Quarterly Review (up to ch. 10) Flashcards
(ch 1) extensive properties relate to
how much matter is present in a sample
(ch 1) intensive properties are characteristic of
the type of matter
(ch 2) law of constant composition: all samples of a pure substance contain
the same elements in the same proportions
(ch 2) law of multiple proportions: for different compounds formed from the same elements, the masses of one element that combine with a fixed mass of the other are in a
ratio of small whole numbers
(ch 2) atomic mass unit (u) is defined as exactly
1/12 off the mass of a carbon-12 atom
(ch 3) neutralization reaction: chemical reaction that takes place between
an acid and a base
(ch 3) combustion reaction: involve reactions with
oxygen
(ch 4) most ionic compounds and a few molecular compounds dissociate completely into ions in water and are known as
strong electrolytes
(ch 4) molarity: the number of
moles of solute per liter of solution
(ch 4) indicators that change color at or near the .. are used to determine when an equivalent amount of the solution of known concentration has been added
equivalence point
(ch 4) titration: a procedure to determine the quantity of one substance by
adding a measured amount of a second substance
(ch 4) gravimetric analysis: one component of a solution is …., separated from solution, dried, and weighed
precipitated selectively
(ch 5) heat transfers from … to …
warmer object; cooler object
(ch 5) universe=
system + surroundings
(ch 5) total energy =
KE + PE
(ch 5) potential energy: energy of
condition or position
(ch 5) enthalpy … be measured
cannot
(ch 5) state function: any property of a system that is determined by the
present conditions of the system
(ch 5) heat capacity: the quantity of heat required to increase the temperature of that object by
1 K
(ch 5) specific heat: heat needed to increase the temp of a
1 g sample by 1 K
(ch 5) hess’s law states that the change in enthalpy for an equation obtained by adding two or more thermochemical equations is the sum of the
enthalpy changes of the equations that were added
(ch 4) soluble ionic compounds without exceptions:
group 1 metals, NH4+, nitrates, perchlorates, acetates
(ch 4) soluble ionic compounds with exceptions
chlorides, bromides, iodides (except: ag+, Hg2^2-, Pb2+)
sulfates (hg2^2-, Pb2+, Sr2+, Ba2+)
(ch 4) insoluble ionic compounds:
carbonates (ex. group 1, nh4+)
phosphates (ex. group 1, nh4+)
hydroxides (ex. group 1, NH4+, Sr2+, Ba2+)
(ch 6) kinetic molecular theory:
gases are .. particles in … and … motion, and there are no forces of attraction or repulsion between any 2 gas particles
small; constant; random
(ch 6) kinetic molecular theory:
gas particles are very small compared with
sample volumes
(ch 6) kinetic molecular theory:
collisions of gas particles with each other and with the walls of the container are
elastic
(ch 6) kinetic molecular theory:
the average kinetic energy of the gas particles is proportional to the
temperature on the kelvin scale
(ch 6) kinetic molecular theory:
the gas particles do not all move at the same speed but have speeds given by the
maxwell-boltzmann distribution
(ch 6) kinetic molecular theory:
exceptions to the premises of the theory occur at
high pressures and low temps
(ch 6) 1 atm = … torr
760
(ch 6) 1 atm= …kPa
101.325 kPa
(ch 6) all gases have the same …. at a ….
average kinetic energy; given temperature
(ch 7) shorter wavelengths are
higher in energy
(ch 7) order of visible light
VIBGYOR
(ch 7) λ= (de Broglie)
h/mv
(ch 7) distribution of wavelengths changes with
temperature
(ch 7) greater value of n=
greater distance from nucleus
(ch 7) l values are
0 to n-1
(ch 7) ml values are
-l to l
(ch 7) pauli exclusion principle: no two atoms can have the
same set of four quantum numbers
(ch 7) aufbau principle: electrons go into
lowest available energy level
(ch 7) hund’s rule: electrons in degenerate orbitals do not pair until there is
one electron in each orbital of the set
(ch 8) isoelectronic series: same number of
electrons for group atoms and ions
(ch 8) atomic radii decrease across periods due to increase in
effective nuclear charge
(ch 8) atomic radii increase down groups due to increased
electron shielding→expanded radius
(ch 8) ionization energy: energy required to
remove 1+ electrons
(ch 8) in an isoelectronic series, the ionization energy is greatest for the species with the
most protons in the nucleus
(ch 8) electron affinity: energy change that accompanies the
addition of an electron to a gaseous atom/ion
(ch 8) in general, elements to the right side and at the top of the periodic table have … elecron affnities
exothermic (favorable)
(ch 9) lattice energy: energy required to separate one mole of crystal lattice into
corresponding ions
(ch 9) coulomb’s law:
E= kQ1Q2/r
(ch 9) the higher the bond order, the … and … the bond
shorter; stronger
(ch 9) bond order=
bonds/ # regions of bonding
(ch 9) dipole moment: measure of the
unequal sharing of electrons
(ch 9) bond energy: energy required to break
1 mol of bonds in a gaseous species
(ch 9) bond energies are
averages
(ch 9) born-haber cycle:
5 simpler reactions; most reactions don’t occur in one step
