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Questions and Answers
What differentiates isotopes of the same chemical element?
What differentiates isotopes of the same chemical element?
Which law states that the total mass remains constant in a closed system?
Which law states that the total mass remains constant in a closed system?
According to Dalton's Atomic Theory, how do atoms of different elements compare?
According to Dalton's Atomic Theory, how do atoms of different elements compare?
What characterizes a polyatomic ion?
What characterizes a polyatomic ion?
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Which of the following elements is categorized as a diatomic ion?
Which of the following elements is categorized as a diatomic ion?
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Which experiment was conducted by Ernest Rutherford?
Which experiment was conducted by Ernest Rutherford?
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What does the Law of Constant Composition state about chemical compounds?
What does the Law of Constant Composition state about chemical compounds?
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How are metal ions typically represented?
How are metal ions typically represented?
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Which statement is true about gases?
Which statement is true about gases?
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What defines an intensive property?
What defines an intensive property?
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What characterizes a compound?
What characterizes a compound?
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Which of the following is an example of a physical property?
Which of the following is an example of a physical property?
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Which type of mixture has components that are evenly distributed?
Which type of mixture has components that are evenly distributed?
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What is true about Bose-Einstein condensate?
What is true about Bose-Einstein condensate?
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What best describes a pure substance?
What best describes a pure substance?
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Which of the following properties is NOT a characteristic of liquids?
Which of the following properties is NOT a characteristic of liquids?
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Which of the following best defines a homogeneous mixture?
Which of the following best defines a homogeneous mixture?
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What is the role of the solute in a solution?
What is the role of the solute in a solution?
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Which method is best suited for separating nonmagnetic solids from magnetic components?
Which method is best suited for separating nonmagnetic solids from magnetic components?
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What component is typically removed when using evaporation to separate a mixture?
What component is typically removed when using evaporation to separate a mixture?
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Which of the following correctly describes ions?
Which of the following correctly describes ions?
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What type of mixture is blood plasma considered to be?
What type of mixture is blood plasma considered to be?
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What does filtration specifically separate in a mixture?
What does filtration specifically separate in a mixture?
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Which of the following best defines a molecule?
Which of the following best defines a molecule?
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What is the correct name for the Fe2+ ion using the Stock Method?
What is the correct name for the Fe2+ ion using the Stock Method?
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Which suffix is used for nonmetal monatomic ions?
Which suffix is used for nonmetal monatomic ions?
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Which of the following describes a ternary polyatomic ion?
Which of the following describes a ternary polyatomic ion?
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What is the name for HCl when dissolved in water?
What is the name for HCl when dissolved in water?
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Which of these compounds is described as being hydrated?
Which of these compounds is described as being hydrated?
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What is the correct name for the polyatomic ion ClO3-?
What is the correct name for the polyatomic ion ClO3-?
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How do you name a transition metal ion with a higher charge according to the classical method?
How do you name a transition metal ion with a higher charge according to the classical method?
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Which of the following is an example of a nonmetal polyatomic ion with fewer oxygen atoms?
Which of the following is an example of a nonmetal polyatomic ion with fewer oxygen atoms?
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Study Notes
States of Matter
- Solid: Definite shape and volume, tightly packed particles in a regular pattern.
- Liquid: Definite volume but no fixed shape, particles can move and are close together.
- Gas: No definite volume or shape, widely separated particles.
- Plasma: No definite volume or shape, widely separated charged particles.
- Bose-Einstein Condensate: Formed when a gas of bosons at low density is cooled to near absolute zero.
Phases Changes
- Melting: Solid to liquid.
- Freezing: Liquid to solid.
- Vaporization: Liquid to gas.
- Condensation: Gas to liquid.
- Sublimation: Solid to gas.
- Deposition: Gas to solid.
Properties of Matter
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Physical Properties: Observable or measurable characteristics of a substance. (e.g., melting ice, changing color, boiling water)
- Intensive Properties: Independent of the quantity of matter. (e.g., density, viscosity, melting point, boiling point)
- Extensive Properties: Dependent on the quantity of matter. (e.g., length, width, height, weight)
- Chemical Properties: Ability of a substance to change into a new substance. (e.g., rusting, burning, decomposition)
Classifications of Matter
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Pure Substance: Unchanging composition, includes elements and compounds.
- Elements: Simplest type of matter, composed of one kind of atom. (e.g., carbon, oxygen)
- Compounds: Two or more elements chemically combined in definite proportions. (e.g., carbon monoxide, water)
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Mixture: Different pure substances physically combined in variable proportions.
- Heterogeneous Mixture: Components are not evenly distributed. (e.g., ice in soda, cereal in milk)
- Homogeneous Mixture: Uniform appearance, properties, and composition throughout. (e.g., perfume, blood plasma)
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Solution: Homogeneous mixture of substances with varying proportions. (e.g., water and salt)
- Solute: Substance that gets dissolved.
- Solvent: Substance present in larger quantities than the solute.
Methods of Separating Mixtures
- Magnets: Removing magnetic solids from nonmagnetic components.
- Decantation: Separating liquid from heavy, insoluble solids.
- Evaporation: Heating a solution to evaporate the liquid, leaving behind the solid.
- Sublimation: Separating volatile solids from nonvolatile substances by heating.
- Filtration: Separating solid from liquid using a filter.
- Distillation: Separating miscible liquids with different boiling points.
- Chromatography: Separating components with different solubilities using a mobile and stationary fluid.
Atoms, Ions, and Molecules
- Atom: Fundamental building block of matter, the smallest indivisible unit of an element retaining its chemical properties. (e.g., hydrogen, oxygen, helium)
- Ion: Electrically charged particle formed when atoms or molecules gain or lose electrons. (e.g., chloride ion, magnesium ion)
- Molecule: Group of two or more atoms chemically bonded together forming a stable, neutral entity. (e.g., hydrogen peroxide, ammonia)
- Isotopes: Atoms of the same element with the same number of protons but different numbers of neutrons. (e.g., Carbon-14, Hydrogen-2)
Fundamental Laws of Chemistry
- Law of Conservation of Mass: Total mass of substances remains constant in a closed system, regardless of changes.
- Law of Constant Composition: A chemical compound always contains the same elements in fixed proportions by mass.
- Law of Multiple Proportions: When two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a simple ratio.
Dalton's Atomic Theory
- Matter is made up of tiny, indivisible particles called atoms.
- Atoms of the same element are identical, but different from other elements.
- Compounds form when atoms of different elements combine in whole number ratios.
- Atoms rearrange during chemical reactions to form new compounds.
Timeline:
- Discovery of electron (J.J. Thompson, 1897)
- Oil drop experiment (Robert Milikan, 1909-1917)
- Gold foil experiment (Ernest Rutherford, 1911)
- Energy levels in atoms (Niels Bohr, 1913)
- Discovery of atomic number (Henry Moseley, 1913-1914)
- Discovery of neutron (James Chadwick, 1932)
Naming Ionic Compounds
- Monatomic Ions: Ions consisting of one atom. (e.g., sodium ion, chloride ion)
- Diatomic Ions: Ions consisting of two atoms. (e.g., oxygen, nitrogen, fluorine, chlorine, bromine, iodine)
- Polyatomic Ions: Ions composed of two or more atoms with a charge. (e.g., sulfate ion, phosphate ion)
Naming Rules for Ionic Compounds
- Metal ions: Named as the element. (e.g., Na+ → sodium)
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Transition Metals:
- Classical Method: Lower charge ends in "-ous"; Higher charge ends in "-ic". (e.g., Fe2+ → ferrous, Fe3+ → ferric)
- Stock Method: Roman numerals indicate the charge in parenthesis. (e.g., Fe2+ → iron (II), Fe3+ → iron (III))
- Non-metal ions: Suffix "-ide" added to the element name for monatomic ions. (e.g, Br → bromide, S → sulfide)
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Non-metal Polyatomic Anions:
- -ite: Lesser oxygen atoms. (e.g., NO2- → nitrite)
- -ate: More oxygen atoms. (e.g., NO3- → nitrate)
- Halogens: Use prefixes to indicate the number of oxygen atoms. (e.g., ClO- → hypochlorite, ClO2- → chlorite, ClO3- → chlorate, ClO4- → perchlorate)
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Ternary Polyatomic Ions: Composed of three elements.
- "bi-": Indicates the presence of hydrogen. (e.g., HCO3- → bicarbonate)
- Greek prefixes: Used to indicate the number of hydrogen atoms. (e.g., H2PO4- → dihydrogen phosphate)
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Hydrated Salts: Compounds with water molecules incorporated in their structure.
- Greek prefixes: Indicate the number of water molecules. (e.g., CuSO4 · 5H2O → copper (II) sulfate pentahydrate)
- Anhydrous Salts: Salts without water molecules. (e.g., CuSO4 → anhydrous copper (II) sulfate)
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Acids: Compounds that release hydrogen ions when dissolved in water.
- Anion name: Prefixed with "hydro-" and suffixed with "-ic" then added "acid" after the name. (e.g., HCl(aq) → hydrochloric acid)
Naming Covalent Compounds
- Covalent Compounds: Formed by two nonmetal atoms. (e.g., carbon dioxide, water)
Naming Rules for Covalent Compounds
- Prefixes: Used to indicate the number of each element. (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-)
- -ide: Suffix added to the second element's name (e.g., carbon dioxide, sulfur trioxide)
- First element: Usually appears first and does not have a prefix if there is only one atom.
- Second element: Suffix "-ide" is added to the element's name.
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Description
Explore the fundamental concepts of states of matter and phase changes with this quiz. Learn about solids, liquids, gases, plasmas, and Bose-Einstein condensates, as well as the physical properties that define them. Test your knowledge on the nature of matter and its transformations.
