Actually the alkenes are the compounds that have a double bond between two carbon atoms. In the formulas given above in case of ethene we have two carbon atoms but in case of methene (just supposing actually it can’t even exist) there isn’t any second carbon atom with which it could make a double bond.
In case of carboxylic acids the negative charge is on the more electronegative element that is oxygen as shown in the structure in both of the resonating structures. The negative charge on the more electronegative element makes it more stable. And thus it shows acidic character easily. But in case of phenols the negative charge
Today I wished to share my thoughts that were struggling to come out of my mind. The first thought is ,” Why we earn ? “ Most of us love to have a luxurious life , an expensive car , house in the most expensive area and holiday tours . But if we think do
the atomic size of Krypton is larger than Bromine.
chlorine shows exceptionally higher electron gain enthalpy than that of florine.
The answer to this question is very simple . There are two major reasons behind it. 1. Catenation :- It is the property by which the carbon can make long chains, branched chains and ring or cylic structural by joining with its own atoms. Due to this it can make a variety of molecules. 2.
The outer or valence shell of these elements is complete. And they need not to make any bond. They do not share or transfer the electrons . Due to fully filled orbitals, Their ionisation enthalpies are also very high. So removing an electron from them is also very difficult. The examples of these are Helium,
To answer this we have to see the reactive nature of phenol and the substituents attached to it. Acidic behavior of phenol depends on the fact that how easily it can loose a proton and make phenoxide ion which is stabilized by resonance. The methoxy group being electron donating group increases the electron density of
White phosphorus exists in p4 molecule. In the molecular strain is quite high and it tends to break it as early as possible. On the other hand red phosphorus exists as polymer like structure. In red phosphorus the molecules join to make long chains and that makes them chemically inert or less reactive. For study
Meaning of diprotic acid is that , it can loose two hydronium ions (H+) . For finding how many H+ ions it can give , we have to see its structure. Here it have only two hydroxyl groups that is -OH groups, and the hydrogen atoms joined to these only are ionisable. So only these
Actually the sigma bond involves head to head overlapping of orbitals, due to which the overlapping takes place on a larger extent. That makes the bond more stronger as compared to pie bond. In pie bond there is a sidewise overlapping of orbitals which leads to lesser extent of overlapping and thus the bond formed
1.Temperature :- With increase in temperature the rate of vaporization also increase thus it creates more pressure. Moreover with increase in temperature the kinetic energy of the vapours also increase. 2. Nature of liquid:- The liquids with lower inter-particulate attractions have high vapour pressure as the formation of vapours is easy . Like acetone is
It is an amorphous solid. In these kind of solids the particles are not properly arranged and it is assumed that the particles do not get enough time to set into a proper arrangement. So these are considered as super cooled liquids.
To understand this concept we must be aware of Threshold energy or activation energy. The threshold energy or the activation energy is the minimum amount of energy that is required for the conversion of reactants into the products . According to collision theory the reactant species collide with each other to make the product. But
How does a radiator of car works? We all are familiar with the coolent that is normally used in radiators but many of us will admit that they don’t know how it works. Well, being a chemistry geek here I will discuss how it works. Ethylene glycol is the liquid that is widely used in
This is the phenomenon which arise due to the inability of inner electrons to take part in the chemical reactions. For example in case of group 15 we have Phosphorus, Arsenic , Tin and Bismuth. They all show the oxidation states of +3 and +5, but as we move down the group we will see
The P2 molecule of phosphorus is not found because of the larger size of the phosphorus atom. The phosphorus is so larger that the p-orbitals which are required to overlapp sideways , are unable to overlapp sufficiently to make a pie bond. Below is the structure of oxygen atom that is showing π-bond But phosphorus
In case of hydrocarbons , the c-c bond is normally safe due to following two reasons :- Difference between the electronegativity of Carbon and Hydrogen. Due to this reason the electrons of the shared pair stays closer to the C-atom which makes it easy to break the C-H bond and release hydrogen as hydronium ion
Kossel and Lewis in 1916 Developed the theory for the bond formation after watching the behavior of noble gases. The noble gases were inert in behavior and do not react with any substance. Kossel and Lewis found that the Octateof noble gases was complete so they do not react. They gave the theory that the
A nice question both silicon and carbon belong to group 14 and have 4 electrons in the outermost shell. Their general valency is 4 , but silicon and other elements show higher oxidation states also. Only carbon is the element in group 14 elements that do not have vacant d-orbital. All other elements like silicon
How are reactions related to chemical bonds? The type of bond has a great effect on the rate of reaction or speed of reaction. Here we are going to discuss why and how it happens, First of all in case of ionic compounds:- Lets take example of Sodium hydroxide and Hydrochloric acid NaOH (aq) +
To understand this we have to go in depth , that how the ionic bond is formed? Ionic bond is a bond basically formed due to strong electrostatic forces of attraction which is totally different from the covalent bond. Ionic bond is formed between atoms with very different ionisation energy and electron affinity. This situation
In case of PF3 the size of F is small and thus it approaches near to the central atom that is P. as it approaches near to P there comes the repulsion between the bond pairs, which widens the bond angle and makes it larger than in case of PCl3. Here two types of forces