CHEMISTRY COMMUNITY

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The hydrogen in the carboxyl group results in the transfer of a proton, making the molecule a proton donator and therefore, an acid.

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Water can act as either an acid or a base depending on what substance it is interacting with.

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It's actually pretty simple once you understand that all you have to do is determine the number of regions of electron density around the atom. After that it will be pretty simple, 1=s, 2=sp, 3=sp2, etc.

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Examine the number of regions of electron density around an atom and it will give you the hybridization. 1=s, 2=sp, 3=sp2, etc.

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Electron affinity increases across a row meaning that elements towards the right side have a higher electron affinity.

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I agree with everyone else. An increase in energy results in an increase in frequency, not necessarily intensity which I believe concerns the amount of photons.

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First you would need to convert CuNO3 into moles and plug it into the equation M=n/v as well as the given molarity. You would then arrive at an answer in L and therefore, would need to convert it into mL.

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mol stands for millimole which is equal to .001 mol.

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The solvent is the substance that dissolves the solute. The way I distinguish the solvent from the solute is by referring to water's characteristic as the universal solvent and water is commonly used to dissolve substances.

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I normally do all the calculations and include significant figures in my final answer. I believe that if you round early in the process, the resulting answer may be a couple decimal places off.

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Yes, the answer would have three significant figures.

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Pi bonds overlap parallel to one another meaning that rotation is not possible. If there was any form of rotation, the bond would be broken as a result.

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Yes, because the after the minimum energy needed to eject an electron from a particular surface, the excess energy is the same as the kinetic energy of the electron.

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I believe it is safe to say that the only constant c we will be encountering for the time being will concern the speed of light.

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Only a lewis dot structure would allow you to identify the types of bonds (single, double, triple) and therefore, determine the number of pi bonds. However, molecular shape does not include the information needed to determine the number of pi bonds in a molecule.

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You can determine if the bond angle is less by examining the number of lone pair electrons. This is because there is a slight electron repulsion and therefore the bond angles will decrease.

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Localized electrons are those that behave normally, their are associated with a single atom. Delocalized electrons behave somewhat abnormally and relate to resonance structures.

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Yes, for a pi bond to be present there must be multiple bonds between two atoms.

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Sigma bonds are formed by end-to-end overlapping while pi bonds are formed by the overlapping of lobes. Sigma bonds are generally stronger than pi bonds primarily due to the fact that they concentrate electrons into a particular area to a greater degree compared to pi bonds.

105618850 · Re: Homework due date It is due on Sundays at 11:59 PM.

It is due on Sundays at 11:59 PM.

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You would also need to consider if the dipole moments, if there are any, cancel each other out.

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What I like to do is review some of the topics discussed in lectures by watching some videos that cover and explain some of the things in greater detail.

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I wouldn't say that would be the case for every molecule. For example, for compounds like H2, Cl2, etc. are all considered non polar.

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Since carbon only possesses two bonds, rather than the four it tends to form. Therefore, due to this abnormality, the formal charge would be -2.

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Isoelectronic is simply a term used to describe atoms with the same amount of electrons.

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Hey! It's pretty simple actually, well only when it concerns the s and p blocks. The number of valence electrons are separated into into the different columns of the periodic table. you can search it up online and it will offer a little trick to memorizing the amount of valence electrons using the p...

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Yes, the molecule will always strive to achieve the greatest amount of stability meaning that it will most likely have the lowest energy.

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I agree with everyone else above. Increasing or decreasing the amount of electrons alters its ionic radius as electrons have a significant contribution to an atoms size.

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I agree, London dispersion forces are the forces between multiple molecules, or intermolecular forces. Topics that concern bond lengths relate to intramolecular forces.

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Electron repulsion occurs when there are multiple electrons present. That is what contributes to a molecules structure and their respective bond lengths.

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Ionic character depends on the difference in electronegativities. The greater electronegativity, the greater tendency to attract electrons or in other words a greater bond strength.

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The concept that you are questioning can be best explained by the equation E=pc. Although a photon does not technically have mass, it has energy which is derived from the motion it possesses.

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I searched it up because I too was unsure about the minimum difference that classifies a molecule as polar. I found that most sources supported everyone else's answer that it must be greater than 0.5.

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It will affect its ionic radius. Adding/removing electrons will alter the atom's characteristics and properties, including its ionic radius.

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The strength increases with the number of bonds. You can also determine the strength by observing the molecular structure of a molecule. By examining the bond length, shortest being the strongest, you can determine the bond strength fairly easily.

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Ionic bonds involve significant differences between electronegativities. Therefore, molecules that display the most covalent character are those with the atoms with the least electronegativity.

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Yes they are considered electron regions. That is why they contribute greatly to bond angles and molecular structure; with their repulsion.

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I do not remember him mentioning that we are required to memorize the bond angles, but I believe you should make an effort to familiarize yourself with which bond angles are associated with their respective molecular shapes.

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Yes, I agree with the comment above the electron repulsion is the primary factor that contributes to slightly smaller bond angles.

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Yes. The lone pairs are what distinguish bent from linear. I believe the repulsion from the lone pairs results in a bent molecular structure.

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You can differentiate between trigonal planar and trigonal pyramidal by examining the different electron regions it possesses. Trigonal planar molecules only have three electron regions while those described as trigonal pyramidal have four. I like to think trigonal planar molecules as Egyptian pyram...

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I use this one a lot (includes bond angles as well):
https://mmstcchemistry.weebly.com/uploa ... ometry.pdf

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I believe that molarity involves a solvent (the universal solvent is water), capable of dissolving a certain amount of solute so the final product will be in the liquid form.

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Polar bonds only concern the interaction between two atoms while polar molecules concern the polarity of the overall molecule itself. Differences in electronegativities help determine if something is polar. You can observe differences in dipole moments and sometimes you can determine if a molecule i...

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It isn't considered polar because the differences in electronegativities isn't that significant. A way that I associated C-H bonds with non polarity is the fact that, in organic chemistry, hydrocarbons are always considered non polar.

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A substance's boiling point often concerns the amount of energy needed to break the intermolecular forces that hold the molecules together. I believe that ionic compounds often have higher boiling points due to the electrostatic interactions between ions.

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You should examine the dipole moments and observe if they cancel each other out. A more simple way of thinking about polarity is looking at the molecule's symmetry. At times, it will be pretty obvious but sometimes I double check using the scientific method rather than just relying on the visual met...

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You should examine the dipole moments and observe if they cancel each other out. A more simple way of thinking about polarity is looking at the molecule's symmetry. At times, it will be pretty obvious but sometimes I double check using the scientific method rather than just relying on the visual met...

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A sigma bond is a bond that results from an interaction that is described as overlapping and enables rotation. The s-p overlaps, etc. simply mean that orbitals are overlapping or occupying the same location.

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I believe that there is an exception with oxygen's radius being slightly larger compared nitrogen. Are there any other exceptions with the trend in atomic radius?

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I believe that there is an exception with oxygen's radius being slightly larger compared nitrogen. Are there any other exceptions with the trend in atomic radius?

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I also believe that it concerns the outermost electrons since ionization energy is the amount of energy required to remove the most loosely bound electron(s) from an isolated molecule/atom.

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Hey! I believe we examine intermolecular forces when determining the boiling point because we are not separating the atoms that compose the molecule, yet the forces that hold identical molecules together.

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Yes, molecular shape often displays polarity. Differences in dipole moments result in an asymmetrical structure/unequal bond lengths.

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What is the importance of Schrodinger Equation in chemistry? In what instances would we need to know the probability of an electron's location. Does it relate to any other topics in chemistry?

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How can you determine which ionic molecules display the greatest covalent character? Is it just by comparing their respective electronegativities or is there another factor that you must consider.

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How does VSEPR determine the molecular shape of isoelectronic species?

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What are the strengths of sigma and pi bonds in relation to others (Covalent, ionic, etc.)

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How do you know which atoms are capable of violating the octet rule? I remember my TA mentioning something about expanded valence shells but I was still a little confused.

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