Pharmaceutical Inorganic Chemistry – Flashcards
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Arrhenius
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Attributes water ion theory of acid and bases
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Sulphate
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Sulfur ion doesn't react with H2SO4
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Sublimation
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Direct transition of solid to vapor state
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Specific heat
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Heat required to raise temp. of 1g by 1 celcius
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Alpha ray
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Radioactive particle weighing the same as Helium
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Molecular formula
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Formula that gives actual number of atoms
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Carbon
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Graphite is an allotrope of the element?
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Halogens
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Salt-forming group of elements
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Amphoteric
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Acts as either an acid or base
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Oxygen
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Most abundant and essential of all elements
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Ferric
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An ion that gives the Prussian blue precipitate with Potassium Ferrocyanide
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Fluorine
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Most electronegative element
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Meyer and Mendeleev
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Author of the Periodic Table
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Bose Consendates
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State of matter that only occurs at near absolute zero
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Molecule
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Atoms that are tightly bound together and behave as one
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Colloid
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Exhibits the Tyndall Effect
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Electronegativity
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Ability to attract electrons of another atom to its side
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Lewis Base
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Electron pair donors
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Molecular mass
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Sum of atomic masses of all the atoms in a molecule
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Neutralization
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Reaction between acid and base that produces salt and water
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Precipitation
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Reaction in which an insoluble solid forms when reactants are combined
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Oxidation
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Involves loss of electrons Involves addition of oxygen and loss of hydrogen
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Reduction
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Involves gain of electrons Involves addition of hydrogen and loss of oxygen
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Enthalpy
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Amount of heat absorbed or released during a reaction
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Exothermic
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A reaction when the energy of products is less than the energy of reactants
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Endothermic
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A reaction when the energy of products is greater than the energy of reactants
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Carbon Dioxide
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Used to mask the disagreeable taste of certain medicines
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Deliquescent
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Substances that take or absorbs sufficient water from the atmosphere forming a liquid
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Cadmium
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Causes Itai-itai Disease
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Chromium
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Element present in insulin
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Zinc
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Added to Copper to produce Yellow Brass
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Alkali metal
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Soluble group of the Periodic Table
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Brick red
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Calcium imparts this color to a non-luminous flame
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Silicosis
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Lung condition resembling tuberculosis symptoms
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Saline Cathartic
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Rochelle Salt is used as:
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Cesium
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First element discovered using spectroscope
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General Anesthetics
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Use of Laughing gas
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Potassium bitartrate
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Cream of tartar is:
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Ferric Oxide
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Imparts pink color to Calamine USP
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Aluminum
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Cation that is used as antacid that cases constipation.
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Lithopone
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Mixture of 30% ZnS and 70% BaS
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Bronsted-Lowry
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Protonic concept of acidity
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Selective Toxicity
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Property of chemical agents to destroy one form of life without harming another.
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Neopentane
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Common name of tetramethylmethane
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Redox
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Infants are capable of this metabolic reaction
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Chemistry
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Branch of science that deals with matter
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Law of Definite Proportions
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Elements combine in fixed ratios of whole numbers to form compounds
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Law of Multiple Proportions
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Elements may combine in different ratios of whole number to form different compounds
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John Dalton
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He discovered the Law of Multiple Proportions
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Antoine Laurent Lavoisier
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He discovered Law of Definite Proportions Tabulated the elements
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Wilhelm Conrad Roentgen
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He discovered the X-Ray
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Antoine Henri Becquerel
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He discovered Uranium
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Marie Curie
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Gave the name Radioactivity
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Radioactivity
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The spontaneous emission of radiation from certain unstable element
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Polonium and Radium
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Pierre Curie and Marie Curie discovered this elements
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Atomic Number
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Specific for each element Same for all atoms of an element Equal to number of protons or electrons
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Mass number
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Represents the number of particles in the nucleus Equal to number of protons + neutrons
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Isotopes
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Atoms with same element having different mass number Have same number of protons but different neutrons
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Pauli's Exclusion Principle
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Each atomic orbital can accommodate 2 electrons No two electrons can have same set of quantum number
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Hund's Rule
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Orbital are filled up singly before pairing up
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Aufbau Principle
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Lower energy levels are filled up first
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Heisenberg Principle
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It is impossible to determine simultaneously the momentum and position of an electron
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Atomic Radius
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Distance between 2 nuclei Increases from right to left Increases from top to bottom
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Electronegativity
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Ability to attract electrons Increases from left to right Increases from bottom to top
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Ionization Energy
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Ability to remove an electron from a positively charged atom Increases from right to left Increases from bottom to top
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Electron affinity
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Property to accept an electron Increases from right to left Increases from top to bottom
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Ionic Compounds
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Has positive and negative ions Have high melting and boiling point Solid at room temperature
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Ionic bond
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Bond that occurs between metal and nonmetal ions
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Covelant bond
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Bond that occurs when atoms share electrons Bond between two nonmetals
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NonPolar bond
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Has equal or almost equal sharing of electrons Almost no electronegativity difference (0.0-0.4)
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Law of Conservation of Mass
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States that matter cannot be created or destroyed
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Polar bond
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Has unequal sharing of electron Moderate electronegativity difference (0.5-1.7)
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Democritus
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Stated that matter is composed of indivisible particles called "atomos"
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John Dalton
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Stated that matter is composed of indivisible particles called "atoms". Proposed the Billiard Ball Model
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JJ Thompson
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Stated that an atom is a sphere of a positive article to which are embedded the negative particles Proposed the Raisin-Bread Model
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Ernest Rutherford
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Proposed the Gold Film Experiment and Nuclear Model
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Neil Bohr
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Proposed the Planetary Model
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Edwin Schrodinger
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Stated that electrons move in a 3D space which is called electron cloud Proposed the Quantum-Mechanical Model
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Quantum Numbers
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Set of numbers that are used to describe electrons
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Principal Quantum
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Determines the total energy of an electron Size of electron cloud Main energy level
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Azimuthal Quantum
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Determines the shape of electron cloud Dependent to Principal Quantum
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Magnetic Quantum
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Determines the orientation in space of the electron cloud
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Magnetic Spin Quantum
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Determines the direction of rotation of the electrons
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Van der waals
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Weakest Intermolecular Force Used by non-polar molecules
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Dipole-dipole
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Stronger van der waals Used by polar molecules
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H-bond
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A bond when Hydrogen attached to N,O,F Strongest intermolecular force
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Boyle's Law
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Volume of gas is inversely proportional to pressure. Constant temperature
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Charles' Law
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Volume of gas is directly proportional to absolute temperature. Constant pressure
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Arrhenius Theory
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States that acids yields H+ while bases yields OH- in a aqueous solution
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Bronsted-Lowry Theory
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States that acid is a proton donor while a base is a proton acceptor
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Lewis Theory
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States that acid is an electron pair acceptor while bases are electron pair donor
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Solution
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Uniform mixture and composed of solute and solvent
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Suspension
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Aka Coarse Mixture, finely divided solid materials distributed in liquid
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Strong Electrolyte
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Dissociate in water producing positive and negative ions Dissolved in water will conduct an electric current
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Weak Electrolyte
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Dissociate only slightly in water Forms a solution with few ions.
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Nonelectrolyte
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Dissolve as a molecule Do not produce ions in water Do not conduct electricity
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Solubility
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The maximum amount of solute that dissolves in a specific amount of solvent
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Osmotic Pressure
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Pressure that prevents the flow of additional water into the more concentrated solution
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Buffers
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Resist changed in pH from the addition of acid or base
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Hydrogen
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Inflammable air Lightest element
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Protium
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Most abundant H isotope
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Deuterium
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Heavy Hydrogen
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Tritium
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Radioactive H
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Lithium
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Lightest metal
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Sodium
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Most abundant extracellular cation
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Potassium
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Most abundant Intracellular cation
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Cesium
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Catalyst in polymerization of resin
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Ammonium
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Hypothetical alkali metal
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Copper
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Only reddish colored material 3rd most malleable metal 3rd best conductor of electricity
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Silver
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2nd most malleable metal 2nd best conductor of electricity Poisoning is called argyria
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Gold
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King of metals Most malleable Best conductor of electricity
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Selenic Acid
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Can dissolve Gold (Au)
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Alkali Metal
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Aka Group 1A Includes H, Li, Na, K, Cs, NH4
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Coinage Metal
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Aka Group 1B Includes Cu, Ag, Au
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Alkaline-Earth Metal
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Aka Group 2A Include Be, Mg, Ca, Sr, Ba, Ra
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Beryllium
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Most toxic metal Causes lung carcinoma, chronic granuloma
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Magnesium
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2nd most abundant intracellular cation Present in chlorophyll Component in Grignard reagent
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Calcium
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2nd most abundant extracellular cation Blood coagulation factor
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Strontium
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Used for red pyrotechnics
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Barium
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Used for green pyrotechnics Causes baritosis
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Zinc
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Also present in insulin Container for batteries and dry cells Protective coating of galvanized iron Deficiency causes parakeratosis
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Mercury
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Causes Minamata disease
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Boron Family
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Aka Group3A Includes B, Al, Ga, Thallium
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Boron
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Used in vulcanizing rubber
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Aluminum
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Most abundant metal 3rd most abundant element Causes Shaver's disease
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Thallium
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Rodenticide Poisoning causes green tongue and alopecia
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Volatile Metal
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Aka Group2B Includes Zn, Cd, Hg
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Carbon Family
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Aka Group 4A Include C, Si, Sn, Pb
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Carbon
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Can form bonds with itself
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Silicon
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2nd most abundant element
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Lead
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Poisoning is called plumbism
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Titanium Family
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Aka Group 4B Includes Ti, Zr
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Titanium
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Powerful reducing agent Reflect UV rays
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Zirconium
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Used deodorant and antiperspirant Causes granuloma formation
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Nitrogen Family
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Aka Group5A Includes N, P, Ar, An, Bi
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Nitrogen
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Inert atmosphere for oxidizable pharmaceuticals
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Arsenic
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Component of salvarsan Aka Lewisite Metal
