DAT FINAL REVIEW FOR CHEM Flashcards
compare energy levels 1 and 2 with 4 and 5
the difference between energy levels 1 and 2 is larger than the difference between energy levels 4 and 5
why are transition metals brightly colored?
Also known as the metals in the d block….. its because the funky way that d orbitals absorb colored light and promoted to higher energy orbitals
what is pauli exclusion principle
no 2 electrons in same atom can have same 4 quantum numbers
what is hunds rule
electrons fill up orbitals one at a time
what is aufbau principle?
electrons fill the lowest energy orbital first
what is paramagnetic attracted to magnets
because it has unpaired electrons
why is diamagnetic repelled by magnets?
it has all paired electrons
02 is what
paramagnetic
N2 is what
diagmagnetic
Odd number of electrons can indicate what
paramagnetic
and even number of electrons can indicate what
either paramagnetic or diamagetic
what is the mnemonic for wave frequency
roman men invented very unusual x ray guns
The R in roman is the lowest energy = highest wave length
___ in energy equals ____ in frequency equals ___ in wavelenth
increase
increase
decrease
ionic bonds properties
high melting point, high bp
molecular bonds properties
low melting point do not conduct electricity
net work covalent bond properties
high melting point, high boiling point, hard, do not conduct electricity…. EX.
metallic bond properties
variable hardness and melting point
conduct electricity and heat
shiny and malleable
what is lattice energy
amount of energy to completely separate an ionic compound
sp angle
180 linear
sp2 angle
120 trigonal planar
sp3 angle
109.5 tetrahedral
geometry of sp2 with a pair of electrons
bent
geometry of sp3 with a a pair of electrons
trigonal pyramidal
geometry of sp3 with 2 pairs of electrons
bent
alkali metals have ___ ionization energy
low
alkaline earth metal have ___ ionization energy
low
halogens are ______ oxidizing agents
good
compare o2 and o3 in terms of oxidizing agent and what it likes to react with?
o2 is good oxidizing agent but o3 is a better one!
likes to react with metal to form metal oxides
ion sizes in terms of minus and positive
the more minus the ion is…. the bigger
the more positive the ion is…. the smaller
what is electron affinity?
energy given off when an atom gains electrons
what is ionization energy
energy required to remove electron from an atom
gas behaves most ideally in what conditions
low pressure and high temp
what is the ideal gas assummption
- volume/ size of gas are insignificant
- most accurate at low pressure - gas collision are elastic, no intermolecular forces
- most accurate at hig temp and low intermolecular forces - average kinetic energy of gas depends on only temp
increase in intermolecular forces causes what?
increase bp, viscosity, surface tension
decreased vapor pressure
simple cubic
1 atom per unit cell
body centered cubic
2 atoms per unit cell
face centered cubic
4 atoms per unit cell
top part of solid - liquid - gas is what???
going from gas to solid
consume heat (endothermic, positive delta h and positive delta s)
bottom part of solid- liquid - gas is what???
going from gas to solid
produce heat (exothermic, - delta h and - s)
another word for melting is w
fusion
going from gas to solid is known as what
depostion
going from solid to gas is known as what
sublimination
liquid water is _____ dense than solid while other solids are denser as solid
more
Water’s lower density in its solid form is due to the way hydrogen bonds are oriented as it freezes: the water molecules are pushed farther apart compared to liquid water. 1: Ice Density: Hydrogen bonding makes ice less dense than liquid water.
what is normal boiling point?
temp at which vapor pressure of liquid is equal to 1 atm
solubility rule (solubles)
group 1 metal cations no3- clo4- acetate c2h3o2- nh4+
solubility rule insolubles
silver ag lead pb sulfide S2- hydroxide Oh- dimercury Hg22+ carbonate Co32- phosphate Po43-
what is colligative property?
depend on # of solute and not nature of solute present in solvent
how to find spectator ions from net ionic equation
NO REACTION
—– if all the states are aq. reaction only happens if there is aleast one solid
step 0. balance
step 1. determine the solubility if not given
step 2. pair the cations and anions to give reactant and product
step 3. cut everything in half
step 4. cancel out things that are the same
step 5. the things you canceled out are the spectator ions
what happens to the solids solubility as temp increases?
the solubility of the solid also increases
think of hot chocolate mix
what happens to the gas solubility as temp increases
lowers…..
when temp gets higher that means it will increase the gas molecules speeds. which will cause more and more of those gas molecules to escape and leave the liquidt
what happens to gas solubility when theres an increase in pressure?
goes up! when you compress a cup with gases in it… it will keep more gasses in it therefore keeping more gas molecules in the cup
increase in solute in solid will do what to the freezing point?
decrease it
increase solute in liquid will do what to the freezing point?
raise it
breaking bonds is an what kind of process
endothermic… heat is consumed as this happens
making bonds is what kind of process?
exothermic… heat releases as this happens
what never appears in a rate law?
intermediates
what only appears in rate law
the reactant
zero order ____- concentration = ____ half life
decreased
decreased
first order ___- half life - independent of
constant
[A]
second order ____ concentration = ___ half life
decreased
increased
larger activation energy =
slower step
intermediates are only found in the
middle… not in the reactant or the product
what does catalyst do
lowers EA
provides alternative pathway
does not shift equilibrium
collision theory
- both molecule collide
- collide with enough energy
- collide with correct 3d orientation
___ temp = ___ K = ____ rate
increase
increase
increase
__ Ea = __ K= __ rate
decrease
increase
increase
for any part of equilibrium constant Ex. Kc Kp and Keq what is ONLY included
aq and gas
Q is less than K.. what is the result
shift rights (products)
what is the difference between Q and K
K is equilibirum
Q may or may not be equilibrium
Q is greater than K.. what is result
shift left (reactant)
Q=K what is result?
equilibrium
Q > ksp equals what
precipitation
Q < ksp equals what
no precipitation
what is le chateliers principle
if a system at equilibrium is disturbed, then it will shift in which ever direction it has to, to restore that equilibrium
strong acids in order
HI HBR HCl ( binary acids)
Hclo3 Hclo4
h2s04
Hno3
trend for strong acid
electronegativity and down
strong base
Group 1 metals with OH
these are group 2 Mg(OH)2 Ca(OH)2 Sr(OH2 Ba(OH)2
types of heat transfer
conduction
convection
radiation
conduction - direct contact: bites pizza
convection - motion of fluid: cook by hot air (oven)
radiation - electromagnetic radiation ( Infrared light)
anode is the site of what?
oxidation
cathode is the site of what
reduction
electrons always flow in what direction in voltaic cell
anode to cathod
the voltaic and galvanic cells the anode is ___ and cathode is ____
negative and positive
in electrolytic cells, the anode is _____ and the cathode is ____
positive
negative
function of salt bridge
let counter anions flow into the anode, and cations to the cathode
anode metals _____ mass and cathode metal ____ mass
loses
gains
the ideal gas law assumptions
- all gas molecules are in constant, raid, and random motion
- there are no attractive or repulsive forces (IM forces) between the gases
- the volume of the molecules is negligibly small compared to the volume of the gas
- all collisions within the gas are perfectly elastic
- the average kinetic energy of the gas molecules depends only on the temp of the system
