ANSWER KEY - GC2 REVIEWER PDF

GRADED REVIEWER IN GENERAL CHEMISTRY 2 LESSON 1: Gas Law Boyle’s Law - It states that the volume of a given mass of gas held at a constant temperature is inversely proportional to its pressure. Charles’s Law - It states that the Kelvin temperature and the volume of gas are dire...

GRADED REVIEWER IN GENERAL CHEMISTRY 2 LESSON 1: Gas Law Boyle’s Law - It states that the volume of a given mass of gas held at a constant temperature is inversely proportional to its pressure. Charles’s Law - It states that the Kelvin temperature and the volume of gas are directly proportional when there is no change in pressure of gas. Avogadro’s Law - It states that equal volume of gases at the same temperature and pressure contain equal number of molecules. Ideal Gas Law - Boyle’s, Charles’s, Gay-Lussac’s and Avogadro’s laws, when combine constitute the Ideal Gas Law. It is based on the experimental measurements of gases: temperature, pressure, volume, and number of moles. TRY THIS! Directions: Read and analyze the situations/equation given below. Identify what gas law id being described. 1. Imagine you have a balloon. When you squeeze it, the balloon shrinks in size and feels harder to press. Essentially, squeezing the balloon makes the air inside more pressurized because it has less space to move around. _____________________________________________________________ 2. Picture a scuba diver planning a dive. They need to calculate how much air to take in their tank. This involves considering how much air will be used at different depths, as pressure increases with depth underwater. The diver needs to make sure there's enough air for the entire dive based on how much space it will occupy under different pressures and temperatures. _____________________________________________________________ 3. Consider a hot air balloon. When you heat the air inside, the balloon gets bigger and rises into the sky. The heated air takes up more space, causing the balloon to expand and lift off. _____________________________________________________________ 4. Think about filling a tire with air. The more air you pump into the tire, the bigger it gets. Adding more air molecules increases the tire's size. _____________________________________________________________ 5. ___________________________________________ 6. __________________________________________ 7. __________________________________________ 8. ______________________________________ 8. A gas occupies a volume of 4.0 liters at a pressure of 1.2 atm. If the pressure is increased to 3.0 atm while the temperature remains constant, what will be the new volume of the gas? 9. A gas at 20.0°C occupies a volume of 2.5 liters. What volume will the gas occupy if the temperature is increased to 60.0°C, assuming the pressure remains constant? 10. If 3.0 moles of a gas occupy a volume of 72.0 liters at a certain temperature and pressure, what will be the volume of the gas if the amount is increased to 5.0 moles, assuming the temperature and pressure remain constant? 11. A gas sample has a volume of 10.0 liters at a pressure of 2.0 atm and a temperature of 300 K. How many moles of gas are present in the sample? LESSON 2: Quantum Mechanics/Electronic Configuration ELECTRONIC CONFIGURATION STEP 1: Determine the atomic number STEP 2: Use the electronic structure/mnemonics to write the correct configuration of a given element. Remember that each orbital has a maximum electron that it can accommodate. s=2 p=6 d = 10 f = 14 STEP 3: Make sure that the superscripts when added are equal to the atomic number. Superscript can be lowered but can never exceed to its maximum. QUANTUM NUMBERS Principal Quantum Number (n) – energy of the electron. Azimuthal or Angular Momentum (𝓵) – shape of the orbital. (s = 0 p=1 d=2 f = 3) Magnetic (𝒎𝓵) – orientation of the orbital in shape. (s = 0 p = +1, 0, -1 d = +2, +1, 0, -2, -1 f = +3, +2, +1, 0, -3, -2, -1) Spin (𝒎𝒔) – spin of an electron. (↑ = +1/2 ↓ = −1/2) TRY THIS! Directions: Read and analyze each question. Encircle the correct letter of your answer. 12. Which sets of quantum numbers is valid for an electron in a 4d orbital? A. n = 3, ℓ = 2, mℓ= 1, ms= -1/2 B. n = 4, ℓ = 3, mℓ= 0, ms= +1/2 C. n = 4, ℓ = 2, mℓ= 1, ms= +1/2 D. n = 4, ℓ = 1, mℓ= -2, ms= -1/2 13. What does the principal quantum number (n) describe? A. The shape of the orbital. B. The orientation of the orbitals. C. The spin direction of the electron. D. The size and energy level of the orbital. 14. Which quantum number determines the shape of the orbitals given subshell? A. Angular momentum quantum number C. Spin quantum number B. Magnetic quantum number D. Principal quantum number 15. For an electron in a 3p orbital, what is the value of the angular momentum number (ℓ)? A. 0 B. 1 C. 2 D. 3  16. If an electron has the following set of quantum numbers: n = 2, ℓ= 1, mℓ= 0, ms= -1/2. In which orbitals is this electron located? A. 2s B. 2p C. 3s D. 3p 17. Write the electronic configuration and condensed configuration of Manganese. ___________________________________________ 18. Write the electronic configuration and condensed configuration of Gold. ___________________________________________ LESSON 3: CHEMICAL BONDING/LEWIS DOT STRUCTURE LEWIS DOT STRUCTURE IN IONIC BONDING – metal + nonmetal (metal as the giver) Example: Lithium (Li) has 1 valence electron Fluorine (F) has 7 valence electrons Lithium is metal so it will give its electron to fluorine to achieve the octet rule. Note: Transferring of electron should be represented by an arrow which has a visible arrow head.  LEWIS DOT STRUCTURE IN COVALENT BONDING – nonmetal + nonmetal (sharing of electrons) Example: H2O Hydrogen (H) has 1 valence electron Oxygen (O) has 6 valence electrons Find the total number of valence electron by adding the electrons of given elements. H–1x2=2 O–6 Total = 8 e- Covalent compound is sharing, the total valence electron you get should be shared for both hydrogen and oxygen equally. (Hydrogen follows the duet rule, oxygen follows octet rule). In covalent bonding, molecular geometry and polarity is also needed. To find the molecular geometry of a covalent compound, VSEPR Theory is used. Refer to the table below. To predict the shape of H2O, add the bond pair and lone pair. [Bond pair is represented as lines, while lone pairs are sots) H 2O Bp = 2 Lp = 2 (Use this to predict the specific geometry, shapes within the yellow box border) Total = 4 (Use this to identify the number of electron dense areas)  The electron dense are is 4 which is equivalent to TETRAHEDRAL, the specific geometry is BENT because there are 2 lone pairs. To identify the polarity of a covalent compound, the number of lone pairs left in the central atom should be considered. Polar = with lone pair Nonpolar = without lone pair Therefore, Water (H2O) has a molecular geometry of TETRAHEDRAL BENT and it is POLAR. TRY THIS! Directions: Draw the Lewis dot structure of the following ionic compounds. 19. MgBr2 20. Al2O3 21. CaCl2 Directions: Draw the Lewis dot structure of the following covalent compounds. Predict the molecular geometry using the VSEPR theory and its polarity. 22. HCl 23. HCN 24. SO2 Molecular geometry: Molecular geometry: Molecular geometry: _____________________________ __________________________ _____________________________ Polarity Polarity Polarity _____________________________ __________________________ _____________________________