Selasa, 23 Mei 2017

Intan's final assignment (Noble Gases Group Elements)


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Noble Gases Group Elements
The noble gases are the elements contained in class VIIIA (in the periodic system located in the rightmost column) which have very high stability and some are found in nature in mono atomic form. The elements contained in the noble gases are Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn). These elements are called noble gases because they are very difficult to react (inert). These gases are very little contents on earth.
 The most glorious gas is Argon (Ar). Although on Earth Helium is not the most noble gas but in the universe the most Helium content among other noble gases because Helium is the fuel of the sun and other stars.
The radius of a noble gas atom is so small that the distance between the valence electrons (the electrons in the outer shell) is essentially very close. As a result the price of energy ionization   very large that cause noble gas is very difficult to remove electrons. While low electron affinity causes noble gases it is very difficult to accept electrons. This combination of properties causes noble gases to be very difficult to react (inert). In nature noble gas is never found in the form of a compound but a mono atomic molecule (a stand-alone atom).
There is also an important thing that causes the noble gas is very stable the electron configuration. Because of its stable electron configuration, noble gases are also commonly used for electron configuration enhancements for other elements.
The noble gas classes have physical properties and chemical properties.
A. Physical properties
ð Noble gas groups are not found natural compounds in nature
ð This class already meets the octet and duplet rules. Duplets for helium (2 outer electrons), while octets (8 outer electrons) for elements other than helium in noble gases
ð The stability is very high, reflected from the enormous ionization energy and the electron affinity is very small
ð The boiling and frozen point of the noble gas rises from top to bottom, reflected by the weak London style. Well, the freezing point reaches absolute (0 K) especially helium
ð The noble gas electron configuration always ends ns2 ns6, unless helium ends in ns2
ð Noble gases are not covalent and ionic
ð Precious gas compounds are most often used for lamps

B. Chemical properties
ð The noble gases have an atomic radius that extends into the radon, making it easier to form a momentary dipole and van der Waals forces
ð The noble gas reactivity increases with the increase of atomic radius
ð Noble gases can only react with elements that have a very high electro negativity, such as fluorine.
ð Precious gases are often called inert gases because they do not react.

C. Uniqueness of noble gases
ð The noble gas elements are the longest studied by scientists because to make them alone requires a high temperature.
ð The noble gas elements have meaning:
* Helium = from the sun
* Krypton = hidden
* Neon = new
* Xenon = unknown or alien
* Radon = radioactive
ð Radon can react spontaneously (E cells marked positive) with fluorine
ð Xenon requires heating or irradiation to start the reaction
ð Krypton is very difficult to react so it is said to be a stingy element. However, krypton will react if a colloidal system is used for electrical sparks
ð Helium, neon, and argon are more difficult to react and have not yet made a compound.
ð Helium is the lightest element, so it is used for balloon filler and tube diver
ð Colored lights are used from krypton and xenon elements.
The colors of the noble gas elements
Helium = colorless, but in orange red lights
Neon = red
Argon = pink (low pressure) and blue (high pressure)
Krypton = bluish white
Xenon = blue
Radon = radioactive rays (alpha, beta, and gamma).

D. Usefulness of noble gases
ð Helium
As an air balloon charger because helium is a substance that is light and not easy burning. At first the balloon air filler is Hydrogen. Although equally light it turns out Hydrogen is highly flammable. As a mixture of oxygen in the diver tube because in high pressure helium is not soluble in the blood. When using ordinary air containing Nitrogen then when the dive pressure becomes high and Nitrogen becomes soluble in the blood. When the diver returns to the surface the pressure becomes lower causing the solubility of Nitrogen in the blood is reduced and out of the blood. This causes severe and dangerous pain. Helium in the form of liquid can also be used as a coolant because it has a very steam point that is very low.

ð Neon
Neon is usually used to fill fluorescent lamps. Neon can be used to share things like high-voltage indicators, refrigerants, lightning rods, and television tubes. Liquid fluid is a refrigerant in the refry generator for low temperatures. Neon can also be used to signal the aircraft because its rays can penetrate the fog.

ð Argon
Argon can be used in titanium welding and stainless steel. Argon is also used as an incandescent light bulb because in high temperatures Argon does not react with the wire / tungsten so that the lamp wire does not break fast.

ð Krypton
Krypton with argon is used as a low pressure fluorescent lamp filler.
Krypton is also used in flash for high speed photography.
ð Xenon

Xenon can be used in the manufacture of incandescent lamps for bactericide (bacteria killer). Xenon is also used in the manufacture of electron tubes.

Sabtu, 20 Mei 2017

RPP K13 on Chemicals: Atomic Model and Periodic System

School                     : SMAN 2 SAROLANGUN
A.  Subjects                   : Chemistry
B.   Class / semester     : X MIA / 1
C.  Basic Material        : Atomic Model and Periodic System
D.  Time allocation      : 6 meetings x 3 hours Lesson (18 Hours Lesson)
E.   Learning objectives    :
After observing the environment, reading the developmental articles and applications of chemistry students can understand and realize the nature, the importance of the role of chemistry in life, the scientific method and work safety.
F.   Basic competencies:
1.   Recognizing the orderliness of the structure of material particles as a manifestation of the greatness of God YME and the knowledge of the structure of matter particles as the result of human creative thinking whose truth is tentative.
2.  Shows scientific behavior (curiosity, discipline, honest, objective, open, able to distinguish facts and opinions, resilient, meticulous, responsible, critical, creative, innovative, democratic, communicative in designing and conducting experiments and discussions embodied in Everyday attitude.
3.  Demonstrate co-operative, courteous, tolerant, peace-loving and caring about the environment and cost-effective in utilizing natural resources.
4. Demonstrate responsive, and proactive and wise behavior as a form of problem-solving ability and decision making.
5.   Analyze the development of the atomic model.
6.  Analyzing atomic structure based on Bohr's atomic theory and quantum mechanical theory.
7.   Analyze the relationship of electron configuration and orbital diagrams to determine the location of elements in the periodic table and the periodic properties of the elements.

G.            Indicators of achievement of competence:
1.   To mention the existence of the order of the structure of material particles as a manifestation of the greatness of God YME and the knowledge of the particle structure of matter as the result of creative human thought which is tentative.
2.   Behave scientific (have a curiosity, discipline, honest, objective, open, able to distinguish facts and opinions, resilient, meticulous, responsible, critical, creative, innovative, democratic, communicative in designing and conducting experiments and discussions embodied in Everyday attitude.
3.   Can cooperate, courteous, tolerant, love peace and care for the environment and efficient in utilizing natural resources.
4.  Be responsive, and proactive and wise as a form of problem-solving ability and make decisions.
5.  Determining elementary particles of atoms (protons, electrons and neutrons)
6. Determining relative atomic mass based on periodic table.
7.  Classify the elements into isotopes, isobars and isotons.
8.  Explain the development of atomic theory to show the weaknesses and advantages of each atomic theory.
9. Explain the difference Bohr's atomic structure and quantum mechanics.
10.          Describe an orbital diagram.
11.  Determine the electron and the valence electron configuration.
12.           Determining the location of classes and period elements in the periodic system based on the electron configuration.
13.           Explain the tendency 4 The nature of the periodicity of the elements in the periodic table


H.        Learning materials:
v atomic number and mass number
v Isotopes, isobars, isotons
v The development of the atomic model
v Bohr and atomic structures
v Bohr electron configuration
v Atomic structure of quantum mechanics.
v Quantum numbers
v Configuration of electrons of quantum mechanics
v Groups and periods
v Orbital diagrams
v The nature of the nature of the elements
v  Orbital shape

I.         Learning method: Scientific, discovery, problem solving
J.      Learning media:
Learning resources: BSE chemistry book Class X
Print media: Magazines, newspapers
Electronic media: Internet articles
K.    Learning steps:
Meeting 1 (3 Hours Lessons = 135 minutes)
Atomic number, mass number, isotope, isobar, isoton
Stage
Activities
Time
preliminary      
  ü Pray with the students
  ü Saying greeting
  ü Checking student attendance
  ü Gathered assignments last week
  ü Listening to the Basic Material / Competence to be studied
  ü Listening to the Learning Method information that will be used
  ü Divide the group
  ü Give homework:
1.     Create concept maps about the development of the atomic model
2.    Summarize how to determine the number of electrons, protons and neutrons
3.    Make a summary of how to determine isotopes, isobars and isotons
15 minutes
Core
·   Observe
Ø Observing atomic particles and their relation to mass numbers and atomic numbers.
Ø Observe the modern periodic table
Ask
1. What are the atomic particles?
2. Where is the position of electrons in the atom?
3. How to specify atomic element number?
4. How to specify the element mass number?
5. Shows what, atomic element number?
6. Shows what, elemental mass number?
7. How to determine the number of proton elements?
8. How to determine the number of element electrons?
9. How to determine the number of neutron elements?
10. What dimadsud with isotopes, isobars and isotons!
    11. Why is the atomic model evolving?

Data collection
ØObserve the atomic number and mass number of several elements to determine the number of electrons, protons and neutrons of the element.
Ø Analyzing the atomic number and mass number of some case examples on elements to understand isotopes, isobars, and isotons.
90 minutes
End
Gathering assignments
ØConcept map about the development of atomic model.
Ø A summary of how to determine the number of electrons, protons and neutrons
ØA  summary of how to determine isotopes, isobars and isotons
Formative Test Written
5 minutes



25 minutes
L.   Assessment of learning outcomes:
1)  Affordable
With Observation
Attitude assessment sheets Attitude during discussions and presentations
2) Cognitive
Task
Create a concept map about the development of the atomic model
Summarize how to determine the number of electrons, protons and neutrons
Make a summary of how to determine isotopes, isobars and isotons

è Affective
With Observation
Attitude assessment sheets Attitude during discussions and presentations.
è Cognitive
Task:
Create a concept map about the development of the atomic model
Summarize how to determine the number of electrons, protons and neutrons
Make a summary of how to determine isotopes, isobars and isotons

è Written Format:
Question :
üHow to determine atomic number and mass number?
ü How to determine the number of electrons, protons, and neutrons of an elemental atom?
üHow to determine isotope, isobar and isoton?
è Psychomotor
Skills Assessment Sheet