Final Exam Review
Chemistry 103 with Wendt at University of Wisconsin - Madison
About this deck
By: Laura Roscizewski
Textbook:
Chemistry and Chemical Reactivity (with General ChemistryNOW CD-ROM)
Created: 2007-12-13
Size: 110 flashcards
Views: 430
Textbook:
Chemistry and Chemical Reactivity (with General ChemistryNOW CD-ROM)Created: 2007-12-13
Size: 110 flashcards
Views: 430
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Hetergeneous Material
Can be physically seperated into different kinds of matter
Ex: chocolate chip cookie
Ex: chocolate chip cookie
Homogeneous Material
Pure substances that cannot be seperated
Ex: water
Ex: water
atom
smallest particle that retains the characteristics of the substance
physical properties
anything that is observable without changing the nature of the substance
extensive properties
properties dependent on the amount of susbstance present
Ex: mass and vloume
Ex: mass and vloume
intensive properties
properties independent of the amount of substance
Ex: color, state, density
Ex: color, state, density
kinetic-molecular theory
all matter consists of tiny particles (atoms, ions, etc) in constant motion
element
pure substance composed of only one type of atom
compound
pure substance composed of more than one type of atom
properties of solids (2)
* tiny paticles are tightly packed (fixed volume)
* particles are not allowed to move past each other (fixed shape)
* particles are not allowed to move past each other (fixed shape)
properties of liquids (2)
* tiny particles are tightly packed (fixed volume)
* free to move past each other (no defined shape)
* free to move past each other (no defined shape)
properties of gases (2)
* particles are far apart from each other (no fixed volume)
* free moving particles (no defined shape)
* free moving particles (no defined shape)
importance of Thomson cathode ray experiment
established the existance of electron and provided mass-to-charge ratio
importance of Millikan oil drop experiment
established charge of an electron as -1 and mass of electron as 9.1 x 10^28 g
importance of Rutheford gold foil experiment
eliminated thomsom electron "soup" model and established idea that all the mass of an atom has to be in one area (nucleus)
3 subatomic particles
proton, neutron, electron
mole
6.022 x 10^23
(avagadro's number)
(avagadro's number)
periodic groups
vertical columns
A- main group elements
B- transition elements
A- main group elements
B- transition elements
periodic periods
horizontal rows
properties of metals
* solid at room temp.
* conductive
* conductive
properties of non metals
* state may vary
* non conductive
* exist in various allotropes
* non conductive
* exist in various allotropes
properties of metalloids
exhibits properties of both metals and non-metals
group 1A
alkali metals
group 2A
alkaline earth metals
group 7A
halogens
group 8A
noble gases
NO2 (-)
nitrite
NO3 (-)
nitrate
PO4 (3-)
phosphate
HPO4 (2-)
hydrogen phospate
H2PO4 (-)
dihydrogen phosphate
CO3 (2-)
carbonate
characteristics of ionic compounds
* generally solid at room temp
* very high melting point and boiling point
*liquid state is conductive, but solid state is not
* very high melting point and boiling point
*liquid state is conductive, but solid state is not
density
mass/ volume
Balance reaction:
C4H10 + O2 --> CO2 + H20
C4H10 + O2 --> CO2 + H20
2 C4H10 + 13 O2 --> 8 CO2 + 10 H2O
Solution
homogeneous mixture of two or more compounds
solvent
predominent compound in a solution
solute
minor compound in a solution
aqueous solution
water is the solvent in a solution
electrolytes
a compound whose aqueous solution conducts
solubility
reduction
gain of electrons
oxidation
loss of electrons
pH scale
0- 7 acidic
7 neutral
7-14 basic
7 neutral
7-14 basic
thermodynamics
study of heat transfer
1st law of thermodynamics
total amount of energy in a reaction is conserved
2 types of kinetic energy
mechanical and thermal
2 types of potential energy
graviational and chemical
exothermic
energy transfered from system to surroundings
endothermic
energy transfered from surroundings to system
specific heat capacity
energy required to raise temperature of substance (1 g) by 1 K (1 degree C)
(J/ gK)
(J/ gK)
warming and cooling specific heat capacity formula
q= Cm(Tf- Ti)
specific heat capacity formula for heat of vaporization and heat of fusion
q= (delta Hf) (mass)
internal energy
sum of all energy sources (E)
Hess's Law
if a reaction can be represented as the sum of 2+ other reactions the the net ?H is simply the sum of the ?H of the components
standard molar enthalpy of formation (?Hf°)
?H for a reaction involving the formation of 1 mole of a species from its constituent elements at standard conditions
wave-like characteristics of light
*interference
*diffraction
*diffraction
interference
"pass through" effect
amplitudes are additive
amplitudes are additive
diffraction
bending of a wavefront when passed through a slit
characteristics of light that are "particle-like" (photelectric effect)
* ejection of electrons is not continuous
* impact energy is not proportional to the intensity
* impact energy is not proportional to the intensity
photon
particle of light
Bohr model of atom
* e- is in an orbit about the nucleus
* orbital distance is quatized (can exist only in specific locations)
* only works for H atom
* orbital distance is quatized (can exist only in specific locations)
* only works for H atom
principle quantum number and possible values
n= 1,2,3,4...
angular momentum number and possible values
l=0,1,2,3,4...n-1
magnetic quantum number and possible values
ml= -l...-3,-2,-1,0,1,2,3...l
spin quantum number and possible values
ms= -1/2, +1/2
Stern-Gerlach experiment
established that electrons split evenly between ms= +1/2 and ms=-1/2, and any extra electrons show no preference to each other
pauli exclusion principle
no 2 e- can share the same set of 4 quantum numbers
paramagnetic
attracted to an external field due to unpaired e-
diamagnretic
not attracted to an external field because all the e- are paired
atomic size periodic trends
increases from left to right and upper to lower
1st ionization energy periodic trends
increases up periodic table and to the right
electron affintity periodic trends
increases up periodic table and to the right
covalent bonding
electrons shared between 2 or more atoms
exceptions to octet rule (3)
*expanded octet
* not enough e-
* odd number of e-
* not enough e-
* odd number of e-
free radicals
very reactive molecules, causes chain reactions in enviroment
electronegativity
the measure of the ability to an atom to attract e-
electron affinity
likelihood of gaining an electron
1st ionization energy
energy required to remove one e- from an atom
electronegativity periodic trends
increases up and to the right on periodic table
TRUE or FALSE: a molecule with resonance structures oscillates between each resonance structure
FALSE, the structure is actually a combination of the resonance structures
TRUE or FALSE: octet rule trumps electronegativity principle
TRUE
VSEPR theory
Valence Shell Electron Repulsion Theory
(says electrons repell each other)
(says electrons repell each other)
bond order formula
bond order= # shared pairs/ # of connections
as bond order increases, bond length...
decreases
as bond order increases, bond energy...
increases
TRUE or FALSE: the formation of a bond is endothermic
FALSE, its exothermic
electron geometry and hybridization for 2 connections
linear, sp
electron geometry and hybridization for 3 connections
trigonal planar, sp2
electron geometry and hybridization for 4 connections
tetrahedral, sp3
electron geometry and hybridization for 5 connections
trigonal bipyramidal, sp3d
electron geometry and hybridization for 6 connections
octahedral, sp3d
2 problems with VB theory
1) No adaquate description of resonance
2) doesn't describe bonding in species as it is known to exist
2) doesn't describe bonding in species as it is known to exist
4 primary quantities of intrest for gases
pressure, volume, temperature, amount
Boyle's Law
P1V1=P2V2
Charles's Law
T1/V1= T2/V2
Ideal Gas Law
PV=nRT
2 Major assumptions of IGL
1) gas molecules do not occupy physical space
2) intermolecular interactions do not exist
2) intermolecular interactions do not exist
Van der Waal's equation
[p+ a(n/v)^2][v-bn]=nRt
simple cubic structure
body centered cubic structure
face centered cubic structure
?H vap
the energy required to break the intermolecular interactions in a substance
3 primary intermolecular interactions
1) dipole-dipole
2) dipole-induced dipole
3) induced dipole-induced dipole
2) dipole-induced dipole
3) induced dipole-induced dipole
requirements for H-bonding
1) lone pair on an electronegatice element
2) polar X-H bond
2) polar X-H bond
key properties of liquids
1) surface tension (energy required to "pierce surface")
2) viscosity (resistance to flow)
2) viscosity (resistance to flow)
supercritical fluid
density like a liquid, temp is large enough to break intermolecular interactions so there is no surface tension or viscosity
two types of solids
crystal (ex: salt) and amorphous (ex: glass)
repeating unit in crystal solids
unit cells
About this deck
By: Laura Roscizewski
Textbook: Chemistry and Chemical Reactivity (with General ChemistryNOW CD-ROM)
Created: 2007-12-13
Size: 110 flashcards
Views: 430
Textbook:
Chemistry and Chemical Reactivity (with General ChemistryNOW CD-ROM)Created: 2007-12-13
Size: 110 flashcards
Views: 430
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
Dennis