MS&E #2 Bonding

20 flashcards · Physics · by Kristóf Nagy

1. Pauli exclusion principle

   Quantum mechanical principle stating that no two fermions (half-integer spin particles, including electrons) can simultaneously occupy the exact same quantum state.

2. Bonding energy

   The amount of energy needed to break a chemical bond between two atoms.

3. Coulombic force

   The electrostatic force acting between charged particles, proportional to the product of their charges and inversely proportional to the square of the distance between them.

4. Covalent bond

   A chemical bond formed due to the sharing of electrons between two atoms.

5. Atomic weight (A)

   The average mass of an element's atoms, measured in atomic mass units (amu), calculated as the weighted sum of an element's isotopes' masses.

6. Atomic number (Z)

   The number of protons present in an atom's nucleus, determining the element's identity.

7. Dipole (electric)

   A pair of equal but oppositely charged regions in a molecule or atom, creating a separation of charge.

8. Atomic mass unit (amu)

   A unit of measurement for an atom's mass, defined as 1/12 of the mass of a carbon-12 atom.

9. Electropositive

   Opposite of electronegative, refers to elements that lose electrons in chemical reactions.

10. Mole

    A standard unit of measure representing the amount of a substance, numerically equivalent to Avogadro's number (~6.02 x 10^23) of elementary entities (atoms, molecules, ions, etc.).

11. Electron configuration

    Describing an atom's electronic structure, specifying the number and distribution of electrons in various energy levels or orbitals.

12. Ground state

    Denotes an atom's default electronic configuration, featuring minimal energy.

13. Hydrogen bond

    A weak interaction between a hydrogen atom attached to an electronegative atom and another electronegative atom bearing a partial negative charge.

14. Ionic bond

    A chemical bond resulting from the electrostatic attraction between positively and negatively charged ions.

15. Electronegative

    Refers to elements that tend to gain electrons in chemical reactions since they have stronger nuclear attractions for valence electrons.

16. Electron state

    Specifies an electron's energy level, angular momentum, magnetic projection, and spin.

17. Isotope

    Different versions of an element with varying numbers of neutrons in the nucleus, maintaining the same atomic number but differing atomic weights.

18. Metallic bond

    A type of bonding prevalent in metals, where delocalized valence electrons create a sea of mobile electrons responsible for the unique properties of metals.

19. Bohr atomic model

    A theoretical framework describing an atom's structure, proposing that electrons travel in circular orbits around the nucleus.

20. Periodic table

    Organizing chart categorizing all known chemical elements by ascending atomic number, presenting recurring patterns reflecting underlying periodic trends.