General Chemistry - Inorganic

• What is the nucleus of an atom composed of?

  Protons and neutrons
• How does the classical model describe electrons?

  As particles orbiting the nucleus
• What does the wave mechanics model suggest about electrons?

  Electrons are waves spread like fog
• What does quantisation refer to in atomic structure?

  Only certain energies of electrons are allowed
• What is an orbital in chemistry?

  A region of space with specific energy
• What is the Schrödinger equation used for?

  To calculate wavefunctions for electrons
• How do electrons transition between energy levels?

  By absorbing or emitting light of specific energy
• How many quantum numbers are used to describe electrons?

  Four quantum numbers
• What does the principal quantum number (n) indicate?

  Size of the orbital
• What does the angular momentum quantum number (l) describe?

  Shape of the orbital

  
• What does the magnetic quantum number (ml) indicate?

  Orientation of the orbital
• What does the spin quantum number (ms) represent?

  Direction of electron spin
• What is the shape of an s orbital?

  Spherical

  
• How many p orbitals are there in a p subshell?

  Three p orbitals
• What is a nodal plane in orbitals?

  A plane where electron density is zero
• What is the maximum number of electrons in the n=1 shell?

  Two electrons
• How many d orbitals are there in a d subshell?

  Five d orbitals
• How many electrons can the n=2 shell hold?

  Eight electrons
• How many electrons can the n=3 shell accommodate?

  18 electrons
• How many electrons can the n=4 shell accommodate?

  32 electrons
• What is the electron configuration for carbon?

  1s² 2s² 2p²
• What does Zeff represent?

  Effective nuclear charge felt by electrons
• What is the trend of ionisation energy across a period?

  Ionisation energy increases across a period
• What happens to ionisation energy down a group?

  Ionisation energy decreases down a group
• Why is it harder to remove an electron from a cation than a neutral atom?

  Cation has a higher effective nuclear charge
• What is the definition of atomic radius?

  Distance to the outermost valence electron
• What is the difference between covalent radius and ionic radius?

  Covalent radius is for diatomic molecules
• What is the significance of Hund's Rule?

  Electrons fill degenerate orbitals singly first
• What is the Aufbau Principle?

  Electrons fill the lowest energy orbitals first

  
• What is the Pauli Exclusion Principle?

  No more than two electrons per orbital
• What is the trend in ionisation energy for Li to Ne?

  Ionisation energy generally increases
• Why do some elements have unexpected ionisation energy trends?

  Due to electron-electron repulsions in orbitals
• What are the general features of the Periodic Table?

  • Arrangement by increasing atomic number
  • Groups and periods indicate similar properties
  • Blocks correspond to electron configurations

  
• What are the trends in physical properties considered in the study material?

  1. Atomic radius
  2. Ionisation energy
  3. Electron affinity
  4. Electronegativity
  5. Oxidation state definition
• What are the types of chemical bonding discussed?

  • Covalent bonding
  • Ionic bonding
  • Metallic bonding
• What is the Valence Shell Electron Pair Repulsion Theory (VSEPRT)?

  • Predicts molecular shapes
  • Based on electron pair repulsion
• What is Molecular Orbital Theory?

  • Describes overlap of orbitals
  • Involves σ and π orbitals

  
• What are the shapes of d-orbitals?

  • dxz
  • dyz
  • dxy
  • dx2-y2
  • dz2

  
• What are the shapes of f-orbitals?

  • l = 3
  • ml = +3, +2, +1, 0, -1, -2, -3

  
• What is the significance of electron configurations in the Periodic Table?

  • Indicates electron arrangement
  • Determines chemical properties