general chem Flashcards
effective nuclear charge _______ from left to right in periods
increases
as you move down elements of given group, ____ increases by one each time
principle quantum number
Zeff is _____ in groups
pretty consistent
atomic radius refers to ______, while ionic radius is dependent on ________
size of neutral element
how the element ionizes based on its element type and group #
______ is essentially the opposite that of all other periodic trends
atomic radius
while other periodic trends _________ going up and to the right, atomic radius _______ going down and to the right
increase
increase
metals ______ e- and become ______
lose
positive
non metals ______ e- and become ____
gain
negative
the nonmetals close to the metalloid line possess a ___ ionic radius than their counterparts closer to group VIIIA
larger
metals closer to the metalloid line have ______ e- to lose to achieve the electronic configuration seen in group VIIIA
more
noble gases are known as ____ because they have minimal chemical reactivity due to their filled valence shells
inert gases
the ng have _ boiling points
low
transition elements are considered to be ___ and have _ electron affinitites, ionization energies, and electronegativities
metals
low
transition metals are capable of losing what
different numbers of e- from s and d orbitals in their valence shells
_______ only need one more electron to have a noble gas-like configuration
halogens
chalcogens
group of non metals and mealloids
size e- in their valence electron shell
small atomic radii and large ionic radii
oxygen is most important element in this group
selenium important for microorganims
at high conc many of these elements can be toxic or damaging
alkaline earth metals
slightly higher effective nuclear charges and slighl smaller atomic radii than alkali metals
two e- in valence shell
alkali and alkaline earth metals togt called active metals
alkali metals
densities lower than other metals
one loosely bound e- in outermost shells
Zeff values low
largest atomic radii of all elemetns in respective periods
low ionization nrg
low e- affinity low electronegativity
pauling electronegativity scale
0.7 cesium
4.0 flourine
electronegativity ____ across period from l to r and __ in group from t to b
increases
decreases
e- affinity is what
energy dissipated by gaseous species when it gains and e-
electron affinity ____ across period from l to r and what from t to b
increases
decreases
noble gases have what electron affiniteis
zero
ionization energy is what
energy required to remove an e- from gaseous species
electron affinity is a what process
exothermic
ionization energy is a what process
endothermic
ionzation energy trend
increases from l to r
decreases t to b
first ionization energy will be ____ than second, will be_____ than third, etc…
smaller
smaller
what are the exceptions to the octet rule?
incomplete octet: stable with fewer than 8 electrons in their valence shell and include hydrogen 2, helium 2,lithium 2, beryllium 4, and boron 6
expanded octet: any element in period 3 and greater can hold more than 8 electrons, phosphorus 10 sulfur 12, chlorin 15, and many others
odd number of electrons: any molecule with odd number of valence electrons cannot distribute those electrons to give eight to each atom - nitric oxide 11
ionic bonding
one or more electrons from an atom with a low ionization energy - typically a metal, are transferred to an atom with high electron affinity - typically nonmetal
covalent bonding
electron pair is shared between two atoms - typically nonmetals that have relatively similar values of EN
coordinate covalent
if both shared electrons are contributed by only one of the two atoms
generally means lone pair of one atom attacked another atom with an unhybridized p orbital to form a bond
ionic compounds melting boiling point etc
high melting / boiling point
bond length
avg distance between two nuclei of atoms in a bond
bond energy
energy required to break a bond by separating its components into their isolated gaseous atomic states
electronic geometry
spatial arragenment of all pairs of electrons around the central atom, including both the bonding and lone pairs
molecular eometry
describes spatial arrangement of only the bonding pairs of electronsco
coordination number
number of atoms that surround and are bonded to a central atom
when orbitals overlap head to head, the resulting bond is a what bond
sigma
they allow for free roation about their axes because the electron density of the bonding orbital is a single linear acumulation between atomic nuclei
when orbitals overlap in such a way that there are two parallel electron cloud densities, a what bond is formed?
pi
do not allow for free rotation because the electron densities of the orbitals are parllel and cannot be twisted in such a way that allows continous overlapping of the clouds of electron densities
law of constant composition
any pure sample of given compound will contain same elements in an identical mass ratio
types of rxns
combination rxn
decomposition rxn
combustion
single displacement
double displacement
neutralization
_____ compounds make good electrolytes becaue they dissolve the most readily
ionic
_____ compounds are the weakest because they do not form current-carrying ions
nonpolar covalent compounds
collision theory of chemcial kinetics
the rate of a reaction is proportional to the number of collisions per second between the reaacting molecules
low activation energy and high temp make the negative exponnent of arrhenius equation ____ in magnitude and thus ____ the rate constant, k
smaller
increases
factors affecting rxn rate
reactant conntrations
temp
medium
catalysts
the greater the conc of the reactants, the ____ the number of effective collisions per unit time
greater
rxn rate will increase for all but zero order rxns
homogenous and heterogenous catalysis
catalyst is in same phase as reactants
caalye is in distinct phase
what are the only things that can change the rate of a zero order reaction?
temperature and addition of catalyst
isothermal processes
adiabatic processes
isobaric
isovlumetric / isochoric
systems temp is constant
no heat is exchaged between syste and enviornment
pressure is contstant
no change in volume
hess’ law states what
enthalpy changes of reactions are additive
boyles law
pressure and volume inversely related
charles’ law
volume and temperature are directly proportional
the ______ of a gas will increase with increasing partial pressu reo fthe gas
solubility
chelation
central cation can be bonded to the same ligand in multiple places
_______ and ______ cells house spontaneous reactions, while _____ cells contain nonspontaneous reactions
galvanic
concentration
electrolytic
purpose of salt bridge
exchange anions and cations to balance, or dissipate newly generated charges
energy density in batteries
measure of a battery’s ability to produce power as a function of its weight
isoelectric focusing
separate amino acids or polypeptides basedo n their isoelectric points
