States of matter

Quinn Karylle Fuentes · 28問 · 2年前

通報

問題一覧

Anything that occupy space and has mass.

Matter.

Particles cannot move; easily compressed.

Solid.

Particles can move; not easily compressed.

Liquid.

Particles easily moved

Gas.

1st part solid/ 1st part liquid.

Mesophase.

Gaseous superfluid cooled with low temperature

Bose Einstein.

Liquid- solid

Freezing.

Solid-liquid.

Melting point.

Solid-gas.

Sublimation.

Gas to solid

Deposition.

Liquid to gas.

Vaporization.

Gas to liquid.

Condensation.

Gas to plasma.

Ionization.

Plasma to gas

Recombination.

•Have kinetic energy rapid motion •Weak intermolecular forces •Capable of filling all available spaces •Many are invincible

Gases.

Iodine gas

Violet.

Chlorine gas.

Greenish.

Bromine gas

Reddish brown.

Temperature/ pressure added.

Enthalpy.

Disorderliness; heat or pressure applied.

Entropy.

Equilibrium pressure of liquid directly proportional to temperature.

Vapor pressure.

Vapor pressure is independent of the surface area

Surface area.

The IMF Is strong VPBis low.

Type of molecule.

at high temp molecules gains enough energy to change phases l and vice versa.

Temperature.

Density smaller than other phase; form homogenous mixture and have a high kinetic energies

Gas.

Ideal gas obey all gas laws under all conditions of temperature and pressure. (true/false)

True.

Obey gas law only at low pressure and high temperature.

Real gas.

What is the ideal gas equation

PV=nRT.

Inverse relationship pressure and volume at constant temperature

Boyle's law.

Direct relationship volume and temperature at constant pressure

Charles law.

Direct relationship volume and temperature at constant pressure

Charles law.

Pressure and temperature are directly proportional.

Gay Lussac's.

Volume of gas is directly proportional the number of moles

Avogadro's law.

At constant temp amount of given gat that dissolve in a volume of liquid is directly proportional to the partial pressure off that gas in equilibrium with that liquid.

Henry's law.

Total pressure exerted = sum of partial pressure of individual gasses.

Dalton's law.

Rate if diffusion or effusion of the gas is inversely proportional ti the square root it's molecular weight.

Graham's law.

With high pressure (pressure filling) temp is reduced (cold filling) result to loss of energy for changing into liquid state.

Liquefaction of gasses.

Max temperature in which gasses cannot be liquified.

Critical temperature.

Required pressure to liquified a gas in it's TC.

Critical pressure.

Vol of mole of gas at its TC and PC

Critical volume.

When pressure is reduced liquid reverts to gas.

Aerosol.

Suspension of fine solid particles or liquid droplets in air or another gas.

Aerosol.

Relation between vapor pressure and absolute temperature of a liquid.

Clausius Clapeyron equation.

Heat taken when liquid vaporized and are lost or liberated when they condense back to liquid.

Latent heat of vaporization.

Heat absorbed by 1 mole of liquid when it passes vapor state.

Molar heat of vaporization.

Absorbed heat is used to change liquid to vapor and does not rise until liquid is completely vaporized.

Boiling point.

In fixed of geometric pattern or lattice.

Crystalline.

Give a definite shape and orderly arrangements.

Lattice.

Imperfections that dictates hardness band strength of metals.

Lattice defects.

Incompressible and brittle than solid.

Crystalline.

Can be broken with equal amount of energy due to same bond length.

Crystalline.

Have definite melting points.

Crystalline.

Respond differently to forces depending on the impact direction.

Anisotropic.

Cubic.

Sodium chloride.

Tetragonal.

Urea.

Hexagonal

Iodoform.

Rhombic.

Iodine.

Monoclinic.

Sucrose.

Triclinic.

Boric acid.

The temperature in which pure liquid and solid exist in equilibrium.

Melting point.

Heat required increase distance to crystalline.

Heat fusion.

Heat absorbed when 1g of solid melts or liberated when it freeze.

Latent heat fusion.

Amount of heat absorbed when 1 mole of solid change into 1mole of liquid.

Molar heat fusion.

String carbon covalent bond

Atoms.

Strong metal bond hardness depends on lattice defects.

Metallic.

Soft covalent bond with low MP

Molecular.

Electrostatic ionic water soluble with high MP

Ionic.

Super cooled liquid with random arrangements.

Amorphous.

Soluble and more bioavailability.

Amorphous.

Respond the same to forces from every direction.

Isotropic.

Di not have definite melting points

Amorphous.

The ability exist in two or more crystalline forms with different arrangements that exhibits different physicochemical properties.

Polymorphism.

Crystalline containing molecules.

Solvates.

Melts at 18°c

Unstable gamma.

Melts at 22°c

Alpha.

Melts at 28°c

Beta prime.

Melts at 34.35°c

Stable beta.

Change in one direction from metastable to stable.

Monotropic.

Change in various direction associated in temperature or solvent.

Enantiotropic.

In what temp to hear cacao butter to not destroy nuclei.

33°

Beta polymorphism is what degree of temperature?

24.5°

Theobroma beta nuclei will be destroyed in what constant temperature

35°

Occurs between solid and liquid posses both characteric of both binding force and random positioning bof liquid.

Mesophase.

Propertyb of crystal and liquid crystal to divide light into two compartment bwith different velocities and refractive index.

Birefringence.

Depending on temp crystal obtain heating from heating solid to obtain mesophase.

Thermotropic.

Mobile in three directions

Nematic.

Mobile in two direction phase with most pharmaceutical significant used in emulsion.

Smectic.

A special type of nematic layer ls of parallel mesogens have their longitudinal axes rotated adjacent layer in certain angle

Cholestric.

Prepared by mixing two or more substances with one being polar molecule derived from the action of certain solvent on solid.

Lyotropic.

First thermotropic liquid crystal studied and recorded by rienitizer in 1888

Cholesteryl Benzoate.

Mesophase from gaseous state that is held under temp and pressure exceed critical point.

Superfluid state.

Stable phase structure with the lowest free energy band randomness or disorder of atoms /molecule.

Phase equilibrium.

Homogenous and physical distinct part of a system having all same physicochemical properties.

Phase.

Least number of independent chemical constituents in terms of composition expressed by means of a chemical equation.

Number of components.

Least number of variable factors are fixed automatically and system is defined.

Degree freedom.

Point where 3 phase co exist.

Eutectic point.

Area with curve represent with the two phase.

Binodal curve.

A temperature beyond that makes A and B one phase.

Critical solutions temperature.

Equilibrium with separate Into conjugate phase.

Tie line.

100

Way to calculate portion of each phase present on a phase diagram in two phase field.

Lever rule.

Cell structure.

Cell structure.

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Electrolytes and non electrolytes

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Introduction.

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Capsule.

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Tablets.

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Transdermal

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Distribution.

Distribution.

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Infectious disease.

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Infectious diseases (2)

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All topic. ( Compressed.)

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All topic ( Compressed)

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All topics (compressed)

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Exercise 6 ; Isotonic solution.

Exercise 6 ; Isotonic solution.

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Exercise 5 : Buffers.

Exercise 5 : Buffers.

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Exercise 7 : Factors affecting solubility.

Exercise 7 : Factors affecting solubility.

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Experiment 8: Disintegration.

Experiment 8: Disintegration.

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Experiment 9 ; Interfacial phenomenon and surface tension.

Experiment 9 ; Interfacial phenomenon and surface tension.

EXP 9 : Aromatic ammonia spirit.

EXP 9 : Aromatic ammonia spirit.

EXP 10-11 : CAMPHOR WATER AND CINNAMON WATER.

EXP 10-11 : CAMPHOR WATER AND CINNAMON WATER.

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EXP 12: ACACIA MUCILAGE

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EXP13&14 : Starch and Barrium sulfate.

EXP13&14 : Starch and Barrium sulfate.

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EXP 15 : Liquid petroleum emulsion 1.0

EXP 15 : Liquid petroleum emulsion 1.0

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EXP 15: Liquid petroleum emulsion 1.1

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Enterobacteriaceae.

Enterobacteriaceae.

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SUSPENSION.

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Colloidal.

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Emulsion.

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EMULSION

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ppr

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Introduction.

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Detect and quality variation.

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INTRODUCTION

INTRODUCTION

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lab (1-2)

lab (1-2)

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lab 1-2

lab 1-2

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Pharmaceutical chemistry.

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Unit 3.

Unit 3.

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PUD.

PUD.

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Lipids.

Lipids.

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lipids.

lipids.

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LAB ✨

LAB ✨

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Drug discovery.

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disease of lipids.

disease of lipids.

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Intro (identify structure)

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Carbohydrates

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Dynamic.

Dynamic.

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Unit 1

Unit 1

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