Blog Post 4

Blog Post 4 (Unit 4)

1. Describe Schrodinger and Heisenberg models of the atom.
Schrodinger proposed that electrons were placed in wrapping waves around the atomic structures.That they were in fact, part of these waves, rather than individual, minuscule particles placed around the nucleus.  

Heisenberg combined the atomic models of Schrodinger and one other atomic scientist. Discovering that the electrons were placed in orbiting rings as Schrodinger thought, but that there were, in fact, small particles within them, that were actually called electrons.  


1. Describe light in terms of frequency, wavelength, and energy. (Include all 7 types of waves).
Light is produced in 7 different types of electromagnetic activity. The first, slowest, lowest frequency and longest wavelength is the radio wave. These are typically used for televisions, and other short distance electronic endeavors. Next, is the microwave. These are slightly smaller, and higher in frequency than the radio waves. These are used for, you guessed it, microwaves, as well as speed cameras. Infrared light has an even smaller wavelength, and are placed immediately next to visible light waves. 


1. What are the photoelectric effect and emission spectra? (It’s the rainbow poster in my room. You may look up this information).
If a light, with a high enough intensity, is shown onto a piece of metal, electrons will be emitted from the metal itself. The energy with which the electron is removed from the substance will depend on the energy of the light. Meaning, the higher the energy within the light is, the electron will be ejected more forcefully. 


1. Write the electron configuration for Antimony.
Atomic number: 51
Number of Protons: 51
Number of Neutrons: 71
Number of Electrons: 51
Electron Configuration: 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4d⁶, 5s², 4d¹⁰, 5p³


1. Write the noble gas configuration for Antimony.





(source) Krypton information myinterestingfacts.com




[Kr] 5s², 4d¹⁰, 4f³ 


1. Draw the orbital diagram (once again, yes draw this one, not find an image on Google).

Antimony (Sb) Block electron diagram drawing.

Antimony (Sb) Orbital diagram drawing.


1. Honors Chem: What are the quantum numbers for antimony? Describe what n, l, m, and s represent.  
n = 5 
l = 1
m = 1
s = +1/2 

n - Represents the energy level placement within the periodic table. 

l - Represents the shape of which the electron creates with its orbital rotation. 

m - represents the order the electrons are placed in with relation to one another within the orbitals. 

s - Represents the either negative, (backward) or positive, (forwards) spin of the electrons. 


1. Describe how you can tell what element this is from the image below and give the correct full electron configuration.



(source) periodictable.com Sulfur information. 




The element shown in the image is Sulfur due to the presence of 4 valence electrons in the picture. Because each arrow represents an electron, there are shown to be 16 electrons in the different, collective, orbitals. This proves it as Sulfur yet again, as it contains 16 electrons. 

Blog Post 3

Blog Post 3 (Unit 3)

1. Describe the history of the atomic model.

To begin with, the atom was seen as a minuscule, indivisible object, typically viewed as being round, and with no internal components. This model was developed by Democritus. After this, it was discovered that atoms possessed negative and positively charged particles within them. This lead to the discovery of protons, and electrons. The nucleus of the atom was eventually concluded to be composed of neutrons and electrons, neutrons being discovered by bombarding the atomic structure with alpha particles. These bounced back, and returned in the direction in which they were launched, proving that there was yet another structure inside the atom. 

1. Explain each subatomic particle including their charge, relative mass, and locations in the atom.

Neutron - Neutrons are neutral, or uncharged subatomic particles occupying the nucleus of the atom. They are the same size as Protons and are 2,000 times larger than the size of an electron.  

Proton - Protons are positively charged subatomic particles placed within the nucleus of the atom alongside the Neutrons. They are the same size of Neutrons and are 2,000 times larger than electrons. The amount of electrical charge possessed by Protons is the same as the amount of electrical charge possessed by Electrons. 

Electron - Electrons negatively charged subatomic particles, located in orbitals around the nucleus of the atom. There are several different orbitals, filled according to how many electrons the atom possessed. Electrons are 2,000 times smaller than 

1. What was Mendeleev’s major contribution to chemistry?

Mendeleev is credited with ordering the elements, in a way nearly accurate to their placement today.  Laying out cards that illustrated the element's properties, and arranging them in such a way that they fit together, is the same method used to organize the periodic table of elements as we see it today. He was the first to try and order them in such a way, and was even able to find spaces, where an undiscovered element would have fit. 

1. Draw and upload a picture of a Bohr model of Gold (yes draw this one, not download a picture).

Electrons: 79

Protons: 79

Neutrons: 118

Energy levels: 6

1. Relate the numbers of the subatomic particles to the atomic number and mass number (use examples).

As one moves through the periodic table, it can be seen that from one element to the next, the atomic mass of the element increases alongside the atomic number of the element. This is what allowed Mendeleev to gain the basis of organization for his periodic table. 

1. Relate the numbers of the subatomic particles to the charge (use examples).

The more protons contained within an atom/isotope, the more positively charged the particle will become. The loss of electrons can also change the charge of the particle, just as the gain of electrons, causes the element to become negatively charged. Noble gasses, have even, and completed outer electron orbitals, resulting in a non-reactive state between them, and even other known elements. The loss, or gain of electrons, changing the charge, and completed status of the valence electron shell, results in the chemical reactions, and chemical bonds seen between elements. 

1. Define atomic mass and use isotopic abundance to calculate. (ex. explain how to find the average mass of Magnesium).

Atomic mass - The average atomic mass of an element is found through the measurement, and averaging of all its isotopic components. Different isotopes are found in different percentages of abundance, thus changing the resulting atomic mass greatly, depending on which is in higher concentration. 

1. Include your calculation for finding the isotope of pennies and identify how many pre-1982 pennies and how many post-1982 pennies were in your unknown container.

x = old pennies

[x(3.1) 10-x(2.5) = 27.26 ] = 2.26 (x = 3.77) 3.77 pennies (4) 

4 Old pennies, and 6 New pennies. Therefore 40% old pennies, and 60% new pennies composed the mixture. 

Blog Post 2

Blog Post 2 (Unit 2)

source: wallpapers-and-backgrounds website: http://wallpapers-and-backgrounds.net/science-wallpaper

1. Draw or describe a particle diagram of an element and compound

Description:  

An element - An element, is a collective substance made up entirely of one type of atom. There are more than 100 different elements, that are the composition of all physical things (that possess a mass) on earth. They are joined by chemical bonds, creating often more complicated forms. 

A compound - A compound, is a collective substance made up of more than one different type of atom. Also referred as a mixture (either homogeneous or heterogeneous). There is a definite ratio of the different atoms, and they are joined by chemical bonds, forming molecules that cannot be separated by physical means. 

1. Draw or describe a homogeneous and heterogeneous mixture.

Description: 

A homogeneous mixture is a blend of multiple different components, that can be combined in a way that the overall mixture has a uniform composition in all respects. 

A heterogeneous mixture is a blend of multiple different components that cannot be combined in a way that the jumble is uniform throughout, and there are obvious separations between the components.  

1. Make a list of 5 physical and 5 chemical properties

Physical: 

• Color
• Volume
• Freezing point
• Temperature
• Mass 

Chemical: 

• toxicity 
• Flammability 
• types of chemical bonds formed 
• The heat of combustion 
• chemical stability 

1. Make a list of 5 physical and 5 chemical changes.

Physical:

• Melting ice cube.
• Chopping wood.
• dissolving another substance into the water. 
• The sublimation of dry ice. 
• Mixing water and oil. 

Chemical:

• Mixing an Acid and a Base.
• Baking a cake.
• Cooking an egg.
• Burning a piece of wood.
• Rusting iron.

1. Describe the 4 states of matter and how energy affects its composition.

Solid - The addition of energy to a solid, causes its componential atoms/particles to move. This, in turn, triggers the solid to switch phases into a liquid due to the increased movement and energy.

Liquid - When more energy is added to a liquid, the particles and atoms increase the speed of their movement until they become airborne and can then be considered a gas.

Gas - Even more energy is added, the gas begins to

Plasma 

1. Describe the 8 different phase changes between the different states of matter.

1. Freezing - The removal of heat from a substance which results in a change from liquid to solid.

2. Melting - The addition of heat to a substance which results in a change from solid to liquid. 

3. Sublimation  - The evaporation, or direct transformation of a substance from solid to gaseous. 

4. Evaporation - The heating of a liquid to the point that it transforms into a gaseous state. 

5. Dissolving - The homogenous combination of two substances, typically solid and liquid to liquid only. 

6. Smoke  - The burning of a solid object until it becomes particularized and gaseous throughout the air. 

7. Condensation - The phase change from gaseous to liquid by the addition of colder temperatures. 

8. Freeze-drying - The freezing, the sublimation of ice particles, so that the substance itself is intact. 

1. Create a pie graph of the %composition of each of the chemicals in the separation of mixture lab. (Either sand, salt, and iron  or  silicon dioxide, sodium chloride, and ammonium chloride).

1. Describe the physical properties used to separate the three chemicals in the lab.

Sublimation, one of the defining properties of the ammonium chloride, was used to initially remove it and measure its absence. The mixture was heated over a hotplate beneath a fume hood, and its gaseous state was evaporated away. Next, water was added to the mixture. This caused the sodium chloride to dissolve into the water, and therefore be evaporated out after being filtered through a coffee filter. Leaving only the silicon dioxide behind. 

Blog Post 1

Blog post 1 (unit 1) 

Japanese Maple Tree, Source: Falcor88 - DeviantArt
https://falcor88.deviantart.com/art/1390614-615874978450917-1162797191-N-413184974 

1. Describe how to find the density of a metal block if the block’s mass is 0.84g, length is 15.55 cm, width is 3.25 cm, and height is 0.00163 cm. (Keep appropriate significant figures

density = mass/volume Volume = length * width * height [Volume = 15.55cm * 3.25cm * 0.00163cm = 0.082]

Density = mass/volume [Density = 0.84g/0.082cm^3 = 10.24]
Density = 10g/cc

1. If you measure 300 cm, how do you convert to meters?

300 centimeters, divided by 100 = 3 meters.

1. List proper safety equipment wardrobe to use during a lab

1. Pants that are long enough to reach below the knee

2. Close toe, and heel shoes

3. safety goggles

4. long hair tied back out of your face
5. Gloves when necessary 
6. Fume hood in lab when working with toxic chemicals 
7. No loose clothing, jewelry etc. 

1. Create a graph for the different thickness of Aluminium foil you measured in the lab. (include proper titles and units and include the accepted value for the thickness).

Graph of Aluminum Foil Measurements 

All units shown are centimeters (The graphing program I used would not allow me to enter units.)

1. What are the rules for zeros for significant figures? (When are they or aren’t they significant?)

Non zero numbers are always significant no matter the placement, any zero placed between two non-zero numbers are counted as significant. Final zeros/trailing zeros following the decimal point are also marked as significant. 

1. Distinguish between accuracy and precision. 

Accuracy: The desired outcome gained, or the state of being correct.

Precision: Every time the result is the same, and repeatable, or the quality of exactness. 

1. What was the % error in your first lab? (Show work)

0.0025 - 0.0024 = 0.0001/0.0024 * 100 = 4.17% error

1. Express the following numbers in scientific notation:

a. 0.000045 = 4.5 × 10-5 

b. 0.023 = 2.3 × 10-2

c. 107,800 = 1.078 × 105

d. 602,000,000,000,000,000,000,000 = 6.02 × 1022