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Unit 4: The Periodic Table Name: _________KEY____________ Text Questions from Corwin 4.4 1. List five properties of metals. solid, has luster, highly dense, has high melting point, and is a good conductor of heat and electricity 2. What is the difference between something being malleable and it being ductile? malleable = able to be hammered into thin sheets; ductile = able to be drawn into fine wire 3. List three properties of nonmetals. has a low density, low melting point, and is a poor conductor of heat and electricity 4. Solid nonmetals, such as _carbon_ and _sulfur_, have a _dull_ appearance. They _crush_ into a _powder_ if hammered. Eleven nonmetals occur naturally in the _gaseous_ state. 5. What is a semimetal, or metalloid? an element that has properties midway between those of metals and nonmetals 6. In the semiconductor industry, the semimetal silicon is used in the making of what two things? transistors and integrated circuits 7. On the periodic table, where are the metals and nonmetals, relative to each other? metals are on the left side; nonmetals are on the right 8. List the names and symbols of the eight semimetals mentioned in the text. astatine (At), boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), polonium (Po) o 9. With the exception of the element _mercury_, all of the metals are in the _solid_ state at 25 C. 10. List the symbols for the… …five nonmetals that are solid at 25oC C, S, P, Se, I …one nonmetal that is liquid at 25oC Br …eleven nonmetals that are gases at 25oC H, N, O, F, Cl, He, Ne, Kr, Xe, Rn 6.1 11. In the 1860s, Mendeleev proposed that the properties of the elements _repeat_ at regular intervals when they are arranged according to… increasing atomic mass 12. Today, Mendeleev is regarded as… the architect of the modern periodic table 13. Mendeleev had the insight to predict what? the existence and properties of three undiscovered elements 14. Why were the gases on the far right side of the periodic table originally called the inert gases? because they showed no chemical reactivity 15. Today, the “inert” gases are known as… the noble gases 6.2 16. According to Moseley, the elements should NOT be arranged according to _atomic_ _mass_ but rather according to… the number of protons in their nucleus 17. What does the periodic law state? that the properties of elements recur in a repeating pattern when arranged by increasing atomic # 6.3 18. With regard to the periodic table, what is the difference between a group and a period? group is a vertical column; period is a horizontal row 19. In the periodic table, there are _7_ periods and _18_ groups. 20. Although there has been historical disagreement about how to number the groups, today UIPAC recommends simply numbering the groups using… the numerals 1 through 18 21. What are the names given to the following groups of elements? Group 1: alkali metals Group 17: halogens Group 2: alkaline earth metals Group 18: noble gases 22. The _representative_ elements (also called the main-group elements) are found on the far _left_ and _right_ sides of the periodic table. The _transition_ elements are found in the _middle_ of the table, while the _inner_ _transition_ elements are found _beneath_ the main portion of the table. 23. The inner transition elements include, firstly, those of the _lanthanide_ series (so named because they follow the element _lanthanum_). These are considered to be a part of _Period_ 6. The elements of the _actinide_ series (so named because they follow the element _actinium_) are also inner transition elements and are a part of _Period_ 7. 24. Elements 93 and above are the results of what? high-energy synthesis in particle accelerators called “atom smashers” 25. Elements 93 and above have isotopes with lifetimes that last for… less than a millisecond 26. What are the transuranium elements? the elements following uranium (i.e., Np through element 118) 6.4 27. What is meant by the term “atomic radius”? the distance from the nucleus to the outermost electrons 28. What happens to the atomic radius of the atoms as we go up a group of elements from bottom to top? it increases 29. How do we explain the trend you stated in Q28? there are fewer energy levels of electrons surrounding the nucleus 30. What happens to the atomic radius of the atoms as we go from left to right with a period? it decreases 31. Because the number of protons increases as we go from left to right across a period, the nuclear charge _increases_. This has the effect of _pulling_ the electrons _closer_ _to_ the nucleus and _reducing_ the size of the atom. 32. As we move from left to right metallic character of the elements _decreases_. As we move up a group, metallic character _decreases_. 6.5 33. How did Mendeleev design the periodic table? so that elements with similar properties were placed in the same group 34. By understanding the organization of elements in the periodic table, it is possible to do WHAT? predict the products of chemical reactions 6.6 35. Groups 1 and 2 are collectively called the _s_ block. Groups 13 through 18 are called the _p_ block. Groups 3 through 12 are called the _d_ block. The inner transition elements comprise the _f_ block.? 6.7 36. What is significant about valence electrons? they form chemical bonds between atoms and are responsible for an element’s chemical behavior 37. The number of valence electrons is equal to the total number of electrons in… the outermost s and p sublevels 38. In the IUPAC designations for group numbers, the last digit of the numbers of the main-group elements indicates what? the number of valence electrons 39. Why is the maximum number of valence electrons equal to 8? because the s and p sublevels can hold only 2 + 6 = 8 electrons 6.9 40. The elements that easily lose electrons are the _metals_, which undergo chemical reactions by… losing one or more valence electrons 41. Metals become _positively_ charged after _losing_ electrons because… electrons are negatively charged 42. What is an ion? an atom bearing a charge 43. A. Define ionization energy. the amount of energy necessary to remove an e- from a neutral atom in the gaseous state B. Write the equation for the ionization energy of sodium. IE Na Na+ + e– 44. Why do the noble gases have such high ionization energies? their valence shells are completely filled (i.e., they don’t need to gain or lose e- to become stable) 45. Ionization energy _increases_ going up a group of elements and generally _increases_ from left to right across a period. 6.10 46. When metals and nonmetals react, what – specifically – happens with regard to both? metals lose e- from their valence shell; nonmetals add electrons to their valence shell 47. Metals become _positive_ ions and nonmetals become _negative_ ions. 48. What does it mean to say that two or more ions are isoelectronic? they have the same # of e49. From which sublevel do the transition metals first lose electrons? the highest s sublevel 50. In core notation, the noble gas symbol represents what? the nucleus and the inner electrons Unit 4: The Periodic Table Name: _________________________ Text Questions from Corwin 4.4 1. List five properties of metals. 2. What is the difference between something being malleable and it being ductile? 3. List three properties of nonmetals. 4. Solid nonmetals, such as _________ and ________, have a _____ appearance. They ______ into a ___________ if hammered. Eleven nonmetals occur naturally in the __________ state. 5. What is a semimetal, or metalloid? 6. In the semiconductor industry, the semimetal silicon is used in the making of what two things? 7. On the periodic table, where are the metals and nonmetals, relative to each other? 8. List the names and symbols of the eight semimetals mentioned in the text. o 9. With the exception of the element ______________, all of the metals are in the _______ state at 25 C. 10. List the symbols for the… …five nonmetals that are solid at 25oC …one nonmetal that is liquid at 25oC …eleven nonmetals that are gases at 25oC 6.1 11. In the 1860s, Mendeleev proposed that the properties of the elements __________ at regular intervals when they are arranged according to… 12. Today, Mendeleev is regarded as… 13. Mendeleev had the insight to predict what? 14. Why were the gases on the far right side of the periodic table originally called the inert gases? 15. Today, the “inert” gases are known as… 6.2 16. According to Moseley, the elements should NOT be arranged according to _________ ______ but rather according to… 17. What does the periodic law state? 6.3 18. With regard to the periodic table, what is the difference between a group and a period? 19. In the periodic table, there are ___ periods and ___ groups. 20. Although there has been historical disagreement about how to number the groups, today UIPAC recommends simply numbering the groups using… 21. What are the names given to the following groups of elements? Group 1: Group 17: Group 2: Group 18: 22. The _______________ elements (also called the main-group elements) are found on the far _____ and _______ sides of the periodic table. The ____________ elements are found in the ________ of the table, while the _______ ___________ elements are found __________ the main portion of the table. 23. The inner transition elements include, firstly, those of the _____________ series (so named because they follow the element _______________). These are considered to be a part of _________ 6. The elements of the ____________ series (so named because they follow the element ____________) are also inner transition elements and are a part of _________ 7. 24. Elements 93 and above are the results of what? 25. Elements 93 and above have isotopes with lifetimes that last for… 26. What are the transuranium elements? 6.4 27. What is meant by the term “atomic radius”? 28. What happens to the atomic radius of the atoms as we go up a group of elements from bottom to top? 29. How do we explain the trend you stated in Q28? 30. What happens to the atomic radius of the atoms as we go from left to right with a period? 31. Because the number of protons increases as we go from left to right across a period, the nuclear charge ___________. This has the effect of __________ the electrons ________ ___ the nucleus and ____________ the size of the atom. 32. As we move from left to right metallic character of the elements ___________. As we move up a group, metallic character _____________. 6.5 33. How did Mendeleev design the periodic table? 34. By understanding the organization of elements in the periodic table, it is possible to do WHAT? 6.6 35. Groups 1 and 2 are collectively called the ___ block. Groups 13 through 18 are called the ___ block. Groups 3 through 12 are called the ___ block. The inner transition elements comprise the ___ block.? 6.7 36. What is significant about valence electrons? 37. The number of valence electrons is equal to the total number of electrons in… 38. In the IUPAC designations for group numbers, the last digit of the numbers of the main-group elements indicates what? 39. Why is the maximum number of valence electrons equal to 8? 6.9 40. The elements that easily lose electrons are the ___________, which undergo chemical reactions by… 41. Metals become ______________ charged after _________ electrons because… 42. What is an ion? 43. A. Define ionization energy. B. Write the equation for the ionization energy of sodium. 44. Why do the noble gases have such high ionization energies? 45. Ionization energy ___________ going up a group of elements and generally __________ from left to right across a period. 6.10 46. When metals and nonmetals react, what – specifically – happens with regard to both? 47. Metals become ______________ ions and nonmetals become _______________ ions. 48. What does it mean to say that two or more ions are isoelectronic? 49. From which sublevel do the transition metals first lose electrons? 50. In core notation, the noble gas symbol represents what?