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Questions and Answers
Forces exist whether a substance is polar or nonpolar.
Forces exist whether a substance is polar or nonpolar.
London
Because carbon monoxide is a polar molecule, forces exist between their molecules.
Because carbon monoxide is a polar molecule, forces exist between their molecules.
dipole-dipole
Which of the following options include only intermolecular forces?
Which of the following options include only intermolecular forces?
- Intramolecular and Hydrogen Bond
- London Force and Intramolecular
- Ion-Dipole and Intramolecular
- London Force and Dipole-Dipole (correct)
What type of intermolecular force will $NaF (aq)$ exhibit?
What type of intermolecular force will $NaF (aq)$ exhibit?
Because carbon dioxide is a nonpolar molecule, _____ forces exist between their molecules.
Because carbon dioxide is a nonpolar molecule, _____ forces exist between their molecules.
Forces are attractive forces that exist within a molecule of a compound.
Forces are attractive forces that exist within a molecule of a compound.
The phase change of solid naphthalene turning into gas is called ______.
The phase change of solid naphthalene turning into gas is called ______.
A ______ is defined as a point of temperature and pressure where all common states of matter intersect or coexist.
A ______ is defined as a point of temperature and pressure where all common states of matter intersect or coexist.
_______ is the minimum energy required for a reaction to occur.
_______ is the minimum energy required for a reaction to occur.
The overall reaction order of $r = k[A][B][C]$ is _______.
The overall reaction order of $r = k[A][B][C]$ is _______.
Atmospheric pressure is a colligative property.
Atmospheric pressure is a colligative property.
Collision Theory states that reactions occur if particles collide with proper energy and orientation.
Collision Theory states that reactions occur if particles collide with proper energy and orientation.
A catalyst increases the activation energy of a reaction.
A catalyst increases the activation energy of a reaction.
Above the critical temperature, you can still apply pressure to condense a gas back into liquid.
Above the critical temperature, you can still apply pressure to condense a gas back into liquid.
In a saturated solution, you cannot dissolve anymore solid solute.
In a saturated solution, you cannot dissolve anymore solid solute.
At equilibrium, the rates of forward and reverse reactions are always equal.
At equilibrium, the rates of forward and reverse reactions are always equal.
Endothermic phase changes that absorb energy include melting, evaporation, and sublimation.
Endothermic phase changes that absorb energy include melting, evaporation, and sublimation.
If temperature increases, the average kinetic energy, on the other hand, decreases.
If temperature increases, the average kinetic energy, on the other hand, decreases.
Pressure does not affect the equilibrium of reactions involving solid reactants and products.
Pressure does not affect the equilibrium of reactions involving solid reactants and products.
Ions and water molecules attract together in a force called ion-dipole interaction.
Ions and water molecules attract together in a force called ion-dipole interaction.
On the provided phase diagram, at which point do all three states of the substance coexist?
On the provided phase diagram, at which point do all three states of the substance coexist?
On the provided phase diagram, what are the phases of the substance at point C?
On the provided phase diagram, what are the phases of the substance at point C?
On the provided phase diagram, what is the phase of the substance at 1 atm and 80°C?
On the provided phase diagram, what is the phase of the substance at 1 atm and 80°C?
Analyze the statements according to the criteria below:
X: As a liquid becomes a gas, its particles move slower.
Y: The particles move slower during evaporation because the phase change is exothermic.
Analyze the statements according to the criteria below: X: As a liquid becomes a gas, its particles move slower. Y: The particles move slower during evaporation because the phase change is exothermic.
When you grind solid materials into powder, you are increasing the ________ to speed up the reaction.
When you grind solid materials into powder, you are increasing the ________ to speed up the reaction.
The reaction A ⇌ B is in equilibrium if ________.
The reaction A ⇌ B is in equilibrium if ________.
Which phase transitions can increase the molecular order?
Which phase transitions can increase the molecular order?
During melting or evaporation, the particles behave in which of the following ways?
During melting or evaporation, the particles behave in which of the following ways?
Calculate the percent by mass of a potassium (KI) iodide solution containing 38 grams of KI and 100 grams of water.
Calculate the percent by mass of a potassium (KI) iodide solution containing 38 grams of KI and 100 grams of water.
Determine the freezing point of a 3.6-m magnesium fluoride ($MgF_2$) solution. (Kf = 1.86°C/m) Round to the nearest tenth.
Determine the freezing point of a 3.6-m magnesium fluoride ($MgF_2$) solution. (Kf = 1.86°C/m) Round to the nearest tenth.
Which of the following would be observed if an endothermic reaction is increased in temperature?
Which of the following would be observed if an endothermic reaction is increased in temperature?
Which of the processes can be increased by putting an enzyme into the reaction.
Which of the processes can be increased by putting an enzyme into the reaction.
Which of the following solutions would have the highest boiling point?
Which of the following solutions would have the highest boiling point?
Which of the following statement relates to the theory that explains the effect of changing concentration of a substance in equilibrium?
Which of the following statement relates to the theory that explains the effect of changing concentration of a substance in equilibrium?
Match the following terms with their descriptions:
Match the following terms with their descriptions:
When a reaction has reached equilibrium, which of the following will be true?
When a reaction has reached equilibrium, which of the following will be true?
What is the effect of adding an inert gas to a reaction at equilibrium?
What is the effect of adding an inert gas to a reaction at equilibrium?
Increasing the pressure in a reaction will favor product formation.
Increasing the pressure in a reaction will favor product formation.
Which of the following is the term for the amount of substance that can disolve in an given amount of solvent?
Which of the following is the term for the amount of substance that can disolve in an given amount of solvent?
Flashcards
London Force
London Force
A weak attractive force that exists between all molecules, whether polar or nonpolar.
Ion-dipole force
Ion-dipole force
An intermolecular attraction between a polar molecule and an ion.
Dipole-dipole forces
Dipole-dipole forces
Attractive forces between polar molecules where the positive end of one molecule is attracted to the negative end of another.
Sublimation
Sublimation
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Triple Point
Triple Point
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Activation Energy
Activation Energy
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Reaction Order
Reaction Order
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Collision Theory
Collision Theory
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Catalyst's effect
Catalyst's effect
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Chemical Equilibrium
Chemical Equilibrium
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Endothermic phase changes
Endothermic phase changes
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Ion-dipole Interaction
Ion-dipole Interaction
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Liquid to gas
Liquid to gas
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Grinding solids
Grinding solids
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Equilibrium Condition
Equilibrium Condition
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Solid to liquid transition
Solid to liquid transition
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During melting or evaporation
During melting or evaporation
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Study Notes
General Chemistry Final Review
- The review covers STEM Grade 11/12 General Chemistry 1, S.Y. 2024-2025
Key Concepts to Review
- Attractive Forces: Focus on intermolecular forces, phase changes, and phase diagrams.
- Solutions: Includes types of solutions (unsaturated, saturated, supersaturated), percent by mass calculation, boiling point elevation, and freezing point depression.
- Chemical Kinetics: Includes factors affecting reaction rates and collision theory, and the orders of reactions.
- Chemical Equilibrium: Includes the definition of chemical equilibrium and Le Chatelier's Principle.
Exam Reminders
- You should bring ballpens and scientific calculators only
- Periodic tables and scratch papers are NOT allowed
- Cellphones are strictly prohibited during the exam.
- You should strictly follow time allotted for the exam.
- Erasures on the exam paper are prohibited.
Attractive Forces Identification
- London Force: Exists regardless of a substance's polarity (polar or nonpolar).
- Dipole-Dipole Forces: Exist between polar molecules, for example, carbon monoxide.
- Intermolecular Forces: London force, Dipole-dipole, Ion-dipole and Hydrogen bond.
- Ion-Dipole Force: The intermolecular force that NaF (aq) exhibits.
- Intramolecular Force: It is the the attractive force within a molecule of a compound.
Phase Changes
- Sublimation: The phase transition of solid naphthalene turning into gas.
- Triple Point: This is where all common states of matter coexist.
- Activation Energy: Energy is required for a reaction to occur.
- Third Order: This is the overall reaction order of r = k[A][B][C].
True or False Questions
- FALSE Atmospheric pressure is colligative property.
- TRUE Collision Theory indicates reactions require particles colliding with proper energy and orientation.
- FALSE A catalyst increases the activation energy of a reaction.
- FALSE Above the critical temperature, pressure cannot condense gas into a liquid.
- TRUE Saturated solutions cannot dissolve more solid solute.
- TRUE Equilibrium is achieved when forward and reverse reaction rates are equal.
- TRUE Melting, evaporation, and sublimation are endothermic phase changes.
- FALSE Increasing temperature decreases average kinetic energy.
- TRUE Pressure does not affect the the equilibrium of reactions involving solid reactants and products.
- TRUE Ion-dipole interaction is the attraction between ions and water molecules.
Analyzing Phase Diagrams
- On a phase diagram, all states coexist at the Triple Point.
- Point C on the phase diagram represents the Liquid and Gas phases.
- At 1 atm and 80°C, the substance is in the Liquid phase.
Multiple choice questions
- Both statements are false:
- X: As a liquid becomes a gas, particles move slower
- Y: The particles move slower during evaporation because the phase change is exothermic
- To speed up reaction rates when grinding solid materials increases the surface area
- The reaction A ⇌ B equilibrium is reached when conversion rate of A to B equals that of B to A
- Molecular order decreases during solid to liquid transitions
- During melting/evaporation, the molecules become more organized.
Problem Solving
- Percent by mass (% m/m) of a solution is calculated using the formula: (Mass of solute / (Mass of solute + Mass of solvent)) × 100
- The percent by mass of a potassium iodide solution containing 38g KI in 100g water is 82.46%
- Freezing point depression is calculated using ΔTf = iKf m and Tf solution = FP of water - ΔTf
- The freezing point of a 3.6 m magnesium fluoride solution is -20.09°C.
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