to explain:redoks reactions

Redox reactions
A redox reaction is a reaction involving a reduction reaction and an oxidation reaction. The meaning of the oxidation reaction and the reduction reaction develops in accordance with the development of chemistry. Reduction reactions and oxidation reactions occur in everyday life, such as combustion reactions, vinegar making from alcohol, glucose breaking events in the body, iron filings, and so on.

Understanding Redox Reactions
Initially the concept of reduction and oxidation (redox) is limited to reactions involving the release and binding of oxygen. The oxidation reaction is the reaction of oxygen binding by a substance.

Oxidation and Redox Reactions
The more universal concept of redox reactions to explain reactions involving covalent compounds is the concept of redox reactions based on changes in oxidation numbers.
The redox reactions that are difficult to explain with the concept of oxygen and the concept of electrons can be easily explained using the concept of oxidant numbers.
Oxidation number
The oxidation or oxidation state of an element is a positive or negative integer given to an element in forming a compound. The oxidation number of an element is determined by considering the following.
A) The ionic compound
The oxidation number of elements in monoatomic ions is the real charge of the compound ions.
Example:
The NaCl compound, formed from Na + and Cl- ions, then the oxidation number of Na atoms in NaCl is +1, and the oxidation number Cl is -1.
B) Covalent compounds
The thing to note in determining the oxidation number in the covalent compound is the price of the electronegativity scale of each of the constituent atoms.
The atomic elements having a higher electronegative scale value indicate that the attraction of the atoms to the bonding electron pair is stronger. Because it is stronger to attract an electron pair, it becomes negative, and therefore the oxidation number is given a negative number. Atoms that have lower electronegativity prices are given positive oxidation numbers.
Example:
HCl compounds are formed from hydrogen atoms (electronegativity H = 2.0) and chlorine atoms (electronegativity Cl = 3.0) by using a common electron pair. These joint electrons are more attracted to Cl atoms, then the chlorine atom is oxidized -1, whereas the hydrogen atom is given the +1 oxidation number.

Determination of oxidation number
To determine the oxidation number of suatau atoms in a compound can be used some of the following provisions.
1. The oxidation number of free element (not compound) is 0 (zero).
2. The number of algebraic oxidation numbers of all atoms in a compound is 0 (zero).
3. The number of algebraic oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion.
4. Certain elements in forming compounds have certain oxidation numbers, for example:

    Group IA atoms (Li, Na, K, Rb, Cs, and Fr) in the compound have +1 oxidation states.
    Group IIA atoms (Be, Mg, Ca, Sr, and Ba) in the compound have a +2 oxidation number.
    Class IIIA (B, Al, and Ga) atoms in the compound have +3 oxidation numbers.
    The hydrogen atom (H) in the compound generally has a +1 oxidation number, except in the metal hydride. Metal hydrides are compounds formed from metal and hydrogen elements. In metal hydrides, such as LiH, NaH, CaH2, MgH2, and AlH3, the hydrogen atom is given a -1 oxidation number.
    The oxygen atom (O) in the compound generally has an oxidation number of -2, except in the peroxide compound and OF2.

In peroxides, such as H2O2, Na2O, and BaO, the oxygen atoms are given the oxidation number -1, whereas at OF2 is given a +2 oxidation number

Redox reactions
A redox reaction is a reaction involving a reduction reaction and an oxidation reaction. The meaning of the oxidation reaction and the reduction reaction develops in accordance with the development of chemistry. Reduction reactions and oxidation reactions occur in everyday life, such as combustion reactions, vinegar making from alcohol, glucose breaking events in the body, iron filings, and so on.

Understanding Redox Reactions
Initially the concept of reduction and oxidation (redox) is limited to reactions involving the release and binding of oxygen. The oxidation reaction is the reaction of oxygen binding by a substance.

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LEARNING IMPLEMENTATION PLAN (RPP)

IDENTITY High school Subject: Chemistry Class / Semester: X / 1 (one) Time Allocation: 3 hours of lesson A.     CORE COMPETENCY KI 1 KI 2 KI 3 KI 4 : Living and practicing the religious teachings it embraces : Living and practicing honest, disciplined, responsible, caring (polite, cooperative, tolerant, peaceful) behavior, courteous, responsive and pro-active and showing attitudes as part of the solution to problems in interacting effectively with the social and natural environment and In placing themselves as a reflection of the nation in the association of the world. : Understanding, applying, analyzing factual, conceptual, procedural knowledge based on his knowledge of science, technology, art, culture, and humanities with the insights of humanity, nationality, state and civilization on the causes of phenomena and events, and applying procedural knowledge to the field of study Which is specific to his or her talents and interests to solve problems. : Processing, reasoning, and recruiting in the realm of concrete and abstract realm related to the development of the self-study in the school independently, and able to use methods according to scientific rules. A.     BASIC COMPETENCE AND INDICATORS Kompetensi Dasar Indikator 3.6 Determining the shape of molecules by using the theory of electron valence shunt pair (VSEPR) or Electron Domain Theory 1. Explain the theory of electron domains 2. Applying the theory of electron domains in determining the shape of molecules 3. Explain the theory of electron valence skin pair reaction (VSEPR) 4. Determining the form of molecules based on the theory of electron valence skin rejection (VSEPR) 5. Determining the nature of polarity based on molecular form 4.6 Make a model of molecular shape by using materials in the environment or chemical software 1. Applying the electron domain theory to predict the shape of the molecule 2. Make a molecular shape by using a balloon 3. Communicate the results of discussions about the molecular form. C. LEARNING MATERIAL 1. Electron Domain Theory 2. Theory of Electrical Couple Calls (VSEPR) 3. Molecular shape D.  LEARNING ACTIVITIES 1.  First Meeting: (3 JP) Indicator: 3.6: 1. Explain the theory of electron domains 2. Applying the theory of electron domains in determining the shape of molecules 3. Explain the theory of electron valence skin pair reaction (VSEPR) 4. Determining the shape of molecules based on the theory of repulsion of electron valence skin pair (VSEPR) 5. Determining the nature of the celiber based on the form of molecules 4.6: 1. Applying the electron domain theory to predict the shape of the molecule 2. Make a molecular shape by using a balloon 3. Communicate the results of discussions about the molecular form. A. Activity Introduction  Teachers greet, pray, check student attendanceü  Apperception:ü 1. Delivering GPA 2. Questions about covalent bonds, image impressions between water in glass and carbon dioxide gas.  Motivation: Observing images of CH4 molecular shapes;ü H2O; NH3 and CO2 B.  Core activities No. Sistax / Stages of Learning Description of Learning Activity 1. Stimulation (giving stimulus) • Given 4 images of molecular forms of compounds H2O, CO2, NH3 and CH4. • Students observe the molecular form of several compounds through images / molymod / animation. 2. Problem Statement • Students are expected to ask: - why are the four molecules of the four compounds different? - How to determine the molecular shape of a compound? - What is the relationship between molecular form and the polarity of the compound? 3. Data Callecting • Students review the literature on electron domain theory and VSEPR theory • Students conduct group discussions to conclude electron domain theory and VSEPR theory • Students conduct class discussions of literature review and group discussion to equate perceptions about electron domain theory and VSEPR theory • Review the literature to predict the shape of molecules and relate the relationship of molecular shapes to the polarity of the compound. 4. Data Proccesing • Students work on LKS about molecular form by way of group discussion 5. Verification • Students can understand the shape of molecules through information discussions with teacher guidance 6. Zeneralication • Students can define molecular shapes based on electron domain theory and VSEPR theory • Students can determine the polarity of the compound based on the molecular shape C. Closing Activity  Students do the exercises about the material being studied.ü  Students are assigned to create molecular models of materials in the surrounding environment or chemical softwareü D.  TECHNICAL  ASSESSMENT 1. Knowledge: Written Problem PG and Description (Attached) 2. Skills: Performance makes the molecular shape of the balloon 1.       ASSESSMENT TECHNIQUE 1. Knowledge: Written Problem PG and Description (Attached) 2. Skills: Performance makes the molecular shape of the balloon F. Media / tools, Materials, and Learning Resources 1. Media / tools: molymode, LKS and Power Point 2. Material: balloon 3. Learning Resources: Chemical Handbook volume 1 and relevant supporting books 1.      Attachments: 1. Learning Materials 2. Assessment Instruments 3. LKS REFLECTION: After doing LK 2 we can determine: 1. RPP 2. Learning models that are applied to learning activities 3. Assessment of psychomotor knowledge and assessment that will be done to measure the achievement of GPA Appendix 1: Learning materials To understand the VSEPR theory we use balloons, when tied between two balloons, the balloon will form linearly, if three or four balloons form a flat or tetrahedral triangle. The shape of the molecule can be estimated using the Lewis structure. For example the Lewis ammonia structure: With three electron pairs attached and a pair of free electrons, then according to the electron domains, they are arranged in tetrahedral form, but that is less precise because of the magnitude of repulsions between H atoms, by repulsion between H atoms and electron pairs it is not as large, Calculated in a separate way, so the right shape is a pyramid. The basic shape of a molecule is determined by the number of pairs of electrons present in the central atom. There are five basic molecular shapes of a compound, namely: 1. Linear 2. Flat Triangle 3. Tetrahedral 4. Trigonal Bipiramida 5. Oktahedral The molecular forms are symmetrical, if a compound having the number of electron pairs in the central atom is the same as the basic molecular form, but has a different shape. This is due to differences in the composition of PEI and PEB of the electron pairs present in the central atom. So that the basic (symmetrical) molecular shape is distorted into different and unsymmetrical molecular shapes. MOLECUL FORM Table Relationships between PEI, PEB, molecular form and examples and drawings   The concept of electron domain theory Find the following molecular form based on PEI and PEB, write the molecular form in the following table!            PEB PEI 1 2 3 2 3 4 5 6   By reading Table Relationship between PEI, PEB, molecular form and examples and drawings Try to assemble molecular compounds using mollymood and draw the results in the following table! NO Chemical formula Number of PEI Number of PEB formula Molecul form 1 CO2 2 BH3 3 CH4 4 PCl5 5 SF6 Forecasting Molecular Form To predict the shape of the molecule, first determine the central atom (A), the number of bonded atoms (X), PEB (E), number PEI (n), and amount PEB (m). Using notation: AXnEm Appendix 2: Assessment Instruments A. The Formulation of Knowledge Problems IndicatorSoal HOTS/LOTS (Low Order Thinking Skiils) Sour Formula • Determine the form of the molecule of its members by the electronic domain theory • Determine the form of molecules by the amount of PEB a compound • Given 2 data atomic number, can determine the shape of molecule • Determine the form of molecules of PEB compoundamonium • Determine the positions of PEB to form octahedral molecules • Determining the form of molecules based on Types / Rumms compounds • Describe electron and VSEPR domain parameters • Diyikandatano atom, candementukmolekul form for some of the data • Classify the polar and non polar HOTS HOTS HOTS HOTS HOTS HOTS LOTS HOTS HOTS 1. According to the theory of domainelektron form molecule compound CH4 Is a .... A. Triangle pelanar B. The trigonal pyramid C. Tetrahedral D. Triangle bipiramida E. Rectangular flat 2. The number of pairs of central atoms of a molecule of compound = 3, while the free electron pair = 0, then the form of the molecules A. Oktahedral B. Equal triangle C. Tetrahedral D. Bipyramide triangle E. Linear 3. The atomic number P is 15, whereas Br is 35, the form of the molecule PBr5 is A. tetrahedral B. equilateral triangle C. trigonal bipiramida D. trigonal pyramid E. squares 4.Alumunium chloride, AlCl3 danamonia, NH3, are covalent molecules. What is the molecular form of ammonia and the number of free electron pairs respectively; A. Trigonal pyramid, 1 B. Trigonal pyramid, 3 C. Equivalent triangle, 1 D. equilateral triangle, 2 E. Planar Triangle, 1 5. In octahedral form, the first free electron pair can occupy any position. Where is the position of the second free electron pair ... A. 45o from the first PEB B. 60o from the first PEB C. 90o from the first PEB D. 180o from PEB E. Adjacent 6. If the central atom is denoted by X, the domain of the bonding electron with Y and the free electron domain with E, then the following molecule having the type XY4 is A. CO2 D. CH4 B. H2O E. SO2 C. NH3 Description: 1. Explain the notion of basic concepts of electron domain theory and VSEPR! 2. Draw the Lewis structure and determine the number of PEI, PEB and molecular forms of the following compounds! (Atomic number H = 1, B = 5, Cl = 17, N = 7, S = 16, F = 9, I = 53) A. BCl3 B. Ccl4 C. NH3 D. SF6 3. Of the following compounds described the compounds belonging to polar and non-polar H2O, CO2,, NH3, PCl5 ddan CH4 B. Observation sheet and presentation performance OBSERVATION OBSERVATION SHEET AND PRESENTATION PERFORMANCE Subject: Chemistry Class / Program: X / M-IPA No Student name Observation Presentation Performance amount Score score Akt Disl Kerjsm Prnsrt Visual Isi (1) (2) (3) (4) (5) (6) 1.        2.        3.        4.           Description of filling the score 4 = Very high 3 = Height 2 = High enough 1 = Less   Appendix 3:   LKS Short Theory: As an analogy of the molecular form based on the electron pair's repulsive theory try to make models of molecular forms with balloons. Work steps: 1. Blow 20 balloons with almost the same size. 2. Make a balloon bond, each 2, 3, 4, 5, and 6 balloons. Tie the balloon tightly, so that one another refuses. 3. Observe the geometric shape of each bond and draw the structure                                         Picture the analogy of Molecular Shapes with balloons.   The number of balloons analogizes the number of electrons surrounding the central atom, the molecular shapes depend on the number of electron pairs being repulsed around the atom. Information: A: Central Atom X: PEI E: PEB N: number of PEI M: number of PEB Using the balloon model, consider predicting the molecular form of the compound in the following table:   picture Molecular form Compound examples 1.      Two ballon 2.      Three ballon 3.      Four ballon 4.      five Ballon 5.      six balon  Complete the following table: NO Formula of chemical compound A X n m Molecular form Form Name Characteristic of Kepolaran 1 BeCl2 2 H2O 3 SO2 4 NH3 5 ClF3 6.. CH4 7 TeCl4 8 XeF2 9 IF5 10 XeF4   Answer the following questions: 1. What is PEI and PEB? 2. How many pairs of electron bonds (PEI) in H2O, NH3 and CO2? 3. How many pairs of free electrons (PEB) in H2O, NH3 and CO2? 4. Do you remember about the charge of electrons, What if one electron with another electron approach each other? 5. Describe possible interactions between central and central electrons in water molecules and carbon dioxide! 6. Make conclusions about PEI-PEI interactions; PEI - PEB; PEB - PEB 7. Can you summarize what causes the structure to form in the compound! 8. How is the relationship between the molecular form and the polarity of the compound?