chem 120a fall 2005 - inorganic chemistry 1 small.pdf · chem 120a fall 2005 ... final exam: dec....

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Tuesday & Thursday 8:00 – 9:20 AMWarren Lecture Hall Room 2005

Prof. Karsten MeyerPacific Hall 4100E

2-4247, [email protected] Hours: Mo 10 – 12AM

Chem 120AFall 2005

Handouts http://www.inorganic-chemistry.net/kmpages/courses.html

Midterm I: 10/11 (30%)Midterm II: 11/08 (30%)

Final Exam: Dec. 6, 2005 @ 8 – 11 AM (40%)

2 hr Review Session Sunday before MidtermMidterm I: 10/9 location & time tbaMidterm II: 11/6 location & time tba

Chem 120A

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PLEASE:

• Try to be on time

•I know you’re busy,……but please turn off your cell phones

• I know it’s early,……but please don’t fall asleep(if you have to, don’t sit in the first row)

Chem 120AFall 2005

PLEASE:

• I know you’re in a rush,……but if you send me an email, please address me and sign your email

• If you do have a question…

…please feel free to interrupt me

…any time!!!

Chem 120A

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Chem 120A

In return, I PROMISE…

• I promise I’ll finish on time

• I promise I’ll help you to understand

• I promise I’ll follow the textbook…

…& Solutions Manual…

…strictly!!!

Chem 120A

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Miessler & Tarr<Inorganic Chemistry>

Brief Contents

9/229/27

9/29 + 10/0410/06 + 10/11

10/18

Mid

-te

rm I

Mid

-te

rm I

I

selected topics 10/2010/25 + 10/27

11/01 + 11/0311/10

Oct

. 1

1N

ov.

08

11/1511/17

11/22

11/29 + 12/01Final Exam

11/24 Thanksgiving

Dec. 06, 8 – 11AM

Chem 120A

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1. Contents

1-1 What is Inorganic Chemistry?

• Organic chemistry is defined as the chemistry of hydrocarbon compounds and their derivatives

But how about CO, CO2, and HCN…for instance?

• Inorganic chemistry can be described broadly as the chemistry of “everything else”

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• Organic chemistry is defined as the chemistry of hydrocarbon compounds and their derivatives

• Inorganic chemistry can be described broadly as the chemistry of “everything else”

may be a little too broadly defined…

• Organometallic chemistry bridges both areas;deals with metal-carbon bonds (incl. La & Ac)

• Bioinorganic chemistry bridges biochemistry &biology with inorganic chemistry (think hemes)

Supramolecular~, Phyisical Inorganic ~ etc…

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Figure 1-1. Single- and Multiple Bonds in Organic and Inorganic Molecules

1-2 Contrasts with Organic Chemistry?

triple bond!

Figure 1-2. Examples of Bonding Interactions


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Figure 1-3. Examples of Inorganic Compounds Containing H’s & Alkyl Ligands


Figure 1-4. Geometries of Inorganic Compounds


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Figure 1-5. Organometallic Compounds Containing π-Bonded Aromatics



Figure 1-6. Carbon-centered Metal Clusters…5- and 6-bonded C!?

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Figure 1-7. Fullerene Compounds…C60…buckminsterfullerene* “buckyballs”

…but don’t forget C70, C76, C84

*Richard Buckminster Fuller, creator of the “geodesic dome”

1-3 “Big Bang”Genesis of the Elements

t = 0: The matter was not actually matter, but pure energy. It contained infinite mass, infinite density, and no volume:Singularity (like Black Holes)

0 – 10-43 s: Mystery…nobody knows, energy behaved as singularity10-43 – 10-35 s: Energy and matter are indistinguishable

@ 10-35 s: Temperature of 1027K (the sun’s surface T is 6000 K)symmetry breaking, forces begin to separate

10-35 – 10-32 s: Inflation; universe grows exponentially (1050 in 10-32s)

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1-3 Big BangGenesis of the Elements

10-35 – 10-32 s: Inflation; universe grows exponentially (1050 in 10-32s)As it cooled, the energy of the universe began to condense. It moved up the list from photons to quarks, neutrinos, electrons, and protons…yippie yeah

1 – 100 s: Era of Nucleosynthesis, almost all of the helium and deuterium nuclei, and some lithium formed

@ 100 s: s all of the neutrons and protons had combined to form helium with trace amounts of a few other materials forming with it.


Then not much happened for about 300,000 years (75% H, 24% He)

1H1mass number

atomic number1H1

proton + neutronnuclear charge

4He2

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H11

99.9855% 0.0145%

most abundant element in the universe

heavy water cosmic radiation inhigh atmospheres

10-15 %

H12 H1

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Hydrogen H Deuterium D Tritium T



Initial Event:

H = p = proton of charge +1 and mass 1.007 mass unit (amu)11

e = e − = electron of charge -1 and mass 1/1823 amu-10

e = e + = positron of charge +1 and mass 1/1823 amu10

ve = a neutrino with no charge and a very small mass10

ve = an antineutrino with no charge and a very small mass10

n = a neutron with no charge and a mass 1.00901

γ = a gamma ray (high-energy photon ) with zero mass

β = a beta particle

α = a alpha particle

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Within minutes@ T = 109 K:

T1/2 (1n ) = 11.3 min

Hydrogen-Burning:

Helium-Burning@ T = 107 – 108 K:

Matarial gatherstogether intogalactic clusters


I guess, you got the idea…

In more massive Stars T > 6 108K:

Carbon-NitrogenCycles

@ still higher T:

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And last but not least…Cosmic Abundance of the Elements

log10/ V

atomic number / Z

nuclear stability most stable near Z = 26

have a close look at what is considered “rare” & “precious”

see what we are made off

1-4 Nuclear Reactions& Reactivity

Stable Isotopes

F only has one stable isotope: 19F

Cl has two stable isotopes: 35Cl (nat. abd.: 75.77%), 37Cl (24.23%)

3H and 14C are constantly formed (cosmic rays, low conc.)

Z = 26 “stable zone”, heavier elements (Z>=40) may have isotopes with long half-lifes, e.g., 40K 1.25 x 109y β− (1.32 MeV)or 234, 235,238U

man-made elements (Transuranics) such as Np and Puvia “Bombardment” of one element with nuclei of another,e.g., n + U folowed by release of β−

H11 H1

2 H13

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α = a alpha particle (He nucleus)

Alpha particles (Ernest Rutherford, England 1899) are a type of ionizing radiation ejected by the nuclei of some unstable atoms. They are large , heavy subatomic fragments consisting of 2 protons and 2 neutrons (4

2He).

Why?With increasing atomic mass, ratio of neutrons to protons increases from 1:1 to 1.6:1 for 238

92U. When the ratio of neutrons to protons in the nucleus is too low, certain atoms restore the balance by emitting alpha particles.

Relative Abundance of Uranium Isotopes Isotope 238-U 235-U 234-UNat. Abundance (%) 99.27 0.72 0.0055Half-life (years) 4.47 billion 700 million 246,000


β = a beta particle (e −)

Beta Particles (Henri Becquerel , 1900) are equivalent to electrons. The difference is that beta particles originate in the nucleus and electrons originate outside the nucleus.

Why?Beta particle emission occurs when the ratio of neutrons to protons in the nucleus is too high: an excess neutron transforms into a proton and an electron. The proton stays in the nucleus and the electron is ejected energetically.-> a new element is born!

Beta emitters are: 99Tc (99Ru) or 60Co (60Ni) or 3H (3He)

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γ = a gamma ray (high-energy photon ) with zero mass

Gamma Rays (Henri Becquerel 1896) have no mass and no electrical charge; they are pure electromagnetic energy(10,000 times as much energy as the photons in the visible)gamma photons travel at the speed of light and can cover hundreds to thousands of meters in air before spending their energy

Why?Gamma radiation emission occurs when the nucleus of a radioactive atom has too much energy (often follows the emission of a beta particle).

E.g.: 137Cs β + (137Ba)* γ + 137Ba

1-6 History ofInorganic Chemistry

gold copper silver tin antimony

3000 BC

lead

1500 BC

iron

colored glasses & ceramic glazesmade from SiO2 and MOx

http://www.chemsoc.org/timeline/pages/timeline.html

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Anno Domini

Simplified, the aims of the alchemists were threefold: to find the Stone of Knowledge (The Philosophers' Stone), to discover the medium of Eternal Youth and Health, and to discover the transmutation of metals. To the medieval alchemist’s mind the different elements were but the same original substance in varying degrees of purity. Gold was the purest of all and silver followed closely.

Alchemy


Anno Domini

Various alchemical symbols used to denote elements until the 18th Century

antimony arsenic bismuth copper gold iron lead

magnesium mercury phosphorous platinum potassium silver sulfur

tin zinc

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Anno DominiIn the 18th century scientists tried to pry loose the real achievements in chemistry, pharmacology and medicine from this confusing cornucopia of science and magic.

Henry Cavendish1731 – 1810

A. L. de Lavoisier1743 – 1794

Discovery of Hydrogen (1766)


By 1869

Concepts of atoms & molecules are well-established:

Dmitri I. Mendeleev (Born in Siberia 1834, 17 Feb. 1869 )

“I began to look about and write down the elements with their atomic weights and typical properties, analogous elements and like atomic weights on separate cards, and this soon convinced me that the properties of elements are in periodic dependence upon their atomic weights.”

--Mendeleev, Principles of Chemistry, 1905, Vol. II

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By 1869


Dmitri I. Mendeleev’s Periodic Table of the Elements (17 Feb. 1869 )


By 1869


Dmitri I. Mendeleev’s Periodic Table of the Elements (17 Feb. 1869 )

I.I. Mendeleev, J. Russ. Phys. Chem., 1869, I,60.

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In 1913

In 1913 British physicist Henry Moseley confirmed earlier suggestions that an element's chemical properties are only roughly related to its atomic weight (now known to be roughly equal to the number of protons plus neutrons in the nucleus). What really matters is the element's atomic number - the number of electrons its atom carries, which Moseley could measure with X-rays.

Ever since, elements have been arranged on the periodic table according to their atomic numbers.


chem 120a fall 2005 - inorganic chemistry 1 small.pdf · chem 120a fall 2005 ... final exam: dec....

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