Chemistry Chapter on Quantum Mechanics

General Instructions

• Read and analyze statements, questions, and illustrations.
• Answer in CAPITAL LETTERS.

Question 1

• Term for describing probable location and energy state of an electron: Quantum numbers.

Question 2

• Atomic configuration 1s²2s²2p⁶ corresponds to Neon.

Question 3

• Principal energy level of an atom: Energy level the electron occupies.

Question 4

• Subatomic particle with negative charge: Electron.

Question 5

• Correct electron configuration of Nitrogen (Atomic Number 7): 1s²2s²2p³.

Question 6

• Difference between Quantum Mechanical Model and older atomic models regarding electron positions: Uses probability to describe likely location in orbitals.

Question 7

• Quantum Mechanical Model's suggestion about electron movement: Exists within regions of space called orbitals.

Question 8

• Meaning of superscript number in electron configuration: Number of electrons in a specific orbital or sublevel.

Question 9

• Aufbau principle regarding electron configuration: Electrons fill orbitals from lowest to highest energy level.

Question 10

• How electron arrangement reflects the Pauli Exclusion Principle in Helium's orbital diagram: Electrons occupy orbitals singly before pairing up.

Question 11

• Which orbital violates maximum electron capacity rule in the diagram: The s orbital (violates rule as it is designed to hold a maximum of 2 electrons).

Question 12

• Bond formed between two nonmetal elements: Covalent bond.

Question 13

• Properties of ionic compounds: Crystal lattice structure.

Question 14

• Example of a covalent bond: NH₃

Question 15

• Example of an ionic bond: KF

Question 16

• Substance conducting electricity when dissolved in water: Sodium chloride (NaCl).

Question 17

• Property NOT of a covalent compound: Exists in a stable crystalline structure.

Question 18

• Substance type represented by diagram 3 (arrangement of particles): Ionic compound.

Question 19

• Property most indicative of an ionic compound: Solubility in water and electrical conductivity in solution.

Question 20

• Type of chemical bond between sodium and fluorine: Ionic bond.

Question 21

• Element transferring electron in Sodium Fluoride bond: Sodium.

Question 22

• Incorrect statement regarding sodium and fluorine bond: Sodium and fluorine share electrons equally.

Question 23

• Ion with positive charge: Cation.

Question 24

• Term for electron in outermost energy level responsible for chemical bonding: Valence electron.

Question 25

• Ion with negative charge: Anion.

Question 26

• Lewis Dot Structure for chlorine (Cl): Cl.

Question 27

• Valence electron for element in Family II, Period III of periodic table: 2.

Question 28

• Unique aspect of carbon: Carbon can form single, double, and triple bonds.

Question 29

• Carbon compound primary component of natural gas: Methane.

Question 30

• Hydrocarbon compound with a double bond: Alkene.

Question 31

• Organic compound used for disinfection: Isopropyl alcohol.

Question 32

• Compound needed to continue driving a car: Gasoline.

Question 33

• Description of organic compounds: Composed mainly of carbon and hydrogen.

Question 34

• Group of hydrocarbons in the provided figure: Alkene.

Question 35

• Number of hydrogen atoms in the given organic compound: 2.

Question 36

• IUPAC name for the given organic compound: Ethene.

Question 37

• Definition of viscosity: Measure of a liquid's resistance to flow.

Question 38

• Definition of odor in organic compounds: Smell of the compound.

Question 39

• Item Victor's grandmother asked him to buy: Gasoline.

Question 40

• Organic compound to protect bicycles from rusting: Lubricating oil.

Question 41

• Compound used to remove nail polish: Acetone.

Question 42

• Organic compound needed to cook the fish: Kerosene.

Question 43

• Molecular formula of methane: CH₄.

Question 44

• Number of atoms in 1 mole of silver: 6.02 x 10²³.

Question 45

• Molar mass of sulfate (SO₄): 96 g/mol.

Question 46

• Number of atoms in 3 moles of oxygen: 1.81 x 10²⁴.

Question 47

• Molar mass of CO₂: 44.01 g/mol.

Question 48

• Number of atoms in 2 moles of potassium: 2.41 x 10²⁴.

Question 49

• Molar mass of SO₂: 64.06 g/mol.

Question 50

• Molar mass of Mg(OH)₂: 58.32 g/mol.