Chemistry Chapter: Electronic Configuration
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Questions and Answers

What does the Pauli Exclusion Principle state?

  • No two electrons in an atom can have the same set of four quantum numbers. (correct)
  • Atoms of different elements can have identical atomic structures.
  • Electrons will occupy degenerate orbitals singly before pairing begins.
  • Electrons fill orbitals starting from the lowest energy level to the highest.

    • Which of the following correctly describes an atomic orbital?

  • It is a region in space where there is a high probability of finding an electron. (correct)
  • It refers to the average distance of an electron from the nucleus.
  • It is solely determined by the magnetic quantum number.
  • It is a fixed location of electrons around the nucleus.

    • Which principle explains why electrons first occupy separate orbitals in a subshell?

  • Pauli Exclusion Principle
  • Aufbau Principle
  • Hund’s Rule of Maximum Multiplicity (correct)
  • Dalton's Atomic Theory

    • According to Dalton's Atomic Theory, what can be said about the atoms of different elements?

    <p>They differ in size, mass, and chemical properties.</p> Signup and view all the answers

    What is the significance of the Aufbau Principle in constructing electronic configurations?

    <p>It dictates the order in which electrons populate orbitals.</p> Signup and view all the answers

    In constructing the abbreviated electronic configuration for an element, which of the following should be included?

    <p>Only the noble gas preceding the element.</p> Signup and view all the answers

    What happens to the electronic configuration of a simple anion?

    <p>It gains electrons, leading to an overall negative charge.</p> Signup and view all the answers

    What is the maximum number of electrons that can occupy the p sublevel?

    <p>6</p> Signup and view all the answers

    Which principle states that no more than two electrons can occupy a single orbital?

    <p>Pauli Exclusion Principle</p> Signup and view all the answers

    According to Hund's Rule, how do electrons fill degenerate orbitals?

    <p>Electrons fill one at a time before any pairing.</p> Signup and view all the answers

    What is the electronic configuration of the element with atomic number 29?

    <p>1s2 2s2 2p6 3s2 3p6 4s1 3d10</p> Signup and view all the answers

    What distinguishes the electron configuration of chromium and copper from others?

    <p>They exhibit half-filled or completely filled d orbitals for extra stability.</p> Signup and view all the answers

    What fundamental process is described in the statement regarding chemical reactions?

    <p>Atoms can be separated, combined, or rearranged.</p> Signup and view all the answers

    What did J.J. Thomson discover using cathode ray tubes?

    <p>The electron as a subatomic particle.</p> Signup and view all the answers

    What is the significance of Thomson's ratio of electric charge to mass for the electron?

    <p>It helps understand the properties of electrons.</p> Signup and view all the answers

    In Thomson's plum-pudding model, how are electrons arranged?

    <p>They are embedded within a positively charged sphere.</p> Signup and view all the answers

    What did Rutherford conclude about the atom's structure from his experiments?

    <p>All positive charges are located in the nucleus.</p> Signup and view all the answers

    Which type of particle did Rutherford use in his experiments to discover the nucleus?

    <p>Alpha particles.</p> Signup and view all the answers

    What analogy did Rutherford use to describe his unexpected experimental results?

    <p>Shooting a bullet at a piece of tissue paper.</p> Signup and view all the answers

    What concept regarding atomic structure did Rutherford's findings challenge?

    <p>Positive charges are evenly distributed in an atom.</p> Signup and view all the answers

    What information is sought about electron arrangements in the context of atomic structure?

    <p>Their organization outside the nucleus.</p> Signup and view all the answers

    What shape does an s-orbital have?

    <p>Sphere shaped</p> Signup and view all the answers

    How many orientations do p-orbitals have?

    <p>Three</p> Signup and view all the answers

    What is the maximum number of electrons that can occupy one atomic orbital?

    <p>2</p> Signup and view all the answers

    Which of the following is true about d-orbitals?

    <p>They have different shapes than s- and p-orbitals</p> Signup and view all the answers

    What type of symmetry is associated with the p-orbital?

    <p>Dumbbell</p> Signup and view all the answers

    How are the d-orbitals classified in terms of energy?

    <p>They are degenerate</p> Signup and view all the answers

    Which description applies to the p-orbitals' shape?

    <p>They are dumbbell shaped.</p> Signup and view all the answers

    How many sets of d-orbitals exist for each energy level?

    <p>Five</p> Signup and view all the answers

    Which orbital type has a spherical shape and increases in energy and distance from the nucleus?

    <p>s-orbital</p> Signup and view all the answers

    What characterizes the energy sublevels in relation to atomic orbitals?

    <p>They contain groups of orbitals with the same energy.</p> Signup and view all the answers

    What does the Uncertainty Principle state about momentum and position?

    <p>The more precisely the position is determined, the less precisely the momentum is known.</p> Signup and view all the answers

    What does the Schrodinger Wave Equation help to determine?

    <p>The probability of finding an electron within a particular position in an atom.</p> Signup and view all the answers

    What are atomic orbitals primarily used for?

    <p>To help understand how atoms interact with each other.</p> Signup and view all the answers

    What does not describe atomic orbitals?

    <p>They always have the same size and energy.</p> Signup and view all the answers

    What is true about the s orbitals?

    <p>They exist at varying distances from the nucleus depending on energy level.</p> Signup and view all the answers

    What is a defining characteristic of atomic orbitals?

    <p>They can exist in multiple dimensions, depending on their shape.</p> Signup and view all the answers

    Why is it important to understand electronic configurations?

    <p>They influence how atoms interact and bond with one another.</p> Signup and view all the answers

    Which statement about the Schrodinger Equation is inaccurate?

    <p>It only applies to particles that are larger than atoms.</p> Signup and view all the answers

    Which of the following is not a feature of atomic orbitals?

    <p>They always contain two electrons.</p> Signup and view all the answers

    During the Solvay Conference of 1927, what significant concept was further discussed?

    <p>Wave-particle duality of matter.</p> Signup and view all the answers

    Study Notes

    Fundamentals of Medicinal and Pharmaceutical Chemistry

    • This course covers the fundamental principles of medicinal and pharmaceutical chemistry.
    • The focus is on electronic configurations of atoms and ions relevant to physiology.
    • Students should consult General Chemistry – The Essential Concepts by Chang and Goldsby (7th edition).
    • Specific sections to review are 2.1, 2.2, 2.5, 7.8, and 7.9.

    Learning Outcomes

    • Students should be able to describe the major contributions of scientists (Thomson, Rutherford, Bohr, Einstein, deBroglie, Heisenberg, and Schrodinger) that led to our understanding of atomic structure.
    • Differentiate between the different types of atomic orbitals (s, p, and d) based on their shapes and energies.
    • Define and explain the concepts of Pauli Exclusion Principle, Aufbau Principle and Hund's Rule of Maximum Multiplicity.
    • Construct electronic configurations for the first 30 elements following the principles of electron filling order in the periodic table.
    • Construct the electronic configurations of ions (cations and anions).

    Dalton's Atomic Theory

    • Elements are comprised of extremely small particles called atoms.
    • All atoms of a particular element are identical in size, mass, and chemical properties.
    • Atoms of different elements are different.
    • Compounds composed of atoms of more than one element; with atoms of various elements combined in definite proportions.
    • Chemical reactions result in the rearrangement of atoms and do not destroy them.

    Early Atomic Structure - Thomson

    • Thomson discovered the electron.
    • Using cathode ray tubes and knowledge of electromagnetism, he calculated the charge-to-mass ratio for an electron (-1.76 x 10⁸ C/g).

    Early Atomic Structure - Rutherford

    • Rutherford proposed that the positive charge of an atom was concentrated in a small, dense nucleus.
    • Positively charged particles within the nucleus are called protons.
    • This model was a significant advancement in understanding atomic structure.

    Early Atomic Structure - Bohr

    • Bohr suggested that electrons orbit the nucleus in specific energy levels.
    • Electron orbitals (or energy levels) have specific, quantized energies .

    Photoelectric Effect - Einstein

    • Einstein established that light particles possess wave-like properties.

    Wave Particle Duality - de Broglie

    • De Broglie showed that matter (like electrons) could also possess wave-like characteristics.

    Uncertainty Principle - Heisenberg

    • It is impossible to simultaneously and precisely determine both the position and momentum of a particle such as an electron.

    Schrödinger Wave Equation

    • Schrödinger developed mathematical equations that describe the behavior of electrons within an atom.
    • These are probability functions, which represent where you are most likely to find a given electron.
    • The solutions to the equations provide quantized energy level descriptions.

    Solvay Conference 1927

    • A famous gathering of prominent physicists that discussed and debated leading-edge discoveries at the time in atomic physics.

    Atomic Orbitals - s Orbitals

    • A sphere-shaped orbital where the electron is likely to be found surrounding the nucleus.
    • There are different types of s orbitals (1s, 2s, 3s…) that have different sizes and energies that directly correlate to their distance from the nucleus.

    Atomic Orbitals - p Orbitals

    • Dumbbell-shaped orbitals that have different orientations within space; namely, px, py, pz.
    • P-orbitals exist as sets of 3, and electrons in each orbital of the set have the same energy.

    Atomic Orbitals - d Orbitals

    • More complex shapes; namely, dxy, dx2-y2, dxz, dyz, dz2.
    • Occur in sets of 5 orbitals with the same energy levels.

    Energy Sublevels

    • Groups of atomic orbitals with the same energy.
    • Each sublevel comprises specific s, p, and d orbitals.

    Electronic Configurations

    • Describes the distribution of electrons within atomic orbitals and sublevels.
    • Electrons fill orbitals following the Aufbau and Hund's rules.

    Pauli Exclusion Principle

    • No two electrons within an atom can have the same set of four quantum numbers.
    • In other words, no more than two electrons can occupy a given orbital. These two electrons must also have opposite spins.

    Aufbau Principle

    • Electrons first occupy the lowest available energy level.

    Hund's Rule

    • Electrons fill degenerate orbitals individually before pairing up. It means each orbital in a given subshells will each have an electron with the same spin before the electrons pair up with opposite spins.

    Electronic Configuration Examples.

    • The notation used for specifying an electron configuration: (e.g. 1s22s2).
      • a prefix (e.g 1 or 2) stands for the principle quantum number that correlates to the energy level
      • superscript correlates to the number of electrons in the orbital.

    Transition Metals

    • Some elements deviate from the typical configuration rules because the slightly reduced energy of a half- or completely filled shell provides extra stability.

    Formation of Ions

    • Cations formed by losing one or more electrons.
    • Anions formed by gaining one or more electrons.

    The Main Positive Ion (Cation) in Blood (Na+)

    • Its formation occurs by the loss of one electron.

    The Main Negative Ion (Anion) in Blood (Cl-)

    • Formed by gaining one electron.

    Try K+: The Main Cation In Cell Fluid

    • K+ cation is formed by losing one electron, and typically occurs in cell fluid.

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    Fundamentals of Medicinal and Pharmaceutical Chemistry PDF

    Description

    Test your understanding of electronic configuration and atomic theory with this quiz. Explore principles such as the Pauli Exclusion Principle, Hund's Rule, and the Aufbau Principle. Assess your knowledge and improve your grasp of these fundamental chemistry concepts.

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