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Turn in homework (78, 1-6) and test corrections in box

Turn in homework (78, 1-6) and test corrections in box Objectives : Name and describe the  mass and charge of the subatomic particles. Find the number of protons, neutrons, and electrons in typical atoms. Catalyst 11/1/10.

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Turn in homework (78, 1-6) and test corrections in box

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  1. Turn in homework (78, 1-6) and test corrections in box Objectives: Name and describe the  mass and charge of the subatomic particles. Find the number of protons, neutrons, and electrons in typical atoms. Catalyst 11/1/10 1. Given the information in the chart, if a student were to apply heat to equal volumes of all four liquids along with a volume of water, which liquids would boil before the water? A. Q and S B. R and T C. Q and R D. S and T2. If a student is performing an experiment that requires a liquid that has a density less than water, has a higher boiling point than water, and has a distinctive odor, which of the liquids on the chart would be best to use? A. Q B. R C. S D. T

  2. Agenda • Subatomic Particle Notes (15-30) • Ion and Isotope Notes (30) • Homework: • Write the Name, Symbol, atomic mass, atomic number, # protons, # neutrons and # electrons of the first 20 elements

  3. Homework:

  4. Dalton’s Atomic theory • Support for his theory came when he began looking at the masses of elements that combined with each other. • He found that elements combine in simple ratios by mass.

  5. Dalton’s atomic theory • Dalton’s atomic theory • all matter is composed of tiny, indivisible particles called atoms. • All atoms of the same element are identical in properties • Atoms of different elements differ in properties. • Atoms can neither be created nor destroyed. • Atoms of two or more different elements can combine in small whole number ratios to form compounds.

  6. Dalton’s atomic theory • 2 problems with his theory: • Atoms of the same element can have different masses • atoms have subatomic particles (electrons, protons and neutrons) So Dalton’s theory is not completely correct.

  7. Two major parts of an atom Nucleus (not to scale) Electron Cloud

  8. Three Major Sub-Atomic Particles • Protons • Neutrons • Electrons

  9. PROTON (p+) a single, relatively large particle with apositive charge that isfound in the nucleus

  10. p+ THE PROTON • Fat (heavy) • Positive (charge) • Doesn’t move (lazy)

  11. NEUTRON (N°) a single, relatively large particle with aneutral charge that isfound in the nucleus

  12. N° THE NEUTRON • Fat (heavy) • Neutral (charge) • Doesn’t move (lazy)

  13. ELECTRON (e-) a single, very small particle with anegative charge that isfound in a “cloud” around the nucleus

  14. e- THE ELECTRON • Skinny (very light) • Negative (charge) • Moves a lot (runs around)

  15. Where are they located? Nucleus: Protons and Neutrons Electron Cloud: Only Electrons

  16. Atoms to Elements • What makes elements different from one another? • The number of protons! Also called the atomic number.

  17. Chemical Symbols • Elements have a single capitalized letter for their symbol or have two letters-the first is capitalized and the second is lower case.

  18. the number of protons in an atom ATOMIC NUMBER (Z)

  19. ATOMIC MASS # (A) The total mass of all of the subatomic particles in an atom (but really # of protons and neutrons)

  20. ELEMENTS Elements are electrically neutral. (They have the same # of p+ and # of e-)

  21. Example: Sodium Atomic Mass # = p+ & N° 22.99 Round this number to the nearest whole number!!! Na 11 Atomic # = # of protons

  22. Another Notation Atomic Mass # = p+ & N° Atomic # = # of protons

  23. To calculate the number of neutrons, subtract the atomic number (smaller) from the atomic mass number (larger)A – Z = # of neutrons

  24. Ex: How many neutrons does Sodium have? Mass # - Atomic # = #N° (You may need to round the atomic #) 22.99 23 - 11 = 12 N° Na 11

  25. Atomic Mass Symbol Atomic Number

  26. Hydrogen Protons: 1 Neutrons: 0 Electrons: 1 H 1 1

  27. Sodium Protons: 11 Neutrons: 12 Electrons: 11 Na 23 11

  28. Rhenium Protons: 75 Neutrons: 111 Electrons: 75 Re 186 75

  29. Homework:

  30. ION Atoms of the same element that differ in charge.(They have the same # of p+, but different # of e-)

  31. Ex: How many electrons does Sodium have? The atomic number equals the number of protons and the number of electrons. 22.99 11 electrons Na 11

  32. Negative Ions(anions) Positive Ions(cations) • Na+ (lost 1 e-) • Ca2+ (lost 2 e-) • Al3+ (lost 3 e-) • Pb4+ (lost 4 e-) • H+ (lost 1 e-) • Cl- (gain 1 e-) • O2- (gain 2 e-) • P3- (gain 3 e-) • S2- (gain 2 e-) • OH- (gain 1 e-)

  33. If an atom GAINS electrons, its overall charge becomes more negative.If it LOSES electrons, its charge becomes more positive

  34. Learning Check – Counting State the number of protons, neutrons, and electrons in each of these ions. 39 K+16O -241Ca +2 19 8 20 #p+ ______ ______ _______ #no ______ ______ _______ #e- ______ ______ _______

  35. ISOTOPE Atoms of the same element that differ in mass.(They have the same # of p+, but different # of N°)

  36. Isotopes are CHEMICALLY the SAME as atoms, but DIFFER PHYSICALLY because they have different masses.

  37. A few examples of isotopes…

  38. Learning Check – Counting Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12C 13C 14C 6 6 6 #p+ _______ _______ _______ #no _______ _______ _______ #e- _______ _______ _______

  39. Answers 12C 13C 14C 6 6 6 #p+666 #no678 #e- 6 66

  40. One Last Learning Check Write the nuclear symbol form for the following atoms or ions: A. 8 p+, 8 n, 8 e- ___________ B. 17p+, 20n, 17e- ___________ C. 47p+, 60 n, 46 e- ___________

  41. So, why do the elements on the PT have masses with decimals???

  42. The periodic table has the average atomic mass of all of the isotopes of a substance

  43. 11B 10B AVERAGE ATOMIC MASS • Because of the existence of isotopes, the mass of a collection of atoms has an average value. • Boron is 20% 10B and 80% 11B. That is, 11B is 80 percent abundant on earth. • For boron atomic weight = 0.20 (10 amu) + 0.80 (11 amu) = 10.8 amu

  44. Average atomic mass is calculated by: • Mass each isotope and multiply by amount • Add calculations for each isotope • Divide sum by the total amount

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