chemistry important question i
... (Atomic mass of Cu = 63.55 u and Avogadro’s number NA = 6.02 × 1023 mol–1) How would you account for the following: (i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent. (ii) In a transition series of metals, the metal which exhibits the greatest ...
... (Atomic mass of Cu = 63.55 u and Avogadro’s number NA = 6.02 × 1023 mol–1) How would you account for the following: (i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent. (ii) In a transition series of metals, the metal which exhibits the greatest ...
Welcome to AP Chemistry!
... 1. The oxidation number of any uncombined element is O. 2. The oxidation number of a monatomic ion equal the charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in ...
... 1. The oxidation number of any uncombined element is O. 2. The oxidation number of a monatomic ion equal the charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in ...
Word - chemmybear.com
... a) all salts containing NH4+ are soluble. b) all salts containing NO3– are soluble. c) all fluorides are soluble. d) all sulfates (except those of Ca2+, Sr2+, Ba2+, and Pb2+) are soluble. e) most hydroxides are insoluble, except those of Ca2+, Sr2+, Ba2+, the alkali metals and NH4+. ...
... a) all salts containing NH4+ are soluble. b) all salts containing NO3– are soluble. c) all fluorides are soluble. d) all sulfates (except those of Ca2+, Sr2+, Ba2+, and Pb2+) are soluble. e) most hydroxides are insoluble, except those of Ca2+, Sr2+, Ba2+, the alkali metals and NH4+. ...
MASS-INDEPENDENT ISOTOPE FRACTIONATION OF CHROMIUM
... Experimental: Experiment (a) Liquid-liquid extraction with macrocyclic compounds is known to be effective to show larger chemical isotope fractionation ...
... Experimental: Experiment (a) Liquid-liquid extraction with macrocyclic compounds is known to be effective to show larger chemical isotope fractionation ...
Semester II Review
... SM II Review • If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase • What happens to the temperature of a gas when it is compressed? Increases • What happens to the pressure of a gas inside a container, if the temperature of the gas ...
... SM II Review • If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase • What happens to the temperature of a gas when it is compressed? Increases • What happens to the pressure of a gas inside a container, if the temperature of the gas ...
File
... solution. since the salt dissociates into 2 particles for every NaCl that dissolves, it will increase the boiling point more that an equal concentration of sugar (a molecular cpd) that does not dissociate or ionize. (c) at low temperatures and high pressures, the methane molecules are slow and close ...
... solution. since the salt dissociates into 2 particles for every NaCl that dissolves, it will increase the boiling point more that an equal concentration of sugar (a molecular cpd) that does not dissociate or ionize. (c) at low temperatures and high pressures, the methane molecules are slow and close ...
Midterm 1 2009 (PDF format)
... d) H is the value of q measured under conditions of constant volume. e) The enthalpy change of a reaction is the reciprocal of the ∆H of the reverse reaction. ...
... d) H is the value of q measured under conditions of constant volume. e) The enthalpy change of a reaction is the reciprocal of the ∆H of the reverse reaction. ...
普通化学 (全英文) 教学大纲
... (a)．Solubility: # grams of solute / 100 g solvent; Molarity: # moles of solute / 1 L solution (b)．Be able to convert between solubility and molarity of a given solution 6.3．Electrolyte (a)．Strong electrolyte: fully dissociate into cations and anions in solution or melt (b)．Weak electrolyte: partiall ...
... (a)．Solubility: # grams of solute / 100 g solvent; Molarity: # moles of solute / 1 L solution (b)．Be able to convert between solubility and molarity of a given solution 6.3．Electrolyte (a)．Strong electrolyte: fully dissociate into cations and anions in solution or melt (b)．Weak electrolyte: partiall ...
Liquid–liquid extraction
Liquid–liquid extraction (LLE) consists in transferring one (or more) solute(s) contained in a feed solution to another immiscible liquid (solvent). The solvent that is enriched in solute(s) is called extract. The feed solution that is depleted in solute(s) is called raffinate.Liquid–liquid extraction also known as solvent extraction and partitioning, is a method to separate compounds based on their relative solubilities in two different immiscible liquids, usually water and an organic solvent. It is an extraction of a substance from one liquid into another liquid phase. Liquid–liquid extraction is a basic technique in chemical laboratories, where it is performed using a variety of apparatus, from separatory funnels to countercurrent distribution equipment. This type of process is commonly performed after a chemical reaction as part of the work-up.The term partitioning is commonly used to refer to the underlying chemical and physical processes involved in liquid–liquid extraction, but on another reading may be fully synonymous with it. The term solvent extraction can also refer to the separation of a substance from a mixture by preferentially dissolving that substance in a suitable solvent. In that case, a soluble compound is separated from an insoluble compound or a complex matrix.Solvent extraction is used in nuclear reprocessing, ore processing, the production of fine organic compounds, the processing of perfumes, the production of vegetable oils and biodiesel, and other industries.Liquid–liquid extraction is possible in non-aqueous systems: In a system consisting of a molten metal in contact with molten salts, metals can be extracted from one phase to the other. This is related to a mercury electrode where a metal can be reduced, the metal will often then dissolve in the mercury to form an amalgam that modifies its electrochemistry greatly. For example, it is possible for sodium cations to be reduced at a mercury cathode to form sodium amalgam, while at an inert electrode (such as platinum) the sodium cations are not reduced. Instead, water is reduced to hydrogen. A detergent or fine solid can be used to stabilize an emulsion, or third phase.