Atomic Models and Principles Quiz

Atomic Models: Principles and Structure

• Bohr Model:

  • Electrons exist in specific energy levels (allowed energy states)
  • Electrons orbit the nucleus in circular paths
  • When electrons absorb energy, they jump to a higher energy level; releasing energy when returning to a lower level.

• De Broglie Model:

  • Electrons exhibit wave-like properties
  • Electrons have specific wavelengths, frequencies, and energies
  • Electrons do not move in fixed circular orbits around the nucleus

• Heisenberg's Uncertainty Principle:

  • Simultaneous precise determination of an electron's position and velocity is impossible
  • It's not possible to predict a fixed path for electrons
  • The probability of finding an electron in a region around the nucleus can be determined

• Schrödinger's Quantum Mechanical Model:

  • Electrons do not have fixed paths around the nucleus
  • Electrons behave as waves
  • The electron cloud represents the greatest probability of finding an electron in a given region around the nucleus

Quantum Mechanical Model Details

• Principal Energy Level (n):

  • Represents the energy level of an electron
  • n = 1, 2, 3 etc (increasing energy levels)

• Sublevels per Level (n):

  • n = 1: 1 sublevel (s) holding 2 electrons
  • n = 2: 2 sublevels (s, p) holding 8 electrons
  • n = 3: 3 sublevels (s, p, d) holding 18 electrons
  • n = 4: 4 sublevels (s, p, d, f) holding 32 electrons

• Orbitals per Sublevel:

  • s: 1 orbital
  • p: 3 orbitals
  • d: 5 orbitals
  • f: 7 orbitals

• Electrons per Orbital/Sublevel:

  • Each orbital holds a maximum of 2 electrons
  • s: 2 electrons
  • p: 6 electrons
  • d: 10 electrons
  • f: 14 electrons

• Orbital Size and Energy:

  • As n increases, orbitals become larger and have higher energy

• Ground State:

  • The lowest energy level of an atom

Electron Arrangement Rules

• Aufbau Principle:

  • Electrons fill the lowest energy orbitals first

• Pauli Exclusion Principle:

  • A maximum of two electrons can occupy an orbital, with opposite spins

• Hund's Rule:

  • Electrons fill orbitals of equal energy singly before doubling up

Electron Configuration Notation Examples

• Electron Configuration Notation:

  • 1s², 2s², 2p⁶, 3s², 3p⁵

• Noble Gas Notation:

  • [Ne] 3s², 3p⁵

• Orbital Diagrams (Example):

  1s   2s        2p        3s        3p 
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Chemical Behavior

• Valence Electrons:
  • Electrons in the outermost energy level
  • Determine the chemical behavior of an element

Electron-Dot Structures

• Components:

  • Valence electrons

• Example (Correct): Cl·

• Example (Incorrect): …… Cl·