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CHMM -Dave's Deck > Hazards of Materials > Flashcards

Hazards of Materials Flashcards

1
Q

Paint Filter Test

A

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

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2
Q

Change of Physical State (phase change)

A

A material changes from solid to liquid, liquid to gas, solid to gas, or vise-versa

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3
Q

Freezing Point

A

The point at which a chemically stable material will be solid below that temperature and liquid above it.

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4
Q

Melting Point

A

The point at which a chemically stable material will be solid below that temperature and liquid above it.

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5
Q

Boiling Point

A

The point at which a chemically stable material will be liquid below that temperature and gas above it.

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6
Q

Sublimation

A

Phase change of a material that transitions directly from solid to gas (dry ice)

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7
Q

Volatilization

A

evaporation of liquids and some solids at temperatures well below their boiling point

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8
Q

Vapor Pressure

A

Pressure of gas above the condensed phase at a particular temperature in a closed container

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9
Q

BLEVE

A

(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

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10
Q

Boiling Liquid Expanding Vapor Explosion

A

highly energetic, occurs when material in a closed container is heated to point where vapor pressure is enough to rupture the container

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11
Q

Volatile Material

A

any material with a vapor pressure greater than 1 mm Hg

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12
Q

Density

A

Ratio of mass to volume d= m/v

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13
Q

Specific gravity

A

ratio between the density of a material and the density of water specific gravity = SGx = dx/dH2O

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14
Q

STP

A

Standart Temperature and Pressure

STP = 1 atm & 25o C

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15
Q

Ideal Gas Law

A

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

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16
Q

Vapor Density

A

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

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17
Q

Solution

A

mixture that is uniform in composition and state of matter

also called homogeneous

also includes solid-solid solutions

Term not applied to gases

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18
Q

Solvent

A

The most abundant compound in a solution

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19
Q

Solute

A

all other compounds in a solution other than most abundant compound (the solvent)

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20
Q

Atomic Number

A

The number of protons in an atom.

Defines the element that the atom represents

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21
Q

Atomic Mass Number

A

sum of all protons and neutrons in an atom

variable (number of protons can change)

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22
Q

Isotope

A

atoms with same atomic number but different atomic mass number

(different number of neutrons)

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23
Q

nuclide

A

nucleus of a specific isotope

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24
Q

Atomic Nomenlature

A

Example

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25
Q

Element

A

Purest form of a substance and consists of one or more atoms

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26
Q

Ion

A

atom, or group of atoms that has gained or lost one or more electrons giving it a positive or negative charge

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27
Q

Cation

A

positively charged ion

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28
Q

anion

A

negatively charged ion

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29
Q

Noble Gases

A

virtually inert elements

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30
Q

5 common properties of metal

A
  1. luster (shinyness)
  2. malleability (able to be shaped by a hammer)
  3. ductility (capible of being drawn when pulled)
  4. heat conductor
  5. electrical conductor
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31
Q

How are elements grouped on Periodic table

A

Based on number of orbitals and electrons within the orbitals

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32
Q

What are the types of orbitals

and how many electrons

A

s : 2 e- per shell

p : 6 e- per shell

d : 10 e- per shell

f : 7 e- Shell

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33
Q

what are the noble gases and why are they stable

A

Elements in column 18

they are stable because s & p orbitals are completely filled

He, Ne, Ar, Kr, Xe, Rn, Uuo

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34
Q

Valence Electrons

A

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)

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35
Q

Why are elements in same column similar

A

elements are similar due to similar valence electron configuration

C & Si have same number of electrons in outer p shell (2)

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36
Q

Why are atoms in d & f transition metals similar

A

similar because an outer s shell is filled before the d & f

4s before 3d

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37
Q

Aufbau principle

A

(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
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38
Q

Alkali metals

A

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

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39
Q

Alkaline Earth Metals

A

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)

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40
Q

d transition metals

A

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

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41
Q

Groups 13-18

Periodic table

A

Widely varying properties

metals

metalloids

non-metals

includes halogens (group 17)

and noble gases (group 18)

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42
Q

What happens when valence orbitals are full (ions)

A

Stability of ion increases significantly, similar to noble gases becuase all s & p outer orbitals are full

Ca2+

Cl-

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43
Q

Ionic Bond

A

Valence electron transfered from one atom to other

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44
Q

Covalent Bond

A

Valence electron shared between two atoms

Could be shared equally or unequally

more difference in electronegativity, more unequally shared

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45
Q

electronegativity

A

1/2 (ionization energy - electron affinity)

Metals least electronegative

Halogens most electronegative

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46
Q

Polar Covalent Bonds

A

some diference in Electronegativity - electron not equally shared

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47
Q

Metalic Bonding

A

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

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48
Q

bond polarity

A

results when Electrons are not shared equally, giving bond an uneven charge

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49
Q

bond dipole

A

result of unequal charge distribution (polar bond)

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50
Q

molecule polarity

A

happens when bond dipoles arranged so they don’t cancel each other out.

H2O Polar

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51
Q

hydrogen bonding

A

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

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52
Q

Solubility

A

ability of substance to disolve into solvent

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53
Q

Solvent

A

the most abundent compound in a solute/solvent combination

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54
Q

-ic

A

higher oxidation state of ion

ie Fe(III) - Fe3+ - Ferric Iron

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55
Q

–ous

A

lower oxidation state of ion

ie Fe(II) - Fe2+ - Ferrous Iron

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56
Q

Common Oxidation State of

iron

A

2+ Ferrous

3+ Ferric

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57
Q

Common Oxidation State of

lead Pb

A

2+ plumbous

4+ plumbic

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58
Q

Common Oxidation State of

tin

A

2+ stannous

4+ stannic

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59
Q

Common Oxidation State of

Copper

A

1+ cuprous

2+ cupric

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60
Q

monoatomic anions end in suffix

A

-ide

SnCl2 - Stannous Chloride

MgO - Magnesium oxide

Na2S - Sodium sulfide

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61
Q

mono-

A

1

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62
Q

di-

A

2

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63
Q

tri-

A

3

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64
Q

tetra-

A

4

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65
Q

pent-

A

5

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66
Q

hex-

A

6

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67
Q

hept-

A

7

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68
Q

oct-

A

8

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69
Q

non-

A

9

70
Q

dec-

A

10

71
Q

Formula for alkane w/ n C

A

CnH2n+2

72
Q

Aliphatic Compounds

A

organic compounds with carbons linked in chains

can be in rings too, but lacks extra stability of aromatic electron-sharing

73
Q

aromatic compounds

A

compound characterized by one or more ring structure with alternating double bonds (resonance structures), giving extra stability because p orbitals are linked together and electrons shared over several atoms

74
Q

Aliphatics compounds divided into what groups:

A

alkanes

cycloalkanes

alkenes

alkynes

75
Q

saturated hydrocarbons

A

contain the maximum number of hydrocabons possible

(no double bonds)

alkanes & cycloalkanes saturated

76
Q

First 10 Straight Chain Alkanes

A
  1. methane - CH4
  2. ethane - CH3CH3
  3. propane - CH3CH2CH3
  4. butane - CH3(CH2)2CH3
  5. pentane - CH3(CH2)3CH3
  6. hexane - CH3(CH2)4CH3
  7. heptane - CH3(CH2)5CH3
  8. octane - CH3(CH2)6CH3
  9. nonane - CH3(CH2)7CH3
  10. decane - CH3(CH2)8CH3
77
Q

methyl

A

CH3-

78
Q

ethyl

A

C2H5

79
Q

propyl

A

C3H7

80
Q

Butyl

A

C4H9

81
Q

pentyl

A

C5H11

82
Q

hexyl

A

C6H13

83
Q

heptyl

A

C7H15

84
Q

octyl

A

C8H17

85
Q

nonyl

A

C9H19

86
Q

Decyl

A

C10H21

87
Q

Alkyl Group Formula

(or radical)

A

for n number of C

CnH2n+1

Allowing 1 Carbon bond at end to bond alkyl group to rest of molecule

88
Q

Isomers

A

compounds with same formula but different structure

Compounds differ only in structure, not in number of atoms (of the same type)

89
Q

Alkene

A

Structure includes a C=C (double) bond

-ane suffix changes to -ene

90
Q

geometric isomerism

A

double bond is rigid, isomers differ in the geometric shape. Same connectivity, but different arangement in 2D space

91
Q

cis-

A

geometric isomer has two same group on same side of double bond

92
Q

trans-

A

geometric isomer has same group on oposite side of double bond

93
Q

trichloroethene

A

TCE - Trichloroethene

94
Q

tetrachloroethene

A

PCE - tetrachloroethene - perchloroethene

95
Q

Chloroethene

A

VC - Vinyl Chloride - chloroethylene

96
Q

cis-1,2-dichloroethene

A

cis-1,2-DCE

97
Q

trans-1,2-dichloroethene

A

trans-1,2-DCE

98
Q
A

trans-1,2-DCE

trans-1,2-Dichloroethene

99
Q
A

cis-1,2-DCE

100
Q
A

1,1-dichloroethene

1,1-DCE

101
Q

Alkynes

A

Contains CC tripple bond

-ane suffix changes to -yne

102
Q

functional group

A

substitution of C or H for other atoms or groups

-OH

103
Q

alcohol

A

O that has single bond to C as -OH group

Example

104
Q

ether

A

O that has single bond to C with alkyl chain on either side of O

Example

105
Q

Ketone

A

O=C with alkyl chain on either side of C

Example

106
Q

aldehyde

A

C=O double bond with H attached to one side of C, alkyl group on other

Example

107
Q

CH3-

A

methyl

108
Q

C2H5

A

ethyl

109
Q

C3H7

A

propyl

110
Q

C4H9

A

Butyl

111
Q

C5H11

A

pentyl

112
Q

C6H13

A

hexyl

113
Q

C7H15

A

heptyl

114
Q

C8H17

A

octyl

115
Q

C9H19

A

nonyl

116
Q

C10H21

A

Decyl

117
Q

-one

A

suffix for ketone

O=C double bond with alkyl groups on either side of C

118
Q

methane

(structure)

A

CH4

119
Q

ethane

A

CH3CH3

120
Q

Propane

A

CH3CH2CH3

121
Q

butane

A

CH3(CH2)2CH3

122
Q

Pentane

A

CH3(CH2)3CH3

123
Q

hexane

A

CH3(CH2)4CH3

124
Q

heptane

A

CH3(CH2)5CH3

125
Q

Octane

A

CH3(CH2)6CH3

126
Q

nonane

A

CH3(CH2)7CH3

127
Q

decane

A

CH3(CH2)8CH3

128
Q

CH4

A

methane

129
Q
A

ethane

130
Q
A

Propane

131
Q
A

butane

132
Q
A

Pentane

133
Q
A

hexane

134
Q
A

heptane

135
Q
A

Octane

136
Q
A

nonane

137
Q
A

decane

138
Q

CH4

A

methane

139
Q

CH3CH3

A

ethane

140
Q

CH3CH2CH3

A

Propane

141
Q

CH3(CH2)2CH3

A

butane

142
Q

CH3(CH2)3CH3

A

Pentane

143
Q

CH3(CH2)4CH3

A

hexane

144
Q

CH3(CH2)5CH3

A

heptane

145
Q

CH3(CH2)6CH3

A

Octane

146
Q

CH3(CH2)7CH3

A

nonane

147
Q

CH3(CH2)8CH3

A

decane

148
Q

Z- Isomer

A

geometric isomer has two same group on same side of double bond

149
Q

E- Isomer

A

geometric isomer has same group on oposite side of double bond

150
Q

Caroxylic Acid

A

General Formula

RCO2H

151
Q
A

Carboxylic Acid General Formula

RCO2H

152
Q
A

Carboxylic ester general formula

RCO2R’

153
Q

RCO2R’

A

Carboxylic Ester general formula

154
Q

Amines

A

can be viewed as substituted Ammonia (NH3)

Alkyl group can replace any or all H

155
Q

primary amine

A
156
Q

secondary amine

A
157
Q

tertiary amine

A
158
Q

Amide

A

N from Amine bonds with C from Carboxyl group

(A can be H or carbon functional group)

159
Q

Oxidizer

A

Compound with atom going from higher oxidation state to lower oxidation state

160
Q

Reducer

A

compound going from lower oxidation state to higher oxidation state

161
Q

redox

A

oxidation - reduction reactions

162
Q

Acids

A

ionize in water and increase concentration of H ions (H+)

163
Q

Bases

A

ionize and increase concentration of OH- ions

164
Q

amphoteric

A

(am-fo-ter- ic)

acts as both acid and base

Water is example

165
Q

pH

A

-log10[H3O+]

quantitative measure of hydronuim ion H3O+

(or conversely hydroxide ion HO-)

166
Q

buffer capacity

A

weak acids don’t fully ionize, so reaction with base encounters more resistance to pH change than would be expected from pH alone

167
Q

Concentration

A

expresses ratio between solvent and specific solute

or ratio of individual component to the complete material

168
Q

lbs of water/gal

A

8.34 lbs/gal

169
Q

lbs of water/ft3

A

62.4 lbs/ft3

170
Q

g of water / mL

A

1.0 g/mL

171
Q
A
172
Q
A

CHMM -Dave's Deck (2 decks)

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