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Chemistry Help!

BuckGup
By BuckGup
in Off Topic
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How do you determine if a compound is ionic or covalent? 

HCl

NaCl

NaF

 

▓ƆԀ▓ S▓₱▓Ɇ▓c▓s▓: i7 6ʇɥפᴉƎ00K (4.4ghz), Asus DeLuxe X99A II, GT҉X҉1҉0҉8҉0 Zotac Amp ExTrꍟꎭe),Si6F4Gb D???????r PlatinUm, EVGA G2 Sǝʌǝᘉ5ᙣᙍᖇᓎᙎᗅᖶt, Phanteks Enthoo Primo, 3TB WD Black, 500gb 850 Evo, H100iGeeTeeX, Windows 10, K70 R̸̢̡̭͍͕̱̭̟̩̀̀̃́̃͒̈́̈́͑̑́̆͘͜ͅG̶̦̬͊́B̸͈̝̖͗̈́, G502, HyperX Cloud 2s, Asus MX34. פN∩SW∀S 960 EVO

Just keeping this here as a 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Ionic has something to do with metals and nonmetals, covalent is nonmetals to nonmetals I belive.

 

That was afew months ago we learned

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By the colors

jk

idk its been a year

I'm talking like electronegative and Lewis Structure

▓ƆԀ▓ S▓₱▓Ɇ▓c▓s▓: i7 6ʇɥפᴉƎ00K (4.4ghz), Asus DeLuxe X99A II, GT҉X҉1҉0҉8҉0 Zotac Amp ExTrꍟꎭe),Si6F4Gb D???????r PlatinUm, EVGA G2 Sǝʌǝᘉ5ᙣᙍᖇᓎᙎᗅᖶt, Phanteks Enthoo Primo, 3TB WD Black, 500gb 850 Evo, H100iGeeTeeX, Windows 10, K70 R̸̢̡̭͍͕̱̭̟̩̀̀̃́̃͒̈́̈́͑̑́̆͘͜ͅG̶̦̬͊́B̸͈̝̖͗̈́, G502, HyperX Cloud 2s, Asus MX34. פN∩SW∀S 960 EVO

Just keeping this here as a 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Posted

i just finished this chapter.

 

I'm talking like electronegative and Lewis Structure

ok i think here's what i remember:

 

2 dots are shared between atoms

4 dots represent a double bond

6 dots represent triple bond.

 

 

elements on the left side have the highest electronegativity, and it increases. fluorine has the highest electronegativity, at 4.0

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Ionic bonds are where an electron is "donated"

Covalent bonds share electrons. Polar covalent bonds form when one atom with a greater electronegativity attracts the electrons of the other atom and forms a bond (H20) forming relationship where there is a slightly negative part and more positive part. Non-polar covalent is equally shared charges and so on...

 

Chem was a while ago...

Don't be lazy and hit up some Kahn academy videos. Great explanations...

https://www.khanacademy.org/science/organic-chemistry/gen-chem-review/electronegativity-polarity/v/electronegativity-and-chemical-bonds 

 

Or Bozeman is even better for science stuff...

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http://phs.psdr3.org/science/chemistry1/Smith/Bonding_files/image003.png

 

This might help. Ionic is when the electronegativities are so different, that one element takes electrons from another. Polar covalent is when the electrons are slightly closer to one atom than another due to electronegativity, but they are still shared (Ex. H2O). Nonpolar covalent is when the electrons are nearly perfectly shared, like in the case of O2.

 

And yes, as others have said, a quick was to tell is covalent will be between two nonmentals, whereas ionic will be between a metal and a nonmetal.

 

In terms of lewis structures, if the structure has an arrow (or something similar) from one electron to the spot where it should be on another atom, that's ionic, since the electron has been moved. Covalent lewis drawings will show a line between two electrons to signify that they are shared.

 

HCl - Covalent (Nonmetal-Nonmetal)

NaCl - Ionic (Metal-Nonmetal)

NaF - Ionic (Metal-Nonmetal)

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Posted

by the charges on the table

 

basically this. 

 

Ionic requires a metal and a non metal
(More correctly two ions)
A covalent requires two (or more) non metals

 
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An Ionic bond is electrostatic attraction between oppositely charged ions. An Ion is a charged particle.

 

In order to obtain a full outer shell, an atom can obtain (essentially) an electron or more than one electron from an atom.

For example:

Lithium is in group 1. It has one electron on it's outer shell so the easiest way to gain a full outer shell is to lose one electron.

Fluorine is in group 7 so needs to gain 1 electron to get a full outer shell.

Lithium in it's reaction with Fluorine will lose an electron, giving it to fluorine. This will create an F- ion and a Li+ ion. The attraction between these is what will cause the ionic bond.

 

Covalent bonds are where atoms share electrons with each other in order to gain the illusive outer shell. Let's use Chlorine as an example.

Chlorine needs a full outer shell and is group 7 so it needs another electron to gain the full outer shell. Another chlorine atom comes along and shared it's 7th electron on it's outside shell with our first chlorine and our first chlorine does the same in return.. These two electrons become a shared pair. The orbits of the electrons change such that they are more involved in each chlorine. Thus, each chlorine behaves as if its got a full outer shell.

 

Metallic bonding is like ionic bonding but there isn't a non-metal to bond with. The metal gives from 1 to all of its electrons on its outside shell to the metallic structure. This creates a positive structure of ions and a negative "sea" of delocalised electrons surrounding it. The attraction between these is metallic bonding.

 

 

This isn't strictly true, but at your level, metallic bonding is between metals, covalent bonding is between non-metals and ionic bonding is between a metal and a non-metal.

As you go on, you'll find that metals can bond covalently and atoms like S can act as centre atoms with the expansion of the octet rule (the concept that atoms can only have 2,8,8,2 in their outer shells).

 

I hope that that helped.

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