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Polarity of Molecules
- 1. POLARITY OF MOLECULE S Prepared by: Najmah Sirad Ampa , LPT, MSciEd(Physics)
- 2. OBJECTIVE: 1.Differentiate polar and nonpolar bonds; 2.Determine the polarity of chemical bonds between atoms using the concept of electronegativity; 3.Familiarize with the different molecular shapes; 4.Explain how polarity of bonds and molecular geometry affects the polarity of molecules.
- 3. MOLECUL ES
- 4. MOLECUL ES It is a group of two or more atoms held together by chemical bonds.
- 5. EXAMPLE OF MOLECULES WATER salT OZONE
- 6. EXAMPLE OF MOLECULES NITROGEN ethYL ALCOHOL SUGAR
- 7. EXAMPLE OF MOLECULES WATER salT OZINE
- 9. HOW TO PLAY? Read the group of unrelated words and solve them into real words/phrases before time runs out.
- 16. GUESS THE GIBBERISH #3 EEL LEAK TRUE NEED GOT THIEVES
- 17. GUESS THE GIBBERISH #3 EEL LEAK TRUE NEED GOT THIEVES BEAT TEA ELECTRONEGATI VITY
- 20. GUESS THE GIBBERISH #5 MALL LET CURE LIAR JAW MEET
- 21. GUESS THE GIBBERISH #5 MALL LET CURE LIAR JAW MEET MOLECULAR GEOMETRY
- 26. It refers to the distribution of electric charge around atoms, chemical groups, or molecules joined by atoms. POLARIT Y
- 27. ï± Electronegativity Difference ï± Molecular Geometry through VSEPR (Valence Shell Electron Pair Repulsion) Theory Factors that determine the POLARITY of molecules
- 28. ï± All compounds can be classified based on what type of chemical bond formed when the atoms combined. ï± The two classification of compounds are âcovalentâ &âionicâ. ï± The classification of compound can be used in determinining whether a molecule is polar or nonpolar molecules POLARITY of the molecules
- 29. Polar molecule ï There is unequal or asymmetrical distribution of electrons among the atoms of a molecule. Polar & nonpolar molecule
- 30. NONPolar molecule ï There is equal or symmetrical distribution of electrons among the atoms in a molecule. Polar & nonpolar molecule
- 31. ïIs a molecule formed by covalent bond in which the atoms share one or more pairs of valence electron. ïAre made of ions in which atoms transfer electrons from one atom to another. Covalent and ionic covale nt ionic
- 33. Tell whether the compound below is an ionic compound (IC) or covalent compound (CC) based on the type of chemical bond present.
- 34. BOND POLARITY Electronegativity ïŒ IS A MEASURE OF HOW STRONGLY ATOMS ATTRACT BONDING ELECTRONS TO THEMSELVES. ïŒ THE HIGHER THE ELECTRONEGATIVITY, THE GREATER AN ATOMSâ ATTRACTION FOR ELECTRON
- 36. EXAMPLE:
- 37. EXAMPLE:
- 38. EXAMPLE:
- 39. Calculate the electronegativity difference and give the type of bond that exists between the atoms in each of the following pairs.
- 40. polarity nonPolar covalent compounds where electrons are shared equally. Polar covalent compounds where electrons are shared unequally. Ionic compounds are highly polar since ions are chargesd atoms.
- 41. MOLECULAR POLARITY ï± For Polyatomic molecules, both the bond Polarity & molecular shape determine the overall molecular polarity. ï± In terms of molecular geometry, the valence shell electron pair repulsiĂłn (VSEPR) theory would help us to determine the spatial arrangement of atoms in a polyatomic molecules.
- 42. BASIC CONCEPTS you need to remember! 1. Lewis electron dot structure (LEDS) 2. Valence shell electron pair repulsion (vsepr) theory
- 43. LEWIS ELECTRON DOT STRUCTURES (LEDS) Valence electrons are represented using a dot around the symbol of the element.
- 44. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 46. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 47. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 48. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 49. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 50. LEWIS ELECTRON DOT STRUCTURES (LEDS)
- 51. Valence Shell electron pair repulsiĂłn (vsepr) theory Key ideas of the vsepr theory: 1. Electron pairs stay as far apart from each other as posible to minimize repulsions. 2. Molecular shape is determined by the number of bond pairs and lone pairs around the atom. 3. Treat multiple bonds as if they were single bonds. 4. Lone pairs occupy more volume than bond pairs.
- 52. You can predict the shape or molecular geometry of a substance using the following steps: Step 1: Determine the central atom of a molecule. The central atom is the least electronegative element. Step 2: Draw the appropriate Lewis dot structure for the molecule. Step 3: Count the number of bonding pairs of electrons and non-bonding (or lone pairs) around the central atom. Step 4: Determine the electron pair orientation using the total number of electron pairs.
- 62. The shape of the molecule is symmetrical. ïŒ Equal sharing of electrons ïŒ Valence electrons are shared equally on both sides of an atom. Polarity using molecular geometry nonpo lar polar The shape of the molecule is asymmetrical. ïŒ Unequal sharing of electrons between atoms.
- 67. CREDITS: This presentation template was created by Slidesgo, including icons by Flaticon, infographics & images by Freepik THAN KS!
Hinweis der Redaktion
- When we say polarity it is the ends. Which ang bawat end ay may may charges. This polarity is the separation of an electric charges which leads a molecule to have a positive and negative charges. Polarity is the equal or unequal sharing of electrons among atoms.
- The two factors that determine the polarity of molecules is through the polarity of the bons between atoms which can be studied based on electronegativity. And the other one is is through the molecular shape of molecules which can be predicted via VSEPR theory.
- This classification of compound can be used in determining whether a molecule is polar or nonpolar.
- VALENCE ELECTRON is the outermost electrons involved in chemical bonding. And ofcors there is a chemincal bonding for the atoms to be stable.
- Remember that in covalent it is SHARING of electrons (by nonmetal vs nonmetal) While the ionic bond is all abount the TRANSFER of electron (by metal to nonmetal)
- Sodium chloride - IC Cardon dioxide - CC Calcium chloride - IC Carbon tetrachloride - CC Iron(III) oxide or ferric oxide - IC Nitrous oxide - CC Phosphorus pentachloride - CC Potassium bromide - IC Hydrogen chloride - CC Aluminum chloride | Aluminum trichloride - IC
- THE HIGHER THE VALUE OF THE ELECTRONEGATIVITY, THE MORE IT TENDS TO ATTRACT ELECTRON TOWARDS ITSELF. Pure covalent is the NONPOLAR covalent. Therefore, less than 0.4 is a nonpolar covalent Between 0.4 and 1.8 is Polar covalent and greater that 1.8 is Ionic
- 2. Ammonia (N-3 & Cl-2.1)=0.9 w/c is between 0..4 and 1.8 therefore it is a Polar Covalent 3. Methane (C-2.5 & H-2.1)=0.4 whic is les tan or equal to 0.4 is a Nonpolar covalent bond 4. H2 92.1-2.1=0 therefore is is also nonpolar 5. wĂĄter= (2.1-3.5=1.4) terefore it is also Polar
- NPCB â there is a bonding of electrons shared equally between two atoms. And there is no charges on atoms. PCB- Bonding of electrons shared unequally between two atoms. There is partial charges on atoms. IB- there is a complete transfer of one or more valence electrons. And there is a full charges on resulting ions.
- Polyatomic molecules are electrically neutral groups of three or more atoms held together by covalent bonds. Aside from electronegativity difference of the atom,we can also determine the polarity of molecules by using the molecular geometry which it is a 3dimensional arrangement of atoms in a molecules.
- Remember that in molecular geometry, the arrangement of the specific number of electron pairs and its corresponding VSEPR shape.
- Remember that in molecular geometry, the arrangement of the specific number of electron pairs and its corresponding VSEPR shape.
- This are the sample of molecular geometry.
- Katong sa angular bent ganina kay 1 lone pair lang pero diri kay duha iyang lone pair.
- Example: Oxygen gas, fluorine gas, chlorine gas, & other diatomic molecules containing atoms of the same elements. As you can see there is no lone pairs in the central atoms because all its electrons are all equally shared to another atoms of the same elements.
- Exapmple is the hydrochloric acid and the hydrofluoric acis. The chlorine and fluorine atoms are more electronegativity than the hydrogen thatâs why the hydrogen is more attractive to chlorinde and fluorine.