Exam #2
... mass of the nucleus is concentrated in a very small volume. The electron diffraction experiment demonstrated Heisenberg’s hypothesis that matter and energy are interconvertable. The solution to the Schrodinger wave equation for the hydrogen atom does not provide a detailed description of the electro ...
... mass of the nucleus is concentrated in a very small volume. The electron diffraction experiment demonstrated Heisenberg’s hypothesis that matter and energy are interconvertable. The solution to the Schrodinger wave equation for the hydrogen atom does not provide a detailed description of the electro ...
CHEM 30
... - use activation energy diagrams and kinetic energy diagrams to show effect of temperature and catalysts on reaction rate - explain reaction rates in terms of the collision theory - effect of changes in temperature, concentrations, nature of the reactants, etc. - identify reaction mechanisms: cataly ...
... - use activation energy diagrams and kinetic energy diagrams to show effect of temperature and catalysts on reaction rate - explain reaction rates in terms of the collision theory - effect of changes in temperature, concentrations, nature of the reactants, etc. - identify reaction mechanisms: cataly ...
CHAPTER 9 HYDROGEN Position of Hydrogen in Periodic Table
... hydrides of group 15 to 17 (NH3, PH3, H2O, H2S, H2Se, H2Te, HF etc.) (iii) Metallic or non-stoichiometric hydrides: These are formed by many d-block and f-block elements These hydrides conducts heat and electricity though not efficient. Water: -Water! It is the major part of all living organisms ...
... hydrides of group 15 to 17 (NH3, PH3, H2O, H2S, H2Se, H2Te, HF etc.) (iii) Metallic or non-stoichiometric hydrides: These are formed by many d-block and f-block elements These hydrides conducts heat and electricity though not efficient. Water: -Water! It is the major part of all living organisms ...
Chemical Reactions
... 1. Aluminum reacts with oxygen to produce aluminum oxide. 2. Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. ...
... 1. Aluminum reacts with oxygen to produce aluminum oxide. 2. Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. ...
SOLUBILITY RULES FOR IONIC COMPOUNDS IN WATER
... *5. A sample may contain any or all of the following ions: Ag+, Ba2+ and Fe2+. A precipitate formed when an aqueous solution of KCl was added. The precipitate was filtered off and an aqueous solution of K2SO4 was added to the remaining solution, but no precipitate was formed. When an aqueous solutio ...
... *5. A sample may contain any or all of the following ions: Ag+, Ba2+ and Fe2+. A precipitate formed when an aqueous solution of KCl was added. The precipitate was filtered off and an aqueous solution of K2SO4 was added to the remaining solution, but no precipitate was formed. When an aqueous solutio ...
X012/12/02
... of potassium iodide solution. Pour these into a dry 100 cm3 glass beaker and place the beaker on the bench. 2. Measure out 5 cm3 of hydrogen peroxide solution and start the timer. 3. Add the hydrogen peroxide solution to the beaker. When the blue/black colour just appears, stop the timer and rec ...
... of potassium iodide solution. Pour these into a dry 100 cm3 glass beaker and place the beaker on the bench. 2. Measure out 5 cm3 of hydrogen peroxide solution and start the timer. 3. Add the hydrogen peroxide solution to the beaker. When the blue/black colour just appears, stop the timer and rec ...
PowerPoint Overview for Introduction
... o If a pure substance cannot be decomposed (at the macroscopic level ) into something else, then the substance is an element. o There are 118 Elements Known o Each element is given a unique chemical symbol (one or two letters). o Elements are Building Blocks of Matter. o Chemical symbols with one le ...
... o If a pure substance cannot be decomposed (at the macroscopic level ) into something else, then the substance is an element. o There are 118 Elements Known o Each element is given a unique chemical symbol (one or two letters). o Elements are Building Blocks of Matter. o Chemical symbols with one le ...
Chapter 12
... Atoms can lose or gains more than one electron. Examples: Mg2+, Fe3+, S2-, and N3A monatomic ion contains only one atom. Mg2+, Fe3+, S2-, Al3+. A polyatomic ion contains more than one atom. OH-, CN-, NH4+. Chemical Formulas are used to express the composition of molecules and ionic compounds in term ...
... Atoms can lose or gains more than one electron. Examples: Mg2+, Fe3+, S2-, and N3A monatomic ion contains only one atom. Mg2+, Fe3+, S2-, Al3+. A polyatomic ion contains more than one atom. OH-, CN-, NH4+. Chemical Formulas are used to express the composition of molecules and ionic compounds in term ...
Specific Reactions Quiz.wpd
... d) the presence of random carbon products prevents balancing e) energy is lost because it remains trapped within any remnant fuel bonds ...
... d) the presence of random carbon products prevents balancing e) energy is lost because it remains trapped within any remnant fuel bonds ...
Redox Flash Cards - No Brain Too Small
... compounds are split into their atoms using electric currents electrolysis ...
... compounds are split into their atoms using electric currents electrolysis ...
Untitled
... Even after _______ turns are all the green gone? Instead of all the green being converted to red and blue a “stale-mate” condition called __________________ is produced, where both reactants and products are present. Important Properties of a reaction at equilibrium 1. The reaction __________ stop. ...
... Even after _______ turns are all the green gone? Instead of all the green being converted to red and blue a “stale-mate” condition called __________________ is produced, where both reactants and products are present. Important Properties of a reaction at equilibrium 1. The reaction __________ stop. ...
Chemistry Standards Review
... 86. What is the strong nuclear force? 87. What is the equation that allows us to calculate the energy released in nuclear reactions? 88. What are the three most common forms of radioactive decay? Describe each type of decay. 89. How does the nucleus change with each type of decay? 90. Complete and b ...
... 86. What is the strong nuclear force? 87. What is the equation that allows us to calculate the energy released in nuclear reactions? 88. What are the three most common forms of radioactive decay? Describe each type of decay. 89. How does the nucleus change with each type of decay? 90. Complete and b ...
Atoms, Molecules and Ions
... forms both Fe+ and Fe2+ ions, we need to use the Stock system and call the compound iron(II) nitrate. (b) The cation is Na+ and the anion is HPO42− (hydrogen phosphate). Because sodium only forms one type of ion (Na+), there is no need to use sodium(I) in the name. The compound is sodium hydrogen ph ...
... forms both Fe+ and Fe2+ ions, we need to use the Stock system and call the compound iron(II) nitrate. (b) The cation is Na+ and the anion is HPO42− (hydrogen phosphate). Because sodium only forms one type of ion (Na+), there is no need to use sodium(I) in the name. The compound is sodium hydrogen ph ...
Assignment 3
... equilibrates with respect to gas-liquid exchange? Assume that redox reactions are kinetically inhibited. ...
... equilibrates with respect to gas-liquid exchange? Assume that redox reactions are kinetically inhibited. ...
CHEMICAL REACTIONS
... 3. reactions with acids : a. carbonates or bicarbonates and acids form a salt, water and CO2 • e.g. 2HCl + Na2CO3 Æ 2 NaCl + H2O + CO2 (net : H+ + CO32- Æ H2O + CO2) b. sulfites and acids form a salt, water and SO2 • e.g. 2 HCl + Na2SO3 Æ 2 NaCl + H2O + SO2 (net : H+ + SO32- Æ H2O + SO2) c. metallic ...
... 3. reactions with acids : a. carbonates or bicarbonates and acids form a salt, water and CO2 • e.g. 2HCl + Na2CO3 Æ 2 NaCl + H2O + CO2 (net : H+ + CO32- Æ H2O + CO2) b. sulfites and acids form a salt, water and SO2 • e.g. 2 HCl + Na2SO3 Æ 2 NaCl + H2O + SO2 (net : H+ + SO32- Æ H2O + SO2) c. metallic ...
Naming Binary Inorganic Compounds
... Compounds formed with polyatomic ions must have _________________________, just like those formed from monatomic ions This means that in many compounds there will be more than one unit of a given polyatomic ion This is reflected in the formulas of these compounds by the use of ______________. The su ...
... Compounds formed with polyatomic ions must have _________________________, just like those formed from monatomic ions This means that in many compounds there will be more than one unit of a given polyatomic ion This is reflected in the formulas of these compounds by the use of ______________. The su ...
Homework,1 Atoms, molecules, and ions
... 16.77 kJ/°C. The temperature of the calorimeter increases from 22.62°C to 26.87°C. What is the heat of combustion per mole of C2H4O? a) −61.2 kJ/mol b) −1.10 x 103 kJ/mol c) −3.93 kJ/mol d) −3.14 x 103 kJ/mol e) −8.90 x 103 kJ/mol f) −260. kJ/mol 3- The specific heat of lead is 0.13 J/g-K. How many ...
... 16.77 kJ/°C. The temperature of the calorimeter increases from 22.62°C to 26.87°C. What is the heat of combustion per mole of C2H4O? a) −61.2 kJ/mol b) −1.10 x 103 kJ/mol c) −3.93 kJ/mol d) −3.14 x 103 kJ/mol e) −8.90 x 103 kJ/mol f) −260. kJ/mol 3- The specific heat of lead is 0.13 J/g-K. How many ...
PH
In chemistry, pH (/piːˈeɪtʃ/) is a numeric scale used to specify the acidity or alkalinity of an aqueous solution. It is the negative of the logarithm to base 10 of the activity of the hydrogen ion. Solutions with a pH less than 7 are acidic and solutions with a pH greater than 7 are alkaline or basic. Pure water is neutral, being neither an acid nor a base. Contrary to popular belief, the pH value can be less than 0 or greater than 14 for very strong acids and bases respectively.pH measurements are important in medicine, biology, chemistry, agriculture, forestry, food science, environmental science, oceanography, civil engineering, chemical engineering, nutrition, water treatment & water purification, and many other applications. The pH scale is traceable to a set of standard solutions whose pH is established by international agreement.Primary pH standard values are determined using a concentration cell with transference, by measuring the potential difference between a hydrogen electrode and a standard electrode such as the silver chloride electrode.The pH of aqueous solutions can be measured with a glass electrode and a pH meter, or indicator.pH is the negative of the logarithm to base 10 of the activity of the (solvated) hydronium ion, more often (albeit somewhat inaccurately) expressed as the measure of the hydronium ion concentration.The rest of this article uses the technically correct word ""base"" and its inflections in place of ""alkaline"", which specifically refers to a base dissolved in water, and its inflections.