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Oxidation States for Metal Cations
Group
Oxidation States for Non-metal Anions
IA
Always +1 (Li, Na, K, Rb, Cs, Fr)
IVA
Always -4 (C4-) as an anion
IIA
Always +2 (Be, Mg, Ca, Sr, Ba, Ra)
VA
Always -3 (N3-, P3-) as an anion
IIIB
Always +3 (Sc, Y, La)
VIA
Always -2 (O2-, S2-, Se2-, Te2-) as an anion
IVB- Note: this list contains commonly-found oxidation states. Oxidation states not shown exist, but they are less-frequently encountered and therefore not "common." Other oxidation states are commonly encountered for metals in polyatomic ions, where the metal is not the cation of a compound. When naming compounds, the oxidation state of the metal cation is given only if the metal has more than one common oxidation state (e.g., Iron(III) or Iron(II) in the name). If you're seeing this message, it means we're having trouble loading external resources on our website. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. Video transcript- [Instructor] Let's get some practice now thinking about how ions typically form, how they might form compounds and how we name those compounds. So let's start with something in group one. In this first column, this first column is often known as alkali metals. So let's start with potassium. K is the symbol for potassium. Now things in group one here, one way to think about is their outermost shell has one electron in it. So they wouldn't mind losing that electron. So when they ionize, they tend to lose an electron and become a cation, a positive ion. And so let's look at a situation where I have some potassium that has been ionized. I could write it just like this, we've seen that in previous videos and we can refer to this just as a potassium ion, we could refer to this as potassium one plus. We could refer to this as a potassium cation. Now let's go on to the other side of the periodic table. Things that would really love to grab an electron. So things in group, in the halides, which is this column right over here. So these are the halides. They have seven electrons in their outermost shell. They would love to have eight, so they tend to be really good at grabbing electrons. And so let's say we're dealing with chlorine, and chlorine is able to ionize. So it's able to grab an electron. When chlorine grabs an electron, it will be a negatively charged ion, so you could write it as Chlorine one minus, but the way that we generally refer to an anion, a negatively charged ion, instead of just calling this the chlorine anion, we would call this chloride. So this we would refer to as Chloride. Now as you can imagine with potassium having a positive one charge or one plus charge and this having a negative charge, they're going to be attracted to each other and they can actually form an ionic compound. The ionic compound they would form, we would write as, you'd write your positive ion first and then you would write your negative ion. And this right over here would be described as potassium chloride. Let me write that down. Potassium, potassium chloride. Now you might be saying, "Well, I just," Let me rewrite the whole thing. So you know the chloride part, you say okay, this is going to be an anion because instead of writing chlorine which is the name of this element, I wrote this IDE at the end to say, "Hey, this is an anion," so I know that this is the chlorine anion, this is chloride, why didn't I do something similar for potassium? Well, the way the convention works is if someone says potassium chloride, you know you're dealing with an ionic compound and if the chlorine has a negative one charge, an ionic compound, the whole thing is gonna be neutral. So if this one over here is one minus, then you know this over here is just one-for-one, this is going to be one plus so you know that you're dealing with a potassium cation and you could say and a chloride ion or a chlorine anion. You could refer to it various ways, but this is potassium chloride. You have a positively charged potassium and you have a negatively charged chlorine, which we would call a chloride. In the next few videos I'll do many, many more examples of this and ones that will be a little bit more complicated. Which of the following is the correct name for F?Having a chemical formula of F−, fluoride ion is the simplest inorganic, monatomic anion of fluorine with basic properties.
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4.3Related Element.. How do you properly name an ion?In the simpler, more modern approach, called the Stock system, an ion's positive charge is indicated by a roman numeral in parentheses after the element name, followed by the word ion. Thus, Fe2+ is called the iron(II) ion, while Fe3+ is called the iron(III) ion.
Which compound contains mn3+ ion?Manganese(3+) | Mn+3 - PubChem.
What types of ions have names ending in IDE?The names of the hydroxide (OH-), cyanide (CN-), and peroxide (O22-) ions, for example, have the -ide ending because they were once thought to be monatomic ions. The bone and tooth enamel in your body contain ionic compounds such as calcium phosphate and hydroxyapatite.
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In which of the following are the symbol and name for the ion given correctly
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