Search found 17 matches

by Justin Ko 4C
Thu Dec 05, 2019 10:36 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Bent Shape
Replies: 29
Views: 273

Re: Bent Shape

Bent shape can have one or two lone pairs. One lone pair turns a trigonal planar into a bent molecule and two lone pairs turn a tetrahedral into a bent molecule.
by Justin Ko 4C
Wed Dec 04, 2019 9:58 pm
Forum: Acidity & Basicity Constants and The Conjugate Seesaw
Topic: 6C.17
Replies: 1
Views: 38

Re: 6C.17

We know that the smaller the pKb of a base, the stronger the base. Using chart 6C.2 from the textbook, we find that pKb of morphine is 5.79. In order to find the pkb of BrO-, we need to take the pKw (which is the equilibrium of pure water) and subtract the pKa of the conjugate acid of BrO- (which is...
by Justin Ko 4C
Tue Dec 03, 2019 11:36 am
Forum: Acidity & Basicity Constants and The Conjugate Seesaw
Topic: 6C.17
Replies: 1
Views: 46

Re: 6C.17

Morphine consists of a nitrogen atom with a lone electron pair. Therefore, morphine is a weak base. Since BrO- is a conjugate base for the weak hypobromous acid, it must be a strong base. Therefore, BrO- is a stronger base than morphine.
by Justin Ko 4C
Mon Dec 02, 2019 9:55 pm
Forum: Calculating the pH of Salt Solutions
Topic: pKa vs Ka
Replies: 6
Views: 50

Re: pKa vs Ka

Ka is the acid dissociation constant. Using the formula to calculate pH, we know that p is -log. Therefore, pKa is the -log of the dissociation constant.
by Justin Ko 4C
Sat Nov 30, 2019 9:13 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: pKb and pKa
Replies: 2
Views: 19

Re: pKb and pKa

Kb value is the value of the dissociation constant of a base. Ka is the value of the dissociation constant of an acid. p is the negative log of the dissociation constant. The lower the pKa or pKb value, the stronger the acid or base. The relation between pKa and pKb is that the sum of their values e...
by Justin Ko 4C
Sat Nov 23, 2019 7:51 pm
Forum: *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids)
Topic: Hydrogen Bonding/Pi bonds
Replies: 11
Views: 132

Re: Hydrogen Bonding/Pi bonds

A Hydrogen bond is a weak bond resulting from the proton's electrostatic attraction in one atom and the electronegativity of another atom. A pi bond is a covalent bond between the unbound p-orbitals of two atom's and restricts the rotation of the atoms.
by Justin Ko 4C
Fri Nov 22, 2019 7:26 pm
Forum: Shape, Structure, Coordination Number, Ligands
Topic: Acids
Replies: 6
Views: 32

Re: Acids

Strong acids fully dissolve into its ions in water, so they have a high concentration of ions in a solution. This, the bonds between the hydrogen atom and another atom of the molecule are weak. Ions are easily broken apart by strong acids. Weak acids partially dissociated into its ions in water, so ...
by Justin Ko 4C
Wed Nov 20, 2019 7:21 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Octahedral
Replies: 6
Views: 49

Re: Octahedral

An octahedron is a shape that consists of two pyramids who share a base. If you look at the molecule shape of an octahedral, it resembles the shape of an octahedron. Hence the name.
by Justin Ko 4C
Mon Nov 18, 2019 9:06 pm
Forum: Ionic & Covalent Bonds
Topic: Lone pairs
Replies: 4
Views: 52

Re: Lone pairs

Electron pairs in bonding pairs repel lone pair electrons, so in the VSEPR model, electron pairs will be placed as far away from each other as possible.
by Justin Ko 4C
Sun Nov 17, 2019 7:20 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Repulsion strength and Bond Angles
Replies: 12
Views: 62

Re: Repulsion strength and Bond Angles

Since the repulsion strength of lone pairs are stronger than the repulsion strength of bonding pairs, the molecule with the lone pair will have more bent bond angles
by Justin Ko 4C
Sat Nov 16, 2019 9:41 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: 3F.5 c)
Replies: 3
Views: 29

Re: 3F.5 c)

Larger atoms have more electrons and higher polarizability. As polarizability increases, the dispersion forces grow stronger. Thus, the molecules attract each other more and increase the strength of intermolecular bonds. Stronger bonds mean higher boiling/melting point, so larger atoms have higher m...
by Justin Ko 4C
Fri Nov 15, 2019 9:02 pm
Forum: Electronegativity
Topic: Ionization Energy vs. Electronegativity
Replies: 9
Views: 72

Re: Ionization Energy vs. Electronegativity

Ionization Energy and Electronegativity are the inverse of each other. Electronegativity is an atom's tendency to attract an electron. In contrast, the ionization energy is the energy needed to remove an electron from an atom. Since having more tendency to attract an electron means that the atom has...
by Justin Ko 4C
Wed Nov 13, 2019 6:43 pm
Forum: Polarisability of Anions, The Polarizing Power of Cations
Topic: Polarizing Power
Replies: 4
Views: 53

Re: Polarizing Power

If cations have the same radius, then the polarizing power is dependent on the charge. The higher the charge, the larger the polarizing power. If cations have the same charge, then the polarizing power is inversely proportional to the size of the radius. The smaller the radius, the larger the polari...
by Justin Ko 4C
Tue Nov 12, 2019 7:42 pm
Forum: Bond Lengths & Energies
Topic: 2.25
Replies: 2
Views: 27

Re: 2.25

Since both of the lewis structures are the same and bond length increases with atomic size, the PF bond in PF3 would be longer since phosphorus is larger than nitrogen
by Justin Ko 4C
Tue Nov 05, 2019 7:46 pm
Forum: Limiting Reactant Calculations
Topic: Test 1 Question
Replies: 5
Views: 133

Re: Test 1 Question

C6H12O6+6O2-->6H2O+6CO2 10gC6H12O6*(1molC6H12O6/180.156g)*(6molH2O/1molC6H12O6)=0.333molH2O*(18.02gO=H2O/1molH2O) =6.002gH2O; 6.002gH2O-5.000gH2O=1.002gH2O*(1molH2O/18.02gH2O) =0.056molH2O excess; 0.056molH2O*(1molC6H12O6/6molH2O)*(180.156gC6H12O6/1molC6H12O6) =1.675gC6H12O6 leftover 6gH2O*(1molH2O/...
by Justin Ko 4C
Wed Oct 30, 2019 10:32 pm
Forum: DeBroglie Equation
Topic: Homework 1B.15
Replies: 3
Views: 43

Re: Homework 1B.15

The photon needs enough energy to release the electron from the surface and move at 3.6*10^3 km.s^-1. The equation for the kinetic energy of the electron is 1/2mv^2, so the energy of the photon will be (1.66*10*-17J) + (1/2(9.11*10^-31kg)(3.6*10*6m.s^-1)^2=2.25*10^-17J. To get wavelength of the phot...
by Justin Ko 4C
Tue Oct 29, 2019 7:37 pm
Forum: Lewis Structures
Topic: Orbitals
Replies: 9
Views: 69

Re: Orbitals

Yes, because you remove electrons from the farthest orbital because the further away an electron is from the nucleus, the easier it is to remove

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