Unit 1: Alchemy Scientific Method Quiz
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Questions and Answers

What is the first step in the Scientific Method?

  • Observation (correct)
  • Experiment
  • Hypothesis
  • Theory Model

    • A hypothesis is a well-tested explanation that is widely accepted in the scientific community.

    False

    What are significant figures in a measurement?

    All the digits that can be known precisely plus one estimated digit.

    A __________ is a scientific procedure undertaken to make a discovery or test a hypothesis.

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

    Match the following terms with their definitions:

    <p>Hypothesis = A starting point for investigation based on limited evidence Theory = An interpretation of why nature behaves in a certain way Law = Measurable behavior based on observations and experiments Observation = Remark based on something one has seen or heard</p> Signup and view all the answers

    Which of the following types of zeros are not considered significant?

    <p>Leading zeros</p> Signup and view all the answers

    A theory model can be modified based on new evidence from experiments.

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

    What is the role of scientific notation?

    <p>To express numbers as the product of a coefficient and a power of ten.</p> Signup and view all the answers

    Which of the following statements about cations is true?

    <p>Cations have a positive charge and have lost electrons.</p> Signup and view all the answers

    According to Hund's rule, electrons will pair up in orbitals before all orbitals of equal energy are filled.

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

    What is the significance of the Pauli Exclusion Principle in orbital diagrams?

    <p>It states that no two electrons in an atom can have the same set of quantum numbers.</p> Signup and view all the answers

    Anions have a ______ charge and have ______ electrons.

    <p>negative, gained</p> Signup and view all the answers

    Which sublevel is always the lowest energy within a principal energy level?

    <p>s sublevel</p> Signup and view all the answers

    Match the following principles with their descriptions:

    <p>Aufbau Principle = Electrons occupy the lowest energy orbitals first. Hund's Rule = Electrons fill orbitals singly before pairing. Pauli Exclusion Principle = Two electrons in the same orbital must have opposite spins. Excited State = An electron that has absorbed energy and moved to a higher energy level.</p> Signup and view all the answers

    What is the formula to calculate the energy needed to excite an electron to the next energy level?

    <p>E = hv</p> Signup and view all the answers

    What does the atomic number represent?

    <p>The number of protons in an atom</p> Signup and view all the answers

    Electrons have a significant impact on the mass number of an atom.

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

    The speed of light (c) is approximately ______ m/s.

    <p>2.998 x 10^8</p> Signup and view all the answers

    What are cations and how are they formed?

    <p>Cations are positively charged ions formed when atoms lose electrons.</p> Signup and view all the answers

    An atom with the same number of protons but a different number of neutrons is called an __________.

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

    Which of the following scientists proposed the Plum Pudding Model?

    <p>JJ Thomson</p> Signup and view all the answers

    Match the following scientists with their contributions:

    <p>John Dalton = Proposed that atoms are indivisible Ernest Rutherford = Discovered the nucleus Robert Millikan = Measured the charge of the electron Niels Bohr = Developed the planetary model of the atom</p> Signup and view all the answers

    Isotopes of an element have different atomic numbers.

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

    What process occurs when four hydrogen nuclei combine to form one helium nucleus?

    <p>Hydrogen fusion</p> Signup and view all the answers

    What do the negative exponents in scientific notation indicate?

    <p>The number is less than 1</p> Signup and view all the answers

    When multiplying decimals, the answer must always contain the highest number of significant figures.

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

    Define the term 'substance'.

    <p>A particular kind of matter that has a uniform and definite composition.</p> Signup and view all the answers

    Density is the ratio of _____ to volume.

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

    Match the following SI units with their corresponding quantities:

    <p>Length = meter (m) Mass = kilogram (kg) Time = seconds (s) Temperature = Kelvin (K)</p> Signup and view all the answers

    Which of the following is a characteristic of a chemical change?

    <p>Bubbles of gas produced</p> Signup and view all the answers

    A mixture contains only one type of substance.

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

    What is the Law of Conservation of Mass?

    <p>Mass is neither created nor destroyed in a chemical reaction.</p> Signup and view all the answers

    A _____ is a substance that contains two or more elements chemically combined.

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

    Which of the following statements is true regarding isotopes?

    <p>Isotopes are atoms of the same element with differing numbers of neutrons.</p> Signup and view all the answers

    Which bond is primarily formed through the sharing of electrons?

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

    Ionic bonds involve the transfer of electrons between two nonmetals.

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

    What term is used to describe the energy required to break a chemical bond?

    <p>Bond energy</p> Signup and view all the answers

    Covalent compounds are typically found in a __________ state.

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

    Match the following types of hydrocarbons with their characteristics:

    <p>Alkanes = Contain only single bonds Alkenes = Contain one double bond Alkynes = Contain one triple bond Aromatic hydrocarbons = Have six-membered ring with delocalized electrons</p> Signup and view all the answers

    What suffix is used when naming binary ionic compounds?

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

    What is the general formula for alkanes?

    <p>C_nH_(2n+2)</p> Signup and view all the answers

    Polar molecules share their electrons equally between atoms.

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

    Which of the following is the strongest type of intermolecular force?

    <p>Hydrogen bonds</p> Signup and view all the answers

    In hydrocarbons, a __________ bond consists of one shared pair of electrons.

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

    What role do functional groups play in organic molecules?

    <p>Define the chemical and physical properties.</p> Signup and view all the answers

    Match the following functional groups with their formulas:

    <p>Alcohol = -OH Ketone = C=O (carbonyl) Carboxylic Acid = C(=O)OH Ester = C(=O)O-</p> Signup and view all the answers

    Which type of bond can occur between two metals?

    <p>Metallic bond</p> Signup and view all the answers

    Covalent networks have weak intermolecular forces.

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

    What is released during a nuclear reaction compared to a chemical reaction?

    <p>Huge amounts of energy</p> Signup and view all the answers

    Alpha particles contain two electrons and have a negative charge.

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

    What is the time required for one half of the nuclei of a radioisotope sample to decay called?

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

    Nuclear fusion occurs when __________ combine to produce a nucleus of greater mass.

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

    Match the types of radiation to their characteristics:

    <p>Alpha = Low penetrating power, easily blocked by paper Beta = Moderate penetrating power, can be stopped by metal foil Gamma = Very high penetrating power, requires lead or concrete for shielding Positron = Same mass as electron but positively charged</p> Signup and view all the answers

    Which of the following describes a characteristic of beta radiation?

    <p>An electron resulting from the breaking apart of a neutron</p> Signup and view all the answers

    Gamma radiation has a high penetrating power and is easily blocked.

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

    What is the band of stability?

    <p>It's the region where stable nuclei that do not change over time are found.</p> Signup and view all the answers

    The outward pressure of nuclear fusion is balanced by the __________ pull of gravity.

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

    Match the following concepts with their definitions:

    <p>Fission = Splitting of a nucleus into smaller fragments Fusion = Combining of nuclei to form a larger nucleus Nuclear decay = Spontaneous transformation of unstable isotopes Photon = Particles of light that carry energy</p> Signup and view all the answers

    What type of particle is emitted during electron capture?

    <p>Beta particle</p> Signup and view all the answers

    Core electrons are located in the outermost shell of an atom.

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

    What is the maximum number of electrons that can fit in an energy level described by the principal quantum number n?

    <p>2n²</p> Signup and view all the answers

    In the Bohr model, electrons are said to occupy specific __________ around the nucleus.

    <p>energy levels</p> Signup and view all the answers

    Which of the following statements is true about nuclear waste?

    <p>Water is used to cool spent rods and shield against radiation.</p> Signup and view all the answers

    Study Notes

    Unit 1: Alchemy

    • Scientific Method: A systematic approach to observation, measurement, experimentation, and hypothesis refinement.
    • Steps of the Scientific Method: Observation → Hypothesis → Experiment → Theory/Law
    • Theory: An explanation of natural behavior.
    • Law: A description of measurable, observed behavior.
    • Experiment: A scientific procedure performed to discover, test a hypothesis, or demonstrate facts.
    • Hypothesis: A proposed explanation, based on limited evidence, for further testing.
    • Observation: A remark based on something seen, heard, or noticed.
    • Theory Model: A representation to help understand a process.
    • Significant Figures: All known digits plus one estimated digit in a measurement.
    • Significant Figures Rules:
      • Nonzero digits are significant.
      • Leading zeros are not significant.
      • Captive zeros are significant.
      • Trailing zeros are significant only if the number contains a decimal point.
    • Measurement and Scientific Notation: Expressing numbers as a coefficient multiplied by a power of 10.
      • Exponents are positive if the number is greater than 10, negative if less than 1.
    • Significant Figures Operations: In addition/subtraction, the answer has the same number of decimal places as the measurement with the fewest decimal places. In multiplication/division, the answer has the fewest significant figures as the measurement with the fewest significant figures.
    • Dimensional Analysis: A problem-solving method using unit conversions.
      • Start with the desired result, then list givens.
      • Determine conversion factors from SI units.
    • SI Units: Standard units of measure for a given quantity.

    Unit 2: Basic Building Blocks

    • Matter: Anything with mass and volume.
    • Substance: Matter with a uniform and definite composition (e.g., sugar, water).
    • Element: A substance containing atoms of only one type.
    • Atom: Basic unit of an element.
    • Compound: Substance formed by two or more elements chemically combined.
    • Chemical Formula: Symbols representing a compound's composition.
    • Subscripts: Numbers in a chemical formula indicating atom ratios.
    • Physical Properties: Characteristics that can change without changing the substance’s composition (e.g., color, melting point, density).
    • Physical Change: Change in appearance without changing composition.
    • Chemical Properties: Characteristics describing a substance's ability to change to a different substance (e.g., flammability).
    • Chemical Change: Results in a new substance with a different chemical formula.
    • Indicators of a Chemical Change: Gas production, precipitate formation, color change, temperature/energy change.
    • Mixture: A physical blend of two or more substances.
    • Homogenous Mixture: Uniform throughout (e.g., sugar water).
    • Heterogenous Mixture: Not uniform throughout (e.g., blood, concrete).
    • Law of Conservation of Mass: Mass is neither created nor destroyed in a chemical reaction.
    • Subatomic Particles:
      • Neutron: Neutral, in the nucleus, 1 amu.
      • Proton: Positive, in the nucleus, 1 amu.
      • Electron: Negative, electron cloud region, very small mass.
    • Atomic Number: Number of protons in an atom.
    • Mass Number: Number of protons plus neutrons in an atom.
    • Isotope: Atoms of the same element with different numbers of neutrons.
    • Atomic Mass (Weight): Weighted average mass of an element's isotopes.
    • Ion: Atom that has gained or lost electrons.
      • Cation: Positive ion.
      • Anion: Negative ion.
    • Dead Chemists (and their contributions): (List from summary, omit names.)

    Unit 3: Subatomic Particles (Nuclear)

    • Sun Formation: Formation of the Sun from a spinning cloud of gas and dust.
    • Sun Composition: Primarily hydrogen and helium.
    • Nuclear Fusion: Hydrogen nuclei combine to form helium.
    • Chemical Reaction vs. Nuclear Reaction:
      • Chemical: Electrons involved, small energy release.
      • Nuclear: Nuclei involved, huge energy release.
    • Gravitational Equilibrium: Balance between outward pressure and inward gravity in a star.
    • Energy Reaches Earth: Photons carry energy from the sun to Earth (taking a long time).
    • Radiation: Penetrating rays and particles from a radioactive source.
    • Nuclear Forces: Strong attractive forces holding nuclear particles together.
    • Nuclear Binding Energy: Energy released when forming a nucleus.
    • Band of Stability: Range of stable isotopes (protons/neutrons).
    • Half-Life: Time for half of a radioactive sample to decay.
    • Fission: Splitting of a heavy nucleus.
    • Fusion: Combining of light nuclei.
    • Uses of Radioactive Materials: Medical diagnosis, carbon dating, etc.

    Unit 4: A Particulate World - Electron Configuration

    • Bohr Model: Electrons orbit the nucleus in discrete energy levels.
    • Quantum of Energy: Energy needed for an electron to jump between energy levels.
    • Electron Shells (Energy Levels): Discrete regions electrons occupy.
    • Electron Shells Capacity: Maximum number of electrons in a shell (2n^2).
    • Quantum Mechanical Model: Probability of finding an electron around the nucleus, not discrete orbits.
    • Quantum Numbers: Describe the location of an electron around the nucleus.
    • Sublevels (Orbitals): s, p, d, f (Different shapes and energy requirements.)
    • Electron Configurations: Arrangement of electrons in atomic orbitals.
    • Principal Quantum Number(n): Energy level
    • Energy Sublevel (s, p, d, f): orbital type
    • Electron Cloud Shape: Each shape corresponds to a sublevel or orbital
    • Electron Configuration Rules
      • Aufbau: Fill the lowest energy orbitals first
      • Pauli Exclusion: A maximum of 2 electrons per orbital, opposite spins
      • Hund: Fill orbitals singly before pairing electrons.
    • Atomic Spectra: Light emitted when electrons return to ground state.
    • Ground State: Lowest energy electron configuration
    • Excited State: Higher energy electron configuration
    • Properties of Light Relationship Use equations to calculate light properties

    Unit 5: Building with Matter

    • Ions: Atoms that have gained or lost electrons
    • Ionic Bonds: Attraction between (+)/(−) ions
    • Covalent Bonds: Sharing of electrons between atoms
    • Bond Energy: Energy needed to break or form a bond.
    • Bond Length: Distance between bonded atoms.
    • Polyatomic Ions: Ions composed of more than one atom.

    Unit 6: Smells (Covalent Bonding)

    • Empirical Formula: Simplest whole number ratio of atoms in a compound.
    • Molecular Formula: Exact number and types of atoms in a molecule.
    • Naming Covalent Compounds: Use prefixes to indicate the number of each element.
    • Hydrocarbons: Compounds containing only carbon and hydrogen.
    • Hydrocarbon Functional Groups:
      • Alkanes: Single bonds
      • Alkenes: Double bonds
      • Alkynes: Triple bonds
      • Aromatics: Benzene ring structures
    • Functional Groups: Sets of atoms giving specific chemical/physical properties to organic molecules.
    • Hybridization: Mixing atomic orbitals to create new hybrid orbitals.
    • Intermolecular Forces (IMF's): Attractions between molecules (weaker than bonds).
    • Dipole-dipole Forces: Attractions between polarized molecules.
    • Hydrogen Bonds: Particularly strong type of dipole-dipole force.
    • London Dispersion Forces: Weakest intermolecular force caused by temporary electron shifts.

    Unit 7: Tracking Toxins

    • Balancing Chemical Equations: Ensuring equal numbers of atoms on both sides of the reaction arrow.
    • Reactants: Starting substances in a reaction.
    • Products: Substances formed in a reaction.
    • Coefficients: Numbers in front of formulas indicating the number of molecules.
    • Subscripts: Numbers below elements indicating number of atoms in a molecule.

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    Test your understanding of the scientific method and its steps, including observation, hypothesis formulation, experimentation, and theory development. This quiz covers key concepts such as significant figures and the characteristics of scientific theories and laws.

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