Chemistry CST Project
600 points
Name:______________________
Period:_______ Date:__________
Student Contract: “I understand that this packet is to be completed and turned in April
25 and is worth 600 points. Each section is graded as an “A” or an “F.”
Student Signature: ____________________________ Parent Signature:________________________________
Purpose: To review you knowledge of chemistry and prepare you for the Chemistry State Test as well as the Final.
Packet Set – up:
1. This handout goes in front.
2. Questions: Complete forty-two questions using the front and back of lined paper.
a. (front page) One question per page and copy the question.
b. (front page) Please draw diagrams, pictures, graphs and equations as part of your answer. 90 % of the
page must be filled.
c. (bottom of page) Define the bolded word in each question.
Resources:
http://syiemchem.weebly.com
http://www.chem4kids.com
*Please use your notes, videos, the Internet and books to answer these questions.
Study Group: If you work in a group, you will get 50 points extra credit.
 You must get one parent signature, as well as a picture of everyone in the study group.
 You must stay in the study group for at least 3 hours.
 You may work with students from other Chemistry classes.
Student 1:________________________________
Student 2:________________________________
Student 3:________________________________
Student 4:________________________________
Student 5:________________________________
Student 6:________________________________
Parent Signature:_____________________________________ Date:_____________
Necessary Project Time: You must put in 6-10 hours to complete it. Do not put it off until the last day. In order to make
sure you did not copy from another student, YOU WILL BE QUIZZED on the material before CST.
Email: esyiem@hlpusd.k12.ca.us
Questions:
Standard: Atomic and Molecular Structure / Nuclear Chemistry
Problem 1: For the element Nitrogen, copy the exact information provided on the periodic table. Afterwards, use arrows
to identify the atomic number, element symbol, and atomic mass. List the number of protons, electrons and neutrons
below. Also identify whether the element is a metal, nonmetal or semimetal.
Problem 2: “The nucleus occupies very little of the atom’s volume but contains most of its mass.” Explain why this is
true by drawing picture along with your explanation. Use the words dense, protons, electrons and neutrons.
Problem 3: Name one element that Iodine would have chemical properties most like. Explain why they are similar. Use
the words: valence electrons, halogen family and group (column). Please include a drawing of all the elements in the same
column as Iodine from the periodic table.
Problem 4: What element on the periodic table attracts electrons the most? What element attracts electrons the least? Use
the words: electronegativity, protons and electrons. You must explain WHY electronegativity increases or decreases.
Problem 5: Why do the noble gases not have electronegativity? Please draw a Bohr Model for Neon in your explanation.
Use the word valence electron.
Problem 6: What element on the periodic table has the smaller atomic radius Carbon or Nitrogen? Draw a Bohr model of
both elements and use the words atomic radius, electronegativity and protons.
Problem 7: Please rate the strength of alpha, beta and gamma radiation in your explanation.
Standard: Chemical Bonds
Problem 8: For each of the following elements, identify how many valence electrons they have. Also explain what
valence electrons are and how to find them on the periodic table. [Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen,
Fluorine and Neon].
Problem 9: Draw the Lewis Dot Structure for: NF3 and then list the steps of how to draw a Lewis Dot Structure.
Problem 10: Most elements either lose or gain electrons and become ions. For the following elements write if they lose or
gain electrons and the charge they form. [Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, Fluorine and Neon].
Example: Lithium (lose electrons). Li +1
Problem 11: What are the main differences between an ionic, covalent and metallic bonds? Use the words: metal,
nonmetal, share, transfer and electrons. Also, explain how to find out if an element is a metal or nonmetal.
Problem 12: Some of the molecules found in the human body are NH2CH2COOH (glycine), C6H12O6 (glucose), and
CH3(CH2)16COOH (stearic acid). What bonds do they form (ionic, covalent or metallic)? List out all the nonmetals on the
periodic table along with your explanation (Hint: there are 18 nonmetals).
Problem 13: Name all the elements that have the same Lewis dot structure as silicon. Why are do all of these elements
have the same Lewis dot structure?
Problem 14: The reason salt crystals, such as KF, hold together so well is because of electrostatic attraction between the
cations and anions. Identify which element is the cation and anion in KF and explain how you know.
Standard: Conservation of Matter and Stoichiometry
Problem 15: C3H8 + O2  CO2 + H2O
This chemical equation represents the combustion of propane. When correctly balanced, the coefficient for CO2 is
____________.
Problem 16: How many moles of fluorine gas are contained in 9.02×1023 molecules?
Problem 17: How many moles of CH4 are contained in 110.0 grams of CH4?
Problem 18: How many atoms are in a chromium sample with a mass of 13 grams?
Problem 19: How many moles of carbon-12 are contained in exactly 6 grams of carbon-12?
Problem 20: Determine the mass of LiOH produced when 105 grams of Li3N reacts with water according to the
following chemical equation. Balance first.
____Li3N + ____H2O  ____NH3 + ____LiOH
Problem 21: How many grams of MgCl2 are produced when 48 grams of Mg react with an excess of HCl according to the
following chemical equation. Balance first.
____Mg + ____HCl  ____MgCl2 + ____H2
Standard: Gases and Their Properties
Problem 22: The temperature at which all molecular motion stops is____________. Why does all motion stop at this
temperature? Use the words: kinetic energy, molecules and motion.
Problem 23: When someone standing at one end of a large room sprays a small amount of perfume, the smell will slowly
travel until everyone in the room can detect the odor. Gas molecules at room temperature move at very high velocities, so
what is responsible for the delay in detection of the perfume? Use the words: random, motion, diffusion and collision.
Problem 24: What is the equivalent of 423 Kelvin in degrees Celsius? What is the equivalent of 25 degrees Celsius in
Kelvin?
Problem 25: Explain conceptually why reducing the volume will increase the pressure of a gas. Use the words:
molecules, collisions and time.
Problem 26: A sample of carbon dioxide gas occupies a volume of 20 L at standard temperature and pressure (STP).
What will be the volume of a sample of argon gas that has the same pressure but three times the temperature?
Problem 27: The volume of 400 mL of chlorine gas at 400 mm Hg is decreased to 200 mL at constant temperature.
What is the new gas pressure?
Problem 28: A 500 L blimp is flying in the skies above Russia, where the pressure is 0.8 atm on a freezing day (-23 oC).
When the blimp lands, it is slightly warmer (27 oC) and the pressure increases to standard pressure at ground level. What
will the volume of the blimp when it lands?
Standard: Acids and Bases / Solutions
Problem 29: List 5 properties each for acids and bases. [Litmus paper color, Phenolphthalein Color, pH range, taste,
reacts with metals (yes/no)]
Problem 30: Which pH represents a solution with the LOWEST concentration of hydrogen ions (H+)? Which pH
represents a solution with the HIGHEST concentration of hydrogen ions (H+)? Define Arrhenius Acid and Arrhenius
Base.
Problem 31: How many moles of HNO3 are needed to prepare 5.0 liters of a 2.0 M solution of HNO3?
Problem 32: A salt is made of a metal and a nonmetal. It is also called an ionic compound. If you put a salt in water,
does it conduct electricity? Why or why not? Use words: ions, water, salt, ionic compound, conduct electricity, dissociate,
ions.
Problem 33: Equal volumes of 1 molar hydrochloric acid (HCl) and 1 molar sodium hydroxide base (NaOH) are mixed.
After mixing, the solution will be _______________(strongly acidic, weakly acidic, nearly neutral, weakly basic). Write a
neutralization reaction equation with HCl and NaOH.
Problem 34: What is the difference between a strong acid and a weak acid? Use a drawing to demonstrate your answer.
Use the words: dissociate and ions.
Problem 35: A teaspoon of dry coffee crystals dissolves when mixed in a cup of hot water. This process produces a
coffee solution. The original crystals are classified as a solute. Draw a before and after picture of this process and label the
solute, solvent and solution. Define solute, solvent and solution.
Standard: Chemical Thermodynamics
Problem 36: For the scenario “boiling water,” identify the system, surroundings, direction of heat flow (in or out) and if
the reaction is exothermic or endothermic. Please draw and label a picture for your answer.
Problem 37: In the space below, draw a heating curve and cooling curve for water. Label the axes and every phase
change. Be sure to label the temperature at which water melts, freezes, boils and condenses. (Tmelting= 0°C Tboiling =
100°C).
Problem 38: For melting, freezing, condensing and boiling, make a table and identify if the phase change absorbs or
releases heat and if it is exothermic or endothermic.
Problem 39: HgO + heat  Hg + O2 For this equation, identify the reactants and products. Afterwards, state if
the reaction is exothermic or endothermic. Provide an explanation of how you know.
Problem 40: a) How much heat is required to raise the temperature of 20 g of mercury from -20oC to 30oC? (use
cp=0.15J/g oC). b) How many calories is this?
Problem 41: A sample of solid gold (specific heat of 0.30 J/g oC) is heated with an electrical coil. If 180 Joules of energy
are added to a 12.0 gram sample initially at 30 oC, what is the final temperature of the gold?
Problem 42: The specific heat of copper is about 0.4 joules/ gram ºC. How much heat is needed to change the
temperature of a 30-gram sample of copper from 20.0 ºC to 80.0 ºC?