Atomic Structure Quiz

Atomic Structure

Protons

• Positive charge
• Located in the nucleus (central part of the atom)
• Mass: approximately 1 atomic mass unit (amu)
• Number of protons determines the element (atomic number)

Neutrons

• No charge
• Located in the nucleus
• Mass: approximately 1 amu
• Number of neutrons varies, leading to different isotopes of the same element

Electron Configuration

• Arrangement of electrons in energy levels (shells) around the nucleus
• Each shell has a specific capacity (number of electrons it can hold)
• Electron configuration determines chemical properties of an element
• Aufbau principle: electrons occupy the lowest available energy level
• Pauli's exclusion principle: each electron has a unique set of quantum numbers

Nuclear Reactions

• Changes in the nucleus of an atom
• Types:
  • Radioactive decay: spontaneous emission of radiation
  • Nuclear fission: splitting of an atomic nucleus
  • Nuclear fusion: combination of atomic nuclei
• Nuclear reactions involve changes in the number of protons, neutrons, or both

Quantum Numbers

• Set of four numbers that describe an electron's energy, shape, and orientation
• Principal quantum number (n): energy level (shell)
• Azimuthal quantum number (l): shape of the orbital
• Magnetic quantum number (m): orientation of the orbital
• Spin quantum number (s): spin of the electron (+1/2 or -1/2)

Discovery of Subatomic Particles

• Proton: Ernest Rutherford (1919)
• Electron: J.J. Thomson (1897)
• Neutron: James Chadwick (1932)

Atomic Models

• Rutherford's Atomic Model (1911):
  • Nucleus with protons and neutrons
  • Electrons orbiting the nucleus
• Bohr's Atomic Model (1913):
  • Energy levels (shells) for electrons
  • Electrons jump to higher or lower energy levels by absorbing or emitting energy
• Quantum Mechanical Model:
  • Electron cloud (probability of finding an electron)
  • Orbitals (shapes of electron clouds)
  • Quantum numbers to describe electrons

Atomic Structure

Protons and Neutrons

• Protons: positively charged, located in the nucleus, approximately 1 amu in mass, and determine the element (atomic number)
• Neutrons: no charge, located in the nucleus, approximately 1 amu in mass, and vary in number to form different isotopes of the same element

Electron Configuration

• Arrangement of electrons in energy levels (shells) around the nucleus
• Each shell has a specific capacity (number of electrons it can hold)
• Determines chemical properties of an element
• Aufbau principle: electrons occupy the lowest available energy level
• Pauli's exclusion principle: each electron has a unique set of quantum numbers

Nuclear Reactions

• Changes in the nucleus of an atom involving protons, neutrons, or both
• Types:
  • Radioactive decay: spontaneous emission of radiation
  • Nuclear fission: splitting of an atomic nucleus
  • Nuclear fusion: combination of atomic nuclei

Quantum Numbers

• Set of four numbers describing an electron's energy, shape, and orientation
• Principal quantum number (n): energy level (shell)
• Azimuthal quantum number (l): shape of the orbital
• Magnetic quantum number (m): orientation of the orbital
• Spin quantum number (s): spin of the electron (+1/2 or -1/2)

Discovery of Subatomic Particles

• Proton: discovered by Ernest Rutherford (1919)
• Electron: discovered by J.J. Thomson (1897)
• Neutron: discovered by James Chadwick (1932)

Atomic Models

• Rutherford's Atomic Model (1911):
  • Nucleus with protons and neutrons
  • Electrons orbiting the nucleus
• Bohr's Atomic Model (1913):
  • Energy levels (shells) for electrons
  • Electrons jump to higher or lower energy levels by absorbing or emitting energy
• Quantum Mechanical Model:
  • Electron cloud (probability of finding an electron)
  • Orbitals (shapes of electron clouds)
  • Quantum numbers to describe electrons