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Name KEY______________________________________________________________ Period __________ Unit 6 K Review 15-16 1. An atom’s nucleus consists of which subatomic particle(s)? __protons and neutrons________ 2. Define atom._ the smallest particle of an element that retains the properties of that element_________ 3. Define atomic mass. _ A weighted average of the mass of all the isotopes (varieties) of an atom_______ 4. What did Rutherford discover about the atom? __discovered protons (+) and the nucleus__ 5. What do all atoms of the same element have in common? _# of protons________ 6. The smallest subatomic particle is the __electron_______________________________. 7. Define atomic number. __ equals the number of protons in an element.________ 8. Atoms with the same atomic number are atoms of the same ___element__. 9. Chadwick discovered the __neutron______. 10. What information about an atom can be obtained by looking at the periodic table? Atomic #, atomic mass, #of protons, # of electrons (neutral atom), chemical symbol 11. How many of each subatomic particle are in Uranium-238? P = __92_ N = _146__ E =__92__ 12. Which type of radiation has the greatest penetrating ability? The least? _gamma, alpha_ 13. Which subatomic particles have the same mass? __protons and neutrons____________ 14. Where can we find a naturally occurring form of fusion? ___sun and stars__ 15. Draw an example of Thomson’s model. 16. Sketch a periodic table block for Oxygen. Label the parts. 17. Draw a picture of Bohr’s model of the atom. 18. Which subatomic particle identifies the element? _____proton_______________ 19. Compared to protons and neutrons, electrons have what mass _zero or negligible_? 20. How many protons and neutrons will be in the nucleus of this atom? Protons = __19_______ Neutrons = ___22_____ 41 K 19 21. Describe the relationship between a proton and an electron in a neutral atom. __The number of protons and electrons are equal giving a neutral or zero net charge.______________________ 22. Calculate the average atomic mass of chlorine if its isotopes and % abundances are as follows. Mass of Isotope % abundance Show all work here. 36.9 24.5 % (36.9) (.245) = 9.0405 34.9 75.5 % (34.9) (.755) = +26.3495 35.39 amu 24 23. 12 Mg p =_12__ n = _12__ mass# __24__ atomic # __12___ 24. Nitrogen - 15 p = _7_ n = _8__ mass # __15__ atomic # __7 25. Complete the following reaction and tell what kind of decay is occurring: 232 4 228 90 Th 2 He + 88 _Ra__________ Type of Decay __alpha_______ 26. Describe a beta particle. _negatively charge particle created when a neutron splits into proton_ 27. Define daughter nuclide. _______nucleus after the decay has occurred_____________________ 28. The most mass is lost by an atom during ___alpha_________ decay. Why? It loses 2 protons and 2 neutrons giving it a loss of 4 amu. Gamma and beta have no change in mass.______ 29. Write the reaction for the beta decay of 88 38 Sr 0 -1e + 88 39Y 30. What is the daughter nuclide in question #29? __Yttrium-88________ 31. 238 88 94 Pu 38 Sr + 150 56 Ba what type of nuclear activity is shown? _ _fission_________ 32. Define fission. __Splitting an atom’s nucleus into 2 smaller daughter nuclei._____________________ 33. What is an ion and how is it formed? _A ion is an atom with a charge, formed by gaining or losing electrons. 34. In isotope notation, which number always stays the same? ___atomic number (bottom #) _____________ Explain why. _Protons identify the element and therefore will not change unless the element changes. 35. These subatomic particles can produce unstable isotopes (nuclides) ___neutrons_____ 36. Fill in the following table. Isotope Isotope Notation Nickel-58 Atomic # Protons Electrons Neutrons Mass Number 28 28 28 30 58 15 15 58 28 Ni Phosphorus30 Iodine-127 15 30 15 P 127 53 I 53 53 53 15 30 74 127 37. Use the following table to answer questions a-f. Atom A B C D E F G # of protons 9 9 9 10 10 11 11 # of neutrons 9 10 11 10 11 11 12 a. How many electrons would atom D need to be neutral? __10_____ b. What is the mass number for atom B? __19____ c. What element is represented by atom G? _Na____ d. How many different elements are shown in this table? __3__ e. How many electrons would be needed for atom E to become an anion with a charge of -3? __13___ f. How many electrons would be needed for atom A to have a net charge of + 3? __6__