Write the Lewis symbols for each of the following ions: (a)...

Key Concepts

Octet Rule

The octet rule is a chemical principle that atoms tend to gain, lose, or share electrons in order to have a full set of eight valence electrons, resembling the electron configuration of a noble gas. This rule is fundamental to understanding why atoms form ions or covalent bonds and is implicitly reflected in the Lewis symbols representing ions.

Ionic Charges

Ionic charges result from the gain or loss of electrons by an atom, leading to the formation of ions. When writing Lewis symbols for ions, additional electrons are added for negatively charged ions (anions) and electrons are removed for positively charged ions (cations), with the net charge indicated as a superscript.

Valence Electrons

Valence electrons are the outermost electrons of an atom that participate in bonding and chemical reactions. In Lewis symbols, the number of dots around the symbol represents the count of valence electrons, which is crucial for determining the chemical behavior of both neutral atoms and ions.

Lewis Dot Structures

Lewis dot structures are diagrams that show the valence electrons of an atom as dots arranged around the element’s chemical symbol. They provide a simple visual representation of an atom’s bonding capabilities and can be adjusted to account for ions by adding or removing electrons while displaying the overall charge.

Transcript

00:01 Okay, so today we're going to be drawing the lewis symbols for a couple ions.

00:06 So the first one we have is as 3 minus, which is going to be arsenic with three more electrons.

00:16 So first off, we have to draw a different color real quick.

00:21 First off we draw the chemical symbol for it, so as.

00:25 And then going around it, we have to add the amount of electrons.

00:32 That it has.

00:33 And since it's gained three more, it's going to have a full set.

00:37 So you have to move around in a clockwise motion, and then that will be number one.

00:47 All right, moving to number two, we have i minus, so iodine minus.

00:55 So you're going to the i for it.

00:59 And iodine is going to be right here and then with one more added electron that's going to also have a full set like as if it were xenon next moving on to the next one c we have b e 2 plus um so virillium is right here and since it has lost two electrons it has no valence electrons so it's actually just going to be be e there uh then moving on to d we have to minus so we're gonna have the symbol for oxygen and then oxygen is right here adding two more electrons puts it here meaning that it'll have a full set so it will have all eight all right and then e we have gallium or ga a 3 plus so first we'll write gaa and then we have to look at how gallium is right here and then it's going to lose three electrons.

02:17 So instead of actually going into the d -orbital here, we have to think about how its electron configuration, it would lose all of its fourth energy level shells first.

02:29 So it's going to lose this one's electron, this one's electron, and then this one's electron...

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