Search found 18 matches

by Ashley Fallon 3C
Sun Dec 10, 2017 10:21 pm
Forum: Acidity & Basicity Constants and The Conjugate Seesaw
Topic: Strengths of Acids
Replies: 2
Views: 313

Re: Strengths of Acids

acid strength can be determined by looking at how stable its conjugate base is. If the conjugate base has more EN atoms, then it creates delocalization of electrons and makes it more stable
by Ashley Fallon 3C
Sun Dec 10, 2017 10:20 pm
Forum: Acidity & Basicity Constants and The Conjugate Seesaw
Topic: Assumption for Subtracting X in Ka or Kb calculation [ENDORSED]
Replies: 3
Views: 344

Re: Assumption for Subtracting X in Ka or Kb calculation [ENDORSED]

the x value is so small compared to the concentration that the change is negligible for when you're calculating x
by Ashley Fallon 3C
Sun Dec 03, 2017 5:23 pm
Forum: Ideal Gases
Topic: Kp and Kc
Replies: 7
Views: 512

Re: Kp and Kc

Kc uses molar concentrations while Kp uses the partial pressures of gasses inside the closed system
by Ashley Fallon 3C
Sun Dec 03, 2017 5:19 pm
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Difference betwen constant and quotient?
Replies: 4
Views: 346

Re: Difference betwen constant and quotient?

They are calculated the same way, but the quotient represents the reaction at any time while the constant is only when the reaction is at equilibrium
by Ashley Fallon 3C
Sun Nov 26, 2017 11:05 pm
Forum: Hybridization
Topic: Pi Bonds vs. Sigma Bonds
Replies: 7
Views: 303

Re: Pi Bonds vs. Sigma Bonds

Sigma bonds are the FIRST bonds to be made between two atoms. They are made from hybridized orbitals. Pi bonds are the SECOND and THIRD bonds to be made. They are made from leftover "p" orbitals
by Ashley Fallon 3C
Sun Nov 26, 2017 11:00 pm
Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
Topic: Diatomic Molecules
Replies: 2
Views: 199

Re: Diatomic Molecules

Heteronuclear diatomic molecules are composed of two atoms of different elements, like in the case of hydrochloric acid and carbon monoxide.
by Ashley Fallon 3C
Sun Nov 19, 2017 7:20 pm
Forum: Bond Lengths & Energies
Topic: Bond Order
Replies: 6
Views: 445

Re: Bond Order

To determine bond order, draw the lewis structure, count the total number of bonds, and divide by the atoms.
by Ashley Fallon 3C
Sun Nov 19, 2017 7:10 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Bent or linear?
Replies: 11
Views: 627

Re: Bent or linear?

If there are no lone pairs then it would be linear because it is lacking the electron repulsion from the lone pairs.
by Ashley Fallon 3C
Sun Nov 12, 2017 10:36 pm
Forum: Lewis Structures
Topic: Lewis acids and bases [ENDORSED]
Replies: 3
Views: 209

Re: Lewis acids and bases [ENDORSED]

A lewis acid accepts electrons while a lewis base donates electrons
by Ashley Fallon 3C
Sun Nov 12, 2017 10:29 pm
Forum: Ionic & Covalent Bonds
Topic: Covalent Bonding: Polar and Non-polar
Replies: 6
Views: 372

Re: Covalent Bonding: Polar and Non-polar

You can tell when comparing the differences in electronegativities of each atom. Generally, if the difference is greater than 2 it is said to be a polar bond.
by Ashley Fallon 3C
Sun Nov 05, 2017 2:08 am
Forum: Lewis Structures
Topic: electron configuration
Replies: 6
Views: 304

Re: electron configuration

I read in the textbook that generally for elements with an atomic number of 20 or above, they begin listing the electron configuration in simple numerical order instead of having configurations where 4s comes before 3d
by Ashley Fallon 3C
Sun Nov 05, 2017 2:00 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Hund's Rule [ENDORSED]
Replies: 6
Views: 369

Re: Hund's Rule [ENDORSED]

For an electron to be spin paired means that one electron within the orbital has a counterclockwise spin, while the other electron occupying that orbital has a clockwise spin.
by Ashley Fallon 3C
Sun Oct 29, 2017 11:33 pm
Forum: Trends in The Periodic Table
Topic: Atomic Radius vs. Ionic Radius [ENDORSED]
Replies: 4
Views: 253

Re: Atomic Radius vs. Ionic Radius [ENDORSED]

Atomic radius is half the distance between two neighboring atoms, and the ionic radius is half the distance between an ionic bond of neighboring atoms.
by Ashley Fallon 3C
Sun Oct 29, 2017 11:29 pm
Forum: Electron Configurations for Multi-Electron Atoms
Topic: Removing an Electron [ENDORSED]
Replies: 5
Views: 292

Re: Removing an Electron [ENDORSED]

It is always the electron in the outer valence shell. As n goes up, energy goes up and the electron eventually escapes from the atom.
by Ashley Fallon 3C
Sun Oct 15, 2017 7:06 pm
Forum: Properties of Electrons
Topic: Threshold level and Work Function [ENDORSED]
Replies: 6
Views: 421

Re: Threshold level and Work Function [ENDORSED]

Yes, the threshold is the same as the work function. Essentially it is just the amount of energy needed to eject an electron from a piece of metal.
by Ashley Fallon 3C
Sun Oct 15, 2017 7:04 pm
Forum: Properties of Light
Topic: Photoelectric Experiments:Light [ENDORSED]
Replies: 4
Views: 251

Re: Photoelectric Experiments:Light [ENDORSED]

They generally use ultraviolet light due to its high energy (high frequency). This gives the individual photons enough energy to eject an individual electron. It follows this 1:1 ratio.
by Ashley Fallon 3C
Sun Oct 08, 2017 10:36 pm
Forum: Significant Figures
Topic: All students read this sig fig post [ENDORSED]
Replies: 91
Views: 9073

Re: All students read this sig fig post [ENDORSED]

Do you know if the problems will specifically tell us how many significant figures to use? No. With the numbers that are given, you should know how many sig figs to use. But when using molecular mass, the best number is 3-4 sig figs. When in doubt, use 3 sig figs. Other than that, always apply the ...
by Ashley Fallon 3C
Sun Oct 08, 2017 10:18 pm
Forum: Balancing Chemical Reactions
Topic: Balancing Chemical equations too slow... any advice? [ENDORSED]
Replies: 18
Views: 1493

Re: Balancing Chemical equations too slow... any advice? [ENDORSED]

I usually start with the element that occurs the least. After balancing that, I go in ascending order until I finish.

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