MISD EAS Chemistry Fall 2024 Final Exam Review PDF

Name: ____________________________________ Period: ________ EAS Chemistry – Fall 2024 Semester Exam Review Unit 2: Matter 1. Know the three states of matter and their properties. a. Fill in the missing information below:...

Name: ____________________________________ Period: ________ EAS Chemistry – Fall 2024 Semester Exam Review Unit 2: Matter 1. Know the three states of matter and their properties. a. Fill in the missing information below: Solid Liquid Gas Property Definite Shape No Definite Volume Yes Atom Movement Free Compressible Almost None Thermal Expansion Large Kinetic Energy High 2. Be able to understand and identify phase changes based on particle structure. a. Define the six changes of state and provide illustrations of the particle structures for each one (the first one is done for you): Melting: solid → liquid Freezing: Evaporation: Condensation: Sublimation: Deposition: 3. Be able to classify, define, and identify the types of matter based on the matter flowchart. a. Fill in the missing information on the matter flowchart below:  EAS Chemistry – Fall 2024 Semester Exam Review b. What is the difference between an element and a compound? c. What is one similarity between an element and a compound? d. What is the difference between compounds and mixtures? e. What is one similarity between compounds and mixtures? f. What is the difference between a heterogeneous and homogeneous mixture? g. What is one similarity between a heterogeneous and homogeneous mixture? 4. Know the difference between a physical and chemical property. a. Define “physical property” and list five examples: i. physical property – 1. 2. 3. 4. 5. b. List and define the two types of physical properties and give three examples of each: i. 1. 2. 3. ii. 1. 2. 3. c. Define “chemical property” and list five examples: i. chemical property – 1. 2. 3. 4. 5. 5. Know the difference between a physical and chemical change. a. Define “physical change” and list five examples: i. physical change – 1. 2. 3. 4. 5. b. Define “chemical change” and list five examples: i. chemical change – 1. 2. 3. 4. 5.  EAS Chemistry – Fall 2024 Semester Exam Review c. List the six signs that a chemical change has occurred: i. ii. iii. iv. v. vi. d. Which type of change (physical or chemical) has to occur to form a compound? 6. Be able to define, calculate, and understand the concept of density. a. Define density: b. Fill in the blank formula triangle below to obtain the formulas involving density (include units): d= units: m= units: V= units: c. Solve the following density problem below (show your work): Mercury metal is poured into a graduated cylinder and it reads exactly 22.5 mL. The mercury used to fill the cylinder has a mass of 306.0 g. Calculate the density of the mercury. d. Is density an extensive or intensive physical property? Explain your answer. e. If a perfectly symmetrical cube is cut exactly in half, what would the density of the two new pieces be? Explain your answer in detail.  EAS Chemistry – Fall 2024 Semester Exam Review f. Properly layer the substances from the table below in the density column: Substance Density (g/mL) Water 1.00 Cork 0.21 Ethyl Alcohol 0.79 Mercury 13.59 Methanol 0.94 Unit 3: Atomic Structure 7. Know the major contributions in the development of atomic theory. a. Using the diagrams of models below, identify the following: (1) the name of the contributor, (2) the name of the model, (3) any discoveries they are credited with, and (4) any experiments they used in their discoveries (if there is no information available, simply put “N/A”): 8. Be able to identify elements with proper atomic notation. a. Identify what the numbers represent in the atomic notation example below: i. b. Write the following elements in proper atomic notation: i. Iron ii. Barium iii. Xenon  EAS Chemistry – Fall 2024 Semester Exam Review 9. Be able to draw Bohr Models for any given element. a. Draw a Bohr Model for the elements below: i. Magnesium ii. Fluorine 10. Familiarize yourself with valence electrons, ions, and ionic notation. a. For each of the elements below, (1) identify the number of valence electrons, (2) how many electrons it gains/loses to become an ion, and (3) the resulting ion written in proper ionic notation (the first one is done for you): i. Sulfur: 6 valence e- → gains 2 e- → S2- ii. Chlorine: iii. Calcium: iv. Lithium: 11. Be able to identify isotopes with proper isotopic notation. a. What does the number in Bromine-81 represent? b. Write the following isotopes in proper isotopic notation: i. The element with an atomic number of 8 and 10 neutrons in the nucleus ii. The element with 26 protons and 32 neutrons in the nucleus 12. Memorize the formula for, and be able to calculate, the average atomic mass of isotopes. a. What is the formula used to calculate the average atomic mass of isotopes? b. Answer the following question (show your work): Using data from the table below, calculate the average atomic mass of Element A: Isotope Mass Percent Abundance A-79 78.92 amu 50.69% A-81 80.92 amu 49.31%  EAS Chemistry – Fall 2024 Semester Exam Review Unit 4: Periodic Table & Electrons in Atoms 13. Know the possible subshells and orbitals for electron configurations of elements. a. Fill in the missing information on the table below: Block on Type Subshell Found # of Orbitals # of electrons held Periodic Table s-block p-block d-block f-block 14. Know how to draw electron orbital diagrams according to the Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule. a. Draw electron orbital diagrams for the following elements in the ground state: i. Carbon ii. Oxygen 15. Be able to write electron configurations for elements and identify elements based on their written electron configurations. a. Write the full electron configuration for the following elements in the ground state: i. Aluminum ii. Chromium b. Identify the elements below based on their electron configurations: i. 1s22s22p63s23p64s2 ii. 1s22s22p63s23p64s23d104p65s24d9 16. Be able to write noble gas (shorthand) electron configurations for elements. a. Write the noble gas configuration for the following elements: i. Tin ii. Nickel  EAS Chemistry – Fall 2024 Semester Exam Review 17. Know the major contributions in the development of the periodic table. a. How did Mendeleev arrange the periodic table? Why? b. How did Moseley arrange the periodic table? Why? 18. Understand the organization of the periodic table and the resulting trends. a. What are the rows on the periodic table called? What do elements in the same row have in common? b. What are columns on the periodic table called? What do elements in the same column have in common? 19. Know the location of the major families on the periodic table along with their properties. a. What are the three major types of elements found on the periodic table? Where are each of them generally located on the periodic table? List three properties of each. i. 1. 2. 3. ii. 1. 2. 3. iii. 1. 2. 3. b. Identify the family of elements according to their group number on the periodic table and list three properties of each: i. Group 1/1A – 1. 2. 3. ii. Group 2/2A – 1. 2. 3. iii. Group 17/7A – 1. 2. 3. iv. Group 18/8A – 1. 2. 3.  EAS Chemistry – Fall 2024 Semester Exam Review 20. Be able to identify the five major trends across the periodic table. a. Define the following trends and then label them on the periodic table below: i. Oxidation number – ii. Atomic radius – iii. Ionization energy – iv. Electron affinity – v. Electronegativity – b. What happens to atomic radius as we go across (→) a period? Why? c. What happens to atomic radius as we go down a group? Why? d. Put the following elements in increasing order (smallest → largest) of atomic radius: i. Copper, Fluorine, Barium, Phosphorus, Chromium e. Which group of elements would be the easiest to remove an electron from? Explain. f. Which group of elements would be the most difficult to remove an electron from? Explain. Unit 5: Nuclear Chemistry & The Electromagnetic (EM) Spectrum 21. Be able to calculate the half-life of an element undergoing nuclear decay. a. If you have 100 grams of a radioactive isotope with a half-life of 10 years: i. How much of the isotope will be left after 10 years? ii. How much of the isotope will be left after 20 years? iii. How many half-lives will occur in 40 years?  EAS Chemistry – Fall 2024 Semester Exam Review 22. Be able to identify the different types of radiation and radioactive decay. a. Label the appropriate type of nuclear particle. i. 42α or 42He ii. 0-1ß or 0-1e iii. 00ℽ b. Identify the type of radiation shown in the following reactions. i. 23592He → 42He + 23190Th ii. 14 C → 147N + 0-1e 6 iii. 99m 43 Tc → 9943Tc + 00ℽ 23. Be able to balance a nuclear equation. a. Balance the following nuclear equations. Be sure to express your answer in the correct nuclear notation. i. _______ → 4020Ca + 0-1e ii. 222 88 Ra → _______ + 42He 24. Be able to calculate the energy, frequency, or wavelength of a photon using the speed of light or Planck’s constant. a. Fill in the blank formula triangle below to obtain the formulas for the frequency or wavelength of a photon using the speed of light (include units): c= units: λ= units: ν= units: b. Fill in the blank formula triangle below to obtain the formulas for the frequency or energy of a photon using Planck’s constant (include units): E= units: h= units: ν= units: c. Answer the following questions using the formulas/triangles above (show your work). i. Calculate the frequency of a photon of light with a wavelength of 4.0x10-7 m. ii. A photon has a frequency of 2.68x106 Hz. The energy of this photon (in J) is…  EAS Chemistry – Fall 2024 Semester Exam Review Unit 6: Ionic Bonding 25. Be able to draw Lewis Dot Structures for given elements. a. Draw the correct Lewis Dot Structure for the following elements: i. Phosphorus iii. Magnesium ii. Oxygen iv. Fluorine 26. Be able to write chemical formulas for binary ionic compounds. a. Write the chemical formula for the following binary ionic compounds: i. Calcium bromide iii. Tin (IV) sulfide ii. Sodium phosphide iv. Nickel (III) selenide 27. Review the rules for naming all binary ionic compounds. a. Write the proper name for the following binary ionic compounds: i. Na2S iii. Cr2O3 ii. Li3P iv. CuO 28. Be able to write chemical formulas for ternary ionic compounds. a. Write the chemical formula for the following ternary ionic compounds: i. Magnesium nitrite iii. Nickel (III) phosphate ii. Aluminum hydroxide iv. Copper (I) carbonate 29. Review the rules for naming all ternary compounds. a. Write the proper name for the following ternary ionic compounds: i. NH4OH iii. Ti(NO3)3 ii. SrSO4 iv. NiCrO4  EAS Chemistry – Fall 2024 Semester Exam Review Unit 7: Covalent Bonding 30. Be able to name and write formulas for covalent compounds. a. Complete the following table for prefixes used in covalent compounds (memorize these): Number of Atoms Prefix 1 2 3 4 5 6 7 8 9 10 b. Write the chemical formula for the following covalent compounds: i. Tetracarbon octahydride ii. Diphosphorus tribromide iii. Carbon monoxide iv. Carbon tetrachloride c. Write the proper name for the following covalent compounds: i. P6O4 iii. C2Cl7 ii. N3O iv. P5Br9  EAS Chemistry – Fall 2024 Semester Exam Review 31. Understand how electrons around the central atom of a molecule affect shape and bond angles. a. Fill in the table below to show how electrons around the central atom affect molecular geometry: #pairs of bonding electrons #pairs of lone electrons VSEPR Geometry Bond Angle on central atom on central atom Linear – AX2 Bent – AX2 Trigonal Planar – AX3 Trigonal Pyramidal – AX3 Tetrahedral – AX4 32. Be able to determine the shape of any covalent compound from its chemical formula. a. From the chemical formulas below, (1) determine valence electron count, (2) draw the Lewis Dot Structure, (3) draw the bonding diagram (in the correct shape), (4) name the correct geometry/shape, and (5) list the correct bond angle (show your work): i. NH3 ii. BeF2 iii. CH4 iv. BF3 v. SCl2  EAS Chemistry – Fall 2024 Semester Exam Review Unit 8: Chemical Reactions & Balancing Equations 33. Be able to define and identify the five basic types of chemical reactions. a. For each of the five types of reactions below, define them, write a general equation for them, and a good way to remember what to look for in that type of reaction. i. Synthesis - ii. Decomposition – iii. Single Replacement (Displacement) – iv. Double Replacement (Displacement) – v. Combustion – b. Classify the reactions below: i. SiO2 + 4HF → SiF4 + 2H2O ii. CH4 + 2O2 ∆→ CO2 + 2H2O iii. N2 + 2O2 + H2O → 2HNO3 iv. Zn + Cu(NO3)2 → Zn(NO3)2 + Cu v. Al2(CO3)3 ∆ → Al2O3 + 3CO2 vi. 2Cl2 + 2MgO → O2 + 2MgCl2 34. Be able to balance chemical equations: a. Classify and balance the following chemical equations: i. ___B + ___O2 → ___B2O3 ii. ___Al + ___Cl2 → ___AlCl3 iii. ___CuCl2 + ___KOH → ___KCl + ___Cu(OH)2 iv. ___C3H8 + ___O2 ∆ → ___CO2 + ___H2O