NAME:
DATE:
CHEMISTRY
BLK:
Chapter 2 Mini Test - Rewrite
Ch. 2 Outcomes:
C2 use the periodic table to compare the characteristics and atomic structure of elements
● explain the organization of the PTE (e.g., atomic number, atomic mass, properties, families)
● distinguish between metals, non-metals, and metalloids
● use PTE to predict the properties of a family of elements (e.g. alkali, alkaline earth, halogens, and noble gases)
● draw a Bohr model of each atom up to atomic number 36
C3 write and interpret chemical symbols of elements
● write chemical symbols for atoms and ions of elements
● differentiate between atoms and ions in terms of structure, using Bohr models
20
≥ 18
Exceeding
Expectations
15 – 17.5
Fully
Meeting
13.5 – 14.5
Minimally
Meeting +
11.5 - 13
Minimally
Meeting
9.5 - 11
Minimally
Meeting -
≤9
Approaching
Expectations
 A teacher-approved Periodic Table is required for this test.
1. State two properties of metals. (2 marks)
2. What is the name of Group 2? (1 mark)
3. Why are noble gases stable? (1 mark)
4. Give an example of an element in period 3 that will lose electrons to form an ion. (1 mark)
5. Which of the alkali metals is most reactive? (1 mark)
6. Describe in detail how an atom of fluorine becomes an ion. (1 mark)
7. How many neutrons does an atom of Beryllium have? (1 mark)
8. What is a metalloid? Describe and provide the name of one. (2 marks)
9. What is the atomic mass of Carbon? (1 mark)
10. Explain why elements gain or lose electrons. (1 mark)
11. What is a valence shell? (1 mark)
12. Use the periodic table to complete the table below. (4 marks – ½ mark each box)
Element Name
Atomic
Number
Nitrogen
Charge
Atom or
Ion?
Number of
Protons
Number of
Electrons
0
4
+2
13. Phosphorus’s atomic number is 15.
(a) Draw a Bohr diagram showing the number of electrons in each energy level (shell) of a
phosphorus atom. (1 mark)
(b) Draw a Bohr diagram showing the number of electrons in each energy level of a phosphorous
ion, P3-. (2 marks)