Hazards of Materials

Question 1

Paint Filter Test

Answer 1

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

Question 2

Change of Physical State (phase change)

Answer 2

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

Question 3

Freezing Point

Answer 3

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

Question 4

Melting Point

Answer 4

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

Question 5

Boiling Point

Answer 5

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

Question 6

Sublimation

Answer 6

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

Question 7

Volatilization

Answer 7

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

Question 8

Vapor Pressure

Answer 8

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

Question 9

BLEVE

Answer 9

(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

Question 10

Boiling Liquid Expanding Vapor Explosion

Answer 10

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

Question 11

Volatile Material

Answer 11

any material with a vapor pressure greater than 1 mm Hg

Question 12

Density

Answer 12

Ratio of mass to volume d= m/v

Question 13

Specific gravity

Answer 13

ratio between the density of a material and the density of water specific gravity = SG_x = d_x/d_H2O

Question 14

STP

Answer 14

Standart Temperature and Pressure

STP = 1 atm & 25^o C

Question 15

Ideal Gas Law

Answer 15

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

Question 16

Vapor Density

Answer 16

Vapor Density = vapor d_x

= realtive gas density_x = R_gasD_x

=d_x/d_air = MM_x/MM_air = MM_x/29

d_x = density of the gas

d_air = density of air

MM_x = molar mass of the gas

MM_air = molar mass of air = 29

Question 17

Solution

Answer 17

mixture that is uniform in composition and state of matter

also called homogeneous

also includes solid-solid solutions

Term not applied to gases

Question 18

Solvent

Answer 18

The most abundant compound in a solution

Question 19

Solute

Answer 19

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

Question 20

Atomic Number

Answer 20

The number of protons in an atom.

Defines the element that the atom represents

Question 21

Atomic Mass Number

Answer 21

sum of all protons and neutrons in an atom

variable (number of protons can change)

Question 22

Isotope

Answer 22

atoms with same atomic number but different atomic mass number

(different number of neutrons)

Question 23

nuclide

Answer 23

nucleus of a specific isotope

Question 24

Atomic Nomenlature

Answer 24

Example

Question 25

Element

Answer 25

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

Question 26

Ion

Answer 26

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

Question 27

Cation

Answer 27

positively charged ion

Question 28

anion

Answer 28

negatively charged ion

Question 29

Noble Gases

Answer 29

virtually inert elements

Question 30

5 common properties of metal

Answer 30

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

Question 31

How are elements grouped on Periodic table

Answer 31

Based on number of orbitals and electrons within the orbitals

Question 32

What are the types of orbitals and how many electrons

Answer 32

s : 2 e- per shell p : 6 e^- per shell d : 10 e^- per shell f : 7 e^- Shell

Question 33

what are the noble gases and why are they stable

Answer 33

Elements in column 18 they are stable because s & p orbitals are completely filled He, Ne, Ar, Kr, Xe, Rn, Uuo

Question 34

Valence Electrons

Answer 34

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)

Question 35

Why are elements in same column similar

Answer 35

elements are similar due to similar valence electron configuration C & Si have same number of electrons in outer p shell (2)

Question 36

Why are atoms in d & f transition metals similar

Answer 36

similar because an outer s shell is filled before the d & f 4s before 3d

Question 37

Aufbau principle

Answer 37

(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

Question 38

Alkali metals

Answer 38

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

Question 39

Alkaline Earth Metals

Answer 39

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)

Question 40

d transition metals

Answer 40

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

Question 41

Groups 13-18 Periodic table

Answer 41

Widely varying properties metals metalloids non-metals includes halogens (group 17) and noble gases (group 18)

Question 42

What happens when valence orbitals are full (ions)

Answer 42

Stability of ion increases significantly, similar to noble gases becuase all s & p outer orbitals are full Ca²⁺ Cl^-

Question 43

Ionic Bond

Answer 43

Valence electron transfered from one atom to other

Question 44

Covalent Bond

Answer 44

Valence electron shared between two atoms Could be shared equally or unequally more difference in electronegativity, more unequally shared

Question 45

electronegativity

Answer 45

1/2 (ionization energy - electron affinity) Metals least electronegative Halogens most electronegative

Question 46

Polar Covalent Bonds

Answer 46

some diference in Electronegativity - electron not equally shared

Question 47

Metalic Bonding

Answer 47

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

Question 48

bond polarity

Answer 48

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

Question 49

bond dipole

Answer 49

result of unequal charge distribution (polar bond)

Question 50

molecule polarity

Answer 50

happens when bond dipoles arranged so they don't cancel each other out. H₂O Polar

Question 51

hydrogen bonding

Answer 51

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

Question 52

Solubility

Answer 52

ability of substance to disolve into solvent

Question 53

Solvent

Answer 53

the most abundent compound in a solute/solvent combination

Question 54

-ic

Answer 54

higher oxidation state of ion ie Fe(III) - Fe³⁺ - Ferric Iron

Question 55

--ous

Answer 55

lower oxidation state of ion ie Fe(II) - Fe²⁺ - Ferrous Iron

Question 56

Common Oxidation State of iron

Answer 56

2+ Ferrous 3+ Ferric

Question 57

Common Oxidation State of lead Pb

Answer 57

2+ plumbous 4+ plumbic

Question 58

Common Oxidation State of tin

Answer 58

2+ stannous 4+ stannic

Question 59

Common Oxidation State of Copper

Answer 59

1+ cuprous 2+ cupric

Question 60

monoatomic anions end in suffix

Answer 60

-ide SnCl₂ - Stannous Chloride MgO - Magnesium oxide Na₂S - Sodium sulfide

Question 61

mono-

Answer 61

1

Question 62

di-

Answer 62

2

Question 63

tri-

Answer 63

3

Question 64

tetra-

Answer 64

4

Question 65

pent-

Answer 65

5

Question 66

hex-

Answer 66

6

Question 67

hept-

Answer 67

7

Question 68

oct-

Answer 68

8

Question 69

non-

Answer 69

9

Question 70

dec-

Answer 70

10

Question 71

Formula for alkane w/ n C

Answer 71

C_nH_2n+2

Question 72

Aliphatic Compounds

Answer 72

organic compounds with carbons linked in chains can be in rings too, but lacks extra stability of aromatic electron-sharing

Question 73

aromatic compounds

Answer 73

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

Question 74

Aliphatics compounds divided into what groups:

Answer 74

alkanes cycloalkanes alkenes alkynes

Question 75

saturated hydrocarbons

Answer 75

contain the maximum number of hydrocabons possible (no double bonds) alkanes & cycloalkanes saturated

Question 76

First 10 Straight Chain Alkanes

Answer 76

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

Question 77

methyl

Answer 77

CH₃-

Question 78

ethyl

Answer 78

C₂H₅

Question 79

propyl

Answer 79

C₃H₇

Question 80

Butyl

Answer 80

C₄H₉

Question 81

pentyl

Answer 81

C₅H₁₁

Question 82

hexyl

Answer 82

C₆H₁₃

Question 83

heptyl

Answer 83

C₇H₁₅

Question 84

octyl

Answer 84

C₈H₁₇

Question 85

nonyl

Answer 85

C₉H₁₉

Question 86

Decyl

Answer 86

C₁₀H₂₁

Question 87

Alkyl Group Formula | (or radical)

Answer 87

for n number of C C_nH_2n+1 Allowing 1 Carbon bond at end to bond alkyl group to rest of molecule

Question 88

Isomers

Answer 88

compounds with same formula but different structure Compounds differ only in structure, not in number of atoms (of the same type)

Question 89

Alkene

Answer 89

Structure includes a C=C (double) bond -ane suffix changes to -ene

Question 90

geometric isomerism

Answer 90

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

Question 91

cis-

Answer 91

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

Question 92

trans-

Answer 92

geometric isomer has same group on oposite side of double bond

Question 93

trichloroethene

Answer 93

TCE - Trichloroethene

Question 94

tetrachloroethene

Answer 94

PCE - tetrachloroethene - perchloroethene

Question 95

Chloroethene

Answer 95

VC - Vinyl Chloride - chloroethylene

Question 96

cis-1,2-dichloroethene

Answer 96

cis-1,2-DCE

Question 97

trans-1,2-dichloroethene

Answer 97

trans-1,2-DCE

Question 98

Answer 98

trans-1,2-DCE trans-1,2-Dichloroethene

Question 99

Answer 99

cis-1,2-DCE

Question 100

Answer 100

1,1-dichloroethene 1,1-DCE

Question 101

Alkynes

Answer 101

Contains CC tripple bond -ane suffix changes to -yne

Question 102

functional group

Answer 102

substitution of C or H for other atoms or groups -OH

Question 103

alcohol

Answer 103

O that has single bond to C as -OH group Example

Question 104

ether

Answer 104

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

Question 105

Ketone

Answer 105

O=C with alkyl chain on either side of C Example

Question 106

aldehyde

Answer 106

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

Question 107

CH₃-

Answer 107

methyl

Question 108

C₂H₅

Answer 108

ethyl

Question 109

C₃H₇

Answer 109

propyl

Question 110

C₄H₉

Answer 110

Butyl

Question 111

C₅H₁₁

Answer 111

pentyl

Question 112

C₆H₁₃

Answer 112

hexyl

Question 113

C₇H₁₅

Answer 113

heptyl

Question 114

C₈H₁₇

Answer 114

octyl

Question 115

C₉H₁₉

Answer 115

nonyl

Question 116

C₁₀H₂₁

Answer 116

Decyl

Question 117

-one

Answer 117

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

Question 118

methane | (structure)

Answer 118

CH₄

Question 119

ethane

Answer 119

CH₃CH₃

Question 120

Propane

Answer 120

CH₃CH₂CH₃

Question 121

butane

Answer 121

CH₃(CH₂)₂CH₃

Question 122

Pentane

Answer 122

CH₃(CH₂)₃CH₃

Question 123

hexane

Answer 123

CH₃(CH₂)₄CH₃

Question 124

heptane

Answer 124

CH₃(CH₂)₅CH₃

Question 125

Octane

Answer 125

CH₃(CH₂)₆CH₃

Question 126

nonane

Answer 126

CH₃(CH₂)₇CH₃

Question 127

decane

Answer 127

CH₃(CH₂)₈CH₃

Question 128

CH₄

Answer 128

methane

Question 129

Answer 129

ethane

Question 130

Answer 130

Propane

Question 131

Answer 131

butane

Question 132

Answer 132

Pentane

Question 133

Answer 133

hexane

Question 134

Answer 134

heptane

Question 135

Answer 135

Octane

Question 136

Answer 136

nonane

Question 137

Answer 137

decane

Question 138

CH₄

Answer 138

methane

Question 139

CH₃CH₃

Answer 139

ethane

Question 140

CH₃CH₂CH₃

Answer 140

Propane

Question 141

CH₃(CH₂)₂CH₃

Answer 141

butane

Question 142

CH₃(CH₂)₃CH₃

Answer 142

Pentane

Question 143

CH₃(CH₂)₄CH₃

Answer 143

hexane

Question 144

CH₃(CH₂)₅CH₃

Answer 144

heptane

Question 145

CH₃(CH₂)₆CH₃

Answer 145

Octane

Question 146

CH₃(CH₂)₇CH₃

Answer 146

nonane

Question 147

CH₃(CH₂)₈CH₃

Answer 147

decane

Question 148

Z- Isomer

Answer 148

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

Question 149

E- Isomer

Answer 149

geometric isomer has same group on oposite side of double bond

Question 150

Caroxylic Acid

Answer 150

General Formula RCO₂H

Question 151

Answer 151

Carboxylic Acid General Formula RCO₂H

Question 152

Answer 152

Carboxylic ester general formula RCO₂R'

Question 153

RCO2R'

Answer 153

Carboxylic Ester general formula

Question 154

Amines

Answer 154

can be viewed as substituted Ammonia (NH₃) Alkyl group can replace any or all H

Question 155

primary amine

Answer 155

Question 156

secondary amine

Answer 156

Question 157

tertiary amine

Answer 157

Question 158

Amide

Answer 158

N from Amine bonds with C from Carboxyl group (A can be H or carbon functional group)

Question 159

Oxidizer

Answer 159

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

Question 160

Reducer

Answer 160

compound going from lower oxidation state to higher oxidation state

Question 161

redox

Answer 161

oxidation - reduction reactions

Question 162

Acids

Answer 162

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

Question 163

Bases

Answer 163

ionize and increase concentration of OH- ions

Question 164

amphoteric

Answer 164

(am-fo-ter- ic) acts as both acid and base Water is example

Question 165

pH

Answer 165

-log₁₀[H₃O⁺] quantitative measure of hydronuim ion H₃O⁺ (or conversely hydroxide ion HO^-)

Question 166

buffer capacity

Answer 166

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

Question 167

Concentration

Answer 167

expresses ratio between solvent and specific solute or ratio of individual component to the complete material

Question 168

lbs of water/gal

Answer 168

8.34 lbs/gal

Question 169

lbs of water/ft³

Answer 169

62.4 lbs/ft³

Question 170

g of water / mL

Answer 170

1.0 g/mL