Gen Chem 1 Flashcards
change in heat of isothermal
non-zero
are standard state and standard temperature and pressure the same
no
half-life
amount of time required for exactly one half of the mass of the substance to disappear due to radioactive decay
work
energy transfer via force or via change in volume at a constant pressure
what happens below pH 7
[H+] > [OH-]
equation for bom calorimeter
q=C(deltaT)
group 2
alkaline earth metals
conjugate base
acid without its H+
beta decay
neutron to a proton, ejection of electron
covalent bonds
between non-metals and involves the sharing of electrons
work
energy transfer via force or via change in volume at a constant pressure
percent mass
mass of an element/ mass of the compound *100%
units of entropy
J/K
reaction rate
change in molarity of reactants per second
attractive electrons in or out of phase
in phase
work done by a system
negative
strong acids have a ____ Ka and a ____ pKa
large, small
change in temperature of isothermal
zero
bronsted-lowry acid
donate H+
endothermic change in enthalpy for fromation
positive
the horizontal regions on a titration curve
buffer
how does change in enthalpy of reaction change with a reaction in reverse
negative
second law of thermodynamics
entropy of a system is always increasing
what is the reverse of vaporization
condensation
area under the P vs V graph
work
atomic radius and the periodic table
increases down and left
molecular formula
same as or multiple of the empirical formula
bicarbonate
HCO3-
Q
reaction proceeds to the right
enzymes
catalyze biochemical reactions
symbol for specific heat capacity
c (lowercase)
Chlorite
ClO2(2-)
Permanganate
MnO4-
magnetic quantum number
orbital orientation
-l to l
Q>K
reaction proceeds to the left
pKw is equal to
pH=pOH=14
What is needed for a reaction to occur (2 things)
enough energy to overcome the activation energy
AND
the correct spatial orientation
pH equals
-log[H+]
A
mass number
number of protons and neutrons
negative change in entropy
decrease randomness
heisenberg uncertainty principle
the more precisely one property is measured the less precisely the other can be known
what happens above pH 7
[H+]
second quantum number
azimuthal (l)
actual yield
how much product is actually made
the only elements to produce a magnetic field
Fe, Co, Ni
when is maximum entropy
equilibrium
Chlorate
ClO3-
first order
ln[A] versus time
-k slope
Noble gases
+/-0
Stable
equation for bom calorimeter
q=C(deltaT)
q=change in enthalpy is only true at
constant pressure
is a lewis acid an electrophile or nucleophile
electrophile
Metals
Loosely held electrons
isotopes
atoms with the same number of protons and different numbers of neutrons
different forms of an element
calorimeters are used to calculate
change in enthalpy
do light or dark colors radiate more?
dark
phenylphtalien
9.3
amphoteric
can act as an acid or base
enthalpy
energy contained within chemical bonds
le-chatelier’s principle
systems at equilibrium that experience change will shift to reduce the effects of that change
strong bases (8)
Group IA hydroxides NH2- H- Ca(OH)2 CaO Sr(OH)2 Ba(OH)2 Na2O
titration
drop by drop mixing of an acid and a base with an indicator
bond dissociation energy
bond energy
group 17
halogens
example of amphoteric molecule
water
spin quantum number
+/-1/2
electronegativity and the periodic table
increases up and across
pOH equals
-log[OH-]
Kw is equal to
10^-14=[H30+][OH-]
what happens at pH of 7
[H+]=[OH-]
hypochlorite
ClO-
periods
rows of the periodic table
elements have the same valence shell
ways to increase entropy (5)
more particles form a gas increase volume increase temperature increase complexity/disorder
pKa of strong acids
below 0
fourth quantum number
spin (ms)
q=change in enthalpy is only true at
constant pressure
negative work
done by the system
is bonding or anitbonding higher in energy
antibonding
is 3d or 4s higher in energy?
3d
isobaric
constant pressure
what is the pH at equivalence for weak base/strong acid
below 7
units of energy
J or cal
radioactive decay
process by which unstable atoms change their chemical composition over time
titrant
being added, known concentration
how many electrons in all shells after the first
8
What is the Bohr model?
Atomic structure
+ nucleus with orbits of electrons
double displacement reaction is also known as
metathesis
molecular weight
mass of the elements in a molecule summed together
perchlorate
ClO4-
metallic character and the periodic table
increases down and left
an increase in temperature of an exothermic reaction
decreases the equilibrium constant
increase in entropy is spontaneous or nonspontaneous
spontaneous
enthalpy
energy contained within chemical bonds
relative heat of combustion
+1 for C
-0.5 for O
How does metallic character change with size?
smaller are less metallic
reverse of fusion
melting
is 5s or 4p higher in energy?
5s
electrolytes
compounds that fully dissociate in water
electron capture
proton to neutron, capture of electron
what is the pH at equivalence for weak acid/strong base
above 7
how many electrons in the first shell
two
lewis acid
accept electron pair
lewis base
donate electron pair
by what mechanism are covalent bonds broken and reformed?
radical reaction
heat capacity
amount of energy a system must absorb to give a unit change in temperature
change in energy is equal to
q+w
standard state
reference point for measurement
what equation shows that kinetic energy and temperature are directly proportional
KE=(3/2)KbT
Ka=
[H+][A-]/[HA]
unit of enthalpy
J
what two measures does the uncertainty principle refer to?
position and momentum
equation for specific heat capacity
c=q/m(deltaT)
q-mc(deltaT)
change in heat of adiabatic
zero
henderson-hasselbach
pH=pKa+log(A-/HA)
does a catalyst change the equilibrium constant
no
energy levels
represent the energies of the electrons in an atom
theoretical yield
prediction of yield under ideal conditions
what is the pH at equivalence for strong base/strong acid
7
unit of enthalpy
J
half equivalence opint
pH=pKa
symbol for heat capacity
C (capital)
what is the pH at equivalence for strong acid/strong base
7
alkali metals
+1
reactive, soft, explode when exposed to water
equilibrium
reactants and products are at concentrations that have no further tendency to change with time
forward and reverse reactions proceed at the same rates
change in enthalpy of vaporization
enthalpy of change from liquid to gas
electron configuration
set of quantum numbers and the number of electrons in each
order the subatomic particles by size
protons=neutrons»>electrons
change in enthalpy of formation
formation of a compound from elements in their standard states
does an anion have more or less electrons than protons
more
