Chemistry Module 1
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Questions and Answers

What is the state of matter characterized by having no definite shape but a definite volume?

  • Solid
  • Plasma
  • Gas
  • Liquid (correct)
  • How much element B would combine with 12 g of element A if 4.0 g of A combine with 10 g of B?

  • 10 g
  • 12 g
  • 24 g
  • 30 g (correct)
  • According to the law of conservation of mass, the mass of a compound formed is _____ the sum of the masses of the individual elements.

  • Less than
  • Either greater than or less than
  • Greater than
  • Equal to (correct)
  • In which state does an electron in a hydrogen atom possess its lowest total energy?

    <p>Ground state</p> Signup and view all the answers

    Who is generally credited with the idea of arranging the elements in the periodic table based on their properties?

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

    Which prefix is used to denote three atoms in a covalent compound?

    <p>Tri-</p> Signup and view all the answers

    What is the correct name for the compound NH₃?

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

    Which of the following compounds is named using the rules for binary acids?

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

    What happens during an exothermic reaction?

    <p>Energy is released.</p> Signup and view all the answers

    Which of the following is not a structural formula model?

    <p>Covalent model</p> Signup and view all the answers

    What is the molecular formula for dinitrogen tetroxide?

    <p>N₂O₄</p> Signup and view all the answers

    Which rule states that hydrogen only needs two electrons?

    <p>Duet rule</p> Signup and view all the answers

    What is the primary purpose of Lewis Structures?

    <p>To indicate bonding arrangements.</p> Signup and view all the answers

    What is sublimation?

    <p>The process of a solid turning into a gas without becoming a liquid first</p> Signup and view all the answers

    Which separation method relies on solubility to distinguish mixtures?

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

    Which scientist believed that all matter was made up of four fundamental elements?

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

    Which of the following is a wrong postulate of Dalton's atomic theory?

    <p>Each atom is indivisible and indestructible</p> Signup and view all the answers

    The Plum Pudding Model was proposed to describe what aspect of atoms?

    <p>The distribution of electrons within an atom</p> Signup and view all the answers

    What discovery did J.J. Thomson contribute to atomic theory?

    <p>The identification of electrons as cathode rays</p> Signup and view all the answers

    What is the significance of isoptopes regarding Dalton's atomic theory?

    <p>They demonstrate that atoms can have different masses</p> Signup and view all the answers

    What occurs during crystallization?

    <p>A dissolved solid forms crystals as the solution becomes more concentrated</p> Signup and view all the answers

    Which group contains the most stable elements with a complete outer electron shell?

    <p>Group 18</p> Signup and view all the answers

    What happens to atomic radius as you move down a group in the periodic table?

    <p>It increases because the energy level is higher.</p> Signup and view all the answers

    What is the correct definition of a cation?

    <p>An atom that loses electrons, resulting in a positive charge.</p> Signup and view all the answers

    Which type of elements tends to gain electrons to achieve stability?

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

    How does ionization energy change as you move from left to right across a period?

    <p>It increases due to stronger nuclear attraction.</p> Signup and view all the answers

    Which series is classified as inner transition metals?

    <p>Lanthanide and actinide series</p> Signup and view all the answers

    Which group in the periodic table is the most reactive?

    <p>Alkali metals</p> Signup and view all the answers

    How do metalloids differ from nonmetals?

    <p>Metalloids have properties of both metals and nonmetals.</p> Signup and view all the answers

    What is the charge of the cation in the ionic compound NaCl?

    <p>+1</p> Signup and view all the answers

    When writing the formula for Iron(III) Oxide, which of the following is true?

    <p>The total charge from the cations and anions must equal zero.</p> Signup and view all the answers

    What should you do when using multiple polyatomic ions in a formula?

    <p>Use parentheses for each polyatomic ion.</p> Signup and view all the answers

    Which statement accurately describes the role of delocalized electrons in metallic bonding?

    <p>They move freely around metal atoms, holding them together.</p> Signup and view all the answers

    When naming the anion in an ionic compound, what suffix should be used?

    <p>-ide</p> Signup and view all the answers

    Which formula represents a correctly balanced ionic compound?

    <p>MgCl₂</p> Signup and view all the answers

    What is the correct way to write an ionic compound with more than one polyatomic ion?

    <p>Use parentheses around the polyatomic ion followed by the subscript.</p> Signup and view all the answers

    What characterizes the electron sea model in metals?

    <p>Electrons are loosely held, allowing free movement around the lattice.</p> Signup and view all the answers

    What is the maximum number of electrons that can occupy the n=3 energy level?

    <p>18</p> Signup and view all the answers

    Which of the following statements about Hund's rule is correct?

    <p>Single electrons must occupy equal energy orbitals before pairing up</p> Signup and view all the answers

    In the context of electron configuration, what does the Pauli exclusion principle indicate?

    <p>No more than two electrons can occupy the same orbital with opposite spins</p> Signup and view all the answers

    Which energy levels possess both s and p sublevels?

    <p>n=2 and n=3</p> Signup and view all the answers

    What is the significance of the noble gas notation in electron configuration?

    <p>It provides a shorthand for writing electron configurations</p> Signup and view all the answers

    What is the total number of valence electrons in Strontium (Sr)?

    <p>2</p> Signup and view all the answers

    According to the periodic law, what occurs when elements are arranged in increasing atomic number?

    <p>There is a periodic repetition of properties</p> Signup and view all the answers

    What is the electron configuration for Bromine (Br)?

    <p>1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2</p> Signup and view all the answers

    Study Notes

    Module 1

    • Chemistry: The study of matter and its changes, including organic, inorganic, physical, analytical, and biochemistry.

    • Matter: Anything that takes up space.

    • Mass: A measurement of the amount of matter.

    • Science: Using evidence to develop testable explanations of natural phenomena.

    • Hypothesis: A testable expectation or prediction of a phenomena.

    • Theory: An explanation of a phenomena based on observations. It can be modified as new evidence arises.

    • Scientific Law: A relationship in nature supported by human experiments.

    • Pure Research: Aims to expand knowledge.

    • Applied Research: Focuses on solving specific problems.

    • Model: A visual or verbal explanation of data.

    • Units: A system of measurements.

    • Base Units: A system of fundamental measurements.

    • Derived Units: Units derived from the combination of base units. (e.g., meters per second).

    • Weight: A measure of the amount of matter and the gravitational force exerted on an object.

    • Time: Measured in seconds.

    • Length: Measured in meters.

    • Mass: Measured in kilograms.

    • Temperature: Measured in Kelvin.

    • Volume: The space occupied by an object, measured in liters.

    Module 2

    • Density: Mass per unit volume (mass/volume).
    • Physical Properties: Properties observed without altering a substance (e.g., color, odor, density, mass, solubility, state, melting point, boiling point).
    • Chemical Properties: Properties observed when a substance undergoes a chemical change (e.g., reactivity, flammability, acidity/basicity, chemical composition).
    • States of Matter:
      • Solids: Have a fixed shape and volume. Particles are tightly packed.
      • Liquids: Have a definite volume but take the shape of their container. Particles move past each other.
      • Gases: Have no fixed shape or volume; they take the shape and volume of their container. Particles are widely dispersed.
      • Plasma: A highly energized ionized gas.

    Module 3

    • Element: A pure substance that cannot be broken down into simpler substances by physical or chemical means.

    • Periodic Table: A table that organizes elements based on their atomic number and recurring chemical properties. Elements are arranged in horizontal rows (periods) and vertical columns (groups).

    • Compound: A substance composed of two or more elements chemically combined in a fixed ratio.

    • The Law of Definite Proportions: A compound has the same elements in the same proportions by mass, regardless of the sample size.

    • The Law of Multiple Proportions: When elements combine to form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element will be small whole numbers.

    • Mixtures: A combination of two or more substances not chemically bonded,

    • Homogenous Mixture: The different substances are evenly mixed and not easily distinguishable (e.g., salt water).

    • Heterogeneous Mixture: Different substances are not evenly mixed, and the components are typically visible (e.g., sand and water).

    • Separation Techniques: Techniques used to separate substances in mixtures, such as filtration and distillation.

    Module 4

    • Atomic Theory: Dalton's atomic theory: Elements are composed of extremely small particles called atoms, atoms of a given element are identical, atoms of different elements have different properties, in chemical reactions, atoms are combined, separated, or rearranged to form new substances, atoms cannot be divided, created, or destroyed.

    Module 5

    • Cathode Rays: Streams of negatively charged particles emitted from a cathode in a vacuum tube (later identified as electrons).
    • Plum Pudding Model (Thomson): Atoms are made up of a positively charged sphere with negatively charged electrons embedded within it, like "plums in a pudding".
    • Rutherford's Gold Foil Experiment: Aimed at testing the plum pudding model. Showed, that atoms have a small, dense, positively charged nucleus at their center with negative electrons surrounding it in a largely empty space.
    • Rutherford's Nuclear Model: Atoms have a dense, positively charged nucleus containing most of the mass, with electrons orbiting the nucleus.
    • Alpha Particles: Particles consisting of two protons and two neutrons with a positive charge.
    • Helium Nucleus: Essentially an alpha particle.

    Module 6

    • Bonding: Atoms form compounds by interacting in order to become more stable

    • Ionic Bonds: Electrons are transferred from one atom to another, forming positive and negative ions that are attracted to each other.

    • Covalent Bonds: Atoms share electrons to achieve a stable electron configuration.

    • Lewis Structures: Diagrams that show the arrangement of atoms and their bonds in a molecule.

    Module 7

    • Bond Energy: The energy required to break or form a chemical bond.

    • Covalent Bond Stability: Bonds formed between atoms in order to attain a more stable electron configuration.

    • Atomic Orbitals: Regions in an atom where electrons are most likely to be found.

    • Quantum Numbers: Numbers that describe the properties of atomic orbitals.

    Module 8 (Questions)

    • Periodic Law: The properties of elements are periodic functions of their atomic numbers.

    • Intensive Properties: Properties that are independent of the amount of matter (e.g., density, melting point, boiling point).

    • Extensive Properties: Properties that depend on the amount of matter (e.g., mass, volume, amount of energy).

    • Atom: The smallest unit of an element that maintains its chemical identity.

    • Electron Configuration: The arrangement of electrons in an atom.

    • Quantum: The minimum amount of energy a photon can have or be absorbed by an electron.

    • Periodic Groups: Columns of elements organized in the periodic table that share similar properties.

    • Periods: Rows of elements organized in the periodic table. Elements on a period share increasing atomic numbers.

    • Electron Affinity: The ability of an atom to accept an electron.

    • Electronegativity: The ability of an atom to attract electrons in a chemical bond.

    • Metallic Character: Tendency of an element to lose electrons.

    • Radioactive Elements: elements that decay by emitting radioactive particles.

    • Unstable Elements: Elements that decay and change over time.

    • Chemical Bond: The force of attraction that holds two or more atoms together. (28)

    • Distillation: Separation technique of substances with different boiling points based on their phase changes (liquids to gases).

    • Filtration: Separation technique using a barrier that allows liquids to pass through but traps solids (e.g., through a filter paper).

    • Homogenous Mixtures: Solutions that have uniform composition throughout (e.g., salt water).

    • Heterogeneous Mixtures: Mixtures where the components are not uniformly spread out (e.g., sand and water).

    • Polyatomic ions: A set of several atoms that act as a single unit (e.g., SO42- or hydroxide ion).

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    Description

    Explore the foundational concepts of chemistry in this quiz. Covering matter, mass, scientific methods, and various types of research, this module helps you understand key scientific principles. Perfect for beginners or as a review for advanced students.

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