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Charge might be misleading sometimes and not show the whole picture. Instead look at whether the compound is electron deficient or rich. If it requires electrons to fulfill an octet then it is an Lewis acid or electron acceptor. If it can provide an electron then it is an Lewis base. Hope this helps!
Lewis acids and bases relate to accepting and gaining electrons to form covalent bonds. The Lewis base, such as an OH- ion will donate an electron to the Lewis acid, such as an H+, which accepts the electron. Hope this helps!
Hi! Lewis acids accept an electron pair and lewis bases donate an electron pair. So molecules that have a positive charge are more likely to be lewis acids and molecules with a negative charge are more likely to be lewis bases.
I find it helpful to think of Lewis acids as the electron deficient compound that accepts electrons whereas the Lewis base in a reaction is the compound or molecule that provides electrons (donates) to form a coordinate covalent bond.
I remember the Lewis acids with the "a" in acids and "a" in accept as well. However, if that doesn't help you, you can always determine which is a Lewis acid and base by drawing the Lewis structures to see which has a lone pair of electrons. The one that has a lone pair of electrons will be the base since it can donate these electrons. The acid is the one that can accept more electrons to complete its octet or the number of electrons it needs to satisfy the amount of valence electrons in the structure.
Hi! Lewis acid always accepts an electron pair while Lewis base typically donates an electron pair and will have lone-pair electrons. This is also shown on the periodic table that the left column elements always donates e while close to the right column accept e.
A good way to determine whether a compound is an acid or a base is by remembering that lewis acids accept electrons. Lewis bases donate electrons. Charge isn't as important in determining whether a compound is an acid or a base. It is more useful to determine whether each compound is electron deficient or not instead.
Lewis acids accept electrons while lewis bases donate electrons. The acids will usually have a positive charge and want electrons to neutralize the charge. Lewis bases will usually be negatively charged and willing to donate the extra electrons.
I usually look at the formula. Acids are electron acceptors. So if you are to look at charges, H+ is what it will break into water. If it starts with H, it's most likely an acid because it will be the electron pair receptor. Bases are electron donors and in water will usually break into OH-. Bases might have an OH in them as an electron pair donor. So if you can see the charges in them, thats good but sometimes it's easier to simplify it. Another way is to look at the structures and identify which molecule would be donating an electron or H+ and which would accept that. Hopefully that will help you figure out which is which!
Kandyce Lance 2L wrote:So Lewis and Bronsted acids/bases are only opposites or different from each other in the context we are defining a molecule?
In terms of the bronsted definition being focused on protons instead of electrons?
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