Unit 2: The Periodic Table
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1 Unit 2: The Periodic Table The following pages are practice questions for this unit, and will be submitted for homework! You must complete: Unit Vocabulary ALL QUESTIONS What Group Am I? ALL QUESTIONS Properties: Metals vs. Non-Metals ALL QUESTIONS Group Matching ALL QUESTIONS Who Lives Here? ALL QUESTIONS Periodic Trend Practice ALL QUESTIONS DUE: Monday October 22,
2 Unit Vocabulary Alkali Metals: Alkaline Earth Metal: Atomic radius: Electronegativity: Family: Group: Halogen: Ionic radius: Ionization energy: Metal: Metalloid: Noble Gas: Nonmetal: Period: Transition metals: 2
3 What Group Am I? Directions: Using your knowledge of chemistry, determine the specific group name of each element. Explain your answer Element Specific Group Name Reasoning Zinc (Zn) Tungsten (W) Krypton (Kr) Vanadium (V) Francium (Fr) Xenon (Xe) Iodine (I) Silicon (Si) Cobalt (Co) Barium (Ba) 3
4 Properties: Metals vs. Non-Metals Directions: Using your knowledge of chemistry, write M if the property describes a metal or NM is the property describes a non-metal. 1. Dull 2. Malleable 3. Luster 4. Ductile 5. Many are gases 6. Brittle (if solid) 7. High density 8. Low density 9. Poor conductor of heat and electricity 10. High melting and boiling point 11. Good conductor of heat and electricity 12. Low melting and boiling point 13. Solids Group Matching Directions: Using your knowledge of chemistry, match the description of the group on the periodic table to its name. Description Group 1, most active metals, react vigorously with water to produce H 2 (g), shiny, easily cut with a knife, reactivity increases as you go down this group. Can be found next to the stair-step line in the periodic table, have physical properties similar to those of metals and chemical properties of nonmetals, solids, shiny, or dull, semi-conductors, (B, Si, Ge, As, Sb, Te, Po) Group 18, colorless gases, do not chemically react with other elements (inert/stable) because of full outer shell (8 valence electrons), usually do not bond with other atoms, are monoatomic (unbonded single atoms) Group 17,, have 7 valence electrons, most active nonmetals, chemical reactivity decreases as you go down the group, form diatomic (2 atoms bonded) molecules Group Name A. Alkali Earth metals B. Transition Metals C. Halogens D. Alkali Metals E. Nobel Gases Group 2, second most active metals Groups 3-12, hard solids, exception mercury (Hg) is a liquid, high melting points, for colored compounds, less reactive than alkali metals F. Metalloids 4
5 Who Lives Here? Directions: Using your knowledge of chemistry, determine which element lives at the address given. 1. The intersection of the Alkali Earth Metal group and Period The intersection of Group 9 and Period The intersection of the Halogens and Period The intersection of the Alkali Metal group and Period The intersection of Period 6 and Group 11. Periodic Trend Practice Directions: Determine if the three trends, shown below, increase or decrease and you move down a group or across (Left à Right) a period. Use the trends to answer the questions below. 1. For each set of atoms, determine which atom has the largest atomic radius. Atom 1 Atom 2 Atom 3 Atom 4 Largest in Set Lithium Carbon Nitrogen Fluorine Calcium Beryllium Radium Magnesium Krypton Zinc Calcium Bromine Polonium Sulfur Oxygen Tellurium 5
6 2. For each set of atoms, determine which atom has the highest electronegativity. Atom 1 Atom 2 Atom 3 Atom 4 Largest in Set Chlorine Sulfur Aluminum Magnesium Boron Indium Aluminum Gallium Nitrogen Oxygen Fluorine Calcium Lithium Calcium Francium Silicon 3. For each set of atoms, determine which atom has the lowest ionization energy electronegativity. Atom 1 Atom 2 Atom 3 Atom 4 Largest in Set Nitrogen Fluorine Oxygen Carbon Iodine Bromine Fluorine Chlorine Lithium Beryllium Boron Carbon Aluminum Silicon Phosphorus Sulfur 4. Which would be larger: The ionic radius or the atomic radius? EXPLAIN IN TERMS OF ELECTRONS a. Calcium b. Fluorine c. Bromine d. Potassium 6
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