so neutrons without a charge go between the positively charged protons in the atom s.
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1 AP Biology Summer Assignment Use Chapter 2 in textbook, Google and videos to answer the questions below I. Basic Chemistry 1. What are the three particles that comprise an atom? 2. Atom Structure: Sub-atomic Particle Proton Neutron Electron Charge Location Periodic Table Like charges repel so neutrons without a charge go between the positively charged protons in the atom s. Like charges repel (push each other away) so electrons all having a negative charge cannot be close together within their energy levels (orbits). The first energy level holds electron, the second holds, and the third holds, and the 4 th holds electrons. The outermost energy level is called the. 3. Why are the following numbers on the periodic table different? Atomic Number: Atomic Mass: 4. Create a Bohr model for each of the following atoms: Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorus and Sulfur. Use candy, or beads and a blank sheet of paper. Include protons, neutrons, and electrons and electron shells. Then, take a picture and include it in the chart below. Atoms Atomic number Atomic mass Number of Protons Number of Electrons Number of Neutrons Picture Carbon Hydrogen Oxygen Nitrogen
2 Phosphorus Sulfur 5. Why must there be equal numbers of protons as electrons? 6. Oppositely charged ions (attract or repel) each other? (Ions are used in car paint to help it stick to the car). 7. Why isn t the charge affected if an element had two different numbers of neutrons? 8. Two atoms with the same atomic number of 92, but different atomic masses (236 and 238) (would or would not) be the same element (hint: iso means the same ). 9. If an atom has too many or too few neutrons its nucleus become unstable forming a radioactive isotope, but not all isotopes are radioactive. Radiocarbon dating uses a radioactive isotope of Carbon to measure the radioactive decay rate to see how old a fossil is. Radioactive oxygen isotope is used to measure climate trends throughout time, and radioactive barium isotope is used to help doctors see your digestive tract. A radioactive isotope of Uranium can cause cancer, nuclear bombs, or nuclear energy (it depends on how fast the problematic neutrons are being released). Are all uranium isotopes radioactive? 10. How can you determine if something is an isotope using the periodic table? 11.Compare the following terms: Normal Atom Ion Isotope 12. Fill in the chart below. Substance: Atom Element Molecule Compound Define: Example:
3 13. Elements are represented by abbreviated symbols. For example, the symbol for Carbon is C and the symbol for Oxygen is O. The compound, Carbon Monoxide, contains one atom of Carbon and one atom of Oxygen. It is written as CO. Why do you think they needed to use a small case o in the symbol for Cobalt Co instead of a CO? 14. The subscript 2 behind CO2 tells you how many atoms of oxygen are in the molecule of Carbon dioxide. Why do you think a subscript is not needed behind the Carbon? 15. Determine the number of atoms of each element in this molecule: H2O Water 2 atoms of Hydrogen and 1 atom of oxygen. H2SO4 Ca(OH)2 Sulfuric Acid Calcium Hydroxide 16. A coefficient is the number in front of the molecule that tells you the number of molecules. If there is not a coefficient assume you only have one molecule of that substance. If there coefficient is 3 there are 3 molecules of CO2. Draw 3 CO2 molecules: 17. There would be a total of carbon atoms and oxygen atoms in 5 CO Determine the total number of atoms of each element for the number of molecules listed (multiply the coefficient by the subscript of each element): 4 H2O 4 x 2 H and 4 x 1 O 8 atoms of Hydrogen and 4 atom of oxygen. 2 H2SO4 19. Draw a circle around the subscripts below and draw a square around the coefficients. H2 2 HCl 4 O2 3 CO2 2 NaOH 3 CO3 20. Circle the number of atoms of each element within the molecule and square around the number of molecules of that substances. H2 2 HCl 4 O2 3 CO2 2 NaOH 3 CO3 21. A chemical reaction uses energy to rearrange chemical bonds to form new substances. Explain the reaction below: 2 H2 + O2 2 H2O 22. The arrow represents the change of energy needed to perform the chemical reaction. The items on the left side of the arrow are called the reactants (ingredients) circle them in the equation today. What are the end products listed at the end of the arrow?
4 23. Tearing paper is only a physical reaction that does not change the make-up of the paper. Whereas, burning paper is a reaction because it forms a new substance by rearranging its energy and chemical bonds. It formed. 24. In a chemical reaction, you cannot create or destroy mass/matter so the mass before and after should be the same. This is the Law of Conservation of Mass. Similar to baking a cake, if you add to 2 eggs to the batter, the cake will come out of the oven with two eggs, but they are changed into a new substance, cake. Likewise, if you started with 5 carbon atoms and 10 oxygen atoms in your reactants then your end products should total atoms of carbon and atoms of oxygen. 25. How to balance a chemical reaction by only changing the coefficients (if you need to). Step 1: Write it out and box molecules H 2 O H 2 + O 2 Coefficient Coefficient Coefficient (# of H2O molecules) (# of H2 molecules) (# of O2 molecules) Step 2: Rewrite vertically. Then start by guessing all coefficients are 1 and then multiply by subscripts. Step 3: Total the atoms on both sides of each element Step 4: Change coefficients to get the atoms of the same element to equal on both sides. 1 X Total H = 2 2 X H 2 O H 2 O Total H = 4 = 2 = 1 Total O = 1 = 4 = 2 Total O = 2 1 X H 2 = 2 1 X O 2 = 2 Total H = 2 2 X H 2 = 4 1 X O 2 = 2 Total H = 4 Total O = 1 Total O = 2 The H is balanced with 2 H atoms on both sides of the arrow but, the oxygen was not. I increased the coefficient on the left, which gave me 2 more O to match the number of O on the left. However, it also increased my H on the left to 4 so I had to get 4 H on the right by increasing its coefficient to 2 as well. Step 5: Write the coefficients into the equation 2 H 2 O H 2 + O 2 Coefficient Coefficient Coefficient (# of H2O molecules) (# of H2 molecules) (# of O2 molecules) Balance the following chemical reaction: H 2 O 2 H 2 O + O 2 Coefficient Coefficient Coefficient
5 (# of H2O molecules) (# of H2 molecules) (# of O2 molecules) X H 2 O 2 = = H X 2 = O = X O 2 = Total H = Total O = Total H = Total O = 27. Comparing Types of Chemical Bonds: Definition: Ionic Covalent Polar (Van der Waals force and Hydrogen) Strength 28. What do you think a double covalent bond is? Draw one: 29. A hydrogen atom uses the first energy level as its valence. This valence needs to electrons to be full, but hydrogen only has one electron. Do you think this atom should react with another atom to give off or pick up another electron? 30.Why do you think hydrogen will pair with another atom? 31. If two hydrogen atoms bond together we call it a diatomic molecule. How many atoms are in a diatomic molecule? 32. If you were to draw out an oxygen atom you would notice that its valence is missing two electrons. How many hydrogen atoms will oxygen bond to if each hydrogen atom has one electron? 33. The molecule below shows one oxygen atom bonded to two hydrogen atoms by sharing electrons. This is known as a covalent bond. If you share work with a co-worker what do think is being shared in a co-valent bond? Valence Valence H O H Each hydrogen shares its 1 valence electron with the oxygen s valence. Now, each hydrogen has 2 electrons filling its valence and the oxygen has all 8 electrons filling its bigger valence. Valence II. Properties of Water
6 Provide a visual representation of each of the properties of water using any items found around your house or outside of your house. Include a description in your own words and take a picture that demonstrates each properties. Properties Explanation Picture Polarity Cohesion Adhesion Surface Tension Capillary Action Specific Heat Density III. Organic Molecules
7 1. Go over 4 macromolecules by watching 2. Access and open the Virtual Lab entitled Nutrition. 3. The left side of the page contains background information and instructions in the Question area. On the bottom of the page are the following icons for your use: Journal (these are questions that may be answered/submitted to your instructor), Calculator (working calculator function), Audio (turns sound on/off) and Print (prints the screen). 4. Read the background information found under the Question area first, and then continue on to reading the procedure information posted there as well. 5. At this point, you are ready to begin the lab exercise. You will need to first open and/or print the Post-Lab Quiz and Lab Report, which can be found on the previous page. Click on the Nutrition Facts Label Guidebook on the lower portion of the activity area and read through the information presented. You should also click on the Daily Calories Chart for additional information regarding individual energy requirements and expenditures. When you are ready, please begin selecting food items and dragging them to the various meal times in the laboratory area. Remember to follow the directions given to you in the Question as well as in the Post-Lab Quiz and Lab Report areas, and refer back to the notes in the Nutrition Facts Label Guidebook and Daily Calories Chart areas if necessary. 6. Complete the exercise as directed, recording any data or information needed in your Lab Report. 7. When you are finished, please answer all of the questions found at the end of the Post-Lab Quiz and Lab Report.
8 IV. Basic Statistics 1) View The Power of Numbers (10 minute video) at 2) Answer the following: a. What is the difference between sample and population? b. What is the purpose of calculating the standard deviation? c. What is the distinction between correlation and causation and which is supported by the use of statistics? 3) Learn how to calculate the standard deviation. To help you with this, you can view: 4) Let s practice!! Formulas: Mode = value that occurs most frequently in a data set Median = middle value that separates the greater and lesser halves of a data set Mean = sum of all data points divided by the number of data points Range = value obtained by subtracting the smallest observation (sample minimum) from the greatest (sample maximum) Standard Deviation = ( x i x) n 1 2 where x = mean and n = size of the sample Example problem: One of the lab groups collected the following data for the heights (in cm) of their Wisconsin Fast Plants: Find the mode, median, mean, and range. Show your work where necessary Mode: Median: Mean: Range: Find the standard deviation by filling in the following table. Heights (x) Mean ( x ) x x ( x x) Interpret the standard deviation in the context of the problem. ( x x) 2 Standard deviation:
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