Name: Hour: Unit 2 Periodic Table Nomenclature Notepack Chapters 5 and 6 1
Periodic Table & Nomenclature Chapter 5 Part One: Review of Atomic Structure (Pages 107-121) A. Define atom 1. proton - 2. neutron- 3. electron 4. nucleus 5. electron energy levels (orbitals) 6. isotopes - B. Define atomic number Mass number C. Draw a simple model of a Helium-4 atom: D. Draw a simple model of a Calcium-40 atom: REVIEW QUESTIONS: 1. What subatomic particle gives an atom its identity? 2. An atom is identified as platinum-195. a. What does the number represent? b. How many protons? c. How many neutrons? d. How many electrons? 3. How are isotopes of the same element alike? How are they different? 4. Draw a model of an argon-40 atom: 2
Chapter 5 Part Two: Review of the Periodic Table: (Pages 123-126) A. What is the periodic table of elements? B. Elements are arranged into rows and columns according to similarities in their properties: 1. Define Groups a. where are the group A elements? b. What are they known as? c. where are the group B elements? d. what are they known as? **Number your periodic table, matching the organization on page124. 2. Define Periods How many periods are on the periodic table? 3. The representative elements can be broken down into three general categories: For each category, list distinguishing properties for them: a. metals b. nonmetals c. metalloids **Mark on your periodic tables the location for each of these categories: Remember the HYDROGEN RULE EXCEPTION!!! 4. What are the group 1A elements known as? 5. What are the group 2A elements known as? 6. What are the group 7A elements known as? 7. What are the group 8A elements known as? 8. Where are the inner transition metals (also called rare earth elements) located? 9. What are the two rows called and why? 10. What period do they belong to? 3
11. 80% of the elements are metals. All metals are solids at room temperature with one exception. What is the name, symbol, and physical state of this element? REVIEW: 1. Identify each element as a metal, metalloid, or nonmetal: a. gold b. silicon c. manganese d. sulfur e. barium 2. Which of the elements in the question above are representative elements? 3. Give the symbol of each element that fits the description: a. any nonmetal in Group 4A: b. the inner transition metal with the lowest atomic number: c. the two elements that are liquid at room temperature: d. any metal in Group 5A: 4. Fill in the following grid: Use your periodic tables! Element Name Symbol Number of Protons Number of Neutrons Number of Electrons Mass Number Calcium 20 Mg 24 53 76 16 31 Atomic Number 1. Draw Simple Models of the following atoms: A. Phosphorus B. Potassium Chapter 6: Nomenclature 6.1 Introduction to Chemical Bonding Ions and Ionic Compounds A. Define Ion B. Define cation- 4
C. Define anion D. How do ions form? Let s use an orbital diagram and electron configuration to help illustrate 1. sodium atom to sodium ion: 2. chlorine atom to chloride ion: E. What type of bond have we formed in the above compound? F. Show a magnesium atom forming a magnesium ion: G. How can we form a compound between magnesium and chlorine? Draw the diagrams here: H. How do we name positive ions? I. How do we name negative ions? J. Describe some physical properties that ionic compounds have in common: Page 137 top paragraph REVIEW: 1. Give the name and symbol of the ion formed when a. a sulfur atom gains two electrons b. an aluminum atom loses three electrons 5
c. a calcium atom loses two electrons 2. How many electrons are lost or gained in forming each ion? a. Ba +2 b. As 3 c. Cu +2 d. S -2 There is a pattern in predicting how many electrons are lost and gained for the REPRESENTATIVE elements, can you guess it? WRITE ON YOUR PERIODIC TABLES THE CHARGES OF THE REPRESENTATIVE ELEMENTS NOW. We cannot determine how many electrons are lost for the transition metals because their electrons number in their outermost shell can change. Chapter 6: Molecular Compounds 1. Molecules and Molecular Compounds: A. Define molecule B. What type of elements are chemically bonded together in a molecule? C. What type of bond exists between the atoms in a molecule? D. Describe how this bond forms: Use a basic model of a hydrogen molecule to help E. Use an Electron Dot structure to show the covalent bonds in a water molecule: F. Draw the Electron Dot Structure for the Water Molecule. G. Draw the Electron Dot Structure for Carbon Dioxide, CO2 H. Create a list of physical properties that molecules share: Page 134 bottom paragraph 6
Chapter 6: Chemical Names and Formulas Reminder: There is a pattern in predicting how many electrons are lost and gained for the REPRESENTATIVE elements, can you guess it? WRITE ON YOUR PERIODIC TABLES THE CHARGES OF THE REPRESENTATIVE ELEMENTS NOW. We cannot determine how many electrons are lost for the transition metals because their electrons number in their outermost shell can change. Section 6.2 Representing Chemical Compounds 1. What is a chemical formula? 2. What do we use to represent the formula of a monatomic (one atom) of an element? 3. IMPORTANT: In nature, there are 7 elements that don t exist as monatomic elements, rather they exist as diatomic elements when they are alone. What are they? Write their symbols below, and put a star in their boxes on your periodic table so you don t forget them. 4. What is a molecular formula? 5. What information can be gathered from the molecular formula CO2? 6. What is a formula unit? 7. Describe how formula units exist in nature? Remember, we know how to form and name ions formed from Group A, or representative, elements. But what about Group B?? page144 8. How can we tell someone how many electrons lost for the transition metals? Examples: Name the following transition metal ions: For help, refer to page 144, table 6.3 a. tin (lost 2 electrons) b. tin (lost 4 electrons) c. iron (lost 3 electrons) d. iron (lost 2 electrons) 7
There are 3 exceptions to this rule: 1. Silver is always a +1 2. Zinc and Cadmium are always a +2 Place their charges in their boxes on your periodic table so you don t forget this rule. DO NOT USE A ROMAN NUMERAL WHEN NAMING SILVER, ZINC AND CADMIUM IONS. ALWAYS USE A ROMAN NUMERAL WHEN NAMING ANY OTHER TRANSITION METAL ION. REVIEW OF FORMING AND NAMING MONATOMIC IONS: 1. What is the charge of the ion typically formed by each element? a. sulfur b. lead (4 electrons lost) c. strontium d. argon e. bromine f. copper (1 electron lost) g. selenium h. silver i. cesium j. phosphorus 2. Write the name of each ion formed in the question above: a. e. i. b. f. j. c. g d. h. 3. Name each ion above as an cation or anion: a. e. i. b. f. j. c. g. d. h. Section 6.4 Ionic Compounds A. Writing Formulas for Binary Ionic Compounds 1. What are Binary Ionic Compounds? 2. What are the rules for writing Binary Ionic Compounds? a. Write the metal (positive) ion first b. Write the nonmetal (negative) ion last c. The net charge for the compound must add to zero (total positive + total negative = 0) d. Use subscripts to indicate how many of each ion you need to balance the charge. e. Another approach to writing a balanced formula for a compound is to use the crisscross method. In this method, the numerical charge of each ion is crossed over and used as the subscript for the other ion. The signs of the numbers are dropped. Practice: *Write the formula for the binary ionic compound formed between magnesium and chlorine. 8
NAME IT *Write the formula for the binary ionic compound formed between sodium and oxygen. NAME IT *Write the formula for the binary ionic compound formed between aluminum and sulfur. NAME IT *Write the formula for the binary ionic compound formed between iron (III) and oxygen. NAME IT *Write the formula for the binary ionic compound formed between calcium and sulfur. NAME IT PRACTICE PROBLEMS: 1. Write the formulas for the compounds formed between these pairs of ions. NAME THEM. a. Ba +2, S -2 b. Li +1, O -2 c. Ca +2, N -3 d. Cu +2, I -1 2. Write formulas for these compounds. a. sodium iodide d. rubidium nitride b. tin (II) chloride e. barium fluoride c. potassium sulfide f. lithium bromide 3. Write names for these binary ionic compounds a. ZnS b. KCl c. BaO d. CuBr2 e. CuO (careful!) f. Ag2S g. Al2Se3 Polyatomic Ions A. What is a polyatomic ion? B. What endings to polyatomic ions receive when naming them? C. There are 3 important exceptions, they are: D. Use chart 6.4 to write the formulas for the following polyatomic ions: 1. ammonium ion 2. sulfate ion 9
3. sulfite ion 4. carbonate ion 5. nitrate ion 6. permanganate ion 7. hypochlorite ion 8. phosphate ion 9. cyanide ion 10. hydroxide ion Reminder: What is a molecule? What is a polyatomic ion? Compare the polyatomic ion sulfite and the molecule sulfur trioxide: Ternary Ionic Compounds A. Define ternary ionic compounds Remember, they are still just two ions, and all rules from before still apply! B. Write the formula for lithium nitrate, a ternary compound: C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this happens, place the polyatomic ion in parenthesis and the subscript outside of the parentheses. D. Write the formula for aluminum carbonate: E. Write the formula for ammonium sulfate: F. Write the formula for calcium phosphate: G. Write the formula for beryllium carbonate: Practice Problems: 1. Write the formulas for compounds formed AND name the compound from these pairs of ions: a. NH4 +1, SO3 2- b. Calcium ion, phosphate ion c. Al 3+, NO3-1 d. Potassium ion, chromate ion 2. Write formulas for these compounds a. lithium hydrogen sulfate b. chromium (III) nitrite 10
c. mercury (II) bromide d. ammonium dichromate 3. Name these compounds: a. LiCN b. (NH4)2C2O4 c. Fe(ClO3)3 d. Sr(H2PO4)2 e. CaC2O4 f. KClO g. KMnO4 h. Li2SO3 Section 6.5 Molecular Compounds and Acids A. Binary Molecular Compounds 1. What is a binary molecular compound? 2. We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following: Prefix Number Prefix Number 1 6 2 7 3 8 4 9 5 10 How do we name binary molecular compound?? *Say the name of the first element, say the name of the second element, ending in IDE, and put the appropriate prefix in to indicate how many of each element there are in the formula: **If the prefix for the first element in a binary molecular compound, it may be dropped. However, it must be said if it is for the second element. **Don t reduce the subscripts (like you did for binary ionic compounds) Name these binary molecular compounds a. N2O b. PCl3 c. SF6 d. OF2 e. Cl2O8 f. SO3 Write formulas for the following binary molecular compounds a. nitrogen trifluoride b. disulfur dichloride c. dinitrogen tetroxide d. octoxygen dichlorice e. trinitrogen pentoxide NAMING ACIDS A. What are acids? 11
B. Write with me the chart that explains how to name acids: C. Practice naming the following acids: 1. HCl 2. HClO3 3. HClO2 4. HClO 5. HClO4 6. H2S 7. H2SO3 8. H2SO4 9. HC2H3O2 D. Write the formula for the following acids: 1. nitric acid 2. hydronitric acid 3. nitrous acid 4. hydrocyanic acid 5. phosphoric acid 6. hydrobromic acid 7. acetic acid 8. nitric acid 12
The Atom Video Notes NAME 1. How long have we been trying to see atoms? 2. With who did the idea of an atom first originate? a. Aristotle B. Democritus c. Mendeleev d. Curry 3. This person also originated the word to represent the smallest particles that make up matter 4. In the early 1800s, a scientist named added to this atomic theory by stating that atoms always combine in simple, whole number ratios. 5. The three basic components of an atom are the, which are positively charged, the, which are neutral, and finally the, which are negatively charged. 6. The two basic regions in an atom are the center area called the and the outer region called the 7. The number of determines an atom s identity. 8. The number of in the cloud will equal the number of in the nucleus. 9. What region of the atom contains the majority of the mass of the atom? 10. What region of the atom is by far the biggest? 11. In 1981, two scientists working for IBS invented the, or STM, which enabled us to see atoms. 12. This invention produces 2-D or 3-D, and color enhanced pictures. True or False 13. Hold the electrons and nucleus together and determines the atom s chemical reactivity. 14. Two positive objects will each other. (repel or attract) 15. Two negative objects will each other. (repel or attract) 16. One positive and one negative charge will each other. (repel or attract) 17. The Crook s Tube is a glowing stream of electrons. True or False 18. Atoms are neutral. True or False 19. Rutherford s Gold Foil experiment determined that an atom is mostly empty space, with very small, positively charged central cores. True or False 20. Electrons move around the nucleus in the same way that planets orbit the sun. True or False 21. are the most important part of an atom because it determines the chemistry of the atom. 22. S clouds represent the shape electron orbital. 23. P clouds represent the shape of an electron orbital. 24. Each of these shapes represents different, or states. 25. Which cloud is the lowest energy? Which cloud is the highest energy? 26. Each atom has a unique cloud shape, and therefore unique energy patterns. True or False 27. What is the technique called that scientists use the electron energy signal to identify and quantify the atoms in an unknown sample? 13
The Periodic Table Movie Notes NAME HR 1. Who invented the periodic table? 2. What are the two types of properties and give examples of each: a. b. 3. What language is the common language used when naming elements long ago? 4. How many neutrons in the rate isotope of helium? What is it s mass number? 5. Elements within a group all have similar. 6. What was prized more than jewels and gold? 7. Describe what happens when the alkali metals are dropped into water: What gas is produced? 8. How does the size of an atom change as you do down a group? How does the size of an atom change as you move across a period? 9. When a steel ball is dropped on a piece of glass containing sodium, what happens? What happens when potassium is used instead of sodium? Why?? 10. Who is Glen Seaborg? What did he contribute to the periodic table? 14
What year did he win the Nobel prize in chemistry? 11. What determines the arrangement of the modern periodic table of elements? 12. What do energy diagrams illustrate? 13. Draw the electron arrangement of the sodium atom: 14. What are valence electrons? 15. List the three basic rules for filling electron orbitals: a. b. c. 16. What is x-ray fluorescence used for? How does it work? 15