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) 9. With the exception of the element _mercury_, all of the metals are in the _solid_ state at 25 o C. 10. List the symbols for the five nonmetals that are solid at 25 o C C, S, P, Se, I one nonmetal that is liquid at 25 o C eleven nonmetals that are gases at 25 o C Br 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 6.7 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.? 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 e- 49. 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. 9. With the exception of the element, all of the metals are in the state at 25 o C. 10. List the symbols for the five nonmetals that are solid at 25 o C one nonmetal that is liquid at 25 o C eleven nonmetals that are gases at 25 o C 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 6.7 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.? 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?