exam 1 part 3 Flashcards
(22 cards)
sublimation
solid to gas
decomposition
gas to solid
fusion
liquid to solid (freezing)
diagonal part of heating curve formula
q=mCp(^t)
horizontal line of heating curve formula
q=m(^H)
triple point
all 3 states of matter exist at this point
critical point
where critical temp = critical pressure coincides (very top of liquid/gas line)
supercritical fluid
temps beyond critical point (liquid and gas phases are indistinguishable)
triple point of CO2
5.11atm
simple cubic unit cell
contains only one atom, length = 2r, and coordination number is 6
body centered cubic unit cell
contains 2 atoms, coordination number 8
face centered cubic unit cell
contains 4 atoms and coordination number 12, strongest IMF than others
coordination number
number of ions/atoms that immediately surround a atom/ion
cubic unit cell volume
v = a(length)^3
molecular solids
non-metal and non-metal, strong covalent bonds, weak IMFs and mod low melting points
ionic solids
non-metal and metal plus polyatomics, IMFs are stronger, high melting points (2nd highest), deals with lattice energy
lattice energy
energy given off when separate gaseous ions come together to form a solid ionic compound (1 mol)
ionic solids depend on what 1st then 2nd
increasing charge and decreasing size
higher lattice energy causes
higher melting point
metallic solids (type of atomic solid)
metal only, like iron and silver, varying melting points (are lower than ionic) and very good conductors
covalent network
highest melting point, harder than metallic and don’t conduct electricity
examples of covalent network
C (graphite and diamond), SiO2, SiC
