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Name Period Date Chemistry 1st Quarter Review Dimensional Analysis Do the following showing all work and putting into correct significant figures. 1. 0.75 kg is _________ grams 2. 1500 millimeters to __________ km 3. 65 kg to _______________ pounds 4. How many nanometers in a micrometer? Density Problems 1. Calculate the density of sulfuric acid if 35.4 mL of the acid weighs 65.14 g. 2. Find the mass of 250.0 mL of benzene. The density of benzene is 0.8765 g/mL. 3. What is the density of water? What is its slope on a graph? (Be able to use graphs as we did in class.) Classifying matter Classify the following as either elements, compounds, homogeneous mixtures (solutions) or heterogeneous mixtures: 1. copper (II) sulfate _________________ 2. Kool Aid _________________ 3. wood ________________ 4. air ________________ 5. Br2________________ 6. CO2________________ 7. Be able to explain the similarities and differences of Compounds and Heterogeneous Mixtures. Vocabulary Proton Neutron Electron Average atomic mass Atomic Number Mass number Isotope Periodic Table Groups Periods Noble Gases Electron Configuration Energy levels Valence Electrons Orbitals (S,P,D,F) Lewis structure Bohr diagram Quantum mechanical model Wavelength Frequency Photon Ground state Excited State Isotope Notation Homogeneous Liquid Heterogeneous Liquid Element Compound Atom Molecule Physical Change Chemical Change Density People (Who were they and what did they do?) Rutherford John Dalton J.J. Thomson Average atomic mass calculation Element X has two natural isotopes. The isotope with a mass number of 6 has a relative abundance of 7.5%. The isotope with a mass number of 7 has a relative abundance of 92.5%. Determine the average molar mass for the element from these figures. What is the true identity and atomic number of element X? Explain why the atomic mass of most elements is not a whole number. Lewis Dot Draw Lewis dot for the following: Li B S Cl Ca Ar Electron Configuration Write the complete electron configurations for the following, including the orbital diagrams: 1. Lithium ________________________________________ 2. Chlorine ________________________________________ 3.Calcium ______________________________________________ 4. Rubidium __________________________________________________ Abbreviated version: Write the complete electron configurations for the following, including the orbital diagrams 1. Sodium 2. Argon 3. Titanium 4. Lead Write the Isotope notation for 1. U-234 2. Carbon 13 3. A copper atom with 34 neutrons Labs that you need to be able to explain what was happening. 1. Mass and Change Mini Lab 2. Flame Lab 3. Density Lab 4. Candium Lab