Search found 55 matches
- Thu Dec 17, 2020 9:38 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Angular Quantum Number
- Replies: 4
- Views: 275
Re: Angular Quantum Number
it gives the number of nodes.
- Thu Dec 17, 2020 9:37 am
- Forum: Balancing Chemical Reactions
- Topic: Diatomic Molecules
- Replies: 7
- Views: 776
Re: Diatomic Molecules
they're just molecules composed of two atoms, but the acronyms others have given are really helpful.
- Thu Dec 17, 2020 9:34 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: VSEPR memorization
- Replies: 7
- Views: 499
Re: VSEPR memorization
it's better if we try to memorize them and what helped me was physically drawing them out.
- Thu Dec 17, 2020 9:32 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Memorizing shapes based on general formula?
- Replies: 5
- Views: 435
Re: Memorizing shapes based on general formula?
it is a good idea to memorize them and what helped me was physically drawing out different examples myself.
- Thu Dec 17, 2020 9:31 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Difference between electron geometry and molecular geometry
- Replies: 12
- Views: 5193
Re: Difference between electron geometry and molecular geometry
the difference is that electron geometry takes into account all regions of electron density, so lone pairs, and atoms, while molecular geometry only accounts for atoms to determine shape.
- Thu Dec 17, 2020 9:29 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular Geometry & Electron Density
- Replies: 5
- Views: 315
Re: Molecular Geometry & Electron Density
Electron geometry refers to the shape accounting regions of electron density, so lone pairs and atoms, while molecular geometry is the shape that accounts for solely atoms. During tests and like more formal you'd be using molecular geometry.
- Thu Dec 17, 2020 9:27 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Shape
- Replies: 6
- Views: 419
Re: Shape
the molecular geometry shape.
- Thu Dec 17, 2020 9:26 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 5
- Views: 413
Re: Bond Angles
I think it all depends on how many planes the molecule takes up.
- Thu Dec 17, 2020 9:25 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 4
- Views: 391
Re: Bond Angles
as previously stated, it's because the tetrahedral shape takes up more than one plane so it doesn't have to stay in the 360-degree pattern.
- Thu Dec 17, 2020 9:22 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Steric #
- Replies: 3
- Views: 279
Re: Steric #
yeah, steric numbers account for the regions of electron density.
- Thu Dec 17, 2020 9:21 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent/Angular Bond Angles
- Replies: 5
- Views: 486
Re: Bent/Angular Bond Angles
yes you're right.
- Thu Dec 17, 2020 9:20 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pairs
- Replies: 15
- Views: 634
Re: Lone Pairs
i think it depends on the number of other ligands attached to it and which shape would account for a greater space due to electron repulsion.
- Thu Dec 17, 2020 9:15 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Determining Shape
- Replies: 10
- Views: 662
Re: Determining Shape
The difference is that electron geometry determines shape based on regions of electron density, so lone pairs, and atoms, while molecular geometry only takes atoms into account when determining shape.
- Thu Dec 17, 2020 9:13 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent vs Angular
- Replies: 20
- Views: 875
Re: Bent vs Angular
bent and angular are both ways of describing that shape.
- Thu Dec 17, 2020 9:11 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond angles
- Replies: 12
- Views: 796
Re: Bond angles
205323697 wrote:By how much would an angle go up or down if we added a lone pair?
I think only slightly because the lone pair does have a slightly stronger repulsion factor than atoms.
- Thu Dec 17, 2020 9:10 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: electronic geometry vs molecular geometry
- Replies: 9
- Views: 1924
Re: electronic geometry vs molecular geometry
the difference is that electron geometry deals with the arrangement of electron densities (so atoms and lone pairs) while molecular geometry only deals with atoms.
- Thu Dec 17, 2020 9:08 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: What are the bond angles for T shaped?
- Replies: 21
- Views: 8464
Re: What are the bond angles for T shaped?
I think slightly less than 90 degrees because of the lone pair repulsion.
- Thu Dec 17, 2020 9:07 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: wedge and dash
- Replies: 14
- Views: 2568
Re: wedge and dash
the solid wedge means that when you are standing straight in front of a molecule that atom or lone pair is coming straight at you. A dashed line means while in the same position that atom or lone pair is shooting straight behind you.
- Thu Dec 17, 2020 9:05 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Seesaw vs. trigonal pyramidal
- Replies: 22
- Views: 2252
Re: Seesaw vs. trigonal pyramidal
They are two different shapes because the seesaw has 5 regions of electron density, trigonal pyramidal only has 4 regions of electron density.
- Thu Dec 17, 2020 9:04 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bent vs Angular
- Replies: 20
- Views: 875
Re: Bent vs Angular
bent and angular are the same thing.
- Thu Dec 17, 2020 9:02 am
- Forum: Hybridization
- Topic: Sigma and Pi bonds
- Replies: 29
- Views: 2590
Re: Sigma and Pi bonds
sigma and pi bonds are formed by the overlap of orbitals. the difference is that sigma bonds overlap in one place (end to end overlapping) and pi-bonds overlap twice (side by side overlapping). All bonds (single, double, triple) have sigma bonds, double bonds have two pi bonds and triple binds have ...
- Thu Dec 17, 2020 8:55 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: tips for memorization
- Replies: 2
- Views: 233
Re: tips for memorization
I think visualizing individual examples of atoms and physically drawing them out myself has helped me.
- Thu Dec 17, 2020 8:53 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: possible angle values
- Replies: 2
- Views: 229
Re: possible angle values
yes because it is trigonal planar based on the lewis structure.
- Thu Dec 17, 2020 8:51 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Tetrahedral molecular shape
- Replies: 10
- Views: 1736
Re: Tetrahedral molecular shape
tetrahedral's aren't confined to only one plane which allows them to be more apart from one another and have higher bonds angle
- Thu Dec 17, 2020 8:49 am
- Forum: Hybridization
- Topic: Hybridization with coefficients
- Replies: 3
- Views: 271
Re: Hybridization with coefficients
I believe that the coefficients relate to how many regions of electron density the atom has.
- Thu Dec 17, 2020 8:44 am
- Forum: Hybridization
- Topic: Non-rotating pi bonds
- Replies: 2
- Views: 318
Re: Non-rotating pi bonds
the shape of the pi bond is basically like a ladder where you have two regions in the p-orbital that overlap and you cannot rotate one of the overlapping parts or a step in a ladder without breaking the whole thing. But with sigma bonds, since there is only one point of overlap it can rotate freely ...
- Thu Dec 17, 2020 8:39 am
- Forum: Hybridization
- Topic: Lone pairs and multiple bonds
- Replies: 3
- Views: 266
Re: Lone pairs and multiple bonds
yes everything is just one region of electron density no matter how many electrons there are.
- Thu Dec 17, 2020 8:38 am
- Forum: Hybridization
- Topic: Electron Density
- Replies: 6
- Views: 411
Re: Electron Density
you do count the lone pairs because it is still a region of electron density, and remember that a double bond is still only one region to count even though there are two bonds.
- Thu Dec 17, 2020 8:36 am
- Forum: Hybridization
- Topic: Pi Bonds Cannot Rotate
- Replies: 29
- Views: 3944
Re: Pi Bonds Cannot Rotate
you basically have two regions of the p-orbital overlapping and you cant rotate one without rotating another and thus breaking the pi bond.
- Thu Dec 17, 2020 8:34 am
- Forum: Hybridization
- Topic: Hybridization
- Replies: 2
- Views: 216
Re: Hybridization
yes because electrons like to be in the lowest energy state possible so they would fill up lower shells first.
- Thu Dec 17, 2020 8:33 am
- Forum: Hybridization
- Topic: Hybridization of 2p and 2p2
- Replies: 2
- Views: 279
Re: Hybridization of 2p and 2p2
their energy levels are the same it's just how many electrons are being filled in the orbitals.
- Thu Dec 17, 2020 8:30 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angle and Terminal Atoms
- Replies: 2
- Views: 275
Re: Bond Angle and Terminal Atoms
it would only be a small effect because the larger atom is obviously larger and would take up more space in the planes, but the difference wouldnt be too substantial.
- Thu Dec 17, 2020 8:26 am
- Forum: Naming
- Topic: oxidation number
- Replies: 9
- Views: 503
Re: oxidation number
I think to find the charge of the ligands you'd have to memorize from the chart. I don't know if there's a better way but that's what I did.
- Thu Dec 17, 2020 8:25 am
- Forum: Naming
- Topic: Naming a compound
- Replies: 10
- Views: 3301
Re: Naming a compound
I watched a lot of my organic chemistry tutor on youtube and I thought how he did it was very helpful. He basically said to start off with finding the oxidation number of the transitions metal by making it an x in a variable equation and have all the other molecules' charges added up and equal to ze...
- Thu Dec 17, 2020 8:22 am
- Forum: Industrial Examples
- Topic: Cisplatin Vs. Transplatin
- Replies: 7
- Views: 1401
Re: Cisplatin Vs. Transplatin
since the cisplatin has both of its chlorine atoms on one side of the molecule it is easier for it to bond to guanine and has a stronger bond.
- Thu Dec 17, 2020 8:18 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3002510
Re: Post All Chemistry Jokes Here
what's the chemical formula for seawater? CH2O.
- Thu Dec 17, 2020 8:17 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3002510
Re: Post All Chemistry Jokes Here
what do you call a tooth in a glass of water? a one molar solution.
- Thu Dec 17, 2020 8:16 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3002510
Re: Post All Chemistry Jokes Here
why did the white bear dissolve in water? because it was polar.
- Thu Dec 17, 2020 8:15 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3002510
Re: Post All Chemistry Jokes Here
why did the attacking army use acid? to neutralize the enemy's base.
- Thu Dec 17, 2020 8:14 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3002510
Re: Post All Chemistry Jokes Here
so oxygen went ona date with potassium today... it went OK.
- Mon Nov 16, 2020 12:12 am
- Forum: Lewis Structures
- Topic: Resonance Structures
- Replies: 2
- Views: 76
Re: Resonance Structures
I think you would still count them because collectively describe the electronic bonding of a single polyatomic species including fractional bonds and fractional charges. It doesn't really matter the stability, each of the resonance structures are representing the same polyatomic species.
- Mon Nov 16, 2020 12:06 am
- Forum: Ionic & Covalent Bonds
- Topic: Bond Length
- Replies: 6
- Views: 751
Re: Bond Length
Bond length correlates to strength. If there is a shorter bond length that means that the bond is stronger because more energy is needed to break it. Longer bond length means that there's a greater distance between the atoms so it takes less energy to try to break them.
- Mon Nov 16, 2020 12:04 am
- Forum: Ionic & Covalent Bonds
- Topic: Sapling #19
- Replies: 2
- Views: 171
Re: Sapling #19
You can tell based on the charges of the atoms in the molecule. If any atom has any type of charge then it's an ion-dipole and if there isn't then it's a dipole-dipole.
- Mon Nov 16, 2020 12:01 am
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent Bonds
- Replies: 9
- Views: 578
Re: Ionic vs Covalent Bonds
You can tell from either the difference in electronegativity or how far away each atom in the molecule is from the periodic table.
If there is an electronegativity difference greater than 1.5 then that bond is ionic.
If there is an electronegativity difference greater than 1.5 then that bond is ionic.
- Sun Nov 15, 2020 11:55 pm
- Forum: Hybridization
- Topic: Charges
- Replies: 9
- Views: 1030
Re: Charges
It's better to include the formal charge of an atom/molecule especially if the formal charge isn't zero.
- Sun Nov 01, 2020 10:01 pm
- Forum: DeBroglie Equation
- Topic: Units for DeBrogile Equation
- Replies: 9
- Views: 496
Re: Units for DeBrogile Equation
For this equation, and the majority of other equations, you would use SI Units. So kg for mass, meters for wavelength, and meters per second for velocity.
- Sun Nov 01, 2020 9:58 pm
- Forum: Photoelectric Effect
- Topic: Lyman Series
- Replies: 30
- Views: 1134
Re: Lyman Series
Yes, Lyman =1 and Balmer =2.
- Sun Nov 01, 2020 9:51 pm
- Forum: Photoelectric Effect
- Topic: Electron Properties
- Replies: 4
- Views: 139
Re: Electron Properties
Usually, anything smaller than 10^-15 m is undetectable for wavelength, in the context of the problems we're doing.
- Sun Nov 01, 2020 9:33 pm
- Forum: Properties of Light
- Topic: Sapling 19
- Replies: 6
- Views: 689
Re: Sapling 19
Hi, you would have to use the de Broglie wavelength equation, which is 入 =h/mv.
入 is wavelength
h is plank's constant (6.626*10^-34 J.s)
m is mass
v is velocity
for this question you would have to rearrange it to v=h/m入 to find the speeds of each different sub-atomic particles. Hope this helps.
入 is wavelength
h is plank's constant (6.626*10^-34 J.s)
m is mass
v is velocity
for this question you would have to rearrange it to v=h/m入 to find the speeds of each different sub-atomic particles. Hope this helps.
- Sun Nov 01, 2020 9:26 pm
- Forum: Ionic & Covalent Bonds
- Topic: intermolecular vs intramolecular
- Replies: 17
- Views: 1873
Re: intermolecular vs intramolecular
Intramolecular forces are the forces that hold atoms together within a molecule. Intermolecular forces are forces that exist between molecules.
- Sun Oct 25, 2020 10:38 pm
- Forum: Ionic & Covalent Bonds
- Topic: lone pairs
- Replies: 5
- Views: 328
lone pairs
hi,
can lone pairs be an indicator of high reactivity in an element?
can lone pairs be an indicator of high reactivity in an element?
- Sun Oct 25, 2020 10:33 pm
- Forum: *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids)
- Topic: determining viscosity
- Replies: 11
- Views: 2503
determining viscosity
How can you determine a liquid has a high viscosity?
- Sun Oct 25, 2020 10:17 pm
- Forum: Ionic & Covalent Bonds
- Topic: variable valence
- Replies: 2
- Views: 240
variable valence
Hi,
Can someone explain to me what variable valance is?
Can someone explain to me what variable valance is?
- Sun Oct 25, 2020 10:13 pm
- Forum: Ionic & Covalent Bonds
- Topic: Non Metals
- Replies: 10
- Views: 707
Non Metals
Why is it that non-metals rarely lose electrons during chemical reactions? Does it have to do with their ionic bonds?
- Sun Oct 25, 2020 10:11 pm
- Forum: Ionic & Covalent Bonds
- Topic: Covalent Bonds
- Replies: 9
- Views: 322
Covalent Bonds
How can you determine which one is stronger, out of ionic, covalent and hydrogen?