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.