CHEMISTRY COMMUNITY

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If we were given a graph to determine the order of a reaction and the Y axis has the units ln(A) and the X axis has the units time but the slope is positive linear what does this tell us about the reaction? In other words if the slope does not match the normal graph for a first order reaction what c...

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Why is combustion a spontaneous process? Wouldn't you have to put in energy (like a flame) for the combustion reaction to occur?

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Why do reactions slow as time goes on? Would a reaction still slow if we had excess reactants?

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Can someone explain what a propagation step is in a chain reaction?

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I read an example online that helped me understand the rate determining step: The rate determining step is like a funnel in which only so much substance can pass at a time. The reaction rate is limited by the width of the "funnel", not by the amount of substance being added to the funnel. ...

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I am not entirely sure if we need to know the steady state approach for the final but it wouldn't hurt to remember for the steady state approximation that the assumption is made that the concentrations of the intermediates remain low and do not change significantly in the course of the reaction. Thu...

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How do you classify elementary reaction steps based on molecularity?

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What does it mean to turn a second order reaction into a pseudo-first-order reaction?

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It is important to know the order of a reaction to predict how a reaction will change over time. For example, if you know a reaction is first order then doubling the concentration of reactants will double the reaction rate.

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Would we ever have to take corrosion into account when dealing with an oxidation half reaction?

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Can you tell if a reaction is spontaneous based on the value of the standard cell potential?

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In a galvanic cell what exactly is a salt bridge made of and how does the salt bridge function?

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Specific heat capacity and molar heat capacity are both intensive because both equations take into account the amount of substance (in either grams or moles). Therefore it does not matter how much of the substance you have, the ability to absorb heat is still the same.

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If a system has adiabatic walls can we assume q=0 and delta U=w?

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Why is it that when delta H is given in a thermodynamics question that this implies constant pressure?

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How can we apply information about thermal disorder in the problems we do in the homework or midterm?

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Can someone further explain Trouton's rule and how it relates to vaporization?

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How does work change depending if the work is done on the system or the surroundings?

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If the bond enthalpy is not given how would we calculate the reaction enthalpy?

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Why is it that an element in its lost stable form has ethalpy of formation equal to zero?

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Why must our gas or solution be put into standard state? (1 atm or 1M)

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In terms of thermodynamics a reversible reaction has no change in entropy, so no extra energy is needed to reverse the reaction. Irreversible reactions on the other hand cause an entropy increase to reverse the reaction.

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Another way to relate heat and work is with the equation U= q + w. U is the change in internal energy, q is heat, and w is work.

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I read in the textbook about adiabatic and diathermic walls, how would we use this information in our calculations?

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Why does adding an inert gas to a reaction have no effect on equilibrium composition?

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Is equilibrium affected by addition/removal of a pure solid or pure liquid?

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Why does increasing the temperature of an endothermic reaction shift the reaction towards products and why does increasing the temperature of an exothermic reaction shift the reaction towards reactants?

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How do you know if a reaction system is at equilibrium?

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The main use of the ideal gas law, PV=nRT, for us is to convert between Kc and Kp (concentration and partial pressure). You can think of the ideal gas equation as Kp=Kc(RT)^(n). In this case n=(c+d)-(a+b) according to the reaction form aA+bB=cC+dD.

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Pure liquids and solids have definite molar concentrations. Gases and aqueous solutions have variable molar concentrations because there is a certain amount of moles of a substance in a certain volume, hence the molarity= moles/Liters. Therefore when pure solids and liquids are involved in a reactio...

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The main use of the ideal gas law, PV=nRT, for us is to convert between Kc and Kp (concentration and partial pressure). You can think of the ideal gas equation as Kp=Kc(RT)^(n). In this case n=(c+d)-(a+b) according to the reaction form aA+bB=cC+dD.

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A couple things that could help you name coordination compounds is to remember to first name the cation then the anion. Also, remember to name the ligands before naming the central metal ion. Furthermore, for anions, the central metal ion has a special name (for example iron would be called ferrate ...

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Iron can form six bonds because it is one of the atoms that can form an expanded octet. Iron can have an expanded octet because electrons can go into the d-orbital found in the third principal energy level.

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Coordination compounds form out of a Lewis acid-base reaction in which neutral or anion molecules bond to a central metal ion. The bond formed is a coordinate covalent bond between the central metal ion and the ligands.

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Once you find the shape of a compound and determine if the compound is polar or non-polar how does this affect our analysis of the compound's boiling point. In other words, how do shape and polarity play into a compounds boiling point?

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To determine the forces present in the molecule it is easiest to first draw out the Lewis structure. First look for ionic forces, look for an interaction between a cation and an anion (Such as Na+ and Cl-). Then, you can look for hydrogen bonding. Hydrogen bonding occurs when a hydrogen is bonded to...

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Can hybridization go past d2sp3? For example, how could you write the hybridization if there were 7 orbitals involved?

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Can someone explain orbital overlap and the role that orbital overlap plays on bond strength?

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Why can sigma bonds rotate, but not pi bonds?

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What does it mean when an electron is promoted? Also, what effect does electron promotion play on the overall molecule or atom?

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What are the characteristics that make a compound polar or non-polar?

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Drawing the molecular shape in three dimensions is useful for understanding and determining the shape. Use a dashed triangle for elements going away from us and use a solid triangle for elements coming towards us.

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How does a density isosurface relate to the electrostatic potential surface? Also, how would you analyze an electrostatic potential surface?

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I read in the book that "a molecule might have an odd number of electrons, so octet formation is numerically impossible". Would it be possible for the molecule to form an octet by gaining or losing an electron? I don't understand why the molecule would not be able to form an octet.

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Based on what I read in the textbook hypervalent compounds and variable covalence is basically the same. Is there a difference between the two terms?

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In resonance structures, the bond is shifted to different configurations, and this can change the lone pairs of the surrounding atoms. For example, carbonate has a resonance structure where one of the outer oxygen molecules has a double bond, while the other two oxygens have single bonds. This doubl...

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I understand single bonds, double bonds, and triple bonds, but I do not understand what the bond order tells us. Can someone explain bond order and give an example?

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The formal charge gives an indication of the extent to which atoms have gained or lost electrons in the process of covalent bond formation. Atom arrangements and Lewis structures with the lowest formal charges are likely to have the lowest energy.

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How do we know which atom to put in the center of a Lewis structure?

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Are compounds with an expanded valence shell considered stable? Also, how would an expanded valence shell occur?

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I don't understand how delocalized electrons work. How are the electrons distributed over several atoms?

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Can someone give me an example of a situation where an element displays variable valence?

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How does shielding from electrons in a multi electron atom effect the nuclear charge?

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What is meant by a positive or negative spin of an electron? Also, why do electron spins have the values of +1/2 and -1/2?

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What happens to the extra or left over energy when an election is ionized from an atom?

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What is the difference between an atomic radius and a covalent radius?

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Why do shorter wavelengths have higher energy light and longer wavelengths have lower energy light?

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What is the significance and use of light intensity when solving electromagnetic radiation questions?

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Why is the theoretical yield always larger than the actual yield?

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Are the terms reactants and reagents interchangeable? I know that reactants are the starting materials that are used up in a chemical reaction, but I am still slightly confused by the term reagent.

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What is the difference between atomic weight and molecular weight?

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