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Quizzes > High School Quizzes > Science

Chem 1311 Exam 3 Practice Quiz

Master chemical concepts with engaging practice exercises

Difficulty: Moderate
Grade: Other
Study OutcomesCheat Sheet
Paper art representing a chemistry trivia quiz for college students preparing for exams.

What does the atomic number of an element represent?
The number of protons in the nucleus
The total number of electrons in the atom
The number of neutrons in the nucleus
The sum of protons and neutrons
The atomic number is defined as the number of protons in an atom's nucleus. This key property uniquely identifies an element and determines its position in the periodic table.
What is the charge of an electron?
Both positive and negative
Negative
Neutral
Positive
Electrons carry a negative charge, which is a fundamental property of subatomic particles. This characteristic is crucial for understanding atomic structure and bonding.
Which of the following subatomic particles is NOT located in the nucleus of an atom?
Electron
Neutron
Proton
Both proton and neutron
In an atom, electrons orbit the nucleus while protons and neutrons reside inside it. Therefore, electrons are not found in the nucleus.
Which of the following best describes an ionic bond?
A bond formed by the sharing of electrons between atoms
A bond formed by the overlap of atomic orbitals without electron transfer
A bond formed by the transfer of electrons from one atom to another resulting in ions
A bond where electrons are delocalized, as in metals
An ionic bond is created when electrons are transferred from one atom to another, leading to the formation of oppositely charged ions. This electrostatic attraction between ions holds the compound together.
How are elements arranged in the modern periodic table?
By increasing atomic mass
By the number of neutrons
By alphabetical order of their names
By increasing atomic number
The modern periodic table arranges elements by increasing atomic number, which is the number of protons. This arrangement highlights recurring periodic trends in element properties.
How many atoms are in one mole of any substance?
6.022 x 10^23 atoms
3.00 x 10^8 atoms
1.00 x 10^6 atoms
6.022 x 10^20 atoms
One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. This constant is a fundamental link between the macroscopic and atomic scales.
Which law states that mass is neither created nor destroyed in a chemical reaction?
Law of Definite Proportions
Newton's Law
Law of Conservation of Mass
Ideal Gas Law
The law of conservation of mass asserts that mass remains constant during a chemical reaction. This principle is essential for balancing chemical equations accurately.
When balancing a chemical equation, what must be conserved?
Only the energy of the system
Only the number of electrons
Only the number of oxygen atoms
Both mass and the number of atoms of each element
A balanced chemical equation requires that the number of atoms for each element is the same on both sides, ensuring conservation of mass. This balancing reflects the fundamental principle that matter is neither created nor destroyed in a reaction.
In a chemical reaction, the substance that is completely consumed first is known as the:
Excess reactant
Product
Catalyst
Limiting reactant
The limiting reactant is the substance that is entirely consumed first, thereby limiting the amount of product that can be formed. Identifying the limiting reactant is vital for stoichiometric calculations in chemical reactions.
Which type of reaction involves two or more substances combining to form a single product?
Double displacement reaction
Synthesis reaction
Decomposition reaction
Single displacement reaction
A synthesis reaction, also known as a combination reaction, involves two or more reactants combining to form one product. This fundamental type of reaction is common in many chemical processes.
Which equation represents the Ideal Gas Law?
P = nRT/V
V = nRT
PV = mRT
PV = nRT
The Ideal Gas Law is expressed as PV = nRT, where P represents pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is the temperature. This relation describes the behavior of an ideal gas under various conditions.
As you move down a group in the periodic table, the atomic radius typically:
Fluctuates unpredictably
Increases
Decreases
Stays the same
Atomic radius increases down a group because additional electron shells are added as you move to elements with higher periods. Despite the increased nuclear charge, the added shells cause the atomic radius to expand.
Across a period in the periodic table, electronegativity generally:
Increases from left to right
Remains constant
Initially increases then decreases
Decreases from left to right
Electronegativity increases from left to right across a period as atoms have an increasing effective nuclear charge. This trend reflects the stronger attraction for electrons in atoms positioned toward the right side of the periodic table.
According to the Brønsted-Lowry theory, an acid is defined as a substance that:
Increases the pH of a solution
Accepts electrons during a reaction
Produces hydroxide ions in water
Donates protons (H+ ions)
Under the Brønsted-Lowry theory, acids are substances that donate protons (H+ ions) in a reaction. This definition focuses on the transfer of protons, distinguishing acids from bases.
How does an increase in temperature generally affect the rate of a chemical reaction?
It increases the reaction rate by providing more kinetic energy to molecules
It decreases the reaction rate by reducing molecular collisions
It stops the reaction altogether
It has no effect on the reaction rate
Raising the temperature increases the kinetic energy of molecules, leading to more frequent and forceful collisions. This generally increases the rate of a chemical reaction.
In an exothermic reaction, what is released into the surroundings?
Pressure
Mass
Heat or energy
Light only
Exothermic reactions release heat energy into the surroundings, often causing an increase in temperature. This is the opposite of endothermic reactions, which absorb energy from their environment.
What is the formula used to calculate the molarity (M) of a solution?
M = moles of solute / liters of solution
M = mass of solute / volume of solution
M = moles of solvent / liters of solute
M = volume of solute / moles of solvent
Molarity is defined as the number of moles of solute per liter of solution. This formula is essential for quantifying the concentration of solutions in chemistry.
A compound has the following percent composition by mass: 40% sulfur and 60% oxygen. What is its simplest empirical formula?
SO
SO3
S2O3
SO2
By assuming a 100 g sample, the compound contains 40 g of sulfur and 60 g of oxygen. Converting these masses to moles and simplifying the ratio yields an empirical formula of SO3.
In a balanced chemical equation, what do the coefficients represent?
The energy change during the reaction
The number of atoms randomly distributed
The mole ratio of reactants and products
The volume of the reactants
The coefficients in a balanced chemical equation indicate the mole ratio between the reactants and products. This ensures that the law of conservation of mass is upheld during the reaction.
What is the oxidation number of sulfur in sulfuric acid (H2SO4)?
+4
+6
0
-2
In H2SO4, each hydrogen has an oxidation state of +1 and each oxygen is -2. Balancing the overall charge to zero results in sulfur having an oxidation number of +6.
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Study Outcomes

  1. Understand fundamental chemical principles including atomic structure and bonding.
  2. Analyze chemical reactions to balance equations and predict outcomes.
  3. Apply stoichiometry to quantitatively solve chemistry problems.
  4. Interpret periodic trends and element properties in the context of chemical behavior.
  5. Evaluate reaction mechanisms and their implications on chemical equilibria.

Chem 1311 Exam 3 Review Cheat Sheet

  1. Master the Ideal Gas Law - PV = nRT is your golden ticket for predicting how gases behave under different conditions - think of it as the ultimate pressure - volume - temperature recipe. At standard temperature and pressure (STP), one mole of an ideal gas happily occupies 22.4 L, giving you a handy reference point. Play around with the variables and watch gas math come to life! Course Hero Study Sheet
  2. Understand Dalton's Law of Partial Pressures - Dalton says that the total pressure of a gas mix is just the sum of each gas's own pressure, so you can think of gases as sharing a dinner table politely. Use mole fractions to figure out how much pressure each guest (gas) brings to the party. This trick is especially helpful when dealing with breathing mixes or industrial gas blends. Course Hero Study Sheet
  3. Grasp Graham's Law of Effusion - Graham's Law tells you that lighter gas molecules effuse faster than heavier ones, inversely proportional to the square root of their molar masses. It's like racing marbles through a tiny hole - small ones win every time. Use this insight to compare how quickly different gases will escape or diffuse. Course Hero Study Sheet
  4. Review Quantum Numbers - Four quantum numbers (n, ℓ, mℓ, ms) uniquely define an electron's "home" in an atom - picture them as the electron's address. The principal quantum number n sets the energy level, ℓ determines the orbital shape (0 = s, 1 = p, 2 = d, etc.), mℓ picks the orientation, and ms picks the spin. Mastering these will unlock your understanding of electronic structure and periodic trends. Quizlet Flashcards
  5. Apply Hess's Law - Hess's Law is the chemistry equivalent of "you can't break even," meaning the total enthalpy change for a reaction is path-independent. Just add up the enthalpy changes of individual steps, and poof - you know the overall ΔH even if you can't measure it directly. It's perfect for piecing together complex reaction networks. Quizlet Flashcards
  6. Understand the Photoelectric Effect - Shine light above a threshold frequency on a metal surface, and electrons get ejected like popcorn in a hot pan - proof that light behaves as particles (photons). The energy of each photon must exceed the metal's work function to set electrons free. This phenomenon laid the foundation for quantum mechanics and earned Einstein a Nobel Prize! GradeBuddy Study Guide
  7. Learn Periodic Trends - Trends across the periodic table are your roadmap for atomic behavior: atomic radius shrinks left-to-right and grows down a group, while ionization energy and electron affinity generally rise across a period and fall down a group. Understanding these patterns helps you predict reactivity and bonding like a pro. GradeBuddy Study Guide
  8. Study Molecular Geometries - VSEPR theory lets you predict molecular shapes by picturing electron pairs repelling each other like solitudes at a party. From linear to trigonal planar, tetrahedral to octahedral, knowing the geometry helps you anticipate bond angles and molecular polarity. It's geometry class meets chemistry lab! UT - Austin Exam Prep
  9. Understand Intermolecular Forces - The strength of attractions between molecules - hydrogen bonds, dipole - dipole, and London dispersion forces - determines boiling points, melting points, and solubility. Think of H‑bonds as VIP interactions, dipoles as polite handshakes, and London forces as fleeting high-fives. Master these to explain why water is a liquid at room temperature! UT - Austin Exam Prep
  10. Review Chemical Bonding Theories - Dive into Valence Bond Theory to see how atomic orbitals overlap for sigma and pi bonds, then level up with Molecular Orbital Theory to understand delocalization and bond order. These frameworks reveal why O₂ is paramagnetic and why conjugated systems glow under UV light! UT - Austin Exam Prep
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