DEUTERONOMY MID SEMESTER

1                                  

         1.  pure substance x is solid at room temperature. if the substance is heated to 230⁰C is melted gradually. if then cooled to room temperature, the liquid can not be frozen

a.        is it possible x of an element or a compound. explain it!

b.      does it a chemical change occured? if so can it be said to undergo an endoterm changing, based on the information provided?

c.       Can it be said that the liquid is an element, based on the information provided.

Answer :

a.  X is an element of pure a.bahan for chemical elements, or simply called elements, are chemical substances that can not be subdivided into smaller substances, or can not be converted into other chemicals by using ordinary chemical methods. At room temperature (25 C) elements can be either solid, liquid, and gas.

b.  In my opinion, no chemical changes in these events because chemistry is the change undergone by an object forming a new substance. While in the event there is no new substance is produced but only changes form or physical yangdisebut with physical changes. physical changes can occur because of changes in the form and any deformities, the X is the material from solid to liquid.

      This reaction is not biased to say the reaction is endothermic because the reaction is endothermic reactions require energy or absorb energy from the environment when the reaction occurs, the reaction generally produces dingin.atau temperature endothermic reaction is a chemical reaction that absorbs heat. Heat is taken from the environment so that the enthalpy increases. in the event of such a reaction is not the case because there is no heat transfer from the system and no one called about energy or enthalpy change.

c.   Yes, because the fluid including an element or elements at room temperature (25 C) and can be solid, liquid or gas.

2.  When a candle that weight 10 gr is burned in oxygen, carbon dioxide and water vapor formed by combustion the weight more than 10 gr. Was this case match whit the law of mass. Explain it.

answer :

      I think this case is not in accordance with the law of conservation of mass because of the law of conservation of mass, also known as the Lomonosov-Lavoisier law is a law that states the mass of a closed system is constant despite the wide range of processes in the system (in a closed system mass of substances before and after the reaction is the same (fixed / constant)). Statements that are commonly used to express the law of conservation of mass is the mass can change form but can not be created or destroyed. For a chemical process in a closed system, the mass of the reactants must equal the mass of the product.

      Lavoiser have observed changes in the nature and substance he argued known as the law of conservation of mass; "In a reaction, the mass of substances before reacting equal to the mass of the substance after reacting". This suggests to us that there is no mass loss during the ongoing reaction.

      For example, if we are reacting substance A which has a mass of 10 grams with substance B (mass 10 grams) to produce substances C and D, where mass quantities of substances produced equals the number of reacting mass is 20 grams.

      Chemical reactions are written with an arrow, to the left of the arrow are substances which react and to the right of the arrows are substances the reaction.

      It is known that the mass after the reaction, is the total mass, which means that the composition of the C and D may be different from the mass of substance A and B are berkomposisi 10 grams and 10 grams. Substance C and D are formed may be 8 grams and 12 grams or 12 grams and vice versa 8 grams. The law of conservation of mass only limits on the amount of the same substance with a substance that occurs before, yet describes compounds formed.

    3.When carbon burns in oxygen under limited number, it will form two gaseous compounds. Suggest the way to differentiate the two compounds with one another.

answer :

When carbon burns under a limited amount of oxygen, it forms two gaseous compounds. These compounds are carbon monoxide.

CO (carbon monoxide) gas is highly toxic because it can bind to hemoglobin in the blood thereby blocking the main function of hemoglobin as an oxygen carrier, formed in incomplete combustion of carbon-containing fuels such as wood and gasoline, because it can burn and produce heat, then gas is used as fuel gas as the reductant in metal processing, making methanol.

carbon monoxide with H2O that forms the central atom lone pair to form a dipole moment so it is polar. based on the nature of the polarity of the molecules makes it possible to separate the pollutant gas molecules using molecular screening in accordance with the properties of impurity gas polarity.

          4.   After mendeev compiled theperiodic table, he conclude that the atomic weight of certain elements was wrong ruling, and this conclusion was apparently correct. How Mendeleev was able to predict that several atomic weight were wrong? Why his predictions are not always right. Explain!

answer :

       Dmitri Ivanovich Mendeleev in 1869 observations of 63 known elements and get the result that       properties      of elements are a periodic function of the relative atomic mass. Certain properties will be repeated periodically if unsurunsur ordered by relative atomic mass increases. The next Mendeleev placed elements with similar properties in the vertical column called class. These elements have also been prepared by the increase relative atomic mass and placed in a column called period.   

      Mendeleev deliberately emptied a few places to establish similar properties in the group. Some boxes also intentionally left blank because Mendeleev sure there's an element of the unknown because it has not been found. One element that is in line with the forecast germanium Mendeleev was previously named ekasilikon by Mendeleev.

          The weakness of this theory is still contained elements of a larger mass that lies in front of a smaller mass   elements. Co: Tellurium (te) = 128 in kiriIodin (I) = 127. this is because the elements have properties kemirpan placed in one class. The weakness of this theory is the atomic mass correction. Previous atomic mass. In previous atomic mass = 76-113. besides Be, 13.5 to 9. N 120-240.

         However, the law considers Mendeleev periodic can not tolerate any exceptions as any deviation from the order of elements by atomic weight. For example, in the case of the elements tellurium and iodine, he predicted that the atomic weights of the two elements is not appropriate because the value provided suggest the opposite order to what is determined by the chemical nature. More specifically, tellurium showed a higher atomic weight in accordance with the values ​​and subsequently measured based sequence element tellurium features will be put in the same chemical group as fluorium, klorium, and bromium, where it is not included in the periodicity of the used chemistry. Apparently, according to Mendeleev reversal sequence that is true but the reason is used inappropriately. The atomic weight is actually approaching accuracy, but the order of elements is better placed by the number of atoms of each element. Schematic sequence elements enhanced by the work of Moseley in 1912, and on the main complication lies in the mixture of isotopes occurring chemical elements are most important.

      Mendeleev periodic believes that the law can be used to predict the existence and properties of some new element compounds, as well as to correct the atomic weights of some elements are already known. However, historian and author of chemistry are emphasized in the legal aspects of prediction. Mendeleev ability to accommodate elements that are known to have contributed positively in the periodic system. For example, the quote that accompanies her awarded the Davy Medal by the Royal Society of London does not mention any of his predictions.

1                    5.    When an aqueous solution of mekuri chloride is added to an aqueous solution of silver nitrate, a white solid forms. Identify the white solid and write the balanced equation for the reaction that occurs.

         answer :

               HgCl2 +2 AgNO3 ---> Hg (NO3) 2 +2 AgCl

                the resulting white powder is silver nitrate (AgCl)

ATOMIC STRUCTURE AND PERIODIC SYSTEM ELEMENTS

PERIODIC SYSTEM ELEMENTS

Development of the Periodic Table of Elements
Grouping elements by similar properties have evolved from the simple to the modern. The history of these developments are described in the following materials.

A. Development of Basic Grouping Elements

1. Grouping Elements Based on Metal and Non-Metal clusters are still too common as it turns out in a variety of metals and non-metallic elements are still there are many variations and the nature of the elements.

2. Law Triade Dobereiner In 1829, Johan Wolfgang Dobereiner see any resemblance between some elements of nature, and then breaks it down in terms of similar existing properties. Apparently each group consisting of three elements, the so-called Triade. If the elements are arranged according to the triade mass increases the atoms, it turns out the atomic mass and properties of the second element is the average of the atomic masses of the first and third elements.
These findings show an association between the atomic mass of the element properties. This grouping weakness lies in the fact that the number of elements with similar properties are not only 3 pieces.



3. Newlands Law of Octaves, 1864, A.R. Newlands announced the discovery of the so-called law of octaves. The elements are arranged by relative atomic mass increases. Apparently disputing elements 1 octave (element number 1 to 8, element number 2 to 9, and so on.) Shows similar properties or it could be said that the element properties change regularly. The trend is expressed as octaves Newland law, namely: If the elements arranged by atomic mass increases the properties of elements will be repeated after the eighth element.

Grouping Elements in Octave Newlands

t Newlands list compiled Octave, noble gas elements have not been
found. It turns out this is only suitable for grouping elements
light (low Ar).

4. law Mendeleyev
In 1869, the Russian scholar Dmitri Ivanovich Mendeleyev
based on observations of 63 elements known as
it concluded that the properties of elements periodic function of atomic mass
relative. That means if the elements are arranged according to the increase of mass
atom relative, certain properties will be repeated periodically.
Mendeleyev also made a list of periodic elements. The elements
which have similarities properties placed in a vertical column
called a class.
In classifying elements, Mendeleyev more emphasis
properties of the elements in the equation than the increase in mass of the atom
relative, so there are empty places in the periodic table
them. Empty places that will be filled later predicted
elements that have not been discovered at that time. At a later date the nature of prophecy
Similar corresponding predictions.
Weakness Mendeleyev Periodic Table as follows.
a. The placement of elements that do not correspond with the increase in mass of the atom
because it maintains relative similarity in the properties of elements
group.
b. There are many elements that have not been known at the time that the
there are plenty of empty tables.

Mendeleyev Periodic Table

5. Tabel Periodik Modern
Tahun 1914, Henry G. J. Moseley menemukan bahwa urutan unsur
dalam tabel periodik sesuai kenaikan nomor atom. Tabel periodik modern
yang disebut juga tabel periodik bentuk panjang, disusun menurut kenaikan
nomor atom dan kemiripan sifat. Tabel periodik modern ini dapat dikatakan
sebagai penyempurnaan Tabel Periodik Mendeleyev.
Tabel periodik bentuk panjang terdiri atas lajur vertikal (golongan) yang
disusun menurut kemiripan sifat dan lajur horizontal (periode) yang disusun
berdasarkan kenaikan nomor atomnya.
a. Lajur vertikal (golongan) ditulis dengan angka Romawi terdiri atas 18
golongan.
1) Golongan A (Golongan Utama)
Gol. IA : Alkali Gol.VA : Nitrogen
IIA : Alkali Tanah VIA : Kalkogen
IIIA : Aluminium VIIA : Halogen
IVA: Karbon VIIIA (0): Gas Mulia

PERIOD AND GROUPS IN MODERN SPU

1. Period

Is the horizontal rows of the periodic table.

Modern SPU consists of 7 periods. Each period stated amount / number of atomic shell elements that occupy those periods.

Period Number = Total Skin Atom

So:

The elements that have 1 skin (skin K only) located in period 1 (row 1), the elements of which have 2 skins (skins K and L) lies in the second period and so on.

example:

9F: 2, 7-second period

12mg: 2, 8, 2 the 3rd period

31Ga: 2, 8, 18, 3 period-4

Note:

a) Period 1, 2 and 3 is called the short period since it contains relatively few elements.

b) Period 4 and so called long period.

c) Period 7 called period is incomplete because not up to class VIII A.

d) To determine the period number of an element by atomic number, you only need to know the atomic number of the element that start each period.

2. Group

• periodic system consists of 18 vertical columns are divided into 8 main groups (group A) and 8 classes of transition (group B).

• The elements that have the same valence electrons are placed in the same group.

• For the elements of class A according to its place in the periodic system:

Group Number = Number of Valence Electrons

The elements of class A has another name, namely:

Group IA Alkali class =

Group IIA = class of Alkali Soil

Group IIIA = class of Boron

Group IVA class = Carbon

Group VA = class of Nitrogen

Group VIA = class of Oxygen

Group VIIA = class Halide / Halogen

Group VIIIA class = Noble Gases

PERIODIC PROPERTIES ELEMENTS

include:

1). Jari-Jari Atom

Is the distance from the nucleus to the electrons in the outer shell.

• The size of the atomic radius is influenced by the size of the atomic number of the element.

• The larger the atomic number of the elements of a class, the more the number of electron shell, so the larger the atomic radius.

So: in one group (from top to bottom), the atomic radius increases.

• In a period (from left to right), atomic number increases, which means the increasing nuclear charge, while the number of electrons fixed skin. As a result of the pull of the nucleus, the greater the outer electrons, resulting in increasingly smaller atomic radius.

So: in a period (from left to right), the atomic radius gets smaller.

2). Ionization Energy

Is the minimum energy required in the form of a gas of neutral atoms to release one electron to form charged ions +1.

If these atoms release electrons which the two then it would take more energy (called the second ionization energy), and so on.

EI 1 <EI 2 <EI 3 ff

In one group (from top to bottom), EI is getting smaller as the atomic radius increases, so gravity core to the outermost electron less. As a result, the outer electrons are easily released.

ü In a period (from left to right), EI greater because the atomic radius so small that gravity core to the outer electrons bigger / stronger. As a result, the outer electrons more difficult to remove.

3). Electron Affinity

• It is the energy released or absorbed by neutral atoms in gas form when receiving an electron to form negative ions.

• The price of a negative electron affinity, the easier atom receive / pull electrons and also the more reactive element.

• electron affinity is not the opposite of ionization energy.

• In one group (from top to bottom), the price of the smaller electron affinity.

• In a period (from left to right), the price of the greater electron affinity.

• main group elements have electron affinities are negative, except for groups IIA and VIIIA.

• has the largest electron affinity group VIIA.

4). electronegativity

• It is the ability of an element to attract electrons in a molecule of a compound (in bond).

• Measured using Pauling scale of between 0.7 (electronegativity Cs) to 4 (electronegativity F).

• Elements that have a large electronegativity prices, will tend to accept electrons and form negative ions.

• Elements that have small electronegativity prices, will tend to lose electrons and form positive ions.

• In one group (from top to bottom) rates, the smaller electronegativity.

• In a period (from left to right), the price of the greater electronegativity.

THE STRUCTURE OF ATOM, ITS HISTORICAL DEVELOPMENT AND QUANTUM NUMBERS

ATOM

 a. Elementary particles: particles forming the atom consists of electrons, protons neutrons den.
1. Proton: atom forming particles that have mass equal to one sma (amu) and charged +1.
2. Neutron: particles forming a sma atomic mass (amu) and neutral.
3. Electron: atom forming particles that have no mass and charged -1.
b. The nucleus: a positively charged nucleus, consisting of protons neutrons den.

c. Notation elements: zA A to X: sign atoms (elements)
Z: atomic number = number of electrons (e)
= Number of protons (p)
A: mass number = number of protons + neutrons
In neutral atoms, applies: the number of electrons = number of protons.
d. No neutral atoms: electrically charged atoms due to excess or deficiency of electrons when compared with the neutral atom.
Positively charged atoms when the electron deficiency, called cations.
Negatively charged atoms when an excess of electrons, called anions.
example:
- Na +: cation with one electron deficiency
- Mg2-: cation with a shortage of 2 electrons
- Cl-: anion with an excess of one electron
- O2: anion with an excess of two electrons
e. Isotopes: elements of the same atomic number, but different mass numbers.
Example: oxygen isotopes: 816 O; 817 O; 818 O

f. Isobar: elements of the same mass number, but different atomic numbers.
Example: 2759 2859 CO with Ni

g. Isoton: elements with the same number of neutrons.
Example: 613 C to 714 N

h. Iso electron: atom / ion with the same number of electrons.
Example: Na + with Mg 2 +
                  K + with Ar

HISTORY AND DEVELOPMENT OF ATOMIC THEORY

From the times of the ancient Greeks to the present, the model and the atomic theory continues to evolve. Through the model and theory of the atom, we can determine the structure of an atom.1. Mr. Democritus and Aristotle


From the times of the ancient Greeks to the present, the model and the atomic theory continues to evolve. Through the model and theory of the atom, we can determine the structure of an atom.1. Mr. Democritus and AristotleThe above picture is the father of Greek genius of expression on the definition of atoms for the first time, the first, circa 460-370BC.Democritus father's opinion about the atomatoms are the elements that make up reality. However, these elements can not be divided lagi.Karena that these elements are named atom. Atom comes from the Greek atomos: a means and Tomos mean divided.

             According to Aristotle a substance composed of fire, water, earth, and air. So who is more right? It must depend on the people who receive it at that time. Apparently the theory of Mr. Aristotle was more widely accepted and used as the basis for the next developmental theorizing by Dalton.2. ATOM THEORY OF DALTONFor a thousand years the term atom sink, like everyone is convinced that what Aristotle says is the truth that has been searched on "whether the material is composed of a substance? '. But apparently in 1803 there was a high school teacher in the UK who are still curious about the atom. By basing on the theory of Aristotle, on a sunny afternoon, Dalton had discovered evidence and the fundamental ideas of the theory. This theory is also able to explain the law of conservation of mass Law of Lavoisier and Proust fixed ratio.Here are 5 Atomic Theory Dalton:1. The elements consist of particles remarkable little that can not be subdivided (called atoms) and a massive round ball shape. In a chemical reaction, they can not be created, destroyed or converted into other types of elements.2. All atoms in the same element are similar and therefore have similar properties, such as mass and size.3. Atoms of different elements types have different properties as well.4. Compounds can be formed when more than one type of element combined.5. Atoms of two or more elements can be reacted in different ratios to produce more than one type of compound.But times were different then Democritus time to time, so many scientists are trying to find a way to the term "fault" of the theory of Dalton. Dalton was still confident. Before anyone finds evidence that his theory was wrong, he thought that his theory is that terbenar.Apparently there finally two scientists who disagree with the Atomic Theory Dalton. They are Sir Humphry Davy (1778-1892) and Michael Faraday (1791-1867). To prove that their opinion is more correct, they are doing experimental chemical change when an electric current passing through an electrolyte solution, or so-called electrolysis. So amazing, Faraday discovered that the amount of a substance produced in the electrolysis current electrodes is proportional to the amount of electrical current. In 1833, Faraday also discovered that the amount of electricity required to produce 1 mole of substance at the electrode is fixed (96.500 C). This relationship is known as Faraday's law of electrolysis. Based on his opinion of a chemist, so he concludes that there is a basic unit in the electrolysis, there are analogous to electricity. He also gave the name of the electrons in this hypothetical unit.Since then several statements Dalton's atomic theory was killed. Weakness Dalton's atomic theory. In Dalton's atomic theory is not explained the source of the charge for electricity according to Dalton when atoms are neutral particles. The surplus is Dalton chemistry provides the basis for what is an atom.3. ATOM THEORY THOMSON

 The inventor of the electron, Mr. J.J. ThomsonAfter Dalton's atomic theory disqualified because there was a question no one has answered it, then Thomson was in about the 1890's trying to do an experiment to find a way out of the problem. The basis of theories of other scientists such as Humphry Davy, who proved that the gas becomes a better conductor of electricity at low pressure, Thomson also conducted experiments using a cathode ray tube. So this is a tube under vacuum tubes, and at each end of the tubes were
 Cathode ray tube voltage electrical current is high enough, it turns on the low pressure and high temperature, the gas in the fluorescent tube will depend on the type of substances in the tube. If the gas pressure is reduced, the front area of ​​the cathode will be dark. The area is growing dark when the gas pressure continues to be reduced. Finally, the entire tube to be dark, but the front of the cathode tube glow with a greenish tint. Through experiments, it can be proved that it was a greenish color particle radiation. Because it comes from the cathode, the beam called cathode rays.Further experiments proved that cathode rays are electrically charged particle radiation negatively hereinafter called electrons.1. Cathode rays propagate straight from the anode towards the cathode surface2. Cathode rays can rotate turbines3. Cathode rays are deflected towards the positive pole"Atom is a ball of solid positively charged and negatively charged electrons scattered didalamya" This is the conclusion of the Thomson theory.
 illustration thomson atomic theoryExcessProving the existence of other negatively charged particles in atoms. Means the atom is not the smallest part of an element.WeaknessThomson's model can not explain the arrangement of positive and negative charges within the atomic sphere, can not explain the chemical reactions that occur between atoms

4. Rutherford Atomic Theory
  Rutherford, the discoverer of the atomic nucleus in collaboration with Thomson
After Thomson proposed his theory in 1910 was no less Rutherford conducted experiments to reveal his version of the theory. With the assistance of two of his disciples, they experiment known as the scattering of alpha rays, which are positively charged particles, and moving forwards, great power that can penetrate through a thin sheet of paper.


The experiment is actually intended to test Thomson opinion of whether the atom is really a solid ball when it is positive that the alpha particles would be reflected or deflected. From their observations, obtained the fact that when alpha particles were fired at a very thin gold plates, then most of the alpha particles passed (no deviation angle less than 1 °), but from observations obtained Marsden fact that one in 20,000 alpha particles will turn angle of 90 ° even more, or there reflected. This is not in accordance with the theory pastialh Thomson which are atoms depicted dense homogeneous in all its parts.
 Based on the experimental genius Rutherford suggested that his idea of ​​the atomic nucleus. According to him, most of the mass of the atom and the positive charge is concentrated at the center of the atom, hereinafter referred to circulate around the core atom.Elektron at distances relatively far away. The distance between the nuclei of atoms until the skin is called the atomic radius.With such a model, the scattering of alpha rays thin gold plates can be explained as follows:1. Most of the particles because the alpha rays can penetrate through sterile areas2. Alpha particles are deflected by the nuclei approach mengalani repulsive core3. Alpha particles towards the nuclei is reflected by the positively charged nucleus and a very solid
"Atomic nuclei are composed of very small and positively charged, surrounded by negatively charged electrons. "So this is the conclusion of how atoms form meurut Rutherford.ExcessHypothesized that atoms are composed of atomic nuclei and electrons that surround the nucleusWeaknessCan not explain why the electrons do not fall into the nucleus. Based on the theory of physics, the motion of electrons around the nucleus is accompanied by transmitting energy so long - eventually the electron energy is reduced and the longer the trajectory will approach the core and falling into the nucleus Take a piece of string and tie one end of your piece of wood while you hold the other end. Rotate the rope over your head. What happened? Right. Eventually the rotation will slow and will hit your head because your rotation is weak and sore holding the rope. Since Rutherford was already introduced trajectory / position of electron later called skin
5. Niels Bohr theory of the atom

Niels Bohr introduced the theory of electron trajectories
Sure enough everything that exists in this world nothing is perfect. Any theory that scientists issued sure there besides the advantages, there are also drawbacks. In the experiments, tahin 1911, Niels Bohr Rutherford tried to improve the theory by conducting experiments hydrogen atom spectrum.

Then from these experiments Niehl Bohr theory of the atom are:
1. According to him, there are only a certain set of possible orbits for an electron in a hydrogen atom. Orbit is known as the stationary state of motion (settled) electron and a circular path around the core
2. As long as the electrons are in a stationary orbit, the electron energy anyway so there is no energy in the form of radiation emitted or absorbed.
3. Electrons can only move from one stationary orbit to another stationary trajectory. In this transition, a certain amount of energy involved, the amount in accordance with Planck equation, ΔE = hv.
4. Stationary trajectory is allowed to have the scale with certain properties, especially property called angular momentum. The magnitude of the angular momentum is a multiple of h/2Π or nh/2Π, where n is an integer and the Planck constant h


So according to Bohr, electrons surrounding the nucleus in certain paths called the electron shell or energy level of the lowest energi.tingkat shell electron is located at dalam.semakin out of her skin and the greater the number the higher the energy level.

excess
Bohr atom that the atom is made ​​up of several skin for a transfer of electrons.
weakness
atomic model is not able to explain the Zeeman effect and the effect Strack6. ATOM THEORY QUANTUM MECHANICS MECHANICS OR WAVES
  Schrodinger
After Niehl Bohr theory it also has weaknesses, subsequent scientists are working to improve Erwin Schrodinger. Based on further development saying that the electron trajectory is not round but like a wave around the nucleus. Therefore, the position can not be known with certainty. Atomic theory of quantum mechanics have in common with the theory of Niels Bohr energy levels or shells, but differ in terms of the trajectory or orbit.
Experiments done is experiment Chadwick


Conclusion The results of the experiment:

  sketch of the theory of quantum mechanics
Shows the electron cloud around the nucleus where the probability of an electron. Orbital describes the energy levels of electrons. Orbitals with the same energy level or nearly the same to form sub shell. Some sub leather combine to make such kulit.Dengan skin consists of several sub-skin and consists of several orbital subshell. Although the skin is the same position but not necessarily the same orbital position.
Weakness Modern Atomic Model
Schrodinger wave equation can be applied only exact for particles in a box with a single electron and atom

QUANTUM NUMBERS

Energy electrons in an orbital is determined by a variety of numbers as the principal quantum number (n), azimuthal quantum number (l), and the magnetic quantum number (m). Energy electron rotation on its axis is determined by the spin quantum number (s).
1. The principal quantum number (n), worth 1, 2, 3, 4, ... and so on. Quantum numbers are consistent with the electron shells in an atom as usual energy level expressed by the skin. The principal quantum number (n): 1 2 3 4 ... In accordance with the skin to: 1 2 3 4 ...
            K L M N ... Thus the principal quantum number indicates the amount of electron trajectories.
2. Azimuthal quantum number (l), value 0, 1, 2, 3, ... (N - 1) quantum number shows in the subshell (sublintasan) where electrons move and also determines the shape of the orbital. subshell l = 0 is also called the orbital s (sharp) subshell l = 1 is also called p orbitals (principle) subshell l = 2 is also called the orbital d (diffuse) subshell l = 3 is also called orbital f (fundamental) Each skin has skin subshell corresponding number, for example: n = 1 (K shell) prices have l = 0, ... (1 - 1) = 0 Skin to-1 (K) has a subshell, the subshell l = 0 or 1s n = 2 (L shell) prices have l = 0, ... (2-1) = 0, 1 Skin to-2 (L) has two subshells, namely subshell l = 0 or 2s orbital and subshell l = 1 or 2p orbitals n = 3 (skin M) has a price l = 0, ... (3-1) = 0, 1, 2 Skin for-3 (M) had 3 subshell, namely: subshell l = 0 or 3s orbital subshell l = 1 or 3p orbitals subshell l = 2 or 3d orbitals n = 4 (leather N) has a price l = 0, ... (4-1) = 0, 1, 2, 3 Skin for-4 (N) had 4 subshell, namely: subshell l = 0 or 4s orbital subshell l = 1 or 4p orbital subshell l = 2 or 4d orbital subshell l = 3 or 4f orbitals
when n = 1, then there is only one possible value of the azimuthal quantum number l = 0 for the first shell (K) consists of only one subshell is s subshell. As for n = 2, then there are two possible subshell l = 0 and l = 1 for the second shell (L) there are two subshell is s and p sub shell.


What about the next skin?
Skin M, then the value of n = 3 and l = 0, 1, and 2 as having subshell s, p, and d.
Leather N, then the value of n = 4 and l = 0, 1, 2, and 3 as having subshell s, p, d, and f.
So the value of azimuthal quantum number is not likely equal to or greater than the main quantum number. A maximum value of l = n - 1.
3. Magnetic quantum number (m), precious-l, ..., 0, ... + L This quantum number determines the position or orientation of the orbital, also indicate the presence of one or more energy levels which constitute the level of a subshell. Any price l have a price m. Example:

conclusion:
s orbital (l = 0) has one orbital, the price of the m = 0.
p orbitals (l = 1) has three orbitals, the price of its m: -1, 0, and +1.
d orbitals (l = 2) have 5 orbitals, the price of its m: -2, -1, 0, +1, and +2.
f orbitals (l = 3) have seven orbitals, the price of its m: -3, -2, -1, 0, +1, +2, and +3.
Orbitals in a subshell have a particular form and is located in a particular space anyway.
Based on observations and mathematical calculations of spherical s orbital, meaning: there are electrons in s orbitals are equally far away and all directions of the atomic nucleus. While the p orbitals have a twisted shape like a balloon. P orbitals have 3 orbitals, each of which lies on the axis of x, y, and z that distinguished p orbitals px, py, and pz.
D orbitals have 5 spread between the axis orbital axis space x, y, and z are each divided into dz ², dx ²-y ², DXZ, DXY, and dyz.
4. Spin quantum number (s), worth +1 / 2 and -1 / 2 (possibly turn right = 1/2 and possibly turn left = 1/2).
This quantum numbers give an idea about the direction of rotation of the electron on its axis.
Each has a price s = m + 1/2 and s = - ½

Quantum Numbers Functions

The four quantum numbers are used to indicate the location of the last electron (outer) of an atom. Starting from the location of the atomic shell (principal quantum number), subshell atom (azimuthal quantum number), the location of orbital (magnetic quantum number) to the velocity of the electron (spin quantum number). So that this quantum number is specific in accordance with the principle of prohibition pauli. Next we combine the four quantum numbers to determine the identity of an electron. In order to determine exactly we should understand the electron configuration and orbital diagram first.
For example, the electron configuration and orbital diagram of sulfur (S) as follows:



To determine the quantum numbers of the last electron we just noticed that the outer subshell 3p:

The depiction of the last electron marked in red. Electrons are located on the skin of 3 means the main quantum number (n) = 3. Located in subshell p mean quantum number azimutnya (l) = 1. As for determining the magnetic quantum number we need to name each subshell 3p orbitals in which the numbers are green. According to the diagram above, the value of the magnetic quantum number (m) = - 1. And because the downward arrows mark the spin quantum number (s) = - ½.