Learn how to name monatomic ions andionic compounds containing monatomic ions, predict charges for monatomic ions, andunderstand formulas.
Log in Abhishek Kumar 8 years agoPosted 8 years ago. Direct link to Abhishek Kumar's post “Can you provide me an exa...” Can you provide me an example of ionic compound where Hydrogen is the anion or the negatively charged section of the bond. Thanks • (43 votes) Aryan Goel 6 years agoPosted 6 years ago. Direct link to Aryan Goel's post “In a chemical reaction wi...” In a chemical reaction with an alkali metal and hydrogen, the hydrogen atom will always form the anion as hydrogen can from both cations and anions, but alkali metals can only form cations. In this case, the alkali metal gets a 1+ charge, and the hydrogen gets a 1- charge. (38 votes) Nell Waldren 9 years agoPosted 9 years ago. Direct link to Nell Waldren's post “When we say "Transition m...” When we say "Transition metals", what does "transition" mean? • (38 votes) Noah Zilberberg 8 years agoPosted 8 years ago. Direct link to Noah Zilberberg's post “it's because they "have a...” it's because they "have an incomplete inner electron shell and that serve as transitional links between the most and the least electropositive in a series of elements" Mohammed Taqee 8 years agoPosted 8 years ago. Direct link to Mohammed Taqee's post “In Example 3, PbCl4 is Le...” In Example 3, PbCl4 is Lead (IV) Chloride, doesn’t Cl4 refer to tetrachloride? • (19 votes) Ernest Zinck 8 years agoPosted 8 years ago. Direct link to Ernest Zinck's post “Yes. For example, CCl₄ is...” Yes. For example, CCl₄ is carbon tetrachloride. But that's how you name covalent compounds. (73 votes) Christopher Lucas 8 years agoPosted 8 years ago. Direct link to Christopher Lucas's post “Hydrogen's preference to ...” Hydrogen's preference to form ions will ultimately be related to the energy associated with the 1s shell. Although, I thought an atom's stability decreased upon forming ions, and so, an atom of hydrogen, with no external influences ( no transfer of energy between it and anything else ) could not form an ion. Energy would first have to be given too, or taken away from hydrogen before any electronic reactions could take place. Returning swiftly back to why hydrogen can easily form ions, well, for the cation, I think it's because only a small amount of energy is needed to remove the electron. A little bit of research led to me ionization energies! 1,312 Joules of energy needed to remove hydrogen's electron. I'm not sure what I can relate that number too though, is it a lot? For the anion, I think it's because the nucleus has a strong positive charge, which will attract any passing electrons. That's my answer, and it could all be complete nonsense. • (32 votes) djones0606 4 years agoPosted 4 years ago. Direct link to djones0606's post “For reference, it would t...” For reference, it would take 1 liter of water that is at 0 degrees celsius and at 1 atm pressure 418100 joules to boil. Also, there are 4184 joules in a kilocalorie. (7 votes) C00L MAN DJ 6 years agoPosted 6 years ago. Direct link to C00L MAN DJ's post “When hydrogen loses an el...” When hydrogen loses an electron won't it just be a proton and no longer hydrogen? Sorry if it's a stupid question • (15 votes) Davin V Jones 6 years agoPosted 6 years ago. Direct link to Davin V Jones's post “A single proton is still ...” A single proton is still atomically hydrogen. It retains all the chemical properties. (29 votes) harsh shah 8 years agoPosted 8 years ago. Direct link to harsh shah's post “hydrogen exists as H2 or ...” hydrogen exists as H2 or H in the atmosphere? • (11 votes) sedspqr 8 years agoPosted 8 years ago. Direct link to sedspqr's post “In particular, there are ...” In particular, there are 7 elements that are called "diatomic," meaning that on their own they will almost always form molecules consisting of two atoms of that element. They are: bromine, iodine, nitrogen, chlorine, hydrogen, oxygen, and fluorine. You can remember them by the acronym Br-I-N-Cl-H-O-F (pronounced "brinkle-hoff"). (21 votes) LILZO 8 years agoPosted 8 years ago. Direct link to LILZO's post “So if you had a magnet at...” So if you had a magnet attached to some compound, could you change the overall charge of the compound?if so, wouldn't it also be true that you could magnetically remove electrons and/or protons, thus changing the compound itself? • (11 votes) Matt B 8 years agoPosted 8 years ago. Direct link to Matt B's post “The magnet will not "stea...” The magnet will not "steal" the electrons from other metallic items. The magnet will simply force all the electrons in the metal to one side (non-permanently) which is how they attract each other. Once you remove the magnet, all electrons go back to where they came from and the metal compound neutral again. (25 votes) stvanbod 8 months agoPosted 8 months ago. Direct link to stvanbod's post “This article needs furthe...” This article needs further work. Words are used without first having had a definition or explanation in the article or earlier in Unit 1. The first is monatomic. Where is monatomic defined in this article or in Unit 1. We are being asked to 'Remember that periodic groups refer to columns on the periodic table, whereas rows are known as periods' when this concept has also not been initially defined in this article or in Unit 1. Octet is used without definition, followed by valence also being used without definition. Where in Unit 1 is Octet and Valence given definition. IUPAC group number is also not described, it is simply used, without definition or prior description. Electron configuration is used as part of a hidden explanation as an answer, yet the article or Unit 1 does not explain what an electron configuration is. Where in Unit 1 is s, p, d, f and shell and subshell defined prior to this article. The use of magnitude is used without being introduced followed by a statement that isn't well described, 'The magnitude of the charge is equal to the number of electrons lost, which is equal to the number of valence electrons in the neutral atom.' Aluminum is in group 13, or IIIA is stated when no introduction has been provided to what IIIA means. What does IIIA mean? The problems are then for ionic compounds that are not monoatomic. Please re-write this article to improve it to explain concepts before they are used in answers or taken for granted as prior knowledge when they have not first been defined in Unit 1. • (14 votes) Karol Zamojcin 9 years agoPosted 9 years ago. Direct link to Karol Zamojcin's post “Hello there, in Example...” Hello there, in Example 2: Finding the name from the chemical formula or is "just" magnesium a good answer afteral ?l. • (5 votes) Esther Dickey 9 years agoPosted 9 years ago. Direct link to Esther Dickey's post “When we name an ionic com...” When we name an ionic compound, the charge is not included unless that element forms multiple ions. For example, if I have Fe2O3, I have to call it iron(III) oxide because iron also forms an ion with a 2+ charge. (14 votes) dmmendoza2 4 years agoPosted 4 years ago. Direct link to dmmendoza2's post “what does the roman numer...” what does the roman numerals mean? like Cobalt(III) sulfide, or lead (IV) • (7 votes)Want to join the conversation?
Lithium hydride (LiH)
Sodium hydride (NaH)
Potassium hydride (KH)
Rubidium hydride (RbH)
Caesium hydride (CsH)
Francium hydride (FrH)
The name of an ionic compound is: name of metal ion + name of anion ( with no multiplying prefix).
So, PbCl₄ is lead(IV) chloride.
Humans require anywhere from 1600-3000 calories to function.
"Therefore, the name for the compound is magnesium phosphide."
Shouldnt it be magnesium ion phosphide or magnesium 2-plus phosphide?.. Im really new to this and it sounds weird but earlier in article its said that : "While we often refer to an ion such as Mg2+ as "magnesium 2-plus", we could also simply say "magnesium ion," "
Magnesium only forms the ion with a 2+ charge, so you don't need to include it.
