Chemistry

Question 1

anything that has mass and occupies space

Answer 1

matter

Question 2

amount of matter contained in an object

Answer 2

mass

Question 3

amount of space occupied by matter

Answer 3

volume

Question 4

4th state of matter, also called liquid crystal, mesophase, supercritical fluid

Answer 4

plasma

Question 5

this is strongly influenced by electric and magnetic fields with a hot ionized gas consisting of approximately equal numbers of positively charged ions and negatively charged electrons

Answer 5

plasma

Question 6

5th state of matter, also called a super atom, and has many properties of a super fluid

Answer 6

bose-einstein condensate

Question 7

m/v

Answer 7

density

Question 8

density of water

Answer 8

1 g/ml=1 g/cm³=1000 kg/m³

Question 9

ratio of the density of a sample and the density of a reference substance

Answer 9

specific gravity (unitless quantity)

Question 10

specific gravity formula

Answer 10

SG=tsample/treference

Question 11

ratio between the weights of equal volumes of a sample and water

Answer 11

apparent specific gravity

Question 12

formula for apparent specific gravity

Answer 12

SGapparent=Wsample/Wwater

Question 13

ratio between the weights in a vacuum of equal volumes of a sample and water

Answer 13

true specific gravity

Question 14

formula for true specific gravity

Answer 14

SGtrue=Wvsample/Wvwater

Question 15

Specific Volume

Answer 15

SV=1/SG

Question 16

when H2O freezes the volume that the same mass of H2O occupies increases because

Answer 16

the molecules become more highly organized

Question 17

highly organized molecules mean

Answer 17

increase in volume, decrease in density

Question 18

ability to float

Answer 18

buoyancy

Question 19

ability to be drawn out into wires

Answer 19

ductility

Question 20

ability to be hammered into sheets

Answer 20

malleability

Question 21

ability to return to its original shape after being deformed

Answer 21

elasticity

Question 22

ability to resist flow

Answer 22

viscosity

Question 23

measure of disorder of a thermodyamic system

Answer 23

entropy

Question 24

amount of energy stored in an object

Answer 24

energy

Question 25

the number of valence electrons is close to completing the octet rule, accepts electrons during ionic bonding, forms anions when ionized

Answer 25

non-metals

Question 26

the number of valence electrons is small, donates electrons during ionic bonding, forms cations when ionized

Answer 26

metals

Question 27

can act as a metal or non-metal depending on the conditions

Answer 27

metalloids

Question 28

components are a pair of anion group and a cation group, electrons are transferred from the cation to the anion

Answer 28

ionic

Question 29

components are both anion groups, electrons are shared within the bond

Answer 29

covalent

Question 30

components are both metals, components are stored in a sea of electrons

Answer 30

metallic

Question 31

commonly called solutions, where only 1 phase is discernable

Answer 31

homogenous

Question 32

measure of the relative amounts of the components of a solution

Answer 32

concentration

Question 33

the component that dissolves in the solution

Answer 33

solute

Question 34

the component that dissolves other components of the solution

Answer 34

solvent

Question 35

the maximum amount of solute that can be dissolved in a particular solvent under specific conditions, often expressed as a ratio or other measures of concentration

Answer 35

solubility [g of solute/100 g of solvent]

Question 36

contains less solute than the maximum quantity of solute that is normally possible at a given temperature [haven’t reached the solubility of your solute]

Answer 36

unsaturated, no crystal formation

Question 37

contains the max amount of solute that is normally possible at a given temperature

Answer 37

saturated, crystal formation

Question 38

contains more solute than normally expected for a saturated solution (unusual amount at a specified temperature]

Answer 38

supersaturated, unstable, triggers fast crystal formation

Question 39

molarity formula

Answer 39

M=moles of solute/liters of solution

Question 40

molality formula

Answer 40

m=moles of solute/kg of solvent

Question 41

mass percent

Answer 41

[mass of solute/mass of solution] x 100

Question 42

volume percent

Answer 42

[volume of solute/volume of solvent] x 100

Question 43

relative amount of solute in a sol’n

Answer 43

saturation

Question 44

IMF charges occur, these IMFs can decrease volume of liquid because of strong interactions that occur in your liquids, this also accounts for changes

Answer 44

on the usage of molality

Question 45

used to describe a certain amount of molecules

Answer 45

moles

Question 46

1 mole = avogadro’s number

Answer 46

6.02 x10²³

Question 47

number of equivalent weights of a solute per liter of the solution

Answer 47

normality

Question 48

normality formula

Answer 48

N=number of equivalent weights/L of solution

Question 49

grams of solute/gram equivalent weight of solute

Answer 49

number of equivalent weight

Question 50

Molarity x factor

Answer 50

Normality

Question 51

refers to the acidic hydrogen [hydronium]

Answer 51

acid factor

Question 52

refers to the number of hydroxide

Answer 52

base factor

Question 53

used to convert mass of substance to moles of substance

Answer 53

molecular weight

Question 54

all alkali metals (group 1a) are

Answer 54

soluble

Question 55

all those with ammonium ion [NH₄⁺] are

Answer 55

soluble

Question 56

all nitrates [NO₃⁻] are

Answer 56

soluble

Question 57

all acetates [C₂H₃O₂⁻] are

Answer 57

soluble

Question 58

all chlorides [Cl⁻] bromides [Br⁻] iodides [I⁻] are soluble except

Answer 58

Ag⁺, Hg₂²⁺, Pb²⁺

Question 59

most sulfates [SO₄²⁻] are soluble except

Answer 59

BaSO₄, PbSO₄, SrSO₄, Hg₂SO₄

Question 60

all hydroxides [OH⁻] are insoluble except those of

Answer 60

Group 1A, Ba(OH)₂, Sr(OH)₂, Ca(OH)₂

Question 61

all sulfides are insoluble except those of

Answer 61

group 1A, group 2A, NH₄⁺

Question 62

all carbonates [CO₃²⁻] are insoluble except those of NH₄⁺ and those of

Answer 62

NH₄⁺ and those of group 1A

Question 63

all phosphates [PO₄³⁻] are insoluble except

Answer 63

NH₄⁺ and those Group1A

Question 64

pressure needed to prevent osmosis which is the spontaneous net movement of solvent molecules through a semi-permeable membrane into a region of higher solute concentration

Answer 64

osmotic pressure

Question 65

osmotic pressure formula

Answer 65

πV=nRT

Question 66

the addition of nonvolatile solute to a volatile solvent will diminish the escaping tendency of the solvent thereby lowering the vapor pressure of the solution

Answer 66

vapor pressure lowering

Question 67

raoult’s law

Answer 67

ΔP=P°Xₛₒₗᵤₜₑ

Question 68

is the temperature at which the vapor pressure of the liquid becomes equal to the external atmospheric pressure [1 atm=760 mmHg]

Answer 68

boiling point

Question 69

the boiling point of a pure solvent is increased by the addition of a non-volatile solute, and the elevation can be measure by

Answer 69

ebullioscopy

Question 70

ebullioscopy

Answer 70

ΔTբ=iKbm

Question 71

is the temperature at which the solid and liquid phases are in equilibrium under an external pressure of 1 atm

Answer 71

freezing point

Question 72

the freezing point of a pure solvent is lowered by the addition of a solute which is insoluble in the solid solvent, and the measurement of this difference is called cryoscopy

Answer 72

freezing point depression

Question 73

freezing point depression formula

Answer 73

ΔTբ=iKբm

Question 74

mixtures wherein 2 or more distinct phases are discernable

Answer 74

heterogenous

Question 75

suspended particles are too large and too heavy to be carried by the motion of the particles in which they are suspended in causing them to settle after sometime

Answer 75

suspensions

Question 76

suspended particles are small and light enough to be carried by the movement of the particles in which they are suspended in

Answer 76

colloids

Question 77

solid in solid colloid

Answer 77

solid sol

Question 78

solid in liquid colloid

Answer 78

sol

Question 79

solid in gas colloid

Answer 79

solid aerosol

Question 80

liquid in solid colloid

Answer 80

gel

Question 81

liquid in liquid colloid

Answer 81

emulsion

Question 82

liquid in gas colloid

Answer 82

aerosol

Question 83

gas in solid colloid

Answer 83

solid foam

Question 84

gas in liquid colloid

Answer 84

foam

Question 85

mass of proton

Answer 85

1.67 x 10⁻²⁷ or 1 amu

Question 86

mass of neutrons

Answer 86

1.67 x 10⁻²⁷ or 1 amu

Question 87

mass of electrons

Answer 87

9.11 x 10⁻³¹

Question 88

mass of the atom is concentrated on the

Answer 88

nucleus

Question 89

atomic number [Z]

Answer 89

number of protons

Question 90

mass number [A]

Answer 90

sum of protons and neutrons

Question 91

charge [q]

Answer 91

difference of the protons and electrons

Question 92

relative abundance of a certain isotope compared to all the isotopes of the same element

Answer 92

percent natural balance

Question 93

weighted average of the mass numbers of the isotopes of that particular element

Answer 93

atomic weight

Question 94

ISOTOPES: atoms of the same element that have the same number of protons but different number of neutrons, thus their mass numbers are

Answer 94

different

Question 95

elements having the same number of neutrons

Answer 95

isotones

Question 96

atomic species having the same mass number but different atomic numbers

Answer 96

isobars

Question 97

elements having the same number of electrons

Answer 97

isoelectronic

Question 98

who discovered atoms as the basic unit of matter

Answer 98

democritus

Question 99

who discovered the billiard ball model

Answer 99

john dalton

Question 100

who discovered the plum pudding model and the electron

Answer 100

j.j. thomson

Question 101

who discovered the gold foil experiment and the proton?

Answer 101

ernest rutherford

Question 102

who discovered the neutron

Answer 102

james chadwick

Question 103

who discovered the planetary model

Answer 103

niels bohr

Question 104

who discovered the quantum theory

Answer 104

erwin schrodinger

Question 105

usually malleable and ductile, highly conductive for heat and electricity, low electronegativities and ionization energies, high melting points and densities

Answer 105

metals

Question 106

brittle solids, poor conductors of heat and electricity, high electronegativities and ionization energies

Answer 106

non-metals

Question 107

properties are in between metals and non-metals, reactivity depends on the elements to be reacted with

Answer 107

metalloids

Question 108

soft metallic solids, shiny and lustrous; reacts vigorously with water to produce hydroxides

Answer 108

alkali metals [group 1A]

Question 109

harder than 1A metals; shiny, lustrous, and oxidizes easily

Answer 109

alkaline earth metals [group 2A]

Question 110

boron group or earth metals

Answer 110

group 3A

Question 111

carbon group or tetrels

Answer 111

group 4A

Question 112

nitrogen group or pnictogens

Answer 112

group 5A

Question 113

oxygen group or chalcogens

Answer 113

group 6A

Question 114

halogens, reactive non-metals

Answer 114

group 7A

Question 115

unreactive under ordinary circumstances; usually found as monoatomic gases

Answer 115

group 8A [noble gases]

Question 116

hard metallic; shiny and lustrous; dense and have high melting points, usually have high oxidation states

Answer 116

transition metals

Question 117

Group B inclusions

Answer 117

transition metals, lanthanides, actinides

Question 118

lightest element

Answer 118

hydrogen

Question 119

densest element

Answer 119

osmium

Question 120

only metal liquid at room temperture

Answer 120

mercury

Question 121

only non metal liquid at room temperature

Answer 121

bromine

Question 122

most abundant intracellular cation

Answer 122

potassium

Question 123

most abundant extracellular cation

Answer 123

sodium

Question 124

most abundant gas in the air

Answer 124

nitrogen

Question 125

most abundant element on earth

Answer 125

oxygen

Question 126

most abundant metal on earth

Answer 126

aluminum

Question 127

most abundant noble gas

Answer 127

argon

Question 128

desire for an electron, desire for negativity, near octet

Answer 128

electronegativity

Question 129

most electronegative

Answer 129

flourine

Question 130

tendency of an electron to bond, increases from left to right along a period, decreases from top to bottom along a column/group

Answer 130

electronegativity

Question 131

energy needed to remove an electron form an atom, increases from left to right along a period, decreases from top to bottom along a column/group

Answer 131

ionization energy

Question 132

energy released when an electron is added to an atom, positive when energy is released and negative when absorbed, increases from left to right along a period, decreases from top to bottom along a column/group

Answer 132

electron affinity

Question 133

farthest extent of the presence of electron decrease from left to right a period, increases from top to bottom along a column/group

Answer 133

atomic size/radius

Question 134

bond between a metal and non-metal [cation and anion], form crystals, high melting and boiling points, hard and brittle, poor conductors when solid, good conductors when dissolved in water

Answer 134

ionic bond

Question 135

bond between non-metals [anions], most have relatively low melting and boiling points, soft and relatively flexible, more flammable, many are insoluble in water and those that do dissolve do not conduct electricity

Answer 135

covalent/molecular bond

Question 136

with unequal sharing

Answer 136

polar bond

Question 137

with equal sharing

Answer 137

nonpolar bond

Question 138

electronegativity difference greater than 0.4 but less than 1.7

Answer 138

polar compound

Question 139

electronegativity difference less than 0.4

Answer 139

nonpolar compound

Question 140

electronegativity difference greater than 1.7

Answer 140

ionic compound

Question 141

types of covalent bonds

Answer 141

pi bond and sigma bond

Question 142

end to end overlap of orbitals; stronger type of bond

Answer 142

sigma bond

Question 143

lateral or sideways overlap of orbitals

Answer 143

pi bond

Question 144

bond between metals [cations] have moderately high melting points, malleable and ductile, good conductors of heat and electricity

Answer 144

metallic bond

Question 145

occurs when orbitals combine to form a hybrid orbital during bond formation

Answer 145

hybrid orbital

Question 146

s orbital combines with 3 p orbitals to form 4 hybridized orbitals

Answer 146

sp³

Question 147

s orbital combines with 2 p orbitals to form 3 hybridized orbitals and 1 normal orbital

Answer 147

sp²

Question 148

s orbital combines with 1 p orbital to form 2 hybridized orbitals and 2 normal orbitals

Answer 148

sp¹

Question 149

[carbon chemical bonds] sp³ hybrid orbitals form sigma bonds with orbitals of other atoms

Answer 149

single bonds

Question 150

[carbon chemical bonds] 1 sp² hybrid from each atom form a sigma bond and 1 p orbital from each atom form a pi bond

Answer 150

double bonds

Question 151

[carbon chemical bonds] 1 sp¹ hybrid from each atom form a sigma bond and 2 p orbitals from each atom form 2 pi bonds

Answer 151

triple bonds

Question 151

presence of double or triple bonds increases

Answer 151

reactivity

Question 152

saturated hydrocarbons do not have

Answer 152

triple or double bonds

Question 153

shows the simplest ratio of the amounts of atoms of each component elements

Answer 153

empirical formula

Question 154

shows the actual amounts of each of the atoms of the component elements

Answer 154

molecular formula

Question 155

shows the approximate arrangement of the atoms within the molecule

Answer 155

structural formula

Question 156

[molecular geometry] steric number 2, no lone pairs

Answer 156

linear

Question 157

[molecular geometry] steric number 3, no lone pairs

Answer 157

trigonal planar

Question 158

[molecular geometry] steric number 3, 1 lone pair

Answer 158

bent or angular

Question 159

[molecular geometry] steric number 4, no lone pairs

Answer 159

tetrahedral

Question 160

[molecular geometry] steric number 4, 1 lone pair

Answer 160

trigonal pyramidal

Question 161

[molecular geometry] steric number 4, 2 lone pairs

Answer 161

bent or angular «109 degrees

Question 162

[molecular geometry] steric number 5, no lone pairs

Answer 162

trigonal bypiramidal

Question 163

[molecular geometry] steric number 5, 1 lone pair

Answer 163

sawhorse or seesaw

Question 164

[molecular geometry] steric number 5, 2 lone pairs

Answer 164

t-shape

Question 165

[molecular geometry] steric number 6, no lone pairs

Answer 165

octahedral

Question 166

[molecular geometry] steric number 6, 1 lone pair

Answer 166

square pyramid

Question 167

[molecular geometry] steric number 6, 2 lone pairs

Answer 167

square planar

Question 168

[molecular geometry] steric number 6, 3 lone pairs

Answer 168

t shape <90 degrees

Question 169

[molecular geometry] steric number 6, 4 lone pairs

Answer 169

linear, vertical 180 degrees

Question 170

influences the final structure of the molecule, boiling and freezing points, heat capacity, solubility

Answer 170

intermolecular forces of attraction

Question 171

attraction between the opposing poles of dipole molecules

Answer 171

electrostatic interactions

Question 172

types of electrostatic interactions

Answer 172

dipole-dipole, ion-dipole, ion-induced dipole, hydrogen bonding

Question 173

weakest electrostatic interaction, sum of all the attractive ad repulsive forces between and within the molecules

Answer 173

van der waals

Question 174

relative amount of particles present in a sample, avogadro’s sample

Answer 174

6.022 x 10²³

Question 175

[gases] an ideal gas is where all interactions between the molecules are only through collisions that are assumed to be completely elastic, gases have no volume, exists in STP of 0 degrees C and 1atm

Answer 175

ideal gas concept

Question 176

[gases] at stp, 1 mole of a gas is occupies 22.4 L

Answer 176

22.4 L

Question 177

[gases] ideal gas equation

Answer 177

PV=nRT

Question 178

in PV=nRT, n is for

Answer 178

the number of moles

Question 179

in PV=nRT, r is equal to

Answer 179

0.0821 [(Latm)/molK]

Question 180

in using gas laws the unit of temperature must be in

Answer 180

kelvin

Question 181

a particular amount of gas at constant temperature increase in volume when the pressure is decreased

Answer 181

boyle’s law

Question 182

boyle’s law equation

Answer 182

P₁V₁=P₂V₂

Question 183

a particular amount of gas in a constant pressure increases in volume when the temperature is increased

Answer 183

charles law

Question 184

charles law equation

Answer 184

V₁/T₁=V₂/T₂

Question 185

a particular amount of gas in a constant volume increase in temperature when the pressure is increased

Answer 185

gay-lussac’s law

Question 186

gay-lussac’s law equation

Answer 186

P₁/T₁=P₂/T₂

Question 187

a gas in a constant pressure and temperature increases in volume when the amount of particles is increased

Answer 187

avogadro’s law

Question 188

combined gas law equation

Answer 188

P₁V₁/V₁n₁=P₂V₂/V₂n₂

Question 189

avogadro’s law equation

Answer 189

V₁/n₁=V₂/n₂

Question 190

dalton’s law is also called

Answer 190

law of partial pressures

Question 191

the pressure of a mixture of gases is the sum of the pressures of the individual components

Answer 191

Ptotal = P₁ + P₂ +…

Question 192

the rate at which a gas diffuses is inversely proportional to the root of its density or mass

Answer 192

law of effusion

Question 193

law of effusion formula

Answer 193

R₁/R₂ = √t₁/t₂

Question 194

all chemical reactions follow the law of

Answer 194

conservation of mass

Question 195

[type of rxn] 2 or more elements or compounds combine to make a more complex substance

Answer 195

synthesis

Question 196

[type of rxn] compounds break down into simpler substances

Answer 196

decomposition/analysis

Question 197

[type of rxn] occurs when 1 element replaces another one in a compound

Answer 197

single replacement

Question 198

[type of rxn] occurs when different atoms in 2 different compounds trade places

Answer 198

double replacement

Question 199

fuel + O₂ -> CO₂ +H₂O

Answer 199

complete combustion

Question 200

fuel + O₂ -> CO₂ + H₂O + residues

Answer 200

incomplete combustion

Question 201

electron transfer from 1 atom to another

Answer 201

redox reaction

Question 202

[type of redox reaction] loss of electrons

Answer 202

oxidation

Question 203

[type of redox reaction] gain of electrons

Answer 203

reduction

Question 204

GEROA

Answer 204

gain of electrons is reduction among oxidizing agents

Question 205

LEORA

Answer 205

loss of electrons is reduction among reducing agents

Question 206

acid + base -> salt + H₂O

Answer 206

neutralization reaction

Question 207

[stoichiometry] reactant that is first to be totally consumed halting further reactions

Answer 207

limiting reagent

Question 208

[stoichiometry] reactant that is left when the limiting reagent is consumed

Answer 208

excess reagent

Question 209

[energy] the total energy of an object or system

Answer 209

enthalpy

Question 210

[energy] reactions that require addition of energy. this means that the product has higher enthalpy than the reactants

Answer 210

endothermic

Question 211

[energy] reactions that require removal of energy. this means that the product has lower enthalpy than the reactants

Answer 211

exothermic

Question 212

[energy] energy required to start a reaction

Answer 212

activation energy

Question 213

[energy] reactions that require a very small activation energy and can start without external interference

Answer 213

spontaneous reactions

Question 214

[energy] any substance that increases the rate of the reaction without being consumed

Answer 214

catalyst

Question 215

[equilibrium] reactions whose products can spontaneously react to form the original reactants thereby reversing the reaction

Answer 215

reversible reactions

Question 216

[equilibrium] state of reaction at which the rate of the forward and reverse reactions are the same producing a condition where the concentrations of the reactant and the products remain relatively constant

Answer 216

equilibrium

Question 216

equilibrium constant K can be derived as

Answer 216

kₑq = [C]ˡ[D]ᵐ/[A]ʲ[B]ᴰ

Question 217

when an equilibrium system is subjected to a change in temp., pressure, or concentration of a reacting species, the system responds by attaining a new equilibrium that partially offsets the impact of the change

Answer 217

le chatelier’s principle

Question 218

[le chatelier’s] effects of changing the amount of reacting species

Answer 218

if the concentration of 1 of the reacting species is increased, it will favor the reaction in which the species is consumed

Question 219

[le chatelier’s] effects of changing in pressure or volume of equilibrium

Answer 219

if the pressure of an equilibrium mixture of gases is increased, the volume is reduced, a net reaction occurs in the direction producing fewer moles of gases

Question 220

[le chatelier’s] effects of temperature on equilibrium

Answer 220

raising the temp. of an equilibrium mixture shifts the equilibrium condition in the direction of endothermic reaction

Question 221

[le chatelier’s] effects of catalysts on equilibrium

Answer 221

a catalyst has no effect on the condition of equilibrium in a reversible reaction

Question 222

[dissociation] ____ occurs when a compound separates into its component molecules

Answer 222

dissociation

Question 223

[acid-base def.] arrhenius acid

Answer 223

H⁺ producer

Question 224

[acid-base def.] arrhenius base

Answer 224

OH⁻ producer

Question 225

[acid-base def.] bronsted-lowry acid

Answer 225

H⁺ donor

Question 226

[acid-base def.] bronsted-lowry base

Answer 226

H⁺ acceptor

Question 227

[acid-base def.] lewis acid

Answer 227

electron pair acceptor

Question 228

[acid-base def.] lewis base

Answer 228

electron pair donor

Question 229

[acid-base] typically sour in taste and are corrosive to most metals

Answer 229

acids

Question 230

[acid-base] typically bitter in taste, and are slippery to touch

Answer 230

bases

Question 231

[conjugate acids and bases] bronsted-lowrey acid

Answer 231

protonated bronsted base

Question 232

[conjugate acids and bases] bronsted-lowrey base

Answer 232

deprotonate bronsted acid

Question 233

acids dissociate to produce

Answer 233

H+ ions and anions

Question 234

bases dissociate to form

Answer 234

OH- ions and cations

Question 235

acids/bases that have dissociation constants close to 1

Answer 235

strong acids/bases

Question 236

acids/bases that have dissociation constants far from 1

Answer 236

weak acids/bases

Question 237

[strong/weak acid] HCl

Answer 237

strong acid

Question 238

[strong/weak acid] H2SO4

Answer 238

strong acid

Question 239

[strong/weak acid] Nitric Acid (HNO3)

Answer 239

strong acid

Question 240

[strong/weak acid] Perchloric Acid (HClO4)

Answer 240

strong acid

Question 241

when acids and bases are in aqueous state, they _____ into their respective ions

Answer 241

dissociate

Question 242

acidity of a substance depend on the concentrations of its

Answer 242

dissociated ions

Question 243

process of determining the concentration of a substance by slowly adding another substance with a known concentration

Answer 243

titration

Question 244

[titration] substance with known concentration to be added

Answer 244

titrant

Question 245

[titration] substance whose unknown concentration is to be determined

Answer 245

analyte

Question 246

[titration] substances that changes property under certain conditions to signal when to stop adding the titrant

Answer 246

indicator

Question 247

[acid-base titration] added titrants neutralizes the analyte

Answer 247

equivalence point

Question 248

[acid-base titration] point when the pH changes the color of the indicator

Answer 248

end point

Question 249

pH = 7

Answer 249

strong acid-strong base

Question 250

pH < 7

Answer 250

strong acid-weak base

Question 251

pH > 7

Answer 251

weak acid-strong base

Question 252

acid + base -> salt + H2O

Answer 252

neutralization reaction

Question 253

[acid-base rxn] resist drastic change in pH contain weak acid and base pairs

Answer 253

buffers

Question 254

[thermochem] amount of heat needed to changethe temp. of 1 g of a substance by 1 degree celsius

Answer 254

C [specific heat capacity]

Question 255

amount of heat required to transform 1 g of substance from liquid to gas or gas to liquid

Answer 255

heat of vaporization [ΔHᵥ]

Question 256

amount of heat required to transform 1 g of a substance from solid to liquid or liquid to solid

Answer 256

heat of fusion [ΔHբ]

Question 257

change in temperature formula

Answer 257

Q = mCqΔT

Question 258

change in phase formula

Answer 258

Q = mΔH

Question 259

common properties of organic compounds

Answer 259

usually combustible, generally have low melting and boiling pts, usually less soluble in water, usually slow to react because they are usually covalent molecules, most have high molecular weights

Question 260

sources of organic compounds

Answer 260

nature, synthesis, fermentation

Question 261

valence electrons of carbon

Answer 261

4

Question 262

what group is carbon in in the periodic table?

Answer 262

group 4A

Question 263

carbon is capable of catenation and _____

Answer 263

hybridization

Question 264

is the ability of carbon to bond with itself and form long chains of organic compounds

Answer 264

catenation

Question 265

concept of mixing non-equivalent atomic orbitals to form equivalent or degenerate hybrid orbitals to form single, double, and triple bonds

Answer 265

hybridization

Question 266

what is the shape, bond angle, and bond type of sp3 orbital?

Answer 266

tetrahedral, 109.5, single

Question 267

what is the shape, bond angle, and bond type of sp2 orbital?

Answer 267

trigonal planar, 120, double

Question 268

what is the shape, bond angle, and bond type of sp orbital?

Answer 268

linear, 180, triple

Question 269

[org chem] different compounds that have the same molecular formula

Answer 269

isomers

Question 270

[forms of isomerism] form if isomerism in which molecules with the same molecular formula have different bonding patterns and atomic organization

Answer 270

structural isomerism

Question 271

[type of structural isomerism] differ in the arrangement of C atoms usually due to the presence of branching

Answer 271

chain isomerism

Question 272

examples of chain isomerism

Answer 272

n-butane, isobutane

Question 273

[type of structural isomerism] the isomers have the same molecular formula but differs mainly in the attached functional groups

Answer 273

functional isomerism

Question 274

examples of functional isomerism

Answer 274

ether and alcohol, aldehyde and ketone

Question 275

[type of structural isomerism] differs in the position of unsaturated bonds (double and triple bonds) or functional groups

Answer 275

positional isomerism

Question 276

examples of positional isomerism

Answer 276

meta isomer, ortho isomer, para isomer

Question 277

[forms of isomerism] isomers that have the same molecular formula and sequence of bonded atoms (constitution), but differ in the 3-dimensional orientations of their atom space

Answer 277

stereoisomerism

Question 278

[types of stereoisomerism] occurs among double bonds

Answer 278

geometric/configurational isomerism

Question 279

[type of geometric isomerism] cis-trans isomerism: the molecule in which the 2 of the same atoms are on the same side of the double bond is known as

Answer 279

cis isomer

Question 280

[type of geometric isomerism] cis-trans isomerism: molecule with the 2 of the same atoms in the opposite side of the double bond is called

Answer 280

trans isomer

Question 281

[type of geometric isomerism] E-Z isomerism: the higher priority groups are on opposite sides of the double bond

Answer 281

E isomer

Question 282

[type of geometric isomerism] E-Z isomerism: the higher priority groups are on the same sides of the double bond

Answer 282

Z isomer

Question 283

[types of stereoisomerism] results from the different ways an atom flexes and bends due to rotation along a single bond or ring flipping among cyclic structures

Answer 283

conformational isomers

Question 284

[types of stereoisomerism] isomers which differ in their ability to rotate plane polarized light

Answer 284

optical isomers

Question 285

[optical isomers] structural requirement for optical activity, carbon with 4 different functional groups or substituents

Answer 285

chiral center

Question 286

types of optical isomers

Answer 286

enantiomers, diastereomers, meso compounds

Question 287

chain or branched chain of organic compounds whose longest chain is made of carbon atoms only

Answer 287

aliphatic compounds

Question 288

aliphatic compounds made up of only hydrogen and carbon

Answer 288

hydrocarbons

Question 289

[type of hydrocarbon] hydrocarbons wherein all carbons are attached together only with single bonds

Answer 289

saturated hydrocarbons

Question 290

properties of saturated hydrocarbons

Answer 290

colorless, tasteless, odorless; boiling and melting pts increases as molecular weight increases while London Dispersion Forces increases, non-polar practically insoluble in water but soluble in organic solvents, stable due to strong c-c and c-h bonds, sigma bonded, tetrahedral

Question 291

CH4

Answer 291

methane

Question 292

C2H6

Answer 292

ethane

Question 293

C3H8

Answer 293

propane

Question 294

C4H10

Answer 294

n-butane

Question 295

(CH3)3CH

Answer 295

isobutane

Question 296

C5H12

Answer 296

n-pentane

Question 297

(CH3)CHCH2

Answer 297

isopentane

Question 298

(CH3)4C

Answer 298

neopentane

Question 299

[common rxns] CH4 + 202 -> CO2 +H2O

Answer 299

oxidation with oxygen in air

Question 300

[common rxns] CH4 +CL2 -> HCl + CH3Cl

Answer 300

halogen substitution

Question 301

[common rxns] occurs when bacteria oxidizes a hydrocarbon underaerobic conditions

Answer 301

biological oxidation

Question 302

[type of hydrocarbon] hydrocarbons containing double or triple bonds

Answer 302

unsaturated hydrocarbons

Question 303

[types & nomenclatures of unsaturated hydrocarbons] properties: non polar, stable due to strong c-c, c-h bonds, sigma and pi bonds, double bond, trigonal planar

Answer 303

alkenes

Question 304

[types & nomenclatures of unsaturated hydrocarbons] properties: triple bond, have 2 pi bonds, very reactive

Answer 304

alkyne

Question 305

[common reactions for alkenes and alkynes] produces glycol

Answer 305

oxidation

Question 306

[common reactions for alkenes and alkynes] hydrogen is bonded to replace double or triple bonds making the compound more saturated

Answer 306

reduction

Question 307

[common reactions for alkenes and alkynes] acids bond across double or triple bonds

Answer 307

addition

Question 308

[common reactions for alkenes and alkynes] unsaturated molecules combine with each other to form polymers with higher molecular weight

Answer 308

polymerization

Question 309

[types & nomenclatures of unsaturated hydrocarbons] hydrocarbons that contain the hydroxyl group OH, product of primary oxidation

Answer 309

alcohols

Question 310

classifications of alcohols

Answer 310

primary, secondary, tertiary

Question 311

properties of alcohols

Answer 311

soluble in water but solubility decreases as molecular weight increases, low boiling and melting points but increases with molecular weight

Question 312

alcohols with 2 or more OH groups

Answer 312

glycols

Question 313

[common reactions in alcohols] reaction with acids to form esters

Answer 313

glycols

Question 314

[common reactions in alcohols] primary alcohols oxidize into aldehydes, secondary alcohols oxidize into ketones

Answer 314

oxidation

Question 315

most common aldehydes

Answer 315

carbohydrates

Question 316

[types & nomenclatures of unsaturated hydrocarbons] contains a carbonyl group at the end of the chain

Answer 316

aldehydes

Question 317

properties of aldehydes

Answer 317

carbonyl group is attached to the end of the alkyl chain, and is a serious air pollutant

Question 318

example of aldehyde that is very toxic to microorganisms and is used as an embalming fluid

Answer 318

formalin

Question 319

example of aldehyde that is a common industrial manufacturing chemical

Answer 319

acetyldehyde

Question 320

[types & nomenclatures of unsaturated hydrocarbons] carbonyl group in the middle of alkyl chain, commonly used as solvents and for industrial manufacturing

Answer 320

ketones

Question 321

[type of ketone] simplest ketone produced from the oxidation of isopropyl alcohol

Answer 321

acetone [dimethyl ketone]

Question 322

[type of ketone] produced from the oxidation of 2-butanol

Answer 322

methyl ethyl ketone

Question 323

properties of ketone

Answer 323

can be oxidized to form its corresponding acid

Question 324

[types & nomenclatures of unsaturated hydrocarbons] highest oxidation state or organic compounds, contains 1 or more carboxyl group

Answer 324

carboxylic acids

Question 325

most common carboxylic acid

Answer 325

free-fatty acids

Question 326

actual source of bod energy are

Answer 326

fats

Question 327

[types of c. acids] contain 1 carboxylic group, commonly known as fatty acids

Answer 327

saturated monocarboxylic

Question 328

[types of c. acids] form metallic acids, can be reduced into saturated acids, used as food by microorganisms

Answer 328

unsaturated monocarboxylic

Question 329

principal acids of unsaturated monocarboxylic

Answer 329

acrylic, oleic, linoleic

Question 330

[types of c. acids] the most important species are the ones that have 2 carboxylic groups one on each end

Answer 330

polycarboxyllic

Question 331

[types of c. acids] contains OH other than c. acid, some species are optically active

Answer 331

hydroxy

Question 332

[types & nomenclatures of unsaturated hydrocarbons] formed by the reaction between acids and alcohols, commonly used in chemical manufacturing, solvents, flavoring extracts and perfumes

Answer 332

esters

Question 333

most common ester

Answer 333

triglycerides

Question 334

alcohol groups and fatty acids are

Answer 334

esterified

Question 335

[types & nomenclatures of unsaturated hydrocarbons] formed by treating alcohols with strong dehydrating agents, has an oxygen sandwiched between 2 organic groups, widely used as a solvent, highly flammable

Answer 335

ethers

Question 336

ethers are susceptible to forming peroxides that are highly explosive when exposed to

Answer 336

air

Question 337

ethers are resistant to

Answer 337

biological oxidation

Question 338

[types & nomenclatures of unsaturated hydrocarbons] organic compounds that contain halogens

Answer 338

alkyl halides and halogenated aliphatic compounds

Question 339

[types & nomenclatures of unsaturated hydrocarbons] nitrogen containing aliphatic compounds

Answer 339

amines, amides, nitriles

Question 340

common example of amines

Answer 340

amino acids

Question 341

[types & nomenclatures of unsaturated hydrocarbons] derived from the reaction between organic acids and ammonia

Answer 341

amides

Question 342

[type of nitrogen containing a. compounds] called naphthenes, have 2 H atoms connected to each C atom

Answer 342

cyclic aliphatic compounds

Question 343

[type of nitrogen containing a. compounds] contains sulfur

Answer 343

mercaptans and thioalcohols

Question 344

cyclic organic compounds with alternating single and double bonds

Answer 344

aromatic compounds

Question 345

parent compound of aromatic compounds

Answer 345

benzene

Question 346

[aromatic hydrocarbons] benzene examples

Answer 346

toluene, ethylbenzete

Question 347

[aromatic hydrocarbons] polyring hydrocarbon example

Answer 347

naphthalene

Question 348

types of aromatic copounds

Answer 348

aromatic hydrocarbons and phenols

Question 349

types of aromatic hydrocarbons

Answer 349

benzenes and polyring hydrocarbons

Question 350

[type of aromatic compound] contains OH

Answer 350

phenols

Question 351

types of phenols

Answer 351

monohydroxy phenols, polyhydroxy phenols

Question 352

[type of monohydroxy phenols] contains alkyl groups

Answer 352

cresols and other alkylphenols

Question 353

[type of monohydroxy phenols] contains chlorine

Answer 353

chlorinated phenols

Question 354

cyclic organic compounds with double bonds or with other elements in the ring

Answer 354

heterocyclic compounds

Question 355

[common food and related compounds] types of carbohydrates

Answer 355

monosaccharides, disaccharides, polysaccharides

Question 356

types of monosaccharides

Answer 356

glucose, fructose, galactose, mannose

Question 357

sweet monosaccharide

Answer 357

fructose

Question 358

types of disaccharides

Answer 358

sucrose [table sugar], maltose

Question 359

fructose is also a

Answer 359

ketohexose

Question 360

glucose is also a

Answer 360

aldohexose

Question 361

[fats, oils, waxes] fatty acid glycerides that are solid at room temp.

Answer 361

fats

Question 362

[fats, oils, waxes] fatty acid glycerides that are liquid at room temp.

Answer 362

oil

Question 363

[fats, oils, waxes] esters of long-chain acids and alcohols

Answer 363

waxes

Question 364

building blocks of protein

Answer 364

amino acids

Question 365

[other organic compounds] contains surfactants that consists of il soluble parts and water soluble parts

Answer 365

detergents

Question 366

[other organic compounds] derived from saponification of fats and oils

Answer 366

soaps

Question 367

[additional] indicator: benedicts solution

Answer 367

simple carbohydrates turns brick red for positive

Question 368

[additional] indicator: iodine solution

Answer 368

complex carbohydrates turns black if positive

Question 369

[additional] indicator: biuret solution

Answer 369

protein, turns violet black if positive

Question 370

[additional] indicator: sudan IV

Answer 370

lipids, turns reddish-orange if positive

Question 371

[additional] examples of non-polar amino acids

Answer 371

glycine, alanine, valine, leucine, isoleucine, methionine, tryptophan, phenylalanine, proline

Question 372

[additional] examples of polar amino acids

Answer 372

serine, threonine, cysteine, tyrosine, asparagine, glutamine

Question 373

[additional] examples of polar charged amino acids

Answer 373

acidic: aspartic acid, glutamic acid; basic: lysine, arginine, histidine