NAME: IPC SEMESTER 2 REVIEW SHEET UNIT #1 CLASSIFICATION OF MATTER 1. Complete the table below to compare and contrast solids, liquids, and gases. Use the word bank provided. NOTE: ALL WORDS MAY BE USED MORE THAN ONCE AND YOU MAY NOT FILL ALL OF THE SLOTS Definite shape Indefinite shape Definite volume Indefinite volume Particles vibrate in place Particles move slightly Particles move rapidly State of matter SOLID LIQUID GAS 2. One property that all particles of matter have in common is they a. Never move in solids b. Only move in gases c. Move constantly d. None of the above 3. Match the following vocabulary words with their correct definitions. 1. melting point A. change from a gas to a liquid 2. boiling point B. temperature at which a substance freezes 3. freezing point C. temperature at which a substance boils 4. condensation D. change from a liquid to a gas 5. vaporization E. change from a liquid to a gas 6. freezing F. temperature at which a substance melts 1
4. is being added between point A and B. This causes the molecules in the substance to more rapidly and thus a rise in the temperature. 5. At point B, the temperature of the substance is. 6. At point C, the substance is completely in the state. 7. Between points D and E the substance is being changed into the state. 8. Describe the difference between a chemical and physical property. 9. Describe the difference between a chemical and physical change. UNIT #2 CHEMICAL BONDING 1. Which part of the atom is responsible for chemical bonding? 2. What are valence electrons(be specific)? 3. Where are valence electrons located (be very specific)? 4. How many valence electrons do most atoms need to have a complete outer shell and be happy? 5. Which two elements only need two valence electrons to be happy? 6. If an element gives away an electron, will it form a positive ion or a negative ion? 2
7. If an element gains an electron, will it form a positive ion or a negative ion? 8. Why does an ion have a charge (be specific)? 9. How do ionic bonds form? 10. How do covalent bonds form? 11. Bond the following atoms. Determine if they are ionic or covalent, circle your choice. Show the valence electrons and how they are either shared between the atoms or how they are transferred between atoms. Then write the chemical formula in the space provided. Ionic or covalent Ionic or covalent C Cl Mg Cl Formula Formula UNIT #3 PERIODIC TABLE Complete the following chart: 3
Draw the Bohr models for the following elements: 1. Oxygen 2. Chlorine 3. Neon 4. Sodium Draw the electron dot diagram for the following elements: 1. Calcium 2. Cobalt 3. Gallium 4. Sulfur Fill in the blanks: 1. A column on a periodic table is called a or. 2. Elements in the same column of the periodic table have the same number of. 3. Elements in the same column of the periodic table have similar properties. 4. A row on a periodic table is called a. 4
5. Elements in the same row have the same number of. 6. Elements in the noble gas family are stable (unreactive) because they have valence electrons. 7. Elements that have the characteristics of both metals and nonmetals are called. 8. Three properties of metals are,, and. 9. Three properties of nonmetals are,, and. UNIT #4 NOMENCLATURE Name the following compounds and tell what type of compound they are (ionic or covalent). 23. FeBr3 24 CBr4 25. Na2SO4 Write the formulas for the following compounds. 26. sodium chlorate 27. lead(ii) phosphate 28. magnesium carbonate 29 ammonium chloride What are the prefixes used to name molecular substances with the following number of atoms? 39. one 40. two 41. three 42. four 43. five 44. eight 5
UNIT #5 BALANCING AND IDENTIFYING REACTION TYPES 1. Zn (s) + AgNO3 (aq) Zn(NO3)2 (aq) + Ag (s) 2. N2 (g) + H2 (g) NH3 (g) 3. NaCl (aq) + AgC2H3O2 (aq) NaC2H3O2 (aq) + AgCl (s) 4. Mg(OH)2 (aq) + H3PO4 (aq) H2O (l) + Mg3(PO4 )2 (aq) 5. HNO3 (aq) + Ni (s) Ni(NO3)2 (aq) + H2 (g) 6. methane (CH4) + oxygen carbon dioxide + water 7. potassium carbonate potassium oxide + carbon dioxide 8. Identify the reaction types for each question above (synthesis, decomposition, single replacement, double replacement, combustion) #1 #2 #3 #4 #5 #6 #7 9. Describe how the activity series is used in determining whether a single replacement reaction will occur or not. 6