CH4 Student Revision Guides pdf | GCE AS/A
... Like alkanes the structure is examined for the longest straight-chain carbon chain. The name is based on the hydrocarbon with the same number of C-atoms as the longest continuous carbon chain that contains the double bond. The lowest number is used to show the position of the double bond. The ending ...
... Like alkanes the structure is examined for the longest straight-chain carbon chain. The name is based on the hydrocarbon with the same number of C-atoms as the longest continuous carbon chain that contains the double bond. The lowest number is used to show the position of the double bond. The ending ...
1 - Cathedral High School
... 3.2.1 Describe and explain the periodic trends in atomic radii, ionic radii, ionization energies, electronegativity and melting points for the alkali metals (Li Cs), halogens (F I) and period 3 elements (Na Ar). Cross reference with topics 2, 4 and 5. Data for all these properties are listed i ...
... 3.2.1 Describe and explain the periodic trends in atomic radii, ionic radii, ionization energies, electronegativity and melting points for the alkali metals (Li Cs), halogens (F I) and period 3 elements (Na Ar). Cross reference with topics 2, 4 and 5. Data for all these properties are listed i ...
KS4-Chemical-Reactions
... Getting more product at equilibrium. • There are some simple rules that can be used to move the position of an equilibrium towards reactants or products: 1. Exothermic reactions give more product at lower temperatures. (Endothermic – the opposite) 2. Increasing the pressure in gas reactions favours ...
... Getting more product at equilibrium. • There are some simple rules that can be used to move the position of an equilibrium towards reactants or products: 1. Exothermic reactions give more product at lower temperatures. (Endothermic – the opposite) 2. Increasing the pressure in gas reactions favours ...
15.0 EquilibriumIHS2014
... • At A, the concentration (or pressure) of every chemical in the system is decreased by increasing the container volume. Then the equilibrium shifts to the left (the side with more moles of gas) • At B, the temperature is increased. Then the equilibrium shifts to left. • At C, C2H6(g) is added to th ...
... • At A, the concentration (or pressure) of every chemical in the system is decreased by increasing the container volume. Then the equilibrium shifts to the left (the side with more moles of gas) • At B, the temperature is increased. Then the equilibrium shifts to left. • At C, C2H6(g) is added to th ...
Descriptive Chemistry of Elements p
... BCl3 and BBr3 can be prepared by direct combination of the two elements. BI3 is made by heating BCl3 with HI. We know that boron halides are electron deficient molecules and boron needs two more electrons to achieve the octet. Thus, these molecules can act as electron acceptors or Lewis acids. For e ...
... BCl3 and BBr3 can be prepared by direct combination of the two elements. BI3 is made by heating BCl3 with HI. We know that boron halides are electron deficient molecules and boron needs two more electrons to achieve the octet. Thus, these molecules can act as electron acceptors or Lewis acids. For e ...
Unit 3 Physical Science: Chemical Reactions
... Teachers could use molecular models to demonstrate correct naming and writing of molecular formulas for a variety of molecular compounds such as methane, water, hydrogen peroxide, ozone, sucrose, ethanol, and methanol. It is important to cover not only common names such as methane (CH4 ) but also th ...
... Teachers could use molecular models to demonstrate correct naming and writing of molecular formulas for a variety of molecular compounds such as methane, water, hydrogen peroxide, ozone, sucrose, ethanol, and methanol. It is important to cover not only common names such as methane (CH4 ) but also th ...
Spring 2014
... 13. The equilibrium constant is equal to 5.00 at 1300 K for the reaction 2 SO2 (g) + O2 (g) W 2 SO3 (g). If initial concentrations are [SO2] = 4.0 M, [O2] = 4.0 M, and [SO3] = 4.0 M, the system is a) not at equilibrium and will shift to the right (products) to achieve an equilibrium state. b) not at ...
... 13. The equilibrium constant is equal to 5.00 at 1300 K for the reaction 2 SO2 (g) + O2 (g) W 2 SO3 (g). If initial concentrations are [SO2] = 4.0 M, [O2] = 4.0 M, and [SO3] = 4.0 M, the system is a) not at equilibrium and will shift to the right (products) to achieve an equilibrium state. b) not at ...
Chapter 16 Aqueous Ionic Equilibrium Lecture Presentation
... • It is a plot of pH versus the amount of added titrant. • The inflection point of the curve is the equivalence point of the titration. • Prior to the equivalence point, the known solution in the flask is in excess, so the pH is closest to its pH. • The pH of the equivalence point depends on the pH ...
... • It is a plot of pH versus the amount of added titrant. • The inflection point of the curve is the equivalence point of the titration. • Prior to the equivalence point, the known solution in the flask is in excess, so the pH is closest to its pH. • The pH of the equivalence point depends on the pH ...
SAT - mvhs-fuhsd.org
... you how many covalent bonds that atom can form with other nonmetals or how many electrons it wants to gain from metals to form an ion. • The number of valence electrons in a metal tells you how many electrons the metal will lose to nonmetals to form an ion. Caution: May not work with transition meta ...
... you how many covalent bonds that atom can form with other nonmetals or how many electrons it wants to gain from metals to form an ion. • The number of valence electrons in a metal tells you how many electrons the metal will lose to nonmetals to form an ion. Caution: May not work with transition meta ...
IGCSE SoW 2013
... Understand ionic bonding as a strong electrostatic attraction between oppositely charged ions ...
... Understand ionic bonding as a strong electrostatic attraction between oppositely charged ions ...
C3 Revision Question Booklet
... What is meant by a weak acid in terms of its ionisation in water? ...
... What is meant by a weak acid in terms of its ionisation in water? ...
AP 2005 Chemistry Free-Response Questions
... INFORMATION IN THE TABLE BELOW AND IN THE TABLES ON PAGES 3-5 MAY BE USEFUL IN ANSWERING ...
... INFORMATION IN THE TABLE BELOW AND IN THE TABLES ON PAGES 3-5 MAY BE USEFUL IN ANSWERING ...
Class: 11 Subject: Chemistry Topic: Equilibrium No. of
... KP = KC (RT)∆n , KP < KC if Δ n is negative. It is the case for the example given in option 2 9. The thermal effects of a reaction depend on? ...
... KP = KC (RT)∆n , KP < KC if Δ n is negative. It is the case for the example given in option 2 9. The thermal effects of a reaction depend on? ...
Addition of ketene to ethylene oxide
... intermediate in the preparation of surface active agents • . This involves a reaction with long chain carboxylic acids to produce a molecule containing both hydrophobic and hydrophilic characteristics. Ethylene oxide undergoes attack by substances containing active hydrogen and also by some substanc ...
... intermediate in the preparation of surface active agents • . This involves a reaction with long chain carboxylic acids to produce a molecule containing both hydrophobic and hydrophilic characteristics. Ethylene oxide undergoes attack by substances containing active hydrogen and also by some substanc ...
Please do not remove this page. The periodic table, constants, and
... b. For 1.0 M solutions of any 2 weak bases, the solution of the base with the larger Kb will have the greater [OH–]. c. A Lewis acid is an electron pair acceptor. d. For a polyprotic acid, Ka1 is always greater than Ka2. e. The pH of a neutral solution is 7.00 at all temperatures. ...
... b. For 1.0 M solutions of any 2 weak bases, the solution of the base with the larger Kb will have the greater [OH–]. c. A Lewis acid is an electron pair acceptor. d. For a polyprotic acid, Ka1 is always greater than Ka2. e. The pH of a neutral solution is 7.00 at all temperatures. ...
Chem 12 Prov Exam PLO Review
... recognize some of the factors that control reaction rates compare and contrast factors affecting the rates of both homogeneous and heterogeneous reactions discuss situations in which the rate of reaction must be controlled ...
... recognize some of the factors that control reaction rates compare and contrast factors affecting the rates of both homogeneous and heterogeneous reactions discuss situations in which the rate of reaction must be controlled ...
Year 9 Chemical Sciences Program Term 3 Course 2 2017
... All matter is made of atoms that are composed of protons, neutrons and electrons; natural radioactivity arises from the decay of nuclei in atoms. (ACSSU177) describing and modelling the structure of atoms in terms of the nucleus, protons, neutrons and electrons comparing the mass and charge of p ...
... All matter is made of atoms that are composed of protons, neutrons and electrons; natural radioactivity arises from the decay of nuclei in atoms. (ACSSU177) describing and modelling the structure of atoms in terms of the nucleus, protons, neutrons and electrons comparing the mass and charge of p ...
Powerpoints - Holy Cross Collegiate
... reactant reacts to make product on the ratio described by the balanced equation. • The quantity of product actually obtained by a reaction is called the experimental yield (which is also known as the actual yield). • In most reactions, the experimental yield will not match exactly with the predicted ...
... reactant reacts to make product on the ratio described by the balanced equation. • The quantity of product actually obtained by a reaction is called the experimental yield (which is also known as the actual yield). • In most reactions, the experimental yield will not match exactly with the predicted ...
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.