Chem S1 Final Review PDF

Unit 1 1. **Subatomic particle** **Mass** **Charge** **Location** ------------------------ --------------- ------------------ ------------------------- **Protons** Small / Large \+ / - / neutral Nucleus / energy levels **Electrons** Small / La...

Unit 1 1. **Subatomic particle** **Mass** **Charge** **Location** ------------------------ --------------- ------------------ ------------------------- **Protons** Small / Large \+ / - / neutral Nucleus / energy levels **Electrons** Small / Large \+ / - / neutral Nucleus / energy levels **Neutrons** Small / Large \+ / - / neutral Nucleus / energy levels 2. a. b. c. 3. 4. Symbol Atomic number Mass number charge Protons Neutrons Electrons --------------- --------------- ------------- -------- --------- ---------- ----------- ^25^~12~Mg 0 4 5 ^15^~8~O^2-^ ^23^~11~Na^+^ Mg-24 0 5. **.** 6. 7. 8. **[Electrons, Energy Levels, and Light]** 1. 2. 3. 4. 5. 6. **[Emission spectra, energy levels]** 7. 8. Refer to the diagram to the right: 9. a. b. c. **[Electron configuration - Energy levels, sublevels, and orbitals]** 1. 2. 3. 4. 5. 6. 7. Element Full electron configuration Abbreviated electron configuration --------- ----------------------------- ------------------------------------ Mn Zr 8. 9. Electron configuration Element ------------------------------------------- --------- 1s^2^2s^2^2p^6^3s^2^ 1s^2^2s^2^2p^6^3s^2^3p^6^4s^2^3d^10^4p^3^ 1s^1^ 10. Element Orbital notation --------- ------------------ Mg Sr Ge Mo Ca Ba Orbital notation Error identified ----------------------- ------------------   Unit 2 **Periodic Table & Valence Electrons** 1. Element Valence electrons Block (s,p,d,f) Group number Group name Period Metal or Nonmetal --------- ------------------- ----------------- -------------- ------------ -------- ------------------- Mn Ba Br Kr Cs 2. 3. **Attractive Force and Periodic Trends** 4. 5. 6. 7. 8. a. b. 9. 10. 11. a. b. 12. a. b. 13. 14. 15. 16. 17. c. d. **Reactivity of Metals and Nonmetals** 18. 19. 20. 21. We are going to learn about the trends in atomic radius and ionic radius. But before we do that, let us see how much we remember about attraction between charges. 1. 2. 3. For nitrogen and neon, compare the nuclear force of attraction on the outermost energy level. Which atom experiences a greater force. **[Explain how you came to your answer based on the number of protons and number of energy levels]**. (if you don't explain, you don't get the grade!) For neon and xenon, compare the nuclear force of attraction on the outermost energy level. Which atom experiences a greater force. **[Explain how you came to your answer based on the number of protons and number of energy levels]**. (if you don't explain, you don't get the grade!) The force of nuclear attraction on the outermost energy level can also determine the radius of the atoms. 1. 2. The number of energy levels also determine the radius of an atom. Regardless of the number of protons, more energy levels means a larger radius. 1. 2. Write out a trend for atomic radius: **Across the period of the periodic table, atomic radius \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_** **Down the group of the periodic table, atomic radius \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_** Now let us look at ions and their radius.**(Hint: write out electron configurations)** 1. 2. 3. 4. 5. 6. 7. 8. Unit 3 **LT3.1: Students will be able to distinguish metallic, ionic and covalent compounds. Students will be able to identify ions and chemical formulas for ionic compounds.** 1. Element Charge Ion Element Charge Ion --------- -------- -------- --------- -------- ----- Li 1+ Li^1+^ N Be O Al F Na S Mg Cl 2. Element 1 Element 2 Formula Element 1 Element 2 Formula ----------- ----------- --------- ----------- ----------- --------- K Cl Ca S Na O Sr P Li N Al O Mg F Cs Se 3. Compound Cation Anion Compound Cation Anion ----------- -------- ------- ---------- -------- ------- FeF~2~ Fe^2+^ F^1-^ Cu~3~N Fe~2~O~3~ Cs~2~X MgX Ag~2~S AlX~3~ ZnS Na~3~X XBr 4. Element/compound Type of bonding Element/compound Type of bonding ------------------ ----------------- ------------------ ----------------- Cl~2~ Cu OF~2~ Rb~2~S MgBr~2~ Fe~2~O~3~ HF O~2~ CaO H~2~O 5. 6. 7. **LT3.2: Students will be able to draw Lewis dot structures and count the number of electron domains around a central atom to predict the electron geometry of molecules using VSEPR, and determine the polarity of molecules.** 8. a. b. c. 9. Electron Domains around the Central Atom Number of lone pairs on the central atom Electron pair geometry Molecular geometry Bond angle ------------------------------------------ ------------------------------------------ ------------------------ -------------------- ------------ 2 0 3 0 3 1 4 0 4 1 4 2 10\. Complete the following table Molecule Lewis Structure \# of electron domains Electron pair geometry Molecular geometry VSEPR Sketch with bond angle ------------ ----------------- ------------------------ ------------------------ -------------------- ------------------------------ COBr~2~ H~2~O NH~3~ BF~3~ CH~2~Br~2~ CO~2~ Unit 4 1. \(a) H~2~O (b) CH~4~ (c) HF (d) NH~3~ (e) CH~3~OH 2. +-------------+-------------+-------------+-------------+-------------+ | **Substance | **Intermole | **Substance | **Intermole | **Which | | \#1** | cular** | \#2** | cular | substance | | | | | Forces** | has a | | | **Forces** | | | higher | | | | | | boiling | | | | | | point?** | | | | | | | | | | | | **(\#1 or | | | | | | \#2) - Why? | | | | | | Explain!** | +=============+=============+=============+=============+=============+ | HCl | | Cl~2~ | | | +-------------+-------------+-------------+-------------+-------------+ | H~2~O | | H~2~S | | | +-------------+-------------+-------------+-------------+-------------+ | CH~3~OH | | HCl | | | +-------------+-------------+-------------+-------------+-------------+ | NH~3~ | | CH~4~ | | | +-------------+-------------+-------------+-------------+-------------+ | C~6~H~14~ | | C~8~H~18~ | | | +-------------+-------------+-------------+-------------+-------------+ 3. 4. For the questions on this page, answer them as though you are explaining the concepts to a friend who is also in a chemistry class but is not able to make sense of IMFs and how they work. You want to explain it to your friend in such a way that **[they understand the concept]** and have the **[vocabulary necessary]** to be successful on a free response question 1. 2. 3. 4. 5. 6. 7. 8. Unit 5 Identify the type of reaction on the line to the right. Balance the chemical equations. 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. C~3~H~8~ + 5 O~2~ → 3 CO~2~ + 4 H~2~O a. b. 17. \_\_\_ AlBr~3~ + \_\_\_ K~2~SO~4~ → \_\_\_ KBr + \_\_\_\_ Al~2~(SO~4~)~3~ c. d. e. 18. \_\_\_ P~4~ + \_\_\_ O~2~ → \_\_\_ P~2~O~3~ f. g. h. i. 19. j. k. l. m. n.