Chemistry fundamentals Flashcards
ammonium
NH4+
Hydronium
H3O+
Acetate
CH3CO-
Bicarbonate
HCO3-
Cyanide
CN-
Hydroxide
OH-
Nitrate
NO3-
Nitrite
NO2-
Perchlorate
ClO4-
Carbonate
CO3(2-)
Sulfate
SO4(2-)
Sulfite
SO3(2-)
Phosphate
PO4(3-)
covalent bonds
are only formed between nonmetal elements
bond dissociation energy
the energy necessary for a complete separation of the bond is given by the vertical distance on the graph between the energy at the bond length and zero
nonpolar covalent bond
when electrons are shared equally between molecules with equivalent electronegativities
polar covalent bonds
when electrons are not shared equally because of a difference in electronegativity
ionic bonds
occur most often between metals and nonmetals
dipole moment
is an example of intermolecular forces and occurs when the center of positive charge in a bond does not coincide with the center of negative charges. given by the equation mew=qd. q is the magnitude of the charge at either end and d is the distance between the centers of charge
strongest type of dipole-dipole interaction
hydrogen bond
hydrogen bonds occur between
a hydrogen that is covalently bound to flourine, oxygen, and nitrogen
cations that have large and small charges are designated differently as
ous for small
ic for big
oxyanions are named
ate as the more oxygens
itse as the least amount of oxygens
for acids the names for more oxygens and less
more = ous less= ic
N units
kg ms-2
empirical formula
is the smallest ratio of whole numbers that can be used to represent these proportions
molecular formula
represent the exact number of elemental atoms in each molecule
percent yield equation
actual yield/theoretical yield *100
difference between thermodynamic and kinetic
thermodynamic product is more stable but it requires higher energy input and is produced more slowly. the kinetic product is less stable but can be formed more rapidly because the required energy input is lower. high temps favor the thermodynamic product while low temps favor the kinetic product
rate constant for chemical kinetics
rate constant is affected by pressure, catalysts, and temperature
reaction rate
describes how quickly the concentration of the reactants or products are changing over the course of the reaction
rate constant
molarity per second
steps after the slow step do not what? steps before the slow step do what?
contribute to the rate law while ones before do
heterogenous catalyst
is in a different phase than the reactants and products, such as when gas or aqueous particles react on a solid
reaction rates can be enhanced by
increasing the surface area of a catalyst
homogenous catalyst
is in the same phase as the reactants and products
a catalyst affects the
kinetics of a reaction but not the thermodynamics
reaction rate of reactions in gas vs liquid
in gas and liquids the reaction rate will be the similar in similar concentrations. The rate of a reaction is affected by stirring or shaking in liquids as well as increasing the temperature
radioactive decay
concerns atoms that spontaneously break apart
half-life
is the length of time necessary for one half of a given amount of substance to decay
half-life follows what order
first order reaction and the constant can be expressed as At=Aoe^(-kt)
beta-decay what particle is released
a neutron is broken down but a proton is added. meaning that the mass number stays the same. a neutrino is released which is a massless particle
