| A | B |
|---|
| valence electrons | Elements of the same group of the periodic table behave similarly because they have the same number of these |
| group number | indicates how many valence electrons that element has |
| octet rule | states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas |
| Lewis Dot Structure | a depiction of valence electrons around the symbol of an element |
| valence electron | an electron in the highest occupied energy level of an atom |
| electrostatic forces | anions and cations attract one another by these |
| ionic bonds | The forces of attraction that bind oppositely charged ions |
| crystalline solids | nearly all ionic compounds at room temperature |
| covalent bonds | When atoms share electrons to gain stable electron configuration of a noble gas, they form this bond |
| single covalent bond | a shared pair of valence electrons |
| unshared pairs | pairs of valence electrons that are not shared between atoms |
| double/triple covalent bonds | two or three pairs of electrons may be shared in these bonds |
| resonance structure | when two or more valid electron dot formulas for a molecule or ion, each formula is referred to as this |
| VSEPR theory | states that because electron pairs repel, molecules adjust their shapes so that valence-electron pairs are as far apart as possible |
| polar bond | covalent bond between two atomsof different electronegativities in which the bonding electrons are not shared equally |
| nonpolar covalent bond | covalent bond formed by the equal sharing of bonding electrons by two atoms |
| Molecule shapes | tetrahedral, pyramidal, bent, linear |
