Search found 30 matches
Search found 30 matches • Page 1 of 1
- Thu Dec 06, 2018 8:50 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: PKa and Pkb vs Ka and Kb
- Replies: 4
- Views: 589
Hi, just want to ask that will this be on the final? Thank you!
- Thu Dec 06, 2018 8:48 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Ka&Final
- Replies: 1
- Views: 98
Hi, do we need to know the concept of Ka for the final?
- Mon Dec 03, 2018 9:22 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands and Lewis bases
- Replies: 3
- Views: 126
A ligand is a type of Lewis base since the definition of a Lewis base is an electron donor. But the definition of ligand is an ion or molecule bound to the central atom to form a coordination complex. So they are not interchangeable.
- Wed Nov 28, 2018 12:07 am
- Forum: Lewis Acids & Bases
- Topic: Difference Between Acids and Bases
- Replies: 4
- Views: 141
You can also tell by whether it has H+ or OH-. However, it's actually the same thing, since H+ attracts electrons and OH- repels electrons. You can interpret repelling electrons as "giving" electrons out; attracting electrons as receiving electrons.
- Fri Nov 16, 2018 10:31 am
- Forum: *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids)
- Topic: Shape and Boiling Point
- Replies: 12
- Views: 843
You can think of it this way: the higher boiling point, the harder it is to separate between molecules. Therefore, a stronger intermolecular force results in a higher boiling point.
- Fri Nov 16, 2018 10:25 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Repulsion Strength
- Replies: 5
- Views: 125
Because electrons are all negatively charged, they repel each other. Since the lone pairs are closer to the nucleus, their domain is smaller (more tightly bounded to the nucleus), which will result in a greater repulsion. For electrons in the bonds, there is a larger domain for them since they are f...
- Fri Nov 09, 2018 11:03 am
- Forum: Electronegativity
- Topic: Electronegativity relationship with Polarizability
- Replies: 3
- Views: 181
I think electronegativity is the ability of drawing the shared electrons towards itself. Polarizability is the ability to form instant dipoles. Electonegativity increase across a row and decrease down a group. This is because, in the same row, the right atoms need more electrons to achieve the most ...
- Wed Oct 31, 2018 1:11 pm
- Forum: Coordinate Covalent Bonds
- Topic: bound atoms vs separate atoms
- Replies: 5
- Views: 361
I think you can think the problem in this way, with the forming of chemical bonds, more electrons are fixed instead of moving freely. So there will be a decrease in energy for a bound atom compared to the separate ones.
- Wed Oct 31, 2018 1:07 pm
- Forum: Bond Lengths & Energies
- Topic: Bond length Correlation
- Replies: 2
- Views: 160
Generally the shorter the bond length, the stronger the bond will be. I think it might be because that if the bond is shorter, the two atoms should be closer. Therefore, more energy is required to break this kind of bonds.
- Fri Oct 26, 2018 3:48 pm
- Forum: Trends in The Periodic Table
- Topic: Removing 2nd Electron
- Replies: 9
- Views: 212
I think you can try to think it this way: the electron on the outer shells are generally less stable than those on the more inside shells, because the inner electrons are closer to the protons so that there is stronger electromagnetic attraction. Removing a second electron is to remove one inner ele...
- Tue Oct 09, 2018 8:27 pm
- Forum: Significant Figures
- Topic: All students read this sig fig post [ENDORSED]
- Replies: 116
- Views: 11210
I heard of a rule about keeping different numbers of sig figs depends on doing multiplication or addition. Does someone know about this rule and maybe help me clarify it? Thank you!
- Tue Oct 02, 2018 10:32 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Advice from a Medical Student [ENDORSED]
- Replies: 154
- Views: 86058
Thank you so much for your useful advice! I think I would try my best to master this course!