Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally decrease when the elements in Period 3 on the Periodic Table are considered in order from left to right? (1) metallic properties and atomic radius (2) metallic properties and ionization energy (3) nonmetallic properties and ionization energy (4) nonmetallic properties and atomic radius 3. Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to bottom on the Periodic Table? (1) a decrease in atomic radius (2) an increase in first ionization energy (3) a decrease in electronegativity (4) an increase in nonmetallic behavior 4. Which element is a metalloid? (1) Al (2) As (3) Ar (4) Au 5. Which general trend is found in Period 3 as the elements are considered in order of increasing atomic number? (1) increasing atomic radius (2) decreasing atomic mass (3) decreasing first ionization energy (4) increasing electronegativity 6. The elements on the Periodic Table are arranged in order of increasing (1) selected oxidation state (2) atomic mass (3) first ionization energy (4) atomic number 7. Which atom has the weakest attraction for electrons in a chemical bond? (1) a boron atom (2) a nitrogen atom (3) a fluorine atom (4) a calcium atom 8. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has (1) a total of eight valence electrons (2) more protons than neutrons (3) a total of two valence electrons (4) more neutrons than protons 9. Magnesium and calcium have similar chemical properties because a magnesium atom and a calcium atom have the same (1) total number of valence electrons (2) mass number (3) total number of electron shells (4) atomic number 10. Which element is a liquid at STP? (1) chlorine (2) argon (3) bromine (4) sulfur 11. Which statement describes the general trends in electronegativity and metallic properties as the elements in Period 2 are considered in order of increasing atomic number? (1) Both electronegativity and metallic properties decrease. (2) Both electronegativity and metallic properties increase. (3) Electronegativity decreases and metallic properties increase. (4) Electronegativity increases and metallic properties decrease. 12. Which Group 14 element is classified as a metal? (1) silicon (2) carbon (3) germanium (4) tin 13. Which atom in the ground state requires the least amount of energy to remove its valence electron? (1) sodium atom (2) lithium atom (3) potassium atom (4) rubidium atom Page 1
14. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) nonmetal (2) metalloid (3) noble gas (4) metal 15. As the elements is Period 3 are considered in order of increasing atomic number, there is a general decrease in (1) first ionization energy (2) atomic mass (3) electronegativity (4) atomic radius 16. Which list of elements contains a metal, a metalloid, a nonmetal, and a noble gas? (1) C, N, Ne, Ar (2) Be, Si, Cl, Kr (3) Na, Zn, As, Sb (4) K, Fe, B, F 17. The chemical properties of calcium are most similar to the chemical properties of (1) Ar (2) Sc (3) K (4) Mg 18. At STP, which element is solid, brittle, and a poor conductor of electricity? (1) K (2) S (3) Ne (4) Al Page 2
19. Base your answer to the following question on the information below. The atomic number and corresponding atomic radius of the Period 3 elements are shown in the data table below. Page 3
On the grid above, plot the data from the data table. Circle and connect the points. Page 4
Base your answers to questions 20 and 21 on the information below and on your knowledge of chemistry. Before atomic numbers were known, Mendeleev developed a classification system for the 63 elements known in 1872, using oxide formulas and atomic masses. He used an R in the oxide formulas to represent any element in each group. The atomic mass was listed in parentheses after the symbol of each element. A modified version of Mendeleev's classification system is shown in the table below. 20. Explain, in terms of chemical reactivity, why the elements in Group 18 on the modern Periodic Table were not identified by Mendeleev at that time. 21. Identify one characteristic used by Mendeleev to develop his classification system of the elements. 22. Base your answer to the following question on the elements in Group 2 on the Periodic Table. State, in terms of the number of electron shells, why the radius of a strontium atom in the ground state is larger than the radius of a magnesium atom in the ground state. Page 5
23. Base your answer to the following question on the information below. Identify one element from this table for each type of element: metal, metalloid, and nonmetal. 24. Base your answer to the following question on the information below. The atomic radius and the ionic radius for some Group 1 and some Group 17 elements are given in the tables below. State the relationship between atomic number and first ionization energy as the elements in Group 1 are considered in order of increasing atomic number. Page 6
25. Base your answer to the following question on the information below. The atomic and ionic radii for sodium and chlorine are shown in the table below. Explain, in terms of atomic structure, why the radius of an Na atom is larger than the radius of an Na + ion. Page 7
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