Search found 10 matches

by Du-A Lee 3C
Sun Dec 06, 2015 4:54 am
Forum: Polyprotic Acids & Bases
Topic: Properties of strong acid/weak base
Replies: 1
Views: 522

Properties of strong acid/weak base

I understand that strong acids lose H+ easily and result with a stable anions. However, what does it mean when the "negative charge on the conjugate base is stabilized by greater number of elections withdrawing atoms"? Is this a different bond property in terms of electronegativity?
by Du-A Lee 3C
Tue Dec 01, 2015 4:27 am
Forum: Conjugate Acids & Bases
Topic: Weak Acid and Weak Base
Replies: 1
Views: 375

Re: Weak Acid and Weak Base

Weak acids and weak bases do not fully dissociate into ions at equilibrium (in water). Calculating pH of these solutions similar method by using ICE table, Ka or Kb constants, etc. in the similar way to calculate strong acids/base. One thing to be mindful is that if the initial concentration of weak...
by Du-A Lee 3C
Tue Nov 24, 2015 11:48 am
Forum: Bronsted Acids & Bases
Topic: Acid Strength?
Replies: 2
Views: 417

Re: Acid Strength?

Acid strength is determined by: - Polarity of the X-H bond: more polar = stronger acid - Size of X atom: go down a periodic column = X-H bond becomes weaker = stronger acid - Charge of the acid/base: negative charge decreases = more acidic - Oxidation state of central atom: *only when polarity, size...
by Du-A Lee 3C
Sat Nov 14, 2015 9:25 pm
Forum: Ideal Gases
Topic: PV=nRT
Replies: 2
Views: 773


According to the Ideal Gas Law, pressure increases as temperature increases, and temperature increases as volume increases. Then why doesn't it make sense for pressure to increase as volume to increase?
by Du-A Lee 3C
Mon Nov 09, 2015 1:03 am
Forum: Shape, Structure, Coordination Number, Ligands
Topic: Naming
Replies: 2
Views: 486

Re: Naming

- When writing a molecule, you want to start with C atoms first, then H, then the rest in alphabetical order. - However, there are exceptions including ionic compounds and oxids/hydroxides/acids. - In an ionic compounds, the action is listed firs and the anion is listed second. - Oxides end in oxyge...
by Du-A Lee 3C
Sun Nov 01, 2015 9:41 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Difference Between Polar and Nonpolar Bonds
Replies: 2
Views: 1535

Re: Difference Between Polar and Nonpolar Bonds

H2O is a polar molecule because of the 2 lone pairs of e- on the central atom O. This makes this an angular/bent shape of molecule (dipole moments won't cancel).
CS2 is a nonpolar molecule because it is linear shaped (dipole moments cancel each other out).
by Du-A Lee 3C
Sun Oct 25, 2015 6:40 am
Forum: Lewis Structures
Topic: ClONO2
Replies: 1
Views: 992

Re: ClONO2

If you put double bonds on both oxygens of NO2, then there will be a total of 5 bond lines which invalidates the octet rule. Otherwise, I think the structure in the solutions manual has the lowest formal charges as it can have.
by Du-A Lee 3C
Sun Oct 18, 2015 7:03 pm
Forum: Ionic & Covalent Bonds
Topic: Ionic Bond Structure
Replies: 1
Views: 327

Re: Ionic Bond Structure

I think that all ionic compounds do have a "crystal structure" - meaning that the larger anions are arranged together in rows with the cations filling in the spaces in-between close packed layers. Lattice energy is used to explain stability of ionic solids.
by Du-A Lee 3C
Sat Oct 10, 2015 4:08 pm
Forum: Trends in The Periodic Table
Topic: Electron Affinity Trends
Replies: 1
Views: 309

Re: Electron Affinity Trends

Upper right elements generally have higher electron affinities because electrons are added to each energy level as they become closer to the nucleus and have stronger attraction. Hence, those same elements have lower atomic radii because the strong attraction pulled in electrons closer to the nucleu...
by Du-A Lee 3C
Fri Oct 02, 2015 5:40 pm
Forum: Properties of Light
Topic: Wavelike Properties of Electromagnetic Radiation/Light
Replies: 2
Views: 463

Re: Wavelike Properties of Electromagnetic Radiation/Light

I agree too. The slope of the EM radiation wave display can be seen by looking at the height/amplitude of the wave. The higher the wave, the stronger the force the field exerts on a charged particle. Low frequency represents low energy with larger wavelengths.

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