CHEMISTRY COMMUNITY

StephanieDoan3B

When drawing Lewis structures of HClO, HClO2, HClO3, HClO4 to compare acid strength due to electron withdrawing atoms, do we need to draw all of the resonance structures of HClO4 and HClO3?

StephanieDoan3B

Which of the following reactions can be classified as reactions between Brønsted acids and bases? For those that can be so classified, identify the acid and the base. NH4I(s) --> NH3(g) + HI(g) What makes NH4+ a Bronsted acid? Isn't it NH4I in solid form not aqueous on the left side of the reaction?

StephanieDoan3B

It is a rule. When the coefficients in an chemical equation is multiplied by 2, the k is squared. This is a rule when manipulating equilibrium constants.

StephanieDoan3B

You can draw the Lewis structure and see where lone pairs can possibly be contributed to the coordinate covalent bond. But for the most commonly used ligands, it would most convenient to memorize if they are mono, bi, tri, etc. -dentate.

StephanieDoan3B

It was stated, "The promotion of electrons will occur if, overall, it leads to a lowering of energy by permitting the formation of more bonds." How come Nitrogen can be hybridized to sp3 if the number of possible bonds (3) doesn't' increase after hybridization?

StephanieDoan3B

There are no unpaired electrons anywhere in CH2, and there is an even number of electrons total, so it cannot be a radical.

StephanieDoan3B

The book states, "It looks as though a carbon atom should have a valence of 2 and form two perpendicular bonds, but in fact it almost always has a valence of 4 (it is commonly “tetravalent”)..." Valence is not the number of valence electrons because Nitrogen's valency is 3. Could someone p...

StephanieDoan3B

Every angle in an octahedral structure is 90 degrees. In other words, the orientation of the molecule doesn't matter, so the electron density you choose for the placement of the first lone pair doesn't matter.

StephanieDoan3B

Yes, polar vs. non polar is geometrically unequal vs. equal distribution of negative charge in the atom.

StephanieDoan3B

For example, in SO2, the most stable structure is O=S=O which gives all three atoms formal charge of zero. However, O=S-O and O-S=O also exist, giving formal charge of -1 to the oxygen attached by single bond and formal charge of +1 to the central S atom. This would also make sense because O is more...

StephanieDoan3B

Oxygen is more electronegative than sulfur and would attract the hydrogen more strongly than sulfur does.

StephanieDoan3B

(Not exactly a joke but a cheeky pickup line)
Can I steal an electron so you can be my +1 to _____?

StephanieDoan3B

Why are there three resonance structures for SO2 when the one with two double bonds has the lowest formal charge? Why would the other two structures (one double, one single) be allowed to exist when they have higher formal charge?

StephanieDoan3B

Does effective nuclear charge increase or decrease down a group? And as we move far down the table, what role do d orbitals play in shielding?

StephanieDoan3B

I don't think we have to or are able to use trends to compare atoms of elements not in the same period or group.

StephanieDoan3B

All three orbitals have the same energy, and the electron will fill any of them first. We designate that px is filled first, then py, and pz because of convention.

StephanieDoan3B

When filling up orbitals with electrons, we fill 4s before 3d. However, we write the electron configuration of V, for example, as [Ar] 3d3 4s2 because here, the 4s is now higher energy than the 3d. Does this mean that the energy levels of orbitals change relative to each other when they become fille...

StephanieDoan3B

Light acts as both a wave and a particle (wave-particle duality) but both natures have never been captured simultaneously in the same experiment. De Broglie's equation, λ=h/mv, illustrates this duality well because λ is wavelength (property of a wave) and m is mass (property of a particle.

StephanieDoan3B

Yes, these series apply only to Hydrogen because electron interaction for atoms with more than one electron will be much more complex. The electrons would interact with other electrons due to electrostatic forces, not accounted for here.

StephanieDoan3B

Yes and if you have a molecule with a single compound, like O2 or N2, keep that for last because it's the easiest to manipulate.

StephanieDoan3B

The book and a previous post from a Moderator said to keep as many sig figs in your calculator as possible and round at the very end. But for problems like combustion, there is a step of addition and/or subtraction (of masses), so I don't know if we have to take off the significant digits based on t...

CHEMISTRY COMMUNITY

Search found 21 matches

Drawing resonance when comparing acid strength

12.9(b)

Re: Notes on 11.37

Re: Monodentate, Tridentate

Nitrogen hybridization

Re: 4.73

Valence/valency?

Re: Octahedral vs Trigonal Bypyramidal family

Re: Polar ve non polar [ENDORSED]

Formal Charge vs. Electronegativity

Re: 3.57 hydrogen sulfite

Re: Post All Chemistry Jokes Here

Sulfur Dioxide?

Effective Nuclear Charge Down a Group [ENDORSED]

Re: Across a period vs. Down a group

Re: P orbitals

4s 3d or 3d 4s?

Re: Light as a wave or a particle [ENDORSED]

Re: Balmer and Lyman Clarification [ENDORSED]

Re: Order of Elements to Balance [ENDORSED]

Re: Clarification