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Name: ___________________________ 19. Define the law of multiple proportions. Elements form compounds in simple whole number ratios 20. What do isotopes of the same element have in common and what is different? Isotopes have the same number of protons, electrons and atomic number Isotopes have a different mass number and number of neutrons 21. Explain how Rutherford’s gold foil experiment worked and what it proved. Rutherford shot particles through gold foil. Most went through, but some bounced back. He concluded that atoms are mostly empty space and the particles bounced off the dense center called the nucleus. 22. What subatomic particle determines the identity of an atom? Protons 23. How do you find the following: A. Number of protons in an atom = __same as the atomic number__ B. Number of neutrons in an atom = __mass # - atomic #__ C. Number of electrons in an atom = __same as the atomic number__ Symbol Atomic Number Mass Number Number of Protons Number of Electrons Number of Neutrons Ag 47 109 47 47 62 Mg 12 24 12 12 12 Ga 31 72 31 31 41 The Periodic Table & Trends: 24. The horizontal rows found on the periodic table are called __periods__, while the vertical columns are called ___groups__ or ___periods___. 25. The most reactive elements on the periodic table are in group __1A – Alkali Metals__. 26. Electronegativity ____decreases_____ (increases/decreases) going down groups and ______increases_____ (increases/decreases) going across periods from left to right. 27. Ionization Energy ______decreases_____ (increases/decreases) going down groups and ______increases_______ (increases/decreases) going across periods from left to right. 28. Atomic radius ________increases______ (increases/decreases) going down groups and _______decreases_______ (increases/decreases) going across periods from left to right. 29. The number of valence electrons ________increases______ as you go across a period, but will ______stay the same____ as you go down a group. 30. The most electronegative element is ________Fluorine_____________. 31. The element with the largest atomic radius is _______Francium______. 32. Which of the following has a bigger atomic radius: Cesium or Calcium? (Circle one.) 33. Which of the following has a higher ionization energy: Potassium or Sulfur? (Circle one.) 34. Classify the following as either an: Alkali Metal, Alkaline Earth Metal, Halogen or Noble Gas A. Strontium __Alkaline Earth Metal____ C. B. Bromine ___Halogen___ D. Krypton Potassium __Alkali Metal___ __Noble Gas____ Electron Configurations & EMR Calculations: 36. Write the long-hand electron configurations AND noble gas notations for the following atoms: A. Calcium 1s22s22p63s23p64s2 [Ar]4s2 B. Iron 1s22s22p63s23p64s23d6 [Ar]4s23d6 37. What do the superscripts add up to in an electron configuration? ____the atomic number___ 38. What is the energy of a photon whose frequency is 6.9 x 1014 Hz? E=hxV E = 6.63 x 10-34 x 6.9 x 1014 E = 4.57 x 10-19 J E=hxv h = 6.63x10-34 J·s 39. What is the packet of light called that is released when an electron relaxes to the ground state? photon Bonding & Ionic Compounds: 40. Name the following compounds: A. BaCO3 _____barium carbonate____ B. NH4OH _____ammonium hydroxide_____ C. NiCl2 _____nickel (II) chloride_____ D. MnCl3 _____manganese (III) chloride____ 41. Write the formula for each of the following compounds: A. Aluminum phosphate ______AlPO4____ B. Copper (III) sulfide _____Cu2S3_____ C. Magnesium chloride _____MgCl2____ D. Potassium nitrate ______KNO3____ 42. Identify each of the following as either an: ionic or covalent bond A. electrons are shared __________covalent_______ B. electrons are transferred _________ionic_________ C. MgCl2 ________ionic_______ D. CO2 _________covalent__________ 43. Why are metals malleable and ductile? _________metals have a “sea of electrons”______