Energy Levels Change the Color

When you heat an atom, some of its electrons are "excited* to higher energy levels.
When an electron drops from one level to a lower energy level, it emits a quantum of energy.
3
The wavelength (colour) of the light depends on the difference in the two energy levels.
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We can see only those transitions that correspond to a visible wavelength.
In a hydrogen atom, for example, we can see only the transitions from higher levels to n = 2 .

As	Arsenic	Blue
B	Boron	Bright green
Ba	Barium	Pale/Yellow-green
Ca	Calcium	Orange-red
Cu (I)	Copper (I)	Blue
Cu (II)	Copper (II) non-halide	Green
Cu (II)	Copper (II) halide	Blue-green
Fe	Iron	Gold
In	Indium	Blue
K	Potassium	Light purple to red
Li	Lithium	Deep pink to dark red
Mg	Magnesium	Bright white
Mn (II)	Manganese (II)	Yellow-green
Mo	Molybdenum	Yellow-green
Na	Sodium	Bright yellow
P	Phosphorous	Pale blue-green
Pb	Lead	Blue
Rb	Rubidium	Red/Purple-red
Sb	Antimony	Pale green
Se	Selenium	Bright blue
Sr	Strontium	Crimson
Te	Tellurium	Pale green
Tl	Thallium	Bright green
Zn	Zinc	Blue-green to pale green

Absorbency

https://drive.google.com/open?
id=0B6biT3nsiazTaDRxTGx1MW9CdGM



This is our lab activity that we measured absorbency and and transmitted. This lab was long and extensive but overall was very informative. I enjoyed how simply the procedure was and doing stuff on excel.

It's Lit

https://drive.google.com/open?id=0B6biT3nsiazTNkI1UnpsZjBaLW8





https://drive.google.com/open?id= 0B6biT3nsiazTcDBvZnN4YkpIQlE


This is our identifying the mystery metal was probably the best lab we've done so far. It was so fascinating how different metals produce different colors when burned. The colors were pretty as well .  I wish we had more labs like this.

Trend Setters

Density Trends:
The density of an element is the amount of mass it has per unit volume. Normally this is measured in g cm⁻³ and at room temperature. Values are shown relative to osmium, the element with the highest density.

Atomic Radius trends:
The non-bonded atomic radius of an atom is half of the distance between two unbonded atoms of the same element when the electrostatic forces are balanced. Atoms are not well defined spheres so there are many ways of calculating atomic radius. Values are shown relative to francium, the element with the highest atomic radius.

Electronegativity trends:
The electronegativity of an atom is how strongly it attracts electrons towards itself. It depends on the atomic radius and the atomic number of the element. Electronegativity is most commonly measured on the Pauling scale. Values are shown relative to fluorine, the element with the highest electronegativity.

Melting Point Trends:
The melting point of an element is the temperature at which the solid–liquid phase change occurs. Values are shown relative to the sublimation point of carbon, the highest temperature at which any element remains solid.

Ionization Energy trends:
The first ionisation energy of an atom is the minimum energy required to remove an electron from a neutral atom in its ground state. Values are shown relative to helium, the element with the highest first ionisation energy.

Useful Links

Periodic Trends Video

Crash Course on Electron Configuration

A few helpful links on periodic trends and electron configuration to aid in studying. These videos are easy to understand and educational.

Summary of Trends

This is the summary of periodic trends.Any atom or group of atoms with a net charge  is called an ion. A positively charged ion is a cation while a negatively charged ion is an anion. Now we are ready to discuss the periodic trends of atomic size, ionization energy, electron affinity, and electronegativity

Think Pink

https://drive.google.com/open?id=0B6biT3nsiazTdy1xQzNaWGFVS0E



This is an image of the titrated solution when too much base is added. There is a fine line from the time you add the perfect amount of solution to one drop extra that makes a bright pink color. In order to get the perfect amount it takes trial and error.

Acid

Must See Video of Titration Lab
Above is a link of our titration lab. You can see the acid solution change colors as the base is added.it took careful concentration to avoid getting the solution too pink so the slower the better.

Titration

The word titration rhymes with tight nation. The medical use of this word is a little different, but in chemistry titration refers to a commonly used method of finding the concentration of an unknown liquid, by comparing it with a known liquid. An acid-base titration is good to consider when learning the method, but there are more uses for the technique. The measure of oxalate ion using potassium permanganate in a warm acid environment is a good example of a redox titration. The Mohr titration is a determination of chloride concentration using known silver nitrate solution and sodium dichromate an indicator.

Acid or Base Buffers

A buffer is a solution that resists changes in pH. A buffer is made with a weak acid and a soluble salt containing the conjugate base of the weak acid or a weak base and a soluble salt containing the conjugate acid of the weak base. Some examples of buffer material pairs are:

acetic acid and sodium acetate, H(C₂H₃O₂) and Na(C₂H₃O₂)
hydrofluoric acid and potassium fluoride, HF and KF
carbonic acid and sodium bicarbonate, H₂CO₃ and NaHCO₃
ammonium hydroxide and ammonium nitrate, NH₄OH and NH₄NO₃
nitrous acid and lithium nitrite, HNO₂ and LiNO₂

Weak Acid and Bases

Weak acids and bases do not ionize very much, so the [H⁺] or [(OH)^-] must be calculated by the equilibrium expression.

This would be easy to know exactly, except that the [HA] is not always equal to the concentration of solute that actually went into the solution. The more accurate way to express the equilibrium expression would be to include in the denominator the idea that the [HA] is really the concentration of solute originally put into solution minus the amount of that solute that ionized. We could represent the amount that ionized by either the [A^-] or the [H⁺], so the denominator should be either [HA] - [A^-] or [HA] - [H⁺]. Let's use the second option for alternative denominator because we want to solve for the hydrogen ion concentration. By the 5% rule, [HA] = [HA] - [H⁺] only if the hydrogen ion concentration is less than five percent of the total solute concentration. This is the case for most weak acids. The only exceptions are when the strongest of the weak acids are in the most dilute solutions.

Acid/Bases

 An acid is a material that can release a proton or hydrogen ion. Hydrogen chloride in water solution ionizes and becomes hydrogen ions and chloride ions. a base, or alkali, is a material that can donate a hydroxide ion. Sodium hydroxide in water solution becomes sodium ions and hydroxide ions. Every ion dissociation that involves a hydrogen or hydroxide ion could be considered an acid- base reaction. Acids are electron pair acceptors and bases are electron pair donors.  Each ionizable pair has a proton donor and a proton acceptor. Acids are paired with bases. One can accept a proton and the other can donate a proton. Each acid has a proton available and another part, called the conjugate base. When the acid ionizes, the hydrogen ion is the acid and the rest of the original acid is the conjugate base.

Solutions

http://study.com/academy/lesson/aqueous-solution-definition-reaction-example.html#lesson

Above is a very helpful video that explains examples of aqueous solutions. The definition is provided and it really dumbs down the lesson plan to where its easily interpreted by anyone.