CHEMISTRY COMMUNITY

lasarro

use slacked lime or quick lime

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not sure, but I know this post is going to count as one!

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Unfortunately not, but the homework problems would help

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how many ligands does a heme complex have

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I didn't see titrations on the syllabus, but it was on the final. If I remember correctly, we were told that titrations wouldn't be emphasized. How were we supposed to know it would be on the final??

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Feel free to use this thread to talk about the final...

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can carbon monoxide bind to a heme complex?

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Can someone answer this learning objective from the acids and bases section?

"Why do salts of weak bases produce acidic solutions and salts of weak acids produce basic solutions?"

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What is the chemical formula for the ligand ethelynediaminetetraaceto?

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bronsted refers to an exchange of protons. Lewis refers to an exchange of electrons

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What is the importance of cisplatinum?

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Is the charge of the transition metal always going to be given to us? If not, how do we know it?

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What is a ligand??

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Why does PBr3 have a higher boiling point than PF3? I thought since the bonds in PF3 are stronger (smaller atoms--> shorter bond length --> stronger bond) it would have a much higher boiling point than PBr3. The solutions manual says that since PBr3 has more electrons, it has a higher boiling point....

lasarro

Do we have to know vapor pressure for test 2? If so what is it?

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How does NH2OH have a dipole-dipole intermolecular force? That means that NH2OH would have to be a polar molecule, but the electronegativity difference between all the elements is very small. Could someone please explain this? Maybe a picture showing the dipole moment if you could find one?

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What can classify as a region of electron density in a molecule?

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What is the seesaw shape?

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Do we have to know hybridization for test 2?

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Could someone please give me an example to explain london dispersion forces and vanderwaals.

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In SO2, for the oxygen that has a single bond to the sulfur atom, could we count the 3 lone pairs on the oxygen atom to be its own region of electron density? Or would we count those three lone pairs and the electrons bonded between the sulfur tom as one region of electron density?

lasarro

On exercise 2E.1, it shows 2 ball-stick models. One of them is a bent shape the other is a linear shape. It asks which model would have lone pairs. How would I know which model would or would not have lone pairs based on the ball and stick shapes?

lasarro

covalent, ionic and metallic are the 3 types of atomic bonds.

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The Ryberg equation measures energy levels

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Lavelle hasn't formally discussed nomenclatures yet, so I don't think we should worry about it until it comes up. But it's nice to now basic prefixes like tri- means three and so on.

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If the highest energy level is a d orbital, then yes, the atom can hold up to 10 valence electrons.

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Noble gases have no electronegativity because they already have a full octet

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Can someone please define what a dipole moment is?

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What does MeV mean?

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Does a resonance structure just mean moving an electron around?

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How do you calculate the dipole moment if we are not given the electronegativity values?

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How do we pick the central atom for a lewis dot structure of a molecule?

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What is an observed bond length and what does it have to do with resonance structures?

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In general, bonding strength and length is proportional to one another. And bond length is always given by experiemental data.

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What's the difference between electron affinity and ionization energy?

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How do I know how many oribitals there are in s,p,d,f?

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What is an atomic radius and how do we calculate it?

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What is an ionic radius and how do we calculate it?

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Can someone explain the relationship between schrodingers equation, wave functions and orbitals?

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I know the speed of light is 3x 10^8 m/s in a vacuum, but what exactly is a vacuum?

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I know Hz is measured per second, but what per second??

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Why do we use the speed of light to calculate the wavelength and frequency of electromagnetic waves, like radiowaves?

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I usually look at the outline and make sure I know every topic on there.

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How is momentum defined and is it different than velocity?

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I would practice with just a symbol and be consistent with it. A lot of the workshops that I went to used problems that only use M as the symbol for molarity, so you may want to use that on your test.

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We are also given a reference sheet that has equations, som unit conversions and constants on it.

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The sig figs are determined by the numbers provided in the initial problem. I.e. if a problem included 2.15 then your answer would be 3 sig figs.

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The number of sig figs are determined by the numbers mentioned in the inital problem.

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Can someone explain how Planck's constant is derived and its significance?

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In most problems that we have seen so far it usually mentions what state the compound/ molecule/ element is in, so I wouldn't worry about it for now for his upcoming exam.

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For tests and exams, I would refer directly to the periodic table that is given for the exam and not round numbers.

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You only assume that the sample is 100g to make the calculations easier. For example if a CH4 sample contains 20% carbon but the sample itself is only 10 grams. You could assume for a second that the sample was 100 grams and 20 grams of that was carbon. Then you could use that ratio to say a 10 g sa...

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If you have 0.018 mol NaCl in a NaCl + H2O solution, you also have to have 1 mol of NaCl and 1 H2O because of the stoichiometric coefficients. How can this be possible if you only have 0.018 mol NaCl present in the solution, but you have to have at least 1 mol of NaCl for the solution?

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Ionic bonds are usually stronger than covalent bonds. A defining characteristic of ionic bonds is that an electron from one atom is "taken" by another atom, whereas in covalent bonds, the electron is shared between the two atoms.

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With stoichiometric problems, think about it as an equation. An equation such as 1=2 is simply not true. In chemistry, it's essentially the same concept. You have to have the same number of atoms on each side of the equation. So if you have N2 on one side you have to have N2 on the other side. The c...

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