General Chemistry Basics Quiz

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Questions and Answers

Which of the following characteristics is NOT associated with a molecular lattice?

Sublimation is common

Low melting point

Conducts electricity (correct)

Soluble in polar solvents

What type of bond primarily holds the atoms in an atomic lattice together?

Hydrogen bonds

Covalent bonds (correct)

Ionic bonds

Metallic bonds

Which of the following is an example of an ionic lattice?

NaCl (correct)

SiO2

C (diamond)

Which statement about metallic lattices is true?

They have high melting points Signup and view all the answers

Which state of matter has a disordered structure and high compressibility?

Gas Signup and view all the answers

In a phase diagram for water, what does the area labeled as solid represent?

Molecules tightly packed in a crystalline structure Signup and view all the answers

Which statement accurately describes the melting point of ionic compounds?

They typically have high melting points Signup and view all the answers

What type of interaction occurs between molecules in a molecular lattice?

Secondary forces such as van der Waals forces Signup and view all the answers

What occurs at the cathode during electrolysis?

Reduction takes place Signup and view all the answers

What does Faraday's first law state about the mass of electrolyzed material?

It is proportional to the charge used Signup and view all the answers

Which compound can act both as an acid and a base according to Bronsted theory?

Water Signup and view all the answers

What is the definition of sublimation?

A phase transition where solid becomes directly vapor. Signup and view all the answers

How is the strength of an acid characterized?

By its dissociation equilibrium constant, K a Signup and view all the answers

According to Arrhenius's law, what does the rate constant (k) depend on?

Pre-exponential factor and temperature Signup and view all the answers

What is the definition of heat of formation?

The reaction heat for one mole of substance from its elements Signup and view all the answers

Which statement correctly defines the order of a reaction?

It is the sum of the exponentiations of the concentrations Signup and view all the answers

How is sublimation heat compared to heat of evaporation?

Sublimation heat is larger than heat of evaporation. Signup and view all the answers

What does partial pressure refer to?

The pressure of a gas as if it was alone in the volume. Signup and view all the answers

What function do catalysts perform in a reaction?

They lower the reaction barrier Signup and view all the answers

According to Hess's Law, how is the total standard reaction heat determined?

It is the sum of heats of formation from all steps Signup and view all the answers

How is a covalent bond formed?

By the sharing of a single electron pair between two atoms Signup and view all the answers

What do acid-base indicators usually consist of?

Weak acids with distinct colors Signup and view all the answers

What is the statement of Dalton's law?

The pressure of a gas mixture is the sum of the component's partial pressures. Signup and view all the answers

What happens to the equilibrium of an exothermic reaction when the temperature is reduced?

The equilibrium constant increases Signup and view all the answers

What is vapor pressure?

The pressure of a vapor above a liquid in equilibrium. Signup and view all the answers

What is a characteristic of an ionic bond?

It results from the attraction between oppositely charged ions Signup and view all the answers

What defines a dative covalent bond?

It involves a lone pair donating to an empty orbital Signup and view all the answers

What is the relationship defined by Amagat's rule?

The volume of a gas mixture is the sum of the component's partial volumes. Signup and view all the answers

Which of the following statements best describes a suspension?

Solid dispersed in liquid Signup and view all the answers

What is the sign convention for reaction heat in an endothermic reaction?

Positive Signup and view all the answers

What describes vapor?

A gas phase substance below the critical temperature. Signup and view all the answers

What describes critical temperature?

The highest temperature at which a substance can exist as a liquid. Signup and view all the answers

What does atomic weight represent?

The number of protons and neutrons in the nucleus Signup and view all the answers

Which of the following elements is part of group 2 of the periodic table?

Mg Signup and view all the answers

What is ionization energy defined as?

Energy needed to remove an electron from an atom or molecule Signup and view all the answers

What is the geometry associated with sp3d hybridization?

Trigonal bipyramid Signup and view all the answers

According to the VSEPR theory, what determines the geometry of a molecule?

The repulsion of valence electron pairs Signup and view all the answers

What does Hund's rule state regarding the occupation of degenerate orbitals?

Each degenerate orbital must have one electron before any orbital has two Signup and view all the answers

Which group contains the element Xenon?

Group 18 Signup and view all the answers

According to the Pauli exclusion principle, what is true about electrons in an atomic system?

Two electrons in the same orbital must have opposite spins Signup and view all the answers

What does osmotic pressure depend on?

The molar concentration and the temperature Signup and view all the answers

How is an isotonic solution defined?

A solution that has an osmotic pressure equal to that in the cell Signup and view all the answers

In a binary, non-azeotropic mixture, how does the concentration of the more volatile component in the vapor compare to the liquid?

It is larger in the vapor than in the liquid Signup and view all the answers

What occurs at the boiling temperature of a liquid?

The vapor pressure equals the outer pressure Signup and view all the answers

Is it possible to experience boiling point depression?

Yes, if a more volatile compound is added Signup and view all the answers

What characterizes the azeotropic composition of a mixture?

The liquid and vapor phases have the same composition Signup and view all the answers

According to Arrhenius, what defines an acid?

A substance that releases H+ in a watery solution Signup and view all the answers

According to Bronsted theory, what is a characteristic of a base?

It accepts H+ ions from acids Signup and view all the answers

Study Notes

General Chemistry Exam Summary

The exam contains "basic questions" covering fundamental chemical concepts.
Concise answers are provided for each question.
Students must answer 5 questions from the list in test format, selecting the correct answer.
Some questions may involve simple calculations, the numerical values might vary.
The material summarizes crucial "basic" knowledge for the General Chemistry exam.
80% efficiency is expected for answering the questions.

Molecular Lattice Characterization

Lattice points are occupied by molecules (atoms or isolated molecules).
Held together by secondary forces (Hydrogen bonding, dispersion forces, van der Waals interactions).

Atomic Lattice Characterization

Lattice points are occupied by atoms bound by strong covalent bonds.
Examples include diamond (C), silica (SiO2), red phosphorus (P), silicon (Si), germanium (Ge), and gray/metallic tellurium (Te).
Usually characterized by high melting points, high hardness, and are insoluble in most solvents.
Do not conduct electricity
Often sublimable.

Ionic Lattice Characterization

Lattice points are occupied by ions, bound by ionic bonds.
Examples include sodium chloride (NaCl), potassium chloride (KCl), magnesium sulfate (MgSO4), potassium fluoride (KF), and lithium bromide (LiBr).
Usually have medium to high melting points.
Soluble in polar solvents.
Non-conductive as solids but conductive in molten form.

Metallic Lattice Characterization

Lattice points are occupied by cations bound by a delocalized cloud of electrons.
Examples include sodium (Na), potassium (K), magnesium (Mg), aluminum (Al), iron (Fe), tungsten (W), copper (Cu), silver (Ag), and gold (Au).
Melting points vary widely.
Physically insoluble (but alloy formation is possible).
Conduct electricity.

States of Matter Characterization

Properties like free path, rotation, vibration, and compressibility differ between solid, liquid, and gas states.
Solids have a small or negligible free path, low compressibility, fixed rotation and vibration modes, and ordered structure.
Liquids have a larger free path than solids, minor compressibility, and disordered structure.
Gases have a large free path, high compressibility, rapid rotation and vibration modes, and disordered structure.

Phase Transitions and Diagrams

Specific details of phase transitions(like sublimation)
Important points(like the triple point) on the phase diagram are shown.
Phase equilibrium curves(such as sublimation, melting, and vaporization).

Sublimation and Definitions

Sublimation is a phase transition from solid directly to gas, without forming a liquid phase.
Sublimation vapor pressure is the pressure of the vapor in equilibrium with the solid.
Sublimation heat is greater than the heat of evaporation (due to needing to overcome the heat of fusion).

Partial Pressure and Dalton's Law

Partial pressure is the hypothetical pressure a component in a gas mixture would exert if it were alone in the given volume and temperature.
Dalton's law states that the total pressure of a gas mixture is the sum of the partial pressures of its components.

Amagat's Rule

Amagat's rule: The total volume of a gas mixture is the sum of the partial volumes of its components.

Vapor Pressure Definition

Vapor pressure (or vapor tension) is the pressure of a vapor in equilibrium with its condensed phase (either solid or liquid) at a given temperature.

Vapour Definitions

Vapor is the gas phase below the critical temperature.
Can be condensed by increasing temperature or decreasing pressure.

Critical Temperature and Pressure

Critical temperature: Temperature above which a substance cannot be liquefied, regardless of pressure.
Critical pressure: Pressure required to liquefy a substance at its critical temperature.

Triple Point Definition

The triple point is a specific set of temperature and pressure where three phases of a substance (solid, liquid, and gas) are in equilibrium.

Avogadro's Rule

Different ideal gases at the same temperature and pressure contain the same number of molecules.

Temperature Dependence of Melting

Pure compounds maintain a constant temperature during melting.

Pressure Changes with Volume and Temperature

changes in pressure during the reduction of volume at constant temperature. This is dependent on if the gas is an ideal gas or not

Freezing Point Depression

The decrease in freezing point of a solvent when a solute is added. The depression is determined by the molar concentration of the solute.

Dilute Solution Definition

A dilute solution is one in which the laws of dilute solutions apply.

Molecular Mass Determination

Molar mass can be calculated using freezing point depression, provided the depression and other relevant values are known.

Boiling Point Elevation/Depression

Boiling point elevation/depression are related to the addition of a non-volatile solute to a solvent.
Boiling Point Elevation/depression is related to the vapor pressure of the solvent and solute.

Osmotic Pressure Dependence

Osmotic pressure depends on molar concentration and temperature.

Isotonic Solutions

An isotonic solution is one where the osmotic pressure of the solution is equal to the osmotic pressure inside cells.

Binary Mixture Vapor-Liquid Composition

The more volatile component has a higher concentration in the vapor phase than in the liquid phase.

Boiling Temperature/Point Definitions

Boiling temperature is reached when the vapor pressure of a liquid equals the external pressure.
Normal boiling point is the boiling temperature at standard atmospheric pressure.

Boiling Point Depression

If a non-volatile solute is added to the solvent, the boiling point will usually increase.

Azeotropic Composition

The azeotropic composition of a mixture is the concentration at which the liquid and vapor concentrations are equal (in equilibrium).

Dew Point Curve and Boiling Point Curve Definitions

Dew Point Curve: Vapor concentrations at a given temperature (vapor in equilibrium with liquid).
Boiling Point Curve: Liquid concentrations at a given temperature (liquid in equilibrium with vapor).

Acid-Base Definitions (Arrhenius, Bronsted, Lewis)

Arrhenius: Acids produce H⁺ ions, bases produce OH⁻ ions in water.
Bronsted-Lowry: Acids donate protons (H⁺), bases accept protons.
Lewis: Acids accept electron pairs, bases donate electron pairs.

Acid-Base Indicators

An acid-base indicator changes color over a particular pH range.

pH Concept

pH is calculated as the negative logarithm of the hydrogen-ion concentration ([H⁺]).
pH measures the acidity (or alkalinity) of a solution.

pH for NaOH Solution

pH is high for basic solutions like NaOH. For example, for a .01 mol/L solution of NaOH, the pH is approximately 12.

pH for HCl Solution

pH is low for acidic solutions like HCl. For example, for a .01 mol/L solution of HCl, the pH is approximately 2.

Buffer Capacity Definition

Buffer capacity is the amount of strong acid/base needed to change the pH of a buffer by one unit.

Buffer pH Calculation

Calculations to determine pH of specific buffer solutions when given necessary components.

Standard Hydrogen Electrode (SHE) Definition

A standard electrode used as a reference in electrochemistry, consisting of platinum electrode immersed in pH = 0 solution saturated with hydrogen gas at 1 atm.

Anode and Cathode

Anode: Oxidation takes place.
Cathode: Reduction takes place.

Electrolyte Definition

Electrolytes are substances that conduct electricity when dissolved in a solvent or in the molten state.

Hydrogen Electrode Potential

The potential of a hydrogen electrode measured under standard conditions—used as an electrochemical reference point.

How to Measure Electrode Potential

Measuring/calculating electrode potential according to given values

Redox Potential Comparison

The oxidizing agent is associated with the more positive standard electrode potential/redox potential.

Faraday's Laws

Mass of material that undergoes reaction is proportional to the total charge used.

Reaction Rate Definitions

Reaction rate is the rate of change of concentration of a reactant or product over time.

Reaction Order Definitions

Reaction order is the sum of the exponentials of concentrations in the rate law.

Activation Energy Definition

Activation energy is the minimum energy required for reactant molecules to undergo reaction.

Temperature Dependence of Rate Constant (Arrhenius's Law)

Arrhenius Equation gives the logarithmic relationship between a rate constant, temperature, and activation energy.

Catalysts

Substances that increase a reaction rate without undergoing permanent chemical change themselves.

Atomic Number/Weight Definitions

Atomic number is the number of protons in the nucleus.
Atomic weight/mass is the sum of protons and neutrons.

List of Periodic Table Elements

List of elements by group number from the periodic table.
VSEPR Theory Principles
Valence Shell Electron Pair Repulsion theory which predicts the shape of molecules based on electron pair repulsion.
Pauli Exclusion Principle
This principle states that no two electrons in an atom can have the same set of quantum numbers.
Hund's Rule
Electrons fill degenerate orbitals individually first before pairing up.

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Description

This quiz tests your knowledge of fundamental concepts in general chemistry. It includes basic questions that cover essential chemical principles and may involve simple calculations. Aim for 80% accuracy by selecting correct answers from the provided options.