Download Fall Semester Review Packet

Name _____________________________________________________________________________ Date ___________________
Midterm Exam Review
1. Two scales were used to measure the mass of an object that was known to have a mass of 32 g. Each
scale measured the mass of the object three times. Use the data table below to answer the following
question.
a. Which scale measured the object
Scale A
Scale B
with the most precision?
b. What is the average mass of the
object measured by scale B?
c. Were the scales accurate?
Trial 1
25 g
27 g
Trial 2
28.5 g
29 g
Trial 3
30 g
28.2 g
2. Identify each of the following as a property of a solid, liquid or gas. (Some may go with more than one)
Flows and takes the shape of its container ______________________________________
Made of particles held in a specific arrangement _________________________________
Compressible ____________________________________________________________
Has a definite volume ______________________________________________________
Always occupies the entire space of its container ________________________________
Has a definite volume, but flows _____________________________________________
3. Which term best describes the process by which a liquid transforms to a solid by the removal of heat?
a. Crystallization (freezing)
b. Condensation c. Particle arrangement
d. Vaporizing
4. Which term best describes the process by which particles escape from a non-boiling liquid to a gas?
a. Evaporation
b. Melting
c. Crystallization (freezing)
d. Aeration
5. What subatomic particle determines the element?
6. List the common ion charges and valence electrons for the following groups;
a. Group 1
c. Group 15
b. Group 13
d. Group 17
7.
How does the atomic radius change across a row in the periodic table (left to right)? Explain the trend.
8. How does ionization energy change across a row in the periodic table (left to right)? Explain the trend.
9.
What element has the electron configuration of 1s2 2s2 2p6 3s2 3p4?
Name _____________________________________________________________________________ Date ___________________
10. Which element has a noble gas configuration of [Kr] 5s1?
11. What is the electron configuration for Co?
12. Which of the following pairs of atoms would have the SAME electron configuration?
a. Mg & Ar
c. K+1 & Br –1
+1
b. Na & Ne
d. Ca & S
13. Br-80 has 45 neutrons. How many ELECTRONS would a neutral atom of bromine contain?
14. How many Protons, electrons and neutrons does the following atom have? 4220Ca +2
15. What do the “dots” represent in an Electron Dot Diagram?
16. Write the formulas for sodium carbonate, sodium bicarbonate, and calcium phosphate.
17. Name these compounds: P2O3, SiS2, SF6
18. Which of the following forms a type of bond where valence electrons are transferred from the cation to
the anion?
a. Potassium chloride
c. Diphosphorus pentaoxide
b. Dihydrogen monoxide
d. Carbon monoxide
19. Which of the following is an IONIC compound?
a. P2O3
b. N2Br3
c. CaBr2
d. CO2
20. Name the compound, Cr(C2H3O2)3. (Remember Transition metals need Roman Numerals: uncross
cross)
21. What is the total number of each atom in the compound, (NH4)3PO4?
22. Which group of elements does not generally form compounds? Explain why?
Name _____________________________________________________________________________ Date ___________________
23. Which of the following is a COVALENT compound?
a. SO2
b. LiCl
c. Pb(NO3)2
d. Fe2O3
24. Using Electron Dot Diagrams, draw the transfer of electrons that occurs in CaF2. Then, describe how
the location of the elements on the periodic table relates to the transfer of electrons that occurs in this
compound.
25. State the law of conservation of mass.
26. What are the diatomic molecules?
27. How many oxygens are in Pb(NO3)4?
28. Which side of chemical reactions are products and reactants?
29. Balance the following reactions.
a. __ C6H6 + __ O2  __ H2O + __ CO2
b. __ NaI + __ Pb(SO4)2  __ PbI4 + __ Na2SO4
c. __ NH3 + __ O2 __ NO + __ H2O
d. __ Fe(OH)3  __ Fe2O3 + __ H2O
30. Write a formula equation and balance the following formulas.
a. Nitrogen and oxygen react to form Nitrogen dioxide.
b. Sodium Chloride reacts with Magnesium to form Magnesium chloride and sodium.
Name _____________________________________________________________________________ Date ___________________
31. Predict the products and balance:
a. _____ FeCl2 + _____K3P ______ _________+ ______ _______
i. Type: _________________
b. ______Al + _____ Pb(NO3)2  ______ _______ + ________ ________
i. Type: ___________________
ii. Which element is reduced and which is oxidized? How can you tell?
32. Explain ALL the differences between an ionic and covalent bond. (Properties, element, electrons, etc.)
The Semester exam is 40 multiple choice and 3 short answer questions
Possible Written Response Questions for Semester Exam
1. Describe the difference between a chemical change and a physical change and give three indications that
a chemical change has occurred. Also, give one example of each type of change.
2. Explain the Law of Conservation of Mass. Include information about the mass of reactants and products
within a chemical equation.
3. Describe the difference between a heterogeneous and a homogeneous mixture and give two examples of
each type.
4. Explain the difference between a pure substance and a mixture and give two examples of each.
5. Explain how the mass number and atomic number of an element can be used in determining the number
of subatomic particles within an atom.
6. Explain how the three isotopes of hydrogen alike and how they are different. (Use the terms: protons,
neutrons, and mass) protium, deuterium, and tritium.
7. List the four parts of Dalton’s Atomic Theory.
Name _____________________________________________________________________________ Date ___________________
8. Describe J.J. Thomson’s and Ernest Rutherford’s contributions to the development of the atom,
including the experiments they performed.
9. Describe how the current periodic table is arranged by comparing groups, periods and properties of the
elements.
10. Explain the difference between a molecule (covalent compound) and an ionic compound. Include the
interaction between valence electrons and the types of bonds for each.
11. There are many components of a scientific experiment, including a manipulated variable, a responding
variable and a control. Describe how these variables relate to one another during an experiment.
12. Explain the difference between accuracy and precision when describing scientific measurements.
13. Explain how atoms of the same element may differ. Include all of the following terms in your
explanation. Isotopes, ions, cations, anions, neutrons, electrons, and protons.
14. Explain the rules and describe the differences in nomenclature for molecular and ionic compounds. Give
several examples.
15. Explain the difference between the atomic mass, atomic number and mass number of an element.
16. Describe the five types of chemical reactions. How are you able to distinguish between the different
reaction types?
17. You may also be asked to identify reaction types and predict products and balance chemical equations.
18. Describe the trends in the periodic table, by group and period for: electronegativity, atomic radii, and
ionization energy. Be sure to include the explanations in terms of Zeff-effective nuclear charge and
shielding.