Search found 56 matches
- Fri Dec 06, 2019 11:13 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: polarizability
- Replies: 4
- Views: 506
Re: polarizability
not necessarily polarizability has more to do with the size of an electron cloud or the charge on a polarizing agent. when looking at two nonpolar molecules with only London Dispersion Forces CH4 and CCl4, the CCl4 would have a high er boiling point and therefore a stronger bond than CH4 because it ...
- Fri Dec 06, 2019 11:11 am
- Forum: Biological Examples
- Topic: Cisplatin H2O
- Replies: 2
- Views: 181
Re: Cisplatin H2O
there is a whole explanation in the book in topic 9C!! the book says the chlorine gets replaced with water so the hydrogens can form H bonds with the lone pair on nitrogen in Guanine but dr lavelle just said that the chlorine gets replaced by the nitrogen in guanine i dont think we will have to know...
- Fri Dec 06, 2019 11:09 am
- Forum: Hybridization
- Topic: hybridization
- Replies: 3
- Views: 217
Re: hybridization
an orbital is hybridized to make everything more stable. when determining the correct hybridization for an atom, you include all the possible electron-dense regions (or bonding regions) which includes lone pairs.
- Fri Dec 06, 2019 11:07 am
- Forum: Air Pollution & Acid Rain
- Topic: Acid Rain
- Replies: 6
- Views: 622
Re: Acid Rain
acid rain is a biological example of acids and bases. carbon dioxide reacts with water to form carbonic acid and hydronium which decreases the pH of the rain. this has many biological implications such as ocean acidification which is destroying ecosystems (especially with the large output of carbon ...
- Fri Dec 06, 2019 11:05 am
- Forum: Resonance Structures
- Topic: Resonance
- Replies: 3
- Views: 315
Re: Resonance
the strength of an acid has to do with how weak the bonds are in comparison to other acids. usually, the main factor that determines this is shielding (because there is a larger electron cloud). i dont think resonance has as big of an impact on acid strength versus something like shielding
- Fri Dec 06, 2019 11:03 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Chelation
- Replies: 4
- Views: 314
Re: Chelation
It is different from polydentate because it forms a ring structure due to the fact that two parts of the ligand bind to one central atom
- Fri Dec 06, 2019 10:59 am
- Forum: Lewis Acids & Bases
- Topic: I am having trouble
- Replies: 4
- Views: 308
Re: I am having trouble
ShravanPatel4G wrote:Are there any unbonded electron pairs on the central atom?
If yes, then this molecule can act as a Lewis Base
Is the valence shell of the central atom filled?
If not, then this molecule can act as a Lewis Acid
THANK YOU!
- Thu Dec 05, 2019 2:13 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Rydberg Equation use
- Replies: 2
- Views: 271
Re: Rydberg Equation use
Parker Smith wrote:Will we lose points on the Final if we use the Rydberg equation for potential atomic spectra problems?
what is the Rydberg equation again?
- Thu Dec 05, 2019 2:12 pm
- Forum: Lewis Acids & Bases
- Topic: I am having trouble
- Replies: 4
- Views: 308
I am having trouble
I am having trouble identifying lewis acids and bases because they aren't like traditional bronstead acids and bases that are easier to pick out
Does anyone have any tips or examples?
Does anyone have any tips or examples?
- Thu Dec 05, 2019 2:07 pm
- Forum: Student Social/Study Group
- Topic: nomenclature for coordination compounds
- Replies: 1
- Views: 191
nomenclature for coordination compounds
Which nomenclature should we use when naming coordination compounds?
ex.
Chlorine:
Chloro or Chlorido
ex.
Chlorine:
Chloro or Chlorido
- Thu Dec 05, 2019 2:03 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: CH4 versus CCl4 (Boiling Point)
- Replies: 3
- Views: 5730
CH4 versus CCl4 (Boiling Point)
Why does CCl4 have a higher Boiling Point when CH4 has a shorter bond length?
- Thu Dec 05, 2019 1:59 pm
- Forum: Student Social/Study Group
- Topic: coordination compounds
- Replies: 2
- Views: 242
coordination compounds
can someone explain the difference between chelating compounds and polydentate compounds?
- Fri Nov 22, 2019 11:33 am
- Forum: Biological Examples
- Topic: Ligands
- Replies: 6
- Views: 933
Re: Ligands
ligands can attach to a transition metal to form a Heme Complex. This then allows for an open binding site. In the example of myoglobin, the open binding site is used to transport oxygen (o2 binds to the transition metal that is bound to the ligand). but there are many more biological applications o...
- Fri Nov 22, 2019 11:31 am
- Forum: Dipole Moments
- Topic: Polarity with non-polar bonds
- Replies: 3
- Views: 315
Re: Polarity with non-polar bonds
as long as dipoles (differences in electronegativity) cancel out symmetrically around the central atom, the molecule will be nonpolar
- Fri Nov 22, 2019 11:30 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: dipole-dipole vs induced dipole
- Replies: 9
- Views: 524
Re: dipole-dipole vs induced dipole
induced dipole= van der waal's forces= london forces, right? not exactly all bonds have some sort of van der waal's forces/london forces however, induced dipole is when the charge/polarity of a polar molecule causes a nonpolar molecule to have an instantaneous dipole. van der waals/london forces ar...
- Fri Nov 22, 2019 11:27 am
- Forum: Hybridization
- Topic: sp hybridization
- Replies: 4
- Views: 289
Re: sp hybridization
anything that has two boding regions (could be bonds or lone pairs) have an sp hybridization
- Fri Nov 22, 2019 11:25 am
- Forum: Lewis Structures
- Topic: Drawing Lewis Structures
- Replies: 7
- Views: 513
Re: Drawing Lewis Structures
usually when given huge molecules like that the atoms are arranged in order of which they are writtem.
For example given CH2CHCN,
the order of the "backbone" of the lewis strucrure would be C-C-C-N and then add in the hydrogens
For example given CH2CHCN,
the order of the "backbone" of the lewis strucrure would be C-C-C-N and then add in the hydrogens
- Fri Nov 15, 2019 12:06 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Test #2
- Replies: 22
- Views: 2830
Re: Test #2
He is also including Sigma and Pi bonds on the test which he is going over during Monday's lecture
- Fri Nov 15, 2019 12:02 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Test topics
- Replies: 5
- Views: 446
Re: Test topics
he is also going to test us on Pi and Sigma bonds which he is covering on monday.
- Fri Nov 15, 2019 11:59 am
- Forum: Administrative Questions and Class Announcements
- Topic: TEST 2
- Replies: 8
- Views: 395
Re: TEST 2
also what he covers about sigma and pi bonds on monday will be on the test
- Fri Nov 15, 2019 11:56 am
- Forum: Hybridization
- Topic: Relationship btw arrangement and hybrid orbitals
- Replies: 2
- Views: 213
Re: Relationship btw arrangement and hybrid orbitals
i think they are just always equally distributed unless there is a lone pair
- Fri Nov 15, 2019 11:54 am
- Forum: Dipole Moments
- Topic: Polarity
- Replies: 6
- Views: 292
Re: Polarity
If all atoms around the central atom are the same, equally distributed, and there are no lone pairs then it is nonpolar.
- Fri Nov 15, 2019 11:52 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pair Repulsion?
- Replies: 5
- Views: 328
Re: Lone Pair Repulsion?
The elctrons arent bound to another atom so there is more repulsion. Most likely there is no attraction from another atomn's protons.
- Fri Nov 08, 2019 11:08 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Water molecules
- Replies: 9
- Views: 899
Re: Water molecules
Water molecules use both hydrogens for hydrogen bonding.
But always remember, hydrogen bonding is always with the elements F, O, and N
F, O, and N always have to have a lone pair for there to be any hydrogen bonding
But always remember, hydrogen bonding is always with the elements F, O, and N
F, O, and N always have to have a lone pair for there to be any hydrogen bonding
- Fri Nov 08, 2019 11:06 am
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarisability vs Polarizing Power
- Replies: 15
- Views: 1043
Re: Polarisability vs Polarizing Power
Also, a trend that goes with it.
Atoms that are larger (and therefore have more electrons) are more Polarizable.
Atoms that are smaller (and have fewer electrons) have more Polarizing Power.
Atoms that are larger (and therefore have more electrons) are more Polarizable.
Atoms that are smaller (and have fewer electrons) have more Polarizing Power.
- Fri Nov 08, 2019 11:04 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Which lewis structure will make the dominant contribution to a resonance hybrid?
- Replies: 5
- Views: 335
Re: Which lewis structure will make the dominant contribution to a resonance hybrid?
Structures with a charge are more likely to contribute to a resonance hybrid because the electrons are delocalized in resonance hybrids.
- Fri Nov 08, 2019 11:03 am
- Forum: Octet Exceptions
- Topic: Lewis Acids and Bases?
- Replies: 11
- Views: 483
Re: Lewis Acids and Bases?
Michelle Xie 3A wrote:A lewis base would donate a pair of electrons and a lewis acid would accept a pair of electrons.
What is the acid/base name for the definition that says it donates/accepts protons? Is that a Bronsted acid/base?
- Fri Nov 08, 2019 11:00 am
- Forum: Administrative Questions and Class Announcements
- Topic: Homework
- Replies: 2
- Views: 187
Re: Homework
Yes, I believe it can be. Whatever we are doing in class is allowed for homework problems.
- Fri Nov 08, 2019 10:58 am
- Forum: Ionic & Covalent Bonds
- Topic: Polarizability
- Replies: 6
- Views: 409
Re: Polarizability
Yes! You are correct. Polarizability increases as molecular mass increases because, as molar mass increases so does the number of electrons in an atom. The more electrons there are, the more polarizability an atom has.
- Tue Nov 05, 2019 3:35 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Atomic vs Molecular Spectroscopy
- Replies: 1
- Views: 319
Atomic vs Molecular Spectroscopy
what is the difference between electronic transitions in atomic orbitals (atomic spectroscopy) and electronic transitions in molecular orbitals (molecular spectroscopy)?
- Fri Nov 01, 2019 2:21 pm
- Forum: Trends in The Periodic Table
- Topic: Noble Gases
- Replies: 10
- Views: 593
Re: Noble Gases
noble gasses are just, VERY special :)
- Fri Nov 01, 2019 2:20 pm
- Forum: Octet Exceptions
- Topic: More than 8 e-
- Replies: 3
- Views: 140
Re: More than 8 e-
having an EMPTY d shell allows for an expanded octet because there is space for more electrons. In contrast, atoms without an empty d orbital cant form expanded octets because there are no shells for the electrons to go in
- Fri Nov 01, 2019 2:18 pm
- Forum: Ionic & Covalent Bonds
- Topic: Transition Metals
- Replies: 3
- Views: 102
Re: Transition Metals
a lot of them have different charges so usually, they will specify in the problem
like iron has a +2 +3 and +4 charge it just depends on the reaction
like iron has a +2 +3 and +4 charge it just depends on the reaction
- Fri Nov 01, 2019 2:11 pm
- Forum: Lewis Structures
- Topic: Expanded Valence Shells
- Replies: 4
- Views: 200
Re: Expanded Valence Shells
it depends on how many empty d or p orbitals there are to determine how many times it can expand an octet.
I dont think it is only empty d orbitals because sulfur can become an expanded octet and it deosnt have an empty d orbital only a p orbital to "tap into"
I dont think it is only empty d orbitals because sulfur can become an expanded octet and it deosnt have an empty d orbital only a p orbital to "tap into"
- Fri Nov 01, 2019 2:09 pm
- Forum: Trends in The Periodic Table
- Topic: Calculating Ionization Energy
- Replies: 1
- Views: 119
Re: Calculating Ionization Energy
Work function is also known as threshold energy which is the amount of energy needed to remove an electron from a metal. So, it is similar to ionization energy but ionization energy is with elements in the gas ohase while this equation with work function is with metals
- Fri Nov 01, 2019 2:07 pm
- Forum: Resonance Structures
- Topic: Resonance
- Replies: 4
- Views: 141
Re: Resonance
They are also more reactive beacuse the electrons have so many possibilities of where they could be at one time. The fancy word for it is delocalization but it makes more sense to me by thinking of it as in we just dont know where they could be because there are multiple favorable structures
- Fri Oct 25, 2019 11:32 am
- Forum: Trends in The Periodic Table
- Topic: Electron Affinty
- Replies: 5
- Views: 178
Re: Electron Affinty
As you move across a period, atoms have higher electron affinity because they want to fill their valence shell. For example, Lithium is less likely to gain an electron because they want to "get rid of" the one they already have in their 2s shell versus Fluorine that wants an electron to co...
- Fri Oct 25, 2019 11:28 am
- Forum: Lewis Structures
- Topic: Exceptions to the Octet Rule
- Replies: 2
- Views: 126
Re: Exceptions to the Octet Rule
Phosphorus, Chloride, and Sulfur are all exceptions to the Octet Rule and can all, therefore, have an expanded octet.
This is because, they have that 2p orbital to "tap into" unlike elements such as Oxygen, Nitrogen, and Flouride.
This is because, they have that 2p orbital to "tap into" unlike elements such as Oxygen, Nitrogen, and Flouride.
- Fri Oct 25, 2019 11:25 am
- Forum: Lewis Structures
- Topic: Bond strength
- Replies: 7
- Views: 285
Re: Bond strength
ionic bonds are stronger than covalent bonds
but, covalent network bonds are the strongest of all bonds and include compounds like diamond and graphite
but, covalent network bonds are the strongest of all bonds and include compounds like diamond and graphite
- Fri Oct 25, 2019 11:19 am
- Forum: Resonance Structures
- Topic: Delocalization
- Replies: 2
- Views: 123
Re: Delocalization
Electrons are delocalized when there is resonance in the structure of the molecule. Delocalization means the electron isn't bound to stay in one subshell, instead it can "move around" from subshell to subshell per se. That is why we draw all the possible structures when we draw resonance b...
- Fri Oct 25, 2019 11:14 am
- Forum: Ionic & Covalent Bonds
- Topic: Resonance
- Replies: 12
- Views: 388
Re: Resonance
Their delocalized electrons also give them a lower activation energy which makes them more stable.
- Fri Oct 18, 2019 11:44 am
- Forum: Properties of Light
- Topic: Where to find equations?
- Replies: 5
- Views: 168
Re: Where to find equations?
what I always do in the back of my notebook is write down all the equations we learn because some aren't on the constants sheet!:)
- Fri Oct 18, 2019 11:42 am
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Best Way To Study?
- Replies: 56
- Views: 3227
Re: Best Way To Study?
2 words...
KAHN. ACADEMY.
especially for equilibrium and acids and bases!!
KAHN. ACADEMY.
especially for equilibrium and acids and bases!!
- Fri Oct 18, 2019 11:35 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Spin State
- Replies: 6
- Views: 202
Re: Spin State
So, spin states depend on how many electrons you have in one orbital. for example, lets say we are dealing with the P orbital which has 3 basically domains (Px, Py, and Pz) each electron can be in. When adding electrons to a system, one must distribute each electron to Px Py and Pz BEFORE adding 2 e...
- Fri Oct 18, 2019 11:28 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: quantum number n, l, m
- Replies: 13
- Views: 383
Re: quantum number n, l, m
Can someone please explain what Px, Py, Pz are and how they relate to -1,0,1? Px Py and Pz are the different parts of an orbital that an electron can occupy. the quantum number "m" refers to the specific electrons within an orbital shell. they are basically the same thing so -1,0,1 is the...
- Fri Oct 18, 2019 11:25 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: p- and d- orbitals and zero e- density
- Replies: 5
- Views: 189
Re: p- and d- orbitals and zero e- density
To explain the symmetry aspect (I am confused about the density part as well), the s orbital has symmetry because it is in the shape of a sphere so any way you cut it/look at it, it will be the same meaning the electrons will be in that vicinity the p and d orbitals do not have symmetry because thei...
- Thu Oct 10, 2019 8:55 pm
- Forum: Limiting Reactant Calculations
- Topic: percent yield
- Replies: 10
- Views: 775
Re: percent yield
Hi!
You can only do percent yield problems if they give you the experimental data so if they give it to you I would do it just in case.
Remember percent yield is,
100(actual yield/theoretical yield)= percent yield.
You can only do percent yield problems if they give you the experimental data so if they give it to you I would do it just in case.
Remember percent yield is,
100(actual yield/theoretical yield)= percent yield.
- Thu Oct 10, 2019 8:47 pm
- Forum: Student Social/Study Group
- Topic: Pen or Pencil for Homework Problems?
- Replies: 8
- Views: 416
Re: Pen or Pencil for Homework Problems?
Because we have to take tests in pen I do homework and notes in pen so I get used to working around mistakes. It also makes me do my work slower and more diligently since I don't want to mess up in pen
- Thu Oct 10, 2019 8:43 pm
- Forum: Limiting Reactant Calculations
- Topic: Showing Work for Limiting Reactant Calculations on Tests [ENDORSED]
- Replies: 68
- Views: 6333
Re: Showing Work for Limiting Reactant Calculations on Tests [ENDORSED]
KatherineValdez_4B wrote:So we can get partial credit if we show our work and we have the right idea, but mess up the calculations?
yes I remember my TA saying we get partial credit for calculations and showing work.
- Thu Oct 10, 2019 8:40 pm
- Forum: Limiting Reactant Calculations
- Topic: Test 1 Calculator
- Replies: 6
- Views: 350
Re: Test 1 Calculator
There are also lots of calculators that have periodic tables inside and different chemistry programs with conversions.
- Thu Oct 10, 2019 8:38 pm
- Forum: Properties of Electrons
- Topic: Constructive and Destructive Interference
- Replies: 4
- Views: 318
Re: Constructive and Destructive Interference
Hello! Constructive interference occurs when two different waves are acting IN phase and the result is more energy. Destructive interference occurs when two different waves are acting OUT OF phase and the result is less energy. Waves are in phase when their troughs and peaks match up and they are ou...
- Tue Oct 01, 2019 1:13 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent
- Replies: 32
- Views: 43023
Re: Ionic vs Covalent
covalent network are the strongest (ex. diamond and graphite) are stronger than ionic however covalent bonds themselves are usually weaker than ionic bonds.
- Tue Oct 01, 2019 1:11 pm
- Forum: Significant Figures
- Topic: Sig Fig Decimal
- Replies: 10
- Views: 446
Re: Sig Fig Decimal
They would be the same thing! Only if the number in the ones place was a zero would you need a decimal to include it in your sig figs.
ex.
114 - 3 sig figs
110 - 2 sig figs
110. - 3 sig figs
ex.
114 - 3 sig figs
110 - 2 sig figs
110. - 3 sig figs
- Tue Oct 01, 2019 1:09 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 2759304
Re: Post All Chemistry Jokes Here
I love to tell chemistry jokes!! But I only get a reaction periodically...
- Tue Oct 01, 2019 1:07 pm
- Forum: Balancing Chemical Reactions
- Topic: Tips on what number to multiply the entire equation if needed
- Replies: 8
- Views: 1588
Re: Tips on what number to multiply the entire equation if needed
It is easiest to write your decimal number as a fraction so you can just divide by the denominator and make every coefficient and integer! I hope this helps.
- Tue Oct 01, 2019 1:06 pm
- Forum: Empirical & Molecular Formulas
- Topic: Rounding [ENDORSED]
- Replies: 12
- Views: 746
Re: Rounding [ENDORSED]
Hello! I usually round with the consideration of sig figs. So, when multiplying or dividing, you always round to the least specific place (ex. 10.0/1 would just have one sig fig because "1" is the least specific). I usually round according to sig figs during the entire problem so I get in ...