Ion Practice Set. 2. What does the number next to the ions signify? Complete the following table, using the periodic table in the back of your book.

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1 Reminders: 1. In a neutral atom the number of protons equals the number of electrons. 2. An atom can NEVER gain or lose protons 3. The number of protons equals the atomic number NAME: Ion Practice Set 1. What is an ion? 2. What does the number next to the ions signify? Complete the following table, using the periodic table in the back of your book. ex ELEMENT NAME ION SYMBOL NUMBER OF PROTONS NUMBER OF ELECTRONS NUMBER OF ELECTRONS LOST OR GAINED Fluorine F gained one gained two potassium lost one Ca +2 Sr +2 H + aluminum H gained two 12 lost two lithium lost one Rb

2 NAME: Isotopes Practice Set 1. What is an isotope? 2. What does the number next to isotopes signify? 3. How can you tell isotopes apart? For each of the following isotopes, write the number of protons, neutrons, and electrons. Chromium-58 Chromium-63 Carbon-12 Carbon-16 Nitrogen-15 Nitrogen-20 Sulfur-23 Sulfur-25 Fill in the isotope names and any missing information, including isotope numbers from the chart. Use your periodic table and the information provided. Iodine- Iodine- Iron- Iron

3 1. Atom #1 has 5 protons and 5 neutrons. Draw its nucleus in the first circle below. 2. Atom #2 has 5 protons and 4 neutrons. Draw its nucleus in the second circle below. Atom 1 Atom 2 : : : : Atomic Mass: Atomic Mass: 3. What is the same for both of your atoms? 4. What is different? 5. These two atoms are the same element. What is the proof of that? 6. What is the average atomic mass of your element? (show your work) 7. Study the following five atoms and find the atomic mass of each. Atom 1 Atom 2 Atom 3 Atom 4 Atom 5 Atomic Atomic Atomic Atomic Atomic Mass Mass Mass Mass Mass 8. Are all of the above the same element? Explain. 9. What is the average atomic mass for the above atoms (to the nearest thousandth)? 10. Why is this number different than the average atomic mass that you calculated in question 6? 11. Round the number you calculated in question 9 to the nearest whole number.

4 12. How many of the five atoms from question 7 have the atomic mass that you calculated in question 10? 13. How many had a different atomic mass? 14. The periodic table shows the average atomic mass of that element and takes into account how many atoms of each isotope are found in nature. If you round it to the nearest whole number, you can find the atomic mass of most common isotope of that element. For instance, the most common isotope of Helium is Helium 4. What is the most common isotope of hydrogen? What is the most common isotope of oxygen? Isotopes can also be written in element notation: The large "X" represents where you will find the atom's symbol. The mass number, which is given the symbol "A", is located in the upper left-hand corner. The atomic number, given the symbol "Z", is found in the lower left corner. For example, the element notation for the most common isotope of carbon is: 15. Write the most common isotope of hydrogen using element notation: 16. Write the element notation for Bromine-82. How many protons does it have? How many neutrons does it have? 17. Fill out the following chart: (assume all are neutral atoms) Isotope Name Calcium-40 Isotope Symbol Atomic Mass Protons Neutrons Electrons Au

5 Atom, Isotope or Ion? The table below contains information about several elements. The elements may be a neutral atom, an isotope of an atom, or an ion. Fill in the missing information from the chart. Element Symbol Atomic Mass Protons Neutrons Electrons Ion, Isotope or Atom? Aluminum Al Bromine Uranium U Helium He 2 4 Helium He Lithium Tungsten W Xenon Magnesium Mg 24 Carbon 6 6 atom +2 ion atom Carbon C Nitrogen 7 14

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