atomic structure mcqs

Atomic Structure MCQs

If you are preparing initial tests of Pakistan Army, Navy or PAF then learn the following questions related to the Atomic Structure of chemistry subject. Anyone hoping to work in the Navy Weapon Engineering or Ordnance branches must have a solid background in atomic structure. Atomic structure MCQs provide a thorough assessment of candidates’ understanding and skill in this branch of chemistry.

These questions cover a wide range of subjects, including as atomic orbitals, quantum numbers, and periodic table structure. Candidates can boost their chances of getting hired in these Navy branches by preparing these atomic structure multiple-choice questions (MCQs) attentively. This will help them face the academic exams with confidence.

Atomic Structure MCQ (Part-2)

  • An atom can have a maximum of ________ electrons in its second shell. (8)
  • The third shell of an atom can contain a maximum of ________ electrons. (18)
  • The electron configuration of helium (He) is ________. (1s²)
  • The electron configuration of carbon (C) is ________. (1s² 2s² 2p²)
  • The electron configuration of oxygen (O) is ________. (1s² 2s² 2p⁴)
  • A typical (N) electron configuration is ________. (1s² 2s² 2p³)
  • The electron configuration of sodium (Na) is ________. (1s² 2s² 2p⁶ 3s¹)
  • The electron configuration of chlorine (Cl) is ________. (1s² 2s² 2p⁶ 3s² 3p⁵)
  • The base number (n) describes the electron in the ____ atom. (energy level)
  • The value of prime (n) can be any positive ________. (integer)
  • The azimuthal quantum number (l) describes the electron at the ________ energy level. (subplane or orbit)
  • The value of the azimuth quantum number (l) varies from ________ to (n – 1). (0)
  • The magnetic quantum number (m_l) describes the ________ orbit of an electron. (orientation or spatial orientation)
  • The value of magnetic quantum number (m_l) ranges from ________ to +l. (–l)
  • The spin number (m_s) describes the ________ of an electron. (spin direction)
  • The value of spin quantum number (m_s) can be either +1/2 (spin ________) or –1/2 (spin ________). (up, down)
  • The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers, including the quantum number ________. (spin)

Structure of Atom MCQs

In the highly competitive world of Forces jobs like the Navy Education Branch, a solid grasp of atomic structure is essential for covering Chemistry subject. Moreover, following mcqs are helpful to cover the area of physics. Candidates can evaluate their knowledge and pinpoint areas that need more focus by using the structure of atoms MCQs on this subject.

Numerous topics are covered in these atomic structure multiple-choice questions (MCQs), such as nuclear chemistry, electron configuration, and atomic spectra. Through the practice of these atomic structure multiple-choice questions, applicants can improve their performance on academic exams related to various Navy branches and deepen their understanding of atomic structure.

Atomic Structure MCQ (Part-3)

  • The maximum number of electrons that can fit into a certain energy level is given by the formula ________, where n represents the principal quantum number. (2n2)
  • The maximum number of sublevels in an energy level is equal to the value of the ________ quantum number (n). (main)
  • The number of orbitals within a sublevel is ________, where l represents the azimuthal quantum number. (2l + 1)
  • The maximum number of electrons that can fit into one orbital is ________. (2)
  • The electron configuration of an atom is determined by the number of orbitals occupied by ________. (quantum)
  • Quantum numbers fully describe the ________ state of an electron in an atom. (quantum or physical)
  • The Aufbau principle states that electrons fill atomic orbitals in order of ________ energy. (increases)
  • According to the Aufbau principle, electrons first occupy the ________ energy level before moving to a higher energy level. (smallest)
  • The Aufbau principle determines the order in which ________ are filled in an atom. (orbitals)
  • The Aufbau principle helps explain the configuration of ________ electrons. (atoms)
  • The principle of Aufbau is based on the principle of ________ exclusion. (Pauli)
  • According to the Aufbau principle, the 1st orbit is filled before the ________ orbit. (2s)
  • The Aufbau principle predicts that the 2p orbitals will be filled after the ________ orbital. (2s)

MCQs on Atomic Structure

A thorough understanding of atomic structure is necessary for those who want to work in PAF Administration & Special Duty Branch or PAF Aeronautical Engineering. Important ideas include atomic models, periodic patterns, and chemical bonding are covered in MCQs on atomic structure.

Candidates can acquaint themselves with the kinds of questions they will probably face in academic exams by practicing these atomic structure multiple-choice questions. With this training, they will be able to succeed in their pursuit of a PAF profession and take the tests with confidence.

Atomic Structure MCQ (Part-4)

  • The Aufbau principle states that the 3s orbital is filled before the ________ orbital. (3p)
  • According to the Aufbau principle, 3d orbitals are filled after ________ orbitals. (4s)
  • The Aufbau principle explains why the electron configuration of oxygen is ________. (1s² 2s² 2p⁴)
  • The electron configuration of the type according to the Aufbau principle is ________. (1s² 2s² 2p³)
  • The Aufbau principle predicts that the electron configuration of calcium is ________. (1s² 2s² 2p⁶ 3s² 3p⁶ 4s²)
  • The Aufbau principle explains why the electron configuration of chromium is ________. (1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵)
  • According to the Aufbau principle, the electron configuration of copper is ________. (1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰)
  • The Aufbau principle is necessary to understand the ________ filling of the electron in the periodic table. (subshells)
  • Valence electrons are electrons found in the ________ energy level of an atom. (external)
  • Valence electrons are involved in the formation of ________ between atoms. (chemical bonds)
  • The number of valence electrons determines the ________ properties of an element. (chemical)
  • Elements in the same group of the periodic table have the same number of ________ electrons. (valence)
  • The valence electrons of an atom are found in its ________. (outer energy level or valence shell)
  • An atom can have a maximum number of valence electrons of ________. (8)
  • Elements in group 1 of the periodic table have ________ valence electrons. (1)
  • Elements in group 2 of the periodic table have ________ valence electrons. (2).
  • Elements in group 13 of the periodic table have ________ valence electrons. (3)
  • Elements in group 17 of the periodic table have ________ valence electrons. (7)
  • Elements in group 18 of the periodic table, also known as noble gases, have ________ valence electrons. (8)
  • Transition metals have ________ valence electrons because they can occupy several energy levels. (changing or variable)
  • The number of valence electrons in an atom can be determined by looking at its ________. (group or column)
  • Carbon has ________ valence electrons. (4)
  • Oxygen has ________ valence electrons. (6)
  • Hund’s rule states that electrons occupy ________ orbitals with the same energy before pairing. (separate or single)
  • According to Hund’s rule, electrons with ________ spin first fill degenerate orbitals. (parallel or same)
  • Hund’s rule helps explain the distribution of electrons in ________. (sublevels or orbitals)
  • Application of Hund’s rule helps determine the ________ configuration of atoms. (electron or ground state)
  • Hund’s rule is based on the ________ exclusion principle. (Pauli)
  • Wunf’s rule states that each electron in a set of degenerate orbitals occupies an empty orbital before pairing because this minimizes ____ repulsion. (electron-electron or interelectron)
  • Hund’s rule predicts that the electron configuration of carbon is ________. (1s² 2s² 2p²)
  • According to Hund’s rule, the electron configuration of nitrogen is ________. (1s² 2s² 2p³)
  • According to Hund’s law, the electron configuration of oxygen is ________. (1s² 2s² 2p⁴)
  • Hund’s law explains why the electron configuration of chromium is ________. (1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵)

Structure of Atom  Multiple Choice Questions

Atomic structure multiple-choice questions are important for the armed forces, the Technical Cadet Course, Army Education Officers, Army EME Officers, and civilians looking for jobs in the armed services. These multiple-choice questions address a broad range of atomic structure-related subjects, such as electron configurations, isotopes, and atomic theory.

Interested candidates can improve their knowledge of atomic structure and raise their chances of success in their chosen career pathways within the defense forces by using these multiple-choice questions as study tools.

Atomic Structure MCQ (Part-5)

  • According to Hund’s rule, the electron configuration of copper is ________. (1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰)
  • Hund’s rule predicts that nitrogen has ________ unpaired electrons in its electron configuration. (3)
  • Hund’s rule states that degenerate orbitals with unpaired electrons have the same ________. (spin or spin state)
  • Hund’s law is necessary to understand ________ fill atoms and ions. (sublevels or orbitals)
  • Hund’s rule plays a role in determining the magnetic properties and ________ of atoms. (chemical reactivity)
  • The Pauli exclusion principle states that no two electrons in an atom can have the same set of ________. (four quantum numbers)
  • According to Pauli’s exclusion principle, electrons must have ________ spin if they are in the same orbit. (opposite or different)
  • Paul’s principle of exclusion helps explain the stability and organization of ________. (electrons in atoms)
  • The Pauli exclusion principle is a consequence of the ________ nature of electrons. (fermionic or quantum)
  • The Pauli exclusion principle is one of the basic principles of ________. (quantum mechanics)
  • According to the Pauli exclusion principle, electrons in the same orbital must have different ________. (spin quantum numbers)
  • The Pauli exclusion principle prevents electrons from occupying the ________ quantum state in an atom. (identical or same)
  • Paul’s exclusion principle applies to all ________, including those on the same inferior level. (electrons)
  • Pauli’s exclusion principle helps determine the configuration of electrons and the arrangement of electrons in ________. (atoms)
  • The Pauli exclusion principle is named after the Austrian physicist ________. (Wolfgang Pauli)
  • Paul’s principle of exclusion is a fundamental principle for understanding ________ behavior. (fermions or particles with half-integer spin)
  • The Pauli exclusion principle is essential to explain the filling of the periodic table and the ________ of the electron. (orbitals or energy levels)
  • The Pauli exclusion principle is a consequence of the ________ principle, which states that the wave function of identical particles must be asymmetric. (exchange or symmetry)
  • The Pauli exclusion principle allows ________ to form within atoms and bonds between atoms. (chemical bonds)
  • The Pauli exclusion principle ensures that the electrons inside an atom have a distribution of ________ quantum numbers. (unique or distinctive).

See More

  • Chemistry MCQs with Answers (Download)
  • Past Papers of Chemistry for Navy Tests (Download)
  • Pak Navy Tests MCQs of Chemistry with Answers (Download)
  • Online Practice Tests of Basic Chemistry Tests (Download)
  • Free online Practice Tests of Chemistry Tests MCQs (Download)

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