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CHEMICAL BASES: ACTIVITY 1 "ATOMS AND MOLECULES" (ATOMIC…
CHEMICAL BASES:
ACTIVITY 1 "ATOMS AND MOLECULES"
Quantum numbers
Principal quantum numbers (n)
It specifies the level of energy in an orbital, and it relates with the average distance between the electron and nucleus
EXAMPLE
If the last level of an element is 3s, then n=3
Angular quantum numbers (l)
It describes the geometrical form of an orbital.
l= n-1
EXAMPLE
If the last level of an element is 3s, then l=0.
3p, l=1
3d, l=2
3f, l=3
Magnetic quantum numbers (m)
It indicates the orientation of the orbital.
m=2l+1
EXAMPLE
s: m=0
p: m= -1,0,+1
d: m= -2,-1,0,+1,+2
f: m= -3,-2,-1,0,+1,+2,+3
Electron spin quantum number (s)
The electron possesses its own quantum number that reveals the direction of rotation of the
electron around its axis when it moves into an orbital.
EXAMPLE
s=-1/2
s= +1/2
ATOMIC ORBITALS
Heisenberg Uncertainty Principle:
"It is impossible to determine, at the same time, the exact momentum and position for an electron."
We can't establish with complete certainty what is the exact position and direction of an electron, but we can calculate its probability. However the higher the probability for an electron's position the lower it will be for its direction, and viceversa.
Orbital:
Regions of space around the nucleus a certain where an electron may be present.
SHAPES OF ORBITALS
F ORBITALS
Has 7 possible orientations (m=-3,-2,-1,0,1,2,3)
Can hold 14 electrons (2 per orientation)
D ORBITALS
Has 5 possible orientations (m=-2,-1,0,1,2)
Can hold 10 electrons (2 per orientation)
P ORBITALS
Shaped like a dumbell
Has 3 possible orientations (m=-1,0,1)
Can hold 6 electrons (2 per orientation)
S ORBITALS
Shaped like a sphere is the only type of orbitals that has only one possible orientation (m quantum number) therefore it can hold only 2 electrons
DISTRIBUTION OF ORBITALS
LEVEL: 1
ORBITALS: 1s
TOTAL OF ELECTRONS: 2
LEVEL: 2
ORBITALS: 2s 2p2p2p
TOTAL OF ELECTRONS: 8
LEVEL: 3
ORBITALS: 3s 3p3p3p 3d3d3d3d3d
TOTAL OF ELECTRONS: 18
LEVEL: 4
ORBITALS: 4s 4p4p4p 4d4d4d4d4d 4f4f4f4f4f4f4f
TOTAL OF ELECTRONS: 32
LEVEL: 5
ORBITALS: 5s 5p5p5p 5d5d5d5d5d 5f5f5f5f5f5f5f
TOTAL OF ELECTRONS: 32
LEVEL: 6
ORBITALS: 6s 6p6p6p 6d6d6d6d6d
TOTAL OF ELECTRONS: 18
LEVEL: 7
ORBITALS: 7s 7p7p7p
TOTAL OF ELECTRONS: 8
CORRECT ORBITAL FILLING
Since electrons are negatively charged, and equal charges repel each other, when filling up the orbitals electrons will try to be as far away from each other as possible. This means then when filling an orbital of equal energy (e.g. p) they will fill up a different orbital first and then pair up.
Orbitals define an element's ionization energy
REFERENCES:
Calbreath, B. (n.d). Hund’s Rule and Orbital Filling Diagrams. August 2017, Lumen, from
https://courses.lumenlearning.com/cheminter/chapter/hunds-rule-and-orbital-filling-diagrams/
James, J. (2017). Review of Atomic Orbitals. August 2017, Master Organic Chemistry, from
http://www.masterorganicchemistry.com/2017/06/07/review-of-atomic-orbitals/
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http://www.m2c3.com/c101/chemistry_in_contextx/ch2/simple_electron_configuration/electron_configuration.htm
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http://www.bbc.co.uk/schools/gcsebitesize/science/add_ocr_gateway/periodic_table/atomstrucrev1.shtml
N.d. (2015). Shapes of Atomic Orbitals. August 2017, Wikibooks, from
https://en.wikibooks.org/wiki/High_School_Chemistry/Shapes_of_Atomic_Orbitals
SparkNotes Editors. (n.d.). SparkNote on Atomic Structure. Retrieved August 11, 2017, from
http://www.sparknotes.com/chemistry/fundamentals/atomicstructure/
Chang, R. (2010). QUÍMICA. DÉCIMA EDICIÓN. McGRAWW-HILL.
Questions and Answers. (n.d.). Retrieved August 14, 2017, from
http://education.jlab.org/qa/molecule_01.html
Helmestine, A. . (2017). What is an atom?. August 14, 2017, de Thought Co. Sitio web:
https://www.thoughtco.com/what-is-an-atom-603816
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https://www.livescience.com/37206-atom-definition.html
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https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Electronic_Structure_of_Atoms_and_Molecules/Electronic_Configurations/The_Octet_Rule
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http://definicion.de/elemento-quimico/
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http://www.dictionary.com/browse/ion
Molecule
A molecule is when you get atoms together. Every compound is a molecule but not every molecule is a compound. A compound is what you get when you join two or more atoms of different elements.
Atom Structure
Every substance is made from atoms. An atom is made up from: A Nucleus witch contains Protons
(Neutrally Charged particles), and Protons (positive charged particles). Atoms are surrounded by Electrons (Negative charged particles) , this makes an equilibrium between charges. Protons and Electrons have
the same mass and electron mass is almost 0 (0.0005 ).
Atom
"Its the fundamental piece of matter and the defining structure of elements. In the universe everything, except energy, is made of atoms.
An atom is made up of 3 subparticles: Protons, neutrons and electrons. Protons and neutrons are together in the nucleus while the electrons orbit around the nucleus."
Octet Rule
The octet rule, created in 1916 by Gilbert N. Lewis, is the tendency of atoms to have 8 electrons in their valence shells. Atoms can either give electrons or recieve electrons depending on how many electrons are in the last level of the valence shell.
When applying the octet rule, you should not consider the d and f orbitals, instead, we focus on the s and p orbitals.
Element
Substance formed by atoms of the same atomic number (their nucleus has the same number of protons, regardless of the number of neutrons).
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Ion
Atom (or group of atoms) electrically charged
formed by the loss or gain of electrons.
A positive ion is called a "cation", which results when an atom loses an electron.
A negative ion is called an "anion", and results when an atom gains an electron.
The valence of an ion refers to the number of electrons lost or gained by the original atom. A plus sign represents cations, and a minus sign represents anions.
For example: Na+, Cl-, Ca 2+
Electronic Configuration
Orbital diagrams
SPDF notation
Noble gas notation
Atomic Number
The atomic number is represented by a letter "Z" and it indicates the number of protons in the nucleus of an atom. If said atom happens to be neutral, the atomic number will also indicate the number of electrons.
EXAMPLE
The atomic number of Carbon is 6. A neutral atom of carbon will have 6 protons and subsequently 6 electrons.
Atomic Mass
The atomic mass is the sum of the neutrons and protons present in an atom, with the exception of hydrogen, which has no neutrons, It can be represented by the letter "A".
EXAMPLE
Carbon has an atomic mass of 12. Since we already know it has 6 protons thanks to its atomic number, we now know that it also has 6 neutrons.
Isotopes
They are atoms that have the same atomic number and different atomic mass. Most elements have isotopes, but they are not very different from each other, since their properties are mainly determined by the number of protons and electrons.
EXAMPLE
Carbon has several different isotopes, one of them is Carbon-13. Carbon-13 has 6 protons and 7 neutrons, it also has an atomic mass of 13.
Is the representation of the arrangement of electrons distributed among the orbital shells and subshells of an atom. There are 3 different ways of writing the electronic configuration of an element:
Shows each of the separate orbitals and the spins on the electrons.
Most common way to describe electron configurations. The total number of electrons in each energy level is described by a superscript thar follows the relating level.
Uses noble gases as reference. the noble gas in the period above the element that your using is used to denote te subshells that elemnt has filled and after which the valence electrons are written.
