Name: Teacher: Gerraputa

Transcription

1 Name: Teacher: Gerraputa 1. Which list of elements contains a metal, a metalloid, and a nonmetal? 1. Ag, Si, I 2 3.K, Cu, Br 2 2. Ge, As, Ne 4.S, Cl 2, Ar 2. The elements on the Periodic Table are arranged in order of increasing 1. mass number 2. atomic number 3. number of isotopes 4. number of valence electrons 3. Which elements are malleable and good conductors of electricity? 1. iodine and silver 3. tin and silver 2. iodine and xenon 4. tin and xenon 4. Which element is a metal that is in the liquid phase at STP? 1. bromine 3. hydrogen 2. cobalt 4. mercury 5. The carbon atoms in graphite and the carbon atoms in diamond have different 1. atomic numbers 3. electronegativities 2. atomic masses 4. structural arrangements 6. Which element is a solid at STP and a good conductor of electricity? 1. iodine 3. nickel 2. mercury 4. sulfur 7. At STP, which element is brittle and not a conductor of electricity? 1. S 3. Na 2. K 4. Ar 8. Which statement correctly describes two forms of oxygen, O 2 and O 3? 1. They have identical molecular structures and identical properties. 2. They have identical molecular structures and different properties. 3. They have different molecular structures and identical properties. 4. They have different molecular structures and different properties. 9. Which statement correctly describes diamond and graphite, which are different forms of solid carbon? 1. They differ in their molecular structure, only. 2. They differ in their properties, only. 3. They differ in their molecular structure and properties. 4. They do not differ in their molecular structure or properties. 10. Which element forms an ion that is larger than its atom? 1. aluminum 3. magnesium 2. chlorine 4. sodium 11. Which property is characteristic of nonmetals? 1. They have a high electronegativity. 2. They lose electrons easily. 3. They have a low first ionization energy. 4. They are good conductors of electricity. 12. Most metals have the properties of 1. brittleness and high ionization energy 2. brittleness and low ionization energy 3. ductility and high ionization energy 4. ductility and low ionization energy Page 1 of 7

2 13. Which symbol represents a particle that has the same total number of electrons as S 2? 1. O2 3. Se2 2. Si 4. Ar 15. Which list of elements is arranged in order of increasing electronegativity? 1.Be, Mg, Ca 3.K, Ca, Sc 2.F, Cl, Br 4.Li, Na, K 14. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar. Answer for #14: Page 2 of 7

3 Figure 1 Base your answer to the question on the information below and on your knowledge of chemistry. There are six elements in Group 14 on the Periodic Table. One of these elements has the symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium. 16. [Refer to figure 1] Explain, in terms of electron shells, why each successive element in Group 14 has a larger atomic radius, as the elements are considered in order of increasing atomic number. 18. Two forms of solid carbon, diamond and graphite, differ in their physical properties due to the differences in their 1.atomic numbers 3. isotopic abundances 2.crystal structures 4. percent compositions Answer for #16: 19. The elements in Group 2 are classified as 1. metals 3. nonmetals 2. metalloids 4. noble gases 17. Which general trends in first ionization energy and electronegativity values are demonstrated by Group 15 elements as they are considered in order from top to bottom? 1. The first ionization energy decreases and the electronegativity decreases. 2. The first ionization energy increases and the electronegativity increases. 3. The first ionization energy decreases and the electronegativity increases. 4. The first ionization energy increases and the electronegativity decreases. Page 3 of 7

4 Figure 2 The ionic radii of some Group 2 elements are given in the table below. 20. [Refer to figure 2] State the trend in ionic radius as the elements in Group 2 are considered in order of increasing atomic number. 23. Explain, in terms of atomic structure, why the atomic radius of iodine is greater than the atomic radius of fluorine. Answer for #20: Answer for #23: 21. Which atom in the ground state requires the least amount of energy to remove its valence electron? 1. lithium atom 3. rubidium atom 2. potassium atom 4. sodium atom 24. An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a 1. metal 3. nonmetal 2. metalloid 4. noble gas 22. When an atom of lithium loses an electron, the atom becomes a 1. negative ion with a radius smaller than the 2. negative ion with a radius larger than the 3. positive ion with a radius smaller than the 4. positive ion with a radius larger than the Page 4 of 7

5 25. Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms of Li, Na, K, and Rb, respectively? When the elements in Group 1 are considered in order from top to bottom, each successive element at standard pressure has 1. a higher melting and a higher boiling 2. a higher melting and a lower boiling 3. a lower melting and a higher boiling 4. a lower melting and a lower boiling 27. When an atom becomes a positive ion, the 1. decreases 2. increases 3. remains the same 28. The strength of an atom s attraction for the electrons in a chemical bond is the atom s 1. electronegativity 3. heat of reaction 2. ionization energy 4. heat of formation As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to 1. decreasing radius and decreasing shielding 2. decreasing radius and increasing shielding 3. increasing radius and decreasing shielding 4. increasing radius and increasing shielding 30. Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? 1. Both electronegativity and atomic radius increase. 2. Both electronegativity and atomic radius decrease. 3. Electronegativity increases and atomic radius decreases. 4. Electronegativity decreases and atomic radius increases. 31. Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? 1. Electronegativity increases, and first ionization energy decreases. 2. Electronegativity decreases, and first ionization energy increases. 3. Electronegativity and first ionization energy both increase. 4. Electronegativity and first ionization energy both decrease. 32. An ion of which element has a larger radius than an atom of the same element? 1. aluminum 3. magnesium 2. chlorine 4. sodium Page 5 of 7

6 33. Which Period 4 element has the most metallic properties? 1. As 3. Ge 2. Br 4. Sc 35. An ion of which element is larger than its atom? 1. Al 3.Ca 2. Br 4.Sr 34. Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? 1. The atomic radius decreases, and the first ionization energy generally increases. 2. The atomic radius decreases, and the first ionization energy generally decreases. 3. The atomic radius increases, and the first ionization energy generally increases. 4. The atomic radius increases, and the first ionization energy generally decreases. Page 6 of 7