Search found 36 matches
Search found 36 matches • Page 1 of 1
- Sun Nov 17, 2019 5:27 pm
- Forum: Bond Lengths & Energies
- Topic: Strongest Bonds
- Replies: 11
- Views: 274
The order from strongest bonds to least strong bonds are ion-ion, ion-dipole, dipole-dipole (which include H-bonding), induced dipole-dipole, and induced-dipole induced-dipole (van der waals/london dispersion forces).
I don't think that the atoms with an expanded octet necessarily have to have 10 electrons. However, you should always make sure that your lewis structure with the atom with an expanded octet has the same amount of electrons as the amount you calculated prior.
- Sun Nov 03, 2019 11:52 pm
- Forum: Resonance Structures
- Topic: Resonance structures
- Replies: 6
- Views: 127
It is basically many different lewis structures drawn for the same molecule, in which the double bonds differ. However, the total charge for all the resonance structures should be the same.
The main way to tell is if the molecule is asymmetric. You should take the formal charges and draw the S+ and S- accordingly on the atoms. Also, draw arrows to the most electronegative atoms.
- Sun Nov 03, 2019 11:44 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent
- Replies: 14
- Views: 172
A main distinction between covalent and ionic bonds are that ionic bonds are between a metal and nonmetal. Covalent bonds are between two nonmetals. Additionally, the EN difference for ionic bonds are greater than 2.5 and lower than 1.5 for covalent bonds.
- Sun Oct 27, 2019 11:46 pm
- Forum: Electronegativity
- Topic: Trend of Electronegativity
- Replies: 18
- Views: 2855
chrisavalos-2L wrote:I was wondering what the trend for electronegativity was, is it the same as ionization energy?
I remember my TA mentioning that it is okay to view them as having the same trends.
Katherine Chhen 3I wrote:For a compound, would the best way to represent it in Lewis structures is to draw out every structure and use double headed arrows?
You have to draw all of the possible Lewis structures and then figure out which one has the formal charge closest to zero.
- Sun Oct 27, 2019 11:40 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge
- Replies: 7
- Views: 99
The resonance structure with the lowest formal change is the most stable. I thought the structure with its formal charge = 0 or closest to 0 was the most stable? You are correct. The structure with the formal charge closest to zero is most stable since that would result in it having no charge of th...
Jorge Ramirez_4H wrote:Is electronegativity important when doing electron configurations?
For electron configurations, you don't really need to know about how electronegative the atom is. It may be more beneficial to know about where it lies in the periodic table in terms of the s,p, and d blocks.
Electronegativity is the ability of an atom to attract a shared pair of electrons. The electronegativity increases as it goes along a period because the atomic number increases, thus increasing the number of protons. The protons make the atom more positive, making it more attracted to electrons.
If the total energy of the photon was equal to the work function, and the kinetic energy was zero, then is the electron ejected? How can the electron be ejected if there is no kinetic energy?
- Sun Oct 13, 2019 7:55 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Atomic Spectra
- Replies: 5
- Views: 54
Each atom absorbs and emits its own specific amount of energy or quanta. The amount absorbed always equals the amount emitted. However, black bodies can absorb all frequencies.
- Sun Oct 13, 2019 7:47 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect and Photons
- Replies: 6
- Views: 57
The professor stated that if the energy per photon is greater or equal to the energy needed to remove an electron only then would the increase in light intensity result in more elected e-s. What exactly does this mean?
- Sun Oct 06, 2019 6:35 pm
- Forum: Limiting Reactant Calculations
- Topic: Two Limiting Reactants
- Replies: 5
- Views: 4451
It is highly unlikely that two reagents would be at the molar specific ratio to be both the limiting reagents. So there are almost never two limiting reactants.