Chemistry Chapter 3 Quiz
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Questions and Answers

Which state of matter has a definite volume but no definite shape?

  • Plasma
  • Solid
  • Gas
  • Liquid (correct)

A physical change results in the formation of a new substance.

False (B)

What is the term for the process of a gas turning directly into a solid?

Deposition

_ is the mass per unit volume of a substance.

<p>Density</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Melting Point = Temperature at which a solid turns into a liquid Boiling Point = Temperature at which a liquid turns into a gas Condensation = Process of gas turning into a liquid Sublimation = Transition of a substance from solid to gas</p> Signup and view all the answers

Which of the following is an example of a covalent compound?

<p>Water (H₂O) (C)</p> Signup and view all the answers

A mixture is formed when two or more elements are chemically bonded.

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

What is the smallest unit of an element?

<p>Atom</p> Signup and view all the answers

Which of the following is a characteristic of acids?

<p>Releases hydrogen ions (H⁺) when dissolved in water (D)</p> Signup and view all the answers

Methane (CH₄) is an example of a complex compound.

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

What is the fundamental equation that describes how the quantum state of a system evolves over time?

<p>Schrödinger Equation</p> Signup and view all the answers

The _______ quantum number defines the shape of an orbital.

<p>angular momentum</p> Signup and view all the answers

Which of the following is NOT a quantum number?

<p>Molecular Quantum Number (M) (A)</p> Signup and view all the answers

According to Hund's Rule, electrons will pair up in degenerate orbitals before occupying them singly.

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

What are the electrons in the outermost shell of an atom that participate in bonding known as?

<p>Valence electrons</p> Signup and view all the answers

What is the term for a positively charged ion?

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

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration of 6 valence electrons.

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

What type of energy is released when ions form a crystalline lattice?

<p>Lattice Energy</p> Signup and view all the answers

A quantum of electromagnetic energy emitted or absorbed by electrons during transitions is called a ______.

<p>photon</p> Signup and view all the answers

Match the following terms to their descriptions:

<p>Valence Electrons = Electrons in the outermost shell of an atom Electronegativity = Ability of an atom to attract electrons in a chemical bond Ionization Energy = Energy required to remove an electron from an atom Electron Affinity = Energy change when an atom gains an electron</p> Signup and view all the answers

What type of bond is formed through the electrostatic attraction between oppositely charged ions?

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

What kind of bond is formed by the sharing of electrons between atoms?

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

Metals typically gain electrons to form anions in ionic bonding.

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

Molecular compounds typically have high melting and boiling points.

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

What is the phenomenon where particles pass through energy barriers they classically cannot surmount?

<p>Quantum Tunneling</p> Signup and view all the answers

What type of intermolecular force is present in all molecules?

<p>london dispersion forces</p> Signup and view all the answers

The tendency of a substance to vaporize is known as ______.

<p>volatility</p> Signup and view all the answers

Which of the following describes a molecule with an uneven distribution of electron density and a net dipole moment?

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

Match the terms describing molecular structure with their definitions:

<p>Intermolecular Forces = Weak forces between molecules Molecular Lattice = Arrangement of molecules in a crystalline structure Amorphous Solid = Non-crystalline solid with no regular arrangement Polarity = Uneven distribution of electron density in a molecule</p> Signup and view all the answers

Molecular compounds are typically good conductors of electricity.

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

The word 'cat' is a good example of a ______.

<p>noun</p> Signup and view all the answers

Flashcards

Matter

Anything that has mass and takes up space.

Mass

The amount of matter in an object.

Volume

The amount of space an object occupies.

Density

The ratio of mass to volume of a substance.

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Compound

A substance formed when two or more elements chemically combine.

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Mixture

A combination of two or more substances that are not chemically bonded.

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Physical Property

A characteristic that can be observed without changing the substance's identity.

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Chemical Property

A characteristic that describes a substance's ability to undergo chemical changes.

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Acids

A substance that releases hydrogen ions (H⁺) when dissolved in water. It exhibits sour taste and reacts with bases to form salts.

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Organic Compounds

Compounds primarily composed of carbon atoms bonded with hydrogen, oxygen, nitrogen, or other elements. They are typically found in living organisms.

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Quantum Mechanics

A branch of physics exploring the behavior of particles at atomic and subatomic scales.

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Wave-Particle Duality

The concept that particles, like electrons, can exhibit both wave-like and particle-like properties.

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Schrödinger Equation

A fundamental equation describing how a quantum system's state changes over time.

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Wavefunction (Ψ)

A mathematical function representing the quantum state of a particle, showing the probability of finding it in a certain region.

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Atomic Orbital

A region in space where there is a high probability of finding an electron.

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Angular Momentum Quantum Number (l)

Defines the shape of an atomic orbital, like s, p, d, or f. It's a quantum number.

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Molecular Structure

The way atoms are arranged in a molecule, determining its shape and properties.

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Covalent Bond

A type of bond formed when two atoms share electrons.

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Intermolecular Forces

Weak forces of attraction between molecules that influence their physical properties.

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Volatility

The tendency of a substance to change from a liquid to a gas.

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Low Melting Point

Substances with weak intermolecular forces tend to melt and boil at lower temperatures.

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Solubility

Describes the ability of one substance to dissolve in another.

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Polarity

An uneven distribution of electron density within a molecule, creating a partial positive and partial negative charge.

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Hydrogen Bonding

A strong intermolecular force involving a hydrogen atom bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine.

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Ion

An atom or molecule with a net electric charge due to the loss or gain of electrons.

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Cation

A positively charged ion formed by the loss of electrons.

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Anion

A negatively charged ion formed by the gain of electrons.

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Electrostatic Force

The force of attraction between oppositely charged ions.

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Electron Transfer

The movement of electrons from one atom to another during ionic bond formation.

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Valence Electrons

Electrons in the outermost shell of an atom, involved in bond formation.

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Octet Rule

Atoms tend to gain, lose, or share electrons to achieve a stable configuration of 8 valence electrons.

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Ionic Bond

A chemical bond formed through the electrostatic attraction between oppositely charged ions.

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