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93 Cards in this Set
- Front
- Back
Coulomb's Law |
The electrostatic force between two charges separated by a distance is FΩ(QeQn)/r^2 |
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Effective Nuclear Charge |
Qneff ~ Qn - (# of shielding electrons) |
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Qe |
-1 |
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Qn |
Charge of the elements nucleus |
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Atomic Radius Trend |
Increases as you down and left. |
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Explanation of Atomic Radius Trend |
Valence shell decreases/stays the same. Core increases/stays the same Qneff decreases/stays the same
Qneff decrease had bigger affect than valence shell decrease(left) When Qneff stays so does valence, core increases size(top to bottom) |
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Ionization Energy |
The energy required to remove the outermost (highest energy) electron from an atom in the gaseous state |
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Ionization Energy Trend |
Increases moving right and up. |
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Ionization Energy Trend Explanation |
Atomic Radius decreases Qneff increases(right)/constant(up) |
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Third Ionization Energy |
Very large increase in IE because the atom is smaller (r smaller) and Qneff is larger |
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Electron Affinity |
The energy change when an electron is added to an atom in the gaseous state. |
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Negative Electron Affinity |
The ion is more stable than the atom. |
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Positive Electron Affinity |
The ion is unstable and doesn't form spontaneously. |
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Negative Electron Affinity Tend |
An electron is added into a partially filled subshell. |
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Positive Electron Affinity Trend |
An electron is added to an element that has filed subshells. |
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Anion Atomic Size |
Larger than there atoms |
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Cation Atomic Size |
Smaller than there atom. |
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Ionic Bond |
One or more electrons is permanently transferred from one atom to another. |
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Lattice Energy |
The energy reqired to create a mole of ionic solid from its constituent ions in the gas phase. Inferred from the force of attraction |
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Force of Attraction |
FΩ(Q1Q2)/r^2 |
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Comparing Lattice Energies |
The size affects r, the charge affects Q1,Q2 |
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Properties of Ionic Materials |
Very high melting points Hard but brittle Conducts electricity: never in solid, always in aqueous solution |
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Covalent Charge |
When 2 nonmetal atoms share electrons. |
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Isoelectric |
Has the same number of electrons |
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Electronegativity |
The ability of an atom to attract the electrons in a chemical bond. |
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Electronegativity Trend |
Increases right and up, same reasons as ionization energy. |
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Rules for Drawing Electron Dot Formulas |
1. Calculate the total number of valence electrons 2. Draw the skeleton structure 3. Distribute the remaining v.e. amongst the outer atoms to complete there octets 4. Place any remaining v.e. on the central atom |
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Delocalized Bonding |
The electrons in the double bond are spread over two bonds |
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Resonance Form |
Each possible lewis structure connected by double-headed arrows. Same atoms arranged in the same way but with double or triple bonds in different places. |
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Bond Order |
Indicates the extent of multiple bonding. Single bond: bond order=1 Triple bond: bond order= 3 |
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Polyatomic Ion |
Molecule with a charge |
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Formal Charge |
(Original # of valence electrons) - ( # of electrons in lone pairs) - (# of bonds) |
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Linear |
2 electron groups |
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Trigonal Planar |
3 electron groups |
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Tetrahedral |
4 electron groups |
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Trigonal Bipyramidal |
5 electron groups |
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Octahedral |
6 electron groups |
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AX2E |
Bent |
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A3E |
Trigonal Pyramidal |
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AX2E2 |
Bent |
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AX3E2 |
T shaped |
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AX4E |
See saw |
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AX2E3 |
Linear |
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AX5E |
Square pyramidal |
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AX4E2 |
Square planar |
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Hybridization |
The blending of occupied atomic orbitals to make the same number of hybrid orbitals |
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Valence Bond Theory Steps |
1. Draw the lewis structure 2. Calculate the formal charge on the atom toy are interested in 3. Draw ground state orbital diagram 4. Promote electrons 5. Keep one p-orbital unhybridized for each pi-bond attached 6. Hybridizevall remaining occupied orbitals in the valence shell |
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Rotational Isomers |
Molecules with the same atoms, but in different arrangements. |
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Phase Diagram |
Shows the phase (state) of a substance as a function of pressure and temperature. |
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Triple Point |
The point at which all three phases are in equilibrium (all present in the same place at the same time) |
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Critical Point |
The end of the gas-liquid phase transition line |
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Supercritical Fluid |
No distinction between liquid and gas. |
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Attractive Forces |
Holding together particles that are weakly attached. Not much energy is required to separate particles. They break apart and reattach often under normal conditions. |
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Bond |
Ionic and covalent attractions between atoms or ions. |
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Chemical Bonds |
Ionic and covalent bonds |
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Intermolecular Forces |
Attractive forces between molecules. |
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Temporary Dipoles |
Form due to random motion of 'electron clouds' |
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London Dispersion Forces |
The attraction between partial charges (temporary dipole and an induced dipole) |
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Dipole-Dipole Forces |
Attraction between permanent dipoles. |
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H-Bonds |
The strong electrostatic attraction between a very Ω+ H-atom and a 'concentrated' lone pair of electrons (Ω-) on an O, N, or F-atom. |
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Dipole-Induced Dipole Forces |
A polar molecule (permanent dipole) can induce a temporary dipolein a nonpolar atom/molecule. |
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Ion-Induced Dipole Forces |
An ion induces a temporary dipole in a nonpolar atom/molecule. |
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Ion-Dipole Forces |
Attractive force between an ion and a molecule with a permanent dipole. |
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Vapor Pressure |
The pressure of the gaseous vapor above a liquid. |
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Boiling |
When the vapor pressure is equal to the atmospheric pressure. |
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Surface Tension |
The energy used to create new surface area (J/m^2). The energy needed to seperate the molecules. |
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Capillary |
When a liquid rises up into a narrow space. Occurs when there is a stronger attraction between liquid molecules and the sides of the glad tube than between the lewis molecules themselves. |
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Viscosity |
How 'thick' or 'sticky' a liquid is. |
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Solution |
Solute dissolved in a solvent. |
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Molarity |
(Moles of solute)/(liters of solution) |
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Molality |
(Moles of solute)/(kg of solution) |
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Mass percent |
(Mass solute)/((mass solute)+(mass solvent)) × 100% |
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Volume Percent |
(Volume of solute)/(volume of solution) × 100% |
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Mole Fraction |
(Moles of A)/(total moles in mixture) |
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^Hsolvent |
The heat required to seperate the solvent molecules so that the solute can be added - endothermic |
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^Hsolute |
The heat required to separate the solute molecules so that they can be dispersed evenly throughout the solvent - endothermic |
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^Hmix |
The heat produced by the attraction between the solvent and solute molecules/ions (bond formation) - exothermic |
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^Hsolution |
The overall enthalpy change when a solute is dissolved in a solvent - tge solute molecules are separated and dispersed homogeneously throughout the solvent. |
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Exothermic |
Enthalpy decreases |
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Endothermic |
Enthalpy increases |
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Gibbs Free Energy |
Thermodynamic potential |
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Entropy |
The something else that turns H until G includes a measure of how disordered the system is. |
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Why Endothermic Reactions Happen |
The product (the solution) is more disordered than the reactants (the solid and the solvent) - The system's entropy increases. Increase in entropy makes a system a little more stable. This added stability can compensate for the loss of stability that accompanies an endothermic process. |
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Polar Solvent |
A liquid composed of polar molecule. |
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Nonpolar Solvent |
A liquid composed of nonpolar molecules. |
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Henry's Law |
Gas solubility = kH × Pgas ((gas solubility 1)/(gas solubility2)) = ((P1)/(P2)) |
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Solubility |
The maximum amount of solute that can be dissolved in a solvent. |
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Colligative Properties of a Solution |
Vapor pressure lowering Freezing point depression Boiling point elevation Osmotic pressure |
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Van't Hoff Factor |
The number of moles of particles produced by 1 mole of solute. |
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Van't Hoff Factor Equation |
i = (moles of particles in solution)/(moles of solute in solution) |
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Raoult's Law |
When a solute, B, is added to a solvent, A, the vapor pressure of the solvent can be found using the mole fraction of the solvent, XA, in the solution; PA=P°A×XA PA - the new vapor pressure of the solvent in the solution P°A - the vapor pressure of the pure solvent. |
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Freezing Point Depression |
^Tf=i×Kf×cm ^Tf - the difference between the freezing point of the pure solvent and that of the mixture. i - van't Hoff factor cm - molal concentration of the solute (mol/kg) |
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Boiling Point Elevation |
^Tf=i×Kb×cm Kb - the boiling poit elevation constant. |