IONIC EQULIBRIUM
... dissociation of a weak electrolyte. The "common" ion shifts the dissociation equilibrium in accordance with LeChatelier's principle. Central metal atom. A cation which accepts electrons from a ligand to form a complex ion. Conjugate acid-base pair. An acid-base pair which differ only by a proton, as ...
... dissociation of a weak electrolyte. The "common" ion shifts the dissociation equilibrium in accordance with LeChatelier's principle. Central metal atom. A cation which accepts electrons from a ligand to form a complex ion. Conjugate acid-base pair. An acid-base pair which differ only by a proton, as ...
Bellin College Homework Supplement
... 1. How can the study of chemistry help you in your desired profession? Limit answer to 1-2 paragraphs. Write clearly and legibly. There is no right or wrong answer. You are simply stating your opinion. ...
... 1. How can the study of chemistry help you in your desired profession? Limit answer to 1-2 paragraphs. Write clearly and legibly. There is no right or wrong answer. You are simply stating your opinion. ...
NH 4 1+
... A strong acid is one that dissociates 100% in water. That is, 100% of the molecules in solution are broken up into its ions. For example, HNO3 breaks apart 100% into its ions: H+ and NO3-. Of all the acids that exist, only six are strong: HCl, HBr, HI, HNO3, HClO4, H2SO4. A weak acid is one that onl ...
... A strong acid is one that dissociates 100% in water. That is, 100% of the molecules in solution are broken up into its ions. For example, HNO3 breaks apart 100% into its ions: H+ and NO3-. Of all the acids that exist, only six are strong: HCl, HBr, HI, HNO3, HClO4, H2SO4. A weak acid is one that onl ...
Aldehydes, Ketones and Carboxylic Acids
... most important functional groups in organic chemistry. In aldehydes, the carbonyl group is bonded to a carbon and hydrogen while in the ketones, it is bonded to two carbon atoms. The carbonyl compounds in which carbonyl group is bonded to oxygen are known as carboxylic acids, and their derivatives ( ...
... most important functional groups in organic chemistry. In aldehydes, the carbonyl group is bonded to a carbon and hydrogen while in the ketones, it is bonded to two carbon atoms. The carbonyl compounds in which carbonyl group is bonded to oxygen are known as carboxylic acids, and their derivatives ( ...
File
... Acid-Base Reactions -historical recognition Acid – sour taste, turns litmus dye red Base – bitter taste, soapy feeling, turns litmus blue (poor procedures) Acids/Bases in aqueous solutionsAn acid molecule reacts with water to produce a hydronium ion HCl(g) + H2O(l) H3O+(aq) + Cl(aq) -does HCl (aq ...
... Acid-Base Reactions -historical recognition Acid – sour taste, turns litmus dye red Base – bitter taste, soapy feeling, turns litmus blue (poor procedures) Acids/Bases in aqueous solutionsAn acid molecule reacts with water to produce a hydronium ion HCl(g) + H2O(l) H3O+(aq) + Cl(aq) -does HCl (aq ...
Topic 1: Quantitative chemistry (12
... Be able to identify the ultraviolet, visible and infrared regions, and to describe the variation in wavelength, frequency and energy across the spectrum. TOK: Infrared and ultraviolet spectroscopy are dependent on technology for their existence. What are the knowledge implications of this? Distingui ...
... Be able to identify the ultraviolet, visible and infrared regions, and to describe the variation in wavelength, frequency and energy across the spectrum. TOK: Infrared and ultraviolet spectroscopy are dependent on technology for their existence. What are the knowledge implications of this? Distingui ...
Chapter 30 - The Chemical Basis of Animal Life
... an electrical charge (because of an electron loss or gain) and attracts an atom or group of atoms with an opposite charge. Figure 30.6 shows how an ionic bond forms between sodium and chlorine to produce sodium chloride. When a sodium atom and chlorine atom come together, the sodium atom donates an ...
... an electrical charge (because of an electron loss or gain) and attracts an atom or group of atoms with an opposite charge. Figure 30.6 shows how an ionic bond forms between sodium and chlorine to produce sodium chloride. When a sodium atom and chlorine atom come together, the sodium atom donates an ...
Chemistry II Exams and Keys 2013 Season
... 10. A sample containing 7.45 grams of KCl is dissolved in sufficient distilled water and reacted with 1000.0 mL 0.300 M AgNO3 solution. Excess silver nitrate solution reacted with the metallic copper according to the following reaction: Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s) The precipitate is f ...
... 10. A sample containing 7.45 grams of KCl is dissolved in sufficient distilled water and reacted with 1000.0 mL 0.300 M AgNO3 solution. Excess silver nitrate solution reacted with the metallic copper according to the following reaction: Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s) The precipitate is f ...
Chemistry Unit Summaries - Oak Park Unified School District
... electrons in a covalent bond. Electronegativity generally increases from left to right in the periodic table and decreases down a column. The difference in atoms' electronegativities is used to determine the polarity of a covalent bond; the greater the difference, the more polar the bond. A polar mo ...
... electrons in a covalent bond. Electronegativity generally increases from left to right in the periodic table and decreases down a column. The difference in atoms' electronegativities is used to determine the polarity of a covalent bond; the greater the difference, the more polar the bond. A polar mo ...
Review
... including: freezing pt. depression, boiling point elevation, vapor pressure lowering, osmotic pressure Use of the definition of the Chemical Potentials, at equil the chemical potentials of a species in all phases must be equal to each other Processes move from a higher chemical potential to a lower ...
... including: freezing pt. depression, boiling point elevation, vapor pressure lowering, osmotic pressure Use of the definition of the Chemical Potentials, at equil the chemical potentials of a species in all phases must be equal to each other Processes move from a higher chemical potential to a lower ...
Chapter 4 - profpaz.com
... This relationship is valid because the product of molarity times volume on each side equals the moles of solute, which remains constant during dilution. Molarity and volume, however, are inversely proportional during the dilution process. ...
... This relationship is valid because the product of molarity times volume on each side equals the moles of solute, which remains constant during dilution. Molarity and volume, however, are inversely proportional during the dilution process. ...
Chemistry 1 Lectures
... • Element closest to bottom of group is 1st • Last element ends in ide (for inorganics) • If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom ...
... • Element closest to bottom of group is 1st • Last element ends in ide (for inorganics) • If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom ...
Complete the following equations
... The reaction between nitrogen and chlorine gas produces nitrogen trichloride, NCl3, as the sole product. However, reactions between phosphorus, Arsenic, and antimony with chlorine gas will produce both trichloride, MCl3, and pentachloride compounds (MCl5). Explain why nitrogen (a member of Group 5A ...
... The reaction between nitrogen and chlorine gas produces nitrogen trichloride, NCl3, as the sole product. However, reactions between phosphorus, Arsenic, and antimony with chlorine gas will produce both trichloride, MCl3, and pentachloride compounds (MCl5). Explain why nitrogen (a member of Group 5A ...
3.98 MB - KFUPM Resources v3
... Water is a bent molecule (not linear). O-H bonds are covalent (O and H atoms share electrons). Because the oxygen atom has a greater attraction for electrons, shared electrons tend to spend more time closer to the oxygen atom than to either of the hydrogen atoms. In H2O, oxygen is partially negative ...
... Water is a bent molecule (not linear). O-H bonds are covalent (O and H atoms share electrons). Because the oxygen atom has a greater attraction for electrons, shared electrons tend to spend more time closer to the oxygen atom than to either of the hydrogen atoms. In H2O, oxygen is partially negative ...
program
... • detecting the presence of oxygen, hydrogen, water, carbon dioxide, sulfur dioxide. Acids and bases The candidate can sb17 recognise the following substances/solutions as an acid/acidic solution: • hydrogen chloride/hydrochloric acid; • sulfuric acid/sulfuric acid solution; • nitric acid/nitric aci ...
... • detecting the presence of oxygen, hydrogen, water, carbon dioxide, sulfur dioxide. Acids and bases The candidate can sb17 recognise the following substances/solutions as an acid/acidic solution: • hydrogen chloride/hydrochloric acid; • sulfuric acid/sulfuric acid solution; • nitric acid/nitric aci ...
Spring Exam 4 - Chemistry
... 16. Consider the reaction 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) Suppose that at a particular moment during the reaction, molecular oxygen is reacting at a rate of 0.450 M/s. At what rate is water forming? ...
... 16. Consider the reaction 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) Suppose that at a particular moment during the reaction, molecular oxygen is reacting at a rate of 0.450 M/s. At what rate is water forming? ...
Answers - Scioly.org
... 20. The student concludes that she has synthesized ethyl butanoate. Use evidence from the two experiments to support or to refute her claim. The peak of highest mass to charge ratio is approximately 116; therefore, the unknown molecule would have a molecular mass of 116. Ethyl butanoate has the chem ...
... 20. The student concludes that she has synthesized ethyl butanoate. Use evidence from the two experiments to support or to refute her claim. The peak of highest mass to charge ratio is approximately 116; therefore, the unknown molecule would have a molecular mass of 116. Ethyl butanoate has the chem ...
SPRING 2002 Test 2 1. Which of the following statements is
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
Chemistry Unit 1
... is also important to realize that hydroxides which react with both acids and bases are described as amphoteric substances. For example, aluminium hydroxide, Al(OH)3, reacts with both acids and bases to form salt and water. So, Al(OH)3, is amphoteric in nature. What is the common characteristic of ac ...
... is also important to realize that hydroxides which react with both acids and bases are described as amphoteric substances. For example, aluminium hydroxide, Al(OH)3, reacts with both acids and bases to form salt and water. So, Al(OH)3, is amphoteric in nature. What is the common characteristic of ac ...
CLASS X carbon and its compound
... Homopolar bond : A chemical bond formed between two non-metallic elements by the mutual sharing of one or more electron pairs is called covalent bond. 2. Covalency : The number of electron pairs which an atom of an element mutually shares with another atom or atoms of the same or different elements, ...
... Homopolar bond : A chemical bond formed between two non-metallic elements by the mutual sharing of one or more electron pairs is called covalent bond. 2. Covalency : The number of electron pairs which an atom of an element mutually shares with another atom or atoms of the same or different elements, ...
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.