Search found 30 matches
- Tue Jun 12, 2018 1:34 pm
- Forum: General Science Questions
- Topic: Bond angles
- Replies: 4
- Views: 851
Re: Bond angles
Something I used to help memorize is once you get the basic shapes down (ones without lone pairs), once you get to the shapes with lone pairs, the bond angles are similar but for exmaple A trigonal planar is AX3 and an angular shaped molecule is AX2E. Both have three regions of electron density. Tri...
- Tue Jun 12, 2018 1:31 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Name of Molecule
- Replies: 4
- Views: 508
Re: Name of Molecule
Lone pairs actually greatly affects the shape. For example a trigonal planar becomes a trigonal pyramidal if there is a lone pair on the central atom.
- Tue Jun 12, 2018 1:29 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3726723
Re: Post All Chemistry Jokes Here
All the good chemistry jokes...
- Sat Jun 02, 2018 4:20 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR
- Replies: 2
- Views: 331
Re: VSEPR
In terms of Lewis structures, theres no set rule. It's all conditional.
If the central atom is period 3 and below, you can stick extra lone pairs to it.
If the central atom is period 3 and below, you can stick extra lone pairs to it.
- Sat Jun 02, 2018 4:18 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR
- Replies: 2
- Views: 331
Re: VSEPR
For VESPR the format is AXE. A represents the central atom. X are the atoms bonded to the centra atom (ligands), and E represents lone pairs.
So the lone pairs for VESPR formula is on the E with a subscript number.
So the lone pairs for VESPR formula is on the E with a subscript number.
- Sat Jun 02, 2018 4:15 pm
- Forum: Hybridization
- Topic: σ vs π bond tips thread
- Replies: 5
- Views: 686
Re: σ vs π bond tips thread
Another alternative is that σ bonds can spin, and the circle shape of O resembles wheels.
- Sun May 27, 2018 6:02 pm
- Forum: Lewis Structures
- Topic: Corbon Monoxide
- Replies: 5
- Views: 874
Re: Corbon Monoxide
So in general, it's always best to fulfill the octet rule for the elements that need the full 8 even with some charge?
- Sun May 27, 2018 5:58 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Resonance
- Replies: 7
- Views: 998
Re: Resonance
Delocalization means that a shared electron pair is distributed over several pairs of atoms and cannot be identified with just one pair of atoms.
This is from the book, page 81
This is from the book, page 81
- Sun May 27, 2018 5:52 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3726723
Re: Post All Chemistry Jokes Here
If the Silver Surfer and Iron Man team up, they’d be alloys.
- Sun May 20, 2018 2:52 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizability
- Replies: 7
- Views: 689
Re: Polarizability
So generally, just to make sure.
Cations increase in polarizability as atomic radius decreases.
Anions increase in polarizability as atomic radius increases ( and less electronegative).
Normal atoms follow same rule as cations ( same trend as radius size)
Cations increase in polarizability as atomic radius decreases.
Anions increase in polarizability as atomic radius increases ( and less electronegative).
Normal atoms follow same rule as cations ( same trend as radius size)
- Sun May 20, 2018 2:49 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizability
- Replies: 7
- Views: 689
Re: Polarizability
Do anions follow the same trend or is there variability?
- Sun May 20, 2018 2:48 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizability
- Replies: 7
- Views: 689
Re: Polarizability
Is this trend the same for cations?
- Sun May 20, 2018 2:46 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizability
- Replies: 7
- Views: 689
Polarizability
Can someone please explain to me the general trend of polarization?
- Mon May 14, 2018 2:05 pm
- Forum: Lewis Structures
- Topic: Corbon Monoxide
- Replies: 5
- Views: 874
Corbon Monoxide
Can someone please explain to me the Lewis structure of carbon monoxide? Is the most stable Lewis structure for it have a charge?
- Mon May 14, 2018 2:00 pm
- Forum: Trends in The Periodic Table
- Topic: electron affinity [ENDORSED]
- Replies: 15
- Views: 2028
Re: electron affinity [ENDORSED]
Fluorine is the most electronegative
- Mon May 14, 2018 1:58 pm
- Forum: SI Units, Unit Conversions
- Topic: Units for Answer
- Replies: 10
- Views: 1198
Re: Units for Answer
I don't think they will, but it is good to show your work for credit and for the process.
- Sun May 06, 2018 1:30 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Unpaired Electrons from Electron Configurations [ENDORSED]
- Replies: 2
- Views: 1260
Re: Unpaired Electrons from Electron Configurations [ENDORSED]
First thing is to look at how many orbitals are in the last sub shell you are given. For example, the last sub shell is p. P has 3 orbitals and can hold 6 electrons. Each orbital must be filled before you can pair electrons. if it is 4p^3, then there are 3 unpaired electrons because you must spread ...
- Sun May 06, 2018 1:12 pm
- Forum: Trends in The Periodic Table
- Topic: Isoelectric Atomic Radii
- Replies: 3
- Views: 374
Re: Isoelectric Atomic Radii
Even if the atoms have the same amount of electrons, you still follow the trend for atomic radii.
- Sun Apr 29, 2018 2:14 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electrons in an Orbital [ENDORSED]
- Replies: 8
- Views: 860
Re: Electrons in an Orbital [ENDORSED]
According to Hund's rule, electrons repulse each other because they are the same charge, and while in the same subshell, they must occupy different orbitals. This means that there are two electrons in the 2p subshell and must first fill two orbitals and have parallel spins. ( two unpaired electrons )
- Sun Apr 29, 2018 2:02 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electrons in an Orbital [ENDORSED]
- Replies: 8
- Views: 860
Re: Electrons in an Orbital [ENDORSED]
Yes, when two electrons are in the same orbital they must have opposite spins. The short term for these electrons is that they are "paired".
- Sun Apr 29, 2018 1:58 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electrons in an Orbital [ENDORSED]
- Replies: 8
- Views: 860
Re: Electrons in an Orbital [ENDORSED]
An orbital can only contain up to 2 electrons. This is Pauli's exclusion principle.
- Sun Apr 22, 2018 1:04 pm
- Forum: Photoelectric Effect
- Topic: Wave vs. Particle
- Replies: 8
- Views: 682
Re: Wave vs. Particle
So basically, increasing the intensity of the light will only result in more electrons coming off of the metal if each photon already has enough energy to remove?
- Sun Apr 22, 2018 12:57 pm
- Forum: Photoelectric Effect
- Topic: Wave vs. Particle
- Replies: 8
- Views: 682
Re: Wave vs. Particle
In regards to intensity, does it vary if you are looking at increasing intensity in the wave vs. particle model?
- Sun Apr 22, 2018 12:50 pm
- Forum: Photoelectric Effect
- Topic: Wave vs. Particle
- Replies: 8
- Views: 682
Wave vs. Particle
I'm still a little confused on the differences between the wave and particle model for light. Could someone explain the differences?
- Wed Apr 11, 2018 11:06 am
- Forum: Molarity, Solutions, Dilutions
- Topic: STEPS to figuring out solutions/ molarity quesitons
- Replies: 2
- Views: 347
Re: STEPS to figuring out solutions/ molarity quesitons
To add to Nicole, many times you will need to find the amount of grams needed to make a certain amount of Molarity as well. This is easy once you find the moles and then convert by multiplying the molecular mass.
- Wed Apr 11, 2018 10:51 am
- Forum: Molarity, Solutions, Dilutions
- Topic: Ionic Concentrations
- Replies: 1
- Views: 283
Re: Ionic Concentrations
You would first find the moles of the entire molecule. Once you have that, you would find the molar ratios. For example, NaCl. If you found the moles of NaCl and need the Cl ion concentration, it is a 1:1 ratio of moles since there is 1 mol of Cl- in the compound. You would use that amount of moles ...
- Wed Apr 11, 2018 10:46 am
- Forum: SI Units, Unit Conversions
- Topic: Formula Units
- Replies: 5
- Views: 900
Re: Formula Units
Yes.
Also just to add, if you are converting a single element using Avogadro's number, you would use atoms as the unit.
Also just to add, if you are converting a single element using Avogadro's number, you would use atoms as the unit.
- Wed Apr 11, 2018 10:43 am
- Forum: SI Units, Unit Conversions
- Topic: Formula Units
- Replies: 5
- Views: 900
Re: Formula Units
In this case, alumina is a covalent bond. Covalent bonds use the unit molecules when converting using Avogadro's number.
Formula units are used when converting an ionic bond.
Formula units are used when converting an ionic bond.
- Wed Apr 11, 2018 10:34 am
- Forum: SI Units, Unit Conversions
- Topic: Formula Units
- Replies: 5
- Views: 900
Re: Formula Units
Formula units is the units used for when converting mass or moles using Avogardro's number. Formula units are used in this case because KNO3 is not a covalent compound.
- Wed Apr 11, 2018 10:25 am
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Help with homework problem section E
- Replies: 1
- Views: 380
Re: Help with homework problem section E
In part a), you had to find the moles of the entire molecule. Once you find that you know the mole ratio of the entire molecule to the amount of Cl is 1 to 2 moles since there are 2 Cl ions the the molecule. So you would take the mole you found in part a) and multiply it by 2 to get the moles of CL ...