CHEMISTRY COMMUNITY

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Intermolecular bonding is between multiple molecules. Intramolecular bonding is within a single molecule.

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An oxyacid is an acid that contains oxygen and contains at least one other element. It also has at least one hydrogen atom bonded to oxygen.

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A ligand is an ion or molecule attached to a metal atom and donates electrons.

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A strong base would have a higher pH due to it accepting more protons. A weak base would have a lower pH.

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A polyprotic acid can donate more than one proton. A polyprotic base can accept more than one proton.

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Yes. There are only radicals when there is an odd number of electrons.

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I would suggest going to the student activities center and trading in your old test for other classes and seeing if there are any old finals for 14a!

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If the electronegativity is higher, the bond is stronger. It also means the bond is shorter.

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I think it would always be the single bonded ones due to the absense of the pi bond but I am not too sure

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Yes. These are the only atoms that can make a hydrogen bond. Hydrogen can make other bonds with other atoms.

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Okay I talked to someone about this question and I also found out that pKa is preferred it is the log version of the number and therefore easier to compare and use rather than the scientific powers of Ka

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Yes. This is the constant value that should always be used.

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Chlorine has a higher electronegativity than phosphorus, so it pulls the oxygen atom electrons towards itself with greater force than phosphorus. The fact that chlorine has a higher pull means that oxygen electrons become less accessible for the hydrogen atoms to "share", making it less fa...

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the second ionization energy of Mg is larger than the first because it takes more energy to remove an electron from a positively charged ion than from a neutral atom

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What happens in hybridization? Like why does it happen? Does it lower the energy of the molecule?

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Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons

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Electronegativity is how much an atom attracts electrons. Ionization energy is needed to remove electrons from atoms.

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Is there a specific atom in a molecule that we should try and get to have a 0 formal charge? If there is a charge we can't avoid where should we put it

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Why do different resonance structures have different formal charges and how do we know which is the major contributor.

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Lewis acids accept electrons while bases donate electrons. Acids are more positive and bases are more negative.

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Hey, could someone please explain to me how conjugation affects hybridization and if we will have to use this concept explicitly.

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Yes due to the partial charges. Nonpolar molecules can have temporary dipoles.

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Hello! Could someone explain why a triple bond has a hybridization of sp

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Yes. Both of the molecules have to be polar. The partial charges created by the dipoles makes it polar.

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How does the conjugation of a molecule affect its energy and bond lengths

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Will someone please explain how pi bonds and their p orbitals cause a lower energy state

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No but they determine whether or not the bond is able to rotate.

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A double bond does not affect the melting point. The intermolecular force is what affects the melting point.

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So basically pi bonds are formed because the side-by-side overlap of p orbitals leads to a lower-energy state than if there were no overlap so it depends on the valence electrons of the atoms and the energy state certain bonds create

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Why is pKa preffered over Ka?

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By definition Molecules that contain dipoles are called polar molecules, so yes the two can't be separated.

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it is a compound that contains hydrogen, oxygen, and at least one other element, with at least one hydrogen atom bond to oxygen that can dissociate to produce the H⁺ cation and the anion of the acid

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Yes. Polar molecules have a permanent dipole moment. Nonpolar molecules can have dipole moments that cancel each other out.

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Out of acetic acid and formic acid, formic acid is considered stronger because the CH3 in acetic acid is electron donating. The CH3 actually contributes electron density towards the O-H bond, making it harder to remove the H, and making acetic acid a weaker acid than formic acid

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I think the exam will consist of problems that incorporate topics we have learned throughout the year with an emphasis on later topics that weren't included on our last test!

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the change in energy of a hydrogen atom is positive

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Ligands are ions or neutral molecules that bond to a central metal atom or ion. Ligands act as Lewis bases (electron pair donors), and the central atom acts as a Lewis acid (electron pair acceptor).

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Your best bet is to identify the central atom in the chemical formula (usually a transition metal) and then adding the number of atoms of the nearest atom/molecule/ions connected to it

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The Lewis definition encompasses the bronsted defintion. Lewis acids can accept an electron pair, while Lewis bases can donate an electron pair where a Bronsted-Lowry acid is defined as a substance that gives up or donates hydrogen ions

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A Lewis acid is an electron-pair acceptor. A Lewis base is an electron-pair donor.

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An oxyacid is an acid that contains an oxygen atom bonded to a hydrogen atom and at least one other element

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When one or more lewis diagram can be drawn, the molecule is said to have resonance. Resonance isn't about the rotation of bonds, but about the delocalization of electrons that contribute to the overall structure. The idea that resonances rotate isn't really valid.

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You know that a ligand is a polydentate if it can bond to a central metal atom in more than one coordinate bonding cites.

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No! You do not need to memorize them, but I would be familiarize yourself with when we use them!

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In both molecules the oxygens are bonded to the chlorine but not to the hydrogen and thus draw the electrons in the O—H bond towards the chlorine and the oxygen, making the O—H bond more polar. This effects chloric acid more than chlorous acid, since the hydrogen will more readily dissociate in a mo...

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Chelation is a type of bonding of ions and molecules to metal ions so look for a central metal atom

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Polarizability increases down a group because atomic size increases and larger electron clouds distort more easily. Polarizability decreases across a period because of increasing nuclear charge

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I think week 9 should be on Coordination Compounds and their Biological Importance and week 10 should be on Acid and Base Structures and Properties.

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Any bond with a Hydrogen and a N, O, or F

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Are the VSEPR shapes that we need to know linear, trigonal planar, tetrahedral, trigonal bypyramidal, and octahedral? Are there any others we should know?

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