Chem Regents Final

Front 1

daltons atomic theory

Back 1

1. all elements are composed of indivisible atoms
2. all atoms of a given element are identical
3. atoms of different elements are different
4. compounds are formed by the combination of atoms of different elements

Front 2

jj thompson

Back 2

cathode ray- electrons with negative charge

Front 3

plum pudding

Back 3

electrons spread out- positively charged with mass evenly distributed

Front 4

rutherford

Back 4

gold foil- some alpha particles get deflected- atoms have a dense central core, called a nucelus, while the rest of the atom is empty space

Front 5

bohr atom

Back 5

dense nucleus with electrons found in surrounding circular orbits- electrons can move to different energy levels- also called planetary model- was not entirely supported

Front 6

wave-mechanical model

Back 6

atom has a dense, positively charge nucleus but the electrons, instead of beinng in definite, fixed orbits, had fixed amounts of energy moving in areas called orbitals

Front 7

orbital

Back 7

a region in which an electron of a particular amount of energy is most likey to be located

Front 8

masses of subatomic particles

Back 8

protons and nuetrons - 1amu
electrons- 1/1836 amu

Front 9

what does each atom of a specific element need to contain

Back 9

the same number of protons as each other atom of that element

Front 10

atomic number

Back 10

the number of protons in the nucelus of an atom

Front 11

mass number

Back 11

the sum of the number of protons and neutrons in an atom

Front 12

isotopes

Back 12

atoms of the same element that have a different number of neutrons and different mass numbers

Front 13

C-12 isotope, what does 12 represent

Back 13

12 is the mass number

Front 14

how do youy calculate the number of neutrons in an isotope

Back 14

it is the difference between the atomic number of the atom and its mass number

Front 15

atomic mass

Back 15

average mass of all the isotopes in a sample of the element

Front 16

ground state

Back 16

when the electrons occupy the lowest availablee orbitals

Front 17

excited state

Back 17

when the electrons are subjected to stimuli such as heat, light,m or electricity, an electron may absorb energy and temproarily move to a higher energy level, which makes it in n unstable condition called an excited state

Front 18

what happens to energgy when an electron moves up/down an energy level

Back 18

up=gains energy
down=emits energy
(always a specific amount of energy)

Front 19

what does the energy look like that is emitted from electrons

Back 19

it comes in the form of infrared, ultraviolet, or visible light

Front 20

what does visible light emitted by electrons look like

Back 20

bright line spectra

Front 21

how does the bright line spectra help us to identify elements

Back 21

individual elements always have hte same lineson the bright line spectra

Front 22

what determines the chemical properties of an atom

Back 22

the arrangement of electrons- the number of electrons in the outer energy level of its atoms (aka the number of valence electrons)

Front 23

principal quantum number

Back 23

the same number as the number of the energy level that contains the electron

Front 24

sublevels

Back 24

s, p, d, f

Front 25

how many orbitals do the sublevels have?

Back 25

s- one
p- three (px, py, pz)
d- 5 orbitals
f- seven orbitals

Front 26

shape of s orbital

Back 26

spherical shapes without sharp edges surrounding the nucelus

Front 27

shape of p orbital

Back 27

dumbbell shape at right angles

Front 28

max number of electrons in each prinicipal energy level

Back 28

1- 2
2- 8
3- 18
4- 32

Front 29

node

Back 29

where it is unlikely to find an electron

Front 30

hunds rule

Back 30

a single electron must be placed into each orbital of a given sublevel before any pairing takes place

Front 31

what comes before 3d

Back 31

4s

Front 32

what comes before 4d

Back 32

5s

Front 33

homogenous

Back 33

uniform throughout- can contain more than one type of particle but particles are evenly mixed

Front 34

heterogenous

Back 34

are made up pf parts with different chemical and physical properties that are not uniformly mixed or dispersed

Front 35

pure substance

Back 35

its composition is the same throughout the sample

Front 36

2 examples of pure substances

Back 36

elements and compounds

Front 37

elements

Back 37

substances that cannot be broken down or decomposed into simpler substances by chemical means

Front 38

compounds

Back 38

composed of two or more elements that are chemically combined in definite proportions by mass- is still the same composition throughout

Front 39

law of definite proportions

Back 39

types of atoms in a compound exist in a fixed ratio

Front 40

mixture

Back 40

combinations of two or more pure substances that can be separated by physical means

Front 41

how are mixtures different from compounds

Back 41

1. their composition is not deifnite or "fixed"; no ratio
2. can be separated by physical means
3. in a mixture, the parts contain their properties; do not in a compound (compound has its own properties)

Front 42

what elements exist in nature as two identical atoms covalently vonded into a diatomic molecule

Back 42

Br, I, N, Cl, H, O, F
(BrINCLHOF)

Front 43

qualitative info

Back 43

relates to things that cannot be counted or measured

Front 44

quantitative info

Back 44

deals with things that can either be counted or measured

Front 45

empirical formula

Back 45

the simplest integer tatio in which atoms combine to form a compound

Front 46

ionic formulas

Back 46

indicate the ratio of the ions in a comound

Front 47

molecules

Back 47

units formed by covalently bonded substances

Front 48

molecular formula

Back 48

a multiple of the emprical formula

Front 49

ions

Back 49

are not neutral-- are either negative or positive and the neg. and pos. attract each other and forms a ratio that produces a neutral compound

Front 50

polyatomic ion

Back 50

a group of atoms covalently bonded together, possessing a charge

Front 51

how do compounds form

Back 51

1. aatraction of oppositely charged ions

Front 52

hydrate

Back 52

when wwater from some ioniic solutions evaporates, the solute forms a crystal lattice that binds water within the structure and forms a compound

Front 53

what do the oxidation numbers correspond to

Back 53

the group number (group one- 1+)

Front 54

order of ions in a binary ionic compound

Back 54

the positive first, then the negative

Front 55

how to name binary ionic compounds

Back 55

ex. NaCl
take the first ion
sodium
change the 2nd ion's ending to ide
chloride
sodium chloride
ex. MgS= magnisium sulfide

Front 56

how to name other ionic ocompunds

Back 56

if the metal is first, keep the name of the metal and the polyatomic ion
ex. KNO3= potassium nitrate

if the neg. is a nonmetal, the ending is -ide
ex. NH4Cl= ammonium chloride

Front 57

binary covalent compound

Back 57

contains 2 metals

Front 58

how do you determine the order of compounds in a binary covalent compound

Back 58

electronegativity- the one with the lower electronegativity is written first

Front 59

how to name binary covalent compounds

Back 59

ends in ide, but uses prefixes to tell how many atoms of each element are present
ex. CO- carbon monoxide
CO2- carbon dioxide
N2O4- dinitrogen tetroxide

Front 60

stock system

Back 60

used if a metal has more than one oxidation number
uses roman numerals to identify

Front 61

physical changes

Back 61

changes that do not result in the formation of a new substance, but only change in appearance
ex. phase changes

Front 62

chemical changes

Back 62

the identity of the products differs from the identity of the reactants
ex. bruning

Front 63

endothermic

Back 63

processes that require energy in order to occur
S->L->G
-lowers surrounding temp. bc energy is abosrbed from the surroundings
-products have more potential energy than the reactants bc the reactants absorb energy as they become products
H2O(s) + energy---> H2O(l)

Front 64

exothermic

Back 64

-processes that release thermal energy when they occur
G->L->S
-raises temp of surroundings bc energy is given off
-products have less potential energy than the reactants
x + y--> x + y + energy

Front 65

law of conservation of mass

Back 65

matter is neither created nor detroyed in chemical reactions- must be balanced

Front 66

the 4 major types of reactions

Back 66

1. synthesis (combination)
2. decomposition (analysis)
3. single replacement reactions
4. double replacement reactions

Front 67

synthesis reactions

Back 67

combination
-when 2 or more reactants combine to form a product
A+B--> AB

Front 68

decomposition

Back 68

-analysis
-reverse of synthesis
-a single compund is broken down (decomposed) into two or more simpler substances
AB--> A + B

Front 69

single replacement

Back 69

where one element replaces another element in a compound
-always involves an element and a compound
-metals replace metals
A + BX --> B + AX

Front 70

how do you know if a metal will replace another metal in a single replacement reaction/ a nonmetal reaplace a nonmetal

Back 70

table j- a metal higher opn the table will replace a metal lower on the table/ a nonmetal higher up is more reactive and will reaplace a nonmetal lower on the table

Front 71

double replacement reactions

Back 71

generally involve two soluble ionic compounds that react in solution to produce a precipitate, a gas, or a molecular compound such as water
AB + CD --> AD + CB

Front 72

3 ways you know if a double replacement reaction will occur

Back 72

1. one product is a solid
2. one product is a gas
3. a molecular substance like water is formed

Front 73

what is the masss of an atom in AMU relatively based on

Back 73

the mass of a carbon-12 atom (amu- 12)

Front 74

formula mass

Back 74

the sum of the atmic masses of all the atoms present (the number of atoms of each elemnt mutiplied by the amu, then add all together)

Front 75

gram formula mass

Back 75

in grams instead of amu
(also gram molecular mass if the elements form molecules)

Front 76

percentage composition

Back 76

the composition of a percentage of each element compared with the total mass of the compound

Front 77

how to find percent composition

Back 77

find the formula mass
divide the mass of the element you are trying to find by the formula mass, and mltiply by 100

Front 78

anhydrous

Back 78

srystals that contain attached water molecules

Front 79

avogadros number

Back 79

the number of particles in a mole of a substance
6.02 x 10^23

Front 80

mole

Back 80

the number of atoms of carbon pressent in 12 grams of c-12

Front 81

gram formula mass & moles

Back 81

the gram formula mass of any substance is the mass of one mole of that substance

Front 82

how to convvert grams to moles

Back 82

moles= number of grams x 1 mole
______
gram mass form

Front 83

how to convert moles to grams

Back 83

grams= number of moles X
gram mass form
_____________
1 mole

Front 84

solid phase

Back 84

-definite volume and shape
-rigid form
-crystalline stucture

Front 85

liquid phase

Back 85

-not as rigid as solid phase
-particles move past each other
-no definite shape, but deifnite volume

Front 86

gaseous phase

Back 86

-noo much attraction
-no definite volume or shape
-spread out

Front 87

fusion

Back 87

melting

Front 88

why does temp remain constant in heating and cooling curves even though heat is being added

Back 88

the heat is bsorbed in the form of potential energy- used to break bonds

Front 89

vaporization

Back 89

boiling

Front 90

on a curve, when are two phases present

Back 90

when the line is straight and temp is not increasing

Front 91

solidification

Back 91

freezing

Front 92

reverse opf boiling

Back 92

condensation

Front 93

sublimation

Back 93

solid changes directly to a gas

Front 94

deposition

Back 94

gas changes directly to a solid

Front 95

temperature

Back 95

measure of kinetic energy

Front 96

which way does heat flow

Back 96

from higher temp to the lower temp until the 2 are the same temp

Front 97

how to determine freezing and boiling points

Back 97

the freezing point/boiling ppoint of a substance is the equilibrium temperature of the two phases

Front 98

how to find kelvin

Back 98

celcius + 273

Front 99

calorimeter

Back 99

used to measure the amount of heat given off in a reaction

Front 100

heat of fusion

Back 100

the amount of heat needed to convert a unit mass of a substance from a solid to liquid at its melting point

Front 101

HEAT OF vaporization

Back 101

the amount of heat needed to convert a unit mass of a substance from its liquid phase to its vapor phase at constant temp

Front 102

kinetic molecular theory

Back 102

used to explain gases:
1. gases contain particles that are n constant, random, straight-line motion
2. gas particles collide with each other and with the wallsof the cnotain- energy is tranfered but not lost- elastic
3. gas partciles are separated- the volume occupied by the particles themselves is negligible
4. gas particles do not attract to eahc other

Front 103

what happens to the pressure if more gas particles are added

Back 103

increase- directy proportional

Front 104

what happens to the pressure of a gas if you increae the volume

Back 104

pressure decreases- indirectly related

Front 105

temp and volume relationship of a gas

Back 105

as temp increases, volume increases
-directly related

Front 106

temp and pressure relationship of a gas

Back 106

as temp increases, pressure increases
-directly related

Front 107

relationship of temp and velocity of a gas

Back 107

as temp increases, velocity increases

Front 108

2 things about the knetic molecular theory that is not completely correct bc it talks about ideal gases

Back 108

1. gas particles do not attract each other- there is small attraction sometimes
2. gas particles do not occupy volume- as pressure increases the volume can no longer be ignored

Front 109

what 2 gases are nearly ideal

Back 109

hydrogen and helium

Front 110

why do gases vary from ideal behavior

Back 110

1. increasing mass
2. increasing polarity

Front 111

where as gases most ideal

Back 111

at low pressures and high temperatures

Front 112

what are a few ways the components of a mixture can be separated?

Back 112

density, molecular polarity, freezing point, and boiling point

Front 113

immiscible

Back 113

two liquids that are not soluble in each other

Front 114

filtration

Back 114

can separate the mixture of a solid in a liquid or se[arate solids and gases

Front 115

separatory funnel

Back 115

separates two liquids by density

Front 116

distillation

Back 116

can separate homogenous solutions of solids dissolved in liquids - separate by boiling points

Front 117

miscible

Back 117

when liquids mix with each other

Front 118

chromatography

Back 118

can separate mixtures

Front 119

what can be separated with a paper filter

Back 119

a solid in a liquid

Front 120

how is gasoline separated into its components

Back 120

fractional distillation

Front 121

what is the principal that allows paper chrmatography to separate mixtures

Back 121

components having differnet attractions to the paper

Front 122

how did mendeleev first putthe periodic table

Back 122

in order of increasing atomic mass

Front 123

how is the periodic table now set up

Back 123

by increasing atomic number

Front 124

henry moseley

Back 124

used x-rays to identify the atomic number of the elements

Front 125

periodic law

Back 125

the properties of the elements are periodic functions of their atomic numbers

Front 126

periods

Back 126

horizontal rows on the table

Front 127

what does the number at the beginning of hte period indicate

Back 127

the principal energy level in which the valence electons are located

Front 128

properties in the period

Back 128

properties change across the period

Front 129

metalloids

Back 129

have some properties of metals and some of not metals
located 4 horizontal from group 13, with 2 in 14 and 2 in 15

Front 130

in what phase are metals and metalloidsa

Back 130

all solid except mercury

Front 131

what phases are nonmetals in

Back 131

all 3

Front 132

groups

Back 132

vertical columns

Front 133

what does each memeber of a given group contain, with a few exceptions

Back 133

the same number of valence electrons, and therefore similar chemical properties

Front 134

where are the most active metals located

Back 134

in group 1 and 21

Front 135

how do metallic properties increase

Back 135

in any group, the metallic properties of the elements increase from the top to the bottom of the group

Front 136

what are some general properties of metals

Back 136

1. solid at room temp except mercury
2. most have densities greater than water, except group 1
3. malleable- can be hammered into shape
4. ductile
5. have luster
6. good conductors of heat and electricity bc of the mobility of their valence electrons
7. have low ionization energy and low electronegavity
8. tend to lose electrons to form positive ions with smaller radii

Front 137

what is group 1 called

Back 137

alkali metals

Front 138

transition elements

Back 138

group 3-group 12
typically hard solids with high melting points
multiple oxidation states
often forms ions that have color

Front 139

properties of nonmetals

Back 139

1. many are gases or solids at room temp
2. not malleable or ductile- are brittle in solid phase
3. no luster- dull surface
4. high ionization energy and high electronegativity
5. poor conductors fo heat and electricity
6. tend to gain electrons to become negative ions with radii larger than their atoms

Front 140

what is a element with more vvalence electrons most likely to do

Back 140

to gain electrons, forming a positive negative ion

Front 141

noble gases

Back 141

the elements in group 18
-are genreally unreactive bc they have completely filled outer energy level, which makes them stable

Front 142

allotropes

Back 142

some nonmetals can consist of two or more forms in the same phase
ex. O2 (oxygen) and O3 (ozone)

Front 143

how are allotropes different

Back 143

different phsical and chemical proeprties

Front 144

where is the highest electronegavity on the table

Back 144

top right

Front 145

ionization eergy

Back 145

the amount of energy needed to remove the most loosely bound electron from a neutral gaseous atom

Front 146

ionization energy and trends in a period

Back 146

values increase across a period from left to right

Front 147

ionization trend in a group

Back 147

decreaes from top to bottom bc the valence electrons are at higher energy levels and are thus farther from the nucleus- it is easier to remove them when they are farther away

Front 148

atomic radius trends in a period

Back 148

from left to right, there is a repeating pattern of decreasing atomic radii (number of protons increase and pulls in electrons, causing decreasing atomic radius)

Front 149

atomic radius and groups

Back 149

atomic radius increases from top to bottom (more inner level electrons shield the valence electrons from the protons in the nucleus)

Front 150

ionic radius

Back 150

distance from hte nucleus to the outer energy level of the ion
-metallic ions are smaller bc it loses electrons when it becomes positive

Front 151

electronegativity trends on the table

Back 151

-highest electronegativity on the top of the group
-increases from left to right on the periods

Front 152

what 3 groups have elements so reactive they cant be found in the free or uncombined state

Back 152

groups 1, 2, and 17

Front 153

propertie of hydrogen

Back 153

-not in a group
-can form ionic compounds and covalent compounds

Front 154

what are elements in group 1 called

Back 154

alkali metals

Front 155

what are the elements of group 2 called

Back 155

alkaline earth metals

Front 156

properties of groups 1 and 2

Back 156

easily lose their electrons
always found in compounds, not alone
-low ionization and electronegativity

Front 157

when is the only time that oxygen has a positive oxidation value

Back 157

when it vonds to the only element more electronegative than itself

Front 158

what is group 17 called

Back 158

halogens

Front 159

halides

Back 159

when atoms of elements in group 17 gain an electron, they get a 1- charge and the salts formed are called halides

Front 160

what is the only group that has 3 states of matter at room temp

Back 160

group 17- halogens

Front 161

what is the rule about electrons and boiling points in nonpolar mmolecules

Back 161

more electrons= higher melting and boiling points
less electrons=lower melting points and boiling points

Front 162

what element comes first when forming a compound

Back 162

the only that loses the electrons comes first

Front 163

what kind of process is the breaking of a chemical bond

Back 163

endothermic- energy is required to break a bond

Front 164

what kinwhat kind of process is the formation of a bond

Back 164

exothermic- breaking a bond releases energy

Front 165

when a chemical bond is formed, does the formed compound have more or less potential energy than the substances from which is was formed

Back 165

less potential energy bc energy is always released when a ond is formed

Front 166

stability vs. energy

Back 166

the greater the energy released during the formation of a bond, the greater its stability

Front 167

kernel

Back 167

the alll of an atoms nonvalence electrons

Front 168

atoms with a double bond

Back 168

oxygen

Front 169

atoms with atriple bond

Back 169

nitrogen

Front 170

boiling and metal points of metals

Back 170

high

Front 171

metallic bonding

Back 171

results from the force of attraction of the mobile valence eletrons for an atom's positively charged kernel

Front 172

what term is used to describe metallic bonding and why

Back 172

"sea of mobile electrons" - freedom of valence electrons

Front 173

where does metal bonding occu

Back 173

between metal atoms that have vacant valence orbitals and low ionization energies

Front 174

crystalline lattice

Back 174

metal

Front 175

octet

Back 175

max number of valence electrons that an atom can have

Front 176

octet rule

Back 176

atoms generally react by gaining, losing, or sharing electrons in order to get 8 valence electrons

Front 177

covalent bond

Back 177

formed when two nuclei share electrons in order to achieve a stable arrangement of electrons
-formed between two nonmetal atoms of the same element

Front 178

non polar covelent ond

Back 178

attraction is equal- between two atoms of the same element - having equal or close electronegativity

Front 179

multiple covalent bond

Back 179

when atoms share more than one pair of electrons (double and triple covalent bonds)

Front 180

polar bond

Back 180

unequal sharing of electrons

Front 181

in a polar bond, which atom pulls harder

Back 181

one with the high electronegativity

Front 182

in a polar bond, which atom has the pos. charge and which has the neg. charge

Back 182

higher electronegativity attracts electrons more strongly, making that negative, and the lower electronegativity positive

Front 183

molecule

Back 183

smallest discrete particle of an element or compound formed by covalently bonded atoms

Front 184

properties of a molecule

Back 184

soft, poor ocnductors of heat and electricity, and low melting and boiling pts
-can be solids, liquids, or gases

Front 185

what happens when metallic atoms react

Back 185

1. lose electrons
2. become pos. charged ions
3. acquire a configuration that has a complete octet of electrons
4. their radii decrease

Front 186

what happens when nonmetallic atoms react

Back 186

1. they gain electrons
2. they become negatively chared ions
3. they acquire a complete octet of electrons
4. their radii increase

Front 187

polarity and electronegativity

Back 187

as the electronegativity difference between two atoms in a bond increases, the bond becomes more polar in nature

Front 188

electronegativity and the type of bond

Back 188

if the difference in electronegativity is -1.7 OR GREATER-, the bond is ionic
if the difference in electronegativity is less than that, it is covalent

Front 189

what do all compouns with polyatomic ions contain

Back 189

both ionic and covalent bonds

Front 190

melting and boiling pts of metallic, covalent, and ionic bonds

Back 190

metallic- high
ionic- high
covalent- low

Front 191

bonds and conductivity

Back 191

metallic- good electrical and thermal conductivity
ionic- bad (unless melted)
covalent- bad

Front 192

hardness of 3 bonds

Back 192

ionic- hard
metallic- hard
covalent- soft

Front 193

dipoles

Back 193

polar molecules (bc they have positive and negative ends)

Front 194

when is the only time ionic molecules have good conductivity

Back 194

in liquid and aqeuous states

Front 195

dipole-dipole forces

Back 195

when the positive area of one dipole molecule is attracted to the negative portion of an adjacent dipole molecule

Front 196

hydrogen bond

Back 196

an intermolecular bond between a hydrogen atom in one molecule and a nitrogen, oxygen, or fluorine atom in another molecule

Front 197

where is hydrogen bonding specifically founbd

Back 197

water

Front 198

why does water have a high boiling pt.

Back 198

hydrogen bonding- stronger than dipole-dipole attraction

Front 199

why does hydrogen only bond with nitrogen, oxygen, and fluorine

Back 199

they are highly electronegative and have small radii

Front 200

solution

Back 200

homogenous mixture of substances in the same physical state- can contain atoms, ions, or molecules of o

Front 201

alloy

Back 201

when metals are mixed to form a solution

Front 202

solute

Back 202

the substance that is being dissolved; present in the smaller amount

Front 203

solvent

Back 203

the substance that dissolves and is the greater amount

Front 204

what is the most common solvent

Back 204

water

Front 205

properties of solutions

Back 205

1. homogenous mixtures
2. clear and do not disperse light
3. have color
4. will not settle on stnading
5.will pass through a filter

Front 206

how does NaCl dissolve in water

Back 206

pos. Na is attracted to the neg. part of the water and the neg. Cl is attracted to the pos. part of hte water

Front 207

like dissolves like

Back 207

yea- but ionic is insoluble in nonpolar solvent and soluble in polar solvent

Front 208

temp and solubility

Back 208

-as temp increases, most solids become more soluble in water
- as temp increases, the solubility of gases decrease

Front 209

pressure and solubility

Back 209

pressure has little or no effect on the solubility of solid or liquid solutes
-incrases the solubility of gases in liquids (ex. soda can is oopened- press decreases and carbon dioxide escapes as bubbles bc it is no longer as soluble at thelowered press)

Front 210

if something is not soluble, what happens when it forms

Back 210

it forms as a precipitate

Front 211

howcan u tell if something is saturated

Back 211

1. if the solution contains some undissolved solute
2. if you add a solute crystal and it dissolves, the orginial solution was unsatured; if it just falls to the bottom, it was saturated; if additinal crystals form, it was supersaturated

Front 212

molarity

Back 212

the number of moles of solute in 1 L of solution

Front 213

percent mass

Back 213

mass of part
----------- x 100
mass of whole

Front 214

percent by volume

Back 214

volume of solute
---------------- x 100
volume of solution

Front 215

what happens when u add salt to water

Back 215

it lowers the freezing point of water

Front 216

one mole of anything will lower the freezing point of water

Back 216

true

Front 217

why do ionic substances lower the freezing of water more than a molecular substance

Back 217

bc when a molecular substance dissolves in water, oone mole of its particules is producted- ionic compounds break into ions so there are more moles

Front 218

one mole of anytihng will raise the boiling pt of water

Back 218

true

Front 219

vapor

Back 219

substance that is normally a solid or a liquid at room temp enters the gas phase

Front 220

vapor pressure

Back 220

as the temp of a liquid increases, the particles have more energy, and more particles escape from the surface- these vapor particles are gaseous particles and exert pressure in the gaseous phase

Front 221

what does it mean if a gas exerts less vapor pressure

Back 221

it has stronger intermolecular foces holding it in the liquid phase

Front 222

when does a gas vaporize

Back 222

when the vapor pressure equals the atmospheric pressrue

Front 223

heatof vaporization

Back 223

the heat required to change 1 mol ofa substance from a liquid at its boiling point to 1 mole of a vapor

Front 224

what happpens to the boiling pt of water if you increase atmosperic pressure

Back 224

the boiling pt increases

Front 225

factors that affect rate of reaction

Back 225

1. nature of the reactants
2. concentration
3. surface area
4. the presence of a catalyst
5. temp.

Front 226

nature of the reactants

Back 226

covalent bonds are slower to react than ionic substance bc of the number of nods that must be broken- needs more energy

Front 227

concentration

Back 227

increase in concentration causes a faster rate bc there are more collisions

Front 228

surface area

Back 228

more surface area=more chances of collision=faster reaction rate

Front 229

catalyst

Back 229

substance that increaes the rate of a reaction by providing a different and easier pathapay for reaction

Front 230

temp

Back 230

increaes temp==faster molecules=more collisions and more energy=faster

Front 231

sum up of factors

Back 231

increasing all of them increaes the rate

Front 232

what must happen in order for a reaction to occur

Back 232

the reactants must have sufficient energy to collide effectively and they must be properly positioned

Front 233

activiated complex

Back 233

temporary, intermediate product thatmay either break apart and reform the reactants or rearrange th atoms and form new products

Front 234

on a potential energy diagram, what is any line that begins at the orgin of the y-axis

Back 234

a measure of PE

Front 235

activation energy

Back 235

the amount of energy needed to form the activated complex from the reatctants

Front 236

heat of reaction (delta H)

Back 236

the difference between the potential energy of the reactants and the potential energy of the products

Front 237

what do catalysts do to teh diagram

Back 237

lower the activiation energy

Front 238

endothermic diagram

Back 238

higher pe at the end

Front 239

exothermic diagram

Back 239

lower pe at the end

Front 240

equilibrium

Back 240

when both forward and reverse reactions occur at the same time- a state of balance between the rates of two opposite processes that are taking place at the same rate

Front 241

common misconceptation about equilibrium

Back 241

the products and reactants dont have to be equal, but the rates of the forward and reverse reactions have to be equal

Front 242

phase equilibrium

Back 242

melting points and freezing points- solid and liquid phases in closed and open containers

Front 243

solution equilibrium

Back 243

dissolving and recristalization are equal- equilibrium exists, solution is saturated

Front 244

le chateliers principle

Back 244

a system at equilibrium responds to relive stress on the system

Front 245

stress

Back 245

any change in temp, concentration, or pressure on an equilibrium system

Front 246

concentration changes

Back 246

if you increase one reactant, the other reactant will decrease and the products will increase- it will shift to the right

-if you decrease one reactant, the other reactant will increase and the products will decrease- shift to the left

Front 247

temp changes

Back 247

if you raise the temp of one reactant, you raise the temp of the other and lower the temps of the two products and produce more heat (favors endothermic reaction)
-if you lower the temp of one reactant, you lower the temp of the other reactant, increae the temp of the products, and decrease the heat released
(favors exothermic reaction)

Front 248

pressure changes

Back 248

(does not affect rate of solids and liquids, but affects rate of gases)
-if pressure is added to the reacants, the system will shift to the right
-if pressure is decreased from hte reacants, the system will shift to the left

Front 249

what if both sides are gaseous

Back 249

an increase in pressure will favor the reaction toward the side with fewer gas molecules
-a decrease in pressure favors the reaction toward the side with the greater number of gas molecules

Front 250

effect of a catalyst oon shifts

Back 250

changes reates equally- doesnt shift

Front 251

enthalpy

Back 251

tendency in nature to change to a state of lower energy

Front 252

entropy

Back 252

tendency in nature to change to a state of greater randomness or disorder- measure of the disorder or randness in a system- greater the disorder, higher the entropy

Front 253

examples of entropy

Back 253

physical changes (phase changes)

Front 254

equilibrium expression

Back 254

1. write a balanced equation for the system
2. place the products as factors in the numberator of the fraction and the reactants as factors in the denominator
3. place a square bracketaround each formula
4. write the coefficient of each substance as the power of its concentration

Front 255

oxidation

Back 255

the loss of electrons by a atom or ion

Front 256

reduction

Back 256

the gain of electrons by an atom or ion

Front 257

redox

Back 257

combined name of oxidation and reduction, bc they cant occur alone

Front 258

LEO says GER

Back 258

loss of electrons- oxidation
gain of electrons- reduction

Front 259

difference between ionic charges and oxidation numbers

Back 259

ion- 2+
oxidation- +2

Front 260

how to recognize a redox reaction

Back 260

1. uncombined element on one side, compound on the other
2. not redox if it is double replacement
3. if oxidation numbers change on hte other side

Front 261

reducing agent

Back 261

gives electrons to reduce something else

Front 262

oxidizing agent

Back 262

accepts electrons from something else

Front 263

oxidized

Back 263

changes from lower oxidation number to a higher one

Front 264

reduction

Back 264

higher oxidation number ot a lower one

Front 265

electrochemical cell

Back 265

involves a chemical reaction and a flow of electrons

Front 266

two types of electrochemical cells

Back 266

1. voltaic cell- spontaenous chemical reaction produces a flow of electrons
2. electrolyic cells- requires an electric current to force a nonspontaneous chemical reaction to occur

Front 267

electrode

Back 267

site at which oxidation or recuation occurs

Front 268

anode

Back 268

where oxidation occurs

Front 269

cathode

Back 269

where reduction occurs

Front 270

RED CAT/ AN OX

Back 270

reducation- cathode
oxidation- anode

Front 271

salt bridge

Back 271

in a voltaic cell, connects the two containers and allows for the flow of ions, which makes a complete circuit and allows the reaction ot procede

Front 272

how do uknow which metal will be oxidized

Back 272

the metal higher on table J will be oxidized

Front 273

differences between voltaic and electrolytic

Back 273

1. voltaic is a battery, electrolytic uses a battery
2. voltaic= reduction is spontaenous, electrolyic is not
3. in voltaic the anode is neg and the cathode is pos
in electrolytic the anode is pos and the cathode is neg.

Front 274

electrolysis

Back 274

when electricity is used to force a chemical reaction to occur

Front 275

characteristics of an acid

Back 275

1. sour taste
2. aqueous solution conducts a current (strong acid=good conductor; weak acid=bad conductor)
3. svifd trsvy eiyh bases to form water and a salt
4. acids react with certain metals to produce hydrogen gas (metals about hydrogen on table j)
5. acids cause acid-base indicators to change color

Front 276

neutralization

Back 276

double replacement reactions
acid+base--> salt + water

Front 277

electrolytes

Back 277

substances that conduct a current

Front 278

solution electric current and ions

Back 278

more ions=better electrical conductivity

Front 279

characteristics of bases

Back 279

1. bitter taste
2. sliperry or soapy feeling
3. conduct electric current (strong base=more ions, more electricity)
4. react with acids to produce water and salt
5. cause acid-baes indicators to change color

Front 280

Arrhenius acid

Back 280

a substance whose water solution contains the hydrogen ion as the only positive ion

Front 281

hydronium ion

Back 281

H3O formed when acids dissolve in water

Front 282

arrhenius base

Back 282

produces hydroxide (OH) ions when dissolved in water

Front 283

distinguishing bases from alcohols

Back 283

alcohols have carbon chains and CH chains

Front 284

naming binary acids

Back 284

hydro- followed by the name of the other element with an -ic ending _ acid

Front 285

ternary acids

Back 285

made of oxygen-containing polyatomic ions
ate->ic
ic->ous

Front 286

naming bases

Back 286

keep the name of the positive ion, and the name of the base ends with hydroxide
ex. Ca (OH)2 is calcium hydroxide

Front 287

naming salts

Back 287

using the name of the positive ion of the base, and the negative ion of the aid

Front 288

what happens when metals reacts with an acid

Back 288

hydrogen gas and a salt are formed

Front 289

forming salts

Back 289

formed by strong acid and strong base= neutral
formed by strong acid and weak base= acidic

Front 290

titration

Back 290

process of adding meaured volumes of an acid or a base of known concentration to an acid or a base of unknown concentration until netralization occurs

Front 291

arrhenius base

Back 291

produces hydroxide (OH) ions when dissolved in water

Front 292

distinguishing bases from alcohols

Back 292

alcohols have carbon chains and CH chains

Front 293

naming binary acids

Back 293

hydro- followed by the name of the other element with an -ic ending _ acid

Front 294

ternary acids

Back 294

made of oxygen-containing polyatomic ions
ate->ic
ic->ous

Front 295

naming bases

Back 295

keep the name of the positive ion, and the name of the base ends with hydroxide
ex. Ca (OH)2 is calcium hydroxide

Front 296

naming salts

Back 296

using the name of the positive ion of the base, and the negative ion of the aid

Front 297

what happens when metals reacts with an acid

Back 297

hydrogen gas and a salt are formed

Front 298

forming salts

Back 298

formed by strong acid and strong base= neutral
formed by strong acid and weak base= acidic

Front 299

titration

Back 299

process of adding meaured volumes of an acid or a base of known concentration to an acid or a base of unknown concentration until netralization occurs

Front 300

how to solve titration

Back 300

Ma x Va= Mv x Vb
(molarity and volume of H+, " " of OH-

Front 301

mono, di, and triprotic acids

Back 301

mono- H+ molarity=molarity of acid solution
di- H+ molarity=double the molarity of the acid solution
tri- triple

Front 302

mono and dihydroxy bases

Back 302

same thing as mono, di, and triprotic acids

Front 303

alkalinity

Back 303

how basic something is

Front 304

pH scale

Back 304

-0-14
7 is neutral, under 7 is acidic, above 7 is basic
-goes by tenfold- pH of 5 is 10 times more acidic than a pH of 6 (10 times more H+ ions)

Front 305

why does phenolphtalein turn pink when a base is adding

Back 305

phen. contains H+ that react with the base, phen. loses its hydrogen atom nad turns pink

Front 306

bronsted-lowry acid

Back 306

any substance that donates a hydrogen (H+) ion
-proton donor

Front 307

bronsted-lowry base

Back 307

any substance that accept a proton (H+)
-proton accetor

Front 308

what makes a conjugate acid-base pair

Back 308

they differ by a hydrogen ion

Front 309

salt

Back 309

ionic substance composed of positively charged metallic or polyatomic ios, and negative ions other than hydroxide ions

Front 310

organic

Back 310

carbon

Front 311

why can carbon form so many compounds

Back 311

it forms chains, rings, and networks of compounds

Front 312

saturated organic compounds

Back 312

containing only single covalent bonds

Front 313

unsaturated organic compounds

Back 313

double or triple covalent bonds

Front 314

buckministerfullerence

Back 314

buckyballl
-single bond to two carbon atoms and double bond to one carbon atom
60 carbon atoms, looks like a soccer ball

Front 315

homologous series

Back 315

a group of related compounds in which each emmeber differs from the one before it by the same additional unit

Front 316

hydrocarbons

Back 316

organic compounds that contain only atoms of hydrogen and carvon

Front 317

3 groups of hydrocarbons

Back 317

alkanes, alkenes, and alkynes

Front 318

alkanes

Back 318

a homologous series of saturated hydrocarbons that release energy when burned
-methane, ehtane, propane, butane

Front 319

formula for an alkane

Back 319

(CnH2n+2)
times two, plus two

Front 320

wht happens to boiling pt as the number of carbons increases in an alkanes series

Back 320

increases

Front 321

alkene series

Back 321

each member contains one double covalent bond between two carbons

Front 322

formula for alkene

Back 322

times two
(CnH2n)

Front 323

alkynes

Back 323

homologous series of unsaturated hydrocarbons that contain one triple bond

Front 324

formula for alkyne

Back 324

CnH2n-2
times two, minus two

Front 325

isomer

Back 325

when a molecular formula canbe represented by more than one structural arrangement
-have the same molecular formula but different chemical and physical properties

Front 326

how to name hydrocarbons that are not straight-chained

Back 326

1. find the longest continuous chain of carbon atoms to name is propane, butane, etc.
2. find if there is a methyl, etc- if necessary, the location is shown with a number (ex 2-methyl)
3. if there are more than one alkyl group attacted, you can use di-, tri-, tetra-
4. if methyls are in different places, use numbers (ex. if there are two methyls o the second carbon and another on the third, it would be 2,2,3-trimethyl butane

Front 327

organic halide

Back 327

halocarbon
when any halogens (F, Cl, Br, or I) replace hydrogen atoms in an alkane

Front 328

how to name an organic halide

Back 328

by citing the location of the halogen attached to the chain
(ex. 2-fluropropane)

Front 329

alcohols

Back 329

organic comoounds in which one or more hydrogen atoms of a hydrocarbon are replaced by an -OH group

Front 330

what gives alcohols their properties

Back 330

hydroxyl group - -OH group- functional group

Front 331

is alcohol an electrolyte

Back 331

no- does not form ions in water

Front 332

primary, secondary, and tertiary alcohols

Back 332

-based on whether the hydroxyl group is attached to a primary, secondary, or tertiary alcohol
(prim- R-OH
sec- R-CH(OH)-R
ter- R1R2R3COH

Front 333

monohydroxy, dihydroxy, trihydroxy alcohols

Back 333

classified by the number of hydroxyl groups that are attached to the carbon chain

Front 334

aldehydge

Back 334

organic compounds in which the carbonyl group (C=O)is found on the end carbon

Front 335

how do u name an aldehydge

Back 335

place an -al instead of the final e of the alkane name

Front 336

ketone

Back 336

forned when the carbonyl group is found on an interior carbon atom that is attached to two other carbon atoms

Front 337

how to name a ketone

Back 337

replace the final -e with -one

Front 338

organic acids

Back 338

functional group is a carboxyl group (-COOH)

Front 339

how to name an organic acid

Back 339

replace -e with -oic

Front 340

amino acid

Back 340

contains -COOH but also an amine group (one of more hydrogen atoms replaced by an alkyl group)

Front 341

combustion

Back 341

burning

Front 342

addition reactions

Back 342

adding one or more atoms at a double or triple bond

Front 343

substitution reaction

Back 343

involves the replacement of one or more of the hydrogen atoms in a saturated hydrocarbon with another atom or group

Front 344

esterification

Back 344

reaction between an organic acid and an alcohol to produce an ester plus water

Front 345

how to name alcohols

Back 345

using the alkyl name of the alcohol plus the acid group with the end -oate

Front 346

saponification

Back 346

when an ester reacts with an inorganic base to produce an alcohol and a soap

Front 347

fermentation

Back 347

chemical process in which yeat cells secret enzume zymase and break the six-carbon chain of sugars into carbon diozide and alcohol

Front 348

polymerization

Back 348

the formation of large polymer molecules

Front 349

addition polymerization

Back 349

the joining of monomers (each individual unit of a polymer) of unsaturated compounds

Front 350

transmutation

Back 350

when the atomic nucelus of one element is changed into the nucelus of a different element

Front 351

radioisotope

Back 351

an isotope that is unstable and thus radioactive

Front 352

alpha particle

Back 352

helium with two protons and two neutrons

Front 353

charge of alpha particle

Back 353

2+

Front 354

charge of positron

Back 354

1+

Front 355

penetrating power of the particles

Back 355

aplha- low
beta and positron- moderate
gamma- high

Front 356

charge of gamma

Back 356

none

Front 357

alpha decay

Back 357

-atomic number decreases by two
-number of protons decreases by two
-number of neutrons decreases by two
-mass number decreases by four

Front 358

beta decay

Back 358

-atomic number increaes by one
-number of protons increases by one
-number of neutrons decreaes by one
-mass number remains the same

Front 359

positron emission

Back 359

-atomic number decreaes by one
-number of protons decreaes byone
-number of neutrons increases by one
-mass number remains the same

Front 360

difference between natural and aritifical transmuation

Back 360

natural- single nucelus undergoing decay
aritiical- two reactants

Front 361

fission

Back 361

splitting of a heavy nucelus to produce lighter nuclei

Front 362

fusion

Back 362

combing of light nuceli to produce a heavier nucelus

Front 363

half life

Back 363

the time it takes for half of the atoms in a given sample of an element to decay

Front 364

c-14

Back 364

known for dating previously living materials

Front 365

U-238

Back 365

radioactive through series until it is Pb-206- used to date rocks, etc

Front 366

1-131, Cobalt 60

Back 366

used for medical conditions