Chemistry Exam Vocab

Front 1

Absolute zero

Back 1

zero on the Kelvin scale

Front 2

accepted value

Back 2

the correct value based on reliable references

Front 3

accuracy

Back 3

how close a measurement comes to the actual value

Front 4

atom

Back 4

the smallest particle of an element that retains the properties of the element

Front 5

atomic number

Back 5

equals the number of protons. never changes. on the bottom if you are writing the element.

Front 6

Bohr model

Back 6

the older model of the atom. Where the electrons travel in a definite orbit around the nucleus.

Front 7

Celsius scale

Back 7

a measure of temperature, where the freezing point is 0 and the boiling point is 100.

Front 8

chemical change

Back 8

implies that a substance has decomposed into a new substance or has been mixed with another chemical to form a new substance.

Front 9

chemical property

Back 9

the ability of a substance to undergo a chemical reaction and from new substances.

Front 10

chemical reaction

Back 10

one or more substances change into new substances.

Front 11

chemistry

Back 11

the study of the composition of matter and the changes it undergoes.

Front 12

compound

Back 12

substances that can be separated into simpler substances only by chemical means

Front 13

density

Back 13

the ratio of the mass of an object to its volume

Front 14

electron

Back 14

negatively charged subatomic particles, in clouds around the nucleus, mass is negligible compared to the nucleus.

Front 15

element

Back 15

the simplest forms of matter that can exist under normal laboratory conditions.

Front 16

error

Back 16

the difference between the accepted value and the experimental value.

Front 17

experimental value

Back 17

the value measured in lab.

Front 18

temperture

Back 18

the measure of the average kinetic energy of a substance

Front 19

gas

Back 19

a form of matter that takes both the shape and volume of its container.

Front 20

group

Back 20

each vertical column of elements in the periodic table.

Front 21

heterogeneous

Back 21

a mixture that is not uniform in composition. It doesn't have just one part, it would be easy to take it apart.

Front 22

homogeneous

Back 22

a mixture that has a completely uniform composition. It would be difficult to take apart.

Front 23

hypothesis

Back 23

a proposed explanation or reason for your observation.

Front 24

isotope

Back 24

atoms that have the same number of protons, but different number of neutrons.

Front 25

Kelvin scale

Back 25

the absolute scale for temperature. 0 is is absolute zero.

Front 26

Law of Conservation of Mass

Back 26

states that in any physical change or chemical reaction, mass is neither created nor destroyed.

Front 27

liquid

Back 27

a form of matter that flows, has a fixed volume, but not shape, and takes the shape of the container its in.

Front 28

mass

Back 28

the amount of matter in an object

Front 29

mass number

Back 29

protons + neutrons. on top if you are writing the element symbol. also called the atomic mass

Front 30

mattter

Back 30

anything that has mass and takes up space.

Front 31

metal

Back 31

have a high electrical conductivity and a high luster when clean, they are malleable and ductile

Front 32

metalloid

Back 32

elements with properties that are intermediate between those of metals and nonmetals

Front 33

mixture

Back 33

a physical blend of two or more substances

Front 34

neutron

Back 34

subatomic particles with no charge, in the nucleus

Front 35

nonmetal

Back 35

elements that are generally nonlusterous and poor conductors of electricity

Front 36

observation

Back 36

using senses to obtain information directly

Front 37

percent error

Back 37

the absolute value of the accepted value minus the experimental value, divided by the accepted value, times by 100. written as a percent. (|acc-exp|/acc)x100

Front 38

period

Back 38

the horizontal rows of the periodic table

Front 39

physical change

Back 39

implies that no new substance is formed

Front 40

physical property

Back 40

a quality or condition of a substance that can be observed or measured without changing the substances composition

Front 41

precision

Back 41

how close measurements are to one another

Front 42

product

Back 42

the substances formed from a chemical reaction.

Front 43

proton

Back 43

positively charged, located in the nucleus, have a mass of one amu.

Front 44

qualitative measurement

Back 44

results that are descriptive without using numbers.

Front 45

quantitative measurement

Back 45

results that use numbers and units to describe the measurement.

Front 46

quantum model

Back 46

new model of an atom that states the probability of finding an electron in certain spot.

Front 47

reactant

Back 47

the starting substances in a chemical reaction.

Front 48

scientific notation

Back 48

a number written as the product of two numbers, the second being 10 raised to a power because the number is so large.

Front 49

significant figures

Back 49

all the digits that can be known precisely in a measurement, plus a last estimated digit

Front 50

solid

Back 50

matter that has a definite shape and volume

Front 51

strong force

Back 51

when subatomic particles are so very close together that they start to attract. they override repulsion forces.

Front 52

vapor

Back 52

describes the gaseous state of a substance that is generally liquid at room temperature

Front 53

weight

Back 53

a force that measure the pull on a given mass by gravity

Front 54

volume

Back 54

the amount of matter an object takes up

Front 55

nuclear reactions

Back 55

when changes occur in the atom's nucleus. produce alpha, beta and gamma radiation

Front 56

energy level

Back 56

around the nucleus where the electron is found. 7 of them right now

Front 57

quantum

Back 57

the amount of energy required to move an electron from its present level of energy to the next higher one.

Front 58

quantum mechanical model

Back 58

the modern description of the electrons in atoms, which uses a mathematical equation to describe the location and energy of an electron.

Front 59

atomic orbitals

Back 59

the region in which electrons are likely to be found in an atom.

Front 60

electron configurations

Back 60

shows where and how electrons are located around the nucleus.

Front 61

Aufbau principle

Back 61

electrons enter orbitals of lowest energy first

Front 62

Pauli Exclusion Principle

Back 62

an atomic orbital can have a maximum of 2 electrons

Front 63

Hund's Rule

Back 63

when electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins

Front 64

Eletromagnetc Radiation

Back 64

light

Front 65

amplitude

Back 65

from the midpoint to the crest of a wave

Front 66

wavelength

Back 66

from crest to crest

Front 67

Heisenberg's Uncertainty Principle

Back 67

states that its impossible to know exactly both the velocity and the position of a particle at the same time.

Front 68

frequency

Back 68

the number of wave cycles to pass a given point per unit of time.

Front 69

hertz

Back 69

the SI unit o f cycles per second. Hz. sec^-1 or 1/sec

Front 70

spectrum

Back 70

the different wavelengths of color when sunlight passes through a prism.

Front 71

atomic emission spectrum

Back 71

when an electric discharge goes through a gas or vapor, the element absorbs energy, then loses it as light. is unique to each element, consist of specific lines, which correspond to a different amount of energy, used to identify elements

Front 72

Planck's constant

Back 72

the constant (h) in the energy of a quantum (h*v)

Front 73

photons

Back 73

light quanta that behaves like particles

Front 74

photoelectric effect

Back 74

when the intensity of photons of the light is strong enough, electrons are ejected from the metal.

Front 75

ground state

Back 75

the lowest energy level of an element's atom.

Front 76

de Broglies equation

Back 76

predicts that all matter exhibits wavelike motions

Front 77

atomic radius

Back 77

one half the distance between the nuclei of two like atoms in a diatomic molecule

Front 78

ionization energy

Back 78

the energy required to overcome the attraction of the nuclear charge and remove an electron from a gaseous atoms

Front 79

electronegativity

Back 79

the tendency for the atoms of the element to attract electrons when they are chemically combined with atoms of another element.

Front 80

electron affinity

Back 80

the energy given off when a neutral atom in gas phase gains an extra electron to form a negatively charged ion.

Front 81

valence electron

Back 81

the electrons in the highest occupied energy level of an elements atom.

Front 82

periodic table

Back 82

an arrangement of the elements according to similarities in their properties

Front 83

periodic law

Back 83

when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

Front 84

groups

Back 84

columns on the periodic table

Front 85

families

Back 85

the columns that have certain names on the periodic table. ex: alkali metals

Front 86

periods

Back 86

rows on the periodic table

Front 87

Alkali metals

Back 87

1A elements

Front 88

alkaline earth metals

Back 88

2A elements

Front 89

halogens

Back 89

7A elements

Front 90

noble gases

Back 90

8A elements

Front 91

transition metals

Back 91

1B-10B elements

Front 92

inner transition metals

Back 92

lanthanides and actinides

Front 93

metals

Back 93

solid, high conductivity of heat and electricity, left side of the periodic table, malleable, ductile

Front 94

nonmetals

Back 94

solids, liquids, or gases; poor conductors, nonmalleable, nonductile, right side of periodic table.

Front 95

metalloids

Back 95

semi-conductors--Si based computer chips; right side of periodic table

Front 96

lanthanides

Back 96

inner transition metals, 6 period

Front 97

actinides

Back 97

inner transition metals, 7 period

Front 98

ductile

Back 98

the ability to be drawn into wires

Front 99

malleable

Back 99

the ability to be hammered or forced into shapes

Front 100

activity

Back 100

the ease with which a metal reacts

Front 101

solubility

Back 101

the amount that dissolves in a given quantity of a solvent at a given temperature to produce a saturated solution

Front 102

precipitate

Back 102

when a solid forms from a reaction

Front 103

acid

Back 103

a compound that produces hydrogen ions in solution, a hydrogen-ion donor, or an electron-pair acceptor

Front 104

alloy

Back 104

mixture composed of two or more elements, at least one of which is a metal

Front 105

anion

Back 105

any atom or gorup of atoms with negative charge

Front 106

binary compound

Back 106

compound composed of two different elements

Front 107

cation

Back 107

positive charged ions

Front 108

chemical formula

Back 108

shows the kinds and numbers of atoms in the smallest representative unit of the substance

Front 109

covalent bond

Back 109

a bond in which tow atoms share a pair of electrons

Front 110

diatomic molecule

Back 110

elements that are present in the gaseous state as molecules composed of tow atoms when they are by themselves

Front 111

double bond

Back 111

covalent bonds that share two pairs of electrons

Front 112

formula unit

Back 112

the lowest whole-number ratio of ions in an ionic compound

Front 113

ion

Back 113

atoms or groups of atoms that have a positive or negative charge

Front 114

ionic bond

Back 114

formed when there is a transfer of electrons to the more electronegative atom

Front 115

ionic compound

Back 115

compounds composed of cations and anions

Front 116

law of definite proportions

Back 116

states that in samples of any chemical compound, the masses of the elements are always in the same proportions

Front 117

law of multiple proportions

Back 117

whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers

Front 118

lewis dot structure

Back 118

diagrams that show valence electrons as dots

Front 119

metallic bond

Back 119

why metals conduct electricity, tend to form crystals, bonding in metals

Front 120

molecular compounds

Back 120

composed of two or more nonmetals. uses prefixes

Front 121

molecular formula

Back 121

shows the kinds and numbers of atoms present in a molecule of a compound

Front 122

molecule

Back 122

smallest electrically neutral unit of a substance that still has the properties of that substance

Front 123

monatomic ion

Back 123

ions consisting of only one element

Front 124

octet rule

Back 124

in forming compounds, atoms tend to achieve the electron configuration of a noble gas

Front 125

polarity

Back 125

when a covalent bond joins two atoms of different elements and the bonding electrons are shared unequally.

Front 126

polyatomic ion

Back 126

element composed of many atoms

Front 127

resonance

Back 127

when electron pairs rapidly flip back and forth

Front 128

ternary compound

Back 128

compounds of 3 elements

Front 129

triple bond

Back 129

covalent bonds that involve three shared pairs of electrons

Front 130

VSEPR

Back 130

states that because electron pairs repel, molecular shape adjusts so the valence electron pairs are as far apart as possible

Front 131

empirical formula

Back 131

the lowest whole-number ratio of the atoms of the elements in a compound

Front 132

molecular formula

Back 132

shows the kinds and numbers of atoms present in a molecule of a compound

Front 133

activity series of metals

Back 133

lists metals in order of decreasing activity. determines whether one metal will replace another metal in a single replacement reaction

Front 134

aqueous

Back 134

dissolved in water

Front 135

balanced equation

Back 135

each side of the equation has the same number of atoms of each element

Front 136

catalyst

Back 136

a substance that increases the rate of a reaction without being used up itself during the reaction

Front 137

chemical equation

Back 137

an equation that represents a chemical reaction, where the reactants and products are connected with an arrow

Front 138

coefficient

Back 138

numbers placed in front of the symbols for the respective parts of a balanced equation

Front 139

combination reaction

Back 139

2 or more reactants combine to form one product.
A+B=AB

Front 140

combustion reaction

Back 140

burning in the presence of oxygen

Front 141

complete ionic equation

Back 141

represent soluble ionic compounds as separated ions

Front 142

covalent bond

Back 142

a bond in which tow atoms share a pair of electrons

Front 143

decomposition reaction

Back 143

one reactant breaks down into two ore more products.
can be explosive.

Front 144

dissociate

Back 144

the breaking down of a compound into its components

Front 145

double replacement reaction

Back 145

exchange of cations.
AB+CD=CB+AD

Front 146

ionic bond

Back 146

the forces of attraction that bind cations and anions

Front 147

metallic bond

Back 147

the attraction of valence electrons towards positively charged meal ions

Front 148

net ionic equation

Back 148

the equation that indicates only those particles that actually take part in the reaction

Front 149

octet rule

Back 149

in the formation of compounds atoms tend to achieve the configuration of a noble gas.

Front 150

precipitate

Back 150

when a solid forms from a reaction

Front 151

spectator ion

Back 151

ions that are not directly involved in a reaction

Front 152

single replacement reaction

Back 152

one element replaces another element in a compound.
A+BC=AC+B

Front 153

mole (mol)

Back 153

equals 6.02x(10^24)
we use this because atoms are so small, we need a way to quantize large quantities

Front 154

Avagadro's number

Back 154

6.02*10^24
the number of representative particles contained in one mole.

Front 155

representative particles

Back 155

the species present in a substance, usually atoms, molecules, or formula units (ions)

Front 156

gram atomic mass

Back 156

the atomic mass of an element expressed in grams (gam)

Front 157

gram molecular mass

Back 157

mass of 1 mole of that compound (gmm)

Front 158

gram formula mass

Back 158

the mass of one mole of an ionic compound (gfm)

Front 159

molar mass

Back 159

the mass in grams of any one mole of the substance.
use the periodic table to find this with the atomic mass

Front 160

STP

Back 160

standard temperature and pressure.
the condition at which the volume of a gas is measured.
T=0 C
P=1 atm

Front 161

molar volume

Back 161

1 mole of gas' volume at STP

Front 162

percent composition

Back 162

the relative amounts of each element in a compound.
percent by mass of each element in the compound

Front 163

thermochemistry

Back 163

concerned with the heat changes that occur during chemical reactions

Front 164

energy

Back 164

the capacity for doing work or supplying heat

Front 165

chemical potential energy

Back 165

energy stored within the structural units of chemical substances

Front 166

heat

Back 166

the flow of energy from a warmer object to a colder one (q)

Front 167

system

Back 167

is the reaction in a calorimeter. the part of the universe on which you focus your attention

Front 168

surroundings

Back 168

is the water in a calorimeter. the remainder of the universe that is outside the system.

Front 169

law of conservation of energy

Back 169

states that in any chemical or physical process, energy is neither created or destroyed

Front 170

endothermic process

Back 170

absorbs heat. feels cold.
change in enthalpy is positive

Front 171

exothermic process

Back 171

releasing heat. feels warm. change in enthalpy is negative

Front 172

calorie

Back 172

the amount of heat required to raise the temperature of 1 gram of pure water 1 degree C

Front 173

Joule

Back 173

the SI unit of heat and energy. 4.184= 1 cal.

Front 174

heat capacity

Back 174

amount of heat needed to raise the temperature of an object exactly 1 degree C. depends on mass and chemical composition of an object

Front 175

specific heat capacity

Back 175

the amount of heat it takes to raise the temperature of 1 gram of the substance 1 degree C.

Front 176

specific heat

Back 176

the amount of heat needed to raise the temperature of 1 gram of a substance 1 degree C.

Front 177

calorimetry

Back 177

accurate and precise measurement of heat change for chemical and physical processes.

Front 178

calorimeter

Back 178

the insulated device used to measure the absorption or release of heat in chemical or physical properties

Front 179

enthalpy (H)

Back 179

heat content at constant pressure

Front 180

thermochemical equation

Back 180

a chemical equation that includes the amount of heat produced or absorbed during the reaction.

Front 181

heat of reaction

Back 181

the heat change from the reaction exactly as it is written

Front 182

heat of combustion

Back 182

the heat of reaction for the complete burning of one mole of a substance

Front 183

molar heat of fusion

Back 183

the heat absorbed by one mole of a substance in melting from a solid to a liquid at a constant temperature

Front 184

molar heat of solidification

Back 184

the heat lost when one mole of a liquid solidifies at a constant temperature

Front 185

molar heat of vaporization

Back 185

the amount of heat necessary to vaporize one mole of a given liquid

Front 186

molar heat of condensation

Back 186

the amount of heat released when one mole of vapor condenses

Front 187

molar heat of solution

Back 187

the heat change caused by dissolution of one mole of substance

Front 188

Hess's law of heat summation

Back 188

if a series of reactions are added together the enthalpy change for the net reaction will be the sum of the enthalpy changes for the individual steps.

Front 189

standard heat of formation

Back 189

the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states at 25 degrees C.

Front 190

universe

Back 190

the totality of all existing things. the system and the surroundings

Front 191

Avagadro's hypothesis

Back 191

the number of mols of a gas is directly related to the volume of the gas

Front 192

Dalton's Law of Partial Pressures

Back 192

at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases

Front 193

gases

Back 193

take the volume of their container, compressible, diffusion occurs quickly, flows readily, few intermolecular forces

Front 194

liquids

Back 194

diffusion occurs slowly, strong intermolecular forces, take the form of their container,flow, fixed volume, and no definite shape

Front 195

solids

Back 195

definite shape and volume, virtually incompressible, doesn't flow, diffusion occurs slowly, strong intermolecular forces.

Front 196

condenses states of matter

Back 196

the liquid and solid phases, in which the particles interact strongly

Front 197

intermolecular forces

Back 197

forces between individual molecules of a substance

Front 198

boiling point

Back 198

the temperature at which the vapor pressure of a liquid is equal to the applied external pressure

Front 199

melting point

Back 199

the temperature at which a substance changes from a solid to a liquid.

Front 200

ion-dipole force

Back 200

intermolecular forces exist between an ion and the partial charge on the end of a polar molecule

Front 201

dipole-dipole force

Back 201

a separation of charge on a molecule- think electronegativity

Front 202

London dispersion force

Back 202

the weakest of all molecular interactions, are caused by electron motion

Front 203

Hydrogen bonding

Back 203

strongest intermolecular force, only occurs when H is bonded to F,O, or N. weaker than chemical bonds.

Front 204

viscosity

Back 204

an internal ability of a fluid that has resistance to flow.

Front 205

surface tension

Back 205

the imbalance of forces at the surface of a liquid

Front 206

cohesive force

Back 206

all the forces of attraction among particles of a liquid

Front 207

adhesive force

Back 207

attractions between a liquid and another surface.

Front 208

capillary action

Back 208

when adhesive forces overcome cohesive forces, a liquid is drawn up inside a small-bore tube

Front 209

condensation

Back 209

vapor or gas to liquid

Front 210

sublimation

Back 210

solid to gas

Front 211

melting

Back 211

solid to liquid

Front 212

evaporation

Back 212

vaporization that occurs at the surface of a liquid.

Front 213

deposition

Back 213

gas to solid

Front 214

freezing

Back 214

liquid to solid

Front 215

critical temperature

Back 215

the temperature of a pure element or compound at a critical point

Front 216

critical pressure

Back 216

the pressure of a pure element or compound at a critical point

Front 217

vapor pressure

Back 217

force due to the gas above the liquid

Front 218

volatile

Back 218

rapid evaporation. passing off readily in the form of vapor

Front 219

normal boiling point

Back 219

the boiling point of a liquid at a pressure of 101.3 kPa

Front 220

phase diagram

Back 220

a graphical way to summarize the conditions under which equilbria exist between the different states of matter.

Front 221

normal melting point

Back 221

the melting point of a substance at 1.0 atm.

Front 222

triple point

Back 222

where 3 curves on a phase diagram meet.

Front 223

crystalline solid

Back 223

have an orderly arrangement of their component ions

Front 224

unit cell

Back 224

the smallest group of particles within a crystal that retains the geometric shape of the crystal.

Front 225

crystal lattice

Back 225

a repeating array of any one of fourteen kinds of unit cells

Front 226

amorphous solid

Back 226

solids that lack an ordered internal structure.
randomly arranged

Front 227

metallic solids

Back 227

good conductors, malleable, ductile.
a solid that has properties of a metal. positive ions surrounded by many mobile valence electrons

Front 228

molecular solids

Back 228

a substance that consists of individual molecules held together in the solid by relatively weak intermolecular bonds. low melting points, don't conduct well

Front 229

ionic solids

Back 229

have high melting points because strong forces hold them together. oppositely charged ions attract each other.

Front 230

covalent-network solid

Back 230

substance which consists of an array of atoms held together by an array of covalent bonds without forming molecules

Front 231

dipole moment

Back 231

a separating of charge on a molecule

Front 232

polar molecule

Back 232

a molecule with a nonzero dipole moment

Front 233

pressure

Back 233

the force exerted per unit area

Front 234

ideal gas law

Back 234

PV=nRT

Front 235

kinetic molecular theory

Back 235

6 postulates that describe how an ideal gas behaves. 3 are assumptions that technically aren't true about real pressures. most behave like ideal gases at normal temp. and pressure

Front 236

real gas

Back 236

don't follow the kinetic molecular theory at certain temperatures and pressures

Front 237

charle's law

Back 237

states that the volume of a fixed mass of a gas is directly proportional to its temperature if the pressure is kept constant and the number of mols are held constant.
V/T=V/T

Front 238

boyle's law

Back 238

states that for a given mass of gas a constant temperature, the volume of the gas varies inversely with pressure, when the number of moles is held constant.
PV=PV

Front 239

vapor

Back 239

describes the gaseous state of a substance that is generally a liquid or solid at room temperature

Front 240

partial pressure

Back 240

the pressure exerted by each gas in a gaseous mixture.

Front 241

monometer

Back 241

device used to determine the vapor pressure of a liquid.
can be closed or open ended

Front 242

gas constant

Back 242

8.134 joules per degree Kelvin. equal to the product of the pressure and the volume of one gram molecule of an ideal gas divided by the absolute temperature.

Front 243

boiling point elevation

Back 243

the difference in temperature between the boiling point of a solution and of the pure solution

Front 244

colligative property

Back 244

depends not on the kind, but the amount of solute particles

Front 245

concentrated solution

Back 245

a solution containing a large amount of solute

Front 246

concentration

Back 246

a measurement of the amount of solute that is dissolved in a gram quantity of solvent; usually expressed in mol/L

Front 247

dilute solution

Back 247

solution that contains a small amount of solute

Front 248

freezing point depression

Back 248

the difference in temperature between the freezing point of a solution and of the pure solvent

Front 249

Henry's Law

Back 249

solubility of a gas is proportional to the partial pressure of the gas above the liquids.
ex: soda pop

Front 250

immiscible

Back 250

liquids that can't mix in any proportion

Front 251

miscible

Back 251

liquid solutions that can mix in any solution

Front 252

molar boiling point elevation constant

Back 252

the change in boiling point for a 1 molol solution of a nonvolatile molecular solute.

Front 253

molar freezing point depression constant

Back 253

the change in freezing point for a 1 molol solution of a nonvolatile molecular solute

Front 254

molality

Back 254

moles of solute dived by kg of solvent

Front 255

molarity

Back 255

moles of solute dived by L of solution

Front 256

mole fraction

Back 256

moles of component divided by the total moles of the solution

Front 257

saturated solution

Back 257

when no more solute can be dissolved in a solution

Front 258

solubility

Back 258

how much of a solute will dissolve in a solvent at a certain temperature

Front 259

solute

Back 259

the substance that is dissolved

Front 260

solution

Back 260

a homogeneous mixture of tow or more substances in a single physical state

Front 261

solvent

Back 261

the substance that does the dissolving

Front 262

supersaturated solution

Back 262

solution that contains more solute than can be dissolved

Front 263

unsaturated

Back 263

solution that has less solute than can be dissolved

Front 264

acid

Back 264

a compound that produces hydrogen ions in solution, a hydrogen-ion donor, or electron-pair acceptor

Front 265

base

Back 265

a compound that produces hydroxide ions in solution, hydrogen-ion acceptor, or electron-pair donor

Front 266

hydroxide ion

Back 266

(OH^-) the negative ion formed when a water molecule loses a hydrogen ion.

Front 267

hydranium ion

Back 267

(H30^+) the positive ion formed when a water molecule gains a hydrogen ion

Front 268

neutral solution

Back 268

an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal.

Front 269

acidic solution

Back 269

any solution in which the hydrogen ion concentration is greater than the hydroxide-ion concentration

Front 270

basic solution

Back 270

any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration

Front 271

alkaline solutions

Back 271

another name for basic solutions

Front 272

pH

Back 272

measures the acidity of a solution

Front 273

monoprotic

Back 273

any acid that contains one ionizable proton

Front 274

diprotic

Back 274

any acid that contains two ionizable protons

Front 275

triprotic

Back 275

any acid that contains three ionizable protons

Front 276

conjugate acid

Back 276

the particle formed when a base gains a hydrogen ion

Front 277

conjugate base

Back 277

the particle that remains when an acid has donated a hydrogen ion

Front 278

lewis acid

Back 278

any substance that can accept a pair of electrons to form a covalent bond.

Front 279

lewis base

Back 279

any substance that can donate a pair of electrons to form a covalent bond

Front 280

amphoteric

Back 280

a substance that can act as both acid and base

Front 281

strong acid

Back 281

an acid that is completely ionized in aqueous solutions

Front 282

weak acid

Back 282

an acid that is only slightly ionized in aqueous solution.

Front 283

strong base

Back 283

a bas that completely dissociates into metal ions and hydroxide ions in aqueous solution.

Front 284

weak base

Back 284

a base that does not dissociate completely in aqueous solution