Search found 50 matches
- Wed Dec 04, 2019 5:45 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Shape
- Replies: 2
- Views: 239
Re: Shape
To find the shape of a coordination compound, count the number of ligands attached to the central atom. This is called the coordination number. If there are 6, the shape is octahedral. If there are 4, it is tetrahedral or square planar, depending on the arrangement of the ligands.
- Wed Dec 04, 2019 5:40 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: J.9
- Replies: 1
- Views: 196
Re: J.9
First, put the acid and bases given on the reactants side. Then, on the products side, put water and combine the elements on the reactants side that are NOT hydrogen or oxygen into one molecule. This is the salt that is formed. Then, balance the two sides of the equation.
- Wed Dec 04, 2019 5:36 pm
- Forum: Polyprotic Acids & Bases
- Topic: amphoteric
- Replies: 5
- Views: 407
Re: amphoteric
To put it simply, all amphiprotic substances are amphoteric, but not all amphoteric substances are amphiprotic. All amphiprotic substances must be able to donate and accept a hydrogen atom.
- Wed Dec 04, 2019 5:28 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Strong acids and bases
- Replies: 2
- Views: 234
Re: Strong acids and bases
As well as memorizing the list of strong bases, it's helpful to know that the hydroxides of group 1 and 2 metals are usually considered to be strong bases.
- Wed Dec 04, 2019 5:20 pm
- Forum: Bronsted Acids & Bases
- Topic: Net Ionic Equation Explanation from Textbook
- Replies: 1
- Views: 210
Re: Net Ionic Equation Explanation from Textbook
I think it's saying that instead of splitting the weak acid/base into its individual elements like usually done in a net ionic equation, they are kept as whole molecules.
- Mon Dec 02, 2019 12:34 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Water as a acid or base
- Replies: 4
- Views: 307
Re: Water as a acid or base
The classification of water depends on the compound it is reacting with. Since it is amphoteric, if it reacts with an acid it will act as a weak base, and if it acts with a base it will act as a weak acid.
- Mon Dec 02, 2019 12:32 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Final Study Methods
- Replies: 11
- Views: 683
Re: Final Study Methods
What helped me a lot was attending the large midterm review session and going over the worksheet given many times in order to catch any mistakes I could potentially make on the test. For the final, I suggest going over missed problems from the midterm and going to future review sessions.
- Mon Dec 02, 2019 12:25 pm
- Forum: Lewis Acids & Bases
- Topic: Difference
- Replies: 4
- Views: 389
Re: Difference
I would study the methods to determine the strength of different acids and how to order them by strength given a list of acids.
- Mon Dec 02, 2019 12:21 pm
- Forum: Polyprotic Acids & Bases
- Topic: Chelates Visual
- Replies: 2
- Views: 301
Re: Chelates Visual
I watched this video and it really helped me understand the concept of chelates: youtube.com/watch?v=RM6l2JfHxg8
- Mon Dec 02, 2019 12:19 pm
- Forum: Hybridization
- Topic: Textbook Focus
- Replies: 2
- Views: 231
Re: Textbook Focus
The sp3 orbital seems to be the most common, with examples such as ch4 or anything with 4 atoms bonded to it.
- Wed Nov 20, 2019 12:26 pm
- Forum: Hybridization
- Topic: hybridizing oxygen
- Replies: 5
- Views: 416
Re: hybridizing oxygen
To find the hybridization of an atom, you need to find its steric number. The steric number is calculated by adding the number of atoms bonded to the central atom plus the number of lone pairs on the central atom. In this case, because oxygen has 1 carbon bonded to it + 2 lone pairs, its steric numb...
- Wed Nov 20, 2019 12:20 pm
- Forum: Hybridization
- Topic: unhybridized p-orbitals
- Replies: 2
- Views: 190
Re: unhybridized p-orbitals
P-orbitals actually are hybridized. They combine with s and orbitals to form sp or spd hybridized orbitals.
- Wed Nov 20, 2019 12:16 pm
- Forum: Hybridization
- Topic: lone pairs in hybridization
- Replies: 8
- Views: 544
Re: lone pairs in hybridization
Lone pairs on the central atom occupy their own separate hybrid orbital, so they count towards the total hybridization of the atom.
- Wed Nov 20, 2019 12:13 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: Ion-dipole vs Hydrogen Bonding
- Replies: 2
- Views: 292
Re: Ion-dipole vs Hydrogen Bonding
No, because ions have far greater charges than those of dipole moments, it will have a stronger attraction and therefore result in a stronger interaction.
- Wed Nov 20, 2019 12:07 pm
- Forum: Hybridization
- Topic: 2F:7.d
- Replies: 2
- Views: 290
Re: 2F:7.d
SeF3+ has 4 regions of electron density because of its lone pair and 3 bonded atoms, so its steric number is 4, giving it a hybridization of sp3.
- Fri Nov 15, 2019 12:39 pm
- Forum: Sigma & Pi Bonds
- Topic: Hybridization
- Replies: 2
- Views: 198
Re: Hybridization
When two atoms use both s and p orbitals to bond, the energy levels of the electrons become unevenly distributed. To equalize this, s and p orbitals hybridize to form a single hybrid orbital. This imbalance does not occur in every molecule, so not all molecules are hybridized.
- Fri Nov 15, 2019 12:26 pm
- Forum: Dipole Moments
- Topic: Polarity
- Replies: 6
- Views: 326
Re: Polarity
To determine polarity, measure the electronegativity of all the atoms in the molecule. If there is an uneven distribution of electronegativity (more electronegativity to one side of the atom), there will be a dipole moment, causing the molecule to be polar.
- Fri Nov 15, 2019 12:22 pm
- Forum: Dipole Moments
- Topic: Shape of Molecules affect boiling point?
- Replies: 7
- Views: 909
Re: Shape of Molecules affect boiling point?
When two rod-shaped molecules come close together, there are more spots to experience London dispersion forces, so they will be more tightly attracted to each other, thus raising the boiling point.
- Fri Nov 15, 2019 12:19 pm
- Forum: Dipole Moments
- Topic: Interaction Potential Energy Equation?
- Replies: 2
- Views: 214
Re: Interaction Potential Energy Equation?
The interaction potential energy is the measurement of the energy that is released when two atoms/molecules interact.
- Fri Nov 15, 2019 12:13 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pair Repulsion?
- Replies: 5
- Views: 378
Re: Lone Pair Repulsion?
Lone pairs are further from the central atom because they aren't being pulled towards another atom, so they will repel more.
- Fri Nov 08, 2019 12:27 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: Interaction energy
- Replies: 3
- Views: 237
Re: Interaction energy
Interaction potential energy measures the strength of the attraction between atoms or molecules. It is affected by factors such as polarizability, size, and shape.
- Fri Nov 08, 2019 12:23 pm
- Forum: Lewis Structures
- Topic: Exceptions to Octet Rule
- Replies: 7
- Views: 418
Re: Exceptions to Octet Rule
Yes, these elements can exceed the octet rule because their empty d-subshell can take on electrons if needed, thus letting the atom hold more than 8 valence electrons.
- Fri Nov 08, 2019 12:14 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: Interaction potential energy
- Replies: 7
- Views: 426
Re: Interaction potential energy
Because the valence electrons on larger atoms are less tightly held, there is a higher chance for them to form temporary dipoles and exhibit intermolecular forces.
- Fri Nov 08, 2019 12:10 pm
- Forum: Ionic & Covalent Bonds
- Topic: Strength of ionic and covalent bonds
- Replies: 5
- Views: 317
Re: Strength of ionic and covalent bonds
Ionic bonds are generally stronger than covalent bonds because of the strong attraction between oppositely charged ions.
- Fri Nov 08, 2019 12:08 pm
- Forum: Photoelectric Effect
- Topic: frequency and ejection of electrons
- Replies: 7
- Views: 808
Re: frequency and ejection of electrons
Frequency is directly proportional to the energy of the incoming light. If this energy exceeds the threshold energy for the surface, it will eject electrons.
- Mon Oct 28, 2019 5:51 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron configuration exceptions
- Replies: 2
- Views: 122
Electron configuration exceptions
If the elements Cr and Cu have different electron configurations than expected because of half-filled and fully filled d subshells, does this also apply to the elements directly under them, like Mo, Ag, etc?
- Mon Oct 28, 2019 5:47 pm
- Forum: Ionic & Covalent Bonds
- Topic: 2A.5
- Replies: 4
- Views: 184
Re: 2A.5
In the case of copper, a full d subshell is more stable than only being partially filled. This means that the electron configuration of Cu is [Ar] 3d10 4s1. Since this question asks about Cu+, there is one less electron, so it is taken out from the s subshell to maintain the full d subshell.
- Mon Oct 28, 2019 5:44 pm
- Forum: Ionic & Covalent Bonds
- Topic: 2A.13
- Replies: 1
- Views: 72
Re: 2A.13
Cl will only become negatively charged if an electron is added, not taken away. This question asks about removing electrons, and Cl would become positively charged if an electron is removed.
- Mon Oct 28, 2019 5:40 pm
- Forum: Ionic & Covalent Bonds
- Topic: valence electrons
- Replies: 6
- Views: 357
Re: valence electrons
Since Manganese is a transition metal with an incomplete d-block, it can use the 5 d-block electrons for bonding, as well as the 2 in the s-block. This adds up to 7 total valence electrons.
- Mon Oct 28, 2019 5:08 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Lanthanides and Actinides
- Replies: 2
- Views: 166
Re: Lanthanides and Actinides
No, in my notes it says we need to know only the s-block, p-block, and the first row of the d block. The Lanthanides and Actinides are also omitted from the homework problems, so I don't think we will be asked about them.
- Sat Oct 26, 2019 1:16 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron Configuration Chart
- Replies: 2
- Views: 121
Re: Electron Configuration Chart
There are two exceptions to determining electron configuration from the periodic table: chromium and copper. In these two cases, a half-full or full d sublevel is more stable than its predicted configuration, so one electron from the s orbital moves to the d orbital.
- Fri Oct 25, 2019 12:34 pm
- Forum: Lewis Structures
- Topic: Double Bonds
- Replies: 6
- Views: 179
Re: Double Bonds
If the formal charge on an atom is not equal to zero, that's a good indication that you will need a double bond at that location.
- Fri Oct 25, 2019 12:13 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Week 5 Homework
- Replies: 9
- Views: 442
Re: Week 5 Homework
It says on the syllabus to do problems from recently covered material, so work on problems relating to chemical bonds.
- Mon Oct 21, 2019 12:11 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron Spin
- Replies: 5
- Views: 328
Re: Electron Spin
Each electron will only have one spin, and it will be either up or down. The quantum number for spin will not take on any values other than +1/2 and -1/2.
- Mon Oct 21, 2019 12:07 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Homework Question
- Replies: 2
- Views: 117
Re: Homework Question
Yes, on the syllabus it says to do homework from recently covered material. Since we haven't started the next chapter yet, you should do work from Quantum World.
- Sat Oct 19, 2019 3:49 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Memorizing electron configuration
- Replies: 3
- Views: 226
Re: Memorizing electron configuration
They fill up from left to right on the periodic table. When it hits the transition metals though, remember to write them before 4s on the electron configuration because it is a lower energy level.
- Sat Oct 19, 2019 3:44 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: determining types of orbitals (?)
- Replies: 4
- Views: 164
Re: determining types of orbitals (?)
groups 1 and 2 are s, groups 3-12 are d, and groups 13-18 are p. The inner transition elements that are placed separately are part the f subshell. Within the groups, you can count the numbers in to determine the subscript
- Sat Oct 19, 2019 3:31 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Frequencies
- Replies: 7
- Views: 485
Re: Frequencies
It also might help to memorize the visible light spectrum, as they might ask about what color a certain wavelength of light is.
- Sat Oct 19, 2019 4:51 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Same spin
- Replies: 10
- Views: 564
Re: Same spin
It's also helpful to note that all electrons will have the same spin until there is no room in the subshell and electrons must pair up (paired electrons have opposite spin). This is explained by Hund's rule.
- Sat Oct 19, 2019 4:27 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Orbitals vs. Shells
- Replies: 5
- Views: 196
Re: Orbitals vs. Shells
A shell is the broad term used to describe an energy level where the electrons reside (same value of n). Within a shell, there are subshells, which also have the same value for l. Orbitals are the specific term to describe where the electrons reside, such as in s or p.
- Sun Oct 13, 2019 4:49 pm
- Forum: Properties of Light
- Topic: Wave vs particle properties
- Replies: 4
- Views: 402
Re: Wave vs particle properties
The idea is that light acts as BOTH a wave and a particle. The diffraction of light through a slit explains it's wave-like properties, and the photoelectric effect supports the argument that it can also behave like a packet of light, or a particle. What helped me understand it was looking more into ...
- Sun Oct 13, 2019 4:36 pm
- Forum: Properties of Light
- Topic: type of light during p.e. experiment
- Replies: 2
- Views: 89
Re: type of light during p.e. experiment
UV light is most commonly used, since it's higher energy has a better chance at ejecting electrons. Hope this helps!
- Sun Oct 13, 2019 4:32 pm
- Forum: Photoelectric Effect
- Topic: Video Modules
- Replies: 7
- Views: 352
Re: Video Modules
Taking notes on the videos definitely helped me understand the material better before lectures. It's highly recommended and beneficial!
- Sun Oct 13, 2019 4:30 pm
- Forum: Photoelectric Effect
- Topic: HW Question 1B.3
- Replies: 2
- Views: 102
Re: HW Question 1B.3
According to the photoelectric effect, light sources with long wavelengths cannot eject electrons, even if they have high intensity. This explains the idea that light acts as a series of packets.
- Sun Oct 13, 2019 4:17 pm
- Forum: Properties of Electrons
- Topic: electron energy levels
- Replies: 6
- Views: 229
Re: electron energy levels
Electrons in the outermost shell take less energy to be removed because they have the weakest attraction to the nucleus. Additionally, they release the most energy when jumping to the innermost energy level.
- Sun Oct 06, 2019 8:35 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Posts
- Replies: 6
- Views: 290
Re: Posts
The 5 posts should be finished before Sunday night, which marks the end of that week. Hope this helps!
- Sun Oct 06, 2019 8:33 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Dilution and Molarity in general
- Replies: 1
- Views: 83
Re: Dilution and Molarity in general
It's also helpful to know that molarity times volume is equal to moles, so mv=mv is essentially saying that initial # of moles = final # of moles.
- Sun Oct 06, 2019 8:30 pm
- Forum: Balancing Chemical Reactions
- Topic: Combustion
- Replies: 17
- Views: 1057
Re: Combustion
Combustion is the reaction between a hydrocarbon and oxygen to produce a CO2 and H2O.
- Sun Oct 06, 2019 8:27 pm
- Forum: SI Units, Unit Conversions
- Topic: 50 Min test
- Replies: 4
- Views: 164
Re: 50 Min test
Just questions about the review of high school chemistry will be asked. Good luck!
- Sun Oct 06, 2019 8:26 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Homework G25
- Replies: 1
- Views: 77
Re: Homework G25
I would start by finding out how much solution there is after 10 mL is doubled 90 times. To do this, you would multiply 10mL by 2^90 to find the final volume.