Search found 50 matches
- Tue Dec 03, 2019 1:33 am
- Forum: Lewis Acids & Bases
- Topic: How many protons can a base accept
- Replies: 1
- Views: 220
Re: How many protons can a base accept
Since oxygen is more electronegative than nitrogen, it is less likely to share its electrons with a proton. Thus, the nitrogens are able to accept protons while the oxygens are not.
- Tue Dec 03, 2019 12:55 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Oxalate denticity
- Replies: 1
- Views: 179
Oxalate denticity
I know oxalate is primarily bidentate, but can it also be a monodentate? Or does the binding of one oxygen atom on oxalate cause an adjacent oxygen to bind to the central metal atom as well due to proximity?
- Tue Dec 03, 2019 12:51 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Polydentate
- Replies: 3
- Views: 286
Re: Polydentate
When the ligand binds to a central metal atom at two or more of its sites, it is considered a polydentate. You can tell where these sites are by looking for lone pairs. Usually I look for oxygens and nitrogens in the ligand to see if they have any lone pairs they can donate. The shape of the ligand ...
- Mon Dec 02, 2019 10:28 pm
- Forum: Conjugate Acids & Bases
- Topic: 6A.9
- Replies: 2
- Views: 232
Re: 6A.9
NH4I is a salt, so there isn't a conjugate acid or base. You can find which acids or bases it is derived from though, which is NH4+ and I - If you look at the other parts of the same question, there are salts, but the conjugate acid and base are easily identifiable. In part a) NH 4 I (aq) +...
- Mon Dec 02, 2019 9:54 pm
- Forum: Conjugate Acids & Bases
- Topic: 6A.9
- Replies: 2
- Views: 232
6A.9
I know this question doesn't ask for a conjugate acid or base, but I was just curious what they would be in this chemical reaction. 6A.9 c) NH 4 I (am) + KNH 2 (am) --> KI (am) + 2NH 3 (l) "am" indicates that liquid ammonia is the solvent The textbook's use ...
- Wed Nov 27, 2019 9:52 am
- Forum: Hybridization
- Topic: Hybridization in Pi Bonds
- Replies: 4
- Views: 305
Hybridization in Pi Bonds
Can someone explain why when C double bonds to another C as in ethylene, the pi bond is a bond between the C's unhybridized 2p orbitals?
- Wed Nov 27, 2019 9:46 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Polydentate ligands/Shapes
- Replies: 2
- Views: 212
Re: Polydentate ligands/Shapes
Dr. Lavelle also said in class that the shape of certain ligands make it easier for them to chelate. For example, although ethylenediamine has its nitrogen atoms at opposite ends of the molecule, its large shape allows it to reach and bind to two points of a central metal atom.
- Wed Nov 27, 2019 9:41 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Ligands
- Replies: 6
- Views: 456
Re: Ligands
Yes, ligands are considered Lewis bases since they are electron pair donators.
- Wed Nov 27, 2019 9:39 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Common Ligand charges
- Replies: 1
- Views: 206
Re: Common Ligand charges
Dr. Lavelle sent an email with this link:
https://lavelle.chem.ucla.edu/wp-conten ... pounds.pdf
I think we just memorize these.
https://lavelle.chem.ucla.edu/wp-conten ... pounds.pdf
I think we just memorize these.
- Wed Nov 27, 2019 9:22 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Indicators of oxides
- Replies: 2
- Views: 214
Re: Indicators of oxides
You can also create a chemical equation with water for oxides. For example: (a) BaO + H 2 O --> Ba(OH) 2 The formation of hydroxide (OH - ) when BaO is added to water shows that BaO is a basic oxide. (b) SO 3 + H 2 O --> H 2 SO 4 , a strong acid For (c) and (d), we see that As 2 O 3 and Bi 2 O 3 - a...
- Fri Nov 22, 2019 9:53 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: LDF vs dipole-dipole
- Replies: 4
- Views: 382
LDF vs dipole-dipole
Can LDF sometimes have more effect on the boiling point of a compound than its dipole-dipole forces? For example, when the structures of two different compounds are identical except for its central atom, are there times when the difference in the molar masses of the central atoms (and hence the diff...
- Fri Nov 22, 2019 9:47 am
- Forum: Biological Examples
- Topic: EDTA
- Replies: 3
- Views: 234
EDTA
Can anyone explain again what Dr. Lavelle explained about EDTA in lecture? What is its significance?
- Fri Nov 22, 2019 9:44 am
- Forum: Sigma & Pi Bonds
- Topic: Coordination # and Steric #
- Replies: 2
- Views: 221
Re: Coordination # and Steric #
Do steric numbers change if bonds are double or triple?
- Fri Nov 22, 2019 9:28 am
- Forum: Hybridization
- Topic: hybridizing d orbitals
- Replies: 7
- Views: 454
Re: hybridizing d orbitals
Kassidy Ford 1J wrote:are we going to have to know the d hybridizations or are we only supposed to know the p hybridizations?
Since Dr. Lavelle mentioned it in class, I think we should be familiar with the d-orbital hybridizations as well.
- Fri Nov 22, 2019 9:19 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Transplatin
- Replies: 3
- Views: 296
Re: Transplatin
Dr. Lavelle explained that since the Cls are pointing in opposite directions in the transplatin molecule, it's impossible for it to bind strongly (with both Cls as cisplatin is able to do) to DNA, hence making the transplatin unable to form a coordination complex with the DNA.
- Fri Nov 15, 2019 12:12 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: T-shaped
- Replies: 3
- Views: 279
Re: T-shaped
A molecule with 3 electron groups (3 bonds) and no lone pairs is called trigonal planar. A trigonal pyramidal molecule has 3 electron groups (3 bonds) and 1 lone pair on the central atom. A T-shaped molecule has 3 electron groups (3 bonds) and 2 lone pairs on the central atom. Basically the differen...
- Fri Nov 15, 2019 12:03 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: bond angles
- Replies: 9
- Views: 616
Re: bond angles
Also, if the atoms bonded to the central atom are not the same atoms (e.g. CH2ClI) bond angles can differ due to differences in the different atoms' electronegativities.
- Thu Nov 14, 2019 11:55 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: Vapor Pressure + IMF
- Replies: 3
- Views: 343
Re: Vapor Pressure + IMF
Vapor pressure also differs at different temperatures. We see this because temperature is essentially a measure of the average kinetic energy of particles of whatever it is we're measuring. As this average kinetic energy rises, more particles (molecules, atoms, etc.) are able to vaporize—since some ...
- Thu Nov 14, 2019 11:25 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Textbook question 2E.1
- Replies: 4
- Views: 274
Re: Textbook question 2E.1
The two molecules attached to the central atom are generally more electronegative than the central atom. There must be lone pairs on the molecule with a 120 degree bond angle so that the otherwise linear molecule "bends" downward through electron repulsion with these more electronegative a...
- Thu Nov 14, 2019 11:19 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Figure 2E.7
- Replies: 1
- Views: 174
Re: Figure 2E.7
I think this figure just illustrates the electron clouds of the chlorines on the molecule. For the VSEPR section of the syllabus, Lavelle said we only need to identify the shape based on the number of bonds and lone pairs and know each shape's corresponding angle.
- Tue Nov 05, 2019 6:25 pm
- Forum: Dipole Moments
- Topic: Dipole Moments
- Replies: 5
- Views: 464
Re: Dipole Moments
Dipole moments arise from differences in electronegativity, which represents a separation of charge. One part of the compound is slightly positive while the other is slightly negative. We represent this using an arrow pointing in the direction of the slightly negative portion. We can also measure th...
- Tue Nov 05, 2019 6:21 pm
- Forum: Dipole Moments
- Topic: Dipole moments
- Replies: 1
- Views: 124
Re: Dipole moments
We can just determine which electronegativity value is higher between the two elements of a bond. The element with higher electronegativity should have a slightly negative charge and the other should be slightly positive. In some compounds, such as symmetrical ones, these dipole moments "cancel...
- Tue Nov 05, 2019 5:37 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge when it's not labelled?
- Replies: 2
- Views: 200
Re: Formal Charge when it's not labelled?
Formal charge just indicates the charge of each element in a molecule regardless of its charge. The formal charges of each element in the molecule should add up to the charge of the ion, or 0 if the molecule is neutral.
- Tue Nov 05, 2019 11:19 am
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge/Lewis structures
- Replies: 5
- Views: 395
Re: Formal Charge/Lewis structures
RoshniVarmaDis1K wrote:If formal charges that are not equal to 0 must exist, they should be as symmetrically spaced out on the outer atoms as possible. This increases surface area and makes the molecule more stable because it has lower energy.
Why does delocalization of electrons like this make the molecule more stable?
- Tue Nov 05, 2019 11:06 am
- Forum: Ionic & Covalent Bonds
- Topic: Polyatomic Ions
- Replies: 2
- Views: 214
Re: Polyatomic Ions
^it would probably be useful to know the charges of these ions as well!
- Thu Oct 31, 2019 8:42 pm
- Forum: Electronegativity
- Topic: 2D.3
- Replies: 2
- Views: 185
Re: 2D.3
I'm thinking that out of the three compounds listed there, Ba and Br have the highest difference in electronegativity values, followed by Ca and Br, and finally by Be and Br. That would make BaBr2 have bonds that are primarily ionic.
- Thu Oct 31, 2019 8:34 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charges on Atoms Summed in Ions?
- Replies: 6
- Views: 225
Re: Formal Charges on Atoms Summed in Ions?
In an ion, generally the formal charges should add up to the charge of the ion. In a molecule, I believe the formal charges should add up to 0.
- Thu Oct 31, 2019 8:32 pm
- Forum: Resonance Structures
- Topic: C4H4
- Replies: 2
- Views: 389
Re: C4H4
If I understand correctly what you mean by "drawing them in a carbon line," this would give you butatriene, with a double bond between each carbon atom and the first and last carbons having two hydrogens each (H 2 C=C=C=CH 2 ). The book's arrangement of C 4 H 4 with the carbons in a "...
- Thu Oct 31, 2019 8:22 pm
- Forum: Lewis Structures
- Topic: Angstrom Measurements on Lewis Structures
- Replies: 3
- Views: 242
Re: Angstrom Measurements on Lewis Structures
Dr. Lavelle gave us the length of covalent bonds in Angstroms to show us that the molecules that we draw using different resonance structures are, in actuality, have bonds that are hybrids of the single/double/triple bond.
- Thu Oct 31, 2019 8:19 pm
- Forum: Ionic & Covalent Bonds
- Topic: Electronegativity
- Replies: 7
- Views: 279
Re: Electronegativity
The values that represent the electronegativity of elements are arbitrary and only used for comparison between elements.
- Fri Oct 25, 2019 5:52 am
- Forum: Lewis Structures
- Topic: Where to start putting dots for electrons
- Replies: 10
- Views: 594
Re: Where to start putting dots for electrons
If an atom, such as oxygen, forms a double bond and has two lone pairs of electrons, should I draw the dots for the lone pairs on diagonal sides of the O (on the other side of the double bond lines), rather than on the top and the bottom?
- Fri Oct 25, 2019 5:50 am
- Forum: Ionic & Covalent Bonds
- Topic: Properties of Metals/Nonmetals/Metalloids
- Replies: 3
- Views: 231
Re: Properties of Metals/Nonmetals/Metalloids
Nonmetals also tend to have higher electron affinities than do metals. We can see this since Groups 7, 8, and 9 generally form negative charges (additional electrons) while Groups 1 and 2 form positive charges.
- Fri Oct 25, 2019 5:39 am
- Forum: Bond Lengths & Energies
- Topic: Bond lengths
- Replies: 15
- Views: 1046
Re: Bond lengths
andrewcj 4I wrote:Debora Fernandez Clemente_ 4H wrote:would the bond length vary when it is a double or triple bond?
Yes! Multiple bonds will be shorter than single bonds.
For example, because a double bond is stronger than a single bond, the double bond's length will be relatively shorter since the atoms are pulled together with more strength.
- Fri Oct 25, 2019 5:35 am
- Forum: Octet Exceptions
- Topic: Octet exception examples
- Replies: 9
- Views: 299
Re: Octet exception examples
Jordan Young 3E wrote:Boron also is an exception at times
Boron typically has 6 valence electrons, forming 3 covalent bonds. Right?
- Fri Oct 25, 2019 5:31 am
- Forum: Resonance Structures
- Topic: Resonance Structures
- Replies: 4
- Views: 171
Re: Resonance Structures
Dr. Lavelle showed us in class that the molecule most likely exists as a hybrid of the resonance structures by comparing the typical bond length between two atoms to the bond length between the same two atoms within a molecule. The difference in the bond lengths proves that the molecule's bonds are ...
- Wed Oct 16, 2019 1:05 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: HW Help
- Replies: 3
- Views: 142
Re: HW Help
Wouldn't the value of l in n=2 be either 0 or 1?
l=0 would correspond with the 2s subshell, which has 1 orbital.
l=1 would correspond with the 2p subshell, which has 3 orbitals.
So there would be four total orbitals in the n=2 energy level.
l=0 would correspond with the 2s subshell, which has 1 orbital.
l=1 would correspond with the 2p subshell, which has 3 orbitals.
So there would be four total orbitals in the n=2 energy level.
- Wed Oct 16, 2019 12:54 am
- Forum: Einstein Equation
- Topic: Equation use
- Replies: 6
- Views: 367
Re: Equation use
If you have one of the two unknown values of this equation (E or v) and need to solve for the other, use this equation.
- Wed Oct 16, 2019 12:33 am
- Forum: Properties of Light
- Topic: Balmer and Lyman in real world
- Replies: 1
- Views: 51
Re: Balmer and Lyman in real world
The Balmer series refers to EM radiation that is emitted when an electron returns from a state n>2 to n=2. The Lyman series corresponds to EM radiation emitted when an electron returns from a state n>1 to n=1. The wavelengths of the EM radiation classified under the Balmer series are within the visi...
- Wed Oct 16, 2019 12:20 am
- Forum: Properties of Light
- Topic: 1A.11
- Replies: 2
- Views: 161
Re: 1A.11
I think the answer is basically saying that for each series there is a common energy level that the electron returns to. For example, the Balmer series corresponds to the EM radiation that is emitted when an electron returns from any higher energy level to the lower energy level n=2, and Lyman to th...
- Tue Oct 15, 2019 11:32 am
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Indeterminacy in Position [ENDORSED]
- Replies: 5
- Views: 265
Indeterminacy in Position [ENDORSED]
In the 10/14/19 lecture, Dr. Lavelle gave an example problem: Incorrect atomic model: electron is located inside the nucleus of the atom. For the H-atom, the electron is then confined to its nuclear diameter. He explained that the nuclear diameter would be the value for the electron's indeterminacy ...
- Fri Oct 11, 2019 9:48 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Quantum number as a discrete unit
- Replies: 3
- Views: 258
Re: Quantum number as a discrete unit
The quantum numbers all correspond to a specific orientation of an orbital, which means that they are bound to certain integers. For example, l consists of integers between 0 and n-1.
- Fri Oct 11, 2019 9:40 am
- Forum: Trends in The Periodic Table
- Topic: Ionization Energy: Na vs. Al
- Replies: 3
- Views: 3974
Re: Ionization Energy: Na vs. Al
The atomic radius of Aluminum is smaller than that of Sodium. Therefore, the outer electrons of an Aluminum atom are closer to the nucleus, and thus are more strongly attracted to the nucleus than are Sodium's electrons.
- Fri Oct 11, 2019 9:26 am
- Forum: Einstein Equation
- Topic: Units
- Replies: 17
- Views: 1780
Re: Units
Do we need to know the SI unit equivalents for each term, like the joule?
- Fri Oct 11, 2019 9:14 am
- Forum: SI Units, Unit Conversions
- Topic: Help on Fundamentals: E21
- Replies: 7
- Views: 469
Re: Help on Fundamentals: E21
Does this mean when a question asks for number of atoms, you can substitute atoms with molecules or particles as well? Are atoms/ molecules/ chemical particles all just different names for the same item? I think the textbook usually specifies whether it is asking for the number of atoms/molecules/p...
- Fri Oct 11, 2019 9:10 am
- Forum: Properties of Light
- Topic: Homework question 1D11?
- Replies: 1
- Views: 89
Re: Homework question 1D11?
a) l=0 describes the s-orbital, which has 1 orbital.
b) l=2 describes the d-orbital, which has 5 orbitals.
c) l=1 describes the p-orbital, which has 3 orbitals.
d) l=3 describes the f-orbital, which has 7 orbitals.
b) l=2 describes the d-orbital, which has 5 orbitals.
c) l=1 describes the p-orbital, which has 3 orbitals.
d) l=3 describes the f-orbital, which has 7 orbitals.
- Thu Oct 03, 2019 11:48 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: HW question G11
- Replies: 3
- Views: 186
Re: HW question G11
We isolate the liters of the solution since that is what the question is asking us to solve for. It's just an algebraic manipulation of the original equation to isolate the unknown variable.
- Thu Oct 03, 2019 11:41 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: HW question G15a
- Replies: 1
- Views: 112
Re: HW question G15a
Since it's asking what volume of 0.778 M should be diluted to make a FINAL SOLUTION of 150.0 mL with concentration 0.0234 M, we know that Vf = 0.1500 L and Mf = 0.0234 M. Therefore, Mi = 0.778 M, and so the question asks to find Vi, initial volume.
- Thu Oct 03, 2019 11:31 pm
- Forum: Limiting Reactant Calculations
- Topic: textbook problem help
- Replies: 4
- Views: 243
Re: textbook problem help
a) Both Copper(II) Nitrate (Cu(NO 3 ) 2 ) and Sodium Hydroxide (NaOH) are soluble in water due to the nitrate and the sodium in each substance respectively. So nitrate and sodium would be spectator ions, which are omitted from the net ionic equation. Thus, the equation would be: Cu 2+ + 2OH - ---> C...
- Thu Oct 03, 2019 11:12 pm
- Forum: SI Units, Unit Conversions
- Topic: Can someone explain why we use kg for mass as the base unit?
- Replies: 9
- Views: 969
Re: Can someone explain why we use kg for mass as the base unit?
Has anyone heard from any past CHEM 14 students whether Dr. Lavelle tests us on small details like this? Or would most of the questions on the tests/quizzes/exams be like the homework problems?
- Thu Oct 03, 2019 10:58 pm
- Forum: SI Units, Unit Conversions
- Topic: Help on Fundamentals: E21
- Replies: 7
- Views: 469
Re: Help on Fundamentals: E21
I'm pretty sure it's Avogadro's number regardless, since a mole of a substance indicates 6.022x10^23 atoms, molecules, or other chemical particles.