Atomic Structure NEET questions focus on essential standards like the discovery of the atom, atomic fashions, subatomic particles, quantum numbers, digital configuration, and periodic residences. These questions check a student’s expertise of the Bohr version, the dual nature of be counted, Heisenberg’s uncertainty principle, and concepts associated with isotopes and isobars. Mastering those topics enables college students address NEET’s competitive exam with accuracy and self belief, as they may be vital in grasping the fundamentals of chemistry.
- Introduction to Atomic Structure for NEET
- Download: Atomic Structure
- Key Concepts of Atomic Structure
- Bohr’s Atomic Model
- Quantum Mechanical Model of the Atom
- Electron Configuration
- Dual Nature of Matter and Radiation
- Important Formulas in Atomic Structure
- Practice NEET Questions on Atomic Structure
- FAQs about Atomic Structure
Introduction to Atomic Structure for NEET
The subject matter of Atomic Structure is essential for NEET aspirants, because it bureaucracy the idea of know-how count number at the microscopic degree. Atomic shape covers key standards just like the discovery of subatomic particles, atomic models, quantum numbers, and electronic configuration. NEET questions on atomic structure regularly require a stable draw close of Bohr’s version, Heisenberg’s uncertainty precept, and quantum mechanical standards. These questions determine a candidate’s capability to understand the association and behavior of electrons in atoms, essential for learning subjects in chemistry and physics. Practicing atomic structure NEET questions facilitates students develop analytical capabilities and enhances their hassle-solving skills, making this subject matter a essential a part of their guidance for reaching high rankings inside the exam.
Importance in NEET Syllabus
Atomic structure is a fundamental topic in the NEET syllabus for numerous reasons:
- Foundation for Chemistry: Understanding atomic structure is critical for knowledge in other areas of chemistry, such as chemical bonding, periodic properties, and reactions.
- Application in Physics: Atomic structure also has applications in physics, particularly in areas like nuclear physics and spectroscopy.
- Conceptual Understanding: A strong grasp of atomic structure helps develop conceptual knowledge and problem-solving abilities, which are critical for success in NEET.
Download: Atomic Structure
| Title | Download |
|---|---|
| Atomic Structure NEET Questions with Answer |
Key Concepts of Atomic Structure
| Concept | Definition | Example |
|---|---|---|
| Subatomic Particles | Particles that make up an atom. | Protons, neutrons, electrons |
| Proton | Positively charged particle found in the nucleus. | Hydrogen atom has 1 proton. |
| Neutron | Neutral particle found in the nucleus. | Deuterium atom has 1 proton and 1 neutron. |
| Electron | Negatively charged particle that orbits the nucleus. | Hydrogen atom has 1 electron. |
| Atomic Number | The number of protons in the nucleus of an atom. | Carbon has an atomic number of 6. |
| Mass Number | The sum of the number of protons and neutrons in the nucleus. | Carbon-12 has a mass number of 12. |
| Isotopes | Atoms of the same element with different numbers of neutrons. | Hydrogen has three isotopes: protium, deuterium, and tritium. |
| Isobars | Atoms of different elements with the same mass number. | Carbon-14 and nitrogen-14 are isobars. |
| Isotones | Atoms of different elements with the same number of neutrons. | Boron-10 and carbon-11 are isotones. |
Bohr’s Atomic Model
Postulates of Bohr’s Model
- Quantized Energy Levels: Electrons can only exist in unique, discrete energy levels or shells around the nucleus. These energy levels are denoted by the principal quantum number (n), where n = 1, 2, 3, and so on.
- No Radiation During Stationary States: When an electron is in a specific energy level, it does not emit or absorb energy. It remains in a stable state.
- Energy Absorption and Emission: An electron can move from a lower energy level to a higher one by absorbing energy (e.g., from light). Conversely, it can move from a higher energy level to a lower one by emitting energy (e.g., as light). The energy difference between the levels corresponds to the energy of the absorbed or emitted photon.
Energy Levels and Orbits
- The energy levels are often depicted as circular orbits around the nucleus.
- The lower energy levels (n = 1, 2) are closer to the nucleus, while the higher energy levels (n = 3, 4) are farther away.
- The maximum number of electrons that can be accommodated in a specific energy level is given by 2n², where n is the principal quantum number.
Limitations of Bohr’s Model
- Inability to Explain Spectra of Multi-electron Atoms: The model could not accurately explain the spectra of atoms with more than one electron.
- Violation of Heisenberg’s Uncertainty Principle: The model assumes that electrons have specific orbits, which contradicts the uncertainty principle, which states that it is impossible to simultaneously determine the exact position and momentum of an electron.
- Ineffectiveness for Relativistic Speeds: The model does not account for relativistic effects, which become significant for electrons moving at high speeds (near the speed of light) in heavier atoms.
Quantum Mechanical Model of the Atom
| Concept | Definition |
|---|---|
| Quantum Numbers | Numbers that describe the nature of an electron in an atom. |
| Principal Quantum Number (n) | Determines the power level or shell of an electron. |
| Azimuthal Quantum Number (l) | Determines the shape of the orbital. |
| Magnetic Quantum Number (ml) | Determines the orientation of the orbital in space. |
| Spin Quantum Number (ms) | Describes the intrinsic spin of an electron. |
| Orbitals | Regions of space where there is a high probability of locating an electron. |
| S Orbital | Spherical shape. |
| P Orbital | Dumbbell shape. |
| D Orbital | Cloverleaf shape. |
| F Orbital | More complex shapes. |
| Aufbau Principle | Electrons fill orbitals in order of increasing energy. |
| Pauli’s Exclusion Principle | No two electrons in an atom can have the same set of quantum numbers. |
| Hund’s Rule | Orbitals within a subshell are filled singly with electrons of the same spin before pairing occurs. |
Electron Configuration
Electron configuration is a shorthand notation that suggests the arrangement of electrons in the orbitals of an atom. It follows a few fundamental policies:
- Aufbau Principle: Electrons fill orbitals in order of increasing energy.
- Pauli Exclusion Principle: No two electrons in an atom can have the equal set of quantum numbers.
- Hund’s Rule: Orbitals within a subshell are crammed singly with electrons of the same spin earlier than pairing takes place.
Here’s an example of the way to write the electron configuration for carbon:
1s² 2s² 2p²
This suggests that carbon has:
- 2 electrons in the 1s orbital
- 2 electrons inside the 2s orbital
- 2 electrons in the 2p orbitals
Stability of Half-Filled and Fully Filled Orbitals
Orbitals that are 1/2-stuffed or absolutely stuffed are typically extra stable than the ones that are partly crammed. This is because of the following motives:
- Electron-Electron Repulsion: When an orbital is half-stuffed, the electrons are paired, that could result in elevated electron-electron repulsion.
- Exchange Energy: In 1/2-stuffed or completely stuffed orbitals, there are more possible approaches for electrons to change positions, which ends up in a decrease energy state.
For example, the electron configuration for chromium is:
1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹
Dual Nature of Matter and Radiation
De Broglie’s Hypothesis
Louis de Broglie proposed that count number, like mild, famous each particle and wave homes. His hypothesis, called de Broglie’s wavelength equation, relates the momentum (p) of a particle to its wavelength (λ):
λ = h / p
where:
- h is Planck’s consistent (6.626 × 10-34 Js)
This equation implies that each one debris have a wave-like nature, and the wavelength of a particle is inversely proportional to its momentum. For macroscopic objects, the wavelength is so small that it isn’t always observable. However, for microscopic particles like electrons, the wavelength may be extensive.
Heisenberg’s Uncertainty Principle
Werner Heisenberg formulated the uncertainty principle, which states that it is impossible to simultaneously decide the precise role and momentum of a particle with absolute precision. The made from the uncertainties in function (Δx) and momentum (Δp) is always more than or identical to a constant:
Δx * Δp ≥ h / 4π
This precept arises from the wave-particle duality of count number. If a particle is localized in space (small Δx), its momentum must be unsure (big Δp). Conversely, if a particle has a well-defined momentum (small Δp), its position need to be unsure (huge Δx).
Important Formulas in Atomic Structure
| Concept | Formula | Description |
|---|---|---|
| Rydberg Equation | 1/λ = R_H (1/n₁² – 1/n₂²) | Calculates the wavelengths of spectral lines in hydrogen. |
| Energy of Electrons | E = – (k * Z²) / n² | Energy of an electron in a hydrogen-like atom, where k is a constant and Z is the atomic number. |
| Wavelength and Frequency | λ = c / f | Relationship between wavelength (λ), frequency (f), and the speed of light (c). |
| Energy and Frequency | E = h * f | Relationship between energy (E) and frequency (f), where h is Planck’s constant. |
Practice NEET Questions on Atomic Structure
Multiple Choice Questions with Solutions
| Question | Answer | Explanation |
|---|---|---|
| Which subatomic particle has the least mass? | Electron | Electrons have a mass of approximately 9.11 × 10⁻³¹ kg, which is significantly smaller than protons and neutrons. |
| What is the maximum number of electrons that can be accommodated in the 3d subshell? | 10 | The maximum number of electrons in a subshell is given by 2(2l + 1), where l is the azimuthal quantum number. For the 3d subshell, l = 2, so the maximum number of electrons is 10. |
| Which of the following is an isotope of hydrogen? | Deuterium | Deuterium has one proton and one neutron in its nucleus, while protium has only one proton. |
Assertion-Reason Questions
| Assertion | Reason |
|---|---|
| The electron configuration of nitrogen is 1s² 2s² 2p³. | Nitrogen has 7 electrons. |
| The Bohr model is relevant to multi-electron atoms. | The Bohr model can accurately give an explanation for the spectra of multi-electron atoms. |
FAQs about Atomic Structure
1. What is the importance of atomic structure in NEET?
Ans: Atomic shape paperwork the basis of chemistry and enables in know-how elements, isotopes, ions, and their behavior in reactions. It’s a fundamental subject matter in NEET.
2. Which subjects from atomic structure are maximum crucial for NEET?
Ans: Key topics consist of Bohr’s model, quantum numbers, Heisenberg’s uncertainty precept, electronic configuration, and atomic orbitals.
3. What form of questions are asked on atomic shape in NEET?
Ans: Conceptual questions, numerical problems, and alertness-primarily based questions related to models, energy degrees, and electronic transitions are commonplace.
4. Are formulas crucial for atomic shape questions in NEET?
Ans: Yes, formulation like the ones associated with strength tiers, Bohr’s radius, and de Broglie wavelength are regularly utilized in solving questions.
5. How many questions are typically from atomic structure in NEET?
Ans: Usually, 1-2 questions from atomic structure appear within the Chemistry segment of NEET.
