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Chemistry Term 1 Periodic Exam 2 Study Guide Give 5 examples of electromagnetic radiation: - - - - What is frequency? What is wavelength? How are frequency and wavelength related to each other? What is a quantum? What is the relationship between the frequency and the energy of electromagnetic radiation? What is the relationship between the wavelength and the energy of electromagnetic radiation? What is an electron’s ground state? What is an electron’s excited state? How/why do electrons move back and forth between ground and excited states? What happens when an electron moves from an excited state to a ground state? Why is the emission-line spectrum of hydrogen (or any element) a series of discrete lines instead of a continuous spectrum? How did Bohr’s model of the atom improve upon Rutherford’s and explain the emission-line spectrum of hydrogen? What was a problem with Bohr’s model of the atom? What is Heisenberg’s Uncertainty Principle? How does the Quantum Model of the atom describe electron orbitals? Whose equations accurately predicted emission-line spectra for all elements and laid the foundation for the Quantum Model? What does the Principle quantum number tell you? How many electrons can exist in the first main energy level? How many electrons can exist in the second main energy level? How many electrons can exist in the third main energy level? How many sublevels are there in the first main energy level? What are they? How many sublevels are there in the second main energy level? What are they? How many sublevels are there in the third main energy level? What are they? How many sublevels are there in the fourth main energy level? What are they? How many orbitals can exist in an s sublevel? How many electrons? How many orbitals can exist in a p sublevel? How many electrons? How many orbitals can exist in a d sublevel? How many electrons? How many orbitals can exist in an f sublevel? How many electrons? What is the Aufbau principle? Give an example: What is the Pauli exclusion principle? Give an example: What is Hund’s rule? Give an example: What two features of elements did Mendeleev use to organize his Table of elements? - - What two features of elements are used to organize the modern Periodic Table? - - What are two characteristics of nonmetals? Where are metalloids found on the Periodic Table? Give three examples. Which Group number includes the halogens? Which Group number includes the Noble gases? Which Group number includes the alkaline earth metals? Which Group number includes the alkali metals? What are the s and p sublevel e- configurations of the Noble gases? What Group numbers include the Main Group elements? Which blocks are these? Which Group numbers include the transition metals? What block is this? Where are the inner transition metals? What block is this? In which Period is the 3d sublevel filled? In which Period is the 5f sublevel filled? In which Period is the 4s sublevel filled? In which Period is the 2p sublevel filled? What is the highest occupied sublevel in a bromine atom? How many electrons are in that sublevel? What is the highest occupied main energy level for a strontium atom? How many electrons are in that main energy level? What is nuclear attraction? Give two examples of how this affects periodic trends: What is shielding? Give two examples of how this affects periodic trends: How does atomic radius change as you go down a Group? Why? How does atomic radius change as you go across a Period? Why? What is ionization energy? How does ionization energy change as you go down a Group? Why? How does ionization energy change as you go across a Period? Why? What is electronegativity? How does electronegativity change as you go down a Group? Why? How does electronegativity change as you go across a Period? Why? What is an ion? What is a cation? Is a cation larger or smaller than the atom from which it formed? What is an anion? Is an anion larger or smaller than the atom from which it formed? What types of elements form cations? What types of elements form anions? What are valence electrons? How many valence electrons in a carbon atom? Potassium? Sodium? Bromine? Describe a chemical bond: Why would two atoms form a bond? What is a covalent bond? What types of atoms form covalent bonds? Give two examples. What is an ionic bond? What types of elements form ionic bonds? Give an example. What is a nonpolar covalent bond? What is a polar covalent bond? Why are some covalent bonds nonpolar and some polar? What is a molecule? What types of atoms form molecules? What is a molecular compound? Give three examples. What are the seven elements that exist as diatomic molecules? What are the three forces at work when two atoms are bonding?- - What is bond energy? How are the energy released when a bond forms and the energy needed to break a bond related? Show the electron dot structures for carbon, potassium, boron and iodine: Predict whether the following pairs would be ionic, nonpolar covalent or polar covalent: S and N Br and H Rb and I Li and Cl S and I C and H Ni and Cl Cu and O H and N 1. Draw the Lewis structures 2. Determine if the molecule is polar carbon dioxide water NO2- CH2Cl2 CH2O C2H4 CN- HCN Atom/ Ion FULL Electron Configuration (Shaded = noble gas configuration) Ni p+ n0 28 30 e- Mass # 1+ 1s2 2s2 2p6 24 50 69 2+ 49 197Au 0 Se 2- 79 Al Atom/ Ion Charge 14 Electron Configuration (write SMALL and NEATLY) p + Rb n 0 0 e - Mass # Charge 48 15 1s22s22p63s23p6 How many atoms in 40.00 g of nickel? How many grams in 3.01 x 1021 atoms of lead? What is the molar mass of Al2O3? -3 16 40 Fe 16 32 40 91 56 -2 How many moles in 45.6g of oxygen? How many moles in 3.01 x 10 27 atoms of radium? How many grams is 10.0 moles of water? How many atoms in 5.5 moles of methane CH4? Six moles of an element has a mass of 823.8 grams. What is the element?
