Chem Final

Front 1

"radio isotopes"

Back 1

nuclei that undergo radioactive decay

can produce one or more types of radiation

Front 2

"background radiation"

Back 2

radiation occuring from natural sources

80% of our radioactivity exposure

Front 3

"ionizing radiation"

Back 3

knocks electrons out of atoms / groups of atoms

-produces ions

-these "charged species" cause damage

Front 4

nuclear equations

Back 4

elements can change

total mass must stay same

sum of atomic numbers must stay same

must specify isotope

Front 5

alpha decay

Back 5

nucleus looses alpha particle

--mass decreases by 4
--atomic # decreases by 2

Front 6

beta decay

Back 6

nucleus looses beta- particle

--no change in mass

--atomic number increases

*neutron converted to proton ..... & electron is ejected*

Front 7

positron emission

Back 7

looses a positron

---equal mass but opposite charge of an electron

--decrease in atomic number no change in mass

Front 8

electron capture

Back 8

nucleus absorbs an electron & releases an X ray

--mass # stays same
--atomic # decreases

*opposite of beta decay*

Front 9

gamma radiation

Back 9

release of high energy photon (-y)

normally occurs after another radioactive decay

--no change in mass number --no change in atomic number

*atom becomes less energetic*

Front 10

4 He
2

Back 10

alpha particle

alpha decay

Front 11

0 e
+1

Back 11

positron

positron emission

Front 12

0 y
0

Back 12

gamma ray

high energy photon

Front 13

0 e
-1

Back 13

beta particle / electron

beta decay / electron capture

Front 14

half life

Back 14

time for 1/2 the original elements to undergo radioactive decay

diff for each isotope

fraction remaining:
1 / 2 ^n (n = number of half lives)

Front 15

radioisotopic dating

Back 15

use certain isotopes to est. age

Front 16

238- U

Back 16

half life = 4.5 bill yrs

determines age of rock

238-U decays to 206Pb ... relative amts determine age

Front 17

3H

Back 17

half life = 12.3 yrs

dates aged wines

Front 18

carbon-14 dating

Back 18

98.9% 12C

produce 14C in upper atmosphere

half life = 5730 yrs

~50,000 yr max age for dating

Front 19

use of radioisotopes -- nuclear medicine

Back 19

1- therapeutic
(treat / cure disease w/ radiation)

2- diagnostic
(get info about patient's health)

Front 20

'imaging'

Back 20

PET (postitron emission tomography)

uses isotope that emits a positron

observe amt of radiation released

Front 21

penetrating power of radiation

Back 21

greater mass of particle = less penetrating

faster the particle = more penetrating

Front 22

prevent radiation damage

Back 22

distance from radioactive sources

use sheilding --- need more when more penetrating

Front 23

e = mc^2

Back 23

loose mass = gain energy
(in chem reactions mass changes not measurable)

(nuclear reactions (mass change is measurable))

Front 24

nuclear fission

Back 24

"splitting the atom"

-break large nuclei into smaller nuclei

Front 25

binding energy

Back 25

holds protons and nuetrons together in nucleus

higher binding energy = more stable the element

Front 26

nuclear chain reaction

Back 26

neutrons from one fission event split further atoms

--only happens w certain isotopes

Front 27

radioactive fallout

Back 27

nuclear bomb detonated

radioactive materials rain down miles away - days later

--some may be unreacted U or Pu

--radioactive isotopes produced during explosion

Front 28

nuclear power plants

Back 28

~20% US electricity
--france = > 70%

-slow, controllled release of energy

-need ~3% 235U

-prob with disposal of radioactive waste

Front 29

nuclear fusion

Back 29

reaction takes smaller nuclei and builds larger ones

--also called thermonuclear reactions

--releases tremendous amt of energy

Front 30

ACIDS

Back 30

litmus paper turns red

taste sour

dissolves active metals, producing H2

reacts w/ bases to produce water and salt

Front 31

BASE

Back 31

turns litmus paper blue

tastes bitter

feels slippery

reacts w/ acids to form water and salt

Front 32

ionization

Back 32

when compound breaks apart in aq solution

[[ HCl --> (H+) + (Cl-) ]]

common for both acids and bases

also occurs w some salts

Front 33

ARRHENIUS theory of ACIDS

Back 33

acid = molecular substance that breaks up in aq solution ... into H+ and anions

ex: HNO3 ---> H+ + NO3-

Front 34

H+

Back 34

"hydrogen ions", or "protons"

H+ gives acid its properties

Front 35

ARRHENIUS theory of BASES

Back 35

base: releases OH- ions in aq solution


ex: NaOH ---> Na+ + OH-

Front 36

OH-

Back 36

"hydroxide"

gives bases their properties

Front 37

limitations of ARRHENIUS theory

Back 37

H+ doesn't exist in solution

more likely to find H+ attached to H2O
((H3O+))

NH3 is a base and doesn't contain OH-

Front 38

BROWNSTED-LOWRY acid/base theory

Back 38

acid: proton (H+) donor

-HCl donates a H+ to NH3
(H+ doesn't exist by itself)

*HCl + NH3 --> NH4 + Cl-*


BASES: accept a proton
--NH3 accepts an H+ from HCl


*H2O + NH3 --> NH4 + OH-

Front 39

acidic anhydrides

Back 39

react w water to form acids

normally non-metal oxides

Front 40

basic anhydrides

Back 40

react w water to form bases

metal oxides

Front 41

STRONG acid

Back 41

acid completely reacts w water

--completely ionizes in water

Front 42

WEAK acid

Back 42

acid reacts slightly w water

partially ionizes in water

Front 43

common STRONG acids

Back 43

HCl, HNO3, H2SO4

...most other acids are weak

Front 44

STRONG Base

Back 44

base completely ionizes in water

Front 45

WEAK Base

Back 45

only slightly ionizes in water

Front 46

common strong bASES

Back 46

NaOH, KOH

most group 1a and 2a hydroxides

Front 47

common weak BASE

Back 47

NH3

Front 48

amphiprotic

Back 48

substance that can either donate or accept a proton

most common-- h2o

ex reaction w base:
H2O + NH3 --> NH4+ + OH-

ex reaction w acid:
H2O + HCl ---> Cl- + H3O+

Front 49

neutralization

Back 49

reaction of acid and base

acid + base --> water + salt

Front 50

pH > 7

Back 50

basic

Front 51

pH < 7

Back 51

acidic

Front 52

"pH"

Back 52

represents the concentration of H+ in the solution

Front 53

pH of normal rain

Back 53

5.6 - 6.5

Front 54

pH of acid rain

Back 54

< 5.6

Front 55

acid rain

Back 55

caused by acidic anhydrides released from burning fossil fuels

involves air and water pollution

Front 56

1 mole has how many atoms

(or other formula unit)

Back 56

avogadros number

6.02 x 10^23

Front 57

EM Spectrum

Back 57

gamma - x - UV - visible - IR - micro - Radio

Front 58

how many electrons in
Fe 3+

Back 58

atomic number - 3

26 -3 = 23

Front 59

best to worst conductor of electricity

Back 59

since metals are on the left side the are better

less conductivity as you go right

Front 60

Strontium
(Sr)
is dangerous to humans bc

Back 60

chemically similar to Ca

Front 61

ammonium nitrate

formula

Back 61

NH4NO3

Front 62

magnesium phosphide

Back 62

Mg3P2

Front 63

name for Fe2O3

Back 63

iron (III) oxide

Front 64

solubility in water

Cl2, ClO, NaCl

lowest to highest?

Back 64

Cl2 < ClO < NaCl

Front 65

HL of carbon-14

Back 65

5730

Front 66

manhattan project

Back 66

scientists obtained fissionable plutonium -239
by BOMBARDING U-238 w NEUTRONS

Front 67

sun heats earth by

Back 67

FUSION

Front 68

breeder reactors in europe based on

Back 68

FISSION

Front 69

H-bomb involves

Back 69

FISSION AND FUSION

Front 70

energy converted to mass in which f?

Back 70

FISSION AND FUSION

Front 71

combustion -- O2 +.... yields

Back 71

CO2 + H2O

Front 72

P V T relationship

Back 72

PV / T = PV / T

Front 73

ozone hole discovered in what month

Back 73

october

Front 74

water breaking down into H and O gas is what change?

Back 74

chemical

Front 75

change in state of matter

Back 75

physical change

Front 76

elements occuring naturally as a molecule

Back 76

N2, O2, H2, Cl2

Front 77

freq wavelength equation

Back 77

c = (freq)(WL)

Front 78

c =

Back 78

c = 3 x 10^8 m/s

Front 79

electron configuration

Back 79

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

Front 80

greater amplitude =

Back 80

brighter

(intensity greater)

Front 81

orbital made up of

Back 81

3 quantum numbers

n,
l
m

Front 82

n

q #

Back 82

principle quantum number

energy level of shell

(+ integer)

Front 83

l

q #

Back 83

angular momentum

determines shape of orbital

(0 to n-1)

Front 84

m

q #

Back 84

magnetic moment

determines orientation of orbital

(-l to +l)

Front 85

l = 0

Back 85

s sublevel

Front 86

l = 1

Back 86

p sublevel

Front 87

l = 2

Back 87

d sublevel

Front 88

l = 3

Back 88

f sublevel

Front 89

Energy =

Back 89

E = (h)(freq)

E = hv

when n constant

when not
E = (change in n)(h)(v)

h = plancks constant
6.626 x 10^-34 Js

Front 90

h

Back 90

6.626 x 10^-34 Js

Front 91

Avogadros #

Back 91

6.02 x 10^23 formula units

(per mole)

Front 92

law of conservation of mass

Back 92

matter not created / destroyed during chem reaction

Front 93

law of definite proportions

Back 93

specific compounds always contain same elements in definite proportions

Front 94

law of multiple proportions

Back 94

element can combine in diff proportions to form new compounds

Front 95

alpha
beta
gamma

Back 95

alpha: mass = 4
charge = 2+

beta: mass 0
charge: -1

gamma: mass 0
charge: 0

Front 96

p
n
e
mass

Back 96

p : 1
n : 1
e : 0

Front 97

binary compounds

Back 97

2-element compounds

Front 98

naming ionic

Back 98

+ ion first, - ion second -ide

Front 99

prefixes for covalent

Back 99

mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca

Front 100

EN

Back 100

measure of attraction of an atom in a molecule
the more EN, the more likely to pull e's in bond toward its end

table:
right more EN than left

Front 101

HONC rules

Back 101

H forms 1 bond
O: 2
N: 3
C: 4

Front 102

"polyatomic ions"

Back 102

charged particles containing 2+ covalently bonded atoms

ex: OH- ... o atom covalently bonded to H atom plus has an extra electron

Front 103

1+

polyatomic ions

Back 103

ammonium ion (NH4)+

hydronium ion (H3O)+

Front 104

1-

polyatomic ions

Back 104

acetate ion (C2H3O2)-
nitrite ion (NO2)-
nitrate ion (NO3)-
cyanide ion (CN)-
hydroxide ion (OH)-
permanganate ion (MnO4)-

Front 105

2-

polyatomic ions

Back 105

carbonate ion (CO3)2-
sulfate ion (SO4)2-
chromate ion (CrO4)2-
di chromate ion (Cr2O7)2-

Front 106

3-

polyatomic ions

Back 106

phosphate ion (PO4)3-

Front 107

ammonium ion

Back 107

(NH4)+

Front 108

hydronium ion

Back 108

(H30)+

Front 109

acetate ion

Back 109

(C2H3O2)-

Front 110

nitrite ion

Back 110

(NO2)-

Front 111

nitrate ion

Back 111

(NO3)-

Front 112

Cyanide ion

Back 112

(CN)-

Front 113

Hydroxide ion

Back 113

(OH)-

Front 114

permanganate ion

Back 114

(MnO4)-

Front 115

carbonate ion

Back 115

(CO3)2-

Front 116

sulfate ion

Back 116

(SO4)2-

Front 117

chromate ion

Back 117

(CrO4)2-

Front 118

di chromate ion

Back 118

(Cr2O7)2-

Front 119

phosphate ion

Back 119

(PO4)3-

Front 120

total e's of polyatomic ions

Back 120

add the charge # to electrons

Front 121

free radical

Back 121

atom / molecule with unpaired electron

((atoms with an ODD # of electrons))

Front 122

an odd # of electrons means

Back 122

its a free radical

Front 123

electron repulsion thoery

Back 123

e's arrange themselves to minimize repulsion

Front 124

non polar geometric arrangement

Back 124

linear

triangular

tetrahedral

Front 125

polar geometric arrangements

Back 125

bent

pyramidal

Front 126

"dipole"

Back 126

molecule with + and - end

Front 127

physical state of something depends on

Back 127

strength of intermolecular forces holding the molecules together

(relative to thermal energy (temp) -- acts to seperate them)

Front 128

"boiling pt"

Back 128

when liquid becomes gas

Front 129

"freezing pt"

Back 129

when liquid becomes solid

Front 130

"melting pt"

Back 130

when solid becomes a liquid

Front 131

condensation

Back 131

vapor -> liquid

Front 132

sublimation

Back 132

solid -> gas

Front 133

q of energy needed to change state depends on

Back 133

strength of bonds

ionic - strongest

Front 134

to form H bond

Back 134

must have F O or N

(the high polarity attracts H)

Front 135

H2o has high melting pt bc

Back 135

bc ability to form H bonds

Front 136

"dispersion forces"

Back 136

electrons move about the atom
when the weak side of an atom is alligned with the strong side of another atom they have a momentary, weak attractive force

Front 137

solutions form most easily when

Back 137

solute and solvent have bonds of similar strengths

(ie non-polar in non-polar)

Front 138

law of combining volumes

Back 138

at a constant T and P
the volume of reactants and products are small whole # ratios

(ie ... the mole # in front of a reactant etc..)

Front 139

equal volumes of gasses at constant T and P

Back 139

have same number of molecules

(avogrado)

Front 140

at constant T and P

if volume 1 = volume 2

Back 140

then both have same # of molecules


ie
the ratio of V1 mass / V2 mass
is the same ratio as
mass molecules 1 / mass molecules 2

Front 141

"mole"

Back 141

amt of substance that has same number of formula units as the the # of atoms in
12 g of C-12

(12 g of C-12 contains:
6.02 x 10^23 atoms)

-- so the amt of a substance that contains 6.02 x 10^23 formula units

Front 142

1 mole NaCl contains

Back 142

6.02 x 10^23 NaCl formula units

ie
6.02 x 10^23 Na+ ions
& 6.02 x 10^23 Cl - ions

Front 143

avogadro's # of molecules / atoms @ given T and P

Back 143

occupies same volume

Front 144

standard T and P

Back 144

standard P = 1atm

standard T = 0 *C
(273K)

Front 145

stochiometry

Back 145

ratio of moles reactants and moles products

ie
1 mole X reacts w 1 mole Y

Front 146

kinetic molecular theory

Back 146

molecules gas in constant random straight line motions

when collide energy is conserved tho taken from one to another

TEMP = measure of avg kinetic energy of gas molecules

Front 147

ideal gas law

Back 147

PV = nRT

R = 0.0821

Front 148

Molarity

Back 148

M = moles solute / L solution

Front 149

percent by vovlume

Back 149

volume solute / volume solution

Front 150

percent by mass

Back 150

mass of solute / mass of SOLUTION

Front 151

substancce

Back 151

element or compound in which COMPOSITION DOESN"T VARY

h2o, Au

Front 152

Mixture

Back 152

TWO + SUBSTANCES

--composition varies

1-homogenous (solution)
(comp varies, and compounds dont bond -- ie salt doesn't bond w water)

2-heterogenous mixture
appearance not the same
sand water

Front 153

atom < element
Molecule < compound

molecule = group of atoms bonded together

Back 153

mmm

Front 154

Si Units

Back 154

length: m
time: s
temp: K
amount: mole

Front 155

He has how many e

Back 155

TWO

Front 156

AMU =

Back 156

mass number

Front 157

BaO transfer of e

Back 157

Ba transferrs to O

B2+ and O2-!!!!

Front 158

nitride ion

Back 158

(N)3-

nitriDe

Front 159

molecular compounds

Back 159

CO, H2, N2

Front 160

when doing sum of coefficients

Back 160

remember to count the 1's

Front 161

mmHg

Back 161

same as torr

760 / atm

Front 162

strong acids:

Back 162

hydrochloric acid (HCl)

nitric acid (HNO3)

sulfuric acid (H2SO4)

hydrobromic acid (Hbr)

hydroiodic acid (HI)

perchloric acid (HClO4)

Front 163

hydrochloric acid

Back 163

HCl

Front 164

Nitric acid

Back 164

HNO3

Front 165

sulfuric acid

Back 165

H2SO4

Front 166

hydrobromic acid

Back 166

HBr

Front 167

hydroiodic acid

Back 167

HI

Front 168

perchloric acid

Back 168

HClO4

Front 169

strong bases

Back 169

sodium hydroxide (NaOH)

Potassium hydroxide (KOH)

lithium hydroxide (LiOH)

calcium hydroxide (Ca(OH)2)

magnesium hydroxide (Mg(OH)2)

ammonia (NH3)

Front 170

common base w no OH

Back 170

ammonia

NH3

Front 171

penetrating power

Back 171

alpha - low
beta - medium
gamma - high

Front 172

treatment of thyroid gland

Back 172

iodine - 131

Front 173

diagnostic purposes

Back 173

technetium-99

bc doesn't produce alpha / beta particles
and has short HL

Front 174

PET scans

Back 174

detect gamma rays

Front 175

brownsted lowry acid
brownsted lowry base

Back 175

acid - must have H+ to donate

base - must have lone pair of e to accept proton

Front 176

alkalosis

Back 176

blood = too alkaline

Front 177

leading chemical product in US

Back 177

H2SO4