FChem

• What is the title of the course related to Structure and Bonding?

  Structure and Bonding I
• Who is the author of the study material?

  Dr Anthony Curtis
• What are the main topics covered in Structure and Bonding?

  • Introduction to the Periodic Table
  • Pharmaceutical Chemistry
  • Electronic structure of atoms
  • Basic atomic and molecular structure
  • Atomic and molecular orbitals
  • Covalent bonding and hybridisation
  • Molecular structures and conformations
  • Drawing structures in organic chemistry
  • Importance of knowing electron locations
• What are the two types of blocks in the periodic table mentioned?

  S Block and P Block
• What does 'Pharmaceutical Chemistry' primarily focus on?

  Chemistry of drug molecules and formulations
• What characterizes organic compounds?

  Compounds of carbon with covalent bonds
• Which elements must also be considered in pharmaceutical chemistry?

  N, O, S, and halogens
• What is the implication of discovering more organic compounds?

  No increase in New Chemical Entities (NCEs)
• What are the essential physicochemical properties of drugs?

  • Molecular structure: bonding, shape, isomers
  • Molecular properties: LogP, pKa, chirality
  • Classification: according to functional groups
  • Reactivity: bond polarity, reaction mechanism
  • Spectroscopy: determining molecular structure
• Why must physicochemical properties be considered in drug design?

  They influence synthesis and formulation
• Who discovered the electron and in what year?

  Thomson in 1897
• What equation did Planck introduce in 1900?

  E = hv
• Who discovered the nucleus and in what year?

  Rutherford in 1909
• What did Millikan measure in 1910?

  The charge on an electron
• What model of the atom did Bohr describe in 1913?

  A quantum model of the atom
• What concept did de Broglie describe in 1924?

  Wave-particle duality
• What is Schrödinger’s equation used for?

  Understanding electron positions in atoms
• What do the three quantum numbers describe in atomic orbitals?

  The properties of each orbital
• What does the principal quantum number (n) represent?

  Energy level of the electron
• What does the angular momentum quantum number (l) indicate?

  Shape of the orbital
• What does the magnetic quantum number (ml) specify?

  Direction of the orbital
• How are the energy and shape of an orbital determined?

  By a combination of quantum numbers
• What does it mean for orbitals to be degenerate?

  They are equal in energy
• What is the 2s orbital associated with?

  n = 2, l = 0
• What is the 2p orbital associated with?

  n = 2, l = 1
• What are the shapes of atomic orbitals?

  • 1s: spherical shape
  • 2s: spherical shape
  • 2p: dumbbell shape

  
• What affects the energy of atomic orbitals in many-electron atoms?

  Effective nuclear charge experienced by electrons
• Why do outer electrons experience lower effective nuclear charge?

  Due to shielding by inner electrons
• How do s and p atomic orbitals differ in many-electron atoms?

  They are not equal in energy
• What are the rules for electronic configurations?

  1. Aufbau principle: electrons fill lowest energy orbitals first
  2. Pauli exclusion principle: no two electrons can have the same four quantum numbers
  3. Hund’s rule: maximize unpaired electrons in degenerate orbitals
• What are valence electrons?

  Outermost electrons enclosing a closed shell
• What is the significance of covalent bonds in carbon?

  They form filled orbitals with opposing spin
• How many covalent bonds can carbon form in the ground state?

  Four covalent bonds
• Does the formation of four covalent bonds lead to stable molecules?

  Yes, it leads to stable molecules
• What is the email address for further information?

  [e-mail]
• What is the title of the study material?

  Structure and Bonding II
• Who is the author of the study material?

  Dr Anthony Curtis
• What is the principal quantum number for the 2s orbital?

  n = 2
• What is the azimuthal quantum number for the 2p orbital?

  l = 1
• What does the quantum number ml represent for l = 1?

  ml = 1, 0, or -1