Search found 37 matches
- Mon Dec 03, 2018 11:51 am
- Forum: Administrative Questions and Class Announcements
- Topic: DOWNLOAD SESSION WORKSHEETS HERE - Sundays 4-6pm (Karen) [ENDORSED]
- Replies: 135
- Views: 38698
Re: DOWNLOAD SESSION WORKSHEETS HERE - Sundays 4-6pm (Karen) [ENDORSED]
Hi, are you going to post a final review packet? Thanks!
- Sat Dec 01, 2018 3:05 pm
- Forum: Naming
- Topic: New IUPAC Name Convention - coordinate compounds
- Replies: 1
- Views: 245
New IUPAC Name Convention - coordinate compounds
In the chart that Professor Lavelle posted on the class website it has the New IUPAC Name Convention, are we going to need to know those for the final?
Re: Ligand
Yes we are supposed to know the names of ligands, here is a link to a quizlet thank could be helpful: https://quizlet.com/_5pyzad
- Sat Dec 01, 2018 2:41 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: oxidation numbers for ligands
- Replies: 2
- Views: 392
oxidation numbers for ligands
I am confused as to how you calculate the oxidation number for ligands in a coordinate compound? If someone could give an example that would be greatly appreciated!
- Sat Dec 01, 2018 2:39 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Final Exam
- Replies: 22
- Views: 1597
Re: Final Exam
It is cumulative and in lecture, Professor Lavelle said that each unit will be equally on the final! It is only 8 questions so basically 1 or 2 questions per concept.
- Sat Dec 01, 2018 2:38 pm
- Forum: Lewis Acids & Bases
- Topic: lewis acid and bases
- Replies: 3
- Views: 361
lewis acid and bases
Does the structure of an atom have anything to do with whether it is a lewis acid or base?
- Mon Nov 26, 2018 1:07 pm
- Forum: Hybridization
- Topic: Hybridization
- Replies: 2
- Views: 316
Hybridization
Are we going to have to draw out the hybridization of an atom for the test?
- Mon Nov 26, 2018 1:06 pm
- Forum: Hybridization
- Topic: When to hybridized?
- Replies: 6
- Views: 493
Re: When to hybridized?
You can find the hybridization of an atom by finding the number of bonding regions plus the number of lone pairs around the central atom (steric number). If the steric number is 4, the atom is s p 3 hybridized. If the steric number is 3, the atom is s p 2 hybridized.
- Sat Nov 24, 2018 3:41 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond angles
- Replies: 2
- Views: 261
Bond angles
I am confused as to how you determine whether an angle is less than 109.5 degrees? Could someone give me an example?
- Sat Nov 24, 2018 11:56 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent - Lone Pairs
- Replies: 8
- Views: 941
Re: Bent - Lone Pairs
Yes, the molecular geometry for both would be bent. However, they would have different electron geometries.
- Sat Nov 24, 2018 11:55 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Does formal charge apply to the VSEPR Model?
- Replies: 6
- Views: 1759
Re: Does formal charge apply to the VSEPR Model?
Yes, when you use the vsepr model you need to be using the most stable Lewis structure to determine the number of lone pairs. So, you need to find the formal charges for the atoms in order determine the electron geometry.
- Sat Nov 24, 2018 11:53 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polarity
- Replies: 7
- Views: 748
Re: Polarity
Dipole moments only occur in polar molecules when there is a difference in electronegativity. If you draw the arrows on the Lewis structure there will be a dipole moment when the arrows do not cancel out, meaning they are not pointing is opposite directions basically.
- Sat Nov 24, 2018 11:51 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond length
- Replies: 2
- Views: 318
Bond length
Will we have to do actual calculations to determine bond length?
- Sat Nov 24, 2018 11:50 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: vsepr model
- Replies: 3
- Views: 432
vsepr model
Can someone explain to me the difference between the electron geometry and the molecular geometry for the VSEPR model?
- Sat Nov 24, 2018 11:44 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: vsepr shape
- Replies: 6
- Views: 674
Re: vsepr shape
I made a chart for the VSEPR model that shows each lewis structure and the particular shape, angle and # of lone pairs that it corresponds to. I would just memorize some of them, it makes it easier to identify atoms.
- Fri Nov 16, 2018 9:36 am
- Forum: Electronegativity
- Topic: Electronegativity
- Replies: 8
- Views: 864
Re: Electronegativity
In the periodic table electronegativity generally follows the trend of increasing left to right. However, this trend does not include the noble gases and fluorine has the highest electronegativity instead of Ne or He.
- Fri Nov 16, 2018 9:28 am
- Forum: Octet Exceptions
- Topic: Octet vs formal charge
- Replies: 16
- Views: 3077
Re: Octet vs formal charge
I would say that finding the lowest possible formal charge to create the most stable Lewis structure is more important because there are various exceptions to the octet rule so you cannot always base where a structure is correct if each atom has a full octet.
- Fri Nov 16, 2018 9:26 am
- Forum: Dipole Moments
- Topic: Induced-dipole
- Replies: 5
- Views: 1824
Re: Induced-dipole
An induced dipole is an attraction that occurs when a polar molecule induces a dipole in an atom or in a nonpolar molecule by changing the arrangement of electrons in the nonpolar species. For example, with HCl and Argon, the electrons on an argon atom are distributed around the nucleus of the atom....
- Tue Nov 13, 2018 1:16 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Determining VSEPR bond angles
- Replies: 5
- Views: 1835
Re: Determining VSEPR bond angles
For the SOCl2 the oxygen atom and two chlorine atoms are both singularly bonded to sulfur. Also, sulfur has a lone pair. So, because there are four regions of electron density with one lone pair, then the shape would be trigonal pyramidal. In part b, all of the OSCL angles would be the same because ...
- Mon Nov 12, 2018 2:22 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Cations and polarizing power
- Replies: 3
- Views: 260
Re: Cations and polarizing power
What I have gathered is that the smaller the size of a the cation the greater its polarizing power and the greater the covalent bond will be. So, as the charge on the ion increases, the electrostatic attraction of the cation for the outer electrons of the anion also increases and then it will be abl...
- Mon Nov 12, 2018 2:17 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 4
- Views: 464
Re: Bond Angles
Yes, the angles depend on the structure of the molecule so for example Trigonal Planar has 0 lone pairs and is 120 degrees, Tetrahedral also has zero lone pairs and is 109.5 degrees and a T - shape has 2 lone pairs and is 90 degrees. Hope this helps!
- Mon Nov 12, 2018 10:17 am
- Forum: Administrative Questions and Class Announcements
- Topic: Test 3 dates?
- Replies: 11
- Views: 1265
Re: Test 3 dates?
Test 3 starts on November 27th in discussion sections so it doesn't affect Thanksgiving break.
- Mon Nov 12, 2018 10:15 am
- Forum: SI Units, Unit Conversions
- Topic: Kiloelectron volt to Joule
- Replies: 5
- Views: 973
Re: Kiloelectron volt to Joule
The conversion factor is 1.602 x 10^19 joule = 1 electron volt.
- Mon Nov 12, 2018 10:14 am
- Forum: Ionic & Covalent Bonds
- Topic: Polarizability vs Polarizing Power
- Replies: 2
- Views: 294
Re: Polarizability vs Polarizing Power
Polarizability is the ability for a molecule to be polarized (have its electron cloud distorted by the pull of the smaller atom, and it increases as the volume occupied by electrons increases. Whereas polarization power is the ability of a cation to distort an anion. If the degree of polarization is...
- Mon Nov 12, 2018 12:12 am
- Forum: Ionic & Covalent Bonds
- Topic: Covalent bond dissociation energy
- Replies: 1
- Views: 247
Re: Covalent bond dissociation energy
Lone pair electrons are related to the strengths of bonds because electrons naturally repel each other, when they’re located on neighboring atoms they will create a repulsion that weakens the bond. So, as the number of lone pairs on neighboring atoms increases, the dissociation energy decreases.
- Mon Nov 12, 2018 12:06 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Calculating Dissociation Energy
- Replies: 3
- Views: 263
Re: Calculating Dissociation Energy
Bond dissociation energy is similar to Bond energy, as both are different terms. Bond dissociation energy one is the measure of the strength of the bond where as bond energy is the total energy contained in a chemical bond.
- Sun Nov 11, 2018 11:59 pm
- Forum: Dipole Moments
- Topic: Hydrogen Bonds
- Replies: 20
- Views: 1470
Re: Hydrogen Bonds
It's a type of weak chemical bond that occurs when the partially positive hydrogen atom participating in a polar covalent bond in a molecule attracts partially negative atom or atoms of neighboring molecules.
- Sun Nov 11, 2018 5:01 pm
- Forum: Lewis Structures
- Topic: Formal charges
- Replies: 15
- Views: 1234
Re: Formal charges
If they are asking for the most stable Lewis structure then the formal charges are necessary but just to be safe I would put them.
- Sun Nov 11, 2018 4:59 pm
- Forum: Lewis Structures
- Topic: Lewis Structure
- Replies: 10
- Views: 829
Re: Lewis Structure
You have to make sure that the elements symmetrically spaced, that the element with the lowest ionization energy is in the middle and that the formal charges are the lowest to make the most stable structure.
- Sun Nov 11, 2018 4:46 pm
- Forum: Octet Exceptions
- Topic: Number of electrons in relation to Octet
- Replies: 3
- Views: 338
Re: Number of electrons in relation to Octet
There are many elements that are exceptions to the octect rule, like all of the third period elements can have expanded octets like CL and Br. The octect rule also doesn’t apply when there are odd valence electrons but the elements cannot share electrons between each other.
- Sat Nov 03, 2018 6:51 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Degeneracy
- Replies: 8
- Views: 1366
Re: Degeneracy
Degenerate orbitals have the same energy levels. The degeneracy of orbitals is basically when they have the same values of n but different values of l. Hope this helps!
- Sat Nov 03, 2018 6:44 pm
- Forum: Lewis Structures
- Topic: Lewis Acids and Bases
- Replies: 5
- Views: 377
Re: Lewis Acids and Bases
Lewis Acids are electron pair acceptor and bases are electron pair donors.
- Sat Nov 03, 2018 6:40 pm
- Forum: Trends in The Periodic Table
- Topic: Effective Nuclear Charge
- Replies: 5
- Views: 518
Re: Effective Nuclear Charge
Effective nuclear charge increases across the period and decreases going down a group.
- Sun Oct 21, 2018 2:46 pm
- Forum: Photoelectric Effect
- Topic: Kinetic energy
- Replies: 4
- Views: 321
Kinetic energy
Will the work function always be given to us when solving a problem are will there be a scenario where we will have to find it ourselves?
- Thu Oct 11, 2018 11:25 am
- Forum: Limiting Reactant Calculations
- Topic: How to determine the limiting reactant???? [ENDORSED]
- Replies: 8
- Views: 11007
Re: How to determine the limiting reactant???? [ENDORSED]
If you're having trouble, I would recommend watching this video https://www.youtube.com/watch?v=Mlu_v8rE1TY. It explains the process very clearly, and lets you see the organization of a limiting reactant problem! Hope that helps!
- Wed Oct 10, 2018 8:39 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Meaning of Quanta/Quantized
- Replies: 2
- Views: 329
Re: Meaning of Quanta/Quantized
I am pretty sure that an electron is quantized when electrons are emitted from a metal's surface when light of a certain frequency shines on it, releasing a photon.
- Wed Oct 10, 2018 8:34 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Threshold Energy
- Replies: 4
- Views: 295
Re: Threshold Energy
The threshold energy is basically the minimum kinetic energy required to remove an electron. Also, the energy of photoelectrons emitted when light hits a metal depends on the frequency. When light with the right frequency is shone onto a metal surface, electrons are emitted from the surface.