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
manganite
MnO
how to determine a formula from the percent mass
change % to mass in g
convert to moles
divide all by the lowest number of moles (coefficient)
work equation
W=P(deltaV)
NH3 and NH4+
base and conjugate acid
HCl and Cl-
acid and conjugate base
hydrolysis of salts
conjugate acid/base combined with a cation/anion
one equivalent
amount of acid or base necessary to produce or consume one mole of H+ ions
percent yield
actual/theoretical *100%
examples of good electrolytes
ionic compounds
strong acids/bases
work on a system
positive
indicators
weak acids that change color when dissociating
how does change in enthalpy of reaction change with a reaction in reverse
negative
catalyst
any substance that increases reaction rate without being consumed in the reaction
does a cation have more or less electrons than protons?
less
do light or dark colors absorb more?
dark
standard state
reference point for measurement
units of specific heat capacity
J/g°C or cal/g°C
zero order
[A] versus time
-k slope
third law of thermodynamics
pure crystalline substances at absolute zero have zero entropy
hydroxide
OH-
Z
atomic number
number of protons
third law of thermodynamics
pure crystalline substances at absolute zero have zero entropy
what type of solution will require a high condosity
more metallic character than NaCl
pauli exclusion principle
no two electrons in a single atom can have the same four quantum numbers
first law of thermodynamics
energy cannot be created or destroyed
equation for coffee cup calorimeter
q=mc(deltaT)
alkaline earth metals
+2
reactive
methyl orange
3.7
positron emmision
emitted as a byproduct
conversion from C to K
°C+273=K
principal quantum number
shell and relative energy of the electron in the shell
conjugate acid
base plus a H+
does adding the salt of a weak acid raise and lower the pH and why
raise because the weak acid reforms, taking away H+
how to find Ka of a weak acid
Ka=(x^2)/([HA]-x)
coulombs law
F=(kqq)/r^2
nitrate
NO3-
Phosphate
PO4(3-)
condosity
concentration of NaCl solution that will conduct the same electronegativity as the solution in question
azimuthal quantum number
subshell of the orbital
s=0 p=1 d=2 f=3
double displacement reaction
AB + CD–> AD +CB
adiabatic
no heat exchange
sign of change in enthalpy for making bonds
negative
Na2CO3
salt of a weak acid (bicarbonate)
second law of thermodynamics
entropy of a system is always increasing
Group 1
alkali metals
positive change in gibbs free energy
non-spontaneous
second order
1/[A] versus time
k slope
non-metals
tightly held electrons
what is always true at the equivalence point
[titrant]=[analyte]
what type of heat exchange is analogous to current through w wire
conduction
change in temperature of adiabatic
non-zero
units of gibbs free energy
J
First quantum number
Principal (n)
pH+pOH=
14
Carbonate
CO3(2-)
Cyanide
CN-
with what variable does the equilibrium constant change
temperature
third quantum number
magnetic (Ml)
can you take ln(-x)
no
how many electrons in a d orbital?
ten
Kb=
[OH-][HA]/[A-]
strong bases have a ____ Kb and a ____ pKb
large, small
what equation shows that kinetic energy and temperature are directly proportional
KE=(3/2)KbT
energy is required to ____ bonds
break
zeroth law of thermodynamics
if A and B are in equilibrium and B and C are in equilibrium, then A and C must be in equilibrium
analyte
in beaker, unknown concentration
change in enthalpy of formation
formation of a compound from elements in their standard states
what are the condition for standard state
changes by table, reference
molar mass
mass of a given substance divided by the amount of substance
litmus
6.5
ionic character
measure of the polarity of a bond
the greater the difference between electronegativity means more ionic character
positive work
done on the system
arrheius base
give up OH- ions
what are the condition for standard state
changes by table, reference
change in standard enthalpy of formation of elements
0
Ka*Kb=
Kw
Balancing reactions
Carbons
Hydrogens
Oxygens
(Others)
single displacement reaction
A + BC–> AC +B
F block
lanthanides and actinides
change in enthalpy of solution
dissolution of a species in solution
Sulfuric acid
H2SO4
buffer solution
weak acid and weak base, often conjugates of one another
quantum mechanics
every electron in an atom has 4 numbers to define shell, subshell, orbital, and spin
ln(0.5)
negative
increase pressure
towards less molecules of gas
bronsted-lowry base
accept H+
does the indicator impact pH
no
zeroth law of thermodynamics
if A and B are in equilibrium and B and C are in equilibrium, then A and C must be in equilibrium
Manganate
MnO4(2-)
an increase in temperature of an endothermic reaction
increases the equilibrium constant
endothermic change in enthalpy for fromation
positive
relationship between size and charge stability
increases with size
negative change in gibbs free energy
spontaneous
lustrous
shiny
which halogens are gas at room temperature
Fl
Cl
Characteristics of metals
shiny, malleable, ductile, conductors, ionic bonds
NH4NO3
salt of a weak base (ammonium)
at what pH should an indicator change color
pH of equivalence
fundamental thermodynamic relation
deltaG=deltaH-T(deltaS)
groups
families
columns of the periodic table
same number of valence electrons
do non-metals form positive or negative ions
negative
arrhenius acid
give up H+ ions
relation between change in gibbs energy and Keq
deltaG= -RTln(Keq)
constant pressure implies
open container
which halogens are solid at room temperature
I
As
f=
v/lamda
area under the P vs V graph
work
positive work
done on the system
carbonic acid
H2CO3
how many electrons in a p orbital
six
strong acids (8)
HI HBr HCl H2SO4 HNO3 HClO4 HClO3 H3O+
what property defines an element
atomic number
electron affinity and the periodic table
increases up and across
specific heat capacity
heat capacity for an individual substance per unit mass
empirical formula
simplest formula for a compound
units of heat capacity
J/K or cal/°C
do bonding have attractive or unattractive electrons
attractive
sign of change in enthalpy for breaking bonds
positive
isothermal
constant temperature
ionic bonds
between a metal and a non-metal due to electrostatic attraction
formation of cations and anions
first law of thermodynamics
energy cannot be created or destroyed
are standard state and standard temperature and pressure the same
no
Ammonium
NH4+
calorimeters are used to calculate
change in enthalpy
at constant pressure, enthalpy change is equal to
q
energy (KE) of the ejected electron
energy minus the work function
anion
negative
Nitrite
NO2-
decrease pressure
towards more molecules of gas
effective nuclear charge
more electrons and more electron shells shield the outer electrons from the positive nucleus
do metals form positive or negative ions
positive
Naming acids
ate–>ic
ite–>ous
do metals or non-metals have lower melting points
non-metals
does a more stable bond have more or less energy than a less stable bond?
more energy
does forming bonds use or release energy?
releases
bonds form that result in a decrease in energy
change in enthalpy of reaction
products-reactants
halogens
-1
non-metallic
characteristics of non-metals
low melting points, covalent bonds
What charge does the nucleus have?
positive
change in enthalpy of fusion
enthalpy of change from liquid to solid
does [H+]=[OH-] always hold true at the equivalence point?
no, only strong acid and strong base titration
ionization energy and the periodic table
increases up and across
E=
hf
hv/lamda
hc/lamda
limiting reagent problems
balance reaction
determine how much product can be made with each reactant
entropy
measure of randomness or disorder in a system
what makes up the nucleus
protons and electrons
pKa+pKb=
14
is a cation smaller or lager than its neutral counterpart
smaller
groups 3-12
transition metals
work done by a system
negative
conduction
molecular collisions carry heat along a conduit such that high energy molecules collide with their neighbors, which in turn collide with their neighbors and spread the energy throughout
how many electrons in an s orbital
two
change in enthalpy of combustion
enthalpy value for combustion of a compound with oxygen to form carbon dioxide and water
coordinate covalent bond
covalent bond in which both electrons shared are donated by the same atom
change in enthalpy of reaction
products-reactants
transition metals
ductile, malleable, conduct electricity and heat, multiple oxidation states
heat of combustion
amount of energy released when a molecule is combustion with oxygen
temperature
average kinetic energy of molecules
decomposition reaction
AB–> A + B
equation for heat capacity
C=g/(deltaT)
convection
hotter portions rise and cooler portions sink in a fluid
when is the maximum buffering strength
[HA]=[A-]
cation
positive
negative natural log
between 0 and 1
work equation
W=P(deltaV)
Group 18
noble gases
negative work
done by the system
equation for coffee cup calorimeter
q=mc(deltaT)
exothermic change in enthalpy of formation
negative
sulfurous acid
H2SO3
exothermic change in enthalpy of formation
negative
conversion from C to K
°C+273=K
more energy available to do work with what change in entropy
positive
change in energy is equal to
q+w
Atomic weight
average weight of an element based on the relative abundance of isotopes
at constant pressure, enthalpy change is equal to
q
which halogens are liquid at room temperature
Br
gibbs free energy
amount of free or useful energy available to do work
unstable molecule has a _____ heat of combustion
high
black body radiator
perfect theoretical radiator
Sulfate
SO4(2-)
work function
energy required to eject an electron from the outermost shell
does a more stable molecule have a higher or lower heat of combustion?
lower
work on a system
positive
how to increase yield
use more reactants
shift equilibrium to the right (often by removing product as it forms)
mole
6.02e23 of anything
positive change in entropy
increase randomness
constant volume implies
rigid walls
change in standard enthalpy of formation of elements
0
radiation
electromagnetic waves emitted from a hot body into surrounding environment
alpha decay
loss of one He nucleus
A: 4 Z: 2
is an anion smaller or larger than its neutral counterparts
larger
ln(10)
positive
stable molecule has a _____ heat of combustion
low
