for covalent bonds a hydrogen molecule doesn't have a more covalent bond than Hydrogen Chloride or Methane or Water. They are all covalent bonds.
Oh I know what electronegativity means and what polar means but how would you order the compounds from most to least covalent and most to least ionic without the use of google
You can't, it's not how it works. Like there is different strengths attraction between the nucleus and the electron in question but that's to do with reactivity and displacement not how "covalent" a bond is
That's not how it works. You can't bonds on how covalent or ionic they are. They either are or aren't depending on the compound. Like say you have a chemical reaction of Sodium+Chlorine----->Sodium Chloride it's obviously an alkali metal+a halogen so a ionic bond. The ionic bond formed is no more ionic than say Potassium Fluoride or Lithium Bromide. The same for covalent bonds a hydrogen molecule doesn't have a more covalent bond than Hydrogen Chloride or Methane or Water. They are all covalent bonds.
Uh no as I wanted to know how to find out what is more covalent and less covalent in A group if covalent compounds and what is more ionic and less ionic in a group of ionic compounds