Download Name: Chemistry A Date: Period: Unit 1 Test Review Packet

Name:
Chemistry A
Date:
Period:
Unit 1 Test Review Packet
Standards Assessed on this Exam
1a Students know how to relate the position of an element in the periodic table to its
atomic number and atomic mass.
1b Students know how to use the periodic table to identify metals, semimetals, nonmetals, and halogens.
1c Students know how to use the periodic table to identify alkali metals, alkaline earth
metals and transition metals, trends in ionization energy, electronegativity, and the
relative sizes of ions and atoms.
1d Students know how to use the Periodic Table to determine the number of electrons
available for bonding.
Subatomic Particles
1. Fill in the following table with the correct information:
Charge
Where are these found in theWhat is the mass of these
atom? (nucleus or electron particles?
cloud)
(high or low)
Protons
Neutrons
Electrons
2. Do we consider the mass of the electron when considering the mass of the atom? WHY
OR WHY NOT?
Atomic Number, Atomic Mass, and the Periodic Table
3. Label the atomic number, atomic mass, element name, and element symbol on the
following element:
Name:
Chemistry A
Date:
Period:
4. Explain how the Periodic Table is arranged. Why is arranged this way?
5. Which of the following elements has the largest atomic mass?
a. Mn
b. Co
c. Ni
d. Fe
6. Which of the following makes one element unique from another element?
a. Atomic mass
b. Atomic number
c. How it looks
d. Number of neutrons
Bohr Electron Configurations, the Octet Rule, and Ions
7. Draw the Bohr electron configuration for phosphorus (before it satisfies the Octet Rule).
8. Draw the Bohr electron configuration for chlorine after it satisfies the Octet Rule.
9. What ion would the following elements form after they satisfy the octet rule?
Element
Ion Formed Cation or Anion?
Na
F
N
Be
Metals, Non-metals, Semi-Metals and Group Naming
Name:
Chemistry A
Date:
Period:
10. On the Periodic Table below label (1) metals, (2) non-metals, (3) semi-metals, (4) alkali
metals, (5) alkaline earth metals, (6) halogens, (7) noble gases, and (8) transition metals.
11. Using the following word bank to classify the following elements. NOTE you can use
more then one word per element.
Metals
Non-metals
Semi-metals
Alkali Metals
Alkaline Earth Metals
Halogens
Transition Metals
Noble Gases
a. Silicon ______________________________
b. Magnesium __________________________
c. Lithium ______________________________
d. Neon ________________________________
e. Iron _________________________________
f. Iodine _______________________________
Ionization Energy
Name:
Chemistry A
Date:
Period:
12. What is ionization energy?
13. Describe why ionization energy increases as you move across a period.
14. Describe why ionization energy decreases as you move down a period.
15. Rank the following elements from smallest to largest ionization energy:
a. Cl, Si, S ___________________
b. F, Li, Be ___________________
c. P, As, N ___________________
Electronegativity
16. What is electronegativity?
17. Describe why electronegativity increases as you move across a period.
18. Describe why electronegativity decreases as you move down a period.
19. Rank the following elements from smallest to largest electronegativity:
Name:
Chemistry A
Date:
Period:
a. Sr, Ba, Mg ___________________
b. F, I, Br ___________________
c. P, Cl, S ___________________