Download Unit 5 Review

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__