Ch. 4 Ionic Bonds & Some Main-Group Chem
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22 terms
Terms | Definitions |
|---|---|
 chemical bonds | join atoms together by electrons classified as either covalent or ionic "share" |
| covalent bonds | primarily occur between nonmetal atoms sharing |
| ionic bonds | primarily occur between metal and nonmetal atoms transferring |
| molecule | unit of matter that results when two or more atoms are joined by covalent bonds |
| ball and stick models | indicate the covalent bonds between atoms |
| space filling models | portray overall molecular shape but don't explicitly show the covalent bonds |
| Diatomic molecules | H2, N2, O2, F2, Cl2, Br2, I2 molecules whose two atoms are held together by a covalent bond |
| ionic bond | transfer of one or more electrons from one atom to another\ strong electrical attraction between two electrons |
| ion | formation of two charged particles |
| cation | positive ion |
| anion | negative ion |
| ionic solids | positive and negative ions are packed together in a regular way (ex: NaCl, MgCl2) can't specify which pairs of ions belong to each other as we can with atoms in covalent molecules |
| polyatomic ions | charged, covalently bonded groups of atoms charged molecules (they consist of specific numbers and kinds of atoms joined together by covalent bonds, with the overall unit having a +/- charge (ex: NH4+, SO4 2+, OH-) |
| metallic elements | on the left side of the periodic table tend to give up electrons in chemical reactions and form cations |
| halogens & some non-metallic elements | on the right side of the table, have a tendency to accept electrons in their chemical reactions and form anions |
| ground state electron configuration | for main group elements, the electrons given up by a metal in forming a cation come from the highest-energy occupied orbital, while the electrons that are accepted by a nonmetal in forming an anion go into the lowest-energy unoccupied orbital |
| aufbau principle | 1. Lower-energy orbitals fill before high-energy orbitals 2. An orbital only holds 2 electrons, which must have opposite spins. *no 2 electrons in an atom can have the same quantum numbers 3. If 2 or more degenerate orbitals are available, one electron goes into each until all are half-full. Only then does a second electron fill one fo the orbitals. The electrons in each of the occupied orbitals must have the same value for their spin quantum number |
| Group 1A | all form positive ions by losing their valence shell s electron when they undergo reactions, and all the resultant ions have noble gas electron configurations |
| Group 2A | all form a doubly positive ion when they react, losing both their valence-shell s electrons, obtains a noble gas configuration |
| Group 6A & 7A nonmetals gain | the appropriate number of electrons when they react with metals |
| halogens in Group 7A | gain one electron to form singly charged anions with noble gas configurations |
| Group 6A | gain two electrons to form doubly charged anions with noble gas configurations |
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