General Chemistry PDF

SUMMARY Debye-Huckel Theory Equation that provides the starting point for PRINCIPLES/LAWS/THEORIES the modern treatment of non-ideality of...

SUMMARY Debye-Huckel Theory Equation that provides the starting point for PRINCIPLES/LAWS/THEORIES the modern treatment of non-ideality of electrolyte solutions Heisenburg Determination of a particle's momentum Uncertainty Principle and position cannot be determined with Henderson- Equation for buffers certainty Hasselbach Theory Proust's Law aka Law of A compound will always have the same Van Slyke Equation Equation for buffer capacity Definite Proportions elements in the same proportion by mass Octet Rule Phenomenon where an atom forms a Law of Multiple When elements combine to form more stable molecule; atoms are most stable Proportions than one compound, their weights when their valence shells are filled combine in a fixed manner in a ratio of small whole numbers Almost always works for C, O, N, F, Law of Elements combine in the ratio of their Na, and Mg Equivalents/Reciprocal combining weights Proportions/Combining Duet rule Applicable to Hydrogen which needs only 2 Weights electrons to be complete Law of Conservation of Matter can neither be created nor Gilbert Lewis Together with Albrecht Kossel, were the first Mass/Dalton's 4th destroyed to explain the formation of chemical Theory bonding Pauli's Exclusion It states that no two electron can have the Boyle's Law Relationship of volume and pressure; Principle same set of quantum number States that at constant temperature, the volume is inversely proportional to the pressure Hund's Rule of Orbitals with the same electrons of the Maximum Multiplicity same energy levels must be filled in singly Charles Law Relationship of temperature and volume; before pairing constant pressure, the volume is directly proportional to the absolute temperature Aufbau Principle Atoms may be built by progressive filling of the main energy levels, the sub-levels, and Gay-Lusaac's Law Relationship of pressure and temperature; orbitals with electrons according to constant volume and mass, when increasing sequence measured at the same temperature and  pressure, the ratios of the volume of Zeroth law If 2 systems are in equilibrium with a third reacting gases are small whole numbers system, the first two are in equilibrium with one another Ideal Gas Law Aka General Gas Law Equation Combined Gas Law Combination of Boyle's Law and Charles MODELS Law; states that in a given mass of a gas, the volume is inversely proportional to the Rutherford/Nuclear Model Protons in nucleus, electrons are pressure and directly proportional to the outside absolute temperature Bohr/Planetary Model Electrons are in several definite orbits Dalton's law of Partial In a mixture of gases, the total pressure is Pressure the sum of the partial pressure of all Wave Mechanical Model Positive nucleus at center with an components aka Electron Cloud Model electron cloud surrounding it Avogadro's Law Equal volumes of different gases at the Thomson/Plum Pudding Spherical atom with electrons same temperature and pressure contain Model embedded equal number of molecules Graham's Law of Under the same conditions, the ratio of Diffusion diffusion of gases is inversely proportional to the square root of their molecular mass IMPORTANT TERMINOLOGIES Chemistry Study of matter, its properties and 1st Law / Law of States that energy cannot be created nor Conservation of destroyed, energy can be transferred behaviors, and the changes that it Energy between a system and a surrounding or undergoes converted but the total amount of energy in Atoms Basic unit (building blocks) that the isolated system remains constant makes up all matter 2nd Law / Law of States that spontaneous natural processes Properties Any characteristic that allow us to Entropy / Law of will increase the entropy and can never distinguish a specific type of matter Disorderliness decrease from other types of matter 3rd Law States that the entropy of a pure crystalline Democritus Coined the term atomos which also substance at absolute zero is also zero meant indivisible Constant value is called residual entropy Quantum Numbers These are electron wave dimensions commonly used in electrochemical indicated by numbers cells, semi-conductors (di-odes) Principal QN (n) Corresponds to the main energy Anode Where a current flows into (entry); level; describes the SIZE of the positively charged electrode orbital Cathode Where a current flows out of (exit); Azimuthal/Angular Describes the SHAPE of the orbital; negatively charged electrode Momentum QN (l) gives angular momentum of electron Pure Substance Made up of only one kind of matter Value = 0 to n-1 with a definite, fixed, and unvarying composition Magnetic QN (m) Describes behavior in magnetic Elements Simplest form of a substance that field and orientation in space cannot be decomposed by Value = -1 to +1 chemical means; building blocks of matter Spin/Electron QN (s) Describes the spin about its own axis in clockwise or counter-clockwise Most abundant elements in the Hydrogen, Helium, and Oxygen direction universe Periods Horizontal rows in the periodic table Most abundant elements in the Oxygen, Silicon, and Aluminum crust Groups/Families Vertical columns in the periodic table Most abundant elements in the Oxygen, Carbon, and Hydrogen body Ions A molecule where the number o felectrons and protons are not Metallic compounds Formed between substances equal, therefore has a net positive or between metals but behave like negative charge ordinary metals Molecules Aggregates of atoms in definite Ionic compounds Involves the transfer of electrons to arrangement held together by a more electronegative atom chemical forces Organic Compounds Compounds with carbon covalently Electrode Conductor used to make contact bonded to other elements with a non-metallic part of a circuit;  **Carbides, carbonates, carbon Ionic Bond Transfer of electrons; usually monoxide, carbon dioxide, and involves metal and non-metals cyanates are exceptions to the rule Covalent Bond Sharing of electrons; common between 2 non-metals Buffer Capacity Maximum amount of a strong acid or base that can be added until a Polar Covalent Bonds/Polar Electrons are significant change in pH will occur Bond shared unequally since more electronegative atoms are present Salts Combination of a positive and which pull electron pairs closer to negative ion; the product of a them, away from the less neutralization reaction electronegative species Acid + Base = Salt and Water Chlorine is the MOST Colloids Have particles larger than solutions electronegative but smaller than suspensions; e.g., shampoo, mayonnaise, toothpaste Coordinate Covalent A bond where one element shares Bond aka Dative/Dipolar Bond two of its own electron with another Chemical Bonds Forces that hold atoms together to element to make a bond form a compound Metallic Bond Term used to describe the collective Isoelectronic/Equal These are two atoms, ions, or sharing of valence electrons between Charge/Equal Electric molecules that have the same several positively charged metal electronic structure; same number of ions valence electrons INTERMOLECULAR BONDS Attractive forces between the Lewis Dot Symbol Consists of the symbol of an element (IMF) positive and negative ends of and one dot for each valence molecules; responsible for most electron physical and chemical properties of matter Transition metals, lanthanides, and actinides have incompletely filled Van der Waals Has very weak forces due to its inner shells and are dependence on generally excluded in the Lewis dot the distance between atoms or symbol molecules Hydrogen Bond A special class of attractive IMF that Ion-induced Dipole Interactions that are similar to the arise due to the dipole-dipole dipole-dipole except for the fact that interaction between the Hydrogen they arise ion bonded to a highly between ions and polar molecules electronegative atom Structural Formula Shows how atoms are bonded to one Polar molecules A molecule that has a combination of another in a molecule a negative and positive charge Molecular Formula Shows the exact number of atoms of Non-polar molecules Do not have opposite charges each element present in a molecule in the smallest unit of a substance Resonance structure 2 molecules where the chemical interactions are Empirical Formula Tells which elements are present and the same but the distribution of expressed in the simplest whole electrons are different number ratio London Weakest bond Thermodynamics Deals with the transfer of Dispersion Forces/Induced Between 2 non-polar energy from one place to another or dipole-Induced dipole molecules one form to another Dispersion happens The key concept is that heat is due to the movement the form of energy that corresponds of electrons leading to a definite amount of mechanical to the formation of work temporary positive and negative charges Entropy The measure of in non-polar disorderliness/randomness in a system Keesom Forces/Dipole-dipole Interaction between the dipoles in polar molecules TABLES Debye Forces/Dipole-induced Caused by the interaction of QUANTUM NUMBERS dipole permanent dipoles and other molecules that lead to the formation Orbital QN Value Shape Value in Electron of induced-dipoles; between polar Config and non-polar molecule s 0 spherical shape 2 p 1 dumbbell shape 6 d 2 complex or double 10 dumbbell shape f 3 clover-leaf shape 14 ELECTRON CONFIG THEORY Main Energy Level Maximum No. of Electron 1st 2 2nd 8 (2s, 6p) 3rd 18 (2s, 6p, 10d) 4th 32 (2s, 6p, 10d, 14f) Theory Acids Bases Arrhenius Dissociate in water to form Dissociate in water to hydrogen ions (H+) e.g. HCl, form hydroxide ions H2SO4, HNO3 (OH-) e.g. KOH Bronsted- Proton DONORS Proton ACCEPTORS Lowry Lewis Electron ACCEPTORS Electron DONOR Litmus Red Blue Paper