Unit 2 Terminology

2. the unequal sharing of electrons between two atoms in a covalent bond.
3. hybrid bonds, formed between two paired atoms, also known as double and triple bonds.
6. a group of atoms, bonded together covalently.
11. Mixing of two or more atomic orbitals to form new hybrid orbitals (double and triple bonds).
12. a positively charged ion.
13. a single covalent bond is also known as this.
14. chemical compound composes of ions held together by electrostatic forces.
15. the distance between the centers of two covalently bonded atoms.
16. a mixture of chemical elements of which at least one is a metal
17. delocalized electrons within certain molecules or polyatomic ions where bonding cannot be expressed by a single Lewis Structure.
19. the charge that is assigned to an atom by taking the difference between the number of valence electrons of an atom, and the number of electrons assigned to that atom in a Lewis Structure.
20. the mutual sharing of one or more pairs of electrons.

1. electrostatic attractive force between conduction electrons ("sea of electrons") and positively charged metal ions.
4. chemical bond that is formed when electrons are shared equally between two atoms.
5. alloy formed by inserting smaller atoms into the spaces between metal atoms in a lattice structure.
7. alloy formed by substituting one metal atom for another metal atom of similar size.
8. electrostatic attraction between oppositely charged ions in chemical compounds
9. any force that binds together the atoms making molecule or compound
10. simplified representation of the valence shell electrons in a molecule.
14. solids held together covalently, in 3-dimensional "lattice" structures.
18. a negatively charged ion.