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Monatomic ion

A monatomic ion is an ion consisting of one or more atoms of a single element (unlike a polyatomic ion, which consists of more than one element in one ion). A type Ibinary ionic compound contains a metal (cation) that forms only one type of ion. A type II ionic compound contains a metal that forms more than one type of ion, i.e., ions with different charges.

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Question:practical inorganic chemistry

Answers:Acid radical: Acid radical is an anion left after removal of hydrogen atoms from an acid. Anions : Anions are atoms or groups of atoms that have gained electrons. Having more negatively charged electrons than positively charged protons, they are negatively charged. The atoms that form ions most easily are the Group 17 (or VII) atoms, also called the halides: F, Cl, Br and I. All these form anions with a -1 charge. O, S, N and P also form anions, carrying charges of -2 (oxygen and sulfur) or -3 (N and P). Most anions are composed from multiple atoms, and are called polyatomic ions (polyatomic = many atoms). Polyatomic ions are usually built around a core atom which is more often than not a non-metal, but some metals, notably manganese and chromium, form polyatomic ions as well. In most polyatomic ions, these atoms combine with oxygen and sometimes with hydrogen as well. As with every other generalisation, there are exceptions. For example, SCN-, the thiocyanate ion, is polyatomic, but has neither oxygen nor hydrogen. (Worse, NH4+ is polyatomic, but is a cation!) But back to the story. The negative charge (the extra electron) in the polyatomic ion is shared around the entire ion. It is not associated with a particular nucleus in the ion, specifically not with the nucleus to which oxygen and/or hydrogen are attached. This is true whether the charge is single or multiple. COMMON NEGATIVE IONS (ANIONS) acetate CH3COO- nitride N3- bromide Br- nitrite NO2- carbonate CO32- oxalate C2O42- hydrogen carbonate HCO3- oxide O2- chlorate ClO3- permanganate MnO4- perchlorate ClO4- phosphide P3- chloride Cl- phosphate PO43- chlorite ClO2- (mono)hydrogen phosphate HPO42- hypochlorite ClO- dihydrogen phosphate H2PO4- chromate CrO42- sulphate SO42- dichromate Cr2O72- hydrogen sulphate HSO4- cyanide CN- sulphide S2- fluoride F- hydrogen sulphide HS- hydride H- sulphite SO32- hydroxide OH- hydrogen sulphite HSO3- iodide I- thiocyanate SCN- nitrate NO3- thiosulphate S2O32- Note that, with the exceptions of hydroxide (OH) and cyanide (CN-), all the names ending in -ide are monatomic. The rest are -ates or -ites. In the days of yore, chemists gathered samples of anions and then tried to give them some order. The rules they came up with went like this: The most frequently occurring version of a polyatomic ion got the name -ate. The most frequently occurring anion of chlorine and oxygen is ClO3-. It was given the name chlorate. One more oxygen? Put a per- on the front. ClO4- is perchlorate. (Per is from the Greek hyper for too much.) One less oxygen? Change the name to -ite. ClO2- is chlorite. Two less oxygens? Put a hypo- on the front. ClO- is hypochlorite. (Hypo is from the Greek for too little or not enough.) So from above discussion we see that all acid radicals are anions but all anions are not acid radicals. Basic radical : The basic radical is the cation left after removal of OH or other alkaline group from the bases. Cations : Cations are atoms that have lost an electron to become positively charged. Sodium has one valence electron, one electron in its outer energy level, so tends to lose one electron, and to become an ion with a +1 charge. The same could be observed for lithium, potassium, rubidium, caesium and francium. Magnesium, along with the other elements in group 2 of the periodic table, has two valence electrons, so tends to become an ion with a +2 charge. Aluminium tends to become +3. What about the transition metals like lead, copper, tin and manganese? Electrons in the transition elements are packed in a way that, generally, places the additional electrons inside the outer energy level. Iron has six more electrons than calcium, but the additional electrons have less energy than the two on the outer. The transition elements tend to have either one or two loosely held (valence) electrons. The six electrons present in iron but absent in calcium are held much less loosely than those in the next level down, but more tightly than those in the outer level. Having removed two electrons from both iron and calcium, removing a third electron would be much, much, much harder from calcium than from iron, since calcium's next electron is both more tightly held (a lower energy level) and in a complete shell. Because of this ambiguity in the transition elements, it is sometimes hard to predict the charge for their corresponding cation. Copper, for example, frequently loses two electrons (Cu2+), but copper ions with a +1 charge (Cu+) are also well known. Tin most often looses two (Sn2+), but frequently loses four (Sn4+). Iron can lose two or three. Manganese? So many choices you don't want to know. For our purposes you will be able to tell which ion you are dealing with by the context it occurs in. You may be given the name of the ion. Sn2+ is named tin(II) [pronounced "tin-two"]. Pb4+ is named lead(IV). You may be given a formula including the ion. FeCl2 is called iron(II) chloride [iron two chloride], containing Fe2+. (Each of the chlorides have accepted one electron, similar to other Group VII elements.) FeCl3 is called iron(III) chloride, containing Fe3+. Thus all basic radicals are cations but all cations are not basic radicals.

Question:I have to explain why cations give off different colours when burnt in a flame. I have started but I am not sure what I am saying is correct. Please correct this and add to this with any details. Ive stopped at the bit: "How we work out the distance through the colour of the flame when burnt." What is the spectrum thing called, I forgot? Cations have a positive charge. Examples of cations include: Potassium, Lithium and Copper. Cations are usually metals. Negative ions are called "anions". Anions tend to be non metals. Metals usually form cations because they are less electronegative than nonmetals. Cations are formed when an atom loses electrons, while anions are formed when an atom gains electrons. Among the atoms, the alkali metals (Group 1) and alkaline-earth metals (Group 2) are the most reactive metals, having one and two valence electrons, respectively. Therefore, metals lose that electrons and form cations. When you heat the atoms and therefore the elections, they become excited and jump to outside rings of the atom. This causes the metal to change colour when burnt in a flame. We know and can work out the colour by the distance the electron jumps. This is measured with the Thanks for any answers.

Answers:What you're saying is basically correct but I'd change a little the language, the way you'll talk about the different colors and emissions. Let me add something: A flame is normally an exothermic reaction. The heat released, f. ex., from the combustion of butane or propane is enough to excite the electrons in an atom or ion, from its original energy level (orbital) to a higher energy level (another orbital). After excitation, many of the electrons come back down to their original electronic orbitals, or to other empty orbitals, and in this process they emit light. But the fundamental point that you should make is the following: The light is characteristics of each metal because the electrons in their electronic shells have different energy! These energy are very specific for each atom. Therefore, these emissions are like "finger prints", from these it is possible to identify which atom has emitted it. In other words, the energy of the electrons 1s in H are quite different from the energy of the 3s electrons in sodium. At the same time, the energy of the other electronic energy levels of H and Na are also quite different, f. ex., the energy of the 4p or 5p (these are empty orbitals in both of them). The light emitted will be related to the energy difference between the energy levels involved. So, the wavelenght (L) of emission by electrons of these atoms, from the same orbitals (say, 3p to 2s) would be: Del E [H (3p-2s)] = E [H (3p)] - E[H(2s)] = (h x c) / L(H) Del E [Na(3p-2s)] = E [Na (3p)] - E [Na(2s)] = (h x c) / L(Na) and the Ls would be different because the Del E would be different for each atom. The fantastic thing in all this, to me, is the fact that we can determine what is the composition of stars, just looking (in details) at the light they emit! Also, remember, things are more complicated than they look: there is also ionization and even chemical reactions in the flames, at the same time ...very busy, very confusing flames are .. Hope you got the idea. Check also the references.

Question:I'm just trying to study and there's a question in the back of the books that says: An ionic bond is formed between a cation A+ and an anion B-. How would the energy of the ionic bond be affected by the following changes? a) doubling the Radius of A+ b) Tripling the charge on A+ c) doubling the charges on A+ d) decreasing the radii of A+ and B- to half their original values. I found an equation to help me but i think i'm still doing it wrong. My test is tomorrow so i'd really like to learn how to do this. Thanks in advance

Answers:a) Doubling the radius will spread the charge of the cation over a larger volume. So, the bond will be weaker. b) Increasing the charge will attract the anions more strongly, making a stronger bond. c) Doubling the charge will have the same effect as b), but just not as much. d) Decreasing the radius will concentrate the charges and will allow the atoms to approach more closely, increasing the strength of the ionic bond.

Question:1. What's the difference between cation and anion hydrolysis? 2. How can you identify the acid and base from the salt that was formed? 3. How do you know if the solutions form buffers? 4. How do you identify solutions as acidic, basic, or neutral- based on the compound's molarity, such as 0.10 M[molarity] Ba(OH)2? Thank you very much!

Answers:2) In a neutralization reaction, the produced salt's cation is always from the base and the anion of the salt is always from the acid. ex. NH4Cl: NH4+ is from the weak base ammonia and the Cl- is from the strong acid Hydrchloric acid. 3) Any time you have a 1) weak acid and a 2) salt that contains the anion of the weak acid (conjugate base), by definition you'll have a buffer. ex. acetic acid (weak acid) and sodium acetate (acetate ion-conjugate base). Also if you have a ) weak base and a 2) salt that contains the cation of the weak base (conjugate acid), by definition you'll have a buffer. ex. ammonia (weak base) and ammonium chloride (ammonium ion-conjugate acid)