Find odd man out chloride nitrate hydride ammonium
If you want to get a feel for chemistry, one way might be to wander through the periodic table, picking one particular type of compound and seeing how things change as you go from element to element. Chlorides, for example, are rabble, as Primo Levi put it memorably. Most other chlorides are nondescript white powders. Pick hydride instead.SEE VIDEO BY TOPIC: How To Make Ammonium Nitrate By Neutralizing HNO3 With NH3
- GENERAL METHODS
- Odd man out. chloride, nitrate, hydride, ammonium.
- MSBSHSE Class 9 Science Chapter 5 Acids, Bases and Salts Solutions
- MSBSHSE Class 9 Science Chapter 5 Acids, Bases and Salts Solutions
- Chloride, nitrate, hydride, ammonium. odd man out.
- Chloride, nitrate,hydride ammonium odd man out
- Wandering Through the Hydrides
Co-ordinate bonding. A covalent bond is formed by two atoms sharing a pair of electrons. The atoms are held together because the electron pair is attracted by both of the nuclei.
In the formation of a simple covalent bond, each atom supplies one electron to the bond - but that doesn't have to be the case. A co-ordinate bond also called a dative covalent bond is a covalent bond a shared pair of electrons in which both electrons come from the same atom.
For the rest of this page, we shall use the term co-ordinate bond - but if you prefer to call it a dative covalent bond, that's not a problem! The reaction between ammonia and hydrogen chloride. If these colourless gases are allowed to mix, a thick white smoke of solid ammonium chloride is formed.
The hydrogen's electron is left behind on the chlorine to form a negative chloride ion. Once the ammonium ion has been formed it is impossible to tell any difference between the dative covalent and the ordinary covalent bonds. Although the electrons are shown differently in the diagram, there is no difference between them in reality. Representing co-ordinate bonds. In simple diagrams, a co-ordinate bond is shown by an arrow. The arrow points from the atom donating the lone pair to the atom accepting it.
Dissolving hydrogen chloride in water to make hydrochloric acid. Something similar happens. In an introductory chemistry course such as GCSE , whenever you have talked about hydrogen ions for example in acids , you have actually been talking about the hydroxonium ion.
A raw hydrogen ion is simply a proton, and is far too reactive to exist on its own in a test tube. When it reacts with something an alkali, for example , the hydrogen ion simply becomes detached from the water molecule again. Note that once the co-ordinate bond has been set up, all the hydrogens attached to the oxygen are exactly equivalent.
When a hydrogen ion breaks away again, it could be any of the three. The reaction between ammonia and boron trifluoride, BF3. If you have recently read the page on covalent bonding, you may remember boron trifluoride as a compound which doesn't have a noble gas structure around the boron atom.
The boron only has 3 pairs of electrons in its bonding level, whereas there would be room for 4 pairs. BF3 is described as being electron deficient.
The lone pair on the nitrogen of an ammonia molecule can be used to overcome that deficiency, and a compound is formed involving a co-ordinate bond. Using lines to represent the bonds, this could be drawn more simply as:. The second diagram shows another way that you might find co-ordinate bonds drawn. The nitrogen end of the bond has become positive because the electron pair has moved away from the nitrogen towards the boron - which has therefore become negative.
We shan't use this method again - it's more confusing than just using an arrow. The structure of aluminium chloride. If it simply contained ions it would have a very high melting and boiling point because of the strong attractions between the positive and negative ions.
The implication is that it when it sublimes at this relatively low temperature, it must be covalent. The dots-and-crosses diagram shows only the outer electrons. AlCl3, like BF3, is electron deficient. There is likely to be a similarity, because aluminium and boron are in the same group of the Periodic Table, as are fluorine and chlorine. Measurements of the relative formula mass of aluminium chloride show that its formula in the vapour at the sublimation temperature is not AlCl3, but Al2Cl6.
It exists as a dimer two molecules joined together. The bonding between the two molecules is co-ordinate, using lone pairs on the chlorine atoms.
Each chlorine atom has 3 lone pairs, but only the two important ones are shown in the line diagram. There's nothing special about those two particular lone pairs - they just happen to be the ones pointing in the right direction. Energy is released when the two co-ordinate bonds are formed, and so the dimer is more stable than two separate AlCl3 molecules. If you are interested in exploring this in more detail, you could have a look at the page about the Period 3 chlorides.
It isn't particularly relevant to the present page, though. If you choose to follow this link, use the BACK button on your browser to return quickly to this page later.
The bonding in hydrated metal ions. Water molecules are strongly attracted to ions in solution - the water molecules clustering around the positive or negative ions. In many cases, the attractions are so great that formal bonds are made, and this is true of almost all positive metal ions. Ions with water molecules attached are described as hydrated ions. Although aluminium chloride is covalent, when it dissolves in water, ions are produced. It's called the hexaaquaaluminium ion - which translates as six "hexa" water molecules "aqua" wrapped around an aluminium ion.
The bonding in this and the similar ions formed by the great majority of other metals is co-ordinate dative covalent using lone pairs on the water molecules. Aluminium is 1s22s22p63s23px1. That means that all the 3-level orbitals are now empty. The aluminium re-organises hybridises six of these the 3s, three 3p, and two 3d to produce six new orbitals all with the same energy.
These six hybrid orbitals accept lone pairs from six water molecules. You might wonder why it chooses to use six orbitals rather than four or eight or whatever. Six is the maximum number of water molecules it is possible to fit around an aluminium ion and most other metal ions. By making the maximum number of bonds, it releases most energy and so becomes most energetically stable.
Only one lone pair is shown on each water molecule. The other lone pair is pointing away from the aluminium and so isn't involved in the bonding. The resulting ion looks like this:. Wedge shaped arrows represent bonds from water molecules in front of the plane of the screen or paper. Two more molecules. Check yours!
If you haven't got a copy of your syllabus , follow this link to find out how to get one. Carbon monoxide, CO. Carbon monoxide can be thought of as having two ordinary covalent bonds between the carbon and the oxygen plus a co-ordinate bond using a lone pair on the oxygen atom. Nitric acid, HNO3. In this case, one of the oxygen atoms can be thought of as attaching to the nitrogen via a co-ordinate bond using the lone pair on the nitrogen atom.
In fact this structure is misleading because it suggests that the two oxygen atoms on the right-hand side of the diagram are joined to the nitrogen in different ways. Both bonds are actually identical in length and strength, and so the arrangement of the electrons must be identical. There is no way of showing this using a dots-and-crosses picture. The bonding involves delocalisation. This page explains the origin of hydrogen bonding - a relatively strong form of intermolecular attraction.
If you are also interested in the weaker intermolecular forces van der Waals dispersion forces and dipole-dipole interactions , there is a link at the bottom of the page. The evidence for hydrogen bonding.
Many elements form compounds with hydrogen - referred to as "hydrides". If you plot the boiling points of the hydrides of the Group 4 elements, you find that the boiling points increase as you go down the group. The increase in boiling point happens because the molecules are getting larger with more electrons, and so van der Waals dispersion forces become greater. If you repeat this exercise with the hydrides of elements in Groups 5, 6 and 7, something odd happens.
Although for the most part the trend is exactly the same as in group 4 for exactly the same reasons , the boiling point of the hydride of the first element in each group is abnormally high.
In the cases of NH3, H2O and HF there must be some additional intermolecular forces of attraction, requiring significantly more heat energy to break. These relatively powerful intermolecular forces are described as hydrogen bonds. The origin of hydrogen bonding. The molecules which have this extra bonding are:.
Dotted bonds are going back into the screen or paper away from you, and wedge-shaped ones are coming out towards you.
Notice that in each of these molecules:. Lone pairs at the 2-level have the electrons contained in a relatively small volume of space which therefore has a high density of negative charge. Lone pairs at higher levels are more diffuse and not so attractive to positive things. Consider two water molecules coming close together. It doesn't go that far, but the attraction is significantly stronger than an ordinary dipole-dipole interaction. Hydrogen bonds have about a tenth of the strength of an average covalent bond, and are being constantly broken and reformed in liquid water.
If you liken the covalent bond between the oxygen and hydrogen to a stable marriage, the hydrogen bond has "just good friends" status. On the same scale, van der Waals attractions represent mere passing acquaintances! Water as a "perfect" example of hydrogen bonding.
Notice that each water molecule can potentially form four hydrogen bonds with surrounding water molecules. This is why the boiling point of water is higher than that of ammonia or hydrogen fluoride. In the case of ammonia, the amount of hydrogen bonding is limited by the fact that each nitrogen only has one lone pair.
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Odd man out. chloride, nitrate, hydride, ammonium.
MSBSHSE Class 9 Science Chapter 5 Acids, Bases and Salts Solutions
These solutions for Acids, Bases And Salts are extremely popular among Class 9 students for Science Acids, Bases And Salts Solutions come handy for quickly completing your homework and preparing for exams. Identify the odd one out and justify. Hydrogen chloride is odd because Hydrogen chloride is acid and rest are base. Sodium carbonate is odd because the solutions of sodium nitrate, sodium sulphate and sodium chloride are neutral. Common salt is odd because on heating, there is no change in color of compound.
Chemical nomenclature is the names we use for chemicals. For instance, H 2 O is called "water", and CH 4 the gas you burn in a stove is called "methane. There are lots of elements and you don't need to memorize them all.
MSBSHSE Class 9 Science Chapter 5 Acids, Bases and Salts Solutions
While chloride Cl - , nitrate NO - and hydride H - are the negatively charged ion anion. Explanation: Hydrogen chloride is odd one out because it is the only acid among the given compounds. Explanation: Acetic acid is odd one out because it is the only organic acid.
A coordination complex consists of a central atom or ion , which is usually metallic and is called the coordination centre , and a surrounding array of bound molecules or ions, that are in turn known as ligands or complexing agents. Coordination complexes are so pervasive that their structures and reactions are described in many ways, sometimes confusingly. The atom within a ligand that is bonded to the central metal atom or ion is called the donor atom. In a typical complex, a metal ion is bonded to several donor atoms, which can be the same or different. A polydentate multiple bonded ligand is a molecule or ion that bonds to the central atom through several of the ligand's atoms; ligands with 2, 3, 4 or even 6 bonds to the central atom are common.
Chloride, nitrate, hydride, ammonium. odd man out.
The questions posted on the site are solely user generated, Doubtnut has no ownership or control over the nature and content of those questions. Doubtnut is not responsible for any discrepancies concerning the duplicity of content over those questions. Study Materials. Crash Course. Question : Find odd one out chloride,nitrate,hydride,ammonium. Describe the action of heat on the following compounds : a Ammonium nitrate b Ammonium nitrite Find the odd one out. Find out the odd one.
Chloride, nitrate,hydride ammonium odd man out
Wandering Through the Hydrides