electronegativity difference greater than or equal to Ionic Bonding occurs between a metal and a nonmetal when there is an

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1 Chemistry Unit 4 Review Packet Sweeeeeeeettt ANSWER KEY For the following compounds identify the bond types as one of the following: Ionic, Metallic, Polar Covalent, Non Polar Covalent, and Moderately Covalent. Hint: SO 4, CO 3, NH 4, OH, and SO 3 are all Polyatomic Ions you may need to use the polyatomic ions reference sheet to identify bond types. 1. CaCl 2 : Ionic Bond 2. CO 2 : Non-Polar Covalent Bond 3. H 2 O: Polar Covalent Bond 4. BaSO 4 : Ionic Bond 5. K 2 O : Ionic Bond 6. Na 2 CO 3 : Ionic Bond 7. CH 4 : Non-Polar Covalent Bond 8. MgO: Ionic Bond 9. NH 4 Cl: Ionic Bond 10. KI: Ionic Bond 11. NaOH: Ionic Bond 12. FeCl 3 : Ionic Bond 13. P 2 O 3: Polar Covalent Bond 14. N 2 O 3 : Moderately Polar Covalent Bond 15. LiBr: Ionic Bond 16. SO 3 : Polar Covalent Bond For the following items show the transfer of electrons for the listed elements if they were to bond. Answer will not bond if it is unlikely that they will bond and explain your reasoning. I apologize for not wanting to draw out the ones I did not provide pictures for below, Your teacher can be lazy sometimes 17. Ionic Bonding occurs between a metal and a nonmetal when there is an electronegativity difference greater than or equal to 1.7.

2 18. Sodium and Chlorine: 19. Potassium and Fluorine 20. Calcium and Oxygen 21. Strontium and Nitrogen 22. Sodium and Phosphorus 23. Rubidium and Selenium N/A via google Images 24. Francium and Nitrogen 25. Lithium and Iodine 26. Beryllium and Carbon DIRECTIONS: For the following Items identify the amount of electrons the atom is trying to give away if the element is a metal. If the Element is a non-metal list the types of covalent bonds that it can make. 27. Carbon: is a non-metal and is capable of forming the following combinations: 4 single bonds; 2 double bonds; 1 single bond and 1 triple bond, 2 single bonds and a double bond. 28. Bromine: Bromine is a Halogen (group 17) and can for 1 single Covalent Bond

3 29. Krypton: is a noble gas (groups 18) and is inert, therefore it does not form any type of bonds under natural circumstances. 30. Magnesium: Is a metal and wants to transfer away 2 valence electrons. 31. Aluminum: Is a metal and wants to transfer away 3 valance electrons. 32. Silicon: Is a metalloid and can bond in the same ways that Carbon can which are as follows: 4 single bonds; 2 double bonds; 1 single bond and 1 triple bond, 2 single bonds and a double bond. 33. Lithium: Is an Alkali Metal and will transfer away 1 valence electron. 34. Chlorine: is a Halogen and is capable of forming one single bond. 35. Silicon: Is listed on here twice My BAD! For the following table fill out the table appropriately. Remember that VSEPR does not work for the structure of Ionic Bonding; Also, don t forget that just because the bond is polar does not mean that the molecule is polar. Compound Ionic or Covalent Molecule Polarity Diatomic Molecule? CH 4 Covalent Non Polar Nope NH 3 Covalent Polar No: Ammonia (Polyatomic Ion) MgCl 2 Ionic Polar (IONIC) No Br 2 Covalent Non Polar YES!! HCl Covalent Polar NO, Strong ACID O 2 Covalent Non Polar YES!! C 6 H 12 O 6 Covalent Non Polar No: Yummmm Sugar!! CO 2 Covalent Non Polar No, Denied N 2 Covalent Non Polar YES!!!!! A molecule is the smallest covalently bonded unit of a compound that still has the properties of that compound. Molecules may be polar or nonpolar depending on the symmetry or asymmetry of charges. Non-Polar compounds have the same charge around the molecule. Polar compounds have a dipole movement throughout the molecule and have opposite charges on opposite ends of the molecules.

4 For the next items Identify how many bonding groups there are Identify how many lone pairs are on the central atom identify the structural shape of the compound identify the molecular shape of the compound If the molecule is Polar draw the molecular shape of the compound and show the Dipole Moment o Dipole Moment: is the measure of net molecular polarity, which is the magnitude of the charge \(Q\) at either end of the molecular dipole times the distance \(r\) between the charges YOU DO NOT HAVE TO CALCULATE THIS, just show it. 36. CO 2 : 2 bonding groups; 0 Lone Pairs; Linear Structure Linear; molecular Shape; Non-Polar Molecule. 37. BrF 5 : 5 bonding groups; 1 Lone Pair; Octahedral structure; Square Pyramidal Molecular Shape, Non-Polar 38. BF 3 : 3 Bonding groups; 0 Lone Paris, trigonal planar structure, Trigonal Planar molecular shape; Non-Polar

5 39. H 2 O: 2 Bonding groups, 2 Lone Pairs; Tetrahedral Structure; Bent Molecular Shape; Polar Molecule Dipole Moment from positive pole to negative pole 40. SF 6 : 6 Bonding Groups; 0 Lone Pairs; Octahedral Structure; Octahedral Shape; Non-Polar Molecule (all bonds are polar but this is not a polar molecule because there is not a negatively charged pole and an oppositely positively charged pole). 41. NH 3 : 3 bonding Groups; 1 Lone Pair; Tetrahedral Structure; Trigonal Pyramidal Molecular Shape; Polar Molecule. 42. CCl 4 : 4 Bonding Groups; 0 Lone Pairs; Tetrahedral Structure and Tetrahedral Molecular Shape; Non-Polar Molecule.

6 43. PF: This was meant to be phosphorus pentafluoride not Phosphorus monoflouride, sorry, this one will not occur naturally. 44. SF 4 4 Bonding groups; 1 Lone Pair; Trigonal Bipyramidal Structure: See Saw Molecular Shape; Non-Polar 45. ClP 3 : 3 Bonding Groups; 2 Lone Pairs; Trigonal Bipyramidal Structure; T- shaped molecular shape; Non Polar Draw the Lewis structures for each of the following. Draw all resonance structures for the compounds. 46. O CHO 2 -

7 48. CO NCO (weird one Cyanate Ion) Sketch a single, double, and triple bond below. Shade and label the hybridized orbital for sigma (σ) and pi (π) bonds accordingly. 50. Single Bond: One single bond can be found in all covalent bonds. In a single covalent bond there is only 1 sigma bond. The sigma bond is the hybridization of the s orbital. I have an image after # 52 to illustrate this 51. Double Bond: In a double bond you will find one sigma bond and one pi bond. A pi bond is the hybridization of the p orbital. 52. Triple Bond: In a triple bond you will find one sigma bond and two pi bonds.