Science Lesson 1: Properties of Matter

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Questions and Answers

Which of the following is NOT a characteristic of Dalton's atomic theory?

  • Atoms of the same element are identical.
  • Atoms can be transformed into one another. (correct)
  • Atoms of different elements have different masses.
  • Atoms are the smallest unit of an element that can exist.

What is the main concept that distinguishes Dalton's atomic theory from the ancient Greek philosopher's ideas?

  • The idea that atoms of different elements have different masses.
  • The existence of atoms as the fundamental building blocks of matter.
  • The use of scientific experimentation to support the theory. (correct)
  • The belief that atoms are indivisible.

Which scientist's experiment provided evidence for the existence of a subatomic particle?

  • Democritus
  • Ernest Rutherford
  • JJ. Thompson (correct)
  • John Dalton

What is the name of the model proposed by JJ. Thompson based on his experiment with the cathode ray tube?

<p>Plum Pudding Model (C)</p> Signup and view all the answers

What is the significance of the deflection of the cathode rays in JJ. Thompson's experiment?

<p>It provided evidence for the existence of negatively charged particles. (D)</p> Signup and view all the answers

What is the major difference between Dalton's atomic theory and Rutherford's model?

<p>Dalton believed that atoms were indivisible, while Rutherford discovered subatomic particles. (A)</p> Signup and view all the answers

What was the primary role of the cathode ray tube in JJ. Thompson's experiments?

<p>It allowed the study of the behavior of negatively charged particles. (D)</p> Signup and view all the answers

What is the chemical symbol for an element?

<p>A shorthand representation of a chemical element consisting of one or two letters derived from the element's name. (A)</p> Signup and view all the answers

Which of these scientist's ideas were challenged by the discoveries of subatomic particles?

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

What is the difference between isotopes of the same element?

<p>The number of neutrons in their nuclei. (A)</p> Signup and view all the answers

Which of the following is NOT a factor that contributes to the atomic mass of an element?

<p>Number of isotopes present. (D)</p> Signup and view all the answers

How is the neutron number of an atom calculated?

<p>By subtracting the atomic number from the mass number. (A)</p> Signup and view all the answers

What is the significance of an element's atomic number?

<p>It determines the element's chemical properties. (D)</p> Signup and view all the answers

What is the term used to describe the time it takes for half of a given sample of a particular isotope to decay?

<p>Half-life (D)</p> Signup and view all the answers

What does the term 'electron configuration' refer to?

<p>The arrangement of electrons in the electron shells around the nucleus. (B)</p> Signup and view all the answers

Isotopes can be formed naturally or through what process?

<p>Nuclear reactions. (D)</p> Signup and view all the answers

What is the name of the model that states that the center of the atom is the nucleus, which contains protons and neutrons?

<p>Quantum Mechanical Model (B)</p> Signup and view all the answers

What does the l quantum number represent?

<p>The shape of the sublevel (B)</p> Signup and view all the answers

Which of the following statements is TRUE about the relationship between the principal quantum number (n) and the energy of an electron?

<p>The larger the value of <em>n</em>, the further it is away from the nucleus, and thus the higher the energy of an electron. (A)</p> Signup and view all the answers

How does the size of the electron cloud relate to the number of electrons?

<p>The bigger the cloud, the more electrons. (D)</p> Signup and view all the answers

What are subshells/sublevels?

<p>A group of orbitals with the same shape. (D)</p> Signup and view all the answers

What is the function of the magnetic quantum number?

<p>To describe the orientation of an orbital in space. (A)</p> Signup and view all the answers

What is the purpose of electron configuration?

<p>To describe the distribution of electrons in each energy level. (C)</p> Signup and view all the answers

Which of the following is NOT a function of a quantum number?

<p>Describing the mass of an electron. (D)</p> Signup and view all the answers

What does the principle quantum number (n) represent in an electron configuration?

<p>The energy level and distance from the nucleus (B)</p> Signup and view all the answers

What is the maximum number of electrons that can occupy a 'd' subshell?

<p>10 (D)</p> Signup and view all the answers

According to Hund's Rule, how are electrons filled into orbitals of equal energy?

<p>Orbitals are filled with one electron each before any orbital is doubly occupied. (B)</p> Signup and view all the answers

What is the primary difference between an atomic orbital and an energy level?

<p>An atomic orbital describes the shape of an electron's wave pattern, while an energy level describes the electron's energy. (C)</p> Signup and view all the answers

What is the spin quantum number (m) used to describe?

<p>The direction of an electron's spin. (A)</p> Signup and view all the answers

What is the main purpose of an orbital diagram?

<p>To visually depict the distribution of electrons in an atom's orbitals. (C)</p> Signup and view all the answers

How do the principle quantum number (n) and the atomic number relate to the electron configuration of an element?

<p>The atomic number determines the number of protons and electrons, which is then used to fill the energy levels (n) in the electron configuration. (D)</p> Signup and view all the answers

Which of the following properties is NOT an extensive property?

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

Which property describes the ability of a material to return to its original shape after being stretched or compressed?

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

What is a physical property defined as?

<p>A characteristic that can be observed or measured without changing the chemical composition of a substance. (D)</p> Signup and view all the answers

Which property describes how easily a substance can be broken apart?

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

Which of these is NOT an example of a physical change?

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

What is the difference between mass and weight?

<p>Mass measures the amount of matter, weight measures the force of gravity on the matter. (B)</p> Signup and view all the answers

Which of the following is a good example of a conductor of heat?

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

What is the temperature at which a substance changes from a liquid to a gas called?

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

What happens when an electron absorbs energy?

<p>It moves to a higher energy level. (D)</p> Signup and view all the answers

What is the relationship between the distance of an energy level from the nucleus and its energy?

<p>The farther the distance, the higher the energy. (B)</p> Signup and view all the answers

Which of these is NOT a source of energy that can cause electrons to jump to higher energy levels?

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

What is the difference between an atom's atomic number and its number of electrons?

<p>In a neutral atom, the atomic number is equal to the number of electrons. (D)</p> Signup and view all the answers

What is the relationship between the atomic number and the number of protons in an atom?

<p>The atomic number is equal to the number of protons. (C)</p> Signup and view all the answers

What is the defining characteristic of an ion?

<p>It has lost or gained electrons. (A)</p> Signup and view all the answers

What is the valence shell of an atom?

<p>The outermost energy level. (D)</p> Signup and view all the answers

What is the main contribution of modern quantum mechanics to atomic theory?

<p>It replaced the idea of fixed orbits for electrons with probabilistic regions. (C)</p> Signup and view all the answers

Flashcards

Subatomic Particles

Particles smaller than an atom that make up matter.

John Dalton

An English physicist who proposed the atomic theory in 1808.

Atomic Theory

Theory that matter is composed of atoms, indivisible and unique to each element.

Cathode Ray Tube

A vacuum tube that generates streams of electrons used in experiments.

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JJ Thomson

Physicist who discovered the electron using the cathode ray tube in 1897.

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Plum Pudding Model

A model where electrons are embedded in a positively charged sphere.

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Solid Sphere Model

Dalton's model of the atom, describing atoms as solid, indivisible spheres.

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Electron

A tiny, negatively charged particle discovered by Thomson.

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Quarks

Smallest building blocks of protons and neutrons.

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Atoms

Basic units made of electrons, protons, and neutrons.

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Extensive Properties

Properties that depend on the amount of substance present.

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Physical Properties

Observable characteristics that do not change chemical composition.

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Elasticity

Ability to return to original shape after stretching or compressing.

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Brittleness

Ability of an object to shatter easily.

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Boiling Point

Temperature at which a substance transitions from liquid to gas.

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Melting Point

Temperature at which a substance transitions from solid to liquid.

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Energy Levels

Regions around the nucleus where electrons can reside, each with a specific distance and energy.

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Electron Jump

The transition of electrons from lower to higher energy levels through absorption or emission of energy.

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Electron Cloud Model

A modern atomic model that depicts probabilistic regions rather than fixed orbits for electron locations.

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Protons and Atomic Number

The atomic number (Z) represents the number of protons in the nucleus of an atom, determining the element.

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Cations

Positively charged ions formed when an atom loses one or more electrons.

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Anions

Negatively charged ions formed when an atom gains one or more electrons.

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Valence Shell

The outermost energy level of an atom, containing the valence electrons that participate in chemical bonding.

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Absorption and Emission

Processes by which electrons gain energy (absorption) or lose energy (emission) to move between energy levels.

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Electron Spin

Electrons can spin in two directions: +½ (clockwise) or -½ (counterclockwise).

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Atomic Orbitals

Regions of space where there is a high probability of finding electrons.

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Orbital Capacity

Different orbitals can hold different maximum numbers of electrons: s=2, p=6, d=10, f=14.

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Principal Quantum Number (n)

Indicates the energy level and size of an electron's orbital.

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Orbital Diagrams

Visual representations showing electron distribution in orbitals.

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Hund's Rule

Electrons fill empty orbitals first before pairing up in one.

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Electron Configuration

The notation that shows the distribution of electrons among orbitals.

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Energy Level Changes

Energy changes occur when electrons shift between different wave patterns.

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Isotopes

Atoms of the same element with different numbers of neutrons.

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Chemical Number

The number of protons in an atom's nucleus, defining the element.

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Chemical Symbol

A one or two-letter abbreviation for a chemical element.

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Neutron Number

The difference between the mass number and the atomic number.

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Mass Number

The total number of protons and neutrons in an atom's nucleus.

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Atomic Mass

The average mass of an atom of an element, accounting for all particles.

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Half-Life

The time required for half of a sample of an isotope to decay.

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Nuclear Decay

The process by which unstable isotopes lose energy by emitting radiation.

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Nucleus

The center of the atom, containing protons and neutrons.

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Angular Momentum Quantum Number

Indicates the shape of orbitals within an energy level, ranging from 0 to (n - 1).

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Subshells/Sublevels

Groups of orbitals within an energy level sharing the same shape.

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Magnetic Quantum Number

Describes the orientation of an orbital in three-dimensional space.

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Spin Quantum Number

Indicates the spin state of an electron within an orbital.

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Study Notes

Table of Contents

  • Lesson 1: Properties of Matter
  • Lesson 2: Phases of Matter
  • Lesson 3: The Atomic Theory of Matter
  • Lesson 4: Ions and Isotopes
  • Lesson 5: Electron Configuration

Lesson 1: Properties of Matter (pp. 193-203)

  • Subchapter 1: Fundamental Concepts
    • Matter: The building blocks of everything, having mass and occupying space (volume). Classified as elements or compounds.
    • Atoms and Molecules: The basic units of matter.
    • Atoms: Composed of electrons, protons, and neutrons (quarks are the building blocks of protons and neutrons). -Elements: A pure substance made of only one type of atom. -Compounds: A pure substance made of two or more different types of atoms chemically combined. -Molecules: Two or more atoms chemically bonded together.
  • Subchapter 2: Introduction to Atoms
    • Atom Structure: Atoms have a nucleus (containing protons and neutrons) at the center, with electrons orbiting around it.
  • Subchapter 3: Classifications of Matter
    • Pure Substances: Made of only one type of particle (composition is fixed)
      • Elements: Only one kind of atom.
      • Compounds: Two or more chemically combined elements.
    • Mixtures: Two or more substances mixed together (composition is variable).
      • Homogeneous: Uniform composition (e.g., saltwater).
      • Heterogeneous: Non-uniform composition (e.g., sand and water).

Lesson 2: Phases of Matter (pp. 204-216)

  • Subchapter 1: Phase Changes
    • Phase Changes: Changes of state (solid, liquid, gas) of matter due to heat absorption or release.
    • States of Matter:
      • Solid: Definite volume and shape; molecules are tightly packed.
      • Liquid: Definite volume, takes the shape of the container; molecules are loosely packed.
      • Gas: No definite volume or shape; molecules move freely.
      • Plasma: High-energy state of matter; molecules are ionized.
    • Water: Exists as a solid (ice), liquid (water), and gas (water vapor) in nature.

Lesson 3: The Atomic Theory (pp.217-232)

  • Subchapter 1: Introduction to the Atom
    • Atom: Smallest unit of an element that still retains its chemical properties.
  • Subchapter 2: Parts of an Atom
    • Nucleus: Dense, central core containing protons (positive charge) and neutrons (neutral charge).
    • Electrons: Negatively charged particles orbiting the nucleus.
  • Subchapter 3: Pioneers of the Atomic Theory
    • Democritus (2400 B.C): Proposed the idea of atoms.
    • Aristotle: Opposed the concept of atoms.
    • Dalton (1808 AD): Developed atomic theory, describing atoms as solid spheres.
    • Thomson (1897): Discovered the electron, proposing the "plum pudding" model of the atom.
    • Rutherford (1909): Discovered the nucleus with the gold foil experiment.
    • Chadwick (1932): Discovered the neutron.
    • Bohr (1913): Proposed that electrons orbit the nucleus in fixed energy levels.
    • Heisenberg and Schrödinger (Present): Developed the quantum mechanical model of the atom describing electrons as clouds of probability.

Lesson 4: lons and Isotopes (pp. 226-232)

  • Subchapter 1: Atomic Numbers
    • Atomic Number: Number of protons in an atom.
    • Chemical Symbol: Short representation of an element.
    • Atomic Mass: Average mass of an atom of an element.
  • Subchapter 2: lons and Isotopes
    • Ions: Atom gaining or losing electrons (becoming charged); cations (positive) and anions (negative).
    • Valence Shell: Outermost electron shell.
    • Isotopes: Atoms of the same element with different numbers of neutrons.

Lesson 5: The Electron Configuration (pp. 233-244)

  • Subchapter 1: Configurate your Mind!
    • Electron Cloud Model: Modern representation of electron distribution around the nucleus (not fixed orbits).
  • Subchapter 2: Quantum Numbers
    • Quantum Numbers: Describe the properties of electrons (energy level, shape, orientation, spin)
  • Subchapter 3: Orbitals
    • Orbitals: Regions of space with high probability of finding electrons (s, p, d, f).
    • Electron Configuration: Arrangement of electrons in orbitals/sublevels.
  • Subchapter 4: Principles of Electron Configuration
    • Aufbau principle: Electrons fill lower-energy levels first.
    • Hund's rule: Electrons singly occupy orbitals of equal energy before pairing up.
    • Pauli exclusion principle: No two electrons in the same atom can have the same set of four quantum numbers.

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