Exam 1 :Ch. 1-5
Chemistry 202 with Geiger at SUNY Geneseo
About this deck
By: Aja Guzman
Created: 2011-09-27
Size: 49 flashcards
Views: 18
Created: 2011-09-27
Size: 49 flashcards
Views: 18
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Avogadro's number
6.02 x 1023
Energy equation in relation to wavelength and frequency
E = hv = hc/ λ
h = 6.63 x 10-34 J sec
c = speed of light
v = velocity
Equation for when an object absorbs or emits energy (interconversion of energy and wavelength)
ΔE = nhv = nhc / λ
n = 1, 2, 3...
Avogadro's number
6.02 x 1023 mol-1
Equation for emitting electrons after light strikes metal
KE = 1/2 mv2
+ constant if there is an incident photon
Energy of incident photon
E = hv
Equation for energy of emitting photon
E = BE + KE
KE = Kinetic energy of ejected photon
BE = Binding energy of the electron = work function (for solid metal) = similar to ionization energy
Equation for when particles have wave qualities
λ = h / mv
Nodes
Where work function = 0
# nodes = n - 1
n = electron orbital
The effect of nodes on orbital shape
On a graph, more nodes cause more hills in the graph (1 more hill than the number of nodes)
Lattice Energy equation
q1 q2 / r
q1 = Charge of cation
q2 = Charge of anion
r = Distance between cation and anion
Ionic compounds are usually soluble...
Double replacement reaction
Swap anions and cations
Molecular equation
Regular equation with reactants and products
Complete ionic equation
Equation shows the ions that are formed on both the reactant and product sides of the equation.
Net ionic equation
Removes spectator ions from the complete ionic equation.
Resonance structure
More possible arrangements of electrons without rearranging the atoms
Violations of the octet rule
Electron deficient molecules
Expanded octet
Electron deficient molecules
When the central atom has less than the amount of electrons they need.
Usually happens to atoms from the 2nd or 3rd group.
Expanded octet
If the central atom is from the 3rd period or beyond, it may have more than an octet (uses d orbitals)
Can be used to make resonance structures by reducing formal charge.
Effective electron pair geometry
Includes lone pairs as a bond.
Molecular geometry
Does not show lone pairs as a bond, but does acknowledge their force on the geometry.
Polar molecules
Have lone pairs
Have unidentical molecules attached to the central atom
Do not have symmetry
Non-polar molecules
Do not have lone pairs
Have identical molecules attached to the central atom
Have symmetry
Stereoisomers
Have the same formula and atom connectivity, but switch the planes of the atom.
Ex. Trans & cis
Strength of bonds
Lone pair > Triple bond > Double bond > Single bond
Molecular geometry: Trigonal planar
Hybridization: sp2
120o angle
Molecular geometry: Tetrahedral
Hybridization: sp3
109.5o
Molecular geometry: Trigonal bipyramidal
Hybridization: dsp3
120o & 90o & 180o
Molecular geometry: Octahedral
Hybridization: d2sp3
90o
Molecular geometry: Square planar
Hybridization: sp3
90o
Molecular geometry: T-Shaped
Hybridization: sp2
90o & 180o (has two lone pairs)
Molecular geometry: Trigonal pyramidal
Hybridization: sp2
Less than 109.5o
Molecular geometry: Seesaw
Hybridization: dsp3
Less than 90, 120, & less than 180 (has two lone pairs)
Name the hybridization and bond angle for a bent molecule.
Hybridization: sp
For one lone pair: Less than 120o
For two lone pairs: Less than 109.5o
How to hybridize
Count the lone pairs and atoms connected to the central atom
Bond order equation
Bond order = (# bonding electrons - #antibonding electrons) / 2
When is the sigma orbital lower in energy that the pi orbital?
When there are more than 10 electrons
Bond order relationships with bond strength, distance, and stability
Inverse relationship: Bond distance
Normal relationship: Bond strength and stability
When is bond order considered stable?
When it is above 0
What is the periodic trend of atom size?
Increases as you go down and to the left.
What is the periodic trend of ionization energy?
It increases as you go up and to the right.
What is the periodic trend of electron affinity?
It becomes more favorable (more negative) as you go down and to the left.
What is the periodic trend of lattice energy?
Becomes more favorable (more negative) as you go up and to the right.
Born-Haber cycle equation
Heat of formation = Heat of sublimation + 1/2(bond disassociation energy) + ionization energy + electron affinity + lattice energy
Naming monatomic ions
Just use their regular name.
Ex. Na+ = Sodium ion
Naming transition metals
If they can form more than one positive ion, then add the charge in roman numerals
Ex. Fe2+ = Iron (II)
Monatomic anions
Change the ending to -ide
O2- = Oxide
Oxoanions
Negative polyatomic ions with oxygen.
End with -ate if it is common (SO4, PO4, CrO4, NO3, ClO3, CO3)
About this deck
By: Aja Guzman
Created: 2011-09-27
Size: 49 flashcards
Views: 18
Created: 2011-09-27
Size: 49 flashcards
Views: 18
About StudyBlue
STUDYBLUE makes things that make you better at school.
Things like online flashcards with photos and audio.
Things like personalized quizzes and friendly reminders about when (and what) to study next.
Think of it as a digital backpack™: access to all of your study materials online and on your phone.
STUDYBLUE exists to make studying efficient and effective for every student, for free. Join us.
“Simply amazing. The flash cards are smooth, there are many different types of studying tools, and there is a great search engine. I praise you on the awesomeness.”
Dennis
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