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1 IPS Unit 2 Worksheet Packet STUDYING THE ATOM Match the following picture or sentence with the scientist who discovered it: D: Dalton R: Rutherford T: Thomson B: Bohr 1.________________ 2.______________ 3.______________ 4.________________ ____ 5. Atoms are small, hard particles. ____ 6. Atoms of the same element are exactly alike. ____ 7. In an atom, electrons move in definite orbits around the nucleus, much like planets circle the sun. ____ 8. An atom is the smallest piece of matter. ____ 9. An atom is mostly empty space with a dense, positively charged nucleus in the center. ____ 10. Atoms are indivisible. ____ 11. An atom has a small, positively charged nucleus surrounded by a large region in which scientists can predict where an electron is likely to be found. ____ 12. An atom is made of positively charged, pudding like material through which negatively charged particles are scattered. ____ 13. In an atom, electrons are located in energy levels that are a certain distance from the nucleus. 2 THE ATOMIC NUCLEUS After much observation and questioning, Democritus concluded that matter could not be divided into smaller and smaller pieces forever. Eventually the smallest possible piece would be obtained. All elements are composed of atoms. Atoms are indivisible and indestructible particles. Atoms of the same element are exactly alike. Atoms of different elements are different. Compounds are formed by the joining of atoms of two or more elements. According to Thomson’s atomic model, the atom was made of a puddinglike positively charged material throughout which negatively charged electrons were scattered, like plums in a pudding. Rutherford reasoned that all of an atom’s positively charged particles were contained in the nucleus. The negatively charged electrons were scattered outside the nucleus around the atom’s edge. According to Bohr’s atomic model, electrons move in definite orbits around the nucleus, much like planets circle the sun. These orbits, or energy levels, are located at certain distances from the nucleus. According to the modern atomic model, an atom has a small positively charged nucleus surrounded by a large region in which there are enough electrons to make the atom neutral. Write five facts about the term nucleus, using the following words as clues. 1. Size 2. Location 3. Rutherford 4. Charge 5. Density 3 THE STRUCTURE OF AN ATOM Using your periodic table, complete the following table. Substance Symbol Helium Bromine Atomic Number Mass Number 2 4 Mg 12 Zn 30 Br Number of Protons 65 80 35 13 U Na Ca Silver Ag 14 146 11 92 12 Kr Calcium Number of Electrons 12 Aluminum Sodium Number of Neutrons 48 40 20 47 61 36 4 Identify each element and choose whether the pair are isotopes to each other or different elements. Element Name Isotope? 1. Element D has 6 protons and 7 neutrons ____________ ____________ Element F has 7 prortons and 7 neutrons 2. Element J has 27 protons and 32 neutrons ____________ ____________ ____________ Element L has 27 prortons and 33 neutrons ____________ 3. Element X has 17 protons and 18 neutrons ____________ ____________ Element F has 18 prortons and 17 neutrons ____________ 4. Element Q has 56 protons and 81 neutrons ____________ ____________ Element R has 56 prortons and 82 neutrons ____________ 5. Element T has an atomic number of 20 and an atomic mass of 40. ____________ ____________ Element Z has an atomic number of 20 and an atomic mass of 41. ____________ 6. Element W has 8 protons and 8 neutrons ____________ Element V has 7 prortons and 8 neutrons ____________ ____________ 7. Element P has an atomic number of 92 and an atomic mass of 238. ____________ ____________ Element S has 92 prortons and 143 neutrons ____________ Complete the following table. Particle Location Proton Electron Neutron Mass (amu) Charge 5 Draw a model of the following atoms. Li C B He Si H N F 6 THE PERIODIC TABLE Use different colored pencils to show each of the following items on the periodic table. Make a key to indicate which color you are using for each item group period metals nonmetals metalloids The diagrams below show three squares from three different periodic tablse. On each diagram, label the following items: element name mass number chemical symbol 190 51 Sb Antimony 122 Os Osmium 76 atomic number 82 207 Lead Pb 7 THE PERIODIC TABLE Examine part of the periodic table shown below. Use this periodic table to answer the following questions relating elements D, F, J, K, and R. K J F D R 1. Which pair of elements has the same number of valence electrons? 2. Which pair of elements is in the same period? 3. Which pair of elements is in the same family? 4. Which element has the smallest atomic number? 5. Which elements would be classified as metals? 6. If the atomic number of Element D is 20, then what is the atomic number of element R? 8 REPRESENTATIVE GROUPS On the periodic table below, label each of the following: actinoid series alkali metals alkaline earth metals boron family carbon family halogen family lantanoid series nitrogen family noble gases oxygen family rare-earth elements transition metals _______________________ IPS Unit 3 Worksheet Packet Page 9 Using the periodic table, identify the elements described in the statements below. 1. This element is in the same family as lead, and it has fewer protons than sodium. 2. This element has an atomic number that is one greater than platinum. 3. This element has the most protons of any element in group 15. 4. This element has more than 50 but less than 75 protons, and it is in group 17. 5. This group 2 element has fewer protons than bromine, but more protons than sulfur. 6. This element has the lowest atomic number of any group 16 element. 7. This element has an atomic number that is double the atomic number of silicon. 8. This element has more valence electrons, than oxygen, fewer valence electrons than neon, more protons than sodium, but fewer protons than argon. 9. This element has an atomic number lower than that of aluminum and one less valence electron than the group 16 elements. 10. This element is in group 1 and has a higher atomic number than chlorine, but a lower atomic number than bromine. IPS Unit 3 Worksheet Packet Page 10 Draw the electron dot diagram for the following atoms a. Hydrogen f. Carbon b. Helium g. Nitrogen c. Lithium h. Oxygen d. Beryllium i. Fluorine e. Boron j. Neon For the atoms above, predict whether they will gain electrons, lose electrons, or neither gain nor lose electrons in a chemical reaction. Write “G” for gain, “L” for lose, and “N” for neither. a. ___ f. ___ b. ___ g. ___ c. ___ h. ___ d. ___ i. ___ e. ___ j. ___ IPS Unit 3 Worksheet Packet Page 11 Draw both the electron dot diagrams for the following atoms and then draw the most likely ion that these atoms will form. Make sure to show the charge for each ion and the electrons if necessary. a. Na e. P b. Mg f. S c. Al g. Cl d. Si h. Ar For the ions above, which are considered cations, and which are considered anions? a. _____________ e. _____________ b. _____________ f. _____________ c. _____________ g. _____________ d. _____________ h. _____________ Name the ions above. a. _____________ e. _____________ b. _____________ f. _____________ c. _____________ g. _____________ d. _____________ h. _____________ IPS Unit 3 Worksheet Packet Page 12 Predict the ionic compound resulting between the following elements. Make sure to take into account the charges on each ion and balance the charges with the correct number of each ion. a. Na and Cl f. Li and N b. Na and O g. K and O c. Mg and S h. Ca and F d. Ca and Br i. Ba and N e. Al and F j. Sr and P Name the above compounds: a. ____________________ b. ____________________ c. ____________________ g. ____________________ h. ____________________ i. ____________________ d. ____________________ j. ____________________ e. ____________________ f. ____________________