Download Chapter 11 and 12-2 Review/Study Guide for Test

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Chapter 11 and 12-2 Review/Study Guide for Test
1. List the major discovery or accomplishment associated with of each of the following
scientists:
a. Democritus – named the atom, stated it was indivisible
b. Dalton – atom is positively charged sphere
- said atoms of different elements are different, atoms of the same element are
the same
c. Thomson – discovered electron , known for plum pudding model
d. Rutherford – Gold Foil Experiment, discovered nucleus, atom is empty space
e. Bohr – said electrons follow definite paths around nucleus
2. How can you distinguish between isotopes? By their mass numbers à # neutrons
3. What is an isotope? When atoms of the same element have a different number of neutrons
4. What determines the identity of an element? The atomic number (# of protons)
5. How do you calculate the atomic mass of an element? Weighted average of the mass
numbers of all the isotopes. You can also add the protons + neutrons for a single atom
6. What is an atom? The smallest particle into which an element can be divided and still be
the same substance
7. Why do scientists say that most of the mass of an atom is located in the nucleus? Nucleus
contains protons and neutrons, which each have a mass of 1 (which is very large!)
8. Honors only: Calculate the atomic mass of silver, which occurs naturally as 52 percent silver107 and 48 percent silver-109. Show your work. Round to the nearest hundredth.
(.52 x 107) x (.48 x 109) = 55.64 + 52.32 = 107.96 amu
9. State the charge, location and mass of each of the particles found in an atom.
Proton
Neutron
Electron
Charge
Positive
0
negative
Location
In nucleus
In nucleus
Outside Nucleus
Mass (amu)
1
1
0
10. Draw a Bohr diagram for Boron-11. (ß Hint: It’s an isotope!)
P=5
E=5
N=6
(drawing has 5 electrons on the outside, 2 on the first shell, 3 on 2nd)
* 1st shell holds 2 electrons, 2nd shell holds 8 electrons, 3rd shell holds 18 electrons. (general rule)
11. What is a strong force? The force keeping the nucleus together.
12. Fill in the missing parts of the chart.
Element
Atomic
Isotope Name
Symbol
Mass
Mass
Number
Atomic
Number
# of
Protons
# of
Neutrons
# of
Electrons
C
Carbon-15
15
15
6
6
9
6
Co
--------------
58.9332
59
27
27
32
27
Ga
--------------
69.723
70
31
31
39
31
Na
Sodium-25
25
25
11
11
14
11
13. Explain the difference between a group and a period on the periodic table of elements.
Groups = columns (there are 18 total) and Periods = Rows (there are 7). Also, a group shares
similar properties.
14. Why are neither the alkali metals nor the alkaline-earth metals found uncombined in
nature? They have one and two valence electrons on the outer shell. Because they do not
have a complete shell with 8 electrons, they need to bond with other atoms making them
VERY REACTIVE!
15. Why is the element hydrogen not part of a group?
- It is a nonmetal
16. Draw the trend in reactivity in the periodic table below, then label the valence electrons.
ß-------------------------------------------------------------à
Reactivity (stops at noble gases)
Groups
Metalloids - red
Alkaline Earth - blue
Halogens - green
Transition Metals - yellow
Alkali Metals - pink
Noble Gases – purple
*See your colored table or quizlet for
answers
17. Which two groups are gases at room temperature? Noble gases and halogens
18. Which group has the highest reactivity? Alkali Metals
19. Which group is not reactive at all? Noble Gases
20. Color each group on the periodic table based on the list above. Have a partner quiz you
on identifying the locations of each group/family.
*You will not be asked about Lanthanides and Actinides