Unit 3: Atomic Structure
Possible Pts.
Name:___________________________
Practice
Test A
Hr:_________
Score
Possible Pts.
Objective 1
30
Objective 4
20
Objective 2
50
Objective 5
30
Objective 3
60
Objective 6
35
Score
Total
Obj. 1: Fill in the grid below. (3 pts/box, 30 pts total)
Mass
Charge
Location in atom
Neutrons
Electrons
Protons
Obj. 2: Complete the table for the following elements: (2pt/box = 50 pts)
Isotopic
Name
Symbol
Atomic
Number
Electrons Neutrons
Mg
Protons
11
38
89
Lead -208
208
13
14
Obj. 3: Draw Bohr Models for the following Isotopes. (15 pts each, 60 total)
Helium 5
Mass
Number
Nitrogen 16
P
P
N
N
Valence
Electrons
Chlorine 36
Potassium 40
P
P
N
N
Objective 4: Isotopes (30 pts)
Use Nitrogen – 13 and Nitrogen – 15 to explain what an “Isotope” is. How are the similar? How are they
different? Use protons, neutrons, and electrons to support your response mathematically. It may be helpful
to draw diagrams of each atom.
Objective 5: Lewis Structures of Chemical Bonding: (30pts)
PART 1: Determine if the compounds are ionic or covalent. (1pt each)
Ionic or Covalent
1.
2.
3.
4.
5.
NaCl
H2O
Strontium Carbide (SrC)
Carbon Monoxide (CO)
Water (H2O)
_______________
_______________
_______________
_______________
_______________
PART 2: Use Lewis dot structures to show the ionic bonding in the following pairs of elements. Show the
transfer of electrons using arrows, include charges. Circle electrons that are gained and lost, x them out where
lost. Write the correct chemical formula for the ionic compound that forms. (5 pts each)
sodium oxide (Na and O)
aluminum phosphide (Al and P)
Formula:____________
Formula:____________
PART 3: Use Lewis dot structures to show the covalent bonding in the following pairs of elements. Do the
math. Once you have determined the structure for the molecule, write its structural formula in the space
provided; use a dash to represent a shared pair of electrons, and dots to show unshared electrons. (5 pts
each)
PH3
SBr2
C2H4
Objective 6: Multiple Choice: Fill in what you think will be the correct response. (1 pt/each)
1. The center of an atom is called the
2. The maximum number of electrons in the second energy level is
3. Elements found on the left side of the periodic table are called
4. Elements that touch two sides of the ladder are called
5. Why do atoms bond?
6. What are the outermost electrons called?
7. Matter cannot be _____________________________________________
8. In the metal activity series lab, which metal was the most reactive?
9. In the metal activity series lab, which metal was the least reactive?
10. When non-metals bond together they…
11. High luster, ability to conduct electricity, and malleable belong to which type of element?
12. Which is a metalloid?
13. During the flame test, what causes the metals produce light?
14. What part of an atom reacts with other atoms?
15. When metals bond to non-metals....
16. In the 1890's, J.J. Thompson did some crucial experiments using cathode ray tubes. The rays were
attracted toward the positively charged end of the tube. This lead to the discovery of the
17. The atomic number of an element is the total number of which particles in the nucleus?
18. The mass number of an element is equal to ____.
19. Different elements are guaranteed to have different numbers of ____.
20. How many neutrons are in the nucleus of gold-196?
21. In the Bohr model, what do the rings represent?
22. What is the trend in atomic size as you move across a row in the Periodic Table from left to right?
23. As you move down the periodic table within a column, what is the trend in atomic radius?
24. How are the valence electrons of the noble gases similar?
25. Name the element that has 1 outer electron and is not a metal
26. The only element that has a different number of valence electrons than it’s representative group number.
27. Francium-223 atoms have how many protons
28. What are isotopes?
29-35 Use the following diagram of the periodic table to answer the next few questions.
29. Which family in the above diagram are the alkali metals? ___
30. Which family in the above diagram are the halogens? ___
31. Which family in the above diagram are the alkaline earth metals? ___
32. Which family in the above diagram are the noble gases?
___
33. Which letter in the above diagram represents a metalloid? ___
34. Which two letters in the above diagram represent metals? ___
35. Which letters in the above diagram represent nonmetals? ___