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chem final
Chem final
| Term | Definition |
|---|---|
| Strong/weak/acid/base/name? HNO_3 | Strong acid, Nitric Acid |
| Strong/weak/acid/base/name? HX | Strong acid, hydrogen hallide |
| Strong/weak/acid/base/name? MOH | Strong base, metal hydroxides |
| Proton transfer reaction | Shows the movement of an H+ or proton from an acid to a base. Ex NH_3 + H_2O -> NH+_4 + OH- |
| intensive properties | independent of the amount of the substance |
| crystallization | a separation technique based upon differences in solubility of the components in a mixture |
| empirical formula | simplest formula for a compound that agrees with the elemental analysis. shows the lowest whole number of moles and gives the relative number of atoms of each element present |
| scientific method | observations, hypothesis, experiment, model (theory), further experiment |
| Name Mg(CO3) | Magnesium Carbonate |
| Name CuCl2 | Copper (II) Chloride |
| Name Fe(OH)3 | Iron (III) Hydroxide |
| Name P2O5 | Diphosphorus Pentoxide |
| Sulfuric Acid | H2SO4 |
| solution | homogenous mixture with a uniform composition |
| spectator ions | ions that are not involved in the chemical change |
| ideal gas | gas that exhibits linear relationships amongst its variables |
| effusion | process by which a gas escapes through a small hole in its container into an evacuated space |
| Hess's Law | the enthalpy change of an overall process is the sum of the enthalpy changes of its individual steps |
| thermochemistry | branch of thermodynamics that deals with the heat involved in chemical and physical change |
| work | energy transferred when an object is moved by a force |
| specific heat capacity | the quantity of heat required to change the temp of 1 g of a substance by 1 K |
| Neutralization reaction | Acid + Base -> Salt + Water |
| Redox reaction | A(neutral) + B (neutral) -> A(Positive charge) + B (negative charge) |
| Precipitation reaction | AB(aq) + CD(aq) -> AD(s) + BC(aq) |
| frequency | number of cycles a wave has per second |
| de Broglie wavelength | formula to find wavelength of electrons |
| quanta | any amount of energy |
| Pauli Exclusion Principle | Each orbital may contain a max of 2 electrons which must have opposite spins |
| covalent radius | half the shortest distance between nuclei of identical, covalently bonded atoms |
| ionization energy | energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions |
| electronegativity | ability of an atom in a covalent bond to attract the shared electron pair |
| bond order | number of electron pairs being shared by a given pair of atoms |
| covalent bonding | involves the sharing of electrons usually when a nonmetal bonds to a nonmetal |
| determining polarity | a molecule is usually polar when the central atom has lone pairs or is surrounded by different types of atoms. |
| nonpolar molecules | Molecules can be nonpolar if their shape is symmetric (e.g., ), as bond dipoles cancel out. Like CO2. Can also be nonpolar if the molecule consists of two identical atoms sharing electrons equally since both atoms have the same electronegativity |
| electronegativity and ionization energy periodic table trends | increases from left to right across periods and decreases down groups |
| atomic radii periodic table trend | increases from top to bottom within a group (column) due to added electron shells and decreases from left to right across a period (row) due to increased nuclear attraction |
| Which bond order has the longest distance between carbon atoms? | One, because the more bonds you have, the stronger the charge and the stronger the attraction. |
| resonance structures | Resonance structures have the same relative placement of atoms but different locations of bonding and lone electron pairs. |
| real structure | the real structure of the resonance hybrid for a molecule is an average of its contributing resonance forms. |
| resonance hybrid | A mule is a genetic mix, a hybrid, of a horse and a donkey. It is not a horse one instant and a donkey the next. Likewise, a resonance hybrid has a single structure although it retains characteristics of its resonance forms. |
| Electron delocalization | Lewis structures depict electrons as localized either on an individual atom (lone pairs) or in a bond between two atoms (shared pair). In a resonance hybrid, electrons are delocalized: their density is “spread” over a few adjacent atoms |
| fractional bond orders | Bond Order = # of shared electron pairs / # of bonded atom pairs |
| formal charge | the charge an atom would have if all electrons were shared equally. |
| oxidation number | bonding electrons are transferred to the more electronegative atom. The oxidation number of an atom is the same in all resonance forms. |
| free radicals | molecules that have an odd number of valence electrons |
| Valence Bond Theory | A covalent bond forms when the orbitals of two atoms overlap and a pair of electrons occupy the overlap region. The space formed by the overlapping orbitals can accommodate a maximum of two electrons and these electrons must have opposite spins. |
| hybridization | the process of orbital mixing |
| features of hybrid orbitals | # of hybrid orbitals formed equals the number of atomic orbitals mixed. Type of hybrid orbitals formed varies w/ the types of atomic orbitals mixed. Shape and orientation of a hybrid orbital maximize overlap with the orbital of the other atom in the bond |
| sigma bond | formed by end-to-end overlap of orbitals (all single bonds are sigma bonds) |
| pi bond | formed by the sideways overlap of orbitals (weaker than sigma bond) |
| Molecular Orbital Theory | a molecule has molecular orbitals of given energies and shapes that are occupied by the molecule's electrons, just as atoms have atomic orbitals |
| MO diagram | shows the relative energy and number of electrons in each MO |
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