Multiple Choice
A 48.3 g sample of an aluminum iodine compound contains 3.2 g of aluminum. What is the empirical formula for the compound?
Table of contents
- 1. Intro to General Chemistry
- Classification of Matter
- Physical & Chemical Changes
- Chemical Properties
- Physical Properties
- Intensive vs. Extensive Properties
- Temperature
- Scientific Notation
- SI Units
- Metric Prefixes
- Significant Figures
- Significant Figures: Precision in Measurements
- Significant Figures: In Calculations
- Conversion Factors
- Dimensional Analysis
- Density
- Density of Geometric Objects
- Density of Non-Geometric Objects
- 2. Atoms & Elements
- The Atom
- Subatomic Particles
- Isotopes
- Ions
- Atomic Mass
- Periodic Table: Classifications
- Periodic Table: Group Names
- Periodic Table: Representative Elements & Transition Metals
- Periodic Table: Element Symbols
- Periodic Table: Elemental Forms
- Periodic Table: Phases
- Periodic Table: Charges
- Calculating Molar Mass
- Mole Concept
- Law of Conservation of Mass
- Law of Definite Proportions
- Atomic Theory
- Law of Multiple Proportions
- Millikan Oil Drop Experiment
- Rutherford Gold Foil Experiment
- 3. Chemical Reactions
- Empirical Formula
- Molecular Formula
- Combustion Analysis
- Combustion Apparatus
- Polyatomic Ions
- Naming Ionic Compounds
- Writing Ionic Compounds
- Naming Ionic Hydrates
- Naming Acids
- Naming Molecular Compounds
- Balancing Chemical Equations
- Stoichiometry
- Limiting Reagent
- Percent Yield
- Mass Percent
- Functional Groups in Chemistry
- 4. BONUS: Lab Techniques and Procedures
- 5. BONUS: Mathematical Operations and Functions
- 6. Chemical Quantities & Aqueous Reactions
- 7. Gases
- Pressure Units
- The Ideal Gas Law
- The Ideal Gas Law Derivations
- The Ideal Gas Law Applications
- Chemistry Gas Laws
- Chemistry Gas Laws: Combined Gas Law
- Mole Fraction of Gases
- Partial Pressure
- The Ideal Gas Law: Molar Mass
- The Ideal Gas Law: Density
- Gas Stoichiometry
- Standard Temperature and Pressure
- Effusion
- Root Mean Square Speed
- Kinetic Energy of Gases
- Maxwell-Boltzmann Distribution
- Velocity Distributions
- Kinetic Molecular Theory
- Van der Waals Equation
- 8. Thermochemistry
- 9. Quantum Mechanics
- Wavelength and Frequency
- Speed of Light
- The Energy of Light
- Electromagnetic Spectrum
- Photoelectric Effect
- De Broglie Wavelength
- Heisenberg Uncertainty Principle
- Bohr Model
- Emission Spectrum
- Bohr Equation
- Introduction to Quantum Mechanics
- Quantum Numbers: Principal Quantum Number
- Quantum Numbers: Angular Momentum Quantum Number
- Quantum Numbers: Magnetic Quantum Number
- Quantum Numbers: Spin Quantum Number
- Quantum Numbers: Number of Electrons
- Quantum Numbers: Nodes
- 10. Periodic Properties of the Elements
- The Electron Configuration
- The Electron Configuration: Condensed
- The Electron Configurations: Exceptions
- The Electron Configuration: Ions
- Paramagnetism and Diamagnetism
- The Electron Configuration: Quantum Numbers
- Valence Electrons of Elements
- Periodic Trend: Metallic Character
- Periodic Trend: Atomic Radius
- Periodic Trend: Ionic Radius
- Periodic Trend: Ionization Energy
- Periodic Trend: Successive Ionization Energies
- Periodic Trend: Electron Affinity
- Periodic Trend: Electronegativity
- Periodic Trend: Effective Nuclear Charge
- Periodic Trend: Cumulative
- 11. Bonding & Molecular Structure
- Lewis Dot Symbols
- Chemical Bonds
- Dipole Moment
- Octet Rule
- Formal Charge
- Lewis Dot Structures: Neutral Compounds
- Lewis Dot Structures: Sigma & Pi Bonds
- Lewis Dot Structures: Ions
- Lewis Dot Structures: Exceptions
- Lewis Dot Structures: Acids
- Resonance Structures
- Average Bond Order
- Bond Energy
- Coulomb's Law
- Lattice Energy
- Born Haber Cycle
- 12. Molecular Shapes & Valence Bond Theory
- 13. Liquids, Solids & Intermolecular Forces
- 14. Solutions
- Solutions: Solubility and Intermolecular Forces
- Molality
- Parts per Million (ppm)
- Mole Fraction of Solutions
- Solutions: Mass Percent
- Types of Aqueous Solutions
- Intro to Henry's Law
- Henry's Law Calculations
- The Colligative Properties
- Boiling Point Elevation
- Freezing Point Depression
- Osmosis
- Osmotic Pressure
- Vapor Pressure Lowering (Raoult's Law)
- 15. Chemical Kinetics
- 16. OLD Chemical Equilibrium
- 17. OLD Acid and Base Equilibrium
- 18. OLD Aqueous Equilibrium
- 19. OLD Chemical Thermodynamics
- 20. OLD Electrochemistry
- 21. OLD Nuclear Chemistry
- 22. OLD Organic Chemistry -
- 23. OLD Chemistry of the Nonmetals
- 24. OLD Transition Metals and Coordination Compounds
- 16. Chemical Equilibrium
- 17. Acid and Base Equilibrium
- Acids Introduction
- Bases Introduction
- Binary Acids
- Oxyacids
- Bases
- Amphoteric Species
- Arrhenius Acids and Bases
- Bronsted-Lowry Acids and Bases
- Lewis Acids and Bases
- The pH Scale
- Auto-Ionization
- Ka and Kb
- pH of Strong Acids and Bases
- Ionic Salts
- pH of Weak Acids
- pH of Weak Bases
- Diprotic Acids and Bases
- Diprotic Acids and Bases Calculations
- Triprotic Acids and Bases
- Triprotic Acids and Bases Calculations
- 18. Aqueous Equilibrium
- Intro to Buffers
- Henderson-Hasselbalch Equation
- Intro to Acid-Base Titration Curves
- Strong Titrate-Strong Titrant Curves
- Weak Titrate-Strong Titrant Curves
- Acid-Base Indicators
- Titrations: Weak Acid-Strong Base
- Titrations: Weak Base-Strong Acid
- Titrations: Strong Acid-Strong Base
- Titrations: Diprotic & Polyprotic Buffers
- Solubility Product Constant: Ksp
- Ksp: Common Ion Effect
- Precipitation: Ksp vs Q
- Selective Precipitation
- Complex Ions: Formation Constant
- 19. Chemical Thermodynamics
- 20. Electrochemistry
- 21. Nuclear Chemistry
- Intro to Radioactivity
- Alpha Decay
- Beta Decay
- Gamma Emission
- Electron Capture & Positron Emission
- Neutron to Proton Ratio
- Band of Stability: Alpha Decay & Nuclear Fission
- Band of Stability: Beta Decay
- Band of Stability: Electron Capture & Positron Emission
- Band of Stability: Overview
- Measuring Radioactivity
- Rate of Radioactive Decay
- Radioactive Half-Life
- Mass Defect
- Nuclear Binding Energy
- 22. Organic Chemistry
- Introduction to Organic Chemistry
- Structural Formula
- Condensed Formula
- Skeletal Formula
- Spatial Orientation of Bonds
- Intro to Hydrocarbons
- Isomers
- Chirality
- Functional Groups in Chemistry
- Naming Alkanes
- The Alkyl Groups
- Naming Alkanes with Substituents
- Naming Cyclic Alkanes
- Naming Other Substituents
- Naming Alcohols
- Naming Alkenes
- Naming Alkynes
- Naming Ketones
- Naming Aldehydes
- Naming Carboxylic Acids
- Naming Esters
- Naming Ethers
- Naming Amines
- Naming Benzene
- Alkane Reactions
- Intro to Addition Reactions
- Halogenation Reactions
- Hydrogenation Reactions
- Hydrohalogenation Reactions
- Alcohol Reactions: Substitution Reactions
- Alcohol Reactions: Dehydration Reactions
- Intro to Redox Reactions
- Alcohol Reactions: Oxidation Reactions
- Aldehydes and Ketones Reactions
- Ester Reactions: Esterification
- Ester Reactions: Saponification
- Carboxylic Acid Reactions
- Amine Reactions
- Amide Formation
- Benzene Reactions
- 23. Chemistry of the Nonmetals
- Main Group Elements: Bonding Types
- Main Group Elements: Boiling & Melting Points
- Main Group Elements: Density
- Main Group Elements: Periodic Trends
- The Electron Configuration Review
- Periodic Table Charges Review
- Hydrogen Isotopes
- Hydrogen Compounds
- Production of Hydrogen
- Group 1A and 2A Reactions
- Boron Family Reactions
- Boron Family: Borane
- Borane Reactions
- Nitrogen Family Reactions
- Oxides, Peroxides, and Superoxides
- Oxide Reactions
- Peroxide and Superoxide Reactions
- Noble Gas Compounds
- 24. Transition Metals and Coordination Compounds
- Atomic Radius & Density of Transition Metals
- Electron Configurations of Transition Metals
- Electron Configurations of Transition Metals: Exceptions
- Paramagnetism and Diamagnetism
- Ligands
- Complex Ions
- Coordination Complexes
- Classification of Ligands
- Coordination Numbers & Geometry
- Naming Coordination Compounds
- Writing Formulas of Coordination Compounds
- Isomerism in Coordination Complexes
- Orientations of D Orbitals
- Intro to Crystal Field Theory
- Crystal Field Theory: Octahedral Complexes
- Crystal Field Theory: Tetrahedral Complexes
- Crystal Field Theory: Square Planar Complexes
- Crystal Field Theory Summary
- Magnetic Properties of Complex Ions
- Strong-Field vs Weak-Field Ligands
- Magnetic Properties of Complex Ions: Octahedral Complexes
- 1. The Chemical World
3. Chemical Reactions
Empirical Formula
Back3. Chemical Reactions
Empirical Formula
- Multiple ChoiceWhich pair of compounds has the same empirical formula?1views
- Multiple ChoiceHow many sulfur atoms are present in the empirical formula for sodium sulfate?
- Multiple ChoiceWhich of the following is the empirical formula for C_2H_6?
- Open QuestionWhich of the following statements about empirical formulas is incorrect?
- Open Question
Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass.
- Multiple ChoiceWhich of the following is NOT an empirical formula?
- Multiple ChoiceWhat is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass?
- Open Question
In [Cu(NH3)4]2+, the subscript 4 indicates which of the following?
- Open Question
What is the empirical formula for Hg2(NO3)2?
- Open Question
What is the empirical formula for a compound if a sample contains 1.0 g of S and 1.5 g of O?
- Open Question
Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
2views - Multiple ChoiceA compound is found to be 30.45% nitrogen (N) and 69.55% oxygen (O) by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the empirical formula of the compound?1views
- Open Question
The lowest whole-number ratio of the elements in a compound is called the
- Open QuestionWhat is the empirical formula of a compound composed of