1. Bellwork (Get out Study Guide..and..) 1)Tear out sheet of paper from notebook. 2)Come up with three possible test questions. Write the answer on the back. 3)Trade with neighbor and see if they can answer them (without you telling them the answer

2. Study Guide: first page Atomic Mass: mass of a specific isotope of an element Atomic Number: the number of protons in an element Mass Number: Protons + Neutrons Isotopes: forms of elements that have different number of neutrons Ions: charged atoms Valence electrons: electrons in the outermost shell

3. Study Guide: First Page ChargeLocationMass Proto n Positive Nucleus 1 atomic mass unit Neutr on Neutral Nucleus 1 atomic mass unit Electr on Negative Cloud 0.00054 amu (small!)

4. Study Guide: First Page Which particle defines the element? Number of protons What charge does the nucleus of an atom normally have? Positive What does it mean for an atom to be neutral? (Explain using the words proton, neutron, electron) No charge. Number of protons= electrons. Neutrons are not charged. How are the electrons arranged in an atom? In shells or orbitals based on energy level.

5. Knowing that every periodic table is different, how do I tell which one thing is the atomic number? It is the whole number (no decimals). Knowing that every periodic table is different, how do I tell which one thing is the atomic mass? It is the decimal number. It is usually larger than the atomic number.

6. If you know an elements Atomic number, what else do you know about the element? (Assume the element is neutral) Number of protons. If the element is neutral, also the number of electrons. How do you get the mass number from the periodic table? Round the average atomic mass. Most of the time, though, you should add protons and neutrons.

7. Study Guide: First Page Electrons do not travel in an orbit. Explain this statement, using the words orbit, orbital, electron cloud, and energy level. Electrons are found approximately in the electron cloud and travel very quickly in orbits. They are found at different energy levels. Electrons closer to the nucleus have less energy because they are strongly attracted to the nucleus.

8. Isotopes and Ions What do the numbers after the name of an element represent? Ex. Magnesium – 26 Mass number. Ex) 26 is the number of protons plus neutrons In the example to the right, why don’t I have to include the number of protons before Magnesium? Ex. Magnesium – 26 The number of protons is always the same for a specific element (it is the atomic number)

9. Isotopes and Ions Assume you have these 2 elements: 55 25 Mn and 56 25 Mn How are these elements different from each other? Different mass numbers What do we call these elements? Isotopes How would you name each element? Manganese-55 and Manganese-56

10. Isotopes and Ions Element/Isotope Information Write the Isotope Notation Name the Element/Isotope p = 19, e= 19, n = 20 39 19 K Potassium-39 p=75, e=75, n = 111 186 75 Re Rhenium- 186 p = 18, e = 18, n = 22 40 18 Ar Argon-40

11. What is a cation? Positively charged atom (has lost electrons) Does a cation have a positive or negative charge? Positive What is an anion? Negatively charged atom (has gained electrons) Does an anion have a positive or negative charge? Negative