CHM 152-Relationships/Things to memorize

Electron and Molecular geometry for 2 areas of electron density

e. geo- linear

m. geo- linear

angle-180

Electron and Molecular geometry for 3 areas of electron density

e. geo- trigonal planar, angle 120

m. geo-

3 bonded 0 lone pairs: Trigonal planar

2 bonded 1 lone pair: bent

Electron and Molecular geometry for 4 areas of electron density

e. geo- tetrahedral, angle 109.5

m. geo.

4 bonded 0 lone pairs: tetrahedral

3 bonded 1 lone pair: trigonal pyramidal

2 bonded 2 lone pairs: bent

Electron and Molecular geometry for 5 areas of electron density

e. geo- trigonal bipyramidal, angles 120 (equatorial) 90 (axial)

m. geo-

5 bonded 0 lone pairs: trigonal bipyramidal

4 bonded 1 lone pair: seesaw

3 bonded 2 lone pairs: T-shaped

2 bonded 3 lone pairs: Linear

Electron and Molecular geometry for 6 areas of electron density

e. geo- octahedral, angle 90

m. geo-

6 bonded 0 lone pairs: octahedral

5 bonded 1 lone pair: square pyramidal

4 bonded 2 lone pairs: square planar

hybridization orbital for molecules with linear electron geometry

sp

hybridization orbital for molecules with trigonal planar electron geometry

sp²

hybridization orbital for molecules with tetrahedral electron geometry

sp³

hybridization orbital for molecules with trigonal bipyramidal electron geometry

sp³d

hybridization orbital for molecules with octahedral electron geometry

sp³d²

Molecular orbital energy diagrams; pi bonds normally have ___ energy than sigma bonds

higher

What molecules are the exception to that rule (pi bonds are below sigma bonds in a molecular orbital diagram)

B2, C2, N2

Heat of Fusion; melting is ___ and freezing is ___

Positive; negative

Heat Vaporization; vaporization is ___ and condensation is ___

positive; negative

As temperature increases, vapor pressure

increases

As intermolecular forces increase, vapor pressure

decreases

As molecular weight increases, viscosity

increases

as temp increases, viscosity

decreases

As molecular weight increases, London Dispersion forces

increase

As intermolecular forces increases, vapor pressure

DECREASES

how to recognize a molecular solid

atoms or molecules held together by Intermolecular forces

How to recognize a metallic solid

atoms held together by metallic bonding (if its a d block metal most of the time)

How to recognize an ionic solid

ions in an ionic bond

Covalent network

atoms held together by covalent bonding

as intermolecular forces increase, melting point

increases

larger radius= ___ solubility

more

as solubility increases, lattice energy

decreases

molality

mol solute/kg solvent

as radius increases, lattice energy

decreases

as lattice energy increases, hydration energy

increases

3 things that impact le chateliers principle

temperature, pressure, concentration of molecules

mass percent of solute

(mass of solute/mass of solution)*100

Mole fractions

mole of one substance/total moles of solution

4 things that can change the rate of a reaction

concentration of reactants

concentration of a catalyst

temperature

surface area

rate laws only include

k value and reactants

when the concentration changes, if the rate is multiplied by 1/2, the reaction order=

-1

when the concentration changes, if the rate is multiplied by 1, the reaction order=

0

when the concentration changes, if the rate is multiplied by 2, the reaction order=

1

when the concentration changes, if the rate is multiplied by 4, the reaction order=

2

[At​]=−kt+[A0​]

zero order integrated rate law

ln([A0​]/[At​])​=−kt

first order integrated rate law

1/[At​]=kt+1/[A0​]

second order integrated rate law

Reaction with a LARGE activation energy will have a ____ k value

small

Reaction with a SMALL activation energy will have a ____ k value

large

Energy diagrams; when energy in products is larger than energy in reactants the reaction is

endothermic

Energy diagrams; when energy in reactants is larger than energy in products the reaction is

exothermic

reaction mechanisms; rate of reaction is always determined by the ____ step of the reaction

slowest

[A0]/2k

zero order half life (if you know this one and the first order one then you the second order one is just the last one ykwis)

equation for how Kp relates to Kc

Kp=Kc(RT)^Δn

If Qc=Kc

the reaction is at equilibrium

If Qc>Kc

the reaction will move to the LEFT; for CH 17, precipitation is expected

If Qc<Kc

the reaction will move toward the RIGHT; for CH 17, precipitation is not expected

Adding a reactant will push the equilibrium

RIGHT (more products)

adding a product will push the equilibrium

LEFT (more reactants)

Removing a reactant will push the equilibrium

LEFT (more reactant)

as volume decreases, pressure

increases

If temperature increases, the reaction will move to

The LEFT

If temp decreases, the reaction will move to

the RIGHT

Strong acids

HCL, HBr, HI

H2SO4, HNO3, HClO4

Strong bases

LiOH, NaOH, KOH

Ca(OH)2, Sr(OH)2, Ba(OH)2

the strongest acids have the ___ conjugate bases

weakest

The weaker the strength of the bond, the ___ the strength of the binary acid

stronger

As electronegativity increases, the strength of an acid

Increases

More oxygen atoms in an oxoacid=___acid strength

higher

the lower the pH the ___ acidic a solution is

MORE

A salt of a strong base and a strong acid=

a neutral solution

a salt of a strong base and a weak acid=

basic solution

a salt of a weak base and strong acid=

acidic solution

how does Kw relate to Ka and Kb

Kw=KaKb

Degree of ionization

found x value [H3O]/original given molarity

a buffer solution consists of

a weak acid and its conjugate base or a weak base and its conjugate acid

when to Henderson Hasselbalch equation

anytime the equation says “buffer” in it!!!

equivalence point

mol acid=mol base

how recognize titration question

NaOH added to an acid

how to calculate pH of titration question

1. determine moles of H+ and OH- (Multiply given M with however many liters is added)

2. Find all OH- reacted by subtracting values from 1