Chemistry Elements and Properties Quiz
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Questions and Answers

Which group of elements is known for having no affinity for electrons?

  • Noble Gases (correct)
  • Halogens
  • Alkali Metals
  • Transition Metals

What is the primary characteristic of Alkali Metals in the periodic table?

  • They are typically unreactive gas at room temperature.
  • They have similar properties to Noble Gases.
  • They are found in the same group as Halogens.
  • They readily lose one electron to form positive ions. (correct)

Which type of orbital is typically associated with Transition Metals?

  • d orbitals (correct)
  • s orbitals
  • f orbitals
  • p orbitals

Which of the following groups contains metals that are found in the outermost regions of the periodic table?

<p>Alkaline Earth Metals (D)</p> Signup and view all the answers

Which elements are classified as non-metals and typically gain electrons?

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

What is the correct relationship for calculating the standard enthalpy change for a reaction?

<p>∆H°reaction = ∆H°products - ∆H°reactants (D)</p> Signup and view all the answers

Which phase transition is represented by the process: Solid ® gas?

<p>Sublimation (C)</p> Signup and view all the answers

At what point in a phase diagram do all three phases of a substance coexist?

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

What does entropy (S) measure in a system?

<p>The degree of energy dispersal in the system (C)</p> Signup and view all the answers

Which of the following describes a supercritical fluid?

<p>A phase with indistinguishable liquid and gas densities (D)</p> Signup and view all the answers

Which equation represents the change in standard entropy of a reaction?

<p>∆S°reaction = ∆S°products - ∆S°reactants (C)</p> Signup and view all the answers

What occurs to entropy at equilibrium?

<p>Entropy is maximized. (C)</p> Signup and view all the answers

Gibbs Free Energy (G) is derived from which two thermodynamic properties?

<p>Enthalpy and Entropy (D)</p> Signup and view all the answers

What is the relationship between Gibbs free energy change (D𝑮) and enthalpy (D𝐇) for spontaneous reactions at high temperatures?

<p>D𝑮 is negative. (C)</p> Signup and view all the answers

Which of the following expressions represents the standard Gibbs free energy change of a reaction?

<p>D𝑮°𝐫𝐱𝐧 = ∆𝑮°𝐟,𝐩𝐫𝐨𝐝𝐮𝐜𝐭𝐬 - ∆𝑮°𝐟,𝐫𝐞𝐚𝐜𝐭𝐚𝐧𝐭𝐬 (A)</p> Signup and view all the answers

Under what condition is a reaction considered non-spontaneous at all temperatures?

<p>D𝐇 is positive and D𝐒 is negative. (D)</p> Signup and view all the answers

What indicates that a system is at equilibrium regarding Gibbs free energy?

<p>D𝑮 = 0 (B)</p> Signup and view all the answers

Which statement best describes ideal gases?

<p>Ideal gas molecules collide elastically. (D)</p> Signup and view all the answers

What happens to real gases under high pressure and low temperature?

<p>They deviate from ideal behavior. (A)</p> Signup and view all the answers

If both D𝐇 and D𝐒 are negative, what is the expected behavior of the Gibbs free energy at low temperatures?

<p>D𝑮 is negative. (A)</p> Signup and view all the answers

Which formula relates Gibbs free energy change to the reaction quotient (Q)?

<p>∆𝐺MNO = −R T ln(Q) (D)</p> Signup and view all the answers

Which type of bond results from the overlap of two unhybridized p-orbitals aligned side-by-side?

<p>Pi bond (C)</p> Signup and view all the answers

What is the primary role of a Lewis Acid in chemical reactions?

<p>To accept electrons (D)</p> Signup and view all the answers

Which statement is true regarding multiple bonds compared to single bonds?

<p>Multiple bonds are shorter and stronger than single bonds (A)</p> Signup and view all the answers

What does an increase in pKa generally indicate about an acid's strength?

<p>The acid is weaker (C)</p> Signup and view all the answers

Which of the following statements about reducing agents is correct?

<p>They donate electrons and are oxidized (B)</p> Signup and view all the answers

What defines an amphoteric molecule?

<p>It can act as either an acid or a base (B)</p> Signup and view all the answers

How is the oxidation state of an atom defined?

<p>By the charge an atom would have with completely ionic bonds (B)</p> Signup and view all the answers

Which of the following best describes a Brønsted-Lowry Base?

<p>A proton acceptor (D)</p> Signup and view all the answers

What is the primary characteristic of SN2 reactions?

<p>They occur in a single step with inversion of stereochemistry. (C)</p> Signup and view all the answers

Which statement accurately describes the stereochemistry of SN2 reactions?

<p>There is inversion of stereochemistry due to backside attack. (D)</p> Signup and view all the answers

What factor does NOT affect the rate of SN2 reactions?

<p>Concentration of the substrate. (D)</p> Signup and view all the answers

Which of the following is true about primary alcohol oxidation?

<p>They can only be oxidized to aldehydes by PCC. (C)</p> Signup and view all the answers

What type of substrate is preferred in SN2 reactions?

<p>Less-substituted substrates. (B)</p> Signup and view all the answers

What is the general formula for alcohols?

<p>ROH (B)</p> Signup and view all the answers

How do phenols differ from simple alcohols?

<p>Phenols contain benzene rings with -OH groups. (C)</p> Signup and view all the answers

What product results when primary alcohols are oxidized by stronger oxidizing agents?

<p>Carboxylic acids. (B)</p> Signup and view all the answers

Real gases occupy less volume than predicted by the ideal gas law under what conditions?

<p>At moderate temperatures and low pressures (B)</p> Signup and view all the answers

What does the Van der Waals equation correct for?

<p>Attractive forces and volume of particles (C)</p> Signup and view all the answers

At standard temperature and pressure (STP), how much volume does 1 mol of gas occupy?

<p>22.4 L (D)</p> Signup and view all the answers

Which gas law states that pressure multiplied by volume equals a constant when the amount of gas and temperature are held constant?

<p>Boyle’s Law (A)</p> Signup and view all the answers

What is the relationship stated by Graham's Law concerning diffusion and effusion?

<p>Molar mass affects the speed of diffusion and effusion (B)</p> Signup and view all the answers

In kinetic molecular theory, how is the average kinetic energy of gas molecules related to temperature?

<p>Higher temperature results in greater average kinetic energy (A)</p> Signup and view all the answers

According to Dalton's Law, how is the total pressure of a gas mixture calculated?

<p>By adding the partial pressures of each individual gas (A)</p> Signup and view all the answers

What principle explains that gas molecules occupy more volume than predicted at extremely high pressures?

<p>Van der Waals equation (C)</p> Signup and view all the answers

How does molar mass affect gas diffusion?

<p>Gas with higher molar mass diffuses more slowly (D)</p> Signup and view all the answers

What does Charles’s Law state about volume and temperature?

<p>Volume increases with increasing temperature at constant pressure (A)</p> Signup and view all the answers

What is the Combined Gas Law an amalgamation of?

<p>Boyle’s Law, Charles’s Law, and Gay-Lussac’s Law (D)</p> Signup and view all the answers

Which of the following gases exist as diatomic molecules?

<p>Oxygen (D)</p> Signup and view all the answers

What happens to the motion of gas molecules as temperature decreases?

<p>Molecules move slower (C)</p> Signup and view all the answers

What does Henry's Law describe regarding gas solubility?

<p>Increased pressure results in greater solubility of gas in liquid (C)</p> Signup and view all the answers

What does the equation for density of gas express in terms of mass and volume?

<p>Density is mass divided by volume (C)</p> Signup and view all the answers

Flashcards

Aufbau Principle

Electrons fill atomic orbitals in order of increasing energy.

Atomic Orbitals

Specific regions around the atom's nucleus where electrons are likely to be found.

s, p, d, f orbitals

Different shapes of electron clouds.

Periodic Table

Table organizing chemical elements by properties.

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Noble Gases

Elements with full outer electron shells, un-reactive.

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Enthalpy Change (∆H)

The amount of heat absorbed or released during a reaction, a measure of energy change.

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Heat of Formation (∆H°f)

The enthalpy change when one mole of a compound is formed from its elements in their standard states.

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Standard Conditions (°)

Conditions defined as 298 K (25 °C) and 1 atm pressure.

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Fusion

The process of a solid changing into a liquid.

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Entropy (S)

A measure of the randomness or disorder of a system.

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Gibbs Free Energy (G)

A thermodynamic potential that combines enthalpy and entropy to determine the spontaneity of a process.

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Standard Entropy of Reaction (∆S°rxn)

The change in entropy accompanying a reaction under standard conditions.

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Supercritical Fluid

A substance at a temperature and pressure above its critical point, where liquid and gas phases are indistinguishable.

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Standard Gibbs Free Energy Change (DG°)

The change in Gibbs free energy for a reaction under standard conditions (298K and 1 atm).

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Spontaneous

A reaction that proceeds without external input of energy. The Gibbs free energy decreases (DG < 0).

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Non-spontaneous

A reaction that requires energy input to occur. The Gibbs free energy increases (DG > 0).

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Equilibrium

State where the forward and reverse reaction rates are equal. The Gibbs free energy remains unchanged (DG = 0).

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What factors affect spontaneity?

Enthalpy (DH), entropy (DS), and temperature (T) influence whether a reaction is spontaneous or not.

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Ideal Gas

A theoretical gas that follows the ideal gas law. Molecules have negligible volume and collisions are perfectly elastic.

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Real Gas

A gas that deviates from ideal behavior, especially at high pressures and low temperatures.

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Antibonding Orbitals

Orbitals formed by the overlap of atomic orbitals with opposite signs, resulting in destructive interference and higher energy.

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Single Bond

A covalent bond formed by the sharing of one electron pair between two atoms.

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Double Bond

A covalent bond formed by the sharing of two electron pairs between two atoms, consisting of one sigma and one pi bond.

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Triple Bond

A covalent bond formed by the sharing of three electron pairs between two atoms, consisting of one sigma and two pi bonds.

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Lewis Acid

A substance that accepts an electron pair, often having vacant orbitals or a positive charge.

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Lewis Base

A substance that donates an electron pair, often having lone pairs of electrons or a negative charge.

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Oxidation Number

The hypothetical charge an atom would have if all its bonds were completely ionic. Represents the number of electrons gained or lost.

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Oxidizing Agent

A substance that gains electrons and gets reduced in a reaction, causing another substance to be oxidized.

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SN2 Reaction

A type of nucleophilic substitution reaction that occurs in one step, where the nucleophile attacks the substrate at the same time as the leaving group departs. This leads to inversion of stereochemistry.

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SN1 Reaction

A two-step nucleophilic substitution reaction, where the leaving group first departs to form a carbocation intermediate. The nucleophile then attacks the carbocation in a separate step, leading to a racemic mixture of products.

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E2 Reaction

A one-step elimination reaction where the base removes a proton and the leaving group departs simultaneously, forming a double bond.

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E1 Reaction

A two-step elimination reaction that involves the formation of a carbocation intermediate followed by the removal of a proton from a neighboring carbon atom to form a double bond.

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Primary Alcohol

An alcohol where the carbon atom attached to the hydroxyl group is bonded to only one other carbon atom.

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Secondary Alcohol

An alcohol where the carbon atom attached to the hydroxyl group is bonded to two other carbon atoms.

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Tertiary Alcohol

An alcohol where the carbon atom attached to the hydroxyl group is bonded to three other carbon atoms.

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Phenol

An aromatic compound containing a hydroxyl group (-OH) directly attached to the benzene ring.

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Ideal Gas Law

A simplified model describing the behavior of gases, assuming particles have no volume and no attractive forces. It relates pressure (P), volume (V), number of moles (n), and temperature (T) using the equation PV = nRT, where R is the ideal gas constant.

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What does the Van der Waals equation account for?

The Van der Waals equation is a modification of the ideal gas law to account for the real-world behavior of gases, particularly the intermolecular forces and the finite volume of gas particles.

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What is the significance of ‘a’ in the Van der Waals equation?

The term 'a' in the Van der Waals equation represents the strength of the attractive forces between gas molecules, which contributes to the deviation from ideal gas behavior.

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What is the significance of ‘b’ in the Van der Waals equation?

The term 'b' in the Van der Waals equation represents the volume occupied by the gas molecules themselves, a factor that contributes to the deviation from ideal gas behavior.

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What is STP?

STP stands for Standard Temperature and Pressure, a reference condition commonly used in chemistry (0°C or 273K, and 1 atm).

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What is the density of a gas?

The density of a gas is its mass per unit volume, typically expressed in grams per liter (g/L).

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What is the combined gas law?

The combined gas law combines Boyle's, Charles's, and Gay-Lussac's laws into a single equation V2 = V1(P1/P2)(T2/T1) , expressing the relationship between pressure, volume, and temperature of a fixed amount of gas.

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What is Avogadro's Principle?

Avogadro's Principle states that equal volumes of different gases at the same temperature and pressure contain the same number of molecules.

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What is Boyle's Law?

Boyle's Law states that the volume of a fixed mass of gas is inversely proportional to its pressure at constant temperature.

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What is Charles's Law?

Charles's Law states that the volume of a fixed mass of gas is directly proportional to its absolute temperature at constant pressure.

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What is Gay-Lussac's Law?

Gay-Lussac's Law states that the pressure of a fixed mass of gas is directly proportional to its absolute temperature at constant volume.

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What is the kinetic molecular theory of gases?

The kinetic molecular theory is a model that explains the behavior of gases based on the motion of particles, assuming there are no intermolecular attractions, particles are in constant random motion, and collisions are perfectly elastic.

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What is diffusion?

Diffusion is the process by which particles spread out from a region of high concentration to a region of low concentration.

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What is effusion?

Effusion is the process by which a gas escapes through a small opening into a vacuum.

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What is Graham's Law?

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

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Study Notes

MCAT Review Sheets - 2019 Revision

  • The document is a set of MCAT review sheets, revised in 2019.
  • Contact information for questions or comments: [email protected]

Contents - General Chemistry

  • Topic 1: Atomic Structure
    • A = Mass number = protons + neutrons
    • Z = Atomic number = # of protons
    • Atomic Weight = weighted average
  • Topic 2: The Periodic Table
  • Topic 3: Bonding and Chemical Interactions
    • Nonpolar Bonds: ΔEN < 0.5
    • Polar Bonds: ΔEN 0.5 - 1.7
    • Covalent Bonds: Bonds formed via electron sharing
    • Bond Order (single, double, or triple) impacts bond strength, energy, and length
    • Coordinate Covalent Bond: One atom provides both bonding electrons.
    • Intermolecular Forces: Hydrogen bonding (O-H, N-H, F-H), dipole-dipole, London Dispersion
  • Topic 4: Compounds and Stoichiometry
  • Topic 5: Chemical Kinetics
    • Equilibrium constant (Keq)
    • Reaction quotient (Qc)
  • Topic 6: Equilibrium
  • Topic 7: Thermochemistry
  • Topic 8: The Gas Phase
  • Topic 9: Solutions
    • % by mass, mole fraction, molarity, molality, normality
    • Dilutions: M1 V1 = M2 V2
  • Topic 10: Oxidation-Reduction Reactions
  • Topic 11: Electrochemistry

Contents - Organic Chemistry

  • Topic 1: Nomenclature
    • IUPAC Conventions:
      • Step 1: Identify the longest carbon chain containing the highest-priority functional group.
      • Step 2: Number the chain to give the highest-priority functional group the lowest possible number.
      • Step 3: Name the substituents with prefixes (di-, tri-, etc.).
      • Step 4: Give each substituent a number assigning it to the carbon where it's attached.
      • Step 5: Alphabetize substituents and write numbers separated by commas and words by hyphens.
  • Topic 2: Hydrocarbons and Alcohols
    • Alkanes, Alkenes, Alkynes, Alcohols, Diols
    • Carbonyl Group: C=O (aldehydes and ketones)
  • Topic 3: Carboxylic Acids & Derivatives
    • Anhydrides, Ester, Amid
  • Topic 4: Isomers
  • Topic 5: Stereoisomers
  • Topic 6: Conformational Isomers
  • Topic 7: Configurational Isomers
  • Topic 8: Enantiomers and Diastereomers
  • Topic 9: Chirality
  • Topic 10: Stereochemistry (Chirality & Stereoisomers)
  • Topic 11: R/S Configuration & Fischer Projections
  • Topic 12: Bonding (Atomic Orbitals, Quantum Numbers, Hybridization)

Contents - Biochemistry

  • Topic 1: Amino Acids, Peptides, and Proteins
  • Topic 2: Enzymes
  • Topic 3: Carbohydrate Structure & Function
  • Topic 4: Carbohydrate Metabolism I
  • Topic 5: Lipid Structure and Function
  • Topic 6: Lipid and Amino Acid Metabolism
  • Topic 7: Bioenergetics and Regulation of Metabolism

Contents - Biology

  • Topic 1: The Cell (including cell types)
  • Topic 2: Reproduction
  • Topic 3: Embryogenesis and Development
  • Topic 4: Nervous System
  • Topic 5: Endocrine System
  • Topic 6: Respiratory System
  • Topic 7: Cardiovascular System
  • Topic 8: Immune System
  • Topic 9: Digestive System
  • Topic 10: Kidney and Skin
  • Topic 11: Muscular System
  • Topic 12: Genetics and Evolution

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Description

Test your knowledge on the periodic table with this quiz focusing on the characteristics and classifications of various elements. Questions include topics related to Alkali Metals, Transition Metals, and non-metals. Challenge yourself to see how well you understand elemental properties!

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