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Periodic Table Book Assignment (Chapter 6) Name ____________________________ 1. List 3 properties of metals. 2. List 3 properties of nonmetals. 3. What are metalloids? Give 2 examples. 4. What are macronutrients? Give 3 examples. 5. What are trace elements? Give 3 examples. 6. Dimitri Mendeleev arranged the periodic table in order of increasing ___________. 7. Currently, the periodic table is arranged in order of increasing _____________. 8. What does the word “periodic” used in the periodic table of elements refer to? 9. Do elements in one family (vertical columns) or elements in one series (horizontal rows) have the most similar characteristics in the periodic table? Explain. 10. Why does atomic radius decrease going across a row of the periodic table? 11. Why does atomic radius increase going down a column of the periodic table? 12. List 2 properties of the alkali metals. 13. List 2 properties of the alkali earth metals. 14. List 2 properties transition metals. 15. List 2 properties of the halogens. 16. Why are the noble gases so stable? 17. True or False: Elements in the same family have the same number of valence electrons. Explain. 18. List 2 electrolytes that are essential to the central nervous systems in humans. Atomic Structure Book Assignment (Chapter 5 – section 5.1 on pages 132-143) 1. What Greek philosopher proposed the idea of the atom? Did he support this idea with experimental evidence? 2. Briefly describe (in your own words) the 4 pieces of Dalton’s atomic theory? 3. In what ways does our current model of the atom differ from Dalton’s model? 4. In 1897, J. J. Thomson discovered __________________ ____________________ charged subatomic particles. which are 5. What piece of equipment helped Thomson make this discovery? 6. In 1910, Ernest Rutherford performed his gold foil experiment. Based on this experiment, summarize Rutherford conclusions about: a. the composition of an atom’s nucleus b. the size of a nucleus compared to the rest of an atom 7. Draw a picture of an atom. Identify the protons, neutrons, and electrons. 8. Are there subatomic particles that are even smaller than protons, neutrons, and electrons? 9. Define atomic number. 10. What is atomic number of lithium? 11. Define isotope. 12. What are 2 isotopes of lithium that are naturally occurring (found in nature)? 13. Define mass number. 14. What is the mass number of lithium-7? 15. What is meant by electron cloud? 16. Opposite charges ___________________; like charges _________________________. Periodic Table Dimitri Mendeleev1. Listed the elements according to their atomic mass. 2. Noticed that similar chemical properties appeared at regular intervals. 3. Published first modern periodic table. Periodic Table of Elements. Henry Moseley- Rearranged PT by atomic number Periods: Horizontal rows on the periodic table. Represent how many energy levels each atom should have. There are 7 periods. Groups/Families: Vertical columns are called this because each group has similar properties because they have the same number of electrons in the outer energy level. There are 18 groups. Locations you should know Metals: Solid at room temp., shiny, good conductors of heat and electricity, malleable (bendable), ductile (made into wires), most can be corroded. Nonmetals: Most are gases, some brittle and powdery solids, poor conductors of heat and electricity, dull in appearance (not shiny). Metalloids: Have properties of both metals and nonmetals. Next to zigzag line on the periodic table. Metalloids often make up the semiconductors found in electronic devices. Metalloids are B, Si, Ge, As, Sb, Te, At. Alkali Metals: Group 1, like metals but HIGHLY REACTIVE. Soft, shiny, silver-white, good conductors. Have one e- in their outer energy level which they like to give up. Never found uncombined in nature. Reactivity increases down a group. Alkali Earth Metals: Group 2, similar characteristics as alkali metals but not quite as reactive. They have 2 electrons in the outer level which they like to give up. Never found uncombined in nature. Transition Metals: Much less reactive than groups 1 and 2. They like to give up electrons – but the number of electrons they give up can vary. Same properties as metals. Halogens: Group 17 or 7A, need one more electron to obtain a stable outer energy level, reactivity decreases as you move down period, gain electron(s) from a metal and form a salt compound. Most reactive nonmetals, mostly gases. Noble Gases: Group 18 or 8A, don’t usually react with other elements because they have a full outer energy level. Also called “inert gases” because they are unreactive. Rare Earth Elements: 1. Lanthanoid Series: Soft malleable metals with high luster and conductivity. 2. Actinoid Series: Radioactive elements made in the laboratory (synthetic). Atomic Structure Proton (p+): + charge, in nucleus, mass=1 amu Neutron (n˚): Neutral charge, in nucleus, mass=1 amu Electron (e-): - charge, floats outside nucleus in energy levels, mass close to 0 amu (1/2000 the size of a proton) Atoms are neutral (# of protons = # of electrons) Atomic # = # of protons, identifies the element Isotope: Atoms of the same element (same # of protons and same # of electrons) that have different numbers of neutrons. (Therefore, mass is different.) Ex. Uranium-235 and Uranium-238, C-12 and C-14 Isotopes have identical chemical properties, but some physical properties will be different. Atomic Mass: Found on Periodic Table Average mass of all the isotopes of that element as they occur in nature. Ex: Carbon’s atomic mass is 12.011. Are there more atoms of carbon-12 or carbon-14? Mass Number = # of protons + # of neutrons OR Rounded atomic mass (on periodic table) Ex: Uranium-235 Atomic #=92, must be 143 neutrons Uranium-238 Atomic #=92, must be 146 neutrons Name Hour THE STRUCTURE OF THE ATOM 1. Complete the following chart: Subatomic Particle proton neutron electron Charge Mass (AMU) Location 2. Important items to remember: Atomic Number = # of _____________________ Mass Number = # of ________________ + _________________ Atoms are: a) Positive b) Negative c) Neutral # of ________________ = # of ________________ in a neutral atom 3. Fill in the chart below: ELEMENT Symbol Atomic Number # of Protons # of Electrons # of Neutrons SODIUM MAGNESIUM Mass # 23 12 NITROGEN 14 ZINC 65 GOLD LEAD 118 207 4. Explain what an isotope is and give an example: Explanation: Example: 5. Fill in the chart below: Element Symbol Atomic # # of p+ # of e- # of n° Carbon C 6 6 6 6 Fluorine Mass Number 12 10 K 39 2 2 P 31 17 18 Copper 63 Copper 65 Sn 68 Sn 69 14 Al Iron 28 14 56 6. There are 2 naturally occurring isotopes of copper. They are copper-63 and copper-65. Which one is found in greater abundance? How do you know this? (Hint: look at copper on your periodic table.) Periodic Table Notes – Reactivity Name ___________________ What combinations of elements can / cannot chemically react? 1. Metals with Nonmetals (can react) Form ionic compounds Metals lose electrons Nonmetals gain electrons Examples: 2. Nonmetals with Nonmetals (can react) Form covalent compounds Each nonmetal shares electrons Examples: 3. Metals with Metals (cannot react – but do form alloys which are mixtures) 4. Special Case – Hydrogen (can react) Hydrogen is versatile Donates 1 electron Examples: Accepts 1 electron Examples: Shares 1 electron Examples: 5. Noble Gases (cannot react – some rare exceptions) Reactivity Worksheet Name ______________________ 1. Could the following elements react based on their position in the periodic table? If so, would they form ionic or covalent compounds? A) calcium and bromine H) hydrogen and strontium B) nitrogen and iodine I) hydrogen and helium C) neon and lithium J) silicon and hydrogen D) cesium and barium K) phosphorus and hydrogen E) xenon and fluorine L) hydrogen and aluminum F) copper and zinc M) oxygen and potassium G) helium and hydrogen N) fluorine and carbon 2. Could the following elements react based on their position in the periodic table? If so, would they form ionic or covalent compounds? A. Nitrogen and oxygen I. cesium and fluorine B. Carbon and hydrogen J. chlorine and fluorine C. Carbon and argon K. oxygen and krypton D. Sodium and chlorine L. strontium and gold E. Sodium and magnesium M. neon and helium F. Tungsten and calcium N. bromine and magnesium G. Copper and chlorine O. hydrogen and chlorine H. Cesium and radium P. oxygen and carbon Periodic Trends 1. Name ______________________ Ionization Energy or IE (amount of energy needed to remove an electron from an atom) Across Table – IE increases because … Down Table – IE decreases because… 2. Atomic Size (radius) Across Table – Size decreases because… Down Table – Size increases because… 3. Melting Points (MP) and Boiling Points (BP) Metals usually higher than nonmetals For metals: Down Table – MP/BP decrease because … For nonmetals: Down Table – MP/BP increase because … 4. Reactivity Sides of table are more reactive (except for the noble gases) For metals: Down Table – Reactivity increases because … For nonmetals: Down Table – Reactivity decreases because … Unit #3 – (Trends, Tables, and More) Name ____________________ 1. Which of the elements in each lettered set has the lowest ionization energy? Which has the highest ionization energy? 2. 3. 4. A) lithium potassium cesium B) lithium boron fluorine C) barium calcium arsenic D) argon magnesium potassium Which of the elements in each lettered set is the smallest? Which is the largest? A) beryllium carbon fluorine B) lithium sodium potassium C) cesium fluorine neon D) calcium rubidium selenium Which element in each lettered set has the lowest melting point? Which has the highest melting point? A) lithium potassium cesium B) fluorine chlorine bromine C) strontium calcium bromine D) fluorine chlorine iron Which element in each lettered set is most reactive? Which is least reactive? A) lithium potassium cesium B) fluorine chlorine bromine C) copper zinc potassium D) carbon fluorine neon Atomic Models: Power Point Worksheet Name ____________________ 1. When did Democritus first propose the idea of the “atom”? 2. Give the 4 parts of Dalton’s atomic theory in your own words. 3. When was the electron discovered and by whom? 4. What is the approximate mass of the electron? 5. What device was used in the discovery of the electron? 6. Explain the model of the atom suggested by J.J. Thomson. (Include a diagram.) 7. Rutherford performed what experiment that helped define an atom? 8. What atomic structure did the above experiment help find? 9. Draw a diagram of the Rutherford experiment. Include labels. 10. Where do electrons go in the Bohr model of the atom? 11. What is the name of the Bohr atom? 12. How is the modern atom different from Bohr’s atom? 13. Who discovered the neutron? 14. What are quarks? What are their charges? History of the Atom – Summary Activity Directions - For each of the following scientists a. Describe their model of the atom b. Draw their representation of a lithium atom c. List the evidence they used to support their model A. John Dalton B. J. J. Thomson C. Ernest Rutherford D. Neils Bohr E. James Chadwick