When the atomic mass is taken to be in grams, the amount of the substance present is the mole (6.02 x )

Transcription

1 The Structure of the Atom 1. Atomic Number of an Element The ATOMIC NUMBER of an element is the number of PROTONS in the nucleus of the atom. All atoms of the same element have the same atomic number. The number of protons that an atom has determines what that element is. 2. Atomic mass of an element. The atomic mass of an atom is the sum of the number of protons and the number of neutrons contained in the nucleus of that atom ATOMIC MASS = number of PROTONS + number of NEUTRONS 3. Neutral Atom In a neutral atom, the number of ELECTRONS EQUALS the number of PROTONS. The electron is considered to have negligible mass. 4. Charged Atom Ions are formed by an atom either losing or gaining electrons. Positive Ion. Loss of electrons (Cation) Negative Ion. Gain of electrons (Anions) Ions are written with the normal symbol such as Oxygen O and added in superscript is the charge - O 2-5. Atomic mass in grams Exercise When the atomic mass is taken to be in grams, the amount of the substance present is the mole (6.02 x ) Fill in the blanks for the neutral atom of the following: Element Atomic # # Protons # Electrons # Neutrons Atomic Mass Iron Calcium Iodine Zinc Bismuth If an element contains 34 protons in its nucleus, this element is called. If the number of neutrons is 46 for this element, the atomic mass is. The number of electrons in the neutral atom is. 3. An ion contains 8 protons and 10 electrons, the symbol for this ion is. 4. Element with atomic number 38 contains 36 electrons. What would the symbol be for this ion? 5. An element has 48 protons and 62 neutrons. This element is called. It has an atomic mass of. 6. An element has 10 neutrons and an atomic mass of 18. What is this element. 7. An element contains 17 electrons in the neutral form. Name the element. 8. An element forms a +3 ion and contains 28 electrons and a mass of 70. Name the element and list the number of each of the fundamental particles. P, N, E 1 Sc09 Chemistry Worksheets Printed September 2009

2 Element Symbol Atomic Number # of Protons # of Electrons Atomic Mass (rounded) # of Neutrons (Atomicmass - Atomic #) Hydrogen H Fluorine F Carbon N Al Potassium Cesium Cu Barium Au Bromine Na 2 Sc09 Chemistry Worksheets Printed September 2009

3 Symbols, Subscripts, Coefficients, Brackets BaF 2 - the 2 in this formula is called the subscript. It refers only to the element preceding it. In this case the F (fluorine). 3 BaF 2 - the 3 in this formula is called the coefficient. It refers to each element that follows. In this case there would be 3 Ba (barium) and 3 F 2 (for a total of 6 fluorine). Al(NO 3 ) 3 - in some chemical formulas it is necessary to use brackets. The subscript outside the brackets refers to all the elements inside the brackets. In this example there are: one Al (aluminum), three N (nitrogen), and nine O (oxygen). Example - calculate the number of atoms in each of the following formulas: 1. KCl - one K (potassium) - one Cl (chlorine) total of 2 2. HNO 3 - one H (hydrogen) - one N (nitrogen) total of 5 - three O (oxygen) 3. Al(OH) 3 - one Al (aluminum) - three O (oxygen) total of 7 - three H (hydrogen) 4. 4 K 2 SO 4 - eight K (potassium) - four S (sulphur) total of 28 - sixteen O (oxygen) In your notebooks calculate the # of atoms for each of the following; 1. NaCl 6. 6 H 2 SO HNO 3 7. Si(HCO 3 ) KOH 8. Al(C 2 H 3 O 2 ) 3 4. KMnO Al(CO 2 ) 3 5. K 2 SO B 2 (CO 3 ) 3 3 Sc09 Chemistry Worksheets Printed September 2009

4 List the elements and number present in each of the following compounds; a) NaCl - 1 SODIUM 1 CHLORINE 2 ATOMS TOTAL. b) LiClO 3 - c) KF - d) MgCO 3 - e) SeBr 2 - f) SO 3 - g) Al(OH) 3 - h) BeSO 4 - i) NCl 3 - j) AgBr - k) P 2 O 5 - l) CoCl 2 - m) MnO 2 - n) CoHCO 3 - o) NiF 3 - p) Al 2 S 3 - q) Sr(HCO 3 ) 2 - r) Ga(OH) 3 - s) NH 4 ClO 3 - t) MoPO 4 - u) AuNO 3 - v) CuOH - w) Fe(OH) 2 - x) Cr 2 CO 3 - y) AgCl - z) SnP 4-4 Sc09 Chemistry Worksheets Printed September 2009

5 Draw the Bohr Diagrams for the following elements Hydrogen Helium Lithium Carbon Oxygen Magnesium Chlorine Argon 5 Sc09 Chemistry Worksheets Printed September 2009

6 1. Give the combining capacity for each of the following elements. (if the element has multiple combining capacities, list all.) a) Be h) I o) Na b) Cu I) N p) Fe c) F j) O q) H d) Pb k) P r) Sn e) K l) S s) Mg f) Ca m) Sr t) He g) Al n) Cl u) Ba 2. Write the chemical formula for the compound that results when each of the following elements combine. a) Lithium and Chlorine - Li + + Cl - LiCl. b) Sodium and Chlorine - c) Magnesium and Bromine - d) Potassium and Iodine - e) Hydrogen and Fluorine - f) Calcium and Oxygen - g) Strontium and Chlorine - h) Aluminum and Oxygen - i) Rubidium and Bromine - j) Copper(II) and Iodine - k) Iron(III) and Oxygen - l) Calcium and Bromine - m) Hydrogen and Chlorine - n) Magnesium and Oxygen - o) Calcium and Iodine - p) Hydrogen and Oxygen - q) Sodium and Nitrogen r) Manganese(II) and Arsenic 6 Sc09 Chemistry Worksheets Printed September 2009

7 Oxygen Fluorine Chlorine Sulphur Phosphorous Nitrogen Symbol & Charge Hydrogen ( H + ) H 2 O H + Lithium Beryllium Sodium Calcium Potassium Zinc Aluminum Iron II Iron III Gallium Barium Magnesium Strontium Rubidium Rb 3 N Rb + Symbol & Charge O 2- N 3-7 Sc09 Chemistry Worksheets Printed September 2009

8 Name the following Polyatomic Ions (Radicals) Symbol Charge Name Symbol Charge Name NH 4 1+ Ammonium HCO 3 CO 3 PO 4 OH HSO 4 SO 4 MnO 4 NO 2 SO 3 CH 3 COO C 2 O 4 NO 3 Cr 2 O 7 Use the above list of polyatomic ions and those from the back of your periodic table to identify the chemical formula; 1. zinc sulfate 2. barium chlorate 3. ammonium chloride 4. potassium permanganate 5. sodium bicarbonate 6. ammonium dichromate 7. aluminum hydroxide 8. sodium hydroxide 9. potassium carbonate 10. lead (II) sulphate 11. calcium phosphate 12. copper (II) sulphate 13. hydrogen phosphate 14. iron (II) phosphate 15. calcium carbonate 8 Sc09 Chemistry Worksheets Printed September 2009

9 Name the following compounds; [ Be careful when naming transitional metals with more than one valence - ie. Copper (I) or Copper (II) ] 1. HNO 3 Hydrogen Nitrate 21. NH 4 OH 2. H 3 PO NaHCO 3 3. Na 2 SO K 2 CO 3 4. Mg(OH) CuSO 4 5. Na 2 CO KHCO 3 6. NaOH 26. H 2 SO 4 7. AgNO Al 2 (SO 3 ) 3 8. Al 2 (SO 4 ) AgNO 3 9. KNO Ba(NO 3 ) Ca(OH) Fe(OH) KNO K 2 SO Mn 3 (PO 4 ) HCH 3 COO 13. Al 2 (SO 3 ) CsHCO Pb(OH) LiOH 15. KMnO BaSO NH 4 NO (NH 4 ) 2 SO NaClO Sc(OH) 3 18.Zn(CH 3 COO) Cd 3 N Zn(HCO 3 ) Hg 3 N PbSO SnBr 4 9 Sc09 Chemistry Worksheets Printed September 2009

10 Write the formula for the following; Remember;- non - metal portion of the compound name ending in ATE usually means that a radical is involved (ie. Nitride is the ion N 3-, whereas Nitrate is the radical NO 3-1. zinc oxide Zn 2+ + O 2- ZnO 2. calcium fluoride 3. barium sulfate 4. silver chloride 5. zinc nitride 6. copper (I) oxide 7. sodium iodide 8. cadmium oxide 9. calcium chloride 10. hydrogen sulfide 11. potassium chloride 12. mercury (II) oxide 13. iron (III) sulfide 14. mercury (I) sulfide 15. tin (IV) bromide 16. aluminum oxide 17. zinc sulfate 18. barium chlorate 19. calcium phosphate 20. copper (II) sulfate 21. hydrogen phosphate 22. iron(ii) phosphate 23. calcium carbonate 24. mercury (I) phosphate 25. ammonium nitrate 10 Sc09 Chemistry Worksheets Printed September 2009

11 Write the formula for the following compounds: 1. Sodium Chloride 26. Mercury (I) Bicarbonate 2. Calcium Nitrate 27. Aluminum Sulphate 3. Lead (II) Hydroxide 28. Radium Phosphate 4. Magnesium Chromate 29. Sodium Dichromate 5. Barium Fluoride 30. Iron (II) Sulphate 6. Potassium Sulphate 31. Cadmium Bisulphite 7. Silver Chlorate 32. Silver Nitrate 8. Aluminum Acetate 33. Magnesium Oxide 9. Mercury (I) Sulphate 34. Beryllium Permanganate 10. Lithium Carbonate 35. Hydrogen Chloride 11. Copper (II) Hydroxide 36. Potassium Sulphide 12. Tin (IV) Sulphate 37. Aluminum Oxide 13. Calcium Fluoride 38. Hydrogen Sulfate 14. Hydrogen Nitrate 39. Lead (IV) Hydroxide 15. Potassium Oxide 40. Cobalt (II) Chloride 16. Francium Hydroxide 41. Sodium Bicarbonate 17. Sodium Phosphate 42. Strontium Iodide 18. Strontium Nitrite 43. Cobalt (II) Hydroxide 19. Hydrogen Phosphate 44. Iron (III) Dichromate 20. Silver Sulphide 45. Tin (IV) Carbonate 21. Magnesium Chloride 46. Lithium Iodide 22. Calcium Bicarbonate 47. Mercury (I) Acetate 23. Hydrogen Sulphite 48. Ammonium Dichromate 24. Zinc Bisulphite 49. Ammonium Phosphate 25. Calcium Iodide 50. Mercury (II) Bisulphate 11 Sc09 Chemistry Worksheets Printed September 2009

12 1. carbon monoxide 2. carbon dioxide 3. sulphur monoxide 4. carbon tetrachloride 5. water 6. dichlorine heptoxide 7. selenium tetrachloride 8. dinitrogen pentaphosphide 9. phosphorous pentafluoride 10. chlorine tetraoxide 11. nitrogen monoxide 12. methane 13. disulphur decafluoride 14. diphosphorous pentaselenide 15. iodine dioxide 16. ammonia 17. carbon tetrachloride 18. tetraphosphorous heptasulphide 19. sulphur tetrafluoride 20. tetrasulphur tetranitride 21. dinitrogen trioxide 22. selenium tetrabromide 23. iodine dioxide 24. dinitrogen monoxide 26. S 2 O NO PI P 2 I CO 31. S 4 N C 2 Cl SO SF SCl N 2 P C 2 Br NH NO 40. S 4 N IF ClF 43. SF P 4 O PCl CO ClO CS CH sulphur monoxide 50. CCl 4 12 Sc09 Chemistry Worksheets Printed September 2009