Chemical Bonding
... These formations are made of crystals of calcium carbonate, CaCO3(s), also known as limestone. Calcium carbonate, as its name and formula suggest, is a compound made up of three different elements. In addition to its crystalline structure, calcium carbonate has high melting and boiling points and di ...
... These formations are made of crystals of calcium carbonate, CaCO3(s), also known as limestone. Calcium carbonate, as its name and formula suggest, is a compound made up of three different elements. In addition to its crystalline structure, calcium carbonate has high melting and boiling points and di ...
Chemistry_Stoichiome..
... 80. 100 mL of 10 % NaOH (w/V) is added to 100 mL of 10 % HCl (w/V). The resultant solution becomes: a) alkaline b) strongly alkaline c) acidic d) neutral 81. Calculate the molality of 1 L solution of 80 % H2SO4 (w/V), given that the density of the solution is 1.80 g mL−1 . a) 9.18 b) 8.6 c) 1.02 d) ...
... 80. 100 mL of 10 % NaOH (w/V) is added to 100 mL of 10 % HCl (w/V). The resultant solution becomes: a) alkaline b) strongly alkaline c) acidic d) neutral 81. Calculate the molality of 1 L solution of 80 % H2SO4 (w/V), given that the density of the solution is 1.80 g mL−1 . a) 9.18 b) 8.6 c) 1.02 d) ...
Peptide bond formation by aminolysin
... should originate from esterified dipeptides (L-Phe-L-Phe-OMe or L-Phe-L-Phe-OEt) due to the following observations: First, L-PheL-Phe-NH2 , the C-terminal modified dipeptide corresponding to the substrates used, only appears in panel A-1. Furthermore, the simple dipeptide L-Phe-L-Phe was observed in a ...
... should originate from esterified dipeptides (L-Phe-L-Phe-OMe or L-Phe-L-Phe-OEt) due to the following observations: First, L-PheL-Phe-NH2 , the C-terminal modified dipeptide corresponding to the substrates used, only appears in panel A-1. Furthermore, the simple dipeptide L-Phe-L-Phe was observed in a ...
Cyanuric Acid and Cyanurates
... The entropy changes and the heat effect of the HCN polymerization are calculated in [22], while the magnetic anisotropy and the charge delocalization in S-triazine are considered in [23]. The IR spectrum of the polymerized HCN is given in [3] (ν, cm–1): 3450, 3370, 3314, 3260, 3219, 3184 ν(NH2); 222 ...
... The entropy changes and the heat effect of the HCN polymerization are calculated in [22], while the magnetic anisotropy and the charge delocalization in S-triazine are considered in [23]. The IR spectrum of the polymerized HCN is given in [3] (ν, cm–1): 3450, 3370, 3314, 3260, 3219, 3184 ν(NH2); 222 ...
Calculations on the equations reaction
... valences this element can have in compounds? Write the formula of highest oxide of this element. 2. An element has serial number 19 define: а) charge of nucleus atom b) number of electrons c) number of neutrons and protons. Write electronic formula of element. What valences this element can have in ...
... valences this element can have in compounds? Write the formula of highest oxide of this element. 2. An element has serial number 19 define: а) charge of nucleus atom b) number of electrons c) number of neutrons and protons. Write electronic formula of element. What valences this element can have in ...
H/ t = W/m
... same thermometer was used during the experiment). Both the thermometer and thermocouple were placed in the beaker of water. The hot plate was used to slowly raise the temperature as the stirring rod allowed the water to maintain a uniform temperature. The Virtual Bench software was used to read volt ...
... same thermometer was used during the experiment). Both the thermometer and thermocouple were placed in the beaker of water. The hot plate was used to slowly raise the temperature as the stirring rod allowed the water to maintain a uniform temperature. The Virtual Bench software was used to read volt ...
Grossmont College Chemistry 120 Laboratory Manual 6th Edition
... and answer important questions that are intended to give you an understanding of the principles in which the experimental procedure is based as you perform the experiment. Scientists learn much by discussion with one another. You may likewise profit by discussion with your classmates-but not by copy ...
... and answer important questions that are intended to give you an understanding of the principles in which the experimental procedure is based as you perform the experiment. Scientists learn much by discussion with one another. You may likewise profit by discussion with your classmates-but not by copy ...
How does it vary with the charge and distance of the ions?
... b) Find out the ground state term symbols for boron (z=5) c) Give the significance of magnetic Q.N. d) Show that the Plank’s constant and the angular momentum have the same dimension. e) In the ground state H-atom, the total energy of the electron is -13.6ev. Determine its kinetic energy and potenti ...
... b) Find out the ground state term symbols for boron (z=5) c) Give the significance of magnetic Q.N. d) Show that the Plank’s constant and the angular momentum have the same dimension. e) In the ground state H-atom, the total energy of the electron is -13.6ev. Determine its kinetic energy and potenti ...
equilibrium - eVirtualGuru
... Kp and K c; • explain various factors that affect the equilibrium state of a reaction; • classify substances as acids or bases according to Arrhenius, Bronsted-Lowry and Lewis concepts; • classify acids and bases as weak or strong in terms of their ionization constants; • explain the dependence of d ...
... Kp and K c; • explain various factors that affect the equilibrium state of a reaction; • classify substances as acids or bases according to Arrhenius, Bronsted-Lowry and Lewis concepts; • classify acids and bases as weak or strong in terms of their ionization constants; • explain the dependence of d ...
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry
... Example: If a solution containing potassium chloride is added to a solution containing ammonium nitrate, will a precipitate form? KCl(aq) + NH4NO3(aq) → K+(aq) + Cl-(aq) + NH4+(aq) + NO3-(aq) Possible reaction products are KCl and NH4NO3, NH4Cl and KNO3. All are soluble, so there is no precipitate. ...
... Example: If a solution containing potassium chloride is added to a solution containing ammonium nitrate, will a precipitate form? KCl(aq) + NH4NO3(aq) → K+(aq) + Cl-(aq) + NH4+(aq) + NO3-(aq) Possible reaction products are KCl and NH4NO3, NH4Cl and KNO3. All are soluble, so there is no precipitate. ...
to view
... electrons occupy anionic vacancies. These sites are called F centers. These electrons absorb energy from the visible region and transmits yellow colour. (ii) In the crystal of FeO, some of the Fe2+ cations are replaced by Fe3+ ions. Three Fe2+ ions are replaced by two Fe3+ ions to make up for the lo ...
... electrons occupy anionic vacancies. These sites are called F centers. These electrons absorb energy from the visible region and transmits yellow colour. (ii) In the crystal of FeO, some of the Fe2+ cations are replaced by Fe3+ ions. Three Fe2+ ions are replaced by two Fe3+ ions to make up for the lo ...
Organic Chemistry Organic Chemistry
... evaporate easily. In fact, they are often gases at room temperature. (b) Polar substances, with strong forces of attraction among the molecules, require considerable energy to evaporate. ...
... evaporate easily. In fact, they are often gases at room temperature. (b) Polar substances, with strong forces of attraction among the molecules, require considerable energy to evaporate. ...
Chapter 23 + Practice Problems - Bloomsburg Area School District
... same numbers of C, H, O, and N atoms but in a different order. For the tripeptide Val–Asp–His, made up of valine, asparagine, and histidine, there are five isomers. There are 120 possible isomers for a pentapeptide of five different amino acids. Even though there are only 20 types of amino acids in ...
... same numbers of C, H, O, and N atoms but in a different order. For the tripeptide Val–Asp–His, made up of valine, asparagine, and histidine, there are five isomers. There are 120 possible isomers for a pentapeptide of five different amino acids. Even though there are only 20 types of amino acids in ...
STUDY GUIDE
... multiple bonds, and they are more reactive than alkanes. They may participate in addition reactions, including hydrogenation, halogenation, hydrohalogenation, and hydration. A naming scheme has been established by the International Union of Pure and Applied Chemistry (IUPAC) to name the organic comp ...
... multiple bonds, and they are more reactive than alkanes. They may participate in addition reactions, including hydrogenation, halogenation, hydrohalogenation, and hydration. A naming scheme has been established by the International Union of Pure and Applied Chemistry (IUPAC) to name the organic comp ...
Acid
An acid (from the Latin acidus/acēre meaning sour) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (like calcium) to form salts. Aqueous solutions of acids have a pH of less than 7. Non-aqueous acids are usually formed when an anion (negative ion) reacts with one or more positively charged hydrogen cations. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.There are three common definitions for acids: the Arrhenius definition, the Brønsted-Lowry definition, and the Lewis definition. The Arrhenius definition defines acids as substances which increase the concentration of hydrogen ions (H+), or more accurately, hydronium ions (H3O+), when dissolved in water. The Brønsted-Lowry definition is an expansion: an acid is a substance which can act as a proton donor. By this definition, any compound which can easily be deprotonated can be considered an acid. Examples include alcohols and amines which contain O-H or N-H fragments. A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. Examples of Lewis acids include all metal cations, and electron-deficient molecules such as boron trifluoride and aluminium trichloride.Common examples of acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute solution of this liquid), sulfuric acid (used in car batteries), and tartaric acid (a solid used in baking). As these examples show, acids can be solutions or pure substances, and can be derived from solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.