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. (D)</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. (C)</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. (B)</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. (A)</p> Signup and view all the answers

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

<p>6 (A)</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 (C)</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. (B)</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 (B)</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. (A)</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. (B)</p> Signup and view all the answers

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

<p>The electron as a subatomic particle. (D)</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. (A)</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. (B)</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. (A)</p> Signup and view all the answers

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

<p>Alpha particles. (C)</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. (A)</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. (D)</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. (A)</p> Signup and view all the answers

What shape does an s-orbital have?

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

How many orientations do p-orbitals have?

<p>Three (C)</p> Signup and view all the answers

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

<p>2 (B)</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 (D)</p> Signup and view all the answers

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

<p>Dumbbell (C)</p> Signup and view all the answers

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

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

Which description applies to the p-orbitals' shape?

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

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

<p>Five (D)</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 (C)</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. (B)</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. (D)</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. (A)</p> Signup and view all the answers

What are atomic orbitals primarily used for?

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

What does not describe atomic orbitals?

<p>They always have the same size and energy. (C)</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. (D)</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. (B)</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. (C)</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. (D)</p> Signup and view all the answers

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

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

Flashcards

Dalton's Atomic Theory: Point 1

Elements are made up of tiny particles called atoms.

Dalton's Atomic Theory: Point 2

All atoms of the same element are identical in size, mass, and chemical properties.

Dalton's Atomic Theory: Point 3

Atoms of different elements are unique and distinct from each other.

Dalton's Atomic Theory: Point 4

Compounds are formed by combining atoms of different elements.

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Dalton's Atomic Theory: Point 5

In any compound, the ratio of atoms of different elements is always a simple whole number.

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Atomic Orbital

A region around the nucleus of an atom where an electron is most likely to be found.

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Electronic Configuration

Describes the distribution of electrons in different energy levels and subshells within an atom.

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Wave-Particle Duality

The idea that particles like electrons can exhibit both wave-like and particle-like properties.

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Heisenberg's Uncertainty Principle

A fundamental principle in quantum mechanics that states it is impossible to simultaneously know both the exact position and momentum of a particle with absolute certainty.

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Schrödinger Wave Equation

A mathematical equation developed by Erwin Schrödinger in 1925 that describes the wave function of an electron in an atom.

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Solvay Conference 1927

A major scientific conference held in 1927 that brought together leading physicists to discuss the emerging field of quantum mechanics, including the wave-particle duality and Heisenberg's Uncertainty Principle.

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s Orbital

The spherical, lowest energy atomic orbital and has a single electron within it.

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Types of Atomic Orbitals

Atomic orbitals are regions that differ in size, shape, and energy, allowing electrons to occupy different spaces around the nucleus.

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Multiple Atomic Orbitals

The ability of some of the same type of atomic orbital to be used by the same nucleus to accommodate multiple electrons.

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Importance of Atomic Orbitals

The arrangement of electrons in orbitals helps us understand how atoms interact and form compounds.

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What does a chemical reaction involve?

A chemical reaction is a process that involves the rearrangement, separation, or combination of atoms, but does not result in the creation or destruction of atoms. It's like rearranging puzzle pieces, not adding or removing them.

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What did J.J. Thomson discover?

J.J. Thomson's discovery of the electron revolutionized our understanding of atomic structure. Using cathode ray tubes, he experimentally determined the ratio of electric charge to mass of a single electron, providing the first evidence for the existence of subatomic particles.

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What was the cathode ray tube experiment about?

The cathode ray tube experiment, devised by J.J. Thomson, demonstrated that cathode rays consisted of negatively charged particles, which were later identified as electrons.

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What is the Plum Pudding model?

Since atoms are electrically neutral, Thomson proposed that the positive charge of an atom must be spread evenly throughout, with negatively charged electrons embedded in it, much like plums in a pudding. This model was later proven incorrect but provided an important initial understanding of the atomic structure.

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What was Rutherford's Gold Foil experiment about?

Rutherford's alpha particle scattering experiment, where positively charged alpha particles were fired at a thin gold foil, led to a surprising discovery: most particles passed through the foil, but some were deflected at large angles, suggesting that the positive charge was concentrated in a small, dense nucleus.

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What is the nucleus of an atom?

The nucleus, as proposed by Rutherford, is the dense central core of an atom that contains the majority of its mass and all of its positive charge. This discovery completely changed the view of the atom. The nucleus is similar to the sun in our Solar system, with the planets orbiting around it, representing electrons.

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What are protons?

Protons are positively charged particles found in the nucleus of an atom. They were identified later by Rutherford, building upon his discovery of the nucleus.

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How are electrons arranged in an atom?

The arrangement of electrons outside the nucleus of an atom is crucial to understanding the chemical properties of an element. Different energy levels exist, and electrons occupy specific orbitals with specific energies.

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Who proposed the first model of the atom?

Bohr proposed a model where electrons occupy specific orbits or energy levels around the nucleus. This model paved the way for understanding how light interacts with atoms and the basis of quantum theory.

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Pauli Exclusion Principle

No more than two electrons can occupy a single atomic orbital. These two electrons must have opposite spins.

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Aufbau Principle

Electrons fill the lowest energy level first, then move to higher energy levels as they become available.

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Hund's Rule

When orbitals of equal energy exist (e.g., px, py, pz), electrons fill them singly first, with one in each before pairing up.

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Electron Configuration Notation

a shorthand notation that uses a prefix to indicate the energy and size of an orbital (principal quantum number), and a superscript to denote the number of electrons in that orbital.

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What is an s-orbital?

An s-orbital is a spherical region around the nucleus where an electron is most likely to be found.

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How are s-orbitals different?

There are different types of s-orbitals, and they are distinguished by their energy levels. Higher energy levels mean the s-orbital is further from the nucleus.

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What is a p-orbital?

A p-orbital is a dumbbell-shaped region around the nucleus where an electron is most likely to be found.

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How many p-orbitals are there?

There are three p-orbitals, each oriented along one of the three axes in space, but they all have the same shape and energy level.

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What is a d-orbital?

A d-orbital is a more complex shaped region around the nucleus where an electron is most likely to be found.

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How many d-orbitals are there?

There are five d-orbitals, each with a unique shape, but all sharing the same energy level.

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What is an energy sublevel?

An energy sublevel is a group of atomic orbitals with the same energy level. For example, the three p-orbitals (px, py, and pz) belong to the same energy sublevel.

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How many electrons can an orbital hold?

Each orbital can hold a maximum of two electrons.

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What means degenerate in the context of orbitals?

A set of orbitals with the same energy level is called degenerate. For example, the three p-orbitals or the five d-orbitals are degenerate.

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How does energy level relate to distance from the nucleus?

The energy levels of electrons in an atom increase with increasing distance from the nucleus.

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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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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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