CHEMISTRY COMMUNITY

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H4O would have a +2 charge, which is very unstable, therefore it would be more willing to give off those extra hydrogens to become more stable (hence making it a stronger acid until it is in its neutral state water).

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Kevin Liu 1J wrote:Noble gases are not included in the trend for electronegativity.

They are usually not included. But Xenon, since it has such a large atomic radius, has very weak control over its valance electrons and therefore can bind with other elements.

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Why are the molecules As2O3 and BiO3 Amphoteric?

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S 1C wrote:Wait if it's an acidic oxide why is the answer basic...? Am i missing something or getting caught up in the wordiness?

The answer is that it would be Acidic.

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When would you use an equilibrium sign instead of just a regular arrow when writing chemical equations?

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For this problem you are prompted to write the chemical equation for the proton transfer equilibria of the following acids in aqueous solution and identify the conjugate acid-base pair.
Part C is H2PO4-
Why is the pair H2PO4- and HPO4-2 instead of H2PO4- and H3PO4?

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If you are referring to diethyl ether to having dipole-dipole intermolecular forces and water to have hydrogen bonding, then water (hydrogen bonding) would have a stronger intermolecular force because hydrogen bonds are stronger than dipole-dipole bonds. Thank you this is what I was asking! Do you ...

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How do you think Professor Lavelle would test us on Coordination Compounds? I feel there is a possibility of naming, but other than that I am unsure of how it would be tested.

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I am really confused about the definitions in coordination compounds. What is a coordination compound and ligand.

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What is the difference between a Bronsted and Lewis Acid?

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In lecture, Professor Lavelle noted that a longer bond length meant a stronger acid but then went on to explain the example of Tricholoracetic Acid and noted that when exchanging Cl for H the acid got stronger through the inductive effect, even though the bond length is shorter. Could somebody clari...

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A pi bond is not two bonds but it does overlap in two places because there is a nodal plane. Since pi bonds overlap side to side there will be overlap above and below the internuclear axis but this is still considered one bond. How would you know what is in the nodal plane and where the internuclea...

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Is there a connection between boiling point and IMF Strength? If so, why or why not?

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Ionic is an intramolecular force (between ions), intermolecular forces refer to forces between molecules and ions such as dipole-dipole or hydrogen bonding.

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If you are referring to diethyl ether to having dipole-dipole intermolecular forces and water to have hydrogen bonding, then water (hydrogen bonding) would have a stronger intermolecular force because hydrogen bonds are stronger than dipole-dipole bonds.

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Jorge Ramirez_4H wrote:So the stronger the forces are the higher the boiling point?

Yes, the stronger the forces, the more energy is needed to vaporize them, therefore, the stronger the forces the higher the boiling point.

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How would you calculate the radius length when trying to find the interaction potential energy?

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Why do regions of lone pairs of electrons repel each other more than lone-bond or bond-bond regions?

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Why do rod-shaped molecules have a higher boiling point than spherical shapes molecules?

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What was Professor Lavelle trying to explain when showing us the 3 hydrocarbon examples and how they are liquid, viscous, and waxy? What concept was it?

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I understand for Dispersion forces, interactions are always present and attractive, but could somebody explain what the Interaction Potential energy is and what the variables in the equation represent (the Ep is proportional to -(symbol1) times (symbol 2) over radius to the sixth power?

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Polarizability power refers to an atom's ability to cause large distortions in the electron cloud while polarizability is an atom's likeliness to undergo a large distortion.

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You can look at an elements electronegativity level. The more electronegative, the more uneven the distribution, and therefore has ionic character.

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At all the review sessions I had gone to including Professor Lavelle's, they did not specify about conditions such as vacuums, therefore, I believe that you shouldn't worry about having to know those concepts. Just how to do the computational calculations.

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Since the molecule also has symmetry in its structure and electron distribution, the polar forces cancel each other and therefore is considered nonpolar.

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One of Lavelle's topics under Quantum world was "Understand the relationship between Schrodinger's equation (H psi =Epsi), wave functions, and orbitals.
Could somebody explain the Hpsi=Epsi relationship and how that relates to wave functions and orbitals?

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To find the wavelength you use DeBroglie's equation which is wavelength=planks constant/(massxvelocity) and when you plug in the given values the wavelength should come out to be 2.0x10-10m.

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All you need to know is that for the Lyman series the final energy level is n=1, the Balmer series the final energy level is n=2, the Paschen series the final energy level is n=3, and the Brackett series the final energy level is n=4. This can be solved by using quantum equations.

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The mass of the electron is 9.1095x10-31 kg. This value will be given to you on the reference sheet for the test so don't worry about it!

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Energy can be measured by using n (energy level), therefore, when the electron moves from the 1st to the 2nd energy level, the energy increases because higher energy levels have a greater energy.

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Since the 4s subshell is farther than the 3d subshell, the electrons would be removed from the shell farthest from the nucleus, therefore taking it out of the 4s rather than the 3d. That is why the ion has a 3d10 configuration rather than a 4s23d8

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Where does the work function come in any of the chemistry problems so far? I do not understand what the work function is and how it relates to any formula so far.

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I am really confused on what it means for an electron to have wavelike or particle-like properties. Could somebody explain which an electron is like or give an example/reference to support one side?

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905416023 wrote:I too am confused about this. On problem 1d.25, there is mention of a g subshell.

That question was referring to "Which of the following does not exsits" to show that the 4g subshell does not exists (which is the answer).

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The spin would be denoted with the 4th Quantum number (+/- 1/2). Another tip is to remember to use the Pauli Exclusion Principal and Hund's Rule when drawing it out. Hope that helps.

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All of these also increase for a hydrogen atom as well. I think the important part of the question is understanding why these increase in a hydrogen atom versus a lithium atom. For a, b, and c, (all properties that apply to single-electron systems), the reason for the increase is the same between h...

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It would be regarded as one question.

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thank you so much I figured it out

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When the question refers to finding the principal, orbital, and magnetic quantum numbers, what is each referring to?

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I was looking at the solutions manual and the value for h is not planks constant (6.626x10-34) but some other value. Can somebody explain why it is different?

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For number 19, we need to use the mass for a proton and neutron. What values would we use for those equations? Thanks

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I am confused on where to start for homework problem 1B parts a - c. Am I supposed to convert the wavelength to energy? I guess I'm also confused about what the question is asking. Could someone help? Thanks?

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Sophia Shaka 3L wrote:From the Comments and Errors file found on the Chem 14A site:
"L.35 in the textbook question:
In the third reaction step the compound "FeBr2" needs to be "Fe3Br8"."

Could you explain why that is?

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I was having trouble with question L.35. I have to balance the following equation
FeBr2 + Na2CO3 = NaBr + CO2 + Fe3O4

Thanks!

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Combustion is another word for burning. In a combustion reaction, the fuel (usually a hydrocarbon or other related molecule), burns with O2 gas. Combustion simply means reacting with O2 and could yield products such as water and carbon dioxide.

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They are the same amount of sig figs! Since they are the same amount of numbers 114 and 114. they are equal in sig figs.

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I am not sure about grading, but rather use unrounded values until the end to ensure you come out with the correct answer. Your answer may be a tad off because you may have been using rounded values throughout.

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That is correct. You would not round values until the end and then the end value would be rounded to three sig figs.

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In most cases, you would not use the number of sig figs in the molar mass, but instead, use the number of sig figs in your given amounts in the question.

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Capital M is usually used to reference molarity while c is another variable used in other equations.

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Yes! Dilution would be adding more solvent (usually an aqueous solution such as water) while keeping the solute amount the same, therefore, changing the molarity of the solution.

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Another tip for balancing combustion equations would be that if you end up with a 1/2 coefficient, multiply all the coefficients by 2 to get the balanced equation.

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I learned this simple trick in my high school Chemistry class.
1. Percent to mass (change the percent sign into a grams sign)
2. Mass to Mole (Convert mass to moles using molar mass)
3. Divide by Small (divide by the smallest number)
4. Times to whole (times to get whole numbers)

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I was a little confused reading the syllabus. What versions of the Texas Instrument calculators are we allowed to use on tests and exams?

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