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Chem 07 Bonding
Ionic, Covalent, and Metallic Bonding. Nomenclature.
| Term | Definition |
|---|---|
| 2 or more elements chemically combined in a set ratio | compound |
| shorthand/abbreviation for a compound (uses symbols and subscripts) | chemical formula |
| number written after and below symbol in chemical formula that tells number of that element in a compound formula | subscript |
| chemically stable elements in group 18 on the periodic table | noble gases |
| chemically stable arrangement of (8) electrons in the outer energy level | stable octet/ngc |
| describes the electrons in the outer lever, or the level itself | valence |
| force that holds atoms together in a compound | chemical bond |
| elements with 5-7 outer e-'s, on right side of PT, tend to gain electrons (during ionic bonding) | nonmetal |
| elements with 1-3 outer e-'s, on left side of PT, tend to lose e-'s | metal |
| an atom with an overall charge (due to gaining or losing e-s) | ion |
| a positively-charged ion (formed by losing electrons) | cation |
| a negatively-charged ion (formed by gaining electrons) | anion |
| attraction between oppositely-charged ions (in an ionic compound) | ionic bond |
| describes a compound composed of (only) two different elements | binary |
| chemical combination of a metal and a nonmetal | ionic compound |
| used to reveal the ion charge of a (transition) metal that can form more than one charge | Roman numerals |
| simplest ratio of ions in an ionic compound | formula unit |
| any system for naming things systematically (such as compounds) | nomenclature |
| solid whose particles are arranged in a regular geometry | crystal |
| smallest repeating part (i.e. building block) of a crystal | unit cell |
| the overall repeating pattern of ions (atoms) within a crystal | lattice |
| tells the # of oppositely-charged ions surrounding a particular ion in a crystal | coordination number |
| the loose (i.e. mobile) outer electrons in metals | valence sea |
| attraction between the valence 'sea' and the + atom cores (kernels) in metals | metallic bonding |
| (definition) can be beaten/hammered (or stretched into wires) without breaking | malleable/ductile |
| simplified Bohr model using only symbols and 'dots' (for valence electrons) | dot diagram |
| cluster of (covalently) bonded atoms with an overall charge (ex: OH-) | polyatomic ion |
| name for the process of writing ionic formulas from individual ions that combine | ion charge/criss cross method |
| unit cell shape for crystal of a table salt (sodium chloride, NaCl) | cubic (isometric) |
| unit cell shape that looks like a 'cereal box' | orthorhombic |
| unit cell shape that looks like a saltine cracker box | tetragonal |
| the two unit cells that are 'leaning' | monoclinic/triclinic |
| 6-sided unit cell shape (ex: quartz!) | hexagonal |
| coordination # for Na+ and Cl- ions in crystal lattice of table salt (NaCl) | six (6) |
| suffixes used in polyatomic ions to indicate the presence of oxygen (in greater or lighter numbers) | -ate/-ite |
| prefixes used in polyatomic ions that mean 'more than' and 'less than' | per-/hypo- |
| # of atoms in a formula unit of (NH4)3PO4 | twenty (20) |
| formation of compounds by sharing electrons between atoms | covalent bonding |
| attraction between atoms mutually sharing electrons | covalent bond |
| made by chemically combining two nonmetal | (binary) covalent compound |
| two electrons shared between bonded atoms | bonding (shared) pair |
| pair of valence electrons in a molecular that are unshared; they only belong to one of the atoms | nonbonding (lone) pair |
| neutral group of covalently bonded atoms (building block of covalent compounds) | molecule |
| shows the arrangement of atoms in space in a molecule ('ball and stick' sketch of the compound) | structural formula |
| just shows the types and # of atoms in one molecule | molecular formula |
| one, two, or three pairs of electrons being shared between two atoms | single, double, triple bonds |
| the (7) diatomic elements that can bond with themselves to make stable, 2-atomed molecules | Br, I, N, Cl, H, O, F |
| explains that molecular geometry is a result of electrons in bonds spreading out to minimize repulsions | VSEPR Theory |
| shape of all 2-atom molecules | linear |
| shape of a water molecule | bent |
| shape of an ammonia (NH3) molecule | pyramidal |
| shape of a methane (CH4) molecule, its bond angle is 109.5° | tetrahedral |
| numerical prefixes for the numbers 1 - 4 | mono-/di-/tri-/tetra- |
| numerical prefixes for the numbers 5 - 7 | penta-/hexa-/hepta- |
| numerical prefixes for the numbers 8 - 10 | octa-/nona-/deca- |
| measures the attraction of an atom for electrons in a bond | electronegativity |
| bond between atoms sharing electrons equally | nonpolar covalent bond |
| bond between atoms that share electrons, but unequally | polar covalent bond |
| attractions (weak) that hold one molecule to another (in solids & liquids) | intermolecular forces |
| the three elements to which hydrogen must be bonded for it to exhibit H-bonding | F, O, N |
| weakest intermolecular force caused by random motion (and occasional unbalanced distribution of) electrons in atoms | dispersion interaction/London forces |
| attractions between polar molecules | dipole-dipole forces |
| a molecule that has overall regions of charge concentration/inbalance | polar molecule/dipole |
| attraction between H in a very polar bond and a lone pair on another nearby molecule; it is about 10% the strength of a covalent bond | hydrogen bonding |
| Name 1 of the 3 important outcomes of H-bonding in nature mentioned in class | freezing water expands; DNA 'unzips', hemoglobin folds |
| electronegativity difference ranges for classifying bonds as: non polar, polar, and ionic | 0.0-0.4/0.5-1.9/≥2.0 |
| formula or name of any 1 of the 3 exceptions to the octet rule having 6, 10, and 12 valence electrons respectively that were mentioned in class | BCl3, PCl5, SF6 |
| statement: during bonding, atoms rearrange electrons so that all bonded atoms have the electron configuration of a noble gas (8 valence electrons) | octet rule |
| the suffix used with the anion of all binary compounds, ionic and covalent | -ide |
| ionic compound with a set # of covalently-bonded water molecules attached to stabilize the crystal lattice | hydrate |
| meaning of "•" symbol in hydrate formula (ex: CaCl2•2H2O) | "attached to" |
| describes the (powdery) part of a hydrate that remains when its water of hydration is removed, usually by heating | anhydrous |
| the water molecules that are attached to the ionic part of a hydrate to hold it together | water of hydration |
| naming pattern for an acid-forming hydrogen compound whose undissolved name ends in –ide | hydro-'root'-ic acid (ex: hydrogen chloride --> hydroCHLORic acid) |
| naming pattern for an acid-forming hydrogen compound whose undissolved name ends in –ate | 'root'-ic acid (ex: hydrogen nitrate --> nitric acid) |
| naming pattern for an acid-forming hydrogen compound whose undissolved name ends in –ite | 'root'-ous acid (ex: hydrogen phosphite --> phosphorous acid) |
Created by:
goakley
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