Trends in the Periodic Table Homework Unit 7 - Topic 4 (Regents)
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1 Trends in the Periodic Table Homework Unit 7 - Topic 4 (Regents) What are the trends in the Periodic Table? Below is a portion of the periodic table. In the answer spaces provided, fill in [1] atomic number, [2] atomic radius, [3] number of shells, and [4] number of valence electrons. Then answer the questions that follow. Symbol [1] Atomic Number [2] Atomic Radius [3] Number of Shells [4] Valence Electrons 1. What scientist created the first periodic table, which arranged the elements accruing to their atomic masses? 2. What scientist developed the periodic table as we know it today, with elements arranged according to their atomic numbers? 3. As you go from left to right across a row of the Periodic Table: 1. What happens to the atomic number and # of protons? 2. As a result, what happens to the pull on the electrons? 3. Therefore, what happens to the atomic radius? 4. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic?
2 Name: 4. As you go from top to bottom down column of the Periodic Table: 1. What happens to the number of shells? 2. As a result, what happens to the atomic radius? 3. Therefore, what happens to the pull on the electrons? 4. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic? 5. Base on the analysis above, where do the metals tend to be located on the Periodic Table? 6. Based on the analysis above, where do the non-metals tend to be located on the Periodic Table? 7. What do the elements at the extreme right of the Periodic Table have in common? What affect does this have on the chemical properties? ATOMIC RADIUS as you go down a group and as you go from left to right across a period.
3 Name: Reactivity 1. When METALS react, they (gain / lose) electrons. 2. Look at Group 1 on the Periodic Table, the Alkali Metals. a) What is similar about their atomic structure? b) Why does Hydrogen fit into this group? c) Why does Hydrogen NOT fit into this group? d) Which metal is the most reactive of the group (loses electrons most easily)? Why? e) Group 2, the Alkaline Earth Metals, follow similar trends. Which element is more reactive, barium or magnesium? 3. When NON-METALS react, they (gain / lose) electrons. 4. Look at Group 17 on the Periodic Table, the Halogens. a) what is similar about their atomic structure? b) Which non-metal is the most reactive of the group (gains electrons most easily)? Why? c) State the relationship between reactivity and size for non-metals. 5. Group 18, the NOBLE GASES, are not reactive at all. Why? For METALS, REACTIVITY as you down a group. For NON-METALS, REACTIVITY as you down a group.
4 Electronegativity Use the App EMD-PTE, your Reference Tables, or your textbook to answer the following questions about electronegativity. man. 1. Define electronegativity: 2. Why would an atom want to gain electrons? 3. When looking at the elements in the same period, from which group does the element come from that has the highest electronegativity value in every case? The lowest? 4. Which has higher electronegativity, metals or non-metals? Why? 5. What is the electronegativity trend from top to bottom in the same group? 6. What is the electronegativity trend from left to right across a period? 7. Based on the definition of electronegativity, why don t the nobel gases have any electronegativity values? 8. Which element has the highest electronegativity of all? Why? ELECTRONEGATIVITY as you go down a group and as you go from left to right across a period.
5 Ionization Energy Use the App EMD-PTE, your Reference Tables, or your textbook to answer the following questions about ionization energy. 1. Define ionization energy: 2. Why is it easier to remove an electron from Na than it is from Cl? 3. Why is ionization energy related to, but not the same as, electronegativity? 4. Describe the trend in ionization energy as you go left to right across a period. 5. Describe the trend in ionization energy as you go down a group. 6. Why do noble gases have the highest ionization energy values? 7. Why do metals have low ionization energy values? 8. Why do nonmetals have high ionization energy values? IONIZATION ENERGY as you go down a group and as you go from left to right across a period.
6 Do you get it?
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