Lecture Notes Flashcards
Types of Chemistry
organic- carbon biochemistry- carbon life physical- physical inorganic- everything else analytical- what and how much
goal of chemistry
understand the atoms and molecules that compose them
observe
measure, interpret, calculate publish
exact
not used in sig figs
inexact
used in sig figs
accurate
how close a measurement to the true value
precison
how close a set of measurements are to each other
add/sbutract
least amount of decimal places
matter
anything that occupies space and has mass
what isnt matter
heat, electricity, and light
types of matter
state- physical form,
composition- basic components that make it up
states of solids
crystalline
amorphous
ionic compound-
metal-nonmetal
covalent compound
nonmetal-nonmetal
diatomic molecules
H2, O2, N2, I2, Cl2, Br2, F2
Universe
helium, hydrogen,
earth’s crust
oxygen, silicon, aluminum, hydrogen, calcium, magnesium
body
carbon, hydrogen, nitrogen, oxygen
isotope
different # of nuetrons
metal ion
cation
nonmetal ion
anion
electron level
1 s2 2 s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6
matter
pure substance or mixture
element or compound and heterogenous or homogenous
compounds ionic or molecular
most oxygen
ate
one less oxygen
ite
acid
ate to ic
ite to ous
classification by atom rearrangement
A+B=C- combination
C= A+B- decmposition
X+YZ=Y+XZ- single replacement
AX+BY=AY+BX- double replacement
acid/base
salt and H2O
combustion
reacts with O2= CO2+H2O
strong acids
HCl HNO3 H2SO4 HBr HI
what are bases
bitter, feel slippery
strong bases
group 1 and 2
and hydroxide
molarity
mol/vol (L)
dilution equation
m1v1=m2v2
acid-base equation
m(a)v(a)=m(b)v(b)(a/b)
oxidization
loss of electrons
reduction
gain of electrons
oxidizing agent
solid
reducing agent
aqueous
ozone
o3
physical characteristics of gases
gases assume the volume and shape of the container
gases are the most compressible state of matter
gases will mix evenly and completely when confined to the same container
gases have much lower density than liquids and solids
gases
shape indefinite
volume indefinite
1 atm
760 mm Hg
gas law
PV=nRT
what releases energy
exothermic
what absorbs energy
endothermic
types of energy
kinetic- motion
potential- position
energy
capacity to do work
energy=
work=force*distance
change in energy
q+w
open sys
mass and energy
closed
energy
isolated
nothing
heat
q=mcchange in time
-
work done by the system on the surroundings
+
work done on the system by the surroundings
+
heat absorbed by the system from the surroundings
endothermic
-
heat absorbed by the surroundings from the system
exothermic
-q sys
qcal+qcontents
101.325 J
1 atm*atm
qcal
Ccal*change in temp
qcon
mconCchange in temp
e
h*nu(frequency)
nu (frequency)
c/lambda(wavelength)
e
ch/lambda(wavelength)
En
Rh(1/ni^2-1/nf^2)
quantum numbers
n- energy level, =1,2,3
l- sublevel, =0, n-1
ml= orientation in space, = 0+-l
ms= spin, = -1/2 or +1/2
of orbitals
2l+1
energy levle- n^2
shpaes of l
l=0 spherical
l=1 principal
l=2 dumbbell
l=3 fundamental
electron config
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10
noble gas Arsenic
[Ar] 4s2 3d10 4p3
shielding and pentration
closer shield electrons and harder to get to outer electrons
effective nuclear charge
ionize an atom easy or hard 1,2,3 cations 5,6,7 anions electron affinity (add) 1,2,3 not taking more electrons 5,6,7 easily take up electrons ionic radius- cation radi smaller, ano- radi higher
Cu +
Cu 2+
4s0 3d10
4s0 3d9
KE
1/2 (mv^2)
state function
thermodynamic quantity whose value depends only on the state at the moment, i. e., the temperature, pressure, volume
En
-2.18*10^-18(1/n^2)
diamagnetism
presence of paired spins
paramagnetism
prescence of unpaired spins
VSEPR
valance shell electron pair repulsion
