London N616 Chem 8/24 (Exam 1) Fall 2011

Front 1

Name 2 characteristics of an inorganic compound & give example

Back 1

Lack carbon
simpler compounds
eg H20

Front 2

Law of conservation of mass

Back 2

mass that enters into a chem rx remains unchanged.
mass is neither created nor destroyed

Front 3

Law of constant composition

Back 3

elements that compose a compound are present in fixed and precise proportion by mass;
--maintains identity eg H20 always H20
--If cpd were composed of atoms w/mass & atoms of another kind having a different mass, then the measured mass ratio of elements must be the mass ratio of constitutent atoms

Front 4

Law of multiple proportions

Back 4

since atoms combine as whole #, compounds form whole #

Front 5

What is the Atomic Theory

Back 5

-elements consist of atoms
-all atoms of element identical & have same mass
-compounds consist of atoms of different elements together
-compounds have constant composition
-chem rx involve rearrangement of combination of atoms

Front 6

What is the smallest indivisible particle of an element

Back 6

Atom

Front 7

What is the periodic table

Back 7

tabular representation of all elements arranged according to ATOMIC NUMBER (the # protons in nucleus) & CHEMICAL PROPERTIES

Front 8

What is the atomic number

Back 8

the number of PROTONS in nucleus

Front 9

What is the octet rule

Back 9

Strong desire for 8 electrons in outer most shell (valence shell)
--represents most stable situation

Front 10

What is number of electrons needed to satisfy octet rule

Back 10

8

Front 11

what is the mass of an atom

Back 11

the sum of Protons & Neutrons

Front 12

the sum of the protons & neutrons give you what number

Back 12

Mass of an atom

Front 13

For a given element, the number of protons (atomic #) is fixed, but the number of ____________ can vary in different ________________

Back 13

neutrons; isotopes

Front 14

Isotopes are represented by ___________numbers

Back 14

superscript before the element

Front 15

Atomic weights are ____________ of the different isotopes, weighted in according to their abundance

Back 15

averages

Front 16

chemical properties are governed by the arrangements of __________around the nucleus of an atom

Back 16

Electrons

Front 17

the number of _____________are the same as the number of protons (atomic #)

Back 17

Electrons

Front 18

what are electrons arranged in? and within these _____

Back 18

shells; orbitals

Front 19

The chemical properties of an element are r/t the # & characteristics of ___________ in the outermost (most energic) orbitals called _______________

Back 19

Electrons;

Valence electrons

Front 20

In periodic table, Columns (groups/family) are those elements with similar #/characteristics of _________________in the outer orbitals, & therefore share similar ________________properties

Back 20

Electrons;

Chemical

Front 21

the outermost shell is called the ____________________; the electrons found in this are called the ___________electrons

Back 21

valence shell;

valence electrons

Front 22

For example, Group 1, 2, 8 elements have ___, ____, ____ electrons in their valence shell, respectively

Back 22

Group 1 = 1 valence electron

Group 2= 2 valence electrons

Group 3= 3 valence electrons

Front 23

Any orbital takes ______ electrons maximum

Back 23

2

Front 24

What gases are inert (don't react), don't like to play with others, & are happy just being themselves? and why?

Back 24

Noble gases (group 8)

b/c 8 electrons in valence shell means they fulfill octet rule

Front 25

These help define the shape of the electron cloud

Back 25

orbitals

Front 26

s orbitals are _________shape; p orbitals are _________shape

Back 26

s orbitals= spherical

p orbitals = teardrop

Front 27

If the atomic number is 18, what is the element, the element symbol, & what is the electron configuration (use orbitals), is it stable and why?

Back 27

Argon, Ar

Electrons = 18 (electrons = protons (or the atomic #) in a neutral element), therefore

1s2, 2s2, 2p6, 3s2, 3p6

Yes it is stable b/c it has 8 electrons in the valence shell satisfying the octet rule

Front 28

If the atomic number is 11, what is the electron configuration?

Back 28

1s2, 2s2, 2p6, 3s1

Front 29

an ______________ is the 3D space where an electron is found 90% of the time

Back 29

orbital

Front 30

Each electron shell consists of a specific number of _______________

Back 30

orbitals

Front 31

each orbital holds up to ________electrons

Back 31

2

Front 32

atomic size is determined by how much space ___________take up

Back 32

electrons

Front 33

This is the energy required to REMOVE the outermost electron from an atom

Back 33

ionization energy

Front 34

The ability of an atom to ATTRACT electrons is this

Back 34

electronegitivity

(Meagan's great example--you are dressed to the nines in a bar and are attracting many other hotties)

Front 35

Electronegativity (attract) goes _________ (up or down?) from left to right across periodic table

Back 35

electronegativity INCREASES left to right

Front 36

Electronegativity (attract) goes __________(up/down?) as you move down columns

Back 36

electronegativity DECreases as you move down the columns b/c outer electrons further away from nucleus atom more willing to let go b/c can't hold on very well

Front 37

covalent bonding results from ______________ one or more electron pairs between atoms

Back 37

sharing

Front 38

Ionic bonding results from ____________ attractions among _____; which are formed by the transfer of one or more ___________from one atom to another

Back 38

electrostatic atraction among ions

electrons

Front 39

H20 is an example of this type of bond

Back 39

covalent b/c share electrons

Front 40

this consists of 2 or more atoms held together by covalent bonds

Back 40

molecule

Front 41

the sharing of one pair of valence electrons is known as a ______bond

Back 41

single bond ------

Front 42

A double bond is the sharing of _________pairs of valence electrons

Back 42

two pairs

Front 43

a triple bond is the sharing of _____________pairs of valence electrons

Back 43

3 pairs

Front 44

Is CH4 (methane) an organic or inorganic compound and why

Back 44

CH4 (methane) is an organic compound because it has carbon

Front 45

what's the difference between Lewis and line-bond structures used to represent electron sharing in covalent bonds?

Back 45

Lewis uses dots ..

line-bond structure uses lines
H-N-H

Front 46

The more electronegative an atom, the __________it pulls shared electrons to itself

Back 46

stronger

Front 47

this attraction quality increases from left to right across the periodic table

Back 47

Electronegativity

Front 48

in a NONpolar covalent bond, the atoms have _____________electronegativities because they __________the electron equally

Back 48

similar;

share

Front 49

in a POLAR covalent bond, the atoms have ______________electronegativity & share the electrons ____________

Back 49

differing;

unequally

Front 50

electron transfer between 2 atoms creates ________

Back 50

ions

Front 51

Ions are atoms with more or fewer _____________than usual

Back 51

electrons

Front 52

Ions are considered (charged or noncharged) atoms

Back 52

ions are charged atoms

Front 53

A negatively charged ion is known as this

Back 53

Anion

Front 54

A cation is a ____________charged ion

Back 54

positively charged

Front 55

an ionic bond is an attraction between _________ & _____________

Back 55

anions and cations

Front 56

ionic compounds are often called ___________, which may form crystals

Back 56

salts

Front 57

in an aqueous solution, each ion is surrounded by ___________molecules

Back 57

water

Front 58

Negatively charged polyatomic ions have more ______________in their covalent bonds than they do protons in all their collective nuclei

Back 58

electrons

Front 59

positively charged polyatomic ions have (more/fewer) electrons in their covalent bonds than protons in all their collective nuclei

Back 59

Fewer electrons

Front 60

polyatomic ions associate w/ions of opposite charge to produce electrical __________in the compound

Back 60

electrical neutrality

Front 61

what am I (anion or cation) & what is my name

CO3 2-

Back 61

anion

carbonate= CO3 2-

Front 62

anion/cation?

name

HCO3 -

Back 62

anion

bicarbonate= HCO3 -

Front 63

anion/cation & name

CN -

Back 63

anion

cyanide = CN -

Front 64

nitrate anion

Back 64

nitrate = NO3 -

Front 65

nitrite/ ion type

Back 65

nitrite = NO2 -

anion

Front 66

anion/name

MnO4 -

Back 66

permanganate= MnO4 -

Front 67

name that anion

O2 2-

Back 67

peroxide = O2 2-

Front 68

P2 O7 4-

Back 68

pyrophasphate= P2 O7 4-

anion

Front 69

PO4 3-

Back 69

Phosphate = PO4 3-

anion

Front 70

Is phosphite PO3 3- a cation or anion

Back 70

anion

Front 71

name this polyatomic ion & charge

CH3CO 2-

Back 71

acetate=CH3CO 2-
anion

Front 72

OH-

Back 72

hydroxide = OH-

anion

Front 73

formate

Back 73

formate HCO 2-

anion

Front 74

(CO2)2 2-

Back 74

oxalate = (CO2)2 2-

Front 75

sulfate

Back 75

sulfate= SO4 2-

anion

Front 76

Sulfite

Back 76

sulfite = SO3 2-

anion

Front 77

Ammonium

Back 77

ammonium NH4+

cation

Front 78

Hydronium

Back 78

hydronium= H3O+

cation

Front 79

Pyridinium

Back 79

pyridinium= C5H5NH +

cation

Front 80

this is very important to its function in the living cell

Back 80

precise shape of a molecule

Front 81

The precise shape of a molecule, which is important to its function, is determined by the positions of its atoms' __________orbital

Back 81

Valence

Front 82

In a covalent bond, the ___ and _____ orbitals may ________creating specific molecular shapes

Back 82

s & p orbitals may hybridize

Front 83

hybridization is a process in which atomic ___________ mix to form new identical orbitals

Back 83

Orbitals

Front 84

what is a chemical bond

Back 84

a chemical bond is a force which holds a group of atoms (at least two) together so as to form an electrically neutral aggregate

Front 85

what is the reason for the formation of chemical bonds?

Back 85

the most stable elements are noble gases. Their stability is based on fact their outer (valence) shells are filled. All other elements have unfilled outer valence shells are therefore are unstable. They can achieve stability by filling valence shells thru chem rx & chem bond formation. Therefore, the principal driving force for formation of chemical bonds is that most elements are inherently unstable

Front 86

This determines how biological molecules recognize & respond to one another with specificity

Back 86

Molecular shape

Front 87

A statement of the ratios of elements that make up a compound

Back 87

formula

Front 88

formula weight is the sum of the ________ weights of the constituent atoms of the formula

Back 88

atomic weight

Front 89

what is the formula mass for methane, CH4

Back 89

CH4

C=12
H=1

(1 x 12) + (4 x1) = 16

Front 90

How do you determine the formula weight

Back 90

1) identify elements/atoms present
2) look for atomic mass
3) add

Front 91

What is the formula mass for CO2

Back 91

Carbon dioxide (CO2)

C=12
O=16

(1x12) + (2 x 16) = 44

Front 92

what is the formula mass for NH3 (name the compound)

Back 92

NH3 = ammonia

N=14
H=1

(1 x 14) + (3 x 1) = 17

Front 93

what is the formula mass for Iron (III) nitrate, Fe(NO3)3

Back 93

Fe= 56

N= 14

O= 16

(1 x 56) + 3[(1x14) + (3 x 16)] =242

Front 94

If we have the same number of moles of two ions or molecules, we will have the same number of each entity, this is the reasoning behind this concept

Back 94

the MOLE

Front 95

one mole = 6.022 x 10 23

this number is called_________

Back 95

Avagadro's number

Front 96

what is Avagadro's number

Back 96

6.022 x 10 23

Front 97

what is Molar mass

Back 97

Molar mass is the mass in grams numerically equal to the atomic weight of the element in grams

Front 98

H has an atomic weight of 1.00794 g therefore
1.00794 g of H atoms = _________atoms

Back 98

6.022 x 10 23 atoms

Front 99

If we want to know how many ions or molecules of reactants are present in a given volume of solution the concept of this was developed to do that

Back 99

molaRity

Front 100

1 molar (M) soluntion is the concentration of 1 mole of a compound in a 1 _____ of solution

Back 100

liter

Front 101

MolaRity

Back 101

moles of solute/liter of solution

Front 102

unit of molaRity ____ symbol of molaRity_____

Back 102

molar, M

a 2.0 M solution is a 2.0 molar solution & its molarity is 2.0 mol/L

Front 103

how would you prepare a 0.5 M aqueous solution of NH4Cl?

Back 103

1. Identify formula weight (mass) for each element in compound
eg: N=14.02
H = 1.01
Cl = 35.45

2. Add the formula weight of these constitutents

eg:
(1 x 14.02) + (1 x 4.04) + (1 x 35.45) = 53.51


therefore, 1 mol NH4Cl = 53.51 g)

3. set up calculation

Molarity = moles of solute/Liter of solution

gx (1 mol/53.51 g NH4Cl) = 0.5 mol

do algebra to figure it out

gx = 26.75

therefore, you need 26.75 g of NH4Cl to prepare a 0.5 M aqueous solution

(shaum p. 111 prob 6.9).

Front 104

0.1 M solution can also be called ____

Back 104

100 mM

Front 105

we can make a 0.1 M solution by dissolving _______of formula weight in 1 L of solution

Back 105

1/10 or 0.1

Front 106

aqueous solutions are solutions in which the solvent is

Back 106

water

Front 107

are water molecules polar or nonpolar?

Back 107

water molecules are polar

Front 108

these substances are easily soluble in water & are said to be

Back 108

hydrophilic

Front 109

if you are a water hater/scared of water, or poorly soluble in water you are said to be

Back 109

hydrophobic

Front 110

usually hydrophilic/soluble solutions have _______________or __________molecules

Back 110

charged or polar

Front 111

Hydrophobic/insoluble substances are

Back 111

not charged; they are nonpolar

Front 112

If you raise the temperature of water, solids are (more/less) soluble

Back 112

more soluble

Front 113

Liquids that dissolve in water are said to be

Back 113

miscible

Front 114

If your beverage of choice is vodka on the rocks & you notice they mix together when the ice cubes melt, this is an example of a __________liquid

Back 114

miscible

Front 115

liquids that do NOT dissolve in water are said to be

Back 115

IMMiscible

Front 116

you notice the oil separates from the water based salad dressing, this is an example of a liquid that is

Back 116

immiscible

Front 117

gases that dissolve in water do so in part because they exert _________ on the surface of water

Back 117

pressure

Front 118

gases dissolve in water according to their ______________-in the atmosphere above/in contact with water

Back 118

partial pressure

Front 119

name a gas that is very soluble in water

Back 119

CO2

Front 120

name a gas that is not so soluble in water

Back 120

O2

Front 121

This is the property that enables substances to become evenly distributed in a solution

Back 121

diffusion

Front 122

all molecules, ions & atoms posses this energy

Back 122

thermal

Front 123

atoms/molecules/ions in a solid are held in place by ________forces & just vibrate b/c of their thermal energy

Back 123

strong attractive

Front 124

atoms/molecules/ions in liquid/gas/solution are free to move in a straight line until they ________with something

Back 124

collide

Front 125

substances always diffuse _______their concentration gradient

Back 125

down

Front 126

substances diffuse down their concentration gradient from ____concentrated areas to ______concentrated areas until all areas have equal concentration

Back 126

more to less

Front 127

osmosis is diffusion that occurs across a ____________membrane

Back 127

semipermeable

Front 128

a _______________membrane will let some components of solution cross, but will exclude others

Back 128

semipermeable

Front 129

most membranes are freely permeable to _______________

Back 129

water

Front 130

biological membranes are made of ___________so most ions & polar molecules can not cross

Back 130

lipids

Front 131

If there are concentration differences across membranes, ___________must cross the membrane to equalize them

Back 131

water

Front 132

the propensity of water to cross a semipermeable membrane to equalize solute concentrations on either side is called

Back 132

osmotic pressure

Front 133

If there are more solutes in beaker A than beaker B making beaker A more concentrated, water will start going into beaker ____ to equalize solute concentrations

Back 133

A

water will cross from dilute conc into more concentrated area to even concentration out

Front 134

Two containers of equal volume separated by semipermeable membrane which only allows water to cross. Solution A has 3 molecules (wt 66,000), & solution B has 15 molecules (wt 180). Into which container will water flow, if any

Back 134

Water will move from A to B to equalize WATER concentrations on either side of membrane, regardless of identify of solute

Front 135

exothermic is energy _____

Back 135

supplying

Front 136

When the energy product is < reactions, the change of H is negative & _______

Back 136

exothermic

Front 137

A + B are reactants

C is the product

when the energy of A +B >C, the chemical reaction is said to be

Back 137

exothermic

Front 138

an endothermic reaction is energy____

Back 138

requiring

Front 139

In the chemical reaction

A + B------> C
where A+ B energy < C at the end & change in H is positive, this is considered a_________-reaction

Back 139

endothermic

Front 140

A+ B < C

positive change in H

C is bigger b/c it required energy to make happen so this is a ___________reaction

Back 140

endothermic

Front 141

A + B > C

negative change in H

C lost energy b/c it is supplying so this is an example of an _____reaction

Back 141

exothermic

Front 142

energy requiring reactions or ______________reactions usually proceed first & then are coupled with an exothermic

Back 142

endothermic (take within)

Front 143

reaction rates depend mostly on _______ & _________

Back 143

concentrations of reactants & temperature

Front 144

these 2 things speed up reactions

Back 144

increasing concentration of reactants & increasing the temperature

Front 145

If you increase the concentration of the reactants & the temperature you do this to the reaction

Back 145

speed it up

Front 146

these speed up reactions by lowering the activation energy

Back 146

catalysts

Front 147

catalysts speed up reactions by _________the activation energy

Back 147

lowering

Front 148

catalysts __________entropy

Back 148

reduce

Front 149

this is a measure of randomness that contributes to activation energy

Back 149

entropy

Front 150

catalysts are usually protein molecules called

Back 150

enzymes

Front 151

the enzyme reduces activation energy by reducing the ____________, or the measure of randomness that contributes to activation energy

Back 151

entropy

Front 152

the enzyme may also _________the energy of ATP hydrolysis to the endothermic reaction (

Back 152

supply

Front 153

endothermic

think 'energy within' the energy product is greater than the energy in the _________

Back 153

reactants

A + B < C

endothermic rx take in energy so have + change in H & the products are greater than the reactants

Front 154

reversible chemical reactions are denoted by

Back 154

-----> and <--------
or <----->

arrows that go back & forth or double arrow

Front 155

will the reaction go completely forward or backward?

Back 155

NO

Front 156

reversible rx have an __________between the forward reaction & backward reaction

Back 156

equilibrium

Front 157

in a molar concentration, the concentrations are raised to the power of the ___________in the balanced equation_

Back 157

coefficient

eg
N2 + O2 <---> 2 NO

K= [NO]2 / [N2][O2]

Front 158

Principle of Le Chatelier

Back 158

-any change in status quo prompts opposing reaction
-when concentration of reactant(s) is increased, the reaction is pushed to the Right;
-when the concentration of the product(s) is increased, the reaction is pushed to the Left

Front 159

Any change in the status quo prompts an opposing reaction in the responding system is the definition of this principle

Back 159

Principle of Le Chatelier

Front 160

when the concentration of one of the reactants is increased, the reaction is pushed toward the __________; this is part of the ___________

Back 160

Right; Principle of Le Chatelier

Front 161

when the concentration of one of the products is increased, the reaction is pushed to the

Back 161

left

Front 162

the French are very hospitable people, so if you have people over to your house, they will invite you back, this is an example of what principle

Back 162

Principle of Le Chatelier

Front 163

the Principle of Le Chatelier concerns the restoration of chemical reaction__________

Back 163

equalibrium

Front 164

some isotopes of elements w/ atomic # < _______ & all isotopes of elements w/atomic # > ______________are radioactive

Back 164

83

Front 165

radioactive isotopes have nuclei that are ___________ & emit energy in the form of ____________ or __________

Back 165

radioactive isotopes have nuclei that are UNSTABLE & emit energy in the form of PARTICLES or POSITRONS (alpha or beta) or ELECTROMAGNETIC WAVES (gamma rays)

Front 166

an alpa particle has ____ protons & _____ neutrons (a helium nucleus)

Back 166

2 protons & 2 neutrons

Front 167

a beta particle has an electron that comes from the

Back 167

nucleus

Front 168

Are gamma rays higher energy than xrays?

Back 168

Yes

Front 169

when alpha or beta particles/positrons are emitted, the nucleus changes its atomic number (number of protons) & therefore becomes another________-

Back 169

element

Front 170

radioactive elements decay according to this

Back 170

half-life

Front 171

isotopes in nuclear medicine have extremely ______half lives

Back 171

short

Front 172

Technetium -99 is an example of a radioactive isotope with a _____ half live

Back 172

short

Front 173

if you have a shorter half life, what is the benefit

Back 173

get rid of it quicker

Front 174

isotopes used in radiation medicine have ____ half lives

Back 174

longer

Front 175

if a pt gets IV radioactive isotope, their excreta will be _______

Back 175

radioactive

Front 176

if a pt has a radioactive implant, their excreta (will/will not) be radioactive

Back 176

will NOT (it is contained)

Front 177

radioactivity produces

Back 177

ionization

Front 178

the most damaging ionization in humans affects the person's

Back 178

DNA

Front 179

this is the purpose of the ionizing radiation directed at tumors

Back 179

cell death

Front 180

increased incidence of second malignancy occurs when

Back 180

pt who receive radiation to treat one cancer have increased incidence of a second malignancy