I disagree with all your opinions.

[Magic_Marker]

Let me explain why you are wrong.

You post an idea you have. I'll explain why you are a sack of shit.

Socialism? Good in THEORY, Smarty, but it leads to evil.

Libertarianism? You want the poor to die!? Go back to studying Solid Snake!

Gay Rights? More like Gay Right, amiright, Noncon?

Cynicism? Try looking at the bright side of life, Fifthfiend.

The answer is all of you

[Seil]

I don't think this thread is a good idea.

[Flarecobra]

I am of the opinion that you are awesome there Magic Marker.

[Magic_Marker]

I don't think this thread is a good idea.

I'll keep that in mind. I wouldn't want this to become a Seil thread.

[Magic_Marker]

I am of the opinion that you are awesome there Magic Marker.

Have you seen how many neurosis I have!? I'm petulant. I have issues with not having enough money. For god's sake Seil just accused me of making a terrible thread.

You have terrible tastes in role models. One wonders if you are going to medical shcool in order to emulate House.

Or Worse. JD.

[Aldurin]

Freedom to be stupid.

[Magic_Marker]

Freedom to be stupid.

This man is the only one who matters.

People, take notes.

[Loyal]

This man is the only one who matters.

People, take notes.

You have the worst opinion ever.

[Tev]

I am of the opinion that it was a great idea for Lev to get his name changed.

[Magic_Marker]

I am of the opinion that it was a great idea for Lev to get his name changed.

Tevosaur? Really? You two have a choice of who to change their name and you didn't jump at the chance to be a dinosaur?

Weak Sauce, man. Weak Sauce.

[Aldurin]

You have the worst opinions ever, and some after that which are so bad they can't exist in our reality.

[Premmy]

I'm the best.

EVER!

[krogothwolf]

Magic Marker does not have homophobia and is not racists, he also doesn't kick babies off of cliffs.

[Krylo]

You know, all of these, "My opinion is that you are awesome" jokes kind of remind me of something...

It's almost as if... yes... yes I think I'm experiencing Deja Vu (http://www.nuklearforums.com/showthread.php?t=38457).

[Premmy]

I just want to see what horrible fabrications someone would need to make to disagree with me being the best.

[Thadius]

Ah yes, this sort of thread. I'm of the opinion it will fail.

[Torque]

The funny thing is... He disagrees with all of our opinions... Yet that does not, in and of itself, mean that our opinions are wrong, or that his are right.
In fact, I posit that this very thread indicates that his opinions, as contrary as they are, are false.

[Loyal]

You know, all of these, "My opinion is that you are awesome" jokes kind of remind me of something...

It's almost as if... yes... yes I think I'm experiencing Deja Vu (http://www.nuklearforums.com/showthread.php?t=38457).I thought this thread looked familiar. Man, has it been four months already?

[Magic_Marker]

WELL EXCUSE ME FOR TRYING TO MAKE A GOOD THREAD. i SLAVE ALL DAY AND NIGHT AND THIS IS THAT THANKS GET?

YOU KNOW YOUR BROTHER NEVER TREATED HIS MOTHER LIKE THIS.

[Torque]

WELL EXCUSE ME FOR TRYING TO MAKE A GOOD THREAD.

Try harder.


i SLAVE ALL DAY AND NIGHT AND THIS IS THAT THANKS GET?


Make me a sandwich, and maybe I'll thank you.


YOU KNOW YOUR BROTHER NEVER TREATED HIS MOTHER LIKE THIS.

Incest is a bitch.

[Magic_Marker]

Magic Marker does not have homophobia and is not racists, he also doesn't kick babies off of cliffs.


Gay Rights? More like Gay Right, amiright, Noncon?

The offense rests.

[mauve]

The representation of disabled and/or physically disfigured persons in mainstream American fims, dating from the birth of the medium to the present, largely adheres to an unspoken yet widely accepted semiotic language of stereotypes to convey nonverbal messages about characters or present ideals to the viewer. This "language" remains largely unchanged through time, (ex: the bitter amputee, the sweet and pure blind young girl and the wise and almost otherworldly blind elderly woman, the morally corrupt hunchback, etc) with variations only occurring in incidences where the disablity is meant to represent an ideal or concept relevant to a social/political shift in the culture of the audience for which the film was originally intended (The Best Years of our Lives versus films made around the time of the Vietnam War, for example.)

Interestingly, while various other stereotypes dating back to the dawn of film have been deemed politically incorrect and even downright insulting over time, nearly all of those relating to the disabled and disfigured are still widely accepted in mainstream media today. Even Disney uses them, largely in their characterization of villains.

[Fifthfiend]

I HEAR SOMEONE POSTED A THREAD ROUN' YONDER

RUSTLE UP A POSSE KID, WE RIDIN' TONIGHT

[Fifthfiend]

FARTZULATOOOOOOOOOOORS

mount up

[POS Industries]

Nah.

S'all good.

[Wigmund]

I'm trying to care what Magic Marker thinks,
but then I remember that he's from Oklahoma.

[Shyria Dracnoir]

RAAAAAAAAAAHG!! RAAGH RRAAAA GGHRRRR RAAAAAAWWWWRR!

[Seil]

This is a pretty skookum Christmas flick. (http://www.youtube.com/watch?v=cYCkFTyADJ0)

[synkr0nized]

Matter – “stuff”; anything that has the properties of inertia | Theory – explanation of phenomenon | nylon – synthetic; developed by Wallace H. Carothers; modeled after silk | Inertia – resistance to any change in motion | Energy – property possessed by all matter. Can be made to do work | Potential Energy – depends upon the position of the object with respect to a reference point; energy available to do work | Kinetic Energy – Energy possessed by an object due to its motion | Energy Transfer - *Direct contact – collision of two swords or two billiard balls (kinetic, also) *Electromagnetic – sun to earth (often called radiant energy) | Law of Conservation of Mass – Mass is always conserved – cannot be created or destroyed, but can change forms (total amount is equal) | Law of Conservation of Energy – Total amount of energy stays the same, but it can change form; cannot be created or destroyed | Einstein developed E=mc2 (energy is interchangeable with matter) -> Law of Conservation of Mass-Energy – Sum of mass and energy is conserved; they can change form, but the sum is still the same | Raw Materials – elements, etc; in nature | Intermediates – from raw, a step in the process towards consumer products | Penicillin – kills bacteria; discovered by Alex Fleming | Chemistry – the study of the properties and structures of matter | Kinetic Energy(motion) – Mechanical (rain, gears turning); Sound (travels on/in waves – medium); Heat molecules/particles moving | Potential Energy – Chemical energy (food); stored energy (book on a table, water held by a dam); Electrical energy | Radiant Energy – travels by electromagnetic waves – light, EMR, radio waves, x-rays
Quantitatively – Describing via properties and using the # of the standard units | Qualitatively – description based on appearance, without measurements | See Conversion Card | SI – Le System International d’Unites | Weight (lb.) – force of gravity between two objects; changes from place to place | Mass (kg) – quantity of matter; doesn’t change Balance – instrument used to determine mass by comparing to known masses | Length (m) – use a ruler; distance covered by a straight line segment connecting 2 points | Time(s) – interval between 2 occurrences | Temp. (Kelvin) – avg. kinetic energy of the particles of object; thermometer; Kelvin is standard, but Celsius is the more common version | Accuracy – how close measurements are to the true value | Precision – how close a set of measurements are to each other | % error – Absolute value (your value – actual value) divided by (actual value); all multiplied by 100(%) | Significant Digits – same # off them as in the data with the least amount of S.D.; *all non-zero digits *zeroes between non-zeroes count *Zeroes used only as place holders do not count *zeroes to the right of the decimal point can count EXAMPLES *361(3) *360(2) *100.5(4) *24009(5) *0.0001(1) *100.0(4) *3.0002(5) | Derived Units – Combinations of SI base units (Area, density, volume) | Density – D=m/v; M=dv; V=m/d
Material – specific kind of matter (wood, or sodium) | Mixtures – two or more materials | phase – region in material with uniform set of proportions | Heterogeneous mixture – more than one phase, meeting at boundaries called interfaces | homogeneous mixture – 1 phase | Solution – mixture with only 1 phase (solute in a solvent) | Solute – dissolved material in a solvent, the dissolving material | Substances – homog. materials with the same substance | Compounds – substances of more than one atom type | elements – substances of only one atom type | Organic Compounds – those containing the element Carbon; inorganic ones do not | Physical change – same substance remains after change 9pounding, cutting, pulling), also melting, boiling (changes of state) | Chemical Change – new substance(s) appear – usually indicated by a precipitate, gas, color, or energy change (burning, digestion, fermentation) | Extensive – depend on the amount of matter present | Intensive – do not (both are physical change properties) | Fractional Crystallization – separation of substances with different solubility | Calorimeter – device used to measure energy changes | q=m?tc (heat gained/lost)=(mass g)(change in temp.)(specific heat of substance); q=(“n”g)(“x” ?C)(“y” J/g?C) – q=”nxy” J (Joules) | Physical Property – behavior while undergoing physical change | Chemical Property – behavior while undergoing a chemical change | Endothermic – energy absorbed in a reaction; energy given off in a reaction is exothermic | Specific heat – the heat needed to raise the temp. of 1g of a substance up one ?C
Compounds – ionic = composed of ions (metal + nonmetal = order of formula); NaCl – sodium chloride; binary(covalent) = use Greek prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-) | Chemical Symbol – represents element’s 1st, or 2nd, or both, letters(1st is capitalized) | Formula – 2 or more symbols + subscript (eg: CaCo, NaCl, Mg(OH)2 | Ion – charged atom, either (+) or (-) because of a loss or gain of electrons, respectively | Molecular Formula – exact # of atoms in the molecule, and the type (using atomic symbols); Benzyne = C6H6, ethyne = C2H2 | Empirical – lowest ratio of atoms in a molecular formula – both the previous examples there are CH in empirical form (+)anion (-)cation
Scientific Notation – # btwn 1-10, multiplied by 10 to a power (n * 10p), the “n” uses the Significant Digits | Molecular Mass – atomic masses of all atoms added together | Formula mass – the mass of ions in a compound | Hydrates – specific ratios of water 9in moles) to compound – CuSO4 • 5H2O means 5 moles of water for each mole of CuSO4, Copper (II) Sulfate pentahydrate | % Composition – (part mass)(whole mass) x 100(%) | Empirical Formula – if you have the % composition – in a 100g sample, n% will be ng; use these grams to find how many moles there would be; divide by the smallest number of moles; ratios must be in whole numbers | Avogadro – 6.022 x 1023 = 1 mole of “particles”; 1 mole of a molecule = moles of atoms added together [NaCl (1 mole of molecule) = 1 mole Na and 1 mole Cl (atoms)]; Amu on Periodic table – convert into grams to get 1 mole of atom
Stoichiometry – study of mass relationships in chem. Equations – to figure out how much X came from 2.5g of Y in the reaction, take #moles of X and Y in the equation to get the molar masses(“n” moles * “z” amu = molar mass total); then go (2.5g Y)*(“nz” X) all divided by (“nz” Y). to get the answer in grams. | Chemical Reactions - reactant + reactant + etc.. ? products; balance the sides left and right in lowest possible ratios; change only the coefficients, not the subscripts | Types of Reactions – Single replacement (Cl2 + 2kBr ? 2KCl + Br2), Double replacement (NaCl + AgNO3 ? AgCl + NaNO3), Synthesis (2H2 + O2 ? 2H2O), Decomposition (CaCO3 ? CaO + CO2), Combustion (C5H12 + 8O2 ? 5CO2 + 6H2O) | % yield – (actual amount of product / theoretical amount of product [from stoichiometry] ) x 100(%)
Democritus – 400 BC; proposed existence of tiny particles, atoms Laviosier – French, experiments w/ closed reactions showed that matter can be changed in form but not created or destroyed Proust – French (both 1700s); concluded that substances contain elements in exact rations (to the mass) Dalton – Atomic Theory (1. Matter = atoms, invisible and indestructible 2. All atoms of the same element are =; different elements have different atoms 3. Compounds = atoms in ratios of small whole numbers); atoms combine in mass ratios to make compounds; ratios of mass combine with constant masses and can be expressed in small, whole numbers (law of mass proportions) Gay-Lussac – 1800; gas reactions under constant temp. and pressure contain these ratios Avogadro - = volumes gases under = conditions, have = molecules Thomson – 1897; worked w/ Cathode ray tubes; rays made of electrons; cookie dough or plum pudding model of atoms Bacquerel – 1897; radioactivity, the spontaneous emission of energy without light Faraday – 1840; studied electricity; coined the terms cation, anion, electrode, cathode, anode Crookes – 1879; Crookes’s tube – glowing ray = cathode ray Millikan- 1900s; used Thomson’s data to find mass of electron; oil drop experiment finds charge of electron Rutherford – 1912-1913, alpha and beta particles; radiation and the gold foil experiment Niels Bohr – “planetary model” of the atom; calculated energy differences btwn orbitals/levels. Energy (light) ? 1/?, where ?=wavelength | Proton = +1, 1 amu, 1.6726x10-24g, nucleus; Neutron = 0, 1amu, 1.6749x10-24g, nucleus; Electron = -1, 0 amu, 9.109x10-28g, shell/cloud

[POS Industries]

Oh come on, let him have his fun. Ain't hurtin' nobody.

[Kim]

My opinion is that Bleach is awful.

[Seil]

I call spam on Synk!

[Fifthfiend]

Matter – “stuff”; anything that has the properties of inertia | Theory – explanation of phenomenon | nylon – synthetic; developed by Wallace H. Carothers; modeled after silk | Inertia – resistance to any change in motion | Energy – property possessed by all matter. Can be made to do work | Potential Energy – depends upon the position of the object with respect to a reference point; energy available to do work | Kinetic Energy – Energy possessed by an object due to its motion | Energy Transfer - *Direct contact – collision of two swords or two billiard balls (kinetic, also) *Electromagnetic – sun to earth (often called radiant energy) | Law of Conservation of Mass – Mass is always conserved – cannot be created or destroyed, but can change forms (total amount is equal) | Law of Conservation of Energy – Total amount of energy stays the same, but it can change form; cannot be created or destroyed | Einstein developed E=mc2 (energy is interchangeable with matter) -> Law of Conservation of Mass-Energy – Sum of mass and energy is conserved; they can change form, but the sum is still the same | Raw Materials – elements, etc; in nature | Intermediates – from raw, a step in the process towards consumer products | Penicillin – kills bacteria; discovered by Alex Fleming | Chemistry – the study of the properties and structures of matter | Kinetic Energy(motion) – Mechanical (rain, gears turning); Sound (travels on/in waves – medium); Heat molecules/particles moving | Potential Energy – Chemical energy (food); stored energy (book on a table, water held by a dam); Electrical energy | Radiant Energy – travels by electromagnetic waves – light, EMR, radio waves, x-rays
Quantitatively – Describing via properties and using the # of the standard units | Qualitatively – description based on appearance, without measurements | See Conversion Card | SI – Le System International d’Unites | Weight (lb.) – force of gravity between two objects; changes from place to place | Mass (kg) – quantity of matter; doesn’t change Balance – instrument used to determine mass by comparing to known masses | Length (m) – use a ruler; distance covered by a straight line segment connecting 2 points | Time(s) – interval between 2 occurrences | Temp. (Kelvin) – avg. kinetic energy of the particles of object; thermometer; Kelvin is standard, but Celsius is the more common version | Accuracy – how close measurements are to the true value | Precision – how close a set of measurements are to each other | % error – Absolute value (your value – actual value) divided by (actual value); all multiplied by 100(%) | Significant Digits – same # off them as in the data with the least amount of S.D.; *all non-zero digits *zeroes between non-zeroes count *Zeroes used only as place holders do not count *zeroes to the right of the decimal point can count EXAMPLES *361(3) *360(2) *100.5(4) *24009(5) *0.0001(1) *100.0(4) *3.0002(5) | Derived Units – Combinations of SI base units (Area, density, volume) | Density – D=m/v; M=dv; V=m/d
Material – specific kind of matter (wood, or sodium) | Mixtures – two or more materials | phase – region in material with uniform set of proportions | Heterogeneous mixture – more than one phase, meeting at boundaries called interfaces | homogeneous mixture – 1 phase | Solution – mixture with only 1 phase (solute in a solvent) | Solute – dissolved material in a solvent, the dissolving material | Substances – homog. materials with the same substance | Compounds – substances of more than one atom type | elements – substances of only one atom type | Organic Compounds – those containing the element Carbon; inorganic ones do not | Physical change – same substance remains after change 9pounding, cutting, pulling), also melting, boiling (changes of state) | Chemical Change – new substance(s) appear – usually indicated by a precipitate, gas, color, or energy change (burning, digestion, fermentation) | Extensive – depend on the amount of matter present | Intensive – do not (both are physical change properties) | Fractional Crystallization – separation of substances with different solubility | Calorimeter – device used to measure energy changes | q=m?tc (heat gained/lost)=(mass g)(change in temp.)(specific heat of substance); q=(“n”g)(“x” ?C)(“y” J/g?C) – q=”nxy” J (Joules) | Physical Property – behavior while undergoing physical change | Chemical Property – behavior while undergoing a chemical change | Endothermic – energy absorbed in a reaction; energy given off in a reaction is exothermic | Specific heat – the heat needed to raise the temp. of 1g of a substance up one ?C
Compounds – ionic = composed of ions (metal + nonmetal = order of formula); NaCl – sodium chloride; binary(covalent) = use Greek prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-) | Chemical Symbol – represents element’s 1st, or 2nd, or both, letters(1st is capitalized) | Formula – 2 or more symbols + subscript (eg: CaCo, NaCl, Mg(OH)2 | Ion – charged atom, either (+) or (-) because of a loss or gain of electrons, respectively | Molecular Formula – exact # of atoms in the molecule, and the type (using atomic symbols); Benzyne = C6H6, ethyne = C2H2 | Empirical – lowest ratio of atoms in a molecular formula – both the previous examples there are CH in empirical form (+)anion (-)cation
Scientific Notation – # btwn 1-10, multiplied by 10 to a power (n * 10p), the “n” uses the Significant Digits | Molecular Mass – atomic masses of all atoms added together | Formula mass – the mass of ions in a compound | Hydrates – specific ratios of water 9in moles) to compound – CuSO4 • 5H2O means 5 moles of water for each mole of CuSO4, Copper (II) Sulfate pentahydrate | % Composition – (part mass)(whole mass) x 100(%) | Empirical Formula – if you have the % composition – in a 100g sample, n% will be ng; use these grams to find how many moles there would be; divide by the smallest number of moles; ratios must be in whole numbers | Avogadro – 6.022 x 1023 = 1 mole of “particles”; 1 mole of a molecule = moles of atoms added together [NaCl (1 mole of molecule) = 1 mole Na and 1 mole Cl (atoms)]; Amu on Periodic table – convert into grams to get 1 mole of atom
Stoichiometry – study of mass relationships in chem. Equations – to figure out how much X came from 2.5g of Y in the reaction, take #moles of X and Y in the equation to get the molar masses(“n” moles * “z” amu = molar mass total); then go (2.5g Y)*(“nz” X) all divided by (“nz” Y). to get the answer in grams. | Chemical Reactions - reactant + reactant + etc.. ? products; balance the sides left and right in lowest possible ratios; change only the coefficients, not the subscripts | Types of Reactions – Single replacement (Cl2 + 2kBr ? 2KCl + Br2), Double replacement (NaCl + AgNO3 ? AgCl + NaNO3), Synthesis (2H2 + O2 ? 2H2O), Decomposition (CaCO3 ? CaO + CO2), Combustion (C5H12 + 8O2 ? 5CO2 + 6H2O) | % yield – (actual amount of product / theoretical amount of product [from stoichiometry] ) x 100(%)
Democritus – 400 BC; proposed existence of tiny particles, atoms Laviosier – French, experiments w/ closed reactions showed that matter can be changed in form but not created or destroyed Proust – French (both 1700s); concluded that substances contain elements in exact rations (to the mass) Dalton – Atomic Theory (1. Matter = atoms, invisible and indestructible 2. All atoms of the same element are =; different elements have different atoms 3. Compounds = atoms in ratios of small whole numbers); atoms combine in mass ratios to make compounds; ratios of mass combine with constant masses and can be expressed in small, whole numbers (law of mass proportions) Gay-Lussac – 1800; gas reactions under constant temp. and pressure contain these ratios Avogadro - = volumes gases under = conditions, have = molecules Thomson – 1897; worked w/ Cathode ray tubes; rays made of electrons; cookie dough or plum pudding model of atoms Bacquerel – 1897; radioactivity, the spontaneous emission of energy without light Faraday – 1840; studied electricity; coined the terms cation, anion, electrode, cathode, anode Crookes – 1879; Crookes’s tube – glowing ray = cathode ray Millikan- 1900s; used Thomson’s data to find mass of electron; oil drop experiment finds charge of electron Rutherford – 1912-1913, alpha and beta particles; radiation and the gold foil experiment Niels Bohr – “planetary model” of the atom; calculated energy differences btwn orbitals/levels. Energy (light) ? 1/?, where ?=wavelength | Proton = +1, 1 amu, 1.6726x10-24g, nucleus; Neutron = 0, 1amu, 1.6749x10-24g, nucleus; Electron = -1, 0 amu, 9.109x10-28g, shell/cloud

http://cdn.anyhub.net/thebest404pageever/swf/snap_your_shit.swf

[synkr0nized]

By the way those are all facts.


e: @POS: I don't recall stopping anything. Crayola_Crayons is free to continue pullin' out the opposite day posts.

[Token]

Matter – “stuff”; anything that has the properties of inertia | Theory – explanation of phenomenon | nylon – synthetic; developed by Wallace H. Carothers; modeled after silk | Inertia – resistance to any change in motion | Energy – property possessed by all matter. Can be made to do work | Potential Energy – depends upon the position of the object with respect to a reference point; energy available to do work | Kinetic Energy – Energy possessed by an object due to its motion | Energy Transfer - *Direct contact – collision of two swords or two billiard balls (kinetic, also) *Electromagnetic – sun to earth (often called radiant energy) | Law of Conservation of Mass – Mass is always conserved – cannot be created or destroyed, but can change forms (total amount is equal) | Law of Conservation of Energy – Total amount of energy stays the same, but it can change form; cannot be created or destroyed | Einstein developed E=mc2 (energy is interchangeable with matter) -> Law of Conservation of Mass-Energy – Sum of mass and energy is conserved; they can change form, but the sum is still the same | Raw Materials – elements, etc; in nature | Intermediates – from raw, a step in the process towards consumer products | Penicillin – kills bacteria; discovered by Alex Fleming | Chemistry – the study of the properties and structures of matter | Kinetic Energy(motion) – Mechanical (rain, gears turning); Sound (travels on/in waves – medium); Heat molecules/particles moving | Potential Energy – Chemical energy (food); stored energy (book on a table, water held by a dam); Electrical energy | Radiant Energy – travels by electromagnetic waves – light, EMR, radio waves, x-rays
Quantitatively – Describing via properties and using the # of the standard units | Qualitatively – description based on appearance, without measurements | See Conversion Card | SI – Le System International d’Unites | Weight (lb.) – force of gravity between two objects; changes from place to place | Mass (kg) – quantity of matter; doesn’t change Balance – instrument used to determine mass by comparing to known masses | Length (m) – use a ruler; distance covered by a straight line segment connecting 2 points | Time(s) – interval between 2 occurrences | Temp. (Kelvin) – avg. kinetic energy of the particles of object; thermometer; Kelvin is standard, but Celsius is the more common version | Accuracy – how close measurements are to the true value | Precision – how close a set of measurements are to each other | % error – Absolute value (your value – actual value) divided by (actual value); all multiplied by 100(%) | Significant Digits – same # off them as in the data with the least amount of S.D.; *all non-zero digits *zeroes between non-zeroes count *Zeroes used only as place holders do not count *zeroes to the right of the decimal point can count EXAMPLES *361(3) *360(2) *100.5(4) *24009(5) *0.0001(1) *100.0(4) *3.0002(5) | Derived Units – Combinations of SI base units (Area, density, volume) | Density – D=m/v; M=dv; V=m/d
Material – specific kind of matter (wood, or sodium) | Mixtures – two or more materials | phase – region in material with uniform set of proportions | Heterogeneous mixture – more than one phase, meeting at boundaries called interfaces | homogeneous mixture – 1 phase | Solution – mixture with only 1 phase (solute in a solvent) | Solute – dissolved material in a solvent, the dissolving material | Substances – homog. materials with the same substance | Compounds – substances of more than one atom type | elements – substances of only one atom type | Organic Compounds – those containing the element Carbon; inorganic ones do not | Physical change – same substance remains after change 9pounding, cutting, pulling), also melting, boiling (changes of state) | Chemical Change – new substance(s) appear – usually indicated by a precipitate, gas, color, or energy change (burning, digestion, fermentation) | Extensive – depend on the amount of matter present | Intensive – do not (both are physical change properties) | Fractional Crystallization – separation of substances with different solubility | Calorimeter – device used to measure energy changes | q=m?tc (heat gained/lost)=(mass g)(change in temp.)(specific heat of substance); q=(“n”g)(“x” ?C)(“y” J/g?C) – q=”nxy” J (Joules) | Physical Property – behavior while undergoing physical change | Chemical Property – behavior while undergoing a chemical change | Endothermic – energy absorbed in a reaction; energy given off in a reaction is exothermic | Specific heat – the heat needed to raise the temp. of 1g of a substance up one ?C
Compounds – ionic = composed of ions (metal + nonmetal = order of formula); NaCl – sodium chloride; binary(covalent) = use Greek prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-) | Chemical Symbol – represents element’s 1st, or 2nd, or both, letters(1st is capitalized) | Formula – 2 or more symbols + subscript (eg: CaCo, NaCl, Mg(OH)2 | Ion – charged atom, either (+) or (-) because of a loss or gain of electrons, respectively | Molecular Formula – exact # of atoms in the molecule, and the type (using atomic symbols); Benzyne = C6H6, ethyne = C2H2 | Empirical – lowest ratio of atoms in a molecular formula – both the previous examples there are CH in empirical form (+)anion (-)cation
Scientific Notation – # btwn 1-10, multiplied by 10 to a power (n * 10p), the “n” uses the Significant Digits | Molecular Mass – atomic masses of all atoms added together | Formula mass – the mass of ions in a compound | Hydrates – specific ratios of water 9in moles) to compound – CuSO4 • 5H2O means 5 moles of water for each mole of CuSO4, Copper (II) Sulfate pentahydrate | % Composition – (part mass)(whole mass) x 100(%) | Empirical Formula – if you have the % composition – in a 100g sample, n% will be ng; use these grams to find how many moles there would be; divide by the smallest number of moles; ratios must be in whole numbers | Avogadro – 6.022 x 1023 = 1 mole of “particles”; 1 mole of a molecule = moles of atoms added together [NaCl (1 mole of molecule) = 1 mole Na and 1 mole Cl (atoms)]; Amu on Periodic table – convert into grams to get 1 mole of atom
Stoichiometry – study of mass relationships in chem. Equations – to figure out how much X came from 2.5g of Y in the reaction, take #moles of X and Y in the equation to get the molar masses(“n” moles * “z” amu = molar mass total); then go (2.5g Y)*(“nz” X) all divided by (“nz” Y). to get the answer in grams. | Chemical Reactions - reactant + reactant + etc.. ? products; balance the sides left and right in lowest possible ratios; change only the coefficients, not the subscripts | Types of Reactions – Single replacement (Cl2 + 2kBr ? 2KCl + Br2), Double replacement (NaCl + AgNO3 ? AgCl + NaNO3), Synthesis (2H2 + O2 ? 2H2O), Decomposition (CaCO3 ? CaO + CO2), Combustion (C5H12 + 8O2 ? 5CO2 + 6H2O) | % yield – (actual amount of product / theoretical amount of product [from stoichiometry] ) x 100(%)
Democritus – 400 BC; proposed existence of tiny particles, atoms Laviosier – French, experiments w/ closed reactions showed that matter can be changed in form but not created or destroyed Proust – French (both 1700s); concluded that substances contain elements in exact rations (to the mass) Dalton – Atomic Theory (1. Matter = atoms, invisible and indestructible 2. All atoms of the same element are =; different elements have different atoms 3. Compounds = atoms in ratios of small whole numbers); atoms combine in mass ratios to make compounds; ratios of mass combine with constant masses and can be expressed in small, whole numbers (law of mass proportions) Gay-Lussac – 1800; gas reactions under constant temp. and pressure contain these ratios Avogadro - = volumes gases under = conditions, have = molecules Thomson – 1897; worked w/ Cathode ray tubes; rays made of electrons; cookie dough or plum pudding model of atoms Bacquerel – 1897; radioactivity, the spontaneous emission of energy without light Faraday – 1840; studied electricity; coined the terms cation, anion, electrode, cathode, anode Crookes – 1879; Crookes’s tube – glowing ray = cathode ray Millikan- 1900s; used Thomson’s data to find mass of electron; oil drop experiment finds charge of electron Rutherford – 1912-1913, alpha and beta particles; radiation and the gold foil experiment Niels Bohr – “planetary model” of the atom; calculated energy differences btwn orbitals/levels. Energy (light) ? 1/?, where ?=wavelength | Proton = +1, 1 amu, 1.6726x10-24g, nucleus; Neutron = 0, 1amu, 1.6749x10-24g, nucleus; Electron = -1, 0 amu, 9.109x10-28g, shell/cloud

Tee-hee.

[Seil]

I'm starting to have a problem with people who use the Seil tag in lame total-spam posts.

[Pip Boy]

He makes a fair point. It takes a very specific kind of awesome/terrible thread to earn a Seilthread tag. Its not like we can just go slapping them on any dump some hobo takes. To earn a Seilthread tag we're talking like 5-star high-class dumps taken by the finest hobos imported from foreign lands.

[Professor Smarmiarty]

My opinion is that this thread was better when I did it due to my title aggressively marketing towards the lowest common denominator- ie denizens of this forum and people with bad opinions. Without a targeted emotive pull in the thread title this thread doesn't know what it wants to be, who it wants to aggress.

[Pip Boy]

Pffft, like anyone is going to take marketing advise from Mr. Commie-nomics!

[Professor Smarmiarty]

I'll admit that we went through some misguided attempts at rebranding in the past, particularly in the 40s-70s, a period henceforth known as "Bubble Tuesday", but I can assure you those responsible are no longer with the company- a fresh envigorating team is ready to adapt to meet the adaptable demands of the modern infomatic world.

[Wigmund]

I only used the Seil tag because we don't have an Earl tag.

[Aldurin]

I only used the Seil tag because we don't have an Earl tag.

But this isn't an Earl thread, just a stupid MM ripoff thread of a Smarty thread. We'd need a pretty complex tag for that.

[Magic_Marker]

When you get down to it, is it really worth a tag?

Tags are for threads of gold quality, or at least fools gold. Threads you remember and want to see again. If you go around labeling everything DANGER: Seil Thread, the label looses its meaning.