Chemistry Mid Term Exam Review Sheet #1

The midterm exam covers chapters 1 810. You should read through each chapter, look over old tests you still have, answer the following questions and do the calculations in order prepare yourself for the midterm.

1. Define the following terms and describe where each is located.

proton ______

neutron ______

electron –______

2. Complete the following table:

Element name / Atomic # / Mass # / # of protons / # of Neutrons / # of Electrons / Symbol
Hydrogen
Carbon
Sodium
Calcium
Fe

3. Define the following and give an example of each usingchemical symbols.

atomic number______/ ______

atomic mass______/ ______

isotope______/ ______

4. Which of the following are isotopes of the same element?199Y 209Y1910Y

5. Describe Rutherford's experiment: ______

______

6. Explain all the major parts of Dalton's Atomic Theory.

a.

b.

c.

d.

7. Balance the following chemical equations:

3 CO + _____ Fe2O3 2 Fe + 3CO2

3 Zn(OH)2 + 2H3PO4 _____ Zn3(PO4)2 + 3H2O

8. Define Ionic and Molecular compounds, and tell how each is formed.

  1. Ionic: oppositely charged particles creation bonds that are formed when electrons transfer
  2. Molecular; Bonds formed when atoms share electrons to complete their valence level

9. Name the following compounds and state if it is ionic or molecular in nature:

  1. Al(OH)3aluminum hydroxide - ionic
  2. N2O5dinitrogen pentoxide - molecular
  3. MgI2magnesium iodide - ionic
  4. Cl2O7dichlorine heptoxide

10. Write a chemic al formula for each name given and tell whether it is an ionic (i) ormolecular (m) compound:

  1. Ammonium Phosphate ______(NH4)3PO4 - I
  2. Magnesium Nitride______Mg3N2 - I
  3. Oxygen Difluoride ______OF2 - M
  4. Carbon Dioxide ______CO2 - M
  5. Sulfur Dioxide______SO2 - M

11. Name and describe the 6 types of chemical reactions. Give an example of each.

  1. : smaller species combine into larger ones – 2H2 + O2 2H2O
  2. Combination Decomposition: larger species breaking down into smaller ones – MgCl2 Mg + Cl2
  3. Single replacement: an element and a compound react and create a different element & compound a + bc  b +
  4. Double replacement: Ions from two ionic compounds swap places to make two different ionic compounds
  5. Usually involve oxygen reacting with a fuel producing H2O & CO2 – CH4 + 2O2 CO22H2O

12. Define and give an example of each:

Element______/ ______

Mixture______/ ______

Compound______/ ______

homogeneous substance______/ ______

heterogeneous substance ______/ ______physical property ______/ ______

chemical property______/ ______

physical change______/ ______

chemical change______/ ______

qualitative measurements______/ ______

quantitative measurement______/ ______

13. Which of the following is a homogeneous mixture?

a. oil in water b. soot in water c. alcohol in water

14. Which of the following could be considered a physical change?

a. cooking a pancake b. burning a tree c. melting an ice cube

15. Which of the following is considered a heterogeneous mixture?

a. salt and sugar b. flour and baking powder c. salt and pepper

16. Classify each as a physical or chemical change.

______a. instant coffee is combined with hot water to produce a brown liquid Physical

______b. from exposure to air and moisture, iron turns reddish and cannot conduct electricity Chemical

______c. iron is heated , turns red and then melts Physical

______d. sugar is heated to produce steam and a black solidChemical

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