Chemistry of Life - juan-roldan
... in a shell distant from the nucleus have greater energy and are called Valence Electrons Valence electrons occupy the valence shell (outermost shell) Changes in electron energy levels are important in energy conversions in organisms ...
... in a shell distant from the nucleus have greater energy and are called Valence Electrons Valence electrons occupy the valence shell (outermost shell) Changes in electron energy levels are important in energy conversions in organisms ...
Factors that affect the rate of reactions
... liquid, liquid and a gas etc. It does not affect reactants that are in the same phase. To summarize the 3 ways to change the rate of a reaction. If you can make the reactants: MOVE FASTER, HIT each other MORE OFTEN with MORE ENERGY The reaction rate will INCREASE ...
... liquid, liquid and a gas etc. It does not affect reactants that are in the same phase. To summarize the 3 ways to change the rate of a reaction. If you can make the reactants: MOVE FASTER, HIT each other MORE OFTEN with MORE ENERGY The reaction rate will INCREASE ...
Activation energy
... separate atoms that are bonded together. • The same energy is released when chemical bonds form. • Atoms form bonds to reach a lower energy state. ...
... separate atoms that are bonded together. • The same energy is released when chemical bonds form. • Atoms form bonds to reach a lower energy state. ...
Chemical Equations and Reactions
... Formula equation- qualitatively represents the reactants and products of a chemical reaction by their symbols or formulas Notice that the formula equation does not give information about the amounts of reactants and products. A formula equation meets two of the three requirements for a correct c ...
... Formula equation- qualitatively represents the reactants and products of a chemical reaction by their symbols or formulas Notice that the formula equation does not give information about the amounts of reactants and products. A formula equation meets two of the three requirements for a correct c ...
3-A
... make proteins, is represented below. Write the formula for methionine and calculate its molar mass. (red = O; gray = C; blue = N; yellow = S; ivory = H) ...
... make proteins, is represented below. Write the formula for methionine and calculate its molar mass. (red = O; gray = C; blue = N; yellow = S; ivory = H) ...
Chapter 6 Notes - Discount Flies
... 1. Write correct formulas for reactants and products first. Don’t ever change the formula of a substance once it is written correctly. 2. Balance O and H last. ...
... 1. Write correct formulas for reactants and products first. Don’t ever change the formula of a substance once it is written correctly. 2. Balance O and H last. ...
Chapter 4
... Balancing Chemical Equations 1. Write the correct formula(s) for the reactants on the left side and the correct formula(s) for the product(s) on the right side of the equation. Ethane reacts with oxygen to form carbon dioxide and water C2H6 + O2 ...
... Balancing Chemical Equations 1. Write the correct formula(s) for the reactants on the left side and the correct formula(s) for the product(s) on the right side of the equation. Ethane reacts with oxygen to form carbon dioxide and water C2H6 + O2 ...
Fall Exam 4 - Chemistry - University of Kentucky
... Questions 1 thru 15 cover the material after Exam III. ...
... Questions 1 thru 15 cover the material after Exam III. ...
Heats of Formation WS
... 7. The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g) 2 NO (g) + O2 (g) 2 NO2 (g) 3 NO2 (g) + H2O (l) 2 HNO3 (aq) + NO (g) [a] Use the values of ∆Hfº to calculate the value of ∆Hº for ...
... 7. The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g) 2 NO (g) + O2 (g) 2 NO2 (g) 3 NO2 (g) + H2O (l) 2 HNO3 (aq) + NO (g) [a] Use the values of ∆Hfº to calculate the value of ∆Hº for ...
Chem 1A Final Exam – Fall 2005
... What is ionization energy? Describe and explain the general trend in the periodic table for the IE. ...
... What is ionization energy? Describe and explain the general trend in the periodic table for the IE. ...
2nd nine weeks benchmark review homework
... to the number of ___ in the nucleus. a- atomic number, neutrons b- atomic number, protons c- atomic mass, neutrons d- atomic mass, protons When the physical composition of a substance changes, the chemical composition- ...
... to the number of ___ in the nucleus. a- atomic number, neutrons b- atomic number, protons c- atomic mass, neutrons d- atomic mass, protons When the physical composition of a substance changes, the chemical composition- ...
THERMOCHEMISTRY ENERGETICS/ENTHALPY
... Chemists generally refer to the energy given out when a fuel burns in kJmol-1 because this compares the same number of molecules of each fuel. For use as fuels it is sometimes better to convert the units from kJmol-1 to kJg-1 (OR the energy density) of a fuel ...
... Chemists generally refer to the energy given out when a fuel burns in kJmol-1 because this compares the same number of molecules of each fuel. For use as fuels it is sometimes better to convert the units from kJmol-1 to kJg-1 (OR the energy density) of a fuel ...
Lecture 2 - Columbia University
... Element: An element is a substance which cannot be decomposed into simpler substances by chemical processes. Exemplars: hydrogen, carbon, oxygen. Atomic interpretation: An element is a substance that contains only one kind of atom. Exemplars: Hydrogen (H) atoms, carbon atoms (C), oxygen atoms (O). ...
... Element: An element is a substance which cannot be decomposed into simpler substances by chemical processes. Exemplars: hydrogen, carbon, oxygen. Atomic interpretation: An element is a substance that contains only one kind of atom. Exemplars: Hydrogen (H) atoms, carbon atoms (C), oxygen atoms (O). ...
acids and bases - No Brain Too Small
... o NH4+ ammonium OH- hydroxide HCO3- hydrogen carbonate NO3- nitrate SO42- sulfate CO32- carbonate E.g. Cu2+ & OH- makes the formula Cu(OH)2 but Cu2+ & CO32- is just CuCO3 E.g.iron (III) hydroxide is Fe(OH)3 ...
... o NH4+ ammonium OH- hydroxide HCO3- hydrogen carbonate NO3- nitrate SO42- sulfate CO32- carbonate E.g. Cu2+ & OH- makes the formula Cu(OH)2 but Cu2+ & CO32- is just CuCO3 E.g.iron (III) hydroxide is Fe(OH)3 ...
Kinetics - A Study o..
... Three conditions must be met at the nanoscale level if a reaction is to occur: • the molecules must collide; • they must be positioned so that the reacting groups are together in a transition state between reactants and products; • and the collision must have enough energy to form the transition sta ...
... Three conditions must be met at the nanoscale level if a reaction is to occur: • the molecules must collide; • they must be positioned so that the reacting groups are together in a transition state between reactants and products; • and the collision must have enough energy to form the transition sta ...
2002 Final Exam for Practice - Department of Chemistry | Oregon
... Sketch a 1s orbital and a 4p orbital side by side, with correct relative scale. ...
... Sketch a 1s orbital and a 4p orbital side by side, with correct relative scale. ...
Standards Practice
... times the number of atoms as one mole of carbon. 14. How many particles are present in 1 mol of the isotope carbon-13 (atomic number = 6; atomic mass = 13)'1 A. 3.01 x 1023 molecules B. 6 x 1013 molecules C. 6.02 x 1023 molecules D. 1.3 x 1024 molecules . 15. How many molecules does I mole of NaOH h ...
... times the number of atoms as one mole of carbon. 14. How many particles are present in 1 mol of the isotope carbon-13 (atomic number = 6; atomic mass = 13)'1 A. 3.01 x 1023 molecules B. 6 x 1013 molecules C. 6.02 x 1023 molecules D. 1.3 x 1024 molecules . 15. How many molecules does I mole of NaOH h ...
Chemical Calculations, Chemical Equations
... don’t have to know it . Names of ionic compounds containing these elements must contain reference as to which ion is involved. This is done by including a roman numeral in the name, showing the charge of the involved ion. So, in order to generate name, you first have to figure out what the charge i ...
... don’t have to know it . Names of ionic compounds containing these elements must contain reference as to which ion is involved. This is done by including a roman numeral in the name, showing the charge of the involved ion. So, in order to generate name, you first have to figure out what the charge i ...
Chemistry Standard Outline
... SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions. SC2c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate • Empirical/molecular formulas, • Mass, moles and molecules relationship ...
... SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions. SC2c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate • Empirical/molecular formulas, • Mass, moles and molecules relationship ...
Chemical Equations and Stoichiometry
... Because of propane’s simple chemical structure, it usually burns cleanly. Unlike gasoline, in a wellventilated area, it will not produce much soot or carbon monoxide. It does however produce the greenhouse gas carbon dioxide, which has been accumulating in the atmosphere since the Industrial Revolut ...
... Because of propane’s simple chemical structure, it usually burns cleanly. Unlike gasoline, in a wellventilated area, it will not produce much soot or carbon monoxide. It does however produce the greenhouse gas carbon dioxide, which has been accumulating in the atmosphere since the Industrial Revolut ...
STOICHIOMETRY REVIEW WORKSHEET
... (a) How many moles of water formed? (b) How many moles of butane burned? (c) How many grams of butane burned? (d) How much oxygen was used up in moles? (e) How much oxygen was used up in grams? 2) Using the following equation: NaOH + ...
... (a) How many moles of water formed? (b) How many moles of butane burned? (c) How many grams of butane burned? (d) How much oxygen was used up in moles? (e) How much oxygen was used up in grams? 2) Using the following equation: NaOH + ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.