Gen Chem Flashcards
It is anything that occupies space and has mass
Matter
It refers to the amount of matter present in the material
Mass
Classifications of Matter
Element
Compound
Mixture
It is the simplest form of matter, 1 kind of material or atom
Element
Refers to substances composed of two or more elements united chemically in definite proportion
Compound
It is composed of 2 or more substances that are not chemicallv combined
Mixture
Colorless fluid part of blood, lymph, or milk in which corpuscles or fat globules are suspended
Plasma
- Amber- colored protein-rich liquid that separates out wen blood coagulates
- used to provide immunity
- Diagnostic agent
Serum
Classification of Mixture According to the Nature of Particles
Homogenous
Heterogenous
Classification of Mixture According to the Size of Particles
Solution
Suspension
Colloid
uniform mixture (homogenous), composed of solute and solvent where solute is soluble
Solution
Coarse Mixture, finely divided solid materials distributed in a liquid where solid is insol.
Suspension
particles of solute not broken down to the size of the molecules but are small enough to remain suspended and evenly dispersed throughout the medium
Colloid
difference in specific gravity or density
Decantation
evaporation and then condensation
Distillation
speeding up of settling process of a precipitate
Centrifugation
lowering of temp so that the more insoluble comp crystallizes out first
Fractional Crystallization
difference in solvent affinity
Chromatography
Properties of Matter
Intrinsic/Intensive
Extrinsic/Extensive
INDEPENDENT of mass or amount (density, specific gravity, melting point)
Intrinsic/Intensive
- DEPENDENT on mass (weight, volume, pressure, heat content)
Extrinsic/Extensive
change in phase
Physical Change
change in both intrinsic and extrinsic properties
Chemical Change
splitting of a heavy atom
Nuclear Fission
union of 2 light atoms to form a bigger molecule
Nuclear Fusion
the number of protons + the number of neutrons
Mass Number
the number of protons
Atomic Number
Mass number – Atomic number
Neutrons
Protons - Charge
Electrons
- Matter is made up of small indivisible particles
- Coined “atomos”
Democritus
“Billiard Ball Model”
John Dalton
atom is a hard indestructible sphere
Billiard Ball Model
Matter is made up of atoms
All atoms of a given element are alike
Atoms enter into a combination with other atoms to form compounds but remain unchanged during ordinary chemical rn
Dalton’s Atomic Theory
“Raisin Bread” model
JJ Thompson
Proton; Gold Film Experiment: Atom is mostly an empty space (99% passed)
Ernest Rutherford
Planetary model
Niel Bohr Model
Quantum Mechanic Model; “Electron Cloud”
Erwin Schrodinger
electrons move in 3D structure (Orbitals)
Electron cloud
Neutron
James Chadwick
It refers to charged atoms
Ions
atoms of different elements can link together in different ways to form substances with dift properties
Allotrope
Allotropes of Carbon
Diamond and Graphite
Allotropes of Oxygen
O - nascent
O2 - molecular
O3 - ozone
region in space where the probability of finding an electron is greatest
Orbitals
Determine the size of the particle
Principal Quantum Number
Subshell or sublevel, determines the shape (s, p, d, f)
Azimuthal or Angular Momentum
Orbitals, determine the orientation
Magnetic Quantum Number
Direction of the spin or rotation
Spin Quantum Number
The total mass of all products of a chemical reaction is equal to the total mass of all reactants of that reaction
Law of Conservation of Mass
- Inorganic compounds
- A chemical compound always contains exactly the same proportion of elements by mass
Law of Definite Proportions/Proust’s Law
- Organic compounds
- When chemical elements combine, they do so in a ratio of small whole numbers
Law of Multiple Proportion
No two electrons can have the same set of 4 quantum numbers.
Each atomic orbital can only accommodate 2 electrons (Ex: 1s2)
Pauli’s Exclusion Principle
Impossible to determine simultaneously the e- momentum & position
Heisenberg’s Uncertainty Principle
Lower energy levels are filled up first
Aufbau Building Up Principle
Orbitals are filled up singly before pairing up
Hund’s Rule of Maximun Multiplicity
He recognized Hydrogen as an element
First true periodic table
Antoine-Laurent Lavoisier
He discovered Triads (Li, Na, K | Ba, Ca, Sr | S, Se, Te | Cl, Br, I)
Johann Dobereiner
Octaves
John Newlands
Physical and chemical properties are periodic functions of their atomic weights
Meyer and Mendeleev
Elements are arranged based on atomic numbers (present)
Henry Mosley
It explains phases of matter based on movement (exclu. direction) of molecules/ions/atoms
Kinematic Molecular Theory
- definite shape and size, definite volume
SOLID
- follows the shape of container, definite volume
LIQUID
- indefinite shape and volume
GAS
homogenous mixture single phase system of two of more substances
Solutions
maximum amount of solute
Saturated Solution
less solute
Unsaturated Solution
more solute than the solvent can dissolve
Supersaturated Solution
maximum amount of solute expressed in grams that can be dissolved in 100 g of water
Solubility
ability of one substance to mix with another substance
Miscibility
solubility decreases with increase in temp (Mg citrate)
Exothermic
solubility increases with increase in temp
Endothermic
↑ temperature = ↓ solubility of a gas
the solubility of a gas increases as pressure increases
Henry’s Law
Decreased particle size = Increased surface area = Increased solubility
presence of salt decreases solubility
Salting Out
presence of salt increases solubility
Salting In
force of attraction within molecules
Intramolecular Forces
Ex of Intra Forces
Covalent Bond - sharing
- polar (unequal)
- nonpolar (equal)
Ionic Bond - transfer
forces of attraction between molecules; physical attraction
Intermolecular Forces
mass per unit volume (M/V)
Density
density of sample/density of standard
Specific Gravity
reciprocal of specific gravity, opposite of density
Specific Volume
property of solution depend on the number of solute particles dissolved in a solvent
Colligative Property
movement of water across a semipermeable membrane from low to high concentration
Osmosis
causes crenation
Hypertonic
causes swelling/lysis
Hypotonic
0.9% (w/v) NaCl
Isotonic
gradual mixing of molecules of one gas with molecules of another gas by virtue of kinetic properties
Diffusion
passage of a gas under pressure through a small opening
effusion
Acid yields H and H2O
Base yields OH
Arrhenius Theory
Acid - proton donor
Base - proton acceptor
Bronsted-Lowry Theory
Acid - E acceptor
Base - E donor
Lewis Theory
progressive addition of a sol’n of known concentration to a substance of unknown conc
Titration
Substance that changes color at the end point
Indicator
point when equal amounts of acid and base have reacted; non-observable
Neutralization point (Stoichiometric point/Equivalence Point/Theoretical Point)
Experimental approximate of neutralization point; observable
Endpoint
the negative logarithm of the H+ concentration
pH
Sorensen’s pH scale
Neutral = 7
Acidic < 7
Basic > 7
Solutions that have the property of resisting changes in pH when acids or bases are added to them
Buffers
Ability of a buffer solution to resist changes in pH
Buffer Capacity (Buffer action/Buffer efficiency/Buffer index/Buffer value)
an energy transfer due to temperature difference
Heat (q)
form of energy transfer between a system and its surroundings in the form of compression or expansion of gas
Work
total energy attributed to the particles of matter and their interactions within a system, composed of thermal energy and chemical energy
Internal Energy (U)
degree of disorderliness
entropy
energy of a reaction
enthalpy
amount of heat required to raise the temperature of an object or substance by 1 degree
Heat Capacity
amount of heat required to raise the temperature of an object per gram
Specific Heat
reaction wherein heat is absorbed by the system, indicated by a (+) change in enthalpy
Endothermic Process
reaction wherein heat is released by the system, indicated by a (-) change in enthalpy
Exothermic Process
This law states that energy cannot be created or destroyed; it can only be redistributed or changed from one form to another.
Law of Conservation of Energy
Most reactive metals
Valence = 1
Group IA - Alkali Metals
Lightest and most reactive element
Hydrogen (Inflammable air)
Isotopes of Hydrogen
Protium
Deuterium
Tritium
o Lightest metal
o Depressant and Diuretic (SE: hyponatremia)
Lithium (Earth)
Depressant
Lithium bromide
DOC for Mania
Lithium Carbonate (Lithase®, Eskalith®)
o Primary extracellular fluid cation
o Action: fluid retention
Sodium (Natrium)
o Most abundant and predominant intracellular cation
o Deficiency: hypokalemia
o Manifestation: muscle paralysis (Barker’s syndrome)
o Diuretic, Important in muscle contraction
Potassium (Kalium)
Never employed in medicine because it is the most toxic metal
Beryllium
o Lightest of all structurally important metal
o 2nd most abundant intracellular cation
Magnesium
Most malleable and ductile, Best conductor of electricity
Gold
o Only reddish metal, 3rd most malleable, 3rd best conductor
o Protein precipitant, Enhances physiological utilization of iron
COPPER (Cuprum)
Catalyst in polymerization of resin forming material
Cesium
Hypothetical alkali metal
Ammonia
contains 10% NH4; is known as 16° ammonia
Household ammonia
o 2nd most abundant cation in extracellular fluid
o Vit. D is needed for its maximum absorption
Calcium
Temperature desensitizing agent (Sensodyne®)
SrCl2
Radioactive element used for cancer radiotherapy & diagnostic purpose
Radium
o Present in inZulin and carbonic anhydraZe
o Parakeratosis
Zinc
Astringent, manufacture of stink bomb
Cadmium
It is used as anti sebborheic
CdS
Industrial use: In vulcanizing rubber
Boron
o Most abundant metal
o 3rd most abundant element
Aluminum
o Pcol use: treatment of cancer-related hypercalcemia by binding with transferring
o Nonpharma: substitute for mercury in manufacture of arc lamps; Galvanized iron
Gallium
Crystalline form of Carbon
Diamond (purest native form)
Graphite (lead pencil)
Amorphous form of Carbon
Coal
Anthracite
2nd most abundant element, Component of glass
Silicon
Powerful reducing agent
Titanium
Opacifying agent (Ocusert®) and UV ray protectant
TiO2
antiperspirant but banned due to granuloma formation
Zirconium
Most abundant gas in air
Nitrogen 71%
White/yellow (poisonous), Red (non-poisonous)
Phosphorus
o Protoplasmic poison
o Insecticide: Copper Aceto Arsenate (Paris green)
Arsenic
First anti-syphilis (Paul Ehrlich)
Salvarsan/Magic Bullet/Compound 606/Arsphenamine
Astringent, Antiseptic, Internal protective for ulcer, Used in silvering of mirror
Bismuth
Not affected by any body fluid, Sheet form used in repair of bones, nerve and tissue
Tantalum
Most abundant element, discovered by Scheele
Oxygen
Antifungal, Parasiticide, Scabicide, Depilatory agent
Sulfur
Promotes Vit. E absorption, Antioxidant (SeS2 /Selsun blue – anti-dandruff)
Selenium
Becquerel, Atomic bombs
Uranium
Co-factor enzyme
Molybdenum
Strongest oxidizing agent
Fluorine
o Most abundant extracellular anion, green gas
o Used as water disinfectant
Chlorine
Used as bleaching agent
Hyporchlorite
Used in treatment of achlorydria
HCl
Dark reddish brown fuming liquid with suffocating odor
Bromine
o Oldest known germicide
o Expectorant, Antifungal
o Preparation of T3 and T4
o Deficiency: Goiter
Iodine
o Only metallic
o Only synthetic halogen
o Only radioactive halogen
Astatine
o 1st element produced artificially
o Used in preparation of radiopharmaceuticals
Technecium
o 2nd lightest gas
o Donald-duck-like sound
Helium
o Least abundant of all noble gases
o Have inhalational anesthetic activity
Krypton
Most abundant noble gas
Argon
o Synthetic noble gas
o Used for treatment of CA (cervical CA)
Radon
electron carrier in respiration chain; responsible for transport of molecular oxygen
iron
alkaline bases used to neutralize the excess gastric HCl associated with gastritis and peptic ulcers
antacids
persistent golden yellow in flame test
Sodium
violet in flame test
Potassium
Carmine red/Pink in flame test
Lithium
Brick red in flame test
Calcium
Blue in flame test
Pb, As, Sb, Bi, Cu
Colorless in flame test
Ammonium
branch of chemistry that deals with carbon-containing compounds with: H, O, P, N, S, X
Organic Chemistry
Contains 4 binding sites for other atoms to attach to it
These four binding sites, when bonded with other atoms/molecules form a tetrahedron
Carbon
deals with the physicochemical properties of drugs that affect its biological action
ORGANIC MEDICINAL CHEMISTRY
introduced phenol (carbolic acid)
Joseph Lister
Who discovered Salvarsan (compound 606), Selective toxicity
Paul Ehrlich
for sleeping sickness
Atoxyl
anti-infective agents that are used locally
germicides
Fe + S -> FeS (all sulfides are BLACK)
Direct Union
Na2CO3 -> Na2O + CO2
Decomposition/Analysis
Na + HCl -> NaCl + H2
Single Replacement
NaCl + AgNO3 -> NaNO3 + AgCl
Double Displacement
Constant in Boyle’s/Mariotte Law
Temperature
Constant in Charles Law
Pressure
Constant in Gay-Lussac’s Law
Volume
Constant in Avogadro’s Law
6.022 x 10^23
Most systematic nomenclature
IUPAC
Carbon valence
4
Carbon Atomic Number
6
It contains added methanol (wood alcohol) and benzene
Denatured Alcohol
Astringent, rubefacient, refrigerant, mild local anesthetic
Rubbing Alcohol (70%)
nlt 99% ethanol; obtained by azeotropic distillation
Dehydrated/Absolute Alcohol
Rapidly bactericidal (50% to 95%), 40% equal antiseptic power to a 60% ethanol
Isopropyl Alcohol
Used to sterilize temp-sensitive medical equipment and those that could not be autoclaved
Ethylene Oxide
ratio of a dilution of a given test disinfectant to the solution of phenol that is required to kill a
strain of S.typhi under carefully controlled time and temperature
Phenol coefficient
Introduced as surgical antiseptic by Joseph Lister; its use is now obsolete
Phenol
Phenol with 10% water
Liquefied Phenol
2% (shampoo), for athlete’s foot and jock itch
p-chloro-m-xylenol
mixture of three isomeric methylphenols; obtained from coal tar or petroleum
Cresol
Preservative more effective against molds
Methylparaben
Preservative more effective against yeast, more oil soluble so it is preffered for oils and fats
Propylparaben
common in vials of injectables with 1%to 4% concentrations in water or saline
Benzyl alcohol
preservatives in foods and pharmaceuticals at low pH
Benzoic acid
DOC for scabies; from Peru balsam and other resins
Benzyl benzoate
Beta-lactam Antibiotics
Penicillin
Beta-lactamase Inhibitors
Cephalosporins
Carbapenem
Monobactam
Binds to 30s
Aminoglycosides
Tetracyclines
Binds to 50s
Macrolides
Lincosamides
Chloramphenicol
