Organic and Nuclear Chemistry

U12L1: Intro to Organic Chemistry

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Organic chemistry - the study of compounds that contain carbon (O R G A N I C C O M P O U N D S M U S T H A V E C A R B O N )

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Properties of Organic Compounds

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Bonding: Covalent = nonmetal + nonmetal

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Solubility: most are insoluble in water (generally

nonpolar) *like dissolves like

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Conductivity: mostly nonconductors (s), (l), & (aq)

states

*Only organic acids ionize in solution = poor

conductors

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Melting/boiling points: weak IMF = low MP’s and BP’s

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Reactivity Rate: react slowly; more bonds to break

Hydrocarbons - organic molecules that contain ONLY carbons

and hydrogens

Saturated hydrocarbons - contains only single bonds

Unsaturated hydrocarbons - contains at least one double or

triple bonds

Alkanes - hydrocarbons with single bonds

Alkenes - hydrocarbons with at least 1 double bond

Alkynes - hydrocarbons with at least 1 triple bond

Table Q can be used to determine what kind of hydrocarbon

you have by comparing the number of C’s and H’s in a

formula

U12L2: Naming and Drawing Hydrocarbons

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Single Chain ALKANES

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Use Table P to determine the number of carbons that are chained together and

proper prefix

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Table Q can assist with the formula and suffix -

“

-ane”

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Carbon should always have 4 bonds/lines coming off of it - fill in empty bonds

with H’s

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Single Chain ALKENES/ALKYNES

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Use Table P to determine the number of carbons that are chained together and proper prefix

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Table Q can assist with the formula and suffix -

“

-ene” if

there is a double bond, and “

-yne” if there is a triple

bond.

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State the location of the START of the double/triple

bond of the lowest # carbon

Branched ALKANES

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Locate the longest continuous carbon chain (parent

chain) in a molecule.

Number the carbons in the parent chain so that the branch(es) fall at the lowest possible number/sum

Name the branches first (separately, in alphabetical order) along with location

■ Prefix based on the # C’s (table P) + suffix –yl

■ Branches are named separately unless there are two of the same - then lump them into the

same branch name (w/ number locations) & add appropriate prefix (di, tri, tetra, etc.

The parent chain is stated last in the name (the # carbons in the parent chain should agree with the

prefix in the last word of the chemical name).

U12L3: Functional Groups

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Table R has all the functional groups you need to know. Table R provides the functional group name, the

structural formula of the functional group, how it would appear in a compound along with an example of the

name of the compound.

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Functional groups give organic molecules distinct physical and chemical properties.

U12L4: Isomers

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Isomers have the SAME molecular formula but

DIFFERENT structural formula

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Isomers of a compound have different

physical and chemical properties because of

the difference in the structures

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A good tip: If you are not sure if something is

an isomer, name it.

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If it has a different name then the

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original compound, it IS an isomer.

If the name is the same, it is NOT an

isomer. Some things may look like isomers

but aren’t actually.

U12L5: Organic Reactions

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Addition

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2 reactants → 2 products

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Combustion

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Organic compound is burned in the

presences of oxygen to produce CO2 and

H2O - O2 is always a REACTANT

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Example: CH4 + 2O2 → CO2 + 2H2O

Substitution

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One or more atoms are replaced by

another atom(s) - Only happens in

alkanes - Results in two products - One

H is switched with one halogen (group

17)

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Adding one or more atoms at a double

or triple bond - Happens in alkenes or

alkynes

C3H6 + Cl2 → C3H6Cl2

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Fermentation

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Enzymatic breakdown of sugar into

alcohol (ethanol) and CO2 - Identify

alcohol and CO2 as a product

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Example: C6H12O6 → 2C2H5OH + 2CO2

Esterification

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The formation of a ester by reacting an

organic acid and an alcohol

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Alcohol (-OH) + Organic acid (-COOH) →

Ester (-COOCH)

Polymerization

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Small molecules called monomers bond

together to form polymers

Saponification

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Ester breaking down into acid and

alcohol - Reverse esterification -

Produces soap

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Fat + strong base → soap + glycerol

U13L1: Nuclear Decay Modes

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Nuclear reactions involve changes or transformations in an atom’s nucleus

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Chemical Reactions vs. Nuclear Reactions

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Chemical Reactions

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■ Atoms are rearranged by the breaking and formation of bonds.

■ Only electrons are involved in the breaking or forming of bonds.

■ Small amounts of energy are absorbed or released

■ Rates of reaction are influenced by temperature, concentration , pressure, and catalysts.

Nuclear Reactions

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■ Elements are converted from one type to another.

■ Protons, neutrons, electrons, and other subatomic particles are involved.

■ Large amounts of energy are absorbed or released.

■ Rates are not affected by temperature, pressure, or catalysts

Transmutation Reactions

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The conversion of an atom of one element to another element

Natural Transmutation Reactions Artificial Transmutation Reactions

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Nuclear Decay Modes

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Table N has the symbol for the decay mode for selected radioisotopes, as well as the half life

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Table O as an explanation of the decay mode symbol that is used to fill in nuclear equations

■ When balancing nuclear equations, the sum of the mass (the top #) on both sides of the reaction but

equal, and the sum of the atomic numbers (the bottom #) must be the same on both sides of the reaction

■ When asked to determine the element in a nuclear reaction - the atomic number (Bottom) tells you what

element it is - if you look at the periodic table

=

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Alpha Decay

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Positron

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Gamma Radiation

Beta Decay

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Comparing Particles

Particle Symbol Mass **Penetrating Power Ionization Power Shielding

Alpha α 4 amu Very Low Very High Paper/Skin

Beta β 1/2000 amu Intermediate Intermediate Aluminum

Gamma 𝛾 0 (energy only) Very High Very Low 2 inches lead

The beta particle is attracted to the positive

plate.The alpha particle is attracted to the

negative plate. The gamma radiation is not

attracted to any charged plate

U13L2: Half Life

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Half Life

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Every radioisotope has a rate of decay.

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Half-life is the time it takes for half of the sample to decay

into new elements.

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Table N lists half-life, decay mode (particles emitted during

decay), nuclide (radioisotope, and name of nuclide.

𝑡𝑜𝑡𝑎𝑙 𝑡𝑖𝑚𝑒

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= ℎ𝑎𝑙𝑓 𝑙𝑖𝑣𝑒𝑠 𝑝𝑎𝑠𝑠𝑒𝑑

𝑡𝑖𝑚𝑒/ℎ𝑎𝑙𝑓−𝑙𝑖𝑓𝑒

Common Isotopes

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Carbon-14 (C-14) has a half-life of 5700 years and is used to

date once living (organic) material

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Uranium-238 (U-238) has a half-life 4.5 billion years and is

used to determine the age of rock

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Iodine-131 (I-131) has a half-life 8.021 days and is used for

treatment of thyroid disorders

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Cobalt-60 (Co-60) has a half-life 5.271years and is used for

cancer treatments

U13L3: Fission vs. Fusion

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Fission

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Artificial transmutation = man made

Fission = splitting of heavy element

(large nucleus)

Heavy element + neutron → 2

middleweight nuclei + 1 or more

neutrons + energy

Example:

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Fusion

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Combines light element to produce a

heavier one

Gives off much more energy than fission

In the sun

Example:

•

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Both fission and fusion reactions produce energy and convert mass into energy

Radioisotopes - Benefits Radioisotopes - Risks:

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Tracers

Medical: radioactive iodine can be used to

diagnose and treat thyroid.

Food can be stored longer.

Nuclear Power

Radioactive dating

U-238 and Pb-206 are used for geological dating.

C-14 used for dating living material.

I-131 treating thyroid problems

Co-60 treating cancer

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Biological Damage: damage or destroy cells

Long Term Storage

Accidents: nuclear explosion

Pollution: nuclear waste