객관식
Which of the following best describes the difference between an atom and a molecule?
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목차
- 1. Intro to General Chemistry3h 58m
- Classification of Matter18m
- Physical & Chemical Changes19m
- Chemical Properties7m
- Physical Properties6m
- Intensive vs. Extensive Properties13m
- Temperature12m
- Scientific Notation13m
- SI Units8m
- Metric Prefixes24m
- Significant Figures9m
- Significant Figures: Precision in Measurements8m
- Significant Figures: In Calculations17m
- Conversion Factors16m
- Dimensional Analysis24m
- Density12m
- Density of Geometric Objects19m
- Density of Non-Geometric Objects5m
- 2. Atoms & Elements4h 34m
- The Atom10m
- Subatomic Particles17m
- Isotopes17m
- Ions27m
- Atomic Mass33m
- Periodic Table: Classifications11m
- Periodic Table: Group Names8m
- Periodic Table: Representative Elements & Transition Metals7m
- Periodic Table: Element Symbols6m
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- Periodic Table: Phases9m
- Periodic Table: Charges20m
- Calculating Molar Mass10m
- Mole Concept31m
- Law of Conservation of Mass5m
- Law of Definite Proportions12m
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- Millikan Oil Drop Experiment8m
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- 3. Chemical Reactions4h 34m
- Empirical Formula18m
- Molecular Formula21m
- Combustion Analysis39m
- Combustion Apparatus16m
- Polyatomic Ions25m
- Naming Ionic Compounds12m
- Writing Ionic Compounds8m
- Naming Ionic Hydrates8m
- Naming Acids23m
- Naming Molecular Compounds8m
- Balancing Chemical Equations14m
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- Percent Yield21m
- Mass Percent6m
- Functional Groups in Chemistry11m
- 4. BONUS: Lab Techniques and Procedures1h 25m
- 5. BONUS: Mathematical Operations and Functions52m
- 6. Chemical Quantities & Aqueous Reactions4h 17m
- Solutions9m
- Molarity22m
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- Dilutions15m
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- Molecular Equations21m
- Gas Evolution Equations13m
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- Complete Ionic Equations18m
- Calculate Oxidation Numbers16m
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- 7. Gases3h 58m
- Pressure Units6m
- The Ideal Gas Law18m
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- Chemistry Gas Laws14m
- Chemistry Gas Laws: Combined Gas Law12m
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- Standard Temperature and Pressure14m
- Effusion15m
- Root Mean Square Speed9m
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- Velocity Distributions4m
- Kinetic Molecular Theory16m
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- 8. Thermochemistry3h 2m
- Nature of Energy6m
- Kinetic & Potential Energy11m
- First Law of Thermodynamics7m
- Internal Energy8m
- Endothermic & Exothermic Reactions10m
- Heat Capacity23m
- Constant-Pressure Calorimetry26m
- Constant-Volume Calorimetry11m
- Thermal Equilibrium8m
- Thermochemical Equations14m
- Formation Equations11m
- Enthalpy of Formation14m
- Hess's Law26m
- 9. Quantum Mechanics3h 4m
- Wavelength and Frequency6m
- Speed of Light9m
- The Energy of Light13m
- Electromagnetic Spectrum10m
- Photoelectric Effect20m
- De Broglie Wavelength9m
- Heisenberg Uncertainty Principle17m
- Bohr Model14m
- Emission Spectrum5m
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- Introduction to Quantum Mechanics5m
- Quantum Numbers: Principal Quantum Number5m
- Quantum Numbers: Angular Momentum Quantum Number10m
- Quantum Numbers: Magnetic Quantum Number11m
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- Quantum Numbers: Nodes7m
- 10. Periodic Properties of the Elements3h 45m
- The Electron Configuration27m
- The Electron Configuration: Condensed4m
- The Electron Configurations: Exceptions13m
- The Electron Configuration: Ions12m
- Paramagnetism and Diamagnetism13m
- The Electron Configuration: Quantum Numbers17m
- Valence Electrons of Elements12m
- Periodic Trend: Metallic Character6m
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- 11. Bonding & Molecular Structure3h 51m
- Lewis Dot Symbols10m
- Chemical Bonds13m
- Dipole Moment15m
- Octet Rule10m
- Formal Charge12m
- Lewis Dot Structures: Neutral Compounds20m
- Lewis Dot Structures: Sigma & Pi Bonds15m
- Lewis Dot Structures: Ions15m
- Lewis Dot Structures: Exceptions14m
- Lewis Dot Structures: Acids17m
- Resonance Structures25m
- Average Bond Order4m
- Bond Energy17m
- Coulomb's Law7m
- Lattice Energy16m
- Born Haber Cycle15m
- 12. Molecular Shapes & Valence Bond Theory2h 11m
- 13. Liquids, Solids & Intermolecular Forces2h 41m
- Molecular Polarity10m
- Intermolecular Forces22m
- Intermolecular Forces and Physical Properties12m
- Clausius-Clapeyron Equation22m
- Phase Diagrams13m
- Heating and Cooling Curves28m
- Atomic, Ionic, and Molecular Solids11m
- Crystalline Solids6m
- Simple Cubic Unit Cell7m
- Body Centered Cubic Unit Cell14m
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- 14. Solutions3h 17m
- Solutions: Solubility and Intermolecular Forces20m
- Molality18m
- Parts per Million (ppm)13m
- Mole Fraction of Solutions9m
- Solutions: Mass Percent12m
- Types of Aqueous Solutions8m
- Intro to Henry's Law4m
- Henry's Law Calculations12m
- The Colligative Properties17m
- Boiling Point Elevation18m
- Freezing Point Depression10m
- Osmosis21m
- Osmotic Pressure10m
- Vapor Pressure Lowering (Raoult's Law)19m
- 15. Chemical Kinetics3h 1m
- 16. Chemical Equilibrium2h 31m
- 17. Acid and Base Equilibrium5h 5m
- Acids Introduction9m
- Bases Introduction7m
- Binary Acids15m
- Oxyacids10m
- Bases14m
- Amphoteric Species5m
- Arrhenius Acids and Bases5m
- Bronsted-Lowry Acids and Bases21m
- Lewis Acids and Bases13m
- The pH Scale17m
- Auto-Ionization9m
- Ka and Kb16m
- pH of Strong Acids and Bases9m
- Ionic Salts17m
- pH of Weak Acids31m
- pH of Weak Bases32m
- Diprotic Acids and Bases8m
- Diprotic Acids and Bases Calculations30m
- Triprotic Acids and Bases10m
- Triprotic Acids and Bases Calculations17m
- 18. Aqueous Equilibrium4h 47m
- Intro to Buffers21m
- Henderson-Hasselbalch Equation19m
- Intro to Acid-Base Titration Curves13m
- Strong Titrate-Strong Titrant Curves9m
- Weak Titrate-Strong Titrant Curves15m
- Acid-Base Indicators8m
- Titrations: Weak Acid-Strong Base38m
- Titrations: Weak Base-Strong Acid41m
- Titrations: Strong Acid-Strong Base11m
- Titrations: Diprotic & Polyprotic Buffers32m
- Solubility Product Constant: Ksp17m
- Ksp: Common Ion Effect18m
- Precipitation: Ksp vs Q12m
- Selective Precipitation9m
- Complex Ions: Formation Constant18m
- 19. Chemical Thermodynamics1h 51m
- 20. Electrochemistry2h 42m
- 21. Nuclear Chemistry2h 37m
- Intro to Radioactivity10m
- Alpha Decay9m
- Beta Decay7m
- Gamma Emission7m
- Electron Capture & Positron Emission9m
- Neutron to Proton Ratio7m
- Band of Stability: Alpha Decay & Nuclear Fission10m
- Band of Stability: Beta Decay3m
- Band of Stability: Electron Capture & Positron Emission4m
- Band of Stability: Overview14m
- Measuring Radioactivity7m
- Rate of Radioactive Decay12m
- Radioactive Half-Life16m
- Mass Defect19m
- Nuclear Binding Energy14m
- 22. Organic Chemistry5h 4m
- Introduction to Organic Chemistry8m
- Structural Formula8m
- Condensed Formula10m
- Skeletal Formula6m
- Spatial Orientation of Bonds3m
- Intro to Hydrocarbons16m
- Isomers11m
- Chirality12m
- Functional Groups in Chemistry11m
- Naming Alkanes4m
- The Alkyl Groups9m
- Naming Alkanes with Substituents13m
- Naming Cyclic Alkanes6m
- Naming Other Substituents8m
- Naming Alcohols11m
- Naming Alkenes11m
- Naming Alkynes9m
- Naming Ketones5m
- Naming Aldehydes5m
- Naming Carboxylic Acids4m
- Naming Esters8m
- Naming Ethers5m
- Naming Amines5m
- Naming Benzene7m
- Alkane Reactions7m
- Intro to Addition Reactions4m
- Halogenation Reactions4m
- Hydrogenation Reactions3m
- Hydrohalogenation Reactions7m
- Alcohol Reactions: Substitution Reactions4m
- Alcohol Reactions: Dehydration Reactions9m
- Intro to Redox Reactions8m
- Alcohol Reactions: Oxidation Reactions7m
- Aldehydes and Ketones Reactions6m
- Ester Reactions: Esterification4m
- Ester Reactions: Saponification3m
- Carboxylic Acid Reactions4m
- Amine Reactions3m
- Amide Formation4m
- Benzene Reactions10m
- 23. Chemistry of the Nonmetals2h 39m
- Main Group Elements: Bonding Types4m
- Main Group Elements: Boiling & Melting Points7m
- Main Group Elements: Density11m
- Main Group Elements: Periodic Trends7m
- The Electron Configuration Review16m
- Periodic Table Charges Review20m
- Hydrogen Isotopes4m
- Hydrogen Compounds11m
- Production of Hydrogen8m
- Group 1A and 2A Reactions7m
- Boron Family Reactions7m
- Boron Family: Borane7m
- Borane Reactions7m
- Nitrogen Family Reactions12m
- Oxides, Peroxides, and Superoxides12m
- Oxide Reactions4m
- Peroxide and Superoxide Reactions6m
- Noble Gas Compounds3m
- 24. Transition Metals and Coordination Compounds3h 19m
- Atomic Radius & Density of Transition Metals11m
- Electron Configurations of Transition Metals7m
- Electron Configurations of Transition Metals: Exceptions11m
- Paramagnetism and Diamagnetism10m
- Ligands10m
- Complex Ions5m
- Coordination Complexes7m
- Classification of Ligands11m
- Coordination Numbers & Geometry9m
- Naming Coordination Compounds22m
- Writing Formulas of Coordination Compounds8m
- Isomerism in Coordination Complexes17m
- Orientations of D Orbitals4m
- Intro to Crystal Field Theory10m
- Crystal Field Theory: Octahedral Complexes5m
- Crystal Field Theory: Tetrahedral Complexes4m
- Crystal Field Theory: Square Planar Complexes4m
- Crystal Field Theory Summary8m
- Magnetic Properties of Complex Ions9m
- Strong-Field vs Weak-Field Ligands6m
- Magnetic Properties of Complex Ions: Octahedral Complexes11m
2. Atoms & Elements
The Atom
객관식
Which of the following best describes the electric charge of a proton?
A
Double positive (+2)
B
Neutral (0)
C
Negative (-1)
D
Positive (+1)
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검증된 단계별 안내1
Recall that the electric charge of subatomic particles is a fundamental property: protons, neutrons, and electrons each have characteristic charges.
Understand that a proton carries a positive electric charge, which is the basic unit of positive charge in chemistry and physics.
Recognize that the magnitude of the proton's charge is equal to the magnitude of the electron's charge but opposite in sign.
Note that the proton's charge is not double positive (+2), neutral (0), or negative (-1), but rather a single positive charge (+1).
Therefore, the best description of the electric charge of a proton is Positive (+1).
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