Chemistry Class 11 - Reaction Types and Stoichiometry

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Questions and Answers

What does 1 nutritional calorie equal in kilojoules?

  • 4.18 kJ (correct)
  • 2.68 kJ
  • 7.2 kJ
  • 3.84 kJ

Which principle explains that energy cannot be created or destroyed?

  • Hess's law
  • First law of thermodynamics (correct)
  • Pauli exclusion principle
  • Heisenberg uncertainty principle

What is the term for the energy required to break one mole of bonds in a gaseous state?

  • Internal energy change
  • Standard enthalpy of combustion
  • Standard enthalpy of formation
  • Bond dissociation energy (correct)

In the Rydberg equation, which variable represents the Rydberg constant?

<p>R_H (A)</p> Signup and view all the answers

What does the principal quantum number (n) indicate in quantum mechanics?

<p>Energy level of an electron (A)</p> Signup and view all the answers

Which quantum number describes the shape of an electron's orbital?

<p>Angular momentum quantum number (l) (A)</p> Signup and view all the answers

What phenomenon does the photoelectric effect demonstrate?

<p>Particle nature of light (A)</p> Signup and view all the answers

Which principle states that no two electrons in an atom can have the same set of quantum numbers?

<p>Pauli exclusion principle (B)</p> Signup and view all the answers

Which of the following statements about redox reactions is true?

<p>Combustion reactions can be recognized as redox reactions. (D)</p> Signup and view all the answers

What determines the theoretical yield in a chemical reaction?

<p>The limiting reactant. (C)</p> Signup and view all the answers

Which equation correctly represents the relationship between heat, specific heat, mass, and change in temperature?

<p>q = c × m × ∆T (D)</p> Signup and view all the answers

In calorimetry, what does it mean when a reaction is described as exothermic?

<p>It releases heat to the surroundings. (B)</p> Signup and view all the answers

To convert Celsius to Kelvin, which operation should be performed?

<p>Add 273.15 to the Celsius temperature. (A)</p> Signup and view all the answers

What is the specific heat of a substance?

<p>The amount of heat required to raise the temperature of one gram by 1°C. (A)</p> Signup and view all the answers

Which process is characterized by the equation qreaction = −qsolution?

<p>The conservation of energy during a chemical reaction. (B)</p> Signup and view all the answers

Which of the following best describes gravimetric analysis?

<p>A method for determining the concentration of a solute based on mass. (B)</p> Signup and view all the answers

Which of the following accurately describes the difference between cations and anions?

<p>Cations are atoms that lose electrons, while anions are atoms that gain electrons. (D)</p> Signup and view all the answers

What is true regarding the octet rule?

<p>Not all elements follow the octet rule, particularly electron deficient species. (B)</p> Signup and view all the answers

Which of the following trends do ionization energy and electron affinity share?

<p>Both are affected by effective nuclear charge. (C)</p> Signup and view all the answers

What does it mean for ionic compounds to have isotropic attractive forces?

<p>The attractive forces are equal in all three-dimensional directions. (A)</p> Signup and view all the answers

Which statement correctly describes a polar covalent bond?

<p>One atom has a higher electronegativity, resulting in unequal sharing of electrons. (D)</p> Signup and view all the answers

When distinguishing between single, double, and triple bonds, which factor directly affects bond length?

<p>The number of bonding pairs of electrons. (B)</p> Signup and view all the answers

In the context of resonance structures, which statement is accurate?

<p>A resonance hybrid represents the average of all possible resonance structures. (D)</p> Signup and view all the answers

Which of the following is true about isoelectronic species?

<p>They possess identical electron configurations. (B)</p> Signup and view all the answers

Flashcards

Redox Reaction

A chemical reaction involving the transfer of electrons between reactants, resulting in changes in oxidation states.

Oxidation

Loss of electrons and increase in oxidation state.

Reduction

Gain of electrons and decrease in oxidation state.

Oxidizing Agent

Substance that causes oxidation in another substance.

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Reducing Agent

Substance that causes reduction in another substance.

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Limiting Reactant

The reactant that is completely consumed in a chemical reaction, thus limiting the amount of product that can be formed.

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Theoretical Yield

The maximum amount of product that can be produced from a given amount of reactants in a chemical reaction.

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Percent Yield

The percentage of the theoretical yield that is actually obtained in a chemical reaction.

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Titration

A technique used to determine the concentration of a solution by reacting it with a solution of known concentration.

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Gravimetric Analysis

A technique for determining the amount of a substance by measuring its mass.

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Kinetic Energy

Energy of motion.

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Potential Energy

Stored energy.

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Calorimetry

Used to measure heat transfer in experiments.

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Endothermic Process

Process that absorbs heat from the surroundings.

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Exothermic Process

Process that releases heat to the surroundings.

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Nutritional Calorie

A unit of energy equal to 1 kilocalorie (kcal).

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First Law of Thermodynamics

Energy cannot be created or destroyed, only transferred or changed from one form to another.

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Internal Energy

The total energy of the particles within a system.

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Expansion Work

Work done by a system as it expands against an external pressure.

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State Function

A property that depends only on the current state of a system, not the path taken to reach that state.

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Enthalpy (H)

A thermodynamic property that is the sum of the internal energy and the product of pressure and volume.

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Enthalpy Change (ΔH)

The change in enthalpy during a process.

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Standard State Conditions

Specific conditions used as a reference point, commonly 25°C (298 K) and 1 atm pressure.

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Standard Enthalpy of Combustion (ΔH°c)

The enthalpy change when one mole of a substance is completely burned in oxygen under standard state conditions.

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Standard Enthalpy of Formation (ΔH°f)

The enthalpy change when one mole of a substance is formed from its elements in their standard states under standard state conditions.

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Hess's Law

The overall enthalpy change for a reaction is independent of the pathway.

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Wavelength

The distance between corresponding points on two consecutive waves.

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Frequency

The number of waves that pass a given point per unit of time.

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Electromagnetic Spectrum

The range of all possible frequencies of electromagnetic radiation.

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Constructive Interference

When two waves combine to form a wave with a larger amplitude.

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Destructive Interference

When two waves combine to form a wave with a smaller amplitude or no wave at all.

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Quantum Numbers

Set of numerical values that specify the properties of atomic orbitals and the electrons in them.

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Orbital Diagrams

Visual representations of electron locations and spin within individual orbitals in an atom.

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Main group elements

Elements in the s and p blocks of the periodic table.

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Transition elements

Elements in the d block of the periodic table.

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Inner transition elements

Elements in the f block of the periodic table.

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Covalent radius

Half the distance between the nuclei of two identical atoms bonded covalently.

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Effective nuclear charge

The net positive charge experienced by a valence electron.

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Ionic radii

The size of an ion.

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Ionization energy

The energy required to remove an electron from a gaseous atom or ion.

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Electron affinity

The energy change that occurs when an electron is added to a gaseous atom or ion.

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Metallic character

The tendency of an element to lose electrons and form positive ions.

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Isoelectronic species

Species with the same number of electrons.

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Cations

Positively charged ions.

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Anions

Negatively charged ions.

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Binary ionic compounds

Compounds containing a metal cation and a nonmetal anion.

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Isotropic

Having the same properties in all directions.

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Inert pair effect

The tendency of heavier elements to not lose their valence s electrons.

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Covalent bonds

Chemical bonds formed by sharing electrons between atoms.

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Polar covalent bonds

Covalent bonds where electrons are shared unequally.

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Pure covalent bonds

Covalent bonds where electrons are shared equally.

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Lewis symbols

Representations of atoms showing valence electrons as dots around the atom symbol.

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Octet rule

The tendency of atoms to gain, lose, or share electrons to achieve a full outer electron shell (8 electrons).

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Single bonds

A covalent bond formed by sharing one pair of electrons.

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Double bonds

A covalent bond formed by sharing two pairs of electrons.

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Triple bonds

A covalent bond formed by sharing three pairs of electrons.

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Lewis structures

Visual representations of molecules showing the arrangement of atoms and bonds.

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Exceptions to the Octet Rule

Some molecules do not follow the octet rule.

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Formal charge

A way to assess the distribution of electrons in a Lewis structure.

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Resonance

Multiple valid Lewis structures for a molecule.

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Study Notes

Section 4.2 Classifying Chemical Reactions

  • Determine if a redox reaction occurred
    • Assign oxidation states
    • Identify oxidized species
    • Identify reduced species
    • Identify oxidizing agent
    • Identify reducing agent
  • Balance redox reactions in acidic and basic conditions
  • Recognize decomposition, combination, single displacement, and combustion reactions as redox reactions

Section 4.3 Reaction Stoichiometry

  • Use stoichiometric coefficients to determine moles of reactants needed for a reaction
  • Relate masses of reactants to masses of products
  • Relate masses of reactants to each other

Section 4.4 Reaction Yields

  • Identify the limiting reactant
  • Theoretical yield is determined by limiting reactant
  • Calculate percent yield

Section 4.5 Quantitative Chemical Analysis

  • Explain techniques like titration, gravimetric analysis, and combustion analysis
  • Determine solution concentration from titration data
  • Determine solute concentration from gravimetric analysis data
  • Determine empirical formulas from combustion analysis data

Chapter 5 Thermochemistry

Section 5.1 Energy Basics

  • Define kinetic, potential, and thermal energy
  • Convert between temperature scales (Celsius, Fahrenheit, Kelvin)
  • Be familiar with energy units (calorie, joule)
  • Distinguish between heat capacity, specific heat, and molar heat capacity
  • Determine heat from q = mc(ΔT)

Section 5.2 Calorimetry

  • Explain how calorimetry is used to measure heat transfer
  • Distinguish between endothermic and exothermic processes
  • Explain how a bomb calorimeter is used
  • Convert Calories to kcal

Section 5.3 Enthalpy

  • State the first law of thermodynamics
  • Explain and apply concepts like internal energy, expansion work, state functions, enthalpy (H), enthalpy change (ΔH), standard state conditions, standard enthalpy of combustion (ΔH°c), and standard enthalpy of formation (ΔH°f)
  • Write and manipulate thermochemical equations
  • Calculate enthalpy of combustion
  • Determine heat of reaction from standard enthalpies of formation

Section 6.1 Electromagnetic Energy

  • Convert between wavelength and frequency
  • Understand relationships between energy, wavelength, and frequency
  • Know the regions of the electromagnetic spectrum
  • Recognize constructive and destructive interference
  • Distinguish between continuous and line spectra

Section 6.2 The Bohr Model

  • Describe the Bohr model of the atom
  • Distinguish between ground and excited states of an electron
  • Use the Rydberg equation to calculate energy of transitions

Section 6.3 Development of Quantum Theory

  • Relate wave-particle duality of light to electrons
  • Understand and apply quantum numbers (principal, angular momentum, magnetic, spin)

Section 6.4 Electronic Structure of Atoms

  • Write electron configurations for atoms and ions
  • Apply orbital diagrams for atoms and ions
  • Understand deBroglie wavelength, Heisenberg uncertainty principle, Pauli exclusion principle, Aufbau principle, Hund's rule
  • Distinguish between valence and core electrons
  • Identify main group, transition, and inner transition elements

Section 6.5 Periodic Variations in Element Properties

  • Describe, explain, and apply periodic trends in covalent radius, effective nuclear charge, ionic radii, ionization energy, electron affinity, and metallic character
  • Recognize isoelectronic species

Chapter 7 Chemical Bonding and Molecular Geometry

Section 7.1 Ionic Bonding

  • Distinguish between cations, anions, atoms, and molecules
  • Explain how cations and anions form
  • Identify properties of ionic compounds
  • Compare properties of ions and atoms
  • Identify binary ionic compounds
  • Explain the formula of an ionic compound
  • Explain the inert pair effect

Section 7.2 Covalent Bonding

  • Explain how covalent bonds differ from ionic bonds
  • Compare properties of molecular and ionic compounds
  • Explain how covalent bonds form
  • Recognize factors affecting bond length
  • Distinguish between polar and pure covalent bonds
  • Differentiate between electronegativity, effective nuclear charge, electron affinity
  • Recognize polyatomic ions as charged molecules

Section 7.3 Lewis Symbols and Structures

  • Write Lewis symbols from valence shell electron configurations
  • Show formation of ions with Lewis symbols
  • Distinguish between lone pair and bonding electrons
  • Explain the octet rule
  • Distinguish between single, double, and triple bonds
  • Draw Lewis structures
  • Recognize exceptions to the octet rule (electron-deficient and hypervalent species)

Section 7.4 Formal Charge and Resonance

  • Assign formal charge to atoms in molecules
  • Use formal charge to determine best Lewis structures
  • Explain resonance
  • Explain how resonance structures differ from isomers
  • Explain resonance hybrid

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