Chemistry Chapter 1 Quiz

Accuracy and Precision

• Accuracy is how close a measurement is to the true value.
• Precision is how close several measurements are to each other.

Atomic Theory

• All matter is made of small particles called atoms.
• Atoms cannot be destroyed or created.

Intensive and Extensive Properties

• Intensive properties are independent of the amount of a substance (e.g., density, boiling point).
• Extensive properties depend on the amount of a substance (e.g., mass, energy).

Avogadro's Number

• 6.022 x 10²³ atoms

Ionic Bonding and Lattice Energy

• Lattice energy is the energy required to separate one mole of an ionic compound into its gaseous ions.
• Lattice energy increases with increasing charge of ions and decreases with increasing size of ions.
• Coulomb's law describes the force between charged particles.

Covalent Bonding and Lewis Structures

• Lewis structures show all valence electrons of atoms in a molecule.
• Example: H₂O and PCl₃ have been demonstrated through an illustrative example of Lewis structures
• Examples: H2O, and PC13.

Formal Charge

• Calculates the difference between the valence electrons of an isolated atom and the number of electrons assigned to that atom in a molecule.

Bond Strength, Bond Length, and Bond Enthalpy

• Bond strength is related to the number of bonds, and bond length between two atoms.
• Bond enthalpy is the energy required to break a bond between two atoms.

Bond Order and Resonance Structures

• Bond order is related to bond strength and bond length
• Resonance structures are multiple Lewis structures to represent a molecule.

Polarity

• Units for measuring length, including meters, centimeters, millimeters, nanometers, and angstroms (Å). Values and conversions for these units are included.

Electromagnetic Radiation

• Energy (E) = hν, where h is Planck's constant and ν is frequency.
• The speed of light (c) = νλ, where ν is frequency and λ is wavelength.
• Planck's constant = 6.626 x 10^-34 Js.
• Speed of light = 3.00 x 10⁸ m/s

Bohr Model

• Electrons orbit the nucleus in quantized energy levels (n).
• Energy levels are quantized for electrons.
• Energy levels are quantized, which means they can only have specific values.

Quantum Mechanics

• Wave function (Ψ): describes the probability of finding an electron in a particular region of space.
• Four quantum numbers describe the properties of an electron. Orbital shape depends on quantum numbers n & l.

Quantum Numbers for Orbitals

• Principle Quantum Number (n): energy level
• Angular momentum Quantum number (l): shape of orbital (0: s, 1: p, 2: d, 3:f)
• Magnetic Quantum Number (ml): orientation of the orbital in space. (-L to +L)

Aufbau Principle

• Electrons fill the lowest energy orbitals first.

Hund's Rule

• Electrons fill degenerate orbitals individually before pairing up.

Atomic Radius and Ionic Radius

• Atomic radius increases down a group.
• Ionic radius: cations (positive charge) are smaller than their parent atoms. Anions (negative charge) are larger. Both get smaller as you move across a period.

Ionization Energy

• Energy needed to remove an electron from an atom. It increases going from left to right across a period and decreases going down a group.

VSEPR Theory

• Valence Shell Electron Pair Repulsion theory determines molecular shape based on electron domain geometry.

Types of Reactions

• Combination reactions: Two or more reactants combine to form one product.
• Decomposition reactions: One reactant breaks down into two or more products.
• Combustion reactions: A substance reacts rapidly with oxygen, producing heat and light.

Gas Laws

• Boyle's Law: Pressure and volume are inversely proportional at constant temperature.
• Charles's Law: Volume and temperature are directly proportional at constant pressure.
• Avogadro's Law: Volume and number of moles are directly proportional at constant temperature and pressure.
• Ideal Gas Law: PV = nRT. where P is pressure, V is volume, n is number of moles, R is the ideal gas constant. and T is the temperature.
• Van der Waals equation: modifies the Ideal Gas law to account for intermolecular forces and size of gas particles

Intermolecular Forces

• London dispersion forces
• Dipole-dipole interactions
• Hydrogen bonds
• Ion-dipole interactions
• Polarity of molecules and relationship between intermolecular forces, weight and molecular shapes.

Liquids and Solids

• Liquid properties: viscosity, surface tension, and vapor pressure.
• Crystalline solids: have regular arrangements of particles, while amorphous solids do not.
• Types of crystalline solids are demonstrated, including primitive cubic, body-centered cubic, and face-centered cubic.

Types of Solids

• Metallic solids: consist of metal atoms in a close-packed arrangement.
• Ionic solids: have positively and negatively charged ions.
• Molecular solids: are composed of molecules held together by intermolecular forces.
• Covalent network solids: have atoms interconnected by covalent bonds.

Polymers

• Polymers are large molecules consisting of repeating units. Addition and condensation polymers are presented

Nanomaterials

• Nanomaterials are materials with one or more dimensions are in the nanometer range.
  • Examples demonstrated include Carbon Nanomaterials such as Fullerenes, nanotubes, and graphene

Thermodynamics

• Energy is the capacity to do work or transfer heat.
  • Kinetic energy is associated with motion.
  • Potential energy is associated with position or chemical composition.
  • Electrostatic potential energy is the energy associated with interactions between charged particles
• Thermochemistry: The study of heat changes accompanying chemical reactions and physical changes
• Internal energy (E): is the sum of all energy in a system.
• State function: property of a system that depends only on the present state of the system and not the path taken to reach that state.

Enthalpy, Hess's Law, and Standard Enthalpies of Formation

• Enthalpy (H): a thermodynamic property that is defined as the sum of the internal energy of the system and the product of its pressure and volume.
• Hess's Law: Enthalpy change of a reaction is the same whether the reaction takes place in one or multiple steps.
• Standard enthalpies of formation are the enthalpy changes when one mole of a substance is formed from its constituent elements under standard conditions.

Spontaneous Processes and Entropy

• Spontaneous processes occur without external intervention
• Entropy (S): a measure of disorder or randomness in a system, for spontaneous processes increasing enthalpy will tend to spread energy out to increase entropy.
• Standard molar entropies (S°) are the values of entropy for one mole of a substance in its standard state

Chemical Equilibrium, Equilibrium Constants

• Chemical equilibrium is a dynamic state where rates of forward and backward reactions are equal, and concentrations of reactants and products remain constant.
• Equilibrium constant (Keq/Kc): the ratio of product concentrations to reactant concentrations at a given temperature. The equilibrium constant Kp is the same ratio under conditions of equilibrium, but the ratio is based on partial pressures.

Heterogeneous Equilibrium

• Heterogeneous equilibrium involves reactants and products in different phases (solid, liquid, gas)

Acids and Bases

• Conjugate acid-base pairs differ in the presence or absence of a proton.
• Strong acids completely dissociate in aqueous solutions, compared to weak acids that only partially dissociate.
• Strong bases are ionic hydroxides of alkali metals.
• Weak bases only partially dissociate.
• Acid-base strength is related to the equilibrium constant for the acid or base dissociation.

Autoionization of Water

• Water undergoes self-ionization (autoprotolysis) to form hydronium (H₃O⁺) and hydroxide (OH^-) ions.

Electrochemistry

• Electrochemistry is the study of the interchange of chemical and electrical energy.
• Oxidation is the loss of electrons, while reduction is the gain of electrons
• Galvanic cells involve spontaneous redox reactions to produce an electrical current in a battery
• Electrolysis involves nonspontaneous reactions to use electrical current to decompose electrolytes.
• Electroplating uses electrolysis to deposit an ionic layer on an object.
• Cell diagrams and standard hydrogen electrode (SHE) in terms of oxidation and reduction and electrochemical reactions are represented.

Test your knowledge on fundamental concepts of chemistry, including accuracy and precision, atomic theory, and various properties of substances. Explore key ideas such as ionic bonding, lattice energy, and covalent bonding through Lewis structures. This quiz is essential for anyone studying introductory chemistry.