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Chemistry - terms
| Term | Definition | |
|---|---|---|
| electrolytic solution | conducts electricity - contains ions | |
| AVOGADRO NUMBER | 1 mol = 6•10²³ atoms | |
| Strong acids | With Cl, HNO3, HBr, HI, H2SO4 | |
| Lattice Energy | Energy released to put together (or separate) 2 ions that form a crystal. chargee of ions ⬆️, LE ⬆️ radius of atoms ⬆️, LE ⬇️ ⬇️ LE, ⬆️ soluble in water LE = (K•Q1•Q2) / R | |
| Allotrope | Different forms of an element; #O2 and O3; Carbon: diamond and graphite (conducts electricity) | |
| Density | d = m/v | |
| Molarity | M = mol/L (moles of solute / L of solution) Also called molar concentration | |
| Molality (m) | m = mol/kg (moles of solute / kg of solution) | |
| Mole fraction | ||
| Xsolute = moles of solute / total moles of solution Xsolvent = moles of solvent / total moles of solution Xsolute + Xsolvent = 1 - useful when calculating partial pressure (Pa) given the total pressure (Pt) in a vessel -> Pa = Xa•Pt | ||
| Formula: Q = m•c•∆T | Q = amount of heat (J) m = mass (g) c = specific heat capacity (J/g•°C) ∆T = variation of temperature (°C) | |
| 1atm | 760mm Hg (1 Torr) | |
| Amphoteric | Can behave as acid (loses a proton = - H+) AND base (receives a proton = + H+) | |
| Potential Energy | Energy released when bonds are broken G > L > S - releases energy → exo → ⬆️PE - absorbs energy → endo → ⬇️PE (not really related to Temperature) - changes when the substance changes between physical states (when there's no temperature change) | |
| n → atomic number (Z) X → element ~ → atomic mass | n - number of p+ (if you use electron configuration, = the sum of "exponents" [e-]) atomic mass - molar mass of an element (1 mol of X has atomic mass Yg) "Weight" | |
| Atomic radius (AR) | Atom's size more levels, bigger less p+, bigger ↓← (increases like that on the periodic table) | |
| Ionization energy (IE) | Energy needed to REMOVE 1 e- →↑ (increases like that on the periodic table) | |
| Electronegativity (EN) | How well an atom can ATTRACT e- F O N Cl Br I S C P H + <———————————————— - →↑ (increases like that on the periodic table) | |
| Electron affinity (EA) | Energy absorbed or released when an e- is ADDED to an atom →↑ (increases like that on the periodic table) | |
| Energy released to put together (or separate) 2 ions that form a crystal. LE = (K•Q1•Q2) / R | #chargee of ions ⬆️, LE ⬆️ ____#radius of atoms ⬆️, LE ⬇️ ____#⬇️ LE, ⬆️ soluble in water | |
| Litmus paper | Basic - blue; acidic - red | |
| Van't Hoff Factor (i) | Number of particles that a compound breaks into when it dissolves in a solution. _____ ⬆️i ⬆️boiling/melting point___________ ∆T=Kb (constant) • M • i | Examples: NaCl → Na+ + Cl- ≈> i=2;__AgNO3 → Ag+ + NO3- ≈> i=2 |
| Entalphy | ∆H = - → exo; ___ ∆H = + → endo | |
| Activation Energy | Difference between the reactants and the transition state. | If it finishes higher than it started = ENDO; ___ if it finishes lower, EXO |
| Gibbs Free Energy | ∆G = ∆H - T • ∆S (entalphy - temperature • entrophy) | ∆G = - → spontaneous reaction; ___ ∆G = + → non spontaneous reaction |
| Vapor pressure | Equilibrium (rate of evaporation of liquid = rate of condensation of gas) pressure of a vapor above its liquid. | Factors that affect V.P.: #Temperature: ⬆️T, ⬆️ V.P ___ #Types of molecules: intermolecular forces ⬆️, VP⬇️; intermolecular forces ⬇️, VP⬆️ |
| Le Chatelier's principle - equilibrium shift | 1. Concentration: increase in one side, the equation "goes" to the other. _._._._._._._._._._._._._._._._._._._._._._._ 2. Temperature: ↑T - goes to ENDO +; ↓T - goes to EXO - | 3. Pressure: ↑P - goes to less volume (smaller coef); ↓P - goes to bigger volume (bigger coef). _._._._._._._._._._._. 4. Catalyst: no shift!! Just makes faster! (Decreases Activation Energy) |
| Entrophy | Degree of disorder | Solids = ↓E; Gas = ↑E |
Created by:
ka_martins
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