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Recent Channel Posts

📖MATHEMATICS

📝NOTE-11

👨‍🏫Mathematical Applications in business

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🔔Remedial chemistry questions with answers👇
https://youtu.be/BZaEw5nREWs

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🔔Top remedial physics questions with explanations👇
https://youtu.be/5FRqEFf4xSU?si=PIapmqGzMJwA_4Ha

1000

16:47

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25. B) Brittleness
🔷Metals are typically ductile and malleable, not brittle.

26. A) Layers of atoms can slide without breaking bonds
🔷Delocalized electrons allow metal ions to move without fracturing.

27. C) Metallic bonding
🔷The electron-sea model describes metallic bonding.

28. C) Soluble in polar solvents
🔷Ionic compounds dissolve in polar solvents like water.

29. B) Molecules with delocalized electrons
🔷Resonance describes structures where electrons are delocalized (e.g., CO₃²⁻).

30. B) 109.5°
🔷Tetrahedral molecules (e.g., CH₄) have ~109.5° bond angles.

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24. Metallic bonding is best described as:
a) A sea of delocalized electrons
b) Transfer of electrons
c) Sharing of electron pairs
d) Hydrogen bonding

25. Which property is NOT typical of metals?
a) High electrical conductivity
b) Brittleness
c) Malleability
d) High melting point

26. Metals are malleable because:
a) Layers of atoms can slide without breaking bonds
b) They have low density
c) They form covalent networks
d) They are brittle

27. The electron-sea model explains:
a) Ionic bonding
b) Covalent bonding
c) Metallic bonding
d) Hydrogen bonding

28. Which of the following is a property of ionic compounds?
a) Low melting point
b) Conduct electricity in solid state
c) Soluble in polar solvents
d) Exist as discrete molecules

29. Resonance structures are used to describe:
a) Molecules with single Lewis structures
b) Molecules with delocalized electrons
c) Only ionic compounds
d) Only metals

30. The bond angle in a tetrahedral molecule is approximately:
a) 90°
b) 109.5°
c) 120°
d) 180°

📝Answers and Explanations:

1. B) To attain noble gas electronic configuration
🔷Atoms bond to achieve stability, often by having 8 valence electrons (Octet Rule).

2. C) Ionic bond
🔷Ionic bonds form when electrons are completely transferred from a metal to a nonmetal.

3. C) Soluble in water and polar solvents
🔷Ionic compounds dissolve in polar solvents due to strong ion-dipole interactions.

4. B) Shared
🔷Covalent bonds involve electron sharing between atoms.

5. B) H₂
🔷Non-polar bonds occur between identical atoms (equal electronegativity).

6. A) Both electrons are donated by one atom
🔷A coordinate bond forms when one atom provides both shared electrons.

7. B) Gain, lose, or share electrons to have 8 valence electrons
🔷The Octet Rule describes atoms striving for 8 valence electrons.

8. B) BF₃
🔷BF₃ is electron-deficient (only 6 valence electrons around B).

9. B) The number of electron pairs around the central atom (VSEPR theory)
🔷VSEPR theory predicts molecular geometry based on electron pair repulsion.

10. C) Occupy more space than bonding pairs
🔷Lone pairs repel more strongly, affecting bond angles.

11. B) CO₂
🔷CO₂ has sp hybridization and a linear shape (180° bond angle).

12. C) Electrons are shared unequally
🔷Polar bonds result from unequal sharing due to electronegativity differences.

13. B) H₂O
🔷H₂O is polar due to its bent shape and lone pairs on oxygen.

14. B) Overlapping of atomic orbitals
🔷Valence Bond Theory explains bonds via orbital overlap.

15. B) Head-on overlapping of orbitals
🔷Sigma bonds form from direct overlap along the internuclear axis.

16. A) Sidewise overlapping of p-orbitals
🔷Pi bonds form from parallel p-orbital overlap.

17. B) Atomic orbitals of the same atom with similar energy
🔷Hybridization mixes orbitals (e.g., s and p) to form new degenerate orbitals.

18. C) Tetrahedral
🔷sp³ hybridization leads to a tetrahedral geometry (e.g., CH₄).

19. B) CO₂
🔷CO₂ has sp hybridization (linear geometry).

20. B) The formation of molecular orbitals from atomic orbitals
🔷MOT describes bonding via molecular orbital combinations.

21. B) Lower energy than atomic orbitals
🔷BMOs are stabilizing (lower energy) due to constructive interference.

22. A) (Number of electrons in BMO - Number of electrons in ABMO) / 2
🔷Bond order = ½(BMO e⁻ – ABMO e⁻).

23. B) Paramagnetic
🔷Paramagnetic substances have unpaired electrons (attracted to magnetic fields).

24. A) A sea of delocalized electrons
🔷Metallic bonding involves mobile electrons surrounding cations.

1100

05:25

02.05.2025

Crypto
🧪CHEMISTRY

♻️30 Multiple Choice Questions on Chemical Bonding and Structure

✍️Questions:

1. What is the primary reason atoms form chemical bonds?
a) To increase their energy
b) To attain noble gas electronic configuration
c) To become less stable
d) To gain more protons

2. Which type of bond involves the complete transfer of electrons from one atom to another?
a) Covalent bond
b) Metallic bond
c) Ionic bond
d) Hydrogen bond

3. Ionic compounds are generally:
a) Soluble in non-polar solvents
b) Poor conductors of electricity in molten state
c) Soluble in water and polar solvents
d) Have low melting and boiling points

4. In a covalent bond, electrons are:
a) Transferred
b) Shared
c) Lost
d) Donated

5. Which of the following is an example of a non-polar covalent bond?
a) HCl
b) H₂
c) HBr
d) NaCl

6. A coordinate covalent bond is formed when:
a) Both electrons are donated by one atom
b) Electrons are transferred
c) Electrons are shared equally
d) Electrons are delocalized

7. The Octet Rule states that atoms tend to:
a) Lose all their electrons
b) Gain, lose, or share electrons to have 8 valence electrons
c) Always share electrons
d) Form only ionic bonds

8. Which molecule is an exception to the Octet Rule?
a) CO₂
b) BF₃
c) H₂O
d) NH₃

9. The shape of a molecule is determined by:
a) The number of protons
b) The number of electron pairs around the central atom (VSEPR theory)
c) The color of the atoms
d) The atomic mass

10. In VSEPR theory, lone pairs of electrons:
a) Do not affect molecular geometry
b) Occupy less space than bonding pairs
c) Occupy more space than bonding pairs
d) Are always shared

11. Which of the following has a linear molecular geometry?
a) H₂O
b) CO₂
c) NH₃
d) CH₄

12. A polar covalent bond occurs when:
a) Electrons are shared equally
b) Electrons are transferred
c) Electrons are shared unequally
d) Electrons are delocalized

13. Which molecule is polar?
a) CO₂
b) H₂O
c) CH₄
d) CCl₄

14. The Valence Bond Theory explains covalent bonding through:
a) Electron transfer
b) Overlapping of atomic orbitals
c) Delocalized electrons
d) Ionic interactions

15. A sigma (σ) bond is formed by:
a) Sidewise overlapping of orbitals
b) Head-on overlapping of orbitals
c) Donation of electrons
d) Hybridization

16. A pi (π) bond is formed by:
a) Sidewise overlapping of p-orbitals
b) Head-on overlapping of s-orbitals
c) Transfer of electrons
d) Hybridization

17. Hybridization is the mixing of:
a) Atomic orbitals of different atoms
b) Atomic orbitals of the same atom with similar energy
c) Protons and neutrons
d) Electrons and protons

18. sp³ hybridization results in which molecular geometry?
a) Linear
b) Trigonal planar
c) Tetrahedral
d) Octahedral

19. Which molecule has sp hybridization?
a) CH₄
b) CO₂
c) NH₃
d) H₂O

20. The Molecular Orbital Theory (MOT) describes:
a) Only ionic bonds
b) The formation of molecular orbitals from atomic orbitals
c) Only metallic bonds
d) Only covalent bonds

21. A bonding molecular orbital (BMO) has:
a) Higher energy than atomic orbitals
b) Lower energy than atomic orbitals
c) The same energy as atomic orbitals
d) No energy

22. The bond order is calculated as:
a) (Number of electrons in BMO - Number of electrons in ABMO) / 2
b) (Number of protons + Number of neutrons)
c) (Number of lone pairs)
d) (Number of sigma bonds)

23. A molecule with unpaired electrons is:
a) Diamagnetic
b) Paramagnetic
c) Ferromagnetic
d) Non-magnetic

1100

05:25

02.05.2025

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