CHEMISTRY COMMUNITY

Daniel Martinez 1k

There are 2 a's, pentaammine.

Daniel Martinez 1k

HClO2 is a stronger acid than HBrO2 because Cl is more electronegative (EN: 3.0) than Br (EN: 2.8).

Daniel Martinez 1k

It would be sp3. It does not matter whether it is an actual bond or a lone pair as long as there is a site of electron density present.

Daniel Martinez 1k

A ligand is a lewis base that donates a pair of electrons to the transition metal it is attached to.

Daniel Martinez 1k

Oxalate is polydentate (Bidentate) so that is the reason it has the prefix "bis-" in front of it. The "bis" prefix suggests that there are 2 oxalate ligands that are attached to the transition metal, which explains why the answer is Na[Fe(OH2)2(C2O4)2].

Daniel Martinez 1k

Coordination number corresponds to the number of electron density regions that are connected to the transition metal. There tends to be a max of 6.

Daniel Martinez 1k

Yes. The ligands donate an electron pair.

Daniel Martinez 1k

Yes, you are correct. The stronger the IMF = more force needed to break the bond (i.e higher melting point).

Daniel Martinez 1k

Ammonia is a base because the lone pair on the nitrogen gets donated to other acids that are in need of an electron pair.

Daniel Martinez 1k

Hybridization works the same for all elements.

Daniel Martinez 1k

Si2F2

Daniel Martinez 1k

Yes the bond angles are all correct.

Daniel Martinez 1k

I think we can still turn in homework on molecular structures because we discussed molecular structures (hybridization) on Monday.

Daniel Martinez 1k

Great question. I would also like to know why so I am commenting so I can locate this post easily.

Daniel Martinez 1k

In order to find hybridization, you have to count the number of regions of electron density around the central atom. It can be useful to draw out the lewis structure to see the regions of e- density. After that, you would simply write out the hybridization: s- 1 region of electron density sp- 2 regi...

Daniel Martinez 1k

Some angles have "less than" because they have lone pairs, which distort the pull that the atoms have on each other.

Daniel Martinez 1k

Definitely not necessary. However, it can help you know how many lone pairs and bonded pairs there are, which is essential for VSEPR.

Daniel Martinez 1k

Electronegativity is the ability of an atom to pull on other atoms. The trend that electronegativity follows is that it increases to the right and up on the periodic table.

Daniel Martinez 1k

The lewis structure would have 4 bonded pairs. So, the C would have a bond pair with 2 Fs and 2 Hs. Since there are 4 bonded pairs and no lone pairs, the shape of the molecule is a tetrahedral.

Daniel Martinez 1k

Linear molecular shapes arise when there are 2 bonded pairs. If there are zero, three, or four lone pairs attached to the central atom that already has two bonded pairs, the molecule would have a linear shape.

Daniel Martinez 1k

Polarizability increases as the charge and the size of the anion increases.

Daniel Martinez 1k

Ionic bonds are stronger than covalent bonds in a vacuum. However, in water, covalent bonds tend to be stronger.

Daniel Martinez 1k

The trend for dissociation energy is that as bond length increases, the dissociation energy decreases.

Daniel Martinez 1k

Sulfur is also an exception to the octet rule. I believe it can go up to 12 electrons as it does in SF6.

Daniel Martinez 1k

The homework questions should consist of chemical bonds. Personally, I included 2D material and on.

Daniel Martinez 1k

Yes. Resonant structures are just different ways of drawing the same structure. These structures should still follow the octet rule when being drawn all of these different ways.

Daniel Martinez 1k

Make sure to remove the electrons from the highest energy orbital. For example Zn: [Ar] 3d^10 4s^2, the electrons would be removed from the 4s orbital since it is the highest energy orbital.

Daniel Martinez 1k

NO2- is not a radical. It has 18 electrons, all of which are paired.

Daniel Martinez 1k

Electronegativity is the tendency of an atom to pull electrons. Electronegativity follows the same trends as ionization energy (Increases up and to the right).

Daniel Martinez 1k

Everything we have been assigned homework on until 2D. In other words, Fundamentals, Quantum World, & Chemical Bonds (up to 2D).

Daniel Martinez 1k

No, the Octet rule does not apply to Boron bc it is more stable with 6 e-.

Daniel Martinez 1k

During Wednesday's lecture, he mentioned H, He, Li, and Be as being exceptions to the octet rule because it was very unlikely that they would gain the electrons needed to complete an octet.

Daniel Martinez 1k

Sb has the electron configuration [Kr] 4d^10 5s^2 5p^3.
Since the 4th shell is completely filled, we only focus on the electrons from the fifth shell. With that being said, we only have 5 valence electrons in the 5th shell (2 e- from s-shell & 3 e- from p-shell).

Daniel Martinez 1k

Since we covered both quantum and chemical bonds this week, it is fine to turn in hw that includes Quantum.

Daniel Martinez 1k

Can someone explain to me as to why 1E.7 letter B is not considered the ground state electron configuration for N. Thank you. :)

Daniel Martinez 1k

Daniel Martinez 1k

If you're eligible, I would suggest joining AAP and attending the peer learning sessions. Really helpful!

Daniel Martinez 1k

Yes, the Rydberg constant is specific to H atoms.

Daniel Martinez 1k

Yes. You have to convert keV to J before starting the problem.

Daniel Martinez 1k

"How many orbitals can have the following quantum numbers in an atom:(a)n=2,l=1;(b)n=4,l=2,ml=-2; (c)n=2;(d)n=3,l=2,ml=+1?"

Can someone help me with this question? Thank you.

Daniel Martinez 1k

From my understanding, photons show wave-particle duality, meaning that they exhibit properties of being a particle and a wave (frequency, amplitude, wavelength, etc).

Daniel Martinez 1k

Here are the rules for sig figs: 1. Non zero digits are significant. 2. Zeros in between other digits are significant. 3. Leading zeros are NOT significant. 4. Trailing decimal zeros are significant. 5. When adding/subtracting, use the fewest number of decimal places. 6. When multiplying/dividing, u...

Daniel Martinez 1k

First, you would need to calculate the molar mass of C7H15NO3. After that, you have to find the molar masses of each element of that molecule. One needs to divide the molar masses of each element by the total molar mass of C7H15NO3 and multiply by 100% to find the mass percentage compositions.

Daniel Martinez 1k

I did not read anything regarding us having to use a pen or pencil on hw problems. However, remember to use a pen when it comes to the exams! :)

Daniel Martinez 1k

A lot of graphing calculators these days are programmable and could contain features that may give others an unfair advantage when it comes to the test. By using a scientific calculator, it ensures that every one has an equal chance.

Daniel Martinez 1k

Does anyone know how to finish this problem after balancing the equations? Thank you!

Daniel Martinez 1k

Can someone help me with this question? I've tried it multiple times and can't seem to get the right answer. Thanks in advance!

Daniel Martinez 1k

Question F3 part A asks "(a) Write the formula for nitric acid." Is this a formula that we are already supposed to know? If not, how does one know the formula without actually calculating the empirical/molecular formulas?

Daniel Martinez 1k

The scientific calculators that you are able to use in this class must not be able to graph or be able to be programmed. I paid $15 for mine, so I assume that anywhere from $10-$15 is a reasonable price for a calculator.

Daniel Martinez 1k

Avogadro's number is 6.0221 x 10^23. It is used to find the number of atoms, molecules, or ions in a mole of any substance.

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