Looking for the eleventh magnificence Chemistry Chapter 6 Chemical bond notes? Here we've got shared the first 12 months of Chemistry Chapter 6 Short Questions Notes.
1st-year Chemistry Chapter 6 Notes pdf Short Questions
01. Bond distance is the compromise distance among atoms. Explain.
When atoms come to shut to every different, they've appeal in addition to repulsion among them. These bonded atoms live at the gap, wherein the appeal is most. This distance is likewise referred to as compromise distance or bond period.
02. The difference between a co-ordinate covalent bond and a covalent bond vanishes after bond formation. Explain with the assistance of an example.
The coordinate covalent bond is fashioned whilst the shared pair of the electron is donated with the aid of using one of the bonded atoms. This bond is represented with the aid of using the arrow (→). Arrowhead is from donor atom in the direction of acceptor atom. After the formation of a bond, distinction vanishes and it behaves similar to covalent.
03. The bonds angles of H2O and NH3 aren't 109.five° like that of CH4 even though O and N atoms are sp3 hybridized. Explain.
In CH4, NH3, and H2O the primary atoms C, N, and O are SP3 hybridized. The bond attitude in NH3 and H2O are 107.5o and 104.5o respectively. The lower in bond attitude is due to the fact one lone pair of N and lone pairs of O repel the bonds pair. NH3 has one lone pair so the attitude is much less decreased even as H2O has lone pairs so the attitude is extra decreased.
04. Πbonds are extra subtle than σ bonds. Or σ bond is more potent than Πbond. Explain.
In the sigma bond, the electron density is among nuclei or on the bond axis. In the case of the π bond, the electron density is above and beneath neath the nuclear axis. In the π bond electron cloud is extended at extra areas than the sigma bond, so the π bond or π electrons are extra subtle than sigma.
05. The abnormality in bond period and bond power in HI is much less distinguished than that of HCl. Explain.
In the case of HI, the calculated bond power is 291kJ/mol even as the experimental bond power is 299kJ/mol. The distinction among the 2 energies is 8kJ/mol. In the case of HCl, the located bond power is 432kJ/mol even as the calculated bond power is 336kJ/mol. The distinction between the 2 energies is 96kJ/mol. Greater power distinction in HCl is because of the extra ionic man or woman of HCl.
06. The dipole second of CO2 and CS2 is 0 however that of SO2 is 1.61D. Explain.
CO2 and SO2 have a linear shape. In linear shape dipole second of man or woman bond cancel the impact of every different. So the internet dipole second is 0. But cancelation does now no longer show up in SO2 due to the fact its shape is angular.
07. The melting and boiling factors of electrovalent compounds (ionic) are very excessive in comparison to covalent compounds. Why?
In ionic compounds robust ionic forces are gifts. A big quantity of power is needed to interrupt those forces of appeal. In covalent compounds, forces amongst debris are weak so much less quantity of power is needed to interrupt those forces. That is why ionic compounds have excessive melting and boiling factors.
09. Why Ï€ − bonds are weaker than σ − bonds.
σ bond is fashioned with the aid of using head-to-head overlapping of orbitals and electron density is most among the 2 nuclei at the bond axis. π-bonds are fashioned with the aid of using sideway overlapping of orbitals and electrons density is a gift above and beneath neath the bond axis. That is π-bonds are weaker than a σ bond.
11. Why MOT is more advanced than VBT?
MOT principle explains the paramagnetic conduct of the O2 molecule. Also, it explains the non-life of the He2 molecule.
12. Why is the power of ABMO is extra than BMO?
In ABMO the electron density is low at the nuclear axis so nucleus-nucleus repulsion is extra and the gadget is risky and of excessive power.
In BMO the electrons density is most at the nuclear axis among the nuclei. So, nucleus-nucleus repulsion is minimal and the gadget is strong and of low power.
13. Why the cationic radius is continually smaller than its determined atom?
The superb ion is continually smaller than its determined atom due to reasons:
a) Because of the lack of an electron, there may be an opportunity that a shell can also be lost.
b) After the lack of an electron, the stability of electron and proton is disturbed. Now there are extra protons for fewer electrons. So, there might be an excessive quantity of appeal of protons for electrons, and for this reason, the length will be lower.
14. Why the anionic radius is continually extra than its determined atom?
The poor ion is continually extra than its determined atom due to reasons: a) The incoming electron can be repelled with the aid of using the already gift electrons withinside the outermost shell and this repulsion can bring about the growth of the digital cloud.
b) After the benefit of the electron, the stability of the electron and proton is disturbed. Now there are extra electrons for fewer protons. So, the pressure of appeal among the nucleus and electrons is reduced which ends up in a growth in length.
15. Why the second ionization power of magnesium is better than the primary one?
It is tough to do away with the second electron from an ion in comparison to an atom. Because nuclear price draws the final electrons strongly. So 2nd ionization power is extra than the first ionization power.
16. Why are the electron affinity of fluorines is much less than chlorine?
Actually, Fluorine has a totally small length and 7 electrons in 2s and 2p orbitals generating a thick digital cloud. Its thick clouds repel the incoming electron.
17. Why there may be no bond in chemistry that is 100% ionic?
A 100% ionic bond is fashioned handiest whilst the electron is absolutely transferred from one atom to the different. It can show up handiest whilst the donor atom has 0 electronegativity fee. However, no atom has 0 electronegativity fee. So, no bond is 100% ionic. The bond among CsF is 92% ionic is the best ionic man or woman. And NaCl is 72% ionic.
18. What is supposed with the aid of using paramagnetic and diamagnetic substances?
Any substance which has an unpair of electrons and is drawn to the robust magnetic subject is referred to as a paramagnetic substance.
Any substance which has a couple of electrons and does now no longer entice in the direction of a robust magnetic subject is referred to as a diamagnetic substance.
19. Why Ionic bonds are non-directional in nature?
The ionic compounds contain electrostatic traces of forces among oppositely charged ions. Therefore, such bonds are non-inflexible and non-directional. Because of this ionic bonds are non-directional in nature.
20. Limitations of the Lewis Model: It doesn’t inform approximately the subsequent factors: i. How do electrons keep away from every difference notwithstanding their repulsion?
ii. Shapes of molecules
iii. The geometry of molecules
iv. Bond polarity
v. Bond period
vi. Various power transition
21. Postulates of VBT:
i. A bond among atoms is fashioned with the aid of using the overlap of 1/2 of-stuffed atomic orbitals of atoms.
ii. The overlapping orbitals hold their identity.
iii. The range of bonds fashioned with the aid of using an atom is identical to the range of 1/2 of-stuffed orbitals.
iv. During the overlapping of orbitals, power is released.
VSEPR-Theory
AB2- Type with bond pairs: In such molecules, the 2 bonding electron pairs organized themselves across the primary atom in any such manner to limit repulsion.
Example: MgCl2, CaCl2, BeCl2 Angle: 180° Structure: Linear
AB3- Type with 3 bond pairs: In such molecules, the 3 bonding electron pairs organized themselves across the primary atom in any such manner to limit repulsion.
Example:
BF3,BH3, AlCl3
Angle:
a hundred and twenty°
Structure:
Triangular.
AB3- Type with bond pairs and one lone pair:
In such molecules, the 2 bond pairs and one lone pair organized themselves across the primary atom
in any such manner to limit repulsion.
Example:
Sn̈Cl2
Angle:
Less than a hundred and twenty°
Structure:
Distorted Triangular
Note: Lone pair exert extra repulsion on bond pair because of which attitude will become much less than a hundred and twenty°.
AB3- Type with more than one bond pair and one lone pair:
In such molecules, the 2 more than one bond pair and one lone pair organized themselves around
the primary atom in any such manner to limit repulsion.
Example:
S̈O2
Angle:
Less than a hundred and twenty.
Structure: distorted triangles
Note: Lone pair exert extra repulsion on bond pair because of which attitude will become much less than a hundred and twenty°. And According to the VSEPR principle double bonds behave like an unmarried bond.
AB3- Type with 3 more than one bond pair:
In such molecules, the 3 more than one bond pairs organized themselves across the primary atom in any such manner to limit repulsion.
Example:
SO3
Angle:
a hundred and twenty°
Structure:
Triangular
Note: According to the VSEPR principle more than one bond is treated as an unmarried bond.
AB4- Type with 4 bond pairs:
In such molecules, the 4 bond pairs organized themselves across the primary atom in any such manner to limit repulsion.
Example: CH4, SiH4, CCl4, SnCl4 Angle: 109. five°
Structure:
Tetrahedral.
AB4 - Type with one lone pair and 3 bond pairs:
A molecule having 3 bond pairs and one lone pair across the primary atom has triangular pyramidal geometry rather than tetrahedral.
Reason:
Due to repulsions among lone pair and bond pairs, the geometry might be pyramidal.
Bond Angle:
The bond attitude reduces to 107.five°
Example:
P̈H3, As̈H3, Sb̈H3, N̈H3
Structure:
Pyramidal
AB4 Type with lone pairs and bond pairs:
In this example presence of lone pairs introduces 3 sorts of repulsions i.e. L.p-L.p, L.p-B.p and B.p-B.p. The participation of the lone pair and bond pair in figuring out the geometry of the H2O molecule. Two corners of the tetrahedron are occupied with the aid of using every one of the 2 lone pairs and final with the aid of using bond pair.
Structure:
Bent or Angular geometry.
Bond Angle: The attitude is, in addition, decreased to 104.five°
You may like:
- 1st-year Chemistry Chapter 7 Notes pdf Short and Long Questions
- 1st-year Chemistry Chapter 5 Notes pdf Short and Long Questions
This is the publish on the subject of the first 12 months of Chemistry Chapter 6 Short Questions Notes. The publish is tagged and categorized beneath neath in eleventh chemistry, eleventh notes, Education News Tags. For extra content material associated with this publication, you could click on the labels link.
Related keyphrases
Here are a number of the associated key phrases to this publish: 1st, Chapter, Short, Notes, Chemistry, 6, Questions
