Download Name: (1 of 2) Math Set # 13 Protons,

 Name: ____________________________________ (1 of 2) Math Set # 13 Protons, Neutrons, Electrons Proton = positive particle in the nucleus of an atom Neutron = positive particle in the nucleus of an atom Electron = negative particle moving around the outer edge of an atom Atomic Number = the number of protons Atomic Mass = the number of protons plus the number of neutrons EXCEPT FOR IONS the number of protons = the number of electrons 1. An atom with an atomic number of 8 has 8 of what particle? 2. An atom with an atomic number of 76 has 108 of what particle? 3. An atom with an atomic mass of 20 has 20 of what particles? 4. An atom with an atomic mass of 11 has 11 of what particles? 5. An atom is NOT an ion. It contains 12 protons. How many electrons does it have? 6. An atom is NOT an ion. It contains 58 protons. How many electrons does it have? 7. An atom is NOT an ion. It has an atomic number of 33. How many electrons does it have? 8. An atom is NOT an ion. It has an atomic number of 1. How many electrons does it have? Name: ____________________________________ (2 of 2) Math Set # 13 Protons, neutrons, electrons # protons = atomic number (ALWAYS) # electrons = # protons (EXCEPT FOR IONS) # neutrons/protons = atomic mass # neutrons = atomic mass minus atomic number Example: An atom of Oxygen has an atomic number of 8 and an atomic mass of 16. It is not an ion. Give the number of protons, neutrons, and electrons ANSWER: Protons = 8 (atomic number) Electrons = 8 (number of protons) Neutrons = 16 proton/neutrons – 8 protons = 8 neutrons 1. Give the number of all three particles for an atom of Fluorine which has an atomic mass of 19 and an atomic number of 9. It is not an ion. 2. Give the number of all three particles for an atom of Iodine which has an atomic mass of 127 and an atomic number of 53. 3. Give the number of all three particles for Hydrogen, which has an atomic mass of 1 and an atomic number of 1. 4. Give the number of all three particles for gold, which has an atomic mass of 197 and an atomic number of 79. Name: ____________________________________ (1 of 2) Math Set # 14 Ions and Isotopes When an atom loses or gains one or more electron it is called an “ion” and the atom now has a charge. For example, if a hydrogen atom has one proton (+) and one electron (-­‐) the two charges cancel each other out. When the electron is lost the hydrogen atom is only a single proton (+)! This makes the whole atom have a charge of +1. Find the charge of each ion described in the problems. EXAMPLE: An atom loses two electrons. What is the total charge of the electrons that were lost? What is the resulting charge of the ion? ANSWER: Two electrons have a total charge of -­‐2. The atom used to be neutral but lost negative charges so it is now positive. Since it lost two negative particles the total charge is +2. EXAMPLE #2: An atom gains two electrons. What is the total charge of the electrons that were gained? What is the resulting charge of the ion? ANSWER: 1.
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The two electrons have a total charge of -­‐2. The atom used to be neutral but gained negative charges so it is now negative. Since it gained two negative particles the total charge is -­‐2. An atom loses one electron. Total charge of the electrons that moved = _____________________ Charge of the remaining ion = ___________________________ An atom loses three electrons. Total charge of the electrons that moved = __________________________ Charge of the remaining ion = ___________________________ An atom gains one electron. Total charge of the electrons that moved = ________________________ Charge of the remaining ion = ____________________________ An atom gains three electrons. Total charge of the electrons that moved = _________________________ Charge of the remaining ion = ______________________________ Name: ____________________________________ (2 of 2) Math Set # 14 Ions and Isotopes The number of protons is ALWAYS the same for an atom of a specific element. Germanium ALWAYS has 32 protons. If you add a proton it is no longer Germanium but becomes Arsenic. The number of neutrons, however, is NOT always the same for an atom of Germanium. Sometimes there are 40 neutrons, but other times there are 41. This means that a specific atom might have a slightly different atomic mass. Method for Finding the AVERAGE atomic mass Chlorine -­‐35 makes up 76% of all chlorine in nature. This means that if you could select 100 atoms of chlorine randomly 76 of them would have an atomic mass of 35. The other 24 atoms of chlorine would be Chlorine-­‐37 which has an atomic mass of 37. What is the average atomic mass for chlorine? STEP ONE: Multiply the mass by the percent and divide by 100 Chlorine-­‐35 35 amu x 76/100 = 26.60 amu (“atomic mass units”) Chlorine-­‐37 37 amu x 24/100 = 8.88 amu STEP TWO: Add the amounts together. The answer is the average atomic mass 26.60 amu + 8.88 amu = 35.48 amu (NOTE: INCLUDE UNITS – amu) DIRECTIONS: Calculate the average atomic mass for each element. Include units! 1. Boron which occurs as 20% Boron-­‐10 and 80% Boron-­‐11. 2. Rubidium which occurs as 72% rubidium-­‐85 and 28% rubidium-­‐87 3.Gallium which occurs as 60% gallium-­‐69 and 40% gallium-­‐71 4. Silver which occurs as 52% silver-­‐107 and 48% silver-­‐109 5. Silicon which occurs as 92% silicon-­‐28, 5% silicon-­‐29, and 3% silicon-­‐30 Name: ____________________________________ (1 of 2) Math Set # 15 Periodic Table Use a Periodic table to find the information asked for below: 1.What is the atomic number of: Calcium __________ Iron ______________ Gold ______________ Uranium _______________ 2. What is the Atomic mass of: Oxygen _____________ Silver _______________ Iron _______________ Xenon _______________ 5. Does mercury have more protons and electrons than tin? 6. Is mercury a heavier element than tin? 7. Does potassium have more electrons than neon? 8. Does hydrogen have more electrons than Uranium? 9. Which has more protons, sulfur or iodine? 10. Which has more protons, iodine or silver? 11. Determine how many electrons, protons, and neutrons there are in each atom: Argon: protons _______________ Carbon: protons ______________ Neutrons ______________ neutrons _____________ Electrons _____________ electrons _____________ DIRECTIONS: use the periodic table to locate the name for each element 12. This element uses the symbol Bi 13 This element has 47 protons 14. This element is in group 17 and has an average atomic mass of 19. 15. This element is in the lanthanides and starts with the letter Y. 16. This element has 2 protons. 17. This element is in period 6 and is abbreviated with only one letter. Name: ____________________________________ (1 of 2) Math Set # 15 Periodic Table There was a newly discovered element name Johnsonium. It is to be added to the Periodic Table of Elements on page 339 of the textbook. Johnsonium has 117 protons and 182 neutrons. It is solid at room temperature. DIRECTIONS: Make a periodic square for this element using the key for the periodic table on page 338 of your textbook. Make sure the color of the letters and the color of the square are correct. Label the square with the group number and the period number. You can give it any initials you like as long as they are not already taken. Make another square with your own created and named element. Follow the directions above to show how your element would fit into the periodic table.
Name: ____________________________________ (1 of 1) Math Set #16 Periodic Table Directions: Use the blank periodic table worksheet to complete ALL steps below. 1. Number the groups. 2. Number the periods 3. Draw a heavy lack line between the metals and nonmetals. 4. Over Group 1 write the words “alkali metals” 5. Over Group 2 write the words “alkaline earth metal” 6. Over Groups 3-­‐12 (collectively) write “transition metals” 7. Over Group 16 write “chalcogens” 8. Over Group 17 write “halogens” 9. Over Group 18 write“Noble gases” 10. Write the names of the two rows at the bottom of the chart: lanthanides and actinides 11. Write the symbol of each element that exists as a gas at ordinary conditions in RED. 12. Write the symbol of each element that is a solid at ordinary conditions in BLACK. 13. Write the symbol of each element that is a liquid at ordinary condition in BLUE. 14. Write the symbol of each element that is a man-­‐made element as an outline. 15. Place the atomic number for each element above the symbol. 16. Use the following to color the periodic table. Halogen blue Noble gases yellow Alkali metals purple Alkaline earth metals red Transition elements green Chalcogens brown Lanthanides orange Actinides light blue Name: ___________________________________ (p. 1 of 2) Math Set #17 Concentration Concentration = grams of solute milliliters of solute Example: What is the concentration of a solution that has 35 g of salt dissolved in 175 mL of water? Concentration = ? Concentration = grams of solute Solute = 35 g milliliters of solute Solvent = 175 mL Concentration = 35 g____ = 0.2 g/mL 175 mL FOR FULL CREDIT: SET UP THE PROBLEM EXACTLY LIKE THE EXAMPLE 1. What is the concentration of solution A if it has 55 g of sugar dissolved in 500 mL of water? 2. What is the concentration of solution B if it as 36 g of sugar dissolved in 144 mL water? 3. How many grams of sugar must be dissolved in 50 mL of water to make a concentration equal to that of solution A? How many grams of sugar must be dissolved in 100 mL of water to make a concentration equal to that of B?
Name: ___________________________________ (p.2 of 2) Math Set #17 Compound Percentages Total Percentage of Elements in a compound = 100% Example: Propanol contains 60.0% carbon and 26.6% oxygen. Hydrogen is the only other element in propanol. Hydrogen makes up what percentage of the compound? %carbon + %oxygen +%hydrogen = 100% 60.0% + 26.6% + %hydrogen = 100% 86.6% + %hydrogen = 100% % hydrogen = 100% -­‐ 86.6% %hydrogen = 13.4% SHOW ALL STEPS FOR FULL CREDIT 1. Sodium Carbonate is made up of sodium, carbon, and oxygen. It has a chemical composition of 43.4% sodium and 11.32% carbon. What is the percentage of oxygen in this compound? 2. Sulfuric Acid is composed of hydrogen, sulfur, and oxygen. It has a percent composition of 2.06% hydrogen and 65.3% oxygen. What is the percentage of sulfur in this compound? Name: ___________________________________ (p.1 of 2) Math Set #18 Solubility Use the following graph to answer the questions on this page and on the next page. 1. On a solubility curve, the lines indicate the concentration of a ____________________________ solution. 2. Values on the graph _____________________________ (below or above) a curve represent unsaturated solutions because more solute could be dissolved at that temperature. 3. A solution contains 70g of NaNO3 at 30 degrees C. Is it saturated or unsaturated? 4. A solution contains 50g of NH4Cl at 50 degrees C. Is it saturated or unsaturated? 5. A solution contains 20g of KCLO3 at 50 degrees C. Is it saturated or unsaturated? 6. A solution contains 70g of KI at 0 degrees. Is it saturated or unsaturated? 7. Normally solubility increases with temperature. Is that true for all the chemicals on this graph? If not, which chemicals are the exeptions?
Name: ___________________________________ (p.2 of 2) Math Set #18 Solubility Use the graph on the previous page to answer the following questions. 8. What mass of solute will dissolve in 100 mL of water at the following temperatures: a. KNO3 at 70 degrees C _______________________________ b. NaCl at 100 degrees C ________________________________ c. NH4Cl at 90 degrees C ________________________________ 9. Which substance is the most soluble in water at 15 degrees C? 10. a. What is the solubility of KCl at 5°C? _______ b. What is the solubility of KCl at 25°C? _______ c. What is the solubility of Ce2(SO4)3 at 10°C? _______ d. What is the solubility of Ce2(SO4)3 at 50°C? _______ 11. a. At 90°C, you dissolved 10 g of KCl in 100. g of water. Is this solution saturated or unsaturated? b. How do you know? 12. A mass of 100 g of NaNO3 is dissolved in 100 g of water at 80ºC. a) Is the solution saturated or unsaturated?______________________________ b) As the solution is cooled, at what temperature should solid first appear in the solution? 13. Use the graph to answer the following two questions: Which compound is most soluble at 20 ºC? ________ Which is the least soluble at 40 ºC? ________ 14. Which substance on the graph is least soluble at 10°C? __________ Name: ____________________________________ (1 of 2) Math Set # 19 Valence Electrons Remember: Two electrons are in the first orbital, 8 in the second, and 8 in the third. The number of electrons in the outermost orbital is the valence number. DIRECTIONS: 1. Place the electrons in the correct orbitals for an atom of each element. 2. Write the number of valence electrons to the right of the diagram.
Hydrogen Oxygen Sulfur Helium Argon Magnesium Sodium Boron Carbon Nitrogen Aluminum Name: ____________________________________ (2 of 2) Math Set # 19 Valence Electrons What is the largest number of electrons that can be in the outermost orbital of the period 2 and period 3 elements? _________________________________ What is the largest number of electrons that can be in the outermost orbital of the period 1 elements (Hydrogen and Helium)? _____________________________ DIRECTIONS: For each of the following elements give the valence number and the charge the atom would have if it had a full or empty outermost orbital. REMEMBER, a valence of 3 or less with empty the outermost orbital and a valence of 5 or more will gain electrons to fill the outermost orbital. 1. Hydrogen: valence = _____ for a full/empty orbital _________________ charge = ______ 2. Carbon: valence = _____ for a full/empty orbital _________________ charge = ______ 3. Magnesium: valence = _____ for a full/empty orbital ________________charge = _______ 4. Lithium: valence = _____ for a full/empty orbital __________________charge= _______ 5. Chlorine: valence = _____ for a full/empty orbital __________________charge= _______ 6. Oxygen valence = _____ for a full/empty orbital __________________charge= _______ 7. Sodium: valence = _____ for a full/empty orbital __________________charge= _______ 8. Aluminum: valence = _____ for a full/empty orbital __________________charge= _______ 9. Beryllium: valence = _____ for a full/empty orbital __________________charge= _______ 10. Neon: valence = _____ for a full/empty orbital __________________charge= _______ 11. Helium: valence = _____ for a full/empty orbital __________________charge= _______ 12. Flourine: valence = _____ for a full/empty orbital __________________charge= ______ 13. Boron: valence = _____ for a full/empty orbital __________________charge= _______ 14. Sulfur: valence = _____ for a full/empty orbital __________________charge= _______ 15. Nitrogen: valence = _____ for a full/empty orbital __________________charge= _______ Name: ____________________________________ (1 of 3) Math Set # 20 Lewis Structures and Ionic Bonds REMEMBER: An ionic bond is created between metals and nonmetals. This is because a metal in group 1 or 2 gives up electrons easily and nonmetals in groups 16 through 18 accept electrons easily. An ionic bond results in two or more ions being attracted to each other. The total charge of the molecule must be zero. Directions: For each combination of atoms indicate how many electrons are passed from one atom to the other, the ions created, and the molecular formula. EXAMPLE: Hydrogen and Chlorine What will happen to the electrons? Hydrogen will give an electron to Chlorine The resulting ions? H+ Cl-­‐ The formula for this compound: HCl 1. Sodium and Chlorine What will happen to the electrons? The resulting ions? The formula? 2. Magnesium and Oxygen What will happen to the electrons? The resulting ions? The formula? 3. Beryllium and Sulfur What will happen to the electrons? The resulting ions? The formula? 4. Hydrogen and Fluorine What will happen to the electrons? The resulting ions? The formula? 5. Lithium and Chlorine What will happen to the electrons? The resulting ions? The formula? Name: ____________________________________ (2 of 3) Math Set # 20 Lewis Structures and Ionic Bonds Lewis Structures REMEMBER: A full valence for all elements except Hydrogen and Helium and the transition metals is 8. Hydrogen and Helium has a full valence of 2. DIRECTIONS: 1. Write the element symbol 2. Find the number of valence electrons 3. Place one dark circle next to the symbol for each valence electron. IMPORTANT RULE: electrons are added one to each side of the symbol until all the sides have a single electron. Additional electrons make pairs on each side. Examples: H Draw Lewis Structures for the Atoms. 1. Calcium 7. Nitrogen 13. Thallium 2. Chlorine 8. Magnesium 14. Sulfur 3. Carbon 9. Hydrogen 15. Arsenic 4. Neon 10. Lithium 16. Fluorine 5. Oxygen 11. Lead 17. Radon 6. Sodium 12. Iodine 18. Aluminum
C Se Xe Name: ____________________________________ Math Set # 20 Lewis Structures and Ionic Bonds EXAMPLES: Hydrogen and Iodine (3 of 3) + H
I Hydrogen will give one electron to Iodine. Hydrogen with have a + charge Iodine will have – charge. DIRECTIONS: Draw the Lewis Structure for the following molecules. Use one color for the symbol and electrons coming from the first atom and another color for the symbol and electrons coming from the second atom. Make each diagram look like the example. 1. Sodium and Chlorine 2. Magnesium and Oxygen 3. Beryllium and Sulfur 4. Hydrogen and Fluorine 5. Lithium and Chlorine -­‐ Name: ____________________________________ (1 of 4) Math Set # 21 Naming Molecules with Ionic Bonds REMEMBER: An ionic bond is always between a metal (left side of the periodic table) and a nonmetal (right side of the periodic table) Rules for IONIC molecules 1. Always name elements from left to right on the periodic table (the positive ion goes first) 2. name the positive element without changing anything. 3. Name the negative element but change the end to an “ide” (NOTE: You do not do anything with prefixes for ionic molecules.) You can think of this as: ELEMENT ELEMENT”ide” EXAMPLE: Chlorine and Hydrogen Name: Hydrogen Chloride DIRECTIONS: Give the names for the following molecules: 1. Magnesium and Chlorine ________________________________________________ 2. Bromine and Rubidium ________________________________________________ 3. Hydrogen and Suflur ________________________________________________ 4. Lithium and Oxygen ________________________________________________ 5. Selenium and Calcium ________________________________________________ 6. Radium and Astatine ________________________________________________ 7. Potassium and Polonium ________________________________________________ 8. Chloride and Potassium ________________________________________________ 9. Lithium and Phosphorous ________________________________________________ 10. Iodine and Sodium ________________________________________________ Name: ____________________________________ (2 of 4) Math Set # 21 Naming Molecules with Covalent Bonds REMEMBER: A covalent bond is always between molecules that are both on the right side of the periodic table. Rules for COVALENT molecules 1.
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Always name elements from left to right on the periodic table Always name elements from top to bottom on the periodic table name the first element without changing anything. Name the last element but change the end to an “ide” Add prefixes to show the number of each atom in the molecule The ONLY time there is not a prefix in front of a name is when the very first element has only one atom. (prefixes are on page 393 of your textbook) EXAMPLES: One Carbon and two Oxygen Name: Carbon Dioxide One Carbon and One Oxygen Name: Carbon Monoxide Two Carbon and Four Oxygen Name: Dicarbon Tetraoxide Name the following molecules: 1. Two Nitrogen and one Oxygen _______________________________________________ 2. One Carbon and four Flourine _______________________________________________ 3. Two Phosphorous and five Oxygen _______________________________________________ 4. Two Boron and six Silicon _______________________________________________ 5. One Selenium and six Fluoride _______________________________________________ 6. Two Silicon and six Bromine _______________________________________________ 7. One Sulfure and four Chlorine ________________________________________________ Give the number of atoms and the name of the elements for the following molecules: 8. iodine pentafluroide ________________________________________________________________ 9. dinitrogen trioxide ________________________________________________________________ 10. phosphorous triiodide ________________________________________________________________
Name: ____________________________________ (3 of 4) Math Set # 21 Chemical Formulas A subscript it gives the number of atoms of the element just in front of it. A coefficient (large number in front )of the molecule gives how many molecules there are. EXAMPLES: H2O has 2 Hydrogen and 1 Oxygen 5 H2O has five molecules of H20 so there are 10 Hydrogen and 5 Oxygen 7NH4 has 7 molecules of Nitrogen and 28 molecules of Hydrogen DIRECTIONS: Give the number of each kind of atom in each formula 1. Al2O3 _____________________________________________________________ 2. 2 Al2O3 3. C2H6 4. 3 C2H6 5. Na2SO4 6. 5 Na2SO4 7. Fe2Br3 8. 10 Fe2Br3 9. 25 Fe2Br3 10. 11 Mg3P2 _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ Name: ____________________________________ Math Set # 21 Balancing Chemical Equations (4 of 4) Balancing Equations 1. Write the equation without any coefficients. 2. Calculate the number of each type of atom on the left side of the arrow. 3. Calculate the number of each type of atom on the right side of the arrow. 4. Add coefficients in front of the molecules until the left side and right side numbers match. IMPORTANT: You can only change coefficients. You CANNOT change subscripts. Examples: Balance the Equation H + O2  H2O left 1 H, 2 O right 2 H, 1 O I give H2O a coefficient of 2 so that the number of oxygen will match H + O2  2 H2O left 2 H, 2 O right 4 H, 2 O I give H a coefficient of 4 so that the number of Hydrogen will match 4H + O2  2 H2O left 4 H, 2 O right 4H, 2 O Balance the Equation Fe + H2O  Fe3O4 + H2 left 1 Fe, 2 H, 1 O right 3 Fe, 2 H, 4 O I give H2O a coefficient of 4 in order to balance the oxygen Fe + 4H2O  Fe3O4 + H2 left 1 Fe, 8 H, 4 O right 3 Fe, 2 H, 4 O I give the Fe a coefficient of 3 in order to balance the iron 3Fe + 4H2O  Fe3O4 + H2 left 3 Fe, 8 H, 4 O right 3 Fe, 2 H, 4 O Everything matches except of the hydrogen. To fix this I give H2 a coefficient of 4. 3Fe + 4H2O  Fe3O4 + 4H2 left 3 Fe, 8 H, 4 O right 3 Fe, 8 H, 4 O DIRECTIONS: Balance the following Equations: 1. H2 + Cl2  HCl 2. Mg + O2  MgO Name: ____________________________________ Math Set # 22 Balancing Chemical Equations DIRECTIONS: Balance the following Equations: 1. KI + Br2  KBr + I2 2. H2 + Cl2  HCl 3. S8 + O2  SO 4. Fe2O3 + C  Fe + CO2 5. Sb + I2  SbI3 6. KBr + Cl2  Br2 + KCl 7. C3H8 + O2  3 CO2 + 4H2O 8. CHALLENGE: C6H14 + O2  H2O + CO2 (1 of 3) Name: ____________________________________ (2 of 3) Math Set # 22 Identifying Reaction Types REACTION TYPES: Synthesis: Two or more reactants combine to make a single product Example: 2 Na + Cl2  2 NaCl Decomposition: A single reactant breaks down to make two or more products Example: H2CO3  H2O + CO2 Single-­‐Displacement: An element replaces another element that is part of a compound Example: Zn + 2HCl  ZnCl2 + H2 Double-­‐Displacement: An element in one compound changes places with an element in another compound Example: NaCl + AgF  NaF + AgCl Combustion Reaction: A carbon compound plus O2 produces heat, CO2 and H2O. Example: CH3OH + O2  CO2 + 2H2O (Hint: look for O2 on one side and H2O on the other) DIRECTIONS: Label each reaction with the reaction type: 1. H2 + Cl2  2HCl 2. 2Mg + O2  2 MgO 3. 2C2H6 + 7O2  4 CO2 + 6H2O 4. H2CO3  CO2 + H2O 5. CH4 + 2O2  CO2 + 2H2O 6. AgNO3 + KCl  AgCl + KNO3 7. 2KClO3  2KCl + 3 O2 8. Zn + HCl  ZnCl2 + H2 9. 2KCl + Na2CO3  K2CO3 + 2NaCl 10. 2H2O  2H2 + O2 Name: ____________________________________ Math Set # 22 Activation Energy (3 of 3) 1. Answer the following questions based on the potential energy diagram shown here: a.
Does the graph represent an endothermic or exothermic reaction? b.
Label the position of the reactants, products, and activated complex. c.
How much energy is released or absorbed during the reaction? d.
How much energy is required for this reaction to occur? 1. Answer the following questions based on the potential energy diagram shown here: a.
b.
Label the position of the reactants, products, and activated complex. c.
d.
How much energy is released or absorbed during the reaction? e.
How much energy is required for this reaction to occur? Does the graph represent an endothermic or exothermic reaction?