Classroom+Notes+(p4)

> > __Assignment: Read Section 1.1__ > __Vocabulary__ > > Chemistry: > > Substance: > > __Assignment: Read Section 1.2__ > __Vocabulary__ > > Mass > > Weight > > __Assignment: Read Section 1.3__ > __Vocabulary__ > > Control > > Dependent variable > > Independent variable > > Hypothesis > > Qualitative Data > > Quantitative Data > > Scientific law > > Theory > > __Assignment Read Section 1.4__ > __Vocabulary__ > > Pure research > > Applied research > > > __LAB SAFETY__ > Safety Rules on p. 19 Table 1.2 > > __Activities__ > Icebreaker (Theory, Substance, Mixture, Metric prefix and meaning, Something in common) > > __CHEMLAB__ Identify the Water Source > > __Assignment__ > ___Discussion Assignment: Visit our Wiki at http://honorschemistrycyhs.wikispaces.com/ > > Pick out an article under the article tab from the selections __posted on the board.__ Read one and post a commentary on it under your name on our wiki. See the rubric presented below. > > See below for the discussion post rubric.* > > __*Post and Response Rubric__ > > || Posts are insightful and show a good comprehension of the content. || Posts are insightful and show a fair comprehension of the content. || Posts are insightful and show a minimum comprehension of the content. || Posts are not insightful and show a minimum comprehension of the content. || Posts are not insightful and show no comprehension of the content. || Posts are not done. || > || Posts and responses are done on time. || Posts and responses are one day late. || Posts and responses are two days late. || Posts and responses are three days late. || Posts and responses are more than three days late. || Posts and responses are not done. || > || Responses are insightful and show a good comprehension of the content. || Responses are insightful and show a fair comprehension of the content. || Responses are insightful and show a minimum comprehension of the content. || Responses are not insightful and show a minimum comprehension of the content. || Responses are not insightful and show no comprehension of the content. || Responses are not done. || > || Posts and responses are minimum of 75 words. || Posts and responses are minimum of 75 words. || Posts and responses are more than 25 words but less than 75. || Posts and responses are less than 25 words. || Posts and responses are less than 10 words. || Posts and responses are not done. || > __Textbook assignment__ > # 31, 32 42, 43, 44, 45 pp 26-27 > Funsie #1 > Quiz #1 > > Section #2 Unit #2
 * **__INTRODUCTION TO CHEMISTRY__**
 * 5 ||  4  ||  3  ||  2  ||  1  ||  0  ||
 * Electrons in Atoms(pd.#4)
 * Electrons in Atoms(pd.#4)
 * Electrons in Atoms(pd.#4)

Light and Quantized Energy

Wave nature of light (Electromagnetic Spectrum)

Frequency (ν)

Wavelength (λ)

Amplitude

Visible Light 400- 750 nm. Which is red? Which is violet?

c = Speed of Light = 2.998 x 108 m/sec = 2.998 x 1017 nm/sec

c =λ x ν

quantum

photon

photoelectric effect

The energy of each photon of light can be calculated by:

E = hν or E = hc/λ Where h is Planck’s constant.

h = 6.626 x 10-34 J.s/photon

atomic emission spectrum

Classwork: YCP worksheet Properties of Light

Lab: Flame Tests

Read and Post : Article on Motion Detectors

Textbook assignment : Read Section 5.1 Do #’s 5-7 p. 143, #13, 14 p. 145
 * 35, 44, 47-51, 55, 58 p. 166

Quantum Theory and the Atom

Bohr Model

Ground state vs Excited state:

Quantum Mechanical Model of the Atom.

The modern day model of the atom uses the concepts of quantum theory to best describe the behavior of electrons. We should not perceive of electrons as orbiting the nucleus like planets around the sun. They behave by a different set of rules.

deBroglie equation:

Heisenburg uncertainty principle

Schrodinger wave equation

TProxy-Connection: keep-alive Cache-Control: max-age=0 descriProxy-Connection: keep-alive Cache-Control: max-age=0 oxy-Connection: keep-alive Cache-Control: max-age=0 the energy%Proxy-Connection: keep-alive Cache-Control: max-age=0 behavior and probable location of an electron we assign each one a unique set of 4 quantum numbers. These are designated with the symbols n, l, ml and ms (See below).

Orbitals can only hold 2 electrons.

Principal quantum number (n): Designates the energy of the electron. Every time you go up a level, you are further from the nucleus. n = 1 (holds 2 electrons), 2 (holds eight electrons), 3 (holds eighteen electrons), 4 (holds thirty-two electrons)…goes to infinity Capacity = 2n^2

In the Bohr Model, the lowest level is n=1. In n=1 only 2 electrons can be seated there at any given time. The level n=2 can seat 8 electrons. The n=3 can seat 18 electrons. The capacity of any level is calculated as Capacity=2n^2. Every Orbital can only hold 2 electrons at a time.

Second (azimuthal) quantum number (l): Designates the shape of the orbital(s); "sub-level" l = 0 (s), 1 (p), 2 (d), 3 (f)…n-1 - maximum These correspond to the shapes of the probability distributions(wave functions or orbitals). The first 4 'l' values are often designated: s; 1 orbital (sphere), p; 3 orbitals (dumbbell/peanuts), The p orbital can be shown in three different ways: "py", "px", "pz". (second letter corresponds with the axis it is on) d; 5 orbitals (clover leaf/dutterflies), f; 7 orbitals (freaks).

Remember: The f orbitals are oddly shaped, and can be remembered as the "freaks".
Third (magnetic) quantum number (ml): Used to designate the orientation of the orbitals in space. ml = -l…0…+l If 'l' = 0, ml can only = 0 If 'l' = 1, ml can equal -1, 0, +1 If 'l' = 2, ml can equal -2, -1, 0, +1, +2

Designates the # of orbitals. If l=0 then ml=0 as well. If l=1 then ml could be ml=-1, ml=0, m=+1. If l=2 then ml could be -2,-1,0,1, or 2. The ml is the NUMBER of NUMBERS.

Fourth quantum number, ms. Used to designate the spin of the electron. ms = +1/2 or - 1/2

Coordinates: 3 (n), 2 (l), +1(ml), +1/2 (ms)

ms = +1/2 or - 1/2 clockwise counter clockwise Ms (designates the spin)

Example: An electrons coordinate could be 3,2,+1, and a spin of +1/2.

Classwork: Worksheets as assigned

Textbook Assignement: Read Section 5.2 Do # 15 p. 155; # 63, 67, 68, 70, 71, 72 p. 167; # 94, 97, 105, 106 p. 168

Electron Configurations, Orbital Diagrams and Abbreviated Electron Configurations

Aufbau principle The Aufbau principle states that each electron will occupy the lowest energy orbital available when at a ground state.

The above images are examples of the classification of the different orbital levels and their energy states. These diagrams are also called an Aufbau Diagram, Aufbau meaning "building up" in German.

Pauli exclusion principle This states that no two electrons in an atom can have an identical quantum number.

Hund’s rule The Hund's rule states that an electron with the same spin must occupy each equal energy orbital before an electron with an opposite spin may occupy the same orbital. In other words, when filling a set of orbitals, you should maximize the amount of unpaired electrons. For example, above is a picture of the element Nitrogen with 7 electrons. Notice that there are three unpaired electrons in the sublevel 2p, not two paired and and one unpaired.

Electron-dot structure The electron dot structure is a picture shown where the viewer can easily distinguish the amount of valence electrons present. It consists of the elements symbol surronded by dots representing the valence electrons. They are placed one at a time on the four sides of the symbol and then paired up until all are used. They CANNOT be paired until there is an electron present on all four sides. As shown above in the element phosphorus, it contains 5 valence electrons. Notice how there are no open sides, and only one pair of electrons. Not two pairs of electrons and and one single electron.

Valence electrons Valence electrons are the total number of electrons in the highest principle level. As shown in the periodic table below, every column lists the amount of valence electrons an element has as shown above the element in roman numeral form. You can use these numbers to find the electron configuration, orbital diagrams, and electron dot configurations. Abbreviated Electron Configurations // 2He 1s^2 // 1= n s= sublevel ^2= number of electrons

Spin: Up arrow for clockwise Down arrow for counter clockwise

Periodic Table: 1s^2 down two over one 2s^2 down two over two p= p block

Example: Beryllium: 5Be 1s^2 2s^2

5B 1s^2 2s^2 2p^1

Nitrogen: 7N 1s^2 2s^2 2p^3 abbreviation: [He] 2s^2 2p^3 The blocks indicate which orbital will be the last filled. For example, in aluminum the last orbital with electrons when it is on the ground state is "p" and for beryllium it is "s".

Overall... An element can be written four different ways as shown for aluminum (which contains 13 electrons, 3 valence electrons, and 1 unpaired electron)
 * the orbital notation
 * [[image:http://www.mrbigler.com/Chem1-C1/topics/quantum/electron-configuration-notations_files/image001.gif width="413" height="68"]]
 * an electron configuration
 * 1s^2 2s^2 2p^6 3s^2 3p^1
 * the noble gas configuration
 * [Ne] 3s^2 3p^1
 * the electron dot diagram
 * [[image:http://envirochem.us/images/periodic/ElectronDot/Al.gif]] (notice it doesn't matter which side you begin to add the dots on)

Exceptions to Normal Electron Configurations Factoid! filled and 1/2 filled sets of orbitals have extra stability therefore electrons automatically settle to become more stable

Exceptions in the transition area "d"
 * Chromium
 * expected for cr(24)= [Ar] 4s^2 3d^4
 * actual for cr(24)= [Ar] 4s^1 3d^5
 * [[image:http://www4b.wolframalpha.com/Calculate/MSP/MSP238219eefii0c354gbhd00005g79ha4d37d9ie61?MSPStoreType=image/gif&s=53&w=120&h=51]] notice in how this picture, the 4s level isn't completely filled, instead an electron jumps up a level into 3d making 3d more stable. This is because 1/2 filled orbitals have extra stability compared to ones that aren't
 * Other examples: Silver, Gold, Copper, and Molybdenum
 * Excited: Cu= [Ar] 4s^1 3d^9 4p^1
 * to return it to it's ground state, the electron will move back down to 3d^9 making it [Ar] 4s^1 3d^10

Electron Arrangement in Ions

Ions= Charged Two Types
 * Cations: "+" ions
 * CATions are nice, thus they are positive
 * Anions: "-" ions

An Example of an Anion... Fluorine= f(9)
 * 1s^2 2s^2 2p^5
 * f-= Fluoride
 * still has 9 protons, but 10 electrons
 * 1s^2 2s^2 2p^6
 * the extra electron makes it stable, creating the same electron configuration of neon, a fairly stable noble gas, however with one less proton.
 * while fluorine is toxic, fluoride is used to clean teeth and is not as toxic

An Example of a Cation... Na(11) The picture above shows how many electrons an element needs to lose to become a cation that is very stable, this is due to the fact it would then have the same electron configuration as a noble gas, elements praised for their ability to remain stable.
 * 1s^2 2s^2 2p^6 3s^1
 * Na+= Sodium
 * still has 11 protons, but 10 electrons
 * 1s^2 2s^2 2p^6
 * once again, this has the same configuration as neon, a stable noble gas making it far less harmful than its toxic counterpart
 * Fe(26)= [Ar] 4s^2 3d^6
 * Fe+2= [Ar] 3d^6
 * Fe+3= [Ar] 3d^5
 * Iron three is the most stable form of iron because it's "d" orbital is exactly half filled (5/10)


 * Note the "d" block may only form cations
 * Note, all "d" block elements lose the "s" electrons first**

Classwork: Worksheets as assigned.

Textbook Assignment: Read Section 5.3 Do #’s 21-24 p. 160; # 29, 30, 33 p. 162; # 81, 86, 87, 88, 112-114 pp 167-169.

The Periodic Table and Periodic Law

Periodic Table

Groups or family: Chemistry a set of elements occupying a column in the periodic table and having broadly similar properties arising from their similar electronic structure.

Ex: Alkali metals : any of the elements lithium, sodium, potassium, rubidium, cesium, and francium, occupying Group IA (1) of the periodic table. They are very reactive, electropositive, monovalent metals forming strongly alkaline hydroxides.

Alkaline Earth Metals: any of the elements beryllium, magnesium, calcium, strontium, barium, and radium, occupying Group IIA (2) of the periodic table. They are reactive, electropositive, divalent metals, and form basic oxides that react with water to form comparatively insoluble hydroxides. Transition metals any of the set of metallic elements occupying a central block (Groups IVB–VIII, IB, and IIB, or 4–12) in the periodic table, e.g., iron, manganese, chromium, and copper. Chemically they show variable valence and a strong tendency to form coordination compounds, and many of their compounds are colored.

Halogens: any of the elements fluorine, chlorine, bromine, iodine, and astatine, occupying group VIIA (17) of the periodic table. They are reactive nonmetallic elements that form strongly acidic compounds with hydrogen, from which simple salts can be made.

Noble or inert gases: any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table. They were long believed to be totally unreactive but compounds of xenon, krypton, and radon are now known.

Metalloids : an element (e.g., arsenic, antimony, or tin) whose properties are intermediate between those of metals and solid nonmetals or semiconductors.

Boron, Silicon, Germanium, Arsenic, Antimony and Tellurium.

Periods: a set of elements occupying an entire horizontal **row** in the periodic table. #’s 1- 7.

Rare Earth elements: any of a group of chemically similar metallic elements comprising the lanthanide series and (usually) scandium and yttrium. They are not esp. rare, but they tend to occur together in nature and are difficult to separate from one another.

Actinides:

Textbook Assignment: Read Section 6.1 and 6.2 Do #’s 2, 4, 5 p. 181; #12, 13 p. 186; # 29, 30, 31, 32, 33 35, 36, 40, 43, 46, 47, 48 pp198-199.

Trends in the Periodic Table

Increasing Core Charge Increasing core charge is related to the horizontal movement on the Periodic table. As you move left across the table, the core charge increases. Core charge, also known as effective nuclear charge, is the number of protons minus the number of core electrons. The core charge is what "pulls" or "reigns" in the valence electrons.

Lithium= 3p - 2e = +1 Beryllium= 4p - 2e = +2 Boron= 5p - 2e = +3 Carbon= 6p - 2e = +4 Nitrogen= 7p - 2e = +5 Oxygen= 8p - 2e = +6 Fluorine= 9p - 2e = +7 Neon= 10p - 2e = +8 "High and tight, in the upper right" "Upper righty tighty." Shielding ||
 * |||||||||| [[image:file:///Users/mwilliams/Library/Caches/TemporaryItems/msoclip/0/clip_image003.png width="168" height="12"]] ||
 * ||  || [[image:file:///Users/mwilliams/Library/Caches/TemporaryItems/msoclip/0/clip_image004.png width="12" height="131"]] ||
 * ||  ||^   ||   ||   || Increasing
 * ||  || [[image:file:///Users/mwilliams/Library/Caches/TemporaryItems/msoclip/0/clip_image004.png width="12" height="131"]] ||
 * ||  ||^   ||   ||   || Increasing
 * ||  ||^   ||   ||   || Increasing

<span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Shielding increases as you move down the periodic table, through the consecutive periods. The core charge within groups(columns) is the same. <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Alkali Metals: <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Lithium= 1s^2,2s^1 <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">2 electron shield <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Sodium= 1s^2,2s^2,2p^6,3s^1 <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">10 electron shield <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Potassium - 18 electron shield <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;"> <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Notice the ever-increasing layers based on the amount in the electron configuration. <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">"Large and loose, in the lower left." <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">"Lower lefty loosy."

<span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;"> <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">The "more famous" elements are in the lower left, so they have a larger "bodyguard circle."

Atomic radius: term used to describe the size of the atom Elements that have larger atomic radius are found in the lower left of the periodic table.

Elements that have smaller atomic radius are found in the upper right of the periodic table.

Ionic Radius: Measure of the size of an atoms ion. Elements that have larger ionic radius are found in the upper right of the periodic table.

Elements that have smaller ionic radius are found in the lower left of the periodic table.



Ionization Energy (I.E.): The energy required to remove an electron

(You can also think of this as how well the atom holds on to its electrons) Na 1s^2 2s^2 2p^6

1st I.E.- (Na^+) --> (Na^+) + (1e-) 2nd I.E.- (NA^+) --> (Na^+2) + (1e-) 3rd I. E.- (NA^+2) --> (Na^+) + (1e-)

DON'T MESS WITH THE CORE

Electronegativity(E.N.): Measure of the amount of attraction an atom has for electrons in a chemical bond

Highest: Flourine Lowest: Cesium

-Another way of thinking of this is: Since the atoms in the upper right are smaller, they will need their electrons more, so they will hold on to them and steal from the atoms with too many electrons.

ALL ATOMS WANT EIGHT VALENCE ELECTRONS, AND WILL LOSE, GAIN, AND SHARE ELECTRONS WITH OTHER ATOMS TO HAVE EIGHT- AND ONLY EIGHT - ELECTRONS (This is the idea of the octet rule)

In the right corner, there are small atoms, with high I.E. and high E.N.

.

In the left corner, there are large atoms, with low I.E. and low E.N.

Textbook Assig

__//** IONIC COMPOUNDS AND METALS **//__

Notes- Na 1s^2 2s^2 2p^6 3s^1 take away and you get **N+1s^2 2s^2 2p^6** **Atoms don't exists as atoms** **In the little boxes in the periodic table in the planner there are little charges written in the boxes.**

**NaCl- is Ionic** **H20- is not** **Co2- is not** **CuCl2- is Ionic** **K No3- is Ionic**

**if you see a metal, you must put ionic. Ionic means there are charges (i.e. +2 charge) When a negative charge and a positive charge then you have an ionic bond.**

Cation- ﻿positively charged ion forms when an atom loses one or more valence electrons.

Lattice Energy: Energy needed to break an ionic lattice into a gas




 * Water is deadly to ionic compounds

Strength of Crystal Lattice: Factors that affect lattice energy are size of ions and charge of ions. 1) Size of ions 2) Charge of ions Electrolyte- Ionic compound who's aqueous conducts electricity. Metal Ions (Group 1, 2, 13)-
 * Small ions have large lattice energy, "little ions pack tightly"
 * Think of if having to fill a jar as full as you can so sand would be better then marbles because they are smaller and can pack better
 * The higher the charge the stronger the lattice energy
 * Example of a very strong ion: Al2 O3 (Al2 has a plus 3 ion charge and O3 has a negative 2 ion charge)
 * Example of a very weak ion: Cs+1 I-1
 * Salt is a strong electrolyte
 * Vinegar is a weak electrolyte
 * Sugar is a non electrolyte

Transition Metal Ions (D block)-

Anion- negatively charged atom

Non-metal Ions-

Group 15, 16, 17- I


 * Textbook Assignment: Read Section 7.1 Do #’s 5, 6 p. 209 # 48, 49, 52-55 p. 232**


 * Textbook Assignment: Read Section 7.2 Do #’s 16, 17 p. 217; # 63, 65, 67, 70, 71, 73, 74, 75 p. 233 # 100, 101 p. 234**

__Using the Periodic Table to Assign Ionic Charges(Oxidation Numbers)__

__Naming and Writing Ionic Formulas__

NO PREFIXES!
 * __Binary Ionic__** 1 metal and 1 nonmetal - a total of 2 ions!

Always cation(typically a metal); anion (typically a non-metal) ending in –ide. Know when to go **Roman!**

Sn2+ O2- : Tin(II) oxide = SnO

More examples of monoatomic ions:

NaCl - sodium chloride

CaF2 - calcium fluoride

AlBr­3 - Aluminum bromide

Cu2O - Copper oxide

PtCl3 - Platinum chloride

KCl - Potassium chloride

H2O - Water!

Aluminum oxide:



Magnesium chloride Mg2+ Cl 1- MgCl 2 Potassium oxide K1+ O 2- K2O Calcium sulfide Ca2+ S2- CaS

"Island of Certainty" No roman numerals allowed here. Group 11 - Ag always +1 Group 12 - Zn, Cd always +2 Group 13 - Al always +3

__Polyatomic Ions__

<span style="font-family: arial,sans-serif; font-size: small; line-height: normal;">of or relating to a molecule made up of more than two atoms


 * __Ionic compounds that contain polyatomic ions__**

"Sulfur called carbon crazy" - for 2- polyatomic ions

Beginnings and Endings:

hypo - under "i" is skinny Nitr__ite__ - NO2 1- "a" is fat Nitr__ate__ - NO3 - per- over "//__per__//iscope" or" "hy//__per__//active a periscope

Ex. CuSO4 copper(II) sulfate

CuSO3 copper(II) sulfite

Magnesium nitrate Mg2+ NO31-

Mg(NO3)2

Ammonium phosphate NH4 1+ PO4 3-

(NH4)3PO4

<span style="color: #da251a; font-family: Impact,Charcoal,sans-serif; font-size: 180%;">Stories:

Hydrox cookie: OH 1- (take off top or -1 and you are left with OH 1- which is Hydroxide )

Phone call: NOOO 1- (Night rate in 15 minutes! = Nitrate or NO3 1-)

Code 1 (take off of Cops): CHO 232 officer Acetate population of -1 (someone died)

officer acetate

Ox story c c __o__ o o o <span style="font-family: 'Comic Sans MS',cursive; font-size: 350%;">That's the stories SUCKA!


 * Textbook Assignment: Read Section 7.3 Do #’s 36, 37, 38, 39 p. 224; 81-86 p. 233; #102, 111 p. 234 + worksheets as assigned.**

Some are incredibly strong while others are very weak.
 * Metallic bonding:** Count on metallic bonds to keep things together and support different objects.


 * Electron sea model:** a lattice of electrons with the valence electrons roaming around the core electrons.

> Ex. Na
 * Delocalized electrons:** Do not stay in one location. They can create electricity because they can move freely.

Sodium-classic metal, not very useful for construction, very soft. 11Na 1s^2 2s^2 2p^2 2p^6 3s^1 11p+ 10e-

They stick together because they create a lattice. Large and loose, no high core charge- free to move around, they roam around like the sea, "sea of electrons."

1. Luster\shiney-ness. 2. They react with oxygen. 3. They conduct electricity and heat. 4. Ductility\malleability Aluminum reacts with oxygen to a point of creating a layer of aluminum oxide that protects the rest of the aluminum..
 * Properties of metals:**


 * Alloys:** An alloy is a mixture of metals such as stainless steel, bronze, and brass. Alloys are used in everyday life like utensils and appliances. They are not bonded but just mixed together.

Stainless steel


 * Textbook Assignment: Read Section 7.4 Do # 44 p. 228; # 87, 91, 96, 98, 113 pp. 233-234; #**

COVALENT BONDING
Covalent Bond //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">the cooperation of the outer electrons

Molecules/Molecular Compounds //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;"> Two or more non-metals chemically combined

<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Examples: <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H2O: Water <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">NH3: Ammonia <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">C2H6O: Ethyl Alcohol (Ethanol) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">C5H12: Pentane

Structural Formulas //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: // <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Condensed Molecular Formula <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Pentane: CH3-Ch2-CH2-Ch2-Ch3 OR Ch3(CH2)3Ch3

Diatomic (two atom) Elements //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;"> Elements that come in pairs covalently bonded together <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">There are seven diatomic elements: H, O, N, Cl, Br, I, F <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Always come with a partner ("buddy system") H2,O2, N2, Cl2, Br2, I2, F2

HONClBrIF <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">--a monster with a sharks body with a hamster's head that can shot laser beams through it's eyes that likes to attack peeps <span style="font-family: 'Times New Roman','serif'; font-size: 12pt; height: 117.75pt; width: 159.75pt;"> ClIF BrOHN <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">--a strong masculine name like James Bond <span style="font-family: 'Times New Roman','serif'; font-size: 12pt; height: 319.5pt; width: 226.5pt;"> <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Six of the seven diatomic element form a seven shape on the periodic table that points (like a dead man pointing) to the seventh element Single covalent bond //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;"> two elements that share two electrons that were "lonely" (unpaired), elements like chlorine form this bond with itself (strong) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">

Double covalent bond //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;"> two elements that share 4 electrons, elements like oxygen form this bond with itself (pretty strong) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">

Triple Covalent Bond //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">: //<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">two electrons that share 6 electrons, elements like nitrogen form this bond with itself (really strong) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;"> <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">1- mon 2- di 3- tri 4- tetra 5- penta <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">6- hexa 7-hepta 8-octa 9-nona 10- deca
 * Binary Molecular** 2 non-metals

<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Examples: <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">CO carbon **mon**oxide <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">PCl3 phosphorous **tri**chloridw <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">N2O **di**nitrogen monoxide

<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H_ -- binary acids contain H and one other element <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H_O -- oxy acids contain H, Oxygen, and one other element
 * Acids**

Binary Acids Hydro-root word ends with an –ic in the acid name

<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Examples: <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">HCl **hydro**chlor**ic** acid <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">HBr **hydro**brom**ic** acid <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H2S **hydro**sulfur**ic** acid <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">HI **hydro**iod**ic** acid

Oxy Acids “I took a b <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">**ite** and became nause**ous**” <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">“I **ate** it and became s**ic**k”

<span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">Examples: <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H2SO4 sulfuric acid (SO4 = sulf**ate**, -ate becomes -ic) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">HNO3 nitric acid (NO3 = nitr**ate**, -ate becomes -ic) <span style="font-family: 'Times New Roman','serif'; font-size: 12pt;">H3PO4 phosphoric acid (PO4 = phosph**ate**, -ate becomes -ic) HNO2 nitrous acid (NO2 = nitr**ite**, -ite becomes -ous) HClO hypochlorous acid (ClO = hypochlor**ite**, -ite becomes -ous) H2SO3 sulfurous acid (SO3 = sulf**ite**, -ite becomes -ous)

= Molecular Structures and Intermolecular Attractions =
 * The shape of the objects depend on the molecular arrangement. This is what makes you different looking from everyone else.

Lewis Structures and IM Forces

Single, Double and Triple Covalent Bonds

Generally occurs between 2 or more non-metal atoms which share valence electrons in order to achieve a Noble gas configuration. (usually 8 electrons). Hence the Octet Rule.

Primo example : HONClBrIF

Bonding Tendencies( Not chiseled in stone)

 * Carbon (C) bonds 4x's: is very complex and is the backbone of life.
 * Nitrogen (N) bonds 3x's
 * Oxygen (O) bonds 2x's
 * Halogens bond 1x
 * Hydrogen (H) bonds 1x.... written in stone!



Lewis Structures Rules p 254 1) Draw a skeleton attaching to all atoms with single covalent bonds. 2) Count all valence electrons. 3) Subtract 2 electrons for each single covalent bond in the skeleton. 4) Distribute remaining electrons as non-bonding pairs.

*Look for double and triple bonds


Ex. NH3



Cl2CO



HCOOH (Formica Acid)--Formica means "Ant" in Latin. When people would mash the ants formica acid would come out of them.



They spit fire out of their butts. -Mr. Williams.....Ouch!!!! April Fools!!!!!!! SO32- -Don't forget to add 2 because of the -2 charge of Sulfite.

" WATCH OUT FOR THE BBe's"
 * Example of exceptions to the Octet Rule**
 * 1) Electron deficient molecule Ex: BF3 and BeF2**
 * 2) Odd number of electrons**
 * 3)More than an octet**
 * BF3 (Example of Rule 1 of Exceptions to Octet Rule**
 * -Boron is stable with 6 electrons **




 * BeF2 (Example of Rule 1 of Exceptions of Octet Rule**
 * -Beryllium is stable with 4 electrons **


 * [[image:webkit-fake-url://48C9C3DB-585B-4523-AC08-B523B7166305/IMG00001.GIF.gif width="276" height="93" caption="IMG00001.GIF.gif"]] 24 valece elc **


 * NO (In the category of the dreaded......." FREE RADICAL" .....OOOOOOOHHHH NOOOOOO!!**
 * -Definition of Free Radical(Chemistry)**

<span style="background-attachment: initial; background-clip: initial; background-color: #ffffff; background-image: initial; background-origin: initial; border-top-color: #ff3300; border-top-style: solid; border-top-width: 3px; display: block; font-family: inherit; font-size: 12px; font-style: inherit; font-weight: inherit; margin-bottom: 0.75em; margin-left: auto; margin-right: auto; margin-top: 0px; padding-bottom: 0px; padding-left: 15px; padding-right: 15px; padding-top: 0px; position: relative; text-align: left; text-decoration: inherit; width: 930px;"> <span style="display: inline !important; font-family: inherit; font-size: 12px; font-style: inherit; font-weight: inherit; margin-bottom: 1.5em; margin-left: 0px; margin-right: 0px; margin-top: 1.5em; padding-bottom: 0px; padding-left: 0px; padding-right: 0px; padding-top: 0px; position: static; text-decoration: inherit; width: 930px; zoom: 1;"> A molecule with an unpaired electron. Because they have a free electron such molecules are highly reactive.-About.com


 * -Free Radicals: take electrons away from the body; Vitamins C & E which are antioxidants react with free radicals and absorb them to not harm your body. So Vitamins are**
 * mmm mmm GOOD!!!!**
 * -Free Radical has an ODD NUMBER of electrons**
 * -HO and NO21- are other examples of Free Radicals**
 * [[image:webkit-fake-url://C3A519EB-CAEF-4CD6-B0A0-026FCFC51753/NO.gif caption="NO.gif"]] 11 valence electrons - 2= 9 electrons **


 * NO21-**
 * -Resonance stabilizes the ion. **
 * -DON'T forget to add 1 because of the 1- charge. **


 * [[image:webkit-fake-url://EB8B6134-F32A-4674-A292-F37D840E149B/ex21_3a.gif caption="ex21_3a.gif"]] 5 valence e-'s + 12=17 +1=18- 4- 14 electrons or 7 electron pairs **


 * Resonance**
 * -Can be seen in different atoms and molecules**
 * -Double bonds can switch places at the speed of light.**
 * Ex: Nitrate: [[image:webkit-fake-url://684919EE-FAE8-4B10-90F6-6AA043E6DB2F/imgres.jpg caption="imgres.jpg"]] **


 * Expanded Octets**


 * -Elements such as Phosphorus and and Sulfur can have more than 4 bonds. **


 * Primo Example:**


 * Non-metal Halides**


 * PCl5**


 * SF6**
 * -Is a very heavy gas**
 * -Breathable; opposite effect of Helium: You will speak LOW!**
 * -Is not harmful**



__Molecular Geometry and Bond Angles__

Valence Shell Electron-Pair Repulsion Theory
 * __VSEPR__**

<span style="font: normal normal normal 13px/normal Arial; letter-spacing: 0px; line-height: 19px; margin: 0px;">**V**alence **S**hell **E**lectron **P**air **R**epulsion theory.

<span style="color: #000099; font: normal normal normal 13px/normal Arial; letter-spacing: 0px; line-height: 19px; margin: 0px;">__[|Wikipedia Methane!]__


 * __Central atom with 4 attachments.__**

Tetrahedral


 * Ex. C H^4 (Methane) **
 * **contains a 109.5 degree angle**


 * __Central atom with 3 attachments and 1 nonbonding pair.__**

Pyrimidal


 * Ex. NH^3 **
 * **contains a 107 degree angle**
 * **angle is less because non-bonding pair repels bonded pairs, pushing them closer together**
 * **pyramidal shape due to non-bonding pair**


 * __Central atom with 2 attachments and 2 nonbonding pairs.__**

Bent


 * Ex. H^2O (water) **
 * **angle is 105**
 * **due to two bonding pairs once again. This causes more of a repelling force than one bonding pair as shown in the pyridmidal**


 * __Central atom with 3 attachments.__**

Trigonal Planar

** Ex. BCl^3 (boron trichloride)**
 * **angle is exactly 120 degrees because it has no bonding pairs**
 * **relatively flat**


 * __Central atom with 2 attachments.__**

Linear



Ex. CO^2
 * angle measures 180 degrees

Expanded Octet Shapes


 * PCl5**


 * SF6**

Textbook Assignment #3 : Read Section 8.3, 8.4 Do #’s 44-46 p. 258; #’s 47,48,52, 54 p. 260; # 63, 64, 67(skip hybrid orbitals) p. 264, # 101, 102, 108, 111, 112(skip hybrid orbitals), 126 pp 274-276.

__Molecular Polarity__


 * A molecule is considered polar if it has a permanent positive region and a permanent negative region. Molecules that are polar are often called dipoles.**


 * In order to be polar a molecule must have polar bonds(eg ∆ EN > 0.3 but < 1.7) and be asymmetrical. That is the effect of the unequal sharing of electrons can’t be cancelled by symmetry.**
 * View this site and the animation found there for further explanations:**


 * [] **

Conditions for polarity(a dipole): 1. Atoms that make up the molecule must have different electron negativities (Delta Electronegativity(DEN) must be greater than 0) jesus8880.com Lowercase delta means partial(partially shared) 2. Molecule must be non-symmetrical - non-polar(non-symmetrical): CO2, BF3 - polar(symmetrical): H2O, NH3

**-Something thats polar has a charge**
 * Ex.**


 * Molecule has to be non symmetical to have polarity.**

__Intermolecular Attractions__**

These are attractions between molecules. They are weaker than the intramolecular attractions better know as covalent bonds that are within a molecule.

Types <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">A brush, a handshake, or an embrace? <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Weak mice, normal mice, super mice!

<span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;"> 1.) Dispersion forces (London) or induced dipole. <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;"><span style="color: #000000; font-family: arial,helvetica,sans-serif;"> Weakest of the forces, the "brush" <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Caused by fluctuations in the electron field (electron cloud), cause a partial negative and partial positive force that create a miniscule attraction <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">These occur between all molecules but are the only force between non-polar molecules. <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">These forces are greater in larger molecules, such as in plastics or Kevlar

2.) Dipole-dipole forces <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;"><span style="color: #000000; font-family: arial,helvetica,sans-serif;"> These are the moderate forces, the "handshakes" <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Dipoles attract at opposite ends, causing a stronger force than London forces <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Greater the polarity of the molecule, the greater the polarity of the dipole-dipole force.

3.) Hydrogen Bonds <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">King of kings <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">

<span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Strongest of forces, "embrace" <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive; line-height: 0px; overflow-x: hidden; overflow-y: hidden;"> <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Hydrogen is TINY <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">If tiny H is attached to F, O, or N in a molecule, huge polarities are created. <span style="color: #0e99be; font-family: 'Comic Sans MS',cursive;">Therefore very strong h-bods form between the molecules

Textbook Assignment # 4 Read Section 8.5 Do #’s 74, 75, 76, 114, 118, 119, 120, 121, 127, 128 138-140

Balancing Chemical Equations

You must have an equal number of each type of atom on either side of the equation. The equation must obey the Law of Conservation of Mass.

Use coefficients to balance equations. Never change subscripts!

Techniques

Save H then O till last.

Eliminate fractions or decimals by multiplication.

Example: Magnesium reacts with oxygen gas to form magnesium oxide.

2Mg(s) + O2(g) → 2 MgO(s)

Physical state symbols: gas(g) liquid(l) solid(s) aqueous(aq)

Watch out for Diatomic elements (elements that occur in pairs)

7 total: H2, O2, N2, Cl2, Br2, I2, F2

Honclbrif HONClBrIF

ClIF BrOHN

Magic 7

Ever play Battleship? Try this version: http://www.quia.com/ba/22228.html

Read Section 9.1 Do #’s 1-3 p. 284. 4-6, p. 287, 12, 13p. 288, 62, 64-66, 68, 71-75 p. 312.

Types of Chemical Reactions

Synthesis A + B → AB examples: this is like when two people are meant to be and they join together.

N2 + H2 --> NH3 code is 1: 3 : 2 anitmony + sulfur --> anitmony (V) sulfide should be 2Sb + 5S --> Sb2S5 nitrogen + oxygen --> dinitrogen pentoxide should be 2N2 + 5O2 --> 2N25N2

Decomposition AB → A + B examples:This is like a divorce. When two people dont work out and they fight all the time so they decided it was best for both of them to go their separate ways and never speak again.

2 AL(OH)3 --> AL2O3 + 3H2O 2KClO3 --> KCl + 3O2 NH4NO2 --> N2 + 2H2O

Single Replacement A + BX → AX + B examples: = If there is a couple and someone is awesome enough they can break into the couple and kick one person out. then they will be lonely. out of the couple. Out on the streets. Being homeless. With nothing to eat because they are lonely so they get depressed =

Double Replacement

AX + BY → AY + BX = This is like the tv show wife swap. picture a and b as the husband and x and y as the wives. the wives swap and go with different husbands. but instead of it being temporary it is forever and ever and ever and ever until some chemical epicness can alter the very fabric of the new husband to wife bond!!!!!!! =

= Or for another example it is much like two couples going to the dance together but then leaves with having the girls and guys swap partners. So the guys just like traded girls or vice versa. What happened was jeanie and joey went to the dance by joey was eyeing up latisha and when jeanie went to the bathroom joey decided to dance with latisha and jeanie found them. So to make joey jealous she started dancing with mustafa (latisha's boyfriend). But it turns out that both couples end up marrying and living happy ever after. =

Combustion

CxHy + O2 → CO2 + H20

WATCH HIS AMAZING VIDEO ON YOUTUBE!!!!!!!!!!!!!!! Think you know your stuff?

Try this quiz : http://www.quia.com/quiz/374715.html?AP_rand=120891224

Read Section 9.2 plus pp 299-302 Do #’s 14-17 p. 291, 18-19 p. 292, 21-24, p. 295, 25- 28, p. 297, # 35- 39, p. 302 – Just chemical equations, 80, 81, 82, 85, 86-88, 100, 107, 112, 126, 128, 130, 133 pp 312-315.

The Mole

Atomic Mass and the Mole

Atomic Mass: The average of all naturally occurring isotopes. (Recall Isotopic Calculations)

Ex. 1 atom Na = 22.98977 amu’s

Carbon-12 C – 12 has a mass of exactly 12.000000…. amu’s All other atoms are compared to C-12. In fact 1 amu is defined to be 1/12 of a C- 12 atom.

Avogadro’s Number and the Mole Mole Examples/Jokes 1 mol = 6.02 X 10 23 602,000,000,000,000,000,000,000,000 602 sextillion

Celebrate Mole Day 6:02 am – 6:02 pm 10/23

Textbook Assignment #1 Read Section 10.1 Do #’s 1-4 p. 323, # 12 p. 324, # 92-94, 99 p. 358,

Mole ← → Gram conversions

Examples

1 mol Na atoms = 6.02 x 10 23 atoms 1 mol Na Atoms = 22.98977 grams

1 mol equals an atom’s atomic mass in grams.

Si – 28 27.977 amu’s = 1 atom.

10.0 g --→ moles?

10.0 g x 1 mol/ 27.977 g = 0.357 mols Si x 6.02 x 10 23 atoms/ 1 mol = 2.15 x 10 23 atoms.

A mole is similar to a dozen – For example:

.333 dozen donuts .333 doz x 12 donuts/dozen = 4 donuts

Still confused? Check out this explanation:

http://www.screencast.com/users/mwilliams536/folders/Jing/media/bef3ed5b-9c12-4e1f-847c-547a8a31b046

Textbook Assignment #2 Read Sections 10.2, 10.3 Do #’s 19 a, c, 20 a, c, e, p. 331, #28 p. 332, #’s 43, 46, p. 339, # 103, 104, 108, 109, 112, 115, 117, 118, 128, 131, 132, 135, 136, 145, 148, 150 pp 358-360.

Percent Composition from Formulas

Cinnabar HgS mercury ore

% of Hg in HgS 200.6 g Hg + 32.1 g S = 232.7 g total

200.6g Hg/ 232.7 total g x 100 = 86.2 % 13.8 % S

Milk of Magnesia Mg(OH)2

% of Mg in Mg (OH)2

24.3 g Mg % Mg = 24.3g Mg/58.3 total g x 100 = 41.7 % Mg 32.0 g O 2.0 g H total = 58.3 g

Simplest Formula from Chemical Analysis

Hydrate example

Na2CrO4. X H2O is experimentally determined to contain 32. 1 % water. Find X.

X = mols H2O/mols Na2CrO4

Assume 100 g of hydrate

32.1 g H2O/ 18.0 g/mol = 1.78 mols

67.9 g Na2CrO4/ 162 g/mol = .419 mols

X= 1.78 mols/.419 mols = 4.25 ⇒ 4 = X=4

Molecular vs Empirical formulas

A molecular compound contains 92.3% carbon and 7.7% hydrogen by mass.

a.) Find its empirical(simplest) formula. The simplest whole # ratio of atoms in a compound.

Assume 100g of compound

92.3 g C/12.0 g/mol = 7.69 mols C

7.7 g H/1.0 g/mol = 7.7 mols H

7.7:7.69 ⇒ 1:1 So emp. Formula is CH

b.) If 0.050 mol of this compound has a mass of 3.90 g, what is its molecular formula?

Emp. Formula is CH Molecular formula could be CH,C2H2,C3H3,C4H4 etc….

Molar mass = 3.90g/.050mol = 78 g/mol

CH???? = 78 g/mol Noooo!!!! It equals 13 g/mol C2H2 ???? = 78 g/mol Noooo!!!! It equals 26 g/mol

Divide 78 by 13 78/13 = 6 so the molecular formula is C6H6 yessss!!!!

Textbook Assignment # 3 Read Sections 10.4, 10.5 Do #’s 68, 69, 73 p. 350, #’s 159, 161, 64, 166, 172, 173, 173, 175, 179, 180, 181, 185, 187, 194, 196, 204, 105, 211 pp 361-363.

Online Quizzes

http://chemunder.chemistry.ohio-state.edu/under/chemed/qbank/quiz/bank2.htm

Try a few on empirical formula, % composition, Avogadro’s number and the mole.

We don't count normally, we count by weighing things.

Carbon is the standard because it is the basis of life. C-12 was put as exactly 12.0000000000000000...amu's and everything is based off of this standard.

10/23 is mole day because mole is 10 to the 23 power. A mole is a very very very large number. A mole of water is equal 18 g.

A link to the mole song!

> Example: 25 grams of NaCl > ? mol's
 * 1)   [|www.youtube.com/watch?v=bjewZs_oAvA]

Na -> 1x 23.0 = 23.0 grams + Cl --> 1x 35.5 = 35.5 grams = 58.5 grams

25.0 grams NaCl= 1 mol\58.5 grams = .428 mol NaCl

Example: 1 mol H2SO4 - 6.02x10^23 molecules - ? grams

2 H's= 2x1.01 grams = 2.02 grams + 1 S= 1x32.1 grams= 32.1 grams + 4 O's= 4x 16.0 grams = 64.0 grams = 98.12 grams\2 = 49.06 grams

Cinnabar Hgs Mercury Ore. - When burned, Cinnabar gives off a sulfur smell (Think of Hades).

<span style="color: #0073ff; font-family: 'Comic Sans MS',cursive; font-size: 180%;">Yay Moles!!!

<span style="color: #e700ff; font-family: Georgia,serif; font-size: 16px; line-height: 23px;">"Molanize It!!!"- Alyssa 'Eary' Ott

__"Molecular Formulas" "Simplified Formulas (Empivical)__

C6H12O6 --> CH2 Ratios= 6:12:6

H2O2 -> HO Ratio= 2:2

H2O > H2O Ratio= 2:1

NaCl Ratio= 1:1 -> NaCl

C4H10 --> C2H5 Ratio= 4:10

__ Reaction Stoichiometry __ Using Balanced Equations to Make Predictions =**__Mol-mol relationships__**=

one step!!
1. convert to mols. Example: View the video found here: [|mol to mol conversion]

=**__Mol-mass relationships__**=

two steps!!
1. convert to mols. 2. find the relationship. Example: View the video found here: [|mass to mols]

=**__Mass-mass relationships__**=

three steps!!!
1. convert to mols. 2. find the relationship. 3. convert back to grams. Example: View the video found here: [|Mass to mass calculation]

Textbook Assignment # 1 Read Section 11.1-11.2, Do #2 p. 371; #9, p. 372; # 12 p. 375; # 14 p. 376; # 16 p. 377; # 21, 22 p. 378; # 50, 51, 53, 59, 60, 62, 64, 66, 69, 70 pp 392-394.


 * __Limiting Reactants and Theoretical Yield/% Yield__**

Support : Go to the following website for examples and explanations: [|Limiting and Excess Reagents]

Example : View the video found here: [|Limiting reagent. Finding theoretical yield and the dreaded amount leftover!]

Quizzes : Try these on for size: [|Matching quiz to see if you know the terminology.]

[|Multiple Choice]

Extra Quizzes: [|Try the following here: Stoichiometry - Mole to Mole Problems, Mole-mass Stoichiometry Problems, Mass-mass Stochiometry Problems, Limiting Reagent, Percent Yield, Percent Yield with Limiting Reagents]

Textbook assignment # 2 Read section 11.3-11.4 Do #’s 23, 24 p. 383; # 27 p. 384; # 34, 35 p. 388; # 75, 77, 79, 81, 89, 90, 94, 103, 109, 110, 111a, c, 113 pp 394-397.

GASES

Gas

Check out the animation: Gases under pressure.

How is a gas different from a solid or liquid? List 5 characteristics of gases. Mostly non-polar molecules. Gases can diffuse. Can't "feel" it-maybe can smell or see. Low density Shapeless but they occupy the volume given to them. Particles are in constant, random, chaotic, motion. Gases are compressable, but liquids are not.

Check out this video: ⇒

Measurements of Gases

Pressure(P)

14.7 lbs/in^2(psi)=101.3 KPa(Kilopascals)=1 atmosphere(atm)=1.013 bars=760 mmHg (Torr)

Volume(V) Usually in Liters

Amount(n)= # of mols

Temperature(T) A lways in Kelvin (K). K= ºC + 273.15

Kinetic Theory K.E.= 1/2mass(velocity)2 - at any given temperature, all gases have the same K.E. on average
 * when dealing with ideal gases

helium= 4 g/mol vs. xenon= 131 g/mol air= 29 g/mol -heavy gases move slowly while light gases move faster because since kinetic energy equals half of the mass times the velocity squared and the mass of xenon is greater, xenon has a lower velocity, moving faster. - if you fill a balloon with helium, it floats while a xenon filled ballon would sink - the next morning, your helium balloon shrinks because on the inside of the ballon, the faster moving helium escapes through the pores of the balloon. An exchange occurs but since the helium moves so fast, no air can enter causing it to shrink -the next morning, your xenon ballon grows because on the outside of the balloon, the faster moving air (xenon moves slow because it has a high mass) exchanges within the pores and the air enters into the ballon, not allowing any xenon to exit. -volume of gas particles is negligible (quantities so small that they can be ignored when studying the larger effect) for "ideal" gases -gas particles have no attractive forces for "ideal" gases -if you compress a gas into a small enough space, the gas turns into a liquid/solid -if you shake a volume of gas particles, they would never stop, just keep moving Tenets p 403
 * doesn't work under high pressure
 * not entirely true




 * Xenon Helium**

Dalton’s Law of Partial Pressures

Ptot = P1 + P2 + P3 +….. Or PA = XA x Ptot Where XA = the mol fraction of A

PN2+PO2+PCO2+PXe+...= 740 Tom -when you add up all the pressure of the gases in a volume, it equals the total pressure P1=X1*total - if you want to find the pressure of one gas, take the total pressure times mole fraction
 * mole fraction is mols of unknown gas/total moles of gases

Subtracting vapor pressure of water when finding the pressure of a gas collected over water.

Textbook Assignment #1 Read Section 12.1 Do #’s 4, 5, 7 p. 409, # 39, 45, 47, 49, 50 p. 434.

THE IDEAL GAS LAWS Boyle’s Law:

P1V1 = P2V2

Sketch graph

Charles Law:

V1/T1 = V2/T2

Sketch graph:

Avogadro’s Law

V1/n1 = V2/n2

Sketch graph:

Gay- Lussac’s Law

P1/T1 = P2/T2

Sketch graph

The Combined gas law and the value for “R” for an ideal gas.

Textbook Assignment # 2 Read Section 13.1 Do #’s 1, 2, 3 p. 443, 4, 6 p. 446, 8, 10 p. 448, 11, 12, 13 p. 450, # 18 p. 451, # 55, 57, 58, 60 p. 468.

IDEAL GAS LAW

PV = nRT One variable calculations.

Using Ideal gas law to find MM and Density.

Textbook Assignment #3: Read Section 13.2 Do #’s 20, 21, 24, 25 p. 453, #’s 26, 28, 30, p. 455, #36 p. 459, # 65, 67, 68, 70, 72, 75, 76, 93, 100 pp 468-470.

Relevant Reading Article on SF6

Demos: Tank of Doom/Flames of Gehenna

Stoichiometry of gaseous reactions

Volume-Volume

Problems can be solved in the same way as mol-mol problems IF temperature and pressure are constant.

Mass – Volume Use molar volume (22.4 L/mol) if the conditions are at STP.

If not use ideal gas law to find n (mols) and then mass (g).

Textbook Assignment # 4: Read Section 13.3 Do #’s 38, 41 p. 461, #’s 42, 44, 45 p. 463, # 82, 84, 87, 89, 90, 103, 108, 110 b, d, f, 112, pp 469-471