Niels Bohr's atomic model successfully explained the spectrum of:
A. Helium atom
B. Hydrogen atom
C. Oxygen atom
D. Carbon atom
Answer: Option B
Solution (By JKSSB Mock Tests)
Bohr's model (1913) could accurately predict the line spectrum of hydrogen and hydrogen-like ions (single-electron species like He⁺, Li²⁺) by introducing quantized energy levels and angular momentum. It failed for multi-electron atoms due to electron-electron interactions. The model explained the Balmer series of hydrogen. Modern quantum mechanics with Schrödinger equation replaced it. Bohr also introduced the concept of stationary orbits.
Explanation:
CO has a triple bond: one sigma and two pi bonds, with a coordinate covalent character where oxygen donates a lone pair to carbon, forming a bond similar to triple bond. Total shared electrons = 6 (three pairs). Lewis structure shows :C≡O: with formal charges. The bond order is 3. It is isoelectronic with N₂ and CN⁻.
Explanation:
Atomic number (Z) = Mass number (A) – Number of neutrons (N) = 39 – 20 = 19. This is potassium (K). Number of protons equals atomic number. In a neutral atom, electrons also equal Z.
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