P Block Elements
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New answer posted
7 months agoContributor-Level 10
7.54
Freons or chlorofluorocarbons [CFCs] are aerosols that accelerate the depletion of ozone. In presence of ultraviolet radiation [UV radiation], these chlorofluorocarbons break down to give chlorine ions which combine with the ozone atoms in the atmosphere to give oxygen atoms.
New answer posted
7 months agoContributor-Level 10
7.53
Stability of an ionic compound depends on its lattice energy. More the lattice energy of a compound, more stable it will be. Lattice energy is directly proportional to the charge carried by an ion.
When a metal combines with oxygen, the lattice energy of the oxide involving O2- ion is much more than the oxide involving O- ion. Hence, the oxide having O2-ions are more stable than oxides having O-. Hence, we can say that formation of O2- is energetically more favorable that formation of O-.
New answer posted
7 months agoContributor-Level 10
7.52
Oxygen is smaller in size as compared to sulphur. Due to its smaller size, it can effectively form p – p bonds and form O2 [O = O] molecule. Also, the intermolecular forces in oxygen are weak van there Wall's, which cause it to exist as a gas.
On the other hand, sulphur does not form M2 molecule but exists as a puckered structure held together by strong covalent bonds. Hence, it is a solid.
New answer posted
7 months agoContributor-Level 10
7.51
The elements of group 16 are collectively called chalcogens.
[i]. Elements of group 16 have six valence electrons each. The general electronic configuration of these elements is ns2 np4, where n varies from 2 to 6.
[ii]. Oxidation state: As these elements have six valence electrons [ns2np4], they should display an oxidation state of -2. However, only oxygen predominantly shows the oxidation state of -2 owing to its high Electronegativity. It also exhibits the oxidation state of -1 [H2O2], zero [O2], and +2 [OF2].
However, the stability of the -2 oxidation state decreases on moving down a group due to a decrease in the El
New answer posted
7 months agoContributor-Level 10
7.50
Phosphorous Pentachloride [PCl5] cannot act as reducing agent because in the PCl5, the oxidation state of chlorine is +5 and it is not possible for Chlorine to increase its oxidation state beyond +5 but it can very easily act as an oxidizing agent because it can easily reduce its oxidation state from +5 to +3.
New answer posted
7 months agoContributor-Level 10
7.49
Disproportionation is a chemical reaction typically a redox reaction where a molecule is transformed into two or more dissimilar products.
On heating, orthophosphorus acid (H3PO3) disproportionate to give orthophosphoric acid (H3PO4)
and phosphine (PH3). The oxidation states of Phosphorous in various species involved in the reaction are mentioned below.
New answer posted
7 months agoContributor-Level 10
7.48
Catenation is the bonding of atoms of the same element into a series to form a chain. Catenation is much more common in phosphorous compounds than in nitrogen compounds.
This is because of the relative weakness of the NN single bond as compared to the PP single bond. Since nitrogen atom is smaller, there is greater repulsion of electron density of two nitrogen atoms, thereby weakening the NN single bond. T
his is the reason why Nitrogen shows catenation properties less than phosphorous.
Phosphorous has larger atomic size because of which it has less repulsion of electron density of two phosphorous atoms and hence P-P single bond is st
New answer posted
7 months agoContributor-Level 10
7.13
Red Phosphorus |
White Phosphorus |
1. It is soft solid and almost colourless but acquires pale yellow colour on standing. | 1. It is a red solid. |
2. It melts at 317 K and boils at 563 K. | 2. It burns at 533K to give phosphorous pentaoxide. |
3. With air contact it undergoes slow combustion and glows in dark. This property is called chemiluminescence. | 3. It does not glow in dark. |
4. It is insoluble in water but readily soluble in carbon disulphide and oils. | 4. It is insoluble in water as well as in carbon disulphide. |
5. It is very reactive and catches fire when heated in air. On burning it gives dense white fumes of phosphorus pentoxide. | 5. It is more stable and chemically less reactive as compared to white phosphorus. |
New answer posted
7 months agoContributor-Level 10
7.46
Nitrogen owing to its small size has a tendency to form p – p multiple bonds with itself. Nitrogen thus forms a very stable diatomic molecule, N2.
On moving down, a group, the tendency to form p–p bonds decreases [because of the large size of heavier elements]. With the increase in the size of atoms, the strength p– p bonds decreases.
Thus p– p bonds are weaker for heavier atoms. Therefore, phosphorus [like other heavier metals] exists in the P4 state, as shown below.
New answer posted
7 months agoContributor-Level 10
7.45
Nitrogen has a smaller size than Bismuth, because on going down the group the atomic size increases
i.e. N
Due to smaller size, there is very high electron density around Nitrogen as compared to Bismuth. Therefore, nitrogen atom can easily release electrons. And, we know higher the electron donating tendency, higher is the basic strength. Due to which NH3 is more basic than BiH3.
Note: The basic strength in group 15 is in the following pattern:
NH3 > PH3 > AsH3 > SbH3 > BiH3
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