Hazards of Materials Flashcards
Paint Filter Test
Used to determine if a material is liquid - by hazardous waste definition. Liquid if 100 grams of material passes through a specified filter in 5 minutes
Change of Physical State (phase change)
A material changes from solid to liquid, liquid to gas, solid to gas, or vise-versa
Freezing Point
The point at which a chemically stable material will be solid below that temperature and liquid above it.
Melting Point
The point at which a chemically stable material will be solid below that temperature and liquid above it.
Boiling Point
The point at which a chemically stable material will be liquid below that temperature and gas above it.
Sublimation
Phase change of a material that transitions directly from solid to gas (dry ice)
Volatilization
evaporation of liquids and some solids at temperatures well below their boiling point
Vapor Pressure
Pressure of gas above the condensed phase at a particular temperature in a closed container
BLEVE
(Bleh’ -vee) Boiling Liquid Expanding Vapor Explosion highly energetic, occurs when material in a closed container is heated to point where vapor pressure is enough to rupture the container
Boiling Liquid Expanding Vapor Explosion
highly energetic, occurs when material in a closed container is heated to point where vapor pressure is enough to rupture the container
Volatile Material
any material with a vapor pressure greater than 1 mm Hg
Density
Ratio of mass to volume d= m/v
Specific gravity
ratio between the density of a material and the density of water specific gravity = SGx = dx/dH2O
STP
Standart Temperature and Pressure
STP = 1 atm & 25o C
Ideal Gas Law
PV = nRT
P = pressure
V = Volume
n = amount (in moles)
R = Ideal Gas Constant (8.3144598(48) J mol−1 K−1[1])
T = Temperature
Vapor Density
Vapor Density = vapor dx
= realtive gas densityx = RgasDx
=dx/dair = MMx/MMair = MMx/29
dx = density of the gas
dair = density of air
MMx = molar mass of the gas
MMair = molar mass of air = 29
Solution
mixture that is uniform in composition and state of matter
also called homogeneous
also includes solid-solid solutions
Term not applied to gases
Solvent
The most abundant compound in a solution
Solute
all other compounds in a solution other than most abundant compound (the solvent)
Atomic Number
The number of protons in an atom.
Defines the element that the atom represents
Atomic Mass Number
sum of all protons and neutrons in an atom
variable (number of protons can change)
Isotope
atoms with same atomic number but different atomic mass number
(different number of neutrons)
nuclide
nucleus of a specific isotope
Atomic Nomenlature
Example
Element
Purest form of a substance and consists of one or more atoms
Ion
atom, or group of atoms that has gained or lost one or more electrons giving it a positive or negative charge
Cation
positively charged ion
anion
negatively charged ion
Noble Gases
virtually inert elements
5 common properties of metal
- luster (shinyness)
- malleability (able to be shaped by a hammer)
- ductility (capible of being drawn when pulled)
- heat conductor
- electrical conductor
How are elements grouped on Periodic table
Based on number of orbitals and electrons within the orbitals
What are the types of orbitals
and how many electrons
s : 2 e- per shell
p : 6 e- per shell
d : 10 e- per shell
f : 7 e- Shell
what are the noble gases and why are they stable
Elements in column 18
they are stable because s & p orbitals are completely filled
He, Ne, Ar, Kr, Xe, Rn, Uuo
Valence Electrons
Electrons avaialble for bonding, make up the outermost shell
except d & f orbitals where outer s fills up before d and f (4s fills before 3d)
Why are elements in same column similar
elements are similar due to similar valence electron configuration
C & Si have same number of electrons in outer p shell (2)
Why are atoms in d & f transition metals similar
similar because an outer s shell is filled before the d & f
4s before 3d
Aufbau principle
(German for buildup principal)
electrons will occupy lowest energy level available
- 1s;
- 2s, 2p;
- 3s, 3p;
- 4s, 3d, 4p;
- 5s, 4d, 5p;
- 6s, 4f,5d,6p;
- 7s, 5f
Alkali metals
Group 1
softest & most reactive metals
Li, NA, K most common in Haz Management
Highly reactive, generates heat and hydrogen when mixed with water
reacts strongly with all acids and most organics
K & Na Dangerous When Wet hazardous category
Alkaline Earth Metals
Group 2
Similar to alkali metals, not as soft or reactive
(Be does not react with H2O, Mg reacts slowly w/ hot H2O, Ca turning react with H2O similar to water)
d transition metals
Group 3 - 12
properties similar w/in each group (column)
Similar across row
Similar because d orbitals filling with electrons while outer s shell (valence electrons) already full
Groups 13-18
Periodic table
Widely varying properties
metals
metalloids
non-metals
includes halogens (group 17)
and noble gases (group 18)
What happens when valence orbitals are full (ions)
Stability of ion increases significantly, similar to noble gases becuase all s & p outer orbitals are full
Ca2+
Cl-
Ionic Bond
Valence electron transfered from one atom to other
Covalent Bond
Valence electron shared between two atoms
Could be shared equally or unequally
more difference in electronegativity, more unequally shared
electronegativity
1/2 (ionization energy - electron affinity)
Metals least electronegative
Halogens most electronegative
Polar Covalent Bonds
some diference in Electronegativity - electron not equally shared
Metalic Bonding
described by electron sea theory
Ultimate delocalized covalent boning
metals exist in 3D lattice of cations surrounded by electrons not attached to a particular cation
bond polarity
results when Electrons are not shared equally, giving bond an uneven charge
bond dipole
result of unequal charge distribution (polar bond)
molecule polarity
happens when bond dipoles arranged so they don’t cancel each other out.
H2O Polar
hydrogen bonding
polar composition of water molecule allows water molecules to bond wiht each other, making water bond stronger, and less likely to turn to gas
Water turns to gas at much higher temperature than similar compounts
Solubility
ability of substance to disolve into solvent
Solvent
the most abundent compound in a solute/solvent combination
-ic
higher oxidation state of ion
ie Fe(III) - Fe3+ - Ferric Iron
–ous
lower oxidation state of ion
ie Fe(II) - Fe2+ - Ferrous Iron
Common Oxidation State of
iron
2+ Ferrous
3+ Ferric
Common Oxidation State of
lead Pb
2+ plumbous
4+ plumbic
Common Oxidation State of
tin
2+ stannous
4+ stannic
Common Oxidation State of
Copper
1+ cuprous
2+ cupric
monoatomic anions end in suffix
-ide
SnCl2 - Stannous Chloride
MgO - Magnesium oxide
Na2S - Sodium sulfide
mono-
1
di-
2
tri-
3
tetra-
4
pent-
5
hex-
6
hept-
7
oct-
8