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All questions of Chemical Bonding and Molecular Structure for NEET Exam
Bond order of 1.5 is shown by : [2012] - a)O2+
- b)O2-
- c)O22+
- d)O2
Correct answer is option 'B'. Can you explain this answer?
Bond order of 1.5 is shown by : [2012]
a)
O2+
b)
O2-
c)
O22+
d)
O2
|
Rajat Kapoor answered |
N₂=N+N = 7e⁻+7e⁻ = 14e- which has bond order =3
O₂=8e⁻+8e⁻ = 16e⁻ which has bond order = 2
O₂⁺=8e⁻+8e⁻ - 1e⁻ = 15e⁻ which has bond order= 2.5
O₂⁻ = 8e⁻ +8e⁻ +1e⁻ =17 e⁻ which has bond order=1.5
So option B is correct .
Which of the following compounds has a 3-centre bond?[1996]- a)Diborane
- b)Carbon dioxide
- c)Boron trifluroide
- d)Ammonia
Correct answer is option 'A'. Can you explain this answer?
Which of the following compounds has a 3-centre bond?[1996]
a)
Diborane
b)
Carbon dioxide
c)
Boron trifluroide
d)
Ammonia
|
Krish Saha answered |
The bond represented by dots form the 3-centred electron pair bond. The idea of three centred electron pair bond B–H–B bridges is necessitated because diborane does not have sufficient electrons to form normal covalent bonds. It has only 12 electrons instead of 14 required to give simple ethane like structure for diborane.
N2 and O2 are converted into monocations, N2+ and O2+ respectively. Which of the following statements is wrong ? [1997]- a)In N2, the N—N bond weakens
- b)In O2, the O—O bond order increases
- c)In O2, paramagnetism decreases
- d)N2+ becomes diamagnetic
Correct answer is option 'B'. Can you explain this answer?
N2 and O2 are converted into monocations, N2+ and O2+ respectively. Which of the following statements is wrong ? [1997]
a)
In N2, the N—N bond weakens
b)
In O2, the O—O bond order increases
c)
In O2, paramagnetism decreases
d)
N2+ becomes diamagnetic
|
Rohan Unni answered |
We know that in O2 bond, the order is 2 and in O2– bond, the order is 1.5. Therefore the wrong statements is (b)
Which of the following has pπ – dπ bonding?- a)NO3–
- b)SO32– [2002]
- c)BO33–
- d)CO32–
Correct answer is option 'B'. Can you explain this answer?
Which of the following has pπ – dπ bonding?
a)
NO3–
b)
SO32– [2002]
c)
BO33–
d)
CO32–
|
Smruti Sucharita answered |
Answer is b bcoz Sulphur has d orbital...
In BrF3 molecule, the lone pairs occupy equatorial positions to minimize [2004]- a)lone pair - bond pair repulsion only
- b)bond pair - bond pair repulsion only
- c)lone pair - lone pair repulsion and lone pair -bond pair repulsion
- d)lone pair - lone pair repulsion only
Correct answer is option 'C'. Can you explain this answer?
In BrF3 molecule, the lone pairs occupy equatorial positions to minimize [2004]
a)
lone pair - bond pair repulsion only
b)
bond pair - bond pair repulsion only
c)
lone pair - lone pair repulsion and lone pair -bond pair repulsion
d)
lone pair - lone pair repulsion only
|
Abhishek Choudhary answered |
In BrF3, both bond pairs as well as lone pairs of electrons are present. Due to the presence of lone pairs of electrons (lp) in the valence shell, the bond angle is contracted and the molecule takes the T-shape. This is due to greater repulsion between two lone pairs or between a lone pair and a bond pair than between the two bond pairs.
Which one of the following arrangements represents the increasing bond orders of the given species? [1999]- a)NO+ < NO < NO– < O2–
- b)O2– < NO– < NO <NO+
- c)NO– < O2– < NO < NO+
- d)NO < NO+ < O2– < NO–
Correct answer is option 'B'. Can you explain this answer?
Which one of the following arrangements represents the increasing bond orders of the given species? [1999]
a)
NO+ < NO < NO– < O2–
b)
O2– < NO– < NO <NO+
c)
NO– < O2– < NO < NO+
d)
NO < NO+ < O2– < NO–
|
Mira Joshi answered |
Bond order of NO+ =
Similarly, Bond order of NO = 
Bond order of NO– 
Bon d order of 
By above calculation, we get Decreasing bond order NO+ > NO > NO– > O-2
In a regular octahedral molecule, MX6 the number of X - M - X bonds at 180° is [2004]- a)three
- b)two
- c)six
- d)four
Correct answer is option 'A'. Can you explain this answer?
In a regular octahedral molecule, MX6 the number of X - M - X bonds at 180° is [2004]
a)
three
b)
two
c)
six
d)
four
|
Lavanya Menon answered |
Thus here bond angles between X4 - M - X2 = 180°
X1 - M - X3 = 180°
X5 - M - X6 = 180°
X1 - M - X3 = 180°
X5 - M - X6 = 180°
The relationship between the dissociation energy of N2 and N2+ is : [2000]- a)Dissociation energy of N2+ > dissociation energy of N2
- b)Dissociation energy of N2 = dissociation energy of N2+
- c)Dissociation energy of N2 > dissociation energy of N2+
- d)Dissociation energy of N2 can either be lower or higher than the dissociation energy of N2+
Correct answer is option 'C'. Can you explain this answer?
The relationship between the dissociation energy of N2 and N2+ is : [2000]
a)
Dissociation energy of N2+ > dissociation energy of N2
b)
Dissociation energy of N2 = dissociation energy of N2+
c)
Dissociation energy of N2 > dissociation energy of N2+
d)
Dissociation energy of N2 can either be lower or higher than the dissociation energy of N2+
|
Mahi Shah answered |
Dissociation energy of any molecules depends upon bond order. Bond order in N2 molecule is 3 while bond order in N+2 is 2.5.
Further we know that more the Bond order, more is the stability and more is the BDE.
Further we know that more the Bond order, more is the stability and more is the BDE.
Which of the following bonds will be most polar?- a)N – Cl
- b)O – F [1992]
- c)N – F
- d)N – N
Correct answer is option 'C'. Can you explain this answer?
Which of the following bonds will be most polar?
a)
N – Cl
b)
O – F [1992]
c)
N – F
d)
N – N
|
Aman Sharma answered |
Polarity of the bond depends upon the electronegativity difference of the two atoms forming the bond. Greater the electronegativity difference, more is the polarity of the bond.
As the electronegativity difference between N and F is maximum hence this bond is most polar.
Which of the following would have a permanent dipolemoment? [2005]- a)SiF4
- b)SF4
- c)XeF4
- d)BF3
Correct answer is option 'B'. Can you explain this answer?
Which of the following would have a permanent dipolemoment? [2005]
a)
SiF4
b)
SF4
c)
XeF4
d)
BF3
|
Prasenjit Pillai answered |
SF4 has permanent dipole moment.
SF4 has sp3d hybridization and see saw shape (irregular geometry).
SF4 has sp3d hybridization and see saw shape (irregular geometry).
Whereas XeF4 shows squre planar geometry SiF4 has tetrahedral shape and BF3 has Trigonal planar shape. All these are symmetric molecules. Hence μ ≠ 0.
The BCl3 is a planar molecule whereas NCl3 is pyramidal because [1995]- a)B-Cl bond is more polar than N-Cl bond
- b)N-Cl bond is more covalent than B-Cl bond
- c)nitrogen atom is smaller than boron atom
- d)BCl3 has no lone pair but NCl3 has a lone pair of electrons
Correct answer is option 'D'. Can you explain this answer?
The BCl3 is a planar molecule whereas NCl3 is pyramidal because [1995]
a)
B-Cl bond is more polar than N-Cl bond
b)
N-Cl bond is more covalent than B-Cl bond
c)
nitrogen atom is smaller than boron atom
d)
BCl3 has no lone pair but NCl3 has a lone pair of electrons
|
Rajeev Sharma answered |
As there is no lone pair on boron in BCl3 therefore no repulsion takes place. But there is a lone pair on nitrogen in NCl3. Therefore repulsion takes place. Thus BCl3 is planar molecule but NCl3 is a pyramidal molecule.
The angle between the overlapping of one s-orbital and one p-orbital is [1988]- a)180°
- b)120°
- c)109°28'
- d)120°, 60°
Correct answer is option 'A'. Can you explain this answer?
The angle between the overlapping of one s-orbital and one p-orbital is [1988]
a)
180°
b)
120°
c)
109°28'
d)
120°, 60°
|
Geetika Shah answered |
The overlap between s- and p-orbitals occurs along internuclear axis and hence the angle is 180°.
Which structure is linear ? [1992]- a)SO2
- b)CO2
- c)CO32-
- d)SO24-
Correct answer is option 'B'. Can you explain this answer?
Which structure is linear ? [1992]
a)
SO2
b)
CO2
c)
CO32-
d)
SO24-
|
Ayush Chavan answered |
CO2 has sp-hybridization and is linear. SO2 and CO2-3 are planar (sp2) while SO2-4 is tetrahedral (sp3).
H2O is polar, whereas BeF2 is not. It is because [2004]- a)the electronegativity of F is greater than that of O
- b)H2O involves hydrogen bonding wher eas BeF2 is a discrete molecule
- c)H2O is linear and BeF2 is angular
- d)H2O is angular and BeF2 is linear
Correct answer is option 'D'. Can you explain this answer?
H2O is polar, whereas BeF2 is not. It is because [2004]
a)
the electronegativity of F is greater than that of O
b)
H2O involves hydrogen bonding wher eas BeF2 is a discrete molecule
c)
H2O is linear and BeF2 is angular
d)
H2O is angular and BeF2 is linear
|
Naina Sharma answered |
In a linear symmetrical molecule like BeF2, the bond angle between three atoms is 180°, hence the polarity due to one bond is cancelled by the equal polarity due to other bond, while it is not so in angular molecules, like H2O
Four diatomic species are listed below in different sequences. Which of these presents the correct order of their increasing bond order ? [2008]- a)
- b)
- c)
- d)
Correct answer is option 'D'. Can you explain this answer?
Four diatomic species are listed below in different sequences. Which of these presents the correct order of their increasing bond order ? [2008]
a)
b)
c)
d)
|
|
Lalit Yadav answered |
Calculating the bond order of various species.
From these values we find the correct order of increasing bond order is
Which of the following species has a linear shape ?- a)SO2
- b)NO2+ [2006]
- c)O3
- d)NO2–
Correct answer is option 'B'. Can you explain this answer?
Which of the following species has a linear shape ?
a)
SO2
b)
NO2+ [2006]
c)
O3
d)
NO2–
|
Ayush Choudhury answered |
NO2+ will have linear shape as it will have sp hybridisation.
Among the following orbital bonds, the angle is minimum between [1994]- a)sp3 bonds
- b)px and py orbitals
- c)H – O – H in water
- d)sp bonds.
Correct answer is option 'B'. Can you explain this answer?
Among the following orbital bonds, the angle is minimum between [1994]
a)
sp3 bonds
b)
px and py orbitals
c)
H – O – H in water
d)
sp bonds.
|
Shanaya Rane answered |
The angle between the bonds formed by px and py orbitals is the minimum i.e. 90°
The correct order of increasing bond angles in the following triatomic species is : [2008] - a)NO2- <NO+2<NO2
- b)NO2- <NO2<NO2+
- c)NO2+ <NO-2<NO
- d)none
Correct answer is option 'B'. Can you explain this answer?
The correct order of increasing bond angles in the following triatomic species is : [2008]
a)
NO2- <NO+2<NO2
b)
NO2- <NO2<NO2+
c)
NO2+ <NO-2<NO
d)
none
|
Sneha Basak answered |
From the structure of three species we can determine the number of lone pair electrons on central atom (i.e. N atom) and thus the bond angle.
We know that higher the number of lone pair of electron on central atom, greater is the lp – lp repulsion between Nitrogen and oxygen atoms. Thus smaller is bond angle..
The correct order of bond angle is
The correct order of bond angle is
NO2 NO2 NO2 i .e. opti on (b) is correct.
In an octahedral structure, the pair of d orbitals involved in d2sp3 hybridization is [2004]- a)
- b)
- c)dz2 , dxz
- d)dxy,dyz
Correct answer is option 'A'. Can you explain this answer?
In an octahedral structure, the pair of d orbitals involved in d2sp3 hybridization is [2004]
a)
b)
c)
dz2 , dxz
d)
dxy,dyz
|
|
Maya Sengupta answered |
Only those d or bital s whose l obes are directed along X, Y and Z directions hybridise with s and p orbitals. In other three d or bitals n amely dxy, dyz and dxz, the lobes are at an angle of 45° from both axis, hence the extent of their overlap with s and p orbitals is much lesser than 
and 
orbitals.
and orbitals.Which of the following molecules has trigonal planar geometry? [2005]
- a)BF3
- b)NH3
- c)PCl3
- d)IF3
Correct answer is option 'A'. Can you explain this answer?
Which of the following molecules has trigonal planar geometry? [2005]
a)
BF3
b)
NH3
c)
PCl3
d)
IF3
|
Tejas Chavan answered |
3 is sp2 hybridised. So, it is trigon al planner. NH3, PCl3 has sp3 hybridisation hence has trigonal bipyramidal shape, IF3, has sp3d hydridization and has linear shape.
Strongest bond is in between [1993]- a)CsF
- b)NaCl
- c)Both (a) and (b)
- d)None of above
Correct answer is option 'A'. Can you explain this answer?
Strongest bond is in between [1993]
a)
CsF
b)
NaCl
c)
Both (a) and (b)
d)
None of above
|
Raghav Khanna answered |
According to Fajan rules, ionic character increases with increase in size of the cation and decrease in size of the anion. Thus, CsF has higher ionic character than NaCl and hence bond in CsF is stronger than in NaCl.
The correct order of C–O bond length among CO, CO32- , CO2 is [2007]- a)CO < CO32– < CO2
- b)CO32– < CO2 < CO
- c)CO < CO2 < CO32–
- d)CO2 < CO32– < CO
Correct answer is option 'C'. Can you explain this answer?
The correct order of C–O bond length among CO, CO32- , CO2 is [2007]
a)
CO < CO32– < CO2
b)
CO32– < CO2 < CO
c)
CO < CO2 < CO32–
d)
CO2 < CO32– < CO
|
|
Anitha Bathula answered |
But bond order inversely proportional to bond length then option a is correct answer
In which of the following the bond angle is maximum? [2001]- a)NH3
- b)SCl2
- c)NH4+
- d)PCl3
Correct answer is option 'C'. Can you explain this answer?
In which of the following the bond angle is maximum? [2001]
a)
NH3
b)
SCl2
c)
NH4+
d)
PCl3
|
Gowri Nair answered |
We know that bond angles of NH3 = 107º, 4+ = 109.5º, PCl3 = 100º. Therefore bond angle of NH4+ is maximum.
Which one shows the strongest hydrogen bonding?- a)H2O
- b)CH3OH
- c) NH3
- d)HF.
Correct answer is option 'D'. Can you explain this answer?
Which one shows the strongest hydrogen bonding?
a)
H2O
b)
CH3OH
c)
NH3
d)
HF.
|
|
Raghav Bansal answered |
Among the F, O, and N, Fluorine has a higher value of electronegativity, this is the reason that fluorine can form the strongest hydrogen bond with the H atom of another molecule.
Just take an idea from the value of the energy of hydrogen bond that is formed with HF, H2O, and NH3
means to break the hydrogen of one mole HF molecules, 10Kcal energy is required.
The angular shape of ozone molecule (O3) consists of : [2008]- a)1 sigma and 2 pi bonds
- b)2 sigma and 2 pi bonds
- c)1 sigma and 1 pi bonds
- d)2 sigma and 1 pi bonds
Correct answer is option 'D'. Can you explain this answer?
The angular shape of ozone molecule (O3) consists of : [2008]
a)
1 sigma and 2 pi bonds
b)
2 sigma and 2 pi bonds
c)
1 sigma and 1 pi bonds
d)
2 sigma and 1 pi bonds
|
Arya Khanna answered |
The shape of ozone molecule is
In it we find 2σ and 1π bond, i.e., option (d) is correct.
The boiling point of p-nitrophenol is higher than that of o-nitrophenol because [1994]- a)NO2 group at p-position behave in a different way from that at o-position.
- b)intramolecular hydrogen bonding exists in p-nitrophenol
- c)there is intermolecular hydrogen bonding in p-nitrophenol
- d)p-nitrophenol has a higher molecular weight than o-nitrophenol.
Correct answer is option 'C'. Can you explain this answer?
The boiling point of p-nitrophenol is higher than that of o-nitrophenol because [1994]
a)
NO2 group at p-position behave in a different way from that at o-position.
b)
intramolecular hydrogen bonding exists in p-nitrophenol
c)
there is intermolecular hydrogen bonding in p-nitrophenol
d)
p-nitrophenol has a higher molecular weight than o-nitrophenol.
|
Amrita Yadav answered |
Explanation:
The boiling point of a compound is influenced by various factors including molecular weight, intermolecular forces, and intramolecular forces. In the case of p-nitrophenol and o-nitrophenol, the difference in their boiling points can be attributed to the presence of intermolecular hydrogen bonding in p-nitrophenol.
Intermolecular Hydrogen Bonding:
Intermolecular hydrogen bonding occurs between molecules of a compound. It is a strong type of dipole-dipole interaction in which a hydrogen atom bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) is attracted to another electronegative atom in a neighboring molecule.
p-Nitrophenol:
In p-nitrophenol, the -OH group is located at the para position (p-position) with respect to the nitro group (-NO2). The presence of the nitro group increases the electronegativity of the oxygen atom in the -OH group, making it more prone to form hydrogen bonds with neighboring molecules. This results in the formation of intermolecular hydrogen bonding in p-nitrophenol.
o-Nitrophenol:
In o-nitrophenol, the -OH group is located at the ortho position (o-position) with respect to the nitro group. Due to the close proximity of the nitro group, the -OH group in o-nitrophenol is unable to form strong intermolecular hydrogen bonds. Instead, it experiences intramolecular hydrogen bonding within the molecule itself. Intramolecular hydrogen bonding occurs when the hydrogen bond donor and acceptor are present within the same molecule.
Boiling Point:
Intermolecular hydrogen bonding is a stronger intermolecular force compared to intramolecular hydrogen bonding. It requires more energy to break the intermolecular hydrogen bonds in p-nitrophenol during the boiling process, resulting in a higher boiling point compared to o-nitrophenol.
Therefore, the correct answer is option C - there is intermolecular hydrogen bonding in p-nitrophenol.
The boiling point of a compound is influenced by various factors including molecular weight, intermolecular forces, and intramolecular forces. In the case of p-nitrophenol and o-nitrophenol, the difference in their boiling points can be attributed to the presence of intermolecular hydrogen bonding in p-nitrophenol.
Intermolecular Hydrogen Bonding:
Intermolecular hydrogen bonding occurs between molecules of a compound. It is a strong type of dipole-dipole interaction in which a hydrogen atom bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) is attracted to another electronegative atom in a neighboring molecule.
p-Nitrophenol:
In p-nitrophenol, the -OH group is located at the para position (p-position) with respect to the nitro group (-NO2). The presence of the nitro group increases the electronegativity of the oxygen atom in the -OH group, making it more prone to form hydrogen bonds with neighboring molecules. This results in the formation of intermolecular hydrogen bonding in p-nitrophenol.
o-Nitrophenol:
In o-nitrophenol, the -OH group is located at the ortho position (o-position) with respect to the nitro group. Due to the close proximity of the nitro group, the -OH group in o-nitrophenol is unable to form strong intermolecular hydrogen bonds. Instead, it experiences intramolecular hydrogen bonding within the molecule itself. Intramolecular hydrogen bonding occurs when the hydrogen bond donor and acceptor are present within the same molecule.
Boiling Point:
Intermolecular hydrogen bonding is a stronger intermolecular force compared to intramolecular hydrogen bonding. It requires more energy to break the intermolecular hydrogen bonds in p-nitrophenol during the boiling process, resulting in a higher boiling point compared to o-nitrophenol.
Therefore, the correct answer is option C - there is intermolecular hydrogen bonding in p-nitrophenol.
Linus Pauling received the Nobel Prize for his work on [1994]- a)atomic structure
- b)ph ot osyn th esis
- c)chemical bonds
- d)thermodynamics
Correct answer is option 'C'. Can you explain this answer?
Linus Pauling received the Nobel Prize for his work on [1994]
a)
atomic structure
b)
ph ot osyn th esis
c)
chemical bonds
d)
thermodynamics
|
Athira Datta answered |
Explanation:
Linus Pauling, an American chemist, received the Nobel Prize for Chemistry in 1954 for his work on chemical bonds. His groundbreaking research and contributions to the understanding of the nature of chemical bonding revolutionized the field of chemistry and had a profound impact on various scientific disciplines.
Chemical Bonds:
Chemical bonds are the forces of attraction that hold atoms together in a molecule or compound. Understanding the nature of chemical bonds is crucial for understanding the properties and behavior of substances. Linus Pauling's work on chemical bonds provided significant insights into the fundamental principles governing the formation and stability of chemical compounds.
Valence Bond Theory:
One of Pauling's most notable contributions was the development of the valence bond theory. This theory describes how chemical bonds are formed through the overlap of atomic orbitals. Pauling proposed that atoms share electrons to achieve a more stable electron configuration, leading to the formation of covalent bonds. His work on the valence bond theory provided a comprehensive framework for understanding the structural and electronic properties of molecules.
Electronegativity and Bond Polarity:
Pauling also introduced the concept of electronegativity, which measures the ability of an atom to attract electrons in a chemical bond. He developed a scale for comparing the electronegativity values of different elements, known as the Pauling electronegativity scale. This scale is widely used to determine the polarity of chemical bonds and predict the behavior of molecules.
Other Contributions:
In addition to his work on chemical bonds, Linus Pauling made significant contributions to various other areas of science. He studied the structure of proteins and proposed the concept of alpha-helices and beta-sheets, which are important structural elements in proteins. Pauling's work on protein structure laid the foundation for the field of molecular biology.
Conclusion:
Linus Pauling's work on chemical bonds, particularly his development of the valence bond theory and the concept of electronegativity, earned him the Nobel Prize in Chemistry in 1954. His contributions have had a lasting impact on the field of chemistry and continue to be influential in various scientific disciplines.
Which one of the following is the correct order of interactions ? [1993]- a)Covalent < hydrogen bonding < vander Waals < dipole-dipole
- b)vander Waals < hydrogen bonding < dipole < covalent
- c)vander Waals < dipole-dipole < hydrogen bonding < covalent
- d)Dipole-dipole < vander Waals < hydrogen bonding < covalent.
Correct answer is option 'B'. Can you explain this answer?
Which one of the following is the correct order of interactions ? [1993]
a)
Covalent < hydrogen bonding < vander Waals < dipole-dipole
b)
vander Waals < hydrogen bonding < dipole < covalent
c)
vander Waals < dipole-dipole < hydrogen bonding < covalent
d)
Dipole-dipole < vander Waals < hydrogen bonding < covalent.
|
Muskaan Kumar answered |
B)Ionic
c)Hydrogen bonding
d)Van der Waals interactions
The correct order of interactions is:
a) Covalent
b) Ionic
c) Hydrogen bonding
d) Van der Waals interactions
This order is based on the strength of the interactions, with covalent bonds being the strongest and van der Waals interactions being the weakest.
c)Hydrogen bonding
d)Van der Waals interactions
The correct order of interactions is:
a) Covalent
b) Ionic
c) Hydrogen bonding
d) Van der Waals interactions
This order is based on the strength of the interactions, with covalent bonds being the strongest and van der Waals interactions being the weakest.
In which of the following molecules / ions BF3, NO2-, NH2- and H2O , [2009] the central atom is sp2 hybridized ?- a)NH2- and H2O
- b)NO2- and H2O
- c)BF3 and NO2-
- d)NO2- and NH2-
Correct answer is option 'C'. Can you explain this answer?
In which of the following molecules / ions BF3, NO2-, NH2- and H2O , [2009] the central atom is sp2 hybridized ?
a)
NH2- and H2O
b)
NO2- and H2O
c)
BF3 and NO2-
d)
NO2- and NH2-
|
|
Abhishek Choudhary answered |
For neutral molecules: No. of electron pairs = No. of atoms bonded
to it +
[Group number of central atom –Valency of the central atom].
For ions : No. of electron pairs = No. of atoms bonded
to it +[Group no. of central atom – valency of the central atom ± no. of electrons] On calcuting no. of electron pairs in given molecules. We find that in the given molecules hybridisation is
to it +
[Group number of central atom –Valency of the central atom].For ions : No. of electron pairs = No. of atoms bonded
to it +
[Group no. of central atom – valency of the central atom ± no. of electrons] On calcuting no. of electron pairs in given molecules. We find that in the given molecules hybridisation is
Which of the following molecules is planar?- a)SF4
- b)XeF4 [1998]
- c)NF3
- d)SiF4
Correct answer is option 'B'. Can you explain this answer?
Which of the following molecules is planar?
a)
SF4
b)
XeF4 [1998]
c)
NF3
d)
SiF4
|
Nilotpal Gupta answered |
XeF4 hybridisation is = 
hence V = 8 (no. of valence e–) X = 4 (no of monovalent atom)
C = 0 charge on cation A = 0 (charge on anion). The shape is
Square planar shape.Which of the following is the electron deficient molecule? [2005]- a)C2H6
- b)B2H6
- c)SiH4
- d)PH3
Correct answer is option 'B'. Can you explain this answer?
Which of the following is the electron deficient molecule? [2005]
a)
C2H6
b)
B2H6
c)
SiH4
d)
PH3
|
Anand Kapoor answered |
**Answer:**
**B2H6** is the electron deficient molecule.
- In order to determine which molecule is electron deficient, we need to consider the number of valence electrons in each molecule and compare it to the number of electrons required for a stable octet or duet.
- Boron (B) has an atomic number of 5, which means it has 5 electrons in its neutral state. Hydrogen (H) has an atomic number of 1, so it has 1 electron in its neutral state.
- In B2H6, we have 2 boron atoms and 6 hydrogen atoms.
- The total number of valence electrons in B2H6 is calculated by adding the valence electrons of each atom:
- 2 boron atoms x 3 valence electrons = 6 valence electrons
- 6 hydrogen atoms x 1 valence electron = 6 valence electrons
- Total = 6 + 6 = 12 valence electrons
- In order to determine if B2H6 is electron deficient, we need to compare the number of valence electrons to the number of electrons required for a stable octet or duet.
- For boron, it requires 8 electrons for a stable octet, and for hydrogen, it requires 2 electrons for a stable duet.
- Therefore, the total number of electrons required for a stable octet or duet in B2H6 is:
- 2 boron atoms x 8 electrons = 16 electrons
- 6 hydrogen atoms x 2 electrons = 12 electrons
- Total = 16 + 12 = 28 electrons
- Since B2H6 has only 12 valence electrons, it is electron deficient because it does not have enough electrons to achieve a stable octet or duet.
- On the other hand, molecules such as C2H6, SiH4, and PH3 have enough valence electrons to achieve a stable octet or duet, so they are not electron deficient.
- Therefore, the correct answer is option **B) B2H6**.
**B2H6** is the electron deficient molecule.
- In order to determine which molecule is electron deficient, we need to consider the number of valence electrons in each molecule and compare it to the number of electrons required for a stable octet or duet.
- Boron (B) has an atomic number of 5, which means it has 5 electrons in its neutral state. Hydrogen (H) has an atomic number of 1, so it has 1 electron in its neutral state.
- In B2H6, we have 2 boron atoms and 6 hydrogen atoms.
- The total number of valence electrons in B2H6 is calculated by adding the valence electrons of each atom:
- 2 boron atoms x 3 valence electrons = 6 valence electrons
- 6 hydrogen atoms x 1 valence electron = 6 valence electrons
- Total = 6 + 6 = 12 valence electrons
- In order to determine if B2H6 is electron deficient, we need to compare the number of valence electrons to the number of electrons required for a stable octet or duet.
- For boron, it requires 8 electrons for a stable octet, and for hydrogen, it requires 2 electrons for a stable duet.
- Therefore, the total number of electrons required for a stable octet or duet in B2H6 is:
- 2 boron atoms x 8 electrons = 16 electrons
- 6 hydrogen atoms x 2 electrons = 12 electrons
- Total = 16 + 12 = 28 electrons
- Since B2H6 has only 12 valence electrons, it is electron deficient because it does not have enough electrons to achieve a stable octet or duet.
- On the other hand, molecules such as C2H6, SiH4, and PH3 have enough valence electrons to achieve a stable octet or duet, so they are not electron deficient.
- Therefore, the correct answer is option **B) B2H6**.
In PO43– ion, the formal charge on each oxygen atom and P—O bond order respectively are- a)–0.75, 0.6
- b)– 0.75, 1.0 [1998]
- c)– 0.75, 1.25
- d)–3, 1.25
Correct answer is option 'C'. Can you explain this answer?
In PO43– ion, the formal charge on each oxygen atom and P—O bond order respectively are
a)
–0.75, 0.6
b)
– 0.75, 1.0 [1998]
c)
– 0.75, 1.25
d)
–3, 1.25
|
Mrprince answered |
C is correct
formal charge =3/4= -0.75
p_o bond order = 1.25
formal charge =3/4= -0.75
p_o bond order = 1.25
In which of the following molecules the central atom does not have sp3 hybridization? [2010]- a)NH+4
- b)CH4
- c)SF4
- d)BF4–
Correct answer is option 'C'. Can you explain this answer?
In which of the following molecules the central atom does not have sp3 hybridization? [2010]
a)
NH+4
b)
CH4
c)
SF4
d)
BF4–
|
Sonal Kulkarni answered |
(a) NH+4 : sp3 hybridisation
(b) CH4: sp3 hybridisation
(c) SF4: sp3 d hybridisation
(d) BF4– : sp3 hybridisation
∴ Correct choice : (c)
(b) CH4: sp3 hybridisation
(c) SF4: sp3 d hybridisation
(d) BF4– : sp3 hybridisation
∴ Correct choice : (c)
Which of the following is paramagnetic ? [NEET 2013]- a)O2-
- b)CN–
- c)NO+
- d)CO
Correct answer is option 'A'. Can you explain this answer?
Which of the following is paramagnetic ? [NEET 2013]
a)
O2-
b)
CN–
c)
NO+
d)
CO
|
Aniket Chawla answered |
Molecular orbital configuration of O2- is
Which one of the following molecules will form a linear polymeric structure due to hydrogen bonding? [2000]
- a)NH3
- b)H2O
- c)HCl
- d)HF
Correct answer is option 'D'. Can you explain this answer?
Which one of the following molecules will form a linear polymeric structure due to hydrogen bonding? [2000]
a)
NH3
b)
H2O
c)
HCl
d)
HF
|
Arnav Chawla answered |
Explanation:
Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom such as nitrogen (N), oxygen (O), or fluorine (F). This type of bonding is a special type of dipole-dipole interaction where the hydrogen atom acts as a bridge between two electronegative atoms.
In the given options, only HF (hydrogen fluoride) contains a hydrogen atom bonded to a highly electronegative atom (fluorine), making it capable of forming hydrogen bonds.
Hydrogen bonding in HF:
- In HF, the hydrogen atom is bonded to fluorine, which is highly electronegative.
- The fluorine atom attracts the electron pair in the H-F bond, creating a partial positive charge on the hydrogen atom and a partial negative charge on the fluorine atom.
- This partial positive charge on the hydrogen atom can then form a hydrogen bond with another electronegative atom, such as another HF molecule.
- The hydrogen bond is formed between the partial positive charge on the hydrogen atom of one HF molecule and the partial negative charge on the fluorine atom of another HF molecule.
Linear polymeric structure:
- In the case of HF, the hydrogen bonds can form between multiple HF molecules, resulting in the formation of a linear polymeric structure.
- The hydrogen bonds act as bridges between the HF molecules, connecting them in a linear chain-like structure.
Other options:
- NH3 (ammonia), H2O (water), and HCl (hydrochloric acid) do not contain a hydrogen atom bonded to a highly electronegative atom, so they cannot form hydrogen bonds.
- NH3 and HCl can form dipole-dipole interactions, but these interactions are not strong enough to result in the formation of a linear polymeric structure.
- H2O can form hydrogen bonds, but the arrangement of the hydrogen bonds in water molecules does not lead to the formation of a linear polymeric structure.
Therefore, the molecule that will form a linear polymeric structure due to hydrogen bonding is HF.
Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom such as nitrogen (N), oxygen (O), or fluorine (F). This type of bonding is a special type of dipole-dipole interaction where the hydrogen atom acts as a bridge between two electronegative atoms.
In the given options, only HF (hydrogen fluoride) contains a hydrogen atom bonded to a highly electronegative atom (fluorine), making it capable of forming hydrogen bonds.
Hydrogen bonding in HF:
- In HF, the hydrogen atom is bonded to fluorine, which is highly electronegative.
- The fluorine atom attracts the electron pair in the H-F bond, creating a partial positive charge on the hydrogen atom and a partial negative charge on the fluorine atom.
- This partial positive charge on the hydrogen atom can then form a hydrogen bond with another electronegative atom, such as another HF molecule.
- The hydrogen bond is formed between the partial positive charge on the hydrogen atom of one HF molecule and the partial negative charge on the fluorine atom of another HF molecule.
Linear polymeric structure:
- In the case of HF, the hydrogen bonds can form between multiple HF molecules, resulting in the formation of a linear polymeric structure.
- The hydrogen bonds act as bridges between the HF molecules, connecting them in a linear chain-like structure.
Other options:
- NH3 (ammonia), H2O (water), and HCl (hydrochloric acid) do not contain a hydrogen atom bonded to a highly electronegative atom, so they cannot form hydrogen bonds.
- NH3 and HCl can form dipole-dipole interactions, but these interactions are not strong enough to result in the formation of a linear polymeric structure.
- H2O can form hydrogen bonds, but the arrangement of the hydrogen bonds in water molecules does not lead to the formation of a linear polymeric structure.
Therefore, the molecule that will form a linear polymeric structure due to hydrogen bonding is HF.
Strongest hydrogen bond is shown by [1992]- a)Water
- b)Ammonia
- c)Hydrogen fluoride
- d)Hydrogen sulphide.
Correct answer is option 'C'. Can you explain this answer?
Strongest hydrogen bond is shown by [1992]
a)
Water
b)
Ammonia
c)
Hydrogen fluoride
d)
Hydrogen sulphide.
|
Charvi Shah answered |
H – F shows strongest H-bonds. Linear combination of two hybridized orbitals leads to the formation of sigma bond.
Among the following the electron deficient compound is : [2000]
- a)BCl3
- b)CCl4
- c)PCl5
- d)SiF4
Correct answer is option 'A'. Can you explain this answer?
Among the following the electron deficient compound is : [2000]
a)
BCl3
b)
CCl4
c)
PCl5
d)
SiF4
|
Snehal Shah answered |
In BCl3 the valence electrons for boron are 6 (3 of boron and 3 of chlorine), so there are two electrons deficient for the octet configuration. Thus, electron deficient molecule is BCl3.
Which of the following statements is not correct for sigma and pi-bonds formed between two carbon atoms? [2003]- a)Sigma-bond deter mines the directi on between carbon atoms but a pi-bond has no primary effect in this regard
- b)Sigma-bond is stronger than a pi-bond
- c)Bond energies of sigma- and pi-bonds are of the order of 264 kJ/mol and 347 kJ/mol, respectively
- d)Free rotation of atoms about a sigma-bond is allowed but not in case of a pi-bond
Correct answer is option 'C'. Can you explain this answer?
Which of the following statements is not correct for sigma and pi-bonds formed between two carbon atoms? [2003]
a)
Sigma-bond deter mines the directi on between carbon atoms but a pi-bond has no primary effect in this regard
b)
Sigma-bond is stronger than a pi-bond
c)
Bond energies of sigma- and pi-bonds are of the order of 264 kJ/mol and 347 kJ/mol, respectively
d)
Free rotation of atoms about a sigma-bond is allowed but not in case of a pi-bond
|
Dipanjan Mehta answered |
As sigma bond is stronger than the π(pi) bond, so it must be having higher bond energy than π (pi) bond.
Which one of the following has the shortest carbon carbon bond length ? [1992]- a)Benzene
- b)Ethene
- c)Ethyne
- d)Ethane
Correct answer is option 'C'. Can you explain this answer?
Which one of the following has the shortest carbon carbon bond length ? [1992]
a)
Benzene
b)
Ethene
c)
Ethyne
d)
Ethane
|
Deepak Joshi answered |
The bond length decreases in the order sp3 > sp2 > sp.
Because of the triple bond, the carbon-carbon bond distance in ethyne is shortest.
Because of the triple bond, the carbon-carbon bond distance in ethyne is shortest.
Which of the following pairs will form the most stable ionic bond ? [1994]- a)Na and Cl
- b)Mg and F
- c)Li and F
- d)Na and F
Correct answer is option 'B'. Can you explain this answer?
Which of the following pairs will form the most stable ionic bond ? [1994]
a)
Na and Cl
b)
Mg and F
c)
Li and F
d)
Na and F
|
Arnab Iyer answered |
The stability of the ionic bond depends upon the lattice energy which is expected to be more between Mg and F due to +2 charge on Mg atom.
Which statement is NOT correct ? [1990]- a)A sigma bond is weaker than a π -bond.
- b)A sigma bond is stronger than a π -bond.
- c)A double bond is stronger than a single bond.
- d)A double bond is shorter than a single bond.
Correct answer is option 'A'. Can you explain this answer?
Which statement is NOT correct ? [1990]
a)
A sigma bond is weaker than a π -bond.
b)
A sigma bond is stronger than a π -bond.
c)
A double bond is stronger than a single bond.
d)
A double bond is shorter than a single bond.
|
Anirban Shah answered |
Understanding Sigma and Pi Bonds
A sigma (σ) bond and a pi (π) bond are two types of covalent bonds that differ in their formation and strength.
Strength of Sigma vs. Pi Bonds
- Sigma bonds are formed by the head-on overlap of atomic orbitals.
- Pi bonds are formed by the side-to-side overlap of atomic orbitals.
- Sigma bonds are generally stronger than pi bonds due to the direct overlap, which allows for a greater electron density between the nuclei of the bonding atoms.
Analysis of Statement A
- Statement A claims that a sigma bond is weaker than a pi bond.
- This statement is incorrect because, as discussed, sigma bonds are stronger due to the nature of their orbital overlap.
Comparison of Single and Double Bonds
- A double bond consists of one sigma bond and one pi bond, making it stronger than a single bond (which consists only of a sigma bond).
- Consequently, a double bond is not only stronger but also shorter than a single bond, due to the additional attraction from the pi bond.
Summary of Correct Statements
- Statement B (Sigma bond is stronger than a pi bond) is correct.
- Statement C (A double bond is stronger than a single bond) is correct.
- Statement D (A double bond is shorter than a single bond) is also correct.
Conclusion
In summary, the incorrect statement is option A, as sigma bonds are indeed stronger than pi bonds, contradicting the claim made in that statement. Understanding these bond types is crucial in grasping the fundamentals of molecular structure and stability.
A sigma (σ) bond and a pi (π) bond are two types of covalent bonds that differ in their formation and strength.
Strength of Sigma vs. Pi Bonds
- Sigma bonds are formed by the head-on overlap of atomic orbitals.
- Pi bonds are formed by the side-to-side overlap of atomic orbitals.
- Sigma bonds are generally stronger than pi bonds due to the direct overlap, which allows for a greater electron density between the nuclei of the bonding atoms.
Analysis of Statement A
- Statement A claims that a sigma bond is weaker than a pi bond.
- This statement is incorrect because, as discussed, sigma bonds are stronger due to the nature of their orbital overlap.
Comparison of Single and Double Bonds
- A double bond consists of one sigma bond and one pi bond, making it stronger than a single bond (which consists only of a sigma bond).
- Consequently, a double bond is not only stronger but also shorter than a single bond, due to the additional attraction from the pi bond.
Summary of Correct Statements
- Statement B (Sigma bond is stronger than a pi bond) is correct.
- Statement C (A double bond is stronger than a single bond) is correct.
- Statement D (A double bond is shorter than a single bond) is also correct.
Conclusion
In summary, the incorrect statement is option A, as sigma bonds are indeed stronger than pi bonds, contradicting the claim made in that statement. Understanding these bond types is crucial in grasping the fundamentals of molecular structure and stability.
In X — H --- Y, X and Y both are electronegative elements- a)Electron density on X will increase and on H will decrease [2001]
- b)In both electron density will decrease
- c)In both electron density will increase
- d)Electron density will decrease on X and will increase on H
Correct answer is option 'A'. Can you explain this answer?
In X — H --- Y, X and Y both are electronegative elements
a)
Electron density on X will increase and on H will decrease [2001]
b)
In both electron density will decrease
c)
In both electron density will increase
d)
Electron density will decrease on X and will increase on H
|
Smruti Sucharita answered |
Bcoz x is more electronegative than H...
Hence option a is correct
Hence option a is correct
H2O has a non zero dipole moment while BeF2 has zero dipole moment because [1989]- a)H2O molecule is linear while BeF2 is bent
- b)BeF2 molecule is linear while H2O is bent
- c)Fluor ine has more electron egativity th an oxygen
- d)Beryllium has more electronegativity than oxygen.
Correct answer is option 'B'. Can you explain this answer?
H2O has a non zero dipole moment while BeF2 has zero dipole moment because [1989]
a)
H2O molecule is linear while BeF2 is bent
b)
BeF2 molecule is linear while H2O is bent
c)
Fluor ine has more electron egativity th an oxygen
d)
Beryllium has more electronegativity than oxygen.
|
|
Aman Sharma answered |
BeF2 is linear and hence has zero dipole moment while H2O, being a bent molecule, has a finite or non-zero dipole moment.
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2D). This is because [2006]- a)in NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions
- b)in NH3 as well as NF3 the atomic dipole and bond dipole are in opposite directions
- c)in NH3 the atomic dipole and bond dipole are in the opposite directions whereas in NF3 these are in the same direction
- d)in NH3 as well as in NF3 the atomic dipole and bond dipole are in the same direction
Correct answer is option 'A'. Can you explain this answer?
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2D). This is because [2006]
a)
in NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions
b)
in NH3 as well as NF3 the atomic dipole and bond dipole are in opposite directions
c)
in NH3 the atomic dipole and bond dipole are in the opposite directions whereas in NF3 these are in the same direction
d)
in NH3 as well as in NF3 the atomic dipole and bond dipole are in the same direction
|
Aniket Basu answered |
Electronegativity Difference
- The electronegativity difference between two atoms in a molecule is a measure of the inequality of sharing of electrons between them.
- In the case of NH3 (ammonia), the electronegativity difference between nitrogen (N) and hydrogen (H) is relatively small, but still greater than that between nitrogen (N) and fluorine (F).
- This is because fluorine is more electronegative than hydrogen, resulting in a larger electronegativity difference between N and F compared to N and H.
Dipole Moment
- The dipole moment of a molecule is a measure of the overall polarity of the molecule.
- It is determined by the magnitude and direction of the individual bond moments within the molecule.
- In the case of NH3, the dipole moment is 1.5 D, which indicates that the molecule is polar.
- In the case of NF3, the dipole moment is 0.2 D, which also indicates that the molecule is polar but to a lesser extent.
Explanation of the Correct Answer (Option A)
- In NH3, the atomic dipole (due to the electronegativity difference between N and H) and the bond dipole (due to the geometry of the molecule) are in the same direction.
- This means that the individual bond moments reinforce each other, resulting in a larger overall dipole moment.
- In NF3, the atomic dipole (due to the electronegativity difference between N and F) and the bond dipole (due to the geometry of the molecule) are in opposite directions.
- This means that the individual bond moments partially cancel each other out, resulting in a smaller overall dipole moment.
Other Options Explanation
- Option B states that in both NH3 and NF3, the atomic dipole and bond dipole are in opposite directions. This is incorrect because the atomic dipole and bond dipole in NH3 are in the same direction.
- Option C states that in NH3, the atomic dipole and bond dipole are in opposite directions, whereas in NF3, they are in the same direction. This is incorrect because in NH3, the atomic dipole and bond dipole are in the same direction.
- Option D states that in both NH3 and NF3, the atomic dipole and bond dipole are in the same direction. This is incorrect because in NF3, the atomic dipole and bond dipole are in opposite directions.
Therefore, the correct answer is option A, where the atomic dipole and bond dipole in NH3 are in the same direction, resulting in a larger dipole moment compared to NF3.
- The electronegativity difference between two atoms in a molecule is a measure of the inequality of sharing of electrons between them.
- In the case of NH3 (ammonia), the electronegativity difference between nitrogen (N) and hydrogen (H) is relatively small, but still greater than that between nitrogen (N) and fluorine (F).
- This is because fluorine is more electronegative than hydrogen, resulting in a larger electronegativity difference between N and F compared to N and H.
Dipole Moment
- The dipole moment of a molecule is a measure of the overall polarity of the molecule.
- It is determined by the magnitude and direction of the individual bond moments within the molecule.
- In the case of NH3, the dipole moment is 1.5 D, which indicates that the molecule is polar.
- In the case of NF3, the dipole moment is 0.2 D, which also indicates that the molecule is polar but to a lesser extent.
Explanation of the Correct Answer (Option A)
- In NH3, the atomic dipole (due to the electronegativity difference between N and H) and the bond dipole (due to the geometry of the molecule) are in the same direction.
- This means that the individual bond moments reinforce each other, resulting in a larger overall dipole moment.
- In NF3, the atomic dipole (due to the electronegativity difference between N and F) and the bond dipole (due to the geometry of the molecule) are in opposite directions.
- This means that the individual bond moments partially cancel each other out, resulting in a smaller overall dipole moment.
Other Options Explanation
- Option B states that in both NH3 and NF3, the atomic dipole and bond dipole are in opposite directions. This is incorrect because the atomic dipole and bond dipole in NH3 are in the same direction.
- Option C states that in NH3, the atomic dipole and bond dipole are in opposite directions, whereas in NF3, they are in the same direction. This is incorrect because in NH3, the atomic dipole and bond dipole are in the same direction.
- Option D states that in both NH3 and NF3, the atomic dipole and bond dipole are in the same direction. This is incorrect because in NF3, the atomic dipole and bond dipole are in opposite directions.
Therefore, the correct answer is option A, where the atomic dipole and bond dipole in NH3 are in the same direction, resulting in a larger dipole moment compared to NF3.
Some of the properties of the two species, NO3- and H3O+ are described below. Which one of them is correct? [2010]- a)Similar in hybridization for the central atom with different structures.
- b)Dissimilar in hybridization for the central atom with different structures.
- c)isostructural with same hybridization for the central atom.
- d)Isostructural with different hybridization for the central atom.
Correct answer is option 'B'. Can you explain this answer?
Some of the properties of the two species, NO3- and H3O+ are described below. Which one of them is correct? [2010]
a)
Similar in hybridization for the central atom with different structures.
b)
Dissimilar in hybridization for the central atom with different structures.
c)
isostructural with same hybridization for the central atom.
d)
Isostructural with different hybridization for the central atom.
|
|
Aniket Chawla answered |
In NO3-2 , nitrogen is in sp2 hybridisation, thus planar in shape. In H3O+ , oxygen is in sp3 hybridisation, thus tetrahedral in shape.
∴ Correct choice : (b)
∴ Correct choice : (b)
Among the following which one is not paramagnetic? [Atomic numbers : Be = 4, Ne = 10, As = 33, Cl = 17] [1998]- a)Cl–
- b)Be+
- c)Ne+2
- d)As+
Correct answer is option 'A'. Can you explain this answer?
Among the following which one is not paramagnetic? [Atomic numbers : Be = 4, Ne = 10, As = 33, Cl = 17] [1998]
a)
Cl–
b)
Be+
c)
Ne+2
d)
As+
|
|
Gowri Nair answered |
Paramagnetic character is based upon presence of unpaired electron
Hence only Cl– do not have unpaired electrons.
In which of the following pairs, the two species are iso-structure? [2007]- a)SO32– and NO3–
- b)BF3 an NF3
- c)BrO3– and XeO3
- d)SF4 and XeF4
Correct answer is option 'C'. Can you explain this answer?
In which of the following pairs, the two species are iso-structure? [2007]
a)
SO32– and NO3–
b)
BF3 an NF3
c)
BrO3– and XeO3
d)
SF4 and XeF4
|
Diya Datta answered |
Hybridization of Br is BrO3–
Total valence elctrons = 7 + 3 × 6 = 25
Charge = –1 hence
Total = 25 + 1 = 26
Total valence elctrons = 7 + 3 × 6 = 25
Charge = –1 hence
Total = 25 + 1 = 26
hybridization = dsp3 hybridization of Xe in XeO3 Total valence electrons
Hybridization = dsp3 In both cases, the structure is trigonal pyramidal.
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