CHEMISTRY COMMUNITY

Andrea_1H

How can you tell which acids and bases are polyproptic? Are there any common examples?

Andrea_1H

For en and EDTA are we only supposed to know that en is bidentate and EDTA is hexadentate?

Andrea_1H

Sydney Pell 3E wrote:What is the function of hemoglobin and myoglobin?

Myoglobin transports oxygen in muscle cells ( heme complex + protein -> myoglobin -> Fe binds to oxygen)

Hemoglobin transports O2 in the blood by binding 4 O2

Andrea_1H

To form a hydrogen bond, do both molecules have to have a hydrogen connected to a F, O or N?

Andrea_1H

Should we assume acids that aren’t one of the string ones are weak or should we also memorize the neutral ones?

Andrea_1H

I'm still confused on when we would use -bis, -tris, -tetrakis etc. Are there any examples of this that we'd be more likely to see on the final?

Andrea_1H

What exactly does it mean for a compound to be amphoteric and how can you figure this out?

Andrea_1H

9C.7 Which of the following isomers of diaminobenzene can form chelating complexes? Explain your reasoning.

How do you know which isomers can form chelating complexes?

Andrea_1H

9C.1 Name each of the following complex ions and identify the oxidation number of the metal: (a) [Fe(CN)6]42; (b) [Co(NH3)6]31; (c) [Co(CN)5(OH2)]22; (d) [Co(NH3)5(SO4)]1.

How would we identify the oxidation number for say a?

Andrea_1H

Why would we consider lone pairs on N or O possible hydrogen bonding sites?

Andrea_1H

Lewis acids accept electron pairs, meanwhile Bronsted acids donate proton.

Andrea_1H

What did Dr. Lavelle say cisplatin does to normal, healthy cells?

Andrea_1H

Why is HCl a stronger acid than HF?

Andrea_1H

How do chelating ligands work?

Andrea_1H

How do you determine hybrid orbitals ?

Andrea_1H

Why do bigger atoms have stronger intermolecular forces?

Andrea_1H

When do dipole-induced dipoles occur? Any examples?

Andrea_1H

In Friday's lecture, what did Lavelle mean when he said that one of the equatorial (?) positions is where we place the lone pairs? What does that mean, and what does that do in terms of the electrons and the bond angles?

Andrea_1H

Why is CH2Cl2 polar and not non polar like other tetrahedrals?

Andrea_1H

What's the difference between trigonal pyramidal and t-shape? For example, why is BrF3 t-shape and NH3 trigonal pyramidal?

Andrea_1H

What is a coordinate covalent bond? How are they different from a covalent bond?

Andrea_1H

So can dipole moments be temporary or all they all permanent?

Andrea_1H

Why are double bonds stronger than single bonds?

Andrea_1H

What exactly is a dipole moment?

Andrea_1H

Why is it that larger atoms have higher polarizability?

Andrea_1H

What’s the difference between polarizability and polarizing power? And how exactly can you tell who unions have higher polarizing power?

Andrea_1H

Why are shorter bond lengths stronger than longer bond lengths?

Andrea_1H

What if we can’t get all the atoms to have a formal charge of 0? Is there a “second best” option?

Andrea_1H

how do we draw dipole moments on Lewis structures?

Andrea_1H

How do you predict bond lengths? I know Dr. Lavelle showed us an example in lecture, but I’m still confused as to how you’d figure that out.

Andrea_1H

Is there a difference between electronegativity and electron affinity?

Andrea_1H

Why are Chromium and Copper exceptions to the Aufbau principle?

Andrea_1H

1E.23. The elements Ga, Ge, As, Se, and Br lie in the same period in the periodic table. Write the electron configuration expected for the ground-state atoms of these elements and predict how many unpaired electrons, if any, each atom has. How exactly do you know how many unpaired electrons an atom ...

Andrea_1H

Is there a specific reason we fill the 4s-orbital before the 3d-orbital when doing the electron configurations? And does that mean when we’re taking electrons away, we take them from 4s first?

Andrea_1H

How can you tell which atom has the lowest ionization energy when constructing a Lewis structure? Or just in general?

Andrea_1H

For ions, how do you know when you need to take away electrons from the configuration, and when you need to add them?

Andrea_1H

For the uncertainty value, you add up the total uncertainty right? So for example, if you have 105 m +/- 3 m, the uncertainty value is 6 m? Or is it 3?

Andrea_1H

For Rydberg's constant, we should only use the one provided in the equations and constants sheet Dr. Lavelle has on his website, right? And we should stick to E= $-\frac{hR}{n^2}$ rather than Rydberg's equation?

Andrea_1H

Why is $\Psi _{2,0,0}$ not possible? I did not understand Dr. Lavelle's explanation in lecture.

Andrea_1H

How do we know when a line is in either the Lyman Series or the Balmer series? I'm still confused as to how you can tell.

Andrea_1H

Dr. Lavelle's explanation of this towards the end of Friday's lecture confused me. Can someone explain what he meant when he showed the two diagrams ("Allowed Energy Level" vs "Not allowed") and why the Allowed Energy Level diagram is the correct one when talking about electrons?

Andrea_1H

What did Dr. Lavelle say was the minimum wavelike properties that could be detected?

Andrea_1H

Will it be enough to just memorize that 400nm-700nm is visible light, and anything less than 400nm is UV, and anything above 700nm is infrared? Can we just assume we don't have to worry about the other ones (e.g., x-rays, microwaves, etc.) right now?

Andrea_1H

Is there a reason that the distance between n=1 and n=2 is greater than say n=2 and n=3?

Andrea_1H

What is the difference between constructive interference and destructive interference?

Andrea_1H

I'm still unclear as to when zeros are counted in the number of sig figs and when they aren't. Why does 1.00 have 3, but 0.01 only have 1? Can someone explain the difference?

Andrea_1H

You could use this formula in a question like: If you dilute 300. mL of a 4.00 M solution of CuCl_{2} to 900. mL, what is the new concentration of the solution? (from a step-up session) First, you'd use your given to figure out what parts of the equation you already have and then just plugging it in...

Andrea_1H

It depends on the problem, I think. You should look at what is given in each problem and then use the lowest number of sig figs.

Andrea_1H

I'm unclear as to why in the solution it goes $(\frac{1 mol Fe_{3}Br_{8}}{8 mol NaBr}) \times (\frac{3 mol FeBr_{2}}{1 mol Fe_{3}Br_{8} })...$
More specifically, why do we multiply those two together?

Andrea_1H

The Law of Conservation of Mass makes sense to me, but in lecture the example used was 2Na(s) + 2H_{2}O(l) \rightarrow 2NaOH(aq) +H_{2}(g) and he put that it's basically 2 moles of sodium + 2 moles of water = 2 moles of NaOH + 1 mole of hydrogen. Does there not have t...

Search found 50 matches