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2 6 The Periodic Table __ /__ pts Anticipatory Response 1. Elements in the same row & column behave similarly? Y N 2. Alkalis are in column 1? Y N 3. Metalloids are on the stair Steps of the table? Y N 4. Metals are on the right? Y N 5. A family, group, or column Are the same thing? Y N Anticipatory Response 1.Elements are bigger toward The right side of a row? Y N 2. Elements get bigger as you Move down a column? Y N 3. It’s harder to remove an electron from metals? Y N 4. Metals have higher ionization Energies than non‐metals? Y N 5. Shielding remains constant In a row or energy level? Y N Summary Section: 2 First Last Name___Per__ Cornell Question & Ans Directions: Make 5 questions & answers that are different than the Anticipatory Response 1. 2. 3. 4. 5. 3 PERIODIC TRENDS 3 Name:________________ Week of:__9/26/2016_____ Weekly Warm-Ups Monday Tuesday Wednesday Period:____ Name:________________ Thursday Friday Week of:__9/26/2016_____ Period:____ Name:________________ Week of:__10/03/2016_____ Weekly Warm-Ups Monday Tuesday Wednesday Period:____ Name:________________ Thursday Friday Week of:__10/03/2016_____ Period:____ 05_CTR_ch06 7/9/04 3:27 PM Page 131 6 Name ___________________________ 6.1 Date ___________________ Class __________________ ORGANIZING THE ELEMENTS Section Review Objectives • Explain how elements are organized in a periodic table • Compare early and modern periodic tables • Identify three broad classes of elements Vocabulary • • • • periodic law metals nonmetals metalloids Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Chemists used the of elements to sort them into groups. The periodic table organizes the elements into vertical and horizontal 3 4 2. _______________________ . The table is 3. _______________________ constructed so that elements that have similar chemical properties 4. _______________________ are in the same 5 in order of increasing 2 1. _______________________ . 6 when cut. Most nonmetals are have a high luster, or sheen, 5. _______________________ 7 6. _______________________ at room temperature. Elements with properties that are similar to those of metals 7. _______________________ 8 8. _______________________ and nonmetals are called . Across the periodic table, the properties of elements become 10 9 metallic and nonmetallic. 9. _______________________ 10. _______________________ 6 ↑ Chapter 6 The Periodic Table 131 05_CTR_ch06 7/9/04 3:27 PM Page 132 Name ___________________________ 7 Date ___________________ Class __________________ Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 10. In his periodic table, Mendeleev arranged the elements in order of atomic number. ________ 11. There are six periods in a periodic table. ________ 12. Most of the elements in the periodic table are metals. ________ 13. The elements within a period have similar properties. Part C Matching Match each description in Column B to the correct term in Column A Column A Column B ________ 14. metals a. a vertical column of elements in the periodic table ________ 15. periods b. good conductors of heat and electric current ________ 16. group c. poor conductors of heat and electric current ________ 17. nonmetals d. have properties that are similar to those of metals and nonmetals ________ 18. metalloids e. the horizontal rows of the periodic table © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part D Questions and Problems Answer the following questions in the space provided. 19. List the elements of Group 5A. Tell whether each is a metal, nonmetal, or metalloid. 20. List three properties of metals. 21. Name two elements that have similar properties to those of chlorine. 132 Core Teaching Resources 7 ↑ 05_CTR_ch06 7/9/04 3:27 PM Page 133 Name ___________________________ 6.2 8 Date ___________________ Class __________________ CLASSIFYING THE ELEMENTS Section Review Objectives • Describe the information in a periodic table • Classify elements based on electron configuration • Distinguish representative elements and transition metals Vocabulary • alkali metals • alkaline earth metals • halogens • noble gases • representative elements • transition metals • inner transition metals Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The periodic table displays the symbols and 1 of 1. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. the elements along with information about the structures of their 2 . The Group 1A elements are called 4 Group 2A elements are called through 7A are called the 6 are , and the 2A and 3A, there are 7 8 5 3 2. , and the 3. . The elements in Groups 1A 4. . The nonmetals of Group 7A 5. make up Group 8A. Between Groups 6. in periods 4 through 7 and 9 in periods 6 and 7. 7. 8. The atoms of the noble gas elements have their highest occupied 9. s and 10 sublevels filled. The highest occupied s and p sublevels of the representative elements are 11 . 10. 11. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 12. Group A elements are representative elements. 8 ↑ Chapter 6 The Periodic Table 133 05_CTR_ch06 7/9/04 3:27 PM Page 134 Name ___________________________ 9 Date ___________________ Class __________________ ________ 13. Chlorine has the electron configuration 1s22s22p63s23p7. ________ 14. The element in Group 4A, period 3, is gallium. ________ 15. There is a relationship between the electron configurations of elements and their chemical and physical properties. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B a. nonmetals of Group 7A ________ 17. inner transition metal b. an element in which the highest occupied s and p sublevels are filled ________ 18. representative element c. Group 2A elements ________ 19. transition metal d. an element whose highest occupied s sublevel and a nearby d sublevel contain electrons ________ 20. noble gas e. an element whose highest occupied s sublevel and a nearby f sublevel generally contain electrons ________ 21. alkaline earth metals f. Group 1A elements ________ 22. halogens g. an element whose highest occupied s or p sublevels are partially filled Part D Questions and Problems Answer the following in the space provided. 23. List the electron configurations for the highest occupied energy level of the elements in period 3 from left to right. 24. List the elements of Group 6A. Tell whether each is a solid, liquid, or gas at room temperature and whether it is a metal, nonmetal, or metalloid. 134 Core Teaching Resources 9 ↑ © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 16. alkali metals 05_CTR_ch06 7/9/04 3:27 PM Page 135 Name ___________________________ 10 Date ___________________ Class __________________ PERIODIC TRENDS 6.3 Section Review Objectives • Describe trends among elements for atomic size • Explain how ions form • Describe and explain periodic trends for first ionization energy, ionic size, and electronegativity Vocabulary • atomic radius • ion • cation • anion • ionization energy • electronegativity Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Atomic radii generally in a period. Atomic size 2 as you move from left to right with atomic number within a group because there are more occupied 3 3. 4 The energy required to remove an electron from an atom is . 4. 5. energy. This quantity generally 6 as you 6. move left to right across a period. Ions form when 7 are 7. than the 7. known as 5 2. and an increased shielding effect, despite an increase in nuclear 1. 8 transferred between atoms. Cations are always atoms from which they form. The ability of an atom to attract electrons when it is in a compound is called value 10 9 , and this as you move from left to right across a period. 8. 9. 10. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. Compounds are composed of particles called ions. 10 ↑ Chapter 6 The Periodic Table 135 05_CTR_ch06 7/9/04 3:27 PM Page 136 11 Name ___________________________ Date ___________________ Class __________________ ________ 12. Removing one electron from an atom results in the formation of a positive ion with a 1 charge. ________ 13. An anion has more electrons than protons. ________ 14. Elements with a high electronegativity value tend to form positive ions. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B ________ 15. ion a. half the distance between the nuclei of two atoms of the same element when the atoms are joined ________ 16. ionization energy b. a negatively charged ion ________ 17. electronegativity c. the energy required to remove an electron from an atom in its gaseous state ________ 18. atomic radius d. an atom or group of atoms that has a positive or negative charge ________ 19. cation e. a positively charged ion ________ 20. anion f. the ability of an atom of an element to attract electrons when the atom is in a compound © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part D Questions and Problems Answer the following in the space provided. 21. For the following pairs of atoms, tell which one of each pair has the largest ionic radius. a. Al, B b. S, O c. Br, Cl d. Na, Al e. O, F 22. Indicate which element of the following pairs is the most electronegative. a. calcium, gallium b. lithium, oxygen c. chlorine, sulfur d. bromine, arsenic 136 Core Teaching Resources 11 ↑ 05_CTR_ch06 7/9/04 3:27 PM Page 142 Name ___________________________ 6 12 Date ___________________ Class __________________ THE PERIODIC TABLE Chapter Quiz Fill in the word(s) that will make each statement true. 1. In the modern periodic table, when elements are arranged 1. 1 according to their atomic , there is a periodic repetition of properties. 6.1 2. 6.1 3 3. The elements in any in the periodic table have similar physical and chemical properties. 3. 6.1 4 4. Oxygen and sulfur, Group 6A elements, have electrons in their highest occupied energy level. 4. 6.2 5. For the inner transition elements, electrons are added to an 5 f sublevel with a principal energy level that is than the period number. 5. 6.2 2. There are 2 periods in the periodic table. Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 6.3 ________ 7. For Group 3A elements, there is a relatively small increase in ionization energy between the second and third ionization energies. 6.3 ________ 8. Anions are smaller than the neutral atoms from which they are formed. 6.3 ________ 9. Atoms with low electronegativity values tend to form positive ions. 6.3 ________ 10. As a group, alkali metals have the highest electronegativities. 6.3 142 Core Teaching Resources 12 ↑ © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 6. The atomic radius of an element in period 3 is larger that the atomic radius of an element in period 2. Name:_____________________________ Date:__________ Period: ________ Answer the following questions while watching the BrainPop video on the Periodic Table 1) How are elements categorized in the Period Table? 2) How are elements listed on the Period Table? 3) Period are vertical or horizontal (circle one) on the Periodic Table. 4) Groups are vertical or horizontal (circle one) on the Periodic Table 5) Why would Group 1 bond with Group 17 6) Write the characteristics of the following categories: Alkali Metals Alkali Earth Metals Transition Poor Semimetals NonMetals Nobel Gases 13 Name Date Period Questions About The Periodic Table 1. 2. 3. 4. 5. 6. 7. Which of the following is a NOBLE GAS? a. Oxygen b. Nitrogen c. Hydrogen d. Helium e. all of the above are noble gasses Sodium and Magnesium are both… a. alkali metals b. alkaline earth metals c. metals d. non-metals e. semi-metals The family (column) at the far right side of the periodic table are called… a. the metallic gasses b. the alkaline earth gasses c. the noble gasses d. the smelly gasses e. all of the above A row in the periodic table (across from left to right) is called a… a. period b. family c. group d. semi-family e. none of the above A semi-metal is the same thing as a ….. a. metal b. non-metal c. metalloid d. semi-non-metal e. both a and b above MALLEABLE means… a. breaks easily b. is made of non-metals c. a mixture of metals d. can be bent or pounded into shapes e. can be found in a MALL DUCTILE means … a. that a substance is brittle b. that a substance easily breaks c. that a substance bends d. that a substance can be pulled into wires e. all of the above 13 14 8. 9. 10. Cesium is …. a. an alkaline earth metal b. an alkali metal c. a non-metal d. a semi-metal e. both a and b above Barium is … a. an alkaline earth metal b. an alkali metal c. a non-metal d. a semi-metal e. both c and d above Two or more metals mixed together are called an… a. alloy b. metal soup c. non-metal d. metalloid e. semi-non-metalloid CIRCLE True or False on the problems below 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. T T T T T T T T T T F F F F F F F F F F An atomic number tells us the number of neutrons in an atom. Protons are located in the nucleus of an atom Uranium is a metal Most elements are non-metals Metals do not conduct electricity metalloids are found along the “zig-zag” on the periodic table metals tend to have very low melting points There are no metals that are a liquid at room temperature Calcium is a white powder non-metal found in bones. All metals conduct electricity. MATCH THE FOLLOWING ON THE LEFT WITH THE CHOICES ON THE RIGHT 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. Argon Silicon Uranium Antimony Oxygen Potassium Iron Chlorine Boron Mercury a. b. c. 14 metal non-metal semi-metal 05_CTR_ch06 7/9/04 3:27 PM Page 137 Name ___________________________ 6 15 Date ___________________ Class __________________ THE PERIODIC TABLE Practice Problems In your notebook, solve the following problems. SECTION 6.1 ORGANIZING THE ELEMENTS 1. Which element listed below should have chemical properties similar to fluorine (F)? a. Li b. Si c. Br d. Ne 2. Identify each element as a metal, metalloid, or nonmetal. a. fluorine b. germanium c. zinc d. phosphorus e. lithium © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 3. Which of the following is not a transition metal? a. magnesium b. titanium c. chromium d. mercury 4. Name two elements that have properties similar to those of the element potassium. 5. Elements in the periodic table can be divided into three broad classes based on their general characteristics. What are these classes and how do they differ? 15 ↑ Chapter 6 The Periodic Table 137 05_CTR_ch06 7/9/04 3:27 PM Page 138 Name ___________________________ 16 Date ___________________ Class __________________ SECTION 6.2 CLASSIFYING THE ELEMENTS 1. Use the periodic table to write the electron configuration for silicon. Explain your thinking. 2. Use the periodic table to write the electron configuration for iodine. Explain your thinking. 3. Which group of elements is characterized by an s2p3 configuration? 4. Name the element that matches the following description. a. one that has 5 electrons in the third energy level b. one with an electron configuration that ends in 4s24p5 c. the Group 6A element in period 4 5. Identify the elements that have electron configurations that end as follows. a. 2s22p4 b. 4s2 c. 3d104s2 6. What is the common characteristic of the electron configurations of the elements Ne and Ar? In which group would you find them? 7. Why would you expect lithium (Li) and sulfur (S) to have different chemical and physical properties? 8. What characterizes the electron configurations of transition metals such as silver (Ag) and iron (Fe)? SECTION 6.3 PERIODIC TRENDS © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium. 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl ion to be larger or smaller than an Mg2 ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S2) is larger than the chloride ion (Cl). 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electronegativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form? Explain. 10. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity. 138 Core Teaching Resources 16 ↑ 18 Image 1 ___________________________ First Name, Last ________ Period SCORE: ___/10 pt 6 Periodicity Formative Assessment 3 Write True or False in the blank. 1. Image 1, shows Electronegativity an increase from the left to the right. This is due to more electrons in the nucleus which can pull on electrons harder. 2. Image 1, shows Ionic Sizes and Shielding to increase from top to bottom of the Periodic Table. This is because there are more energy levels. 3. Below in Graph 1, one can observe that atomic radii decreases as we move from LEFT to RIGHT with in a period or row because of greater proton pull. 4. In Graph 1, one can observe that atomic radii increase as we move down a column Or family because there are more energy levels. 5. In Graph 2, one can observe that ionization energy increases as we move from Left to right with in a period or row because of more protons pulling electrons. 6. In Graph 2, one can observe that ionization energy decreases as we move down a Column or family because of a great atomic radius. 7. Image 1 Which metal is smallest because of the least amount of energy levels & more relative protons or nuclear charge? A. Li B. Be C. Na D. Ca 8. Which metal has the lowest ionization energy because of relatively few protons for its’ energy level and yet the most energy levels? A. Rb B. Cs C. Sr D. Ba 9. Which nonmetal has the highest electro-negativity because of the smallest atomic radius more protons or nuclear charge? A. O B. N C. S D. P 10. Which nonmetal has the smallest radii because of the most protons (nuclear charge)? A. O B. N C. S D. P Graph 1 Graph 2 18 20 ___________________________ First Name, Last ________ Period SCORE: ___/10 pts s1 d1 p1 Periodic Table Formative Assessment 1 1. Which does not fit in because 2 elements do not behave similarly? a. groups b. family c. period d. column 2. Which element is in group 2 and period 4? a. Be b. Ca c. Ti d. none correct Which does not fit in? a. family b. period c. row d. energy level Which is an alkali earth metal? a. K b. Mg c. Sc d. Ge e. Br Which is a transition metal? a. K b. Mg c. Sc d. Ge e. Br Which is a metalloid? a. K b. Mg c. Sc d. Ge e. Br Which in a nonmetal? a. K b. Mg c. Sc d. Ge e. Br 3. 4. 5. 6. 7. 8. 9. 10. Where are the metals compared to the stair steps? a. right b. left c. on the steps Where are the inner transition metals? a. between the metals & nonmetals b. between alkali earth & transitions Which electron configuration is a noble gas? a. 1s22s22p6 3s23p6 b. 1s22s22p6 3s23p5 c. 1s2 2s22p6 d. 1s1 e. more than 1 correct 20 b. d. d. none correct right of the stair step none correct