Search found 45 matches
- Mon Dec 02, 2019 2:40 am
- Forum: Conjugate Acids & Bases
- Topic: Conjugate acids and bases with lewis/bronsted acids
- Replies: 3
- Views: 73
Re: Conjugate acids and bases with lewis/bronsted acids
An acid is generally specific to its conjugate base, and a base is specific to its conjugate acid. Whether it is a Lewis or Bronsted base won't change what conjugate it forms.
- Mon Dec 02, 2019 2:39 am
- Forum: Conjugate Acids & Bases
- Topic: Product of Acid and Base
- Replies: 5
- Views: 97
Re: Product of Acid and Base
In a reaction with acid containing hydrogen and a base containing hydroxide, the two will neutralize each other and give off their ions, meaning the H+ and OH- ions can now combine into H2O. The remaining ions can combine into a salt.
- Mon Dec 02, 2019 2:35 am
- Forum: Conjugate Acids & Bases
- Topic: Conjugate/Bronsted/Lewis
- Replies: 2
- Views: 66
Re: Conjugate/Bronsted/Lewis
Lewis and Bronsted definitions have been explained above already, but just know that a conjugate base occurs when an acid donates an H+ and thus the product is now able to accept an H+ back in the reverse reaction.
- Mon Dec 02, 2019 2:33 am
- Forum: Conjugate Acids & Bases
- Topic: Ligands
- Replies: 12
- Views: 160
Re: Ligands
Ligands are found in coordination compounds, meaning they donate an electron pair to a central atom.
- Mon Dec 02, 2019 2:33 am
- Forum: Conjugate Acids & Bases
- Topic: Conjugate Acids and Bases
- Replies: 4
- Views: 95
Re: Conjugate Acids and Bases
Conjugate acids and bases can arise in reversible reactions. For example, an acid donates an H+ to another molecule, and then turns into a product with one less H+. This is now a conjugate base, because in the reverse reaction, it can accept an H+.
- Mon Nov 25, 2019 4:02 am
- Forum: Coordinate Covalent Bonds
- Topic: Electronegativity
- Replies: 12
- Views: 1069
Re: Electronegativity
There are just certain periodic trends to know. In basic terms, electronegativity is mainly reliant on an atom's positive charge and the "shielding" of electrons. N is more electronegative than C because it has one more proton, allowing it to attract electrons more tightly. F is more elect...
- Mon Nov 25, 2019 3:58 am
- Forum: Coordinate Covalent Bonds
- Topic: coordinate covalent bond
- Replies: 7
- Views: 574
Re: coordinate covalent bond
Some atoms can't complete their octet unless another atom donates a whole electron pair (2 electrons instead of 1). This is known as a coordinate covalent bond.
- Mon Nov 25, 2019 3:57 am
- Forum: Coordinate Covalent Bonds
- Topic: carbon monoxide formal charges
- Replies: 5
- Views: 215
Re: carbon monoxide formal charges
Simple formal charge calculations. The carbon atom, for example, has 4 valence electrons, but if you take the electrons in a CO molecule (2 lone electrons and 3 bonded electron pairs) you will get 4 - 5 = -1 formal charge.
- Mon Nov 25, 2019 3:55 am
- Forum: Coordinate Covalent Bonds
- Topic: Coordinate Covalent Bonds
- Replies: 5
- Views: 269
Re: Coordinate Covalent Bonds
Coordinate covalent bonds allow certain atoms to complete the octet. Boron, a big example, needs to accept a whole lone pair from another atom to complete its octet.
- Mon Nov 25, 2019 3:53 am
- Forum: Coordinate Covalent Bonds
- Topic: Covalent character: BeCl2 Vs MgCl2
- Replies: 4
- Views: 1565
Re: Covalent character: BeCl2 Vs MgCl2
BeCl2. As stated, the molecule with smaller electronegativity difference has more covalent character. A larger difference becomes more ionic.
- Fri Nov 22, 2019 12:42 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Specific Naming Question
- Replies: 4
- Views: 116
Re: Specific Naming Question
The electron geometry is considering all areas of electron density. Because this molecule has 5 such areas, it would be a trigonal bipyramidal shape. However, because one of the areas is a lone pair, the actual shape is a see-saw
- Fri Nov 22, 2019 12:38 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Week 8 homework
- Replies: 2
- Views: 90
Re: Week 8 homework
Should be fine, it makes sense to do homework on whatever you studied.
- Fri Nov 22, 2019 12:36 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Removing Non-Axis Atoms First
- Replies: 4
- Views: 129
Re: Removing Non-Axis Atoms First
The goal of the VSEPR model is showing how each region of electron density repels others. You do not always remove non-axis electrons first, it depends on whatever creates the farthest distance between each electron density region.
- Fri Nov 22, 2019 12:33 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: NO Shape and Polarity
- Replies: 4
- Views: 105
Re: NO Shape and Polarity
Diatomic molecules like NO are always linear, as there's only one way to connect them. But this molecule is indeed polar because of the electronegativity difference between N and O.
- Fri Nov 22, 2019 12:31 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Shape of Diatomic Molecules
- Replies: 5
- Views: 85
Re: Shape of Diatomic Molecules
The shape is always linear, just make sure not to confuse it with polarity. Diatomic molecules are not always nonpolar.
- Sun Nov 17, 2019 6:46 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR Angles
- Replies: 4
- Views: 99
Re: VSEPR Angles
Atomic radius only affects bond length. For VSEPR, you don't need to worry about atomic radius, just look at the areas of electron density.
- Sun Nov 17, 2019 6:44 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Dipole moment
- Replies: 5
- Views: 102
Re: Dipole moment
Dipole moment is just a term to describe attraction between molecules. Atoms in a molecule like H2O are unequal in electronegativity; the O atom pulls electrons more strongly, obtaining a partial negative charge, while the H atoms become partially positive. This creates a dipole.
- Sun Nov 17, 2019 6:35 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: single, double, and triple bonds
- Replies: 6
- Views: 122
Re: single, double, and triple bonds
Whether the bond is single, double, or triple, it is still grouped as one area of electron density, so it can be treated the same as a different type of bond.
- Sun Nov 17, 2019 6:33 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Prediction of Angles
- Replies: 4
- Views: 81
Re: Prediction of Angles
There are resources and charts to show the bond angles of specific shapes. The angles themselves though are determined by the areas of electron density repelling each other.
- Sun Nov 17, 2019 6:30 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR
- Replies: 3
- Views: 98
Re: VSEPR
The basis of VSEPR is that areas of electron density repel each other and try to get as far from each other as possible. This repulsion determines the shape of the molecule and how the atoms are positioned.
- Fri Nov 08, 2019 4:35 am
- Forum: Electronegativity
- Topic: Website
- Replies: 3
- Views: 142
Re: Website
You probably already tried, but just make sure you use LL14A19, which is the password he gave us.
- Fri Nov 08, 2019 4:33 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Which lewis structure will make the dominant contribution to a resonance hybrid?
- Replies: 5
- Views: 115
Re: Which lewis structure will make the dominant contribution to a resonance hybrid?
If there can be a resonance structure with no formal charges on any atoms, that will be the most stable structure. However, if this is not possible, you would indeed place the charge on the more electronegative atom.
- Fri Nov 08, 2019 4:31 am
- Forum: Resonance Structures
- Topic: Drawing the resonance hybrid
- Replies: 2
- Views: 82
Re: Drawing the resonance hybrid
The exam already passed but for future reference, it's good to draw the different resonance structures. Usually the question will ask for this.
- Fri Nov 08, 2019 4:27 am
- Forum: Lewis Structures
- Topic: Midterm grades
- Replies: 26
- Views: 547
Re: Midterm grades
Like the above post says, probably about a week. It mostly depends on how fast the TA's will grade the tests.
- Fri Nov 08, 2019 4:26 am
- Forum: Octet Exceptions
- Topic: radicals
- Replies: 3
- Views: 115
Re: radicals
One tip is that in most examples I've seen, the central atom will NOT have the single electron. This is not the specific rule, but we've learned that the central atom is least electronegative, so that one will not pull electrons as strongly as the outer, more electronegative atoms.
- Sun Nov 03, 2019 7:19 am
- Forum: Lewis Structures
- Topic: Ion formation vs molecule
- Replies: 2
- Views: 43
Re: Ion formation vs molecule
The lowest energy is basically just a way of saying which bond is likely to form. NaCl, for example has a large electronegativity difference between Na and Cl, making it ionic.
- Sun Nov 03, 2019 7:16 am
- Forum: Resonance Structures
- Topic: resonance hybrid vs resonance structure
- Replies: 2
- Views: 41
Re: resonance hybrid vs resonance structure
Resonance hybrid is how a molecule actually appears, when all the possible resonance structures are blended together.
- Sun Nov 03, 2019 7:14 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge vs Actual Charge
- Replies: 2
- Views: 53
Re: Formal Charge vs Actual Charge
Yes, like the above student said, the numbers should add up to the charge of the actual molecule, showing that it is indeed the most favorable model.
- Sun Nov 03, 2019 7:12 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charges
- Replies: 3
- Views: 47
Re: Formal Charges
The textbook includes formal charge numbers just to show which resonance structures would be more favorable, but it isn't required unless asked.
- Sun Nov 03, 2019 7:10 am
- Forum: Lewis Structures
- Topic: Delocalized Electrons
- Replies: 4
- Views: 36
Re: Delocalized Electrons
The position of double bonds can change between resonance structures, because the electrons are not in a specific place but rather scattered around the atom. This is why they are called "delocalized."
- Mon Oct 28, 2019 3:04 am
- Forum: Lewis Structures
- Topic: Orbitals
- Replies: 9
- Views: 149
Re: Orbitals
Yes, it might be confusing because 3d comes before it and d is higher energy, but you can just think of the highest shell (n = ...) as the outer layer to take electrons from.
- Mon Oct 28, 2019 3:02 am
- Forum: Electronegativity
- Topic: Fluorine's Electronegativity
- Replies: 6
- Views: 146
Re: Fluorine's Electronegativity
Fluorine only has electrons in the n=2 shell, meaning there are no higher layers to "shield" the positive charge from attracting electrons. It also has the highest number of protons in its period, making the nucleus attract electrons very strongly.
- Mon Oct 28, 2019 2:59 am
- Forum: Electronegativity
- Topic: Electronegativity in Covalent Bonds
- Replies: 3
- Views: 49
Re: Electronegativity in Covalent Bonds
Yes, but if you are referring to the electronegativity difference between two atoms, you can just know that ionic bonds happen when the electronegativity difference is greater than 1.6.
- Mon Oct 28, 2019 2:57 am
- Forum: Ionic & Covalent Bonds
- Topic: periodic table
- Replies: 10
- Views: 131
Re: periodic table
Kennedi3K wrote:Is this the same for ionization energy?
Yes, if electronegativity increases, the nucleus attracts electrons more strongly, meaning the electrons are also harder to remove.
- Mon Oct 28, 2019 2:55 am
- Forum: Ionic & Covalent Bonds
- Topic: Mnemonics for the period table trends
- Replies: 3
- Views: 72
Re: Mnemonics for the period table trends
I don't know any mnemonics, but I can try to help. If we're just talking about electron affinity, ionization energy, and atomic radius, you can just remember one: that atomic radius increases as you go to the left and downwards. The other 2 trends are just the opposite (IE and electron affinity incr...
- Sun Oct 20, 2019 2:25 am
- Forum: Trends in The Periodic Table
- Topic: calculating the state
- Replies: 3
- Views: 59
Re: calculating the state
Px, Py, Pz just refers to the orientation of the P orbital, the subscript x, y, z, means that the orbital is positioned along whichever axis.
- Sun Oct 20, 2019 1:03 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Spin up and spin down
- Replies: 13
- Views: 229
Re: Spin up and spin down
I'm not sure how to tell if an electron is in up or down spin state, but just know the spin quantum number (ms) can only be -1/2 or +1/2, meaning down spin and up spin respectively.
- Sat Oct 19, 2019 3:57 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Electron Configuration
- Replies: 2
- Views: 63
Re: Electron Configuration
Yes, the quantum numbers tell you things like which subshell and orbital, using this information you can know the electron configuration.
- Sat Oct 19, 2019 3:55 pm
- Forum: Photoelectric Effect
- Topic: One photon one atom interaction
- Replies: 14
- Views: 239
Re: One photon one atom interaction
It would increase. Simply increasing the intensity (or number) of photons will not eject more electrons, but increasing the frequency will.
- Sat Oct 19, 2019 3:51 pm
- Forum: Properties of Light
- Topic: Problem 1A9. How to determine which values the reading event corresponds to?
- Replies: 4
- Views: 93
Re: Problem 1A9. How to determine which values the reading event corresponds to?
Basically looking at something is just processing visible light. Generally we know that visible light wavelengths range from about 400 to 700 nm, so 600 nm would be suitable for reading.
- Fri Oct 04, 2019 9:42 am
- Forum: Molarity, Solutions, Dilutions
- Topic: Solutions vs. Dilutions
- Replies: 4
- Views: 113
Re: Solutions vs. Dilutions
As the others have stated, the difference between solution and dilution is almost like creation and modifying. Dilution is simply using a concentrated solution to create a less concentrated one.
- Fri Oct 04, 2019 9:31 am
- Forum: Balancing Chemical Reactions
- Topic: PSA on L35 typo
- Replies: 1
- Views: 54
Re: PSA on L35 typo
Thank you for ur PSA!
- Fri Oct 04, 2019 9:27 am
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: E.15
- Replies: 4
- Views: 93
Re: E.15
You're given one thing: the molar mass of M(OH)2. We can subtract molar mass of (OH)2 from this to find the mass of M, the unknown metal. Next, the sulfide is simply the molecule after (OH)2 is replaced by a sulfur ion, becoming MS. You can just add the known mass of M to the mass of sulfur to find ...
- Fri Oct 04, 2019 9:15 am
- Forum: Significant Figures
- Topic: Lab Sig Figs
- Replies: 2
- Views: 52
Re: Lab Sig Figs
I'm not completely sure, but there can be times where a constant is given like the speed of light c (3 x 10^8). In that case, you would not have to take into account that the constant only has 1 sig fig, it is just given to complete calculations.
- Fri Oct 04, 2019 9:08 am
- Forum: SI Units, Unit Conversions
- Topic: Homework
- Replies: 9
- Views: 242
Re: Homework
I just wrote mine with pencil, as it wasn't really specified :)