Matter Classification Quiz

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Questions and Answers

Which characteristic is NOT true for pure substances?

  • Have consistent properties
  • Cannot be broken down into simpler substances
  • Can be separated by physical means (correct)
  • Have a uniform composition

Which of the following is an example of a compound?

  • Oxygen
  • Salt (correct)
  • Iron
  • Gold

Which property is NOT associated with metals?

  • Lustrous
  • Malleable
  • Are poor conductors of heat (correct)
  • Conduct heat and electricity

What primarily distinguishes metalloids from metals?

<p>They have intermediate properties (D)</p> Signup and view all the answers

Which of the following describes elements?

<p>Basic form of matter (C)</p> Signup and view all the answers

Which of the following is a property of non-metals?

<p>Poor conductors of heat (B)</p> Signup and view all the answers

What defines a mixture?

<p>A combination of two or more substances that are not chemically bound (A)</p> Signup and view all the answers

Which of the following is NOT a property of metals?

<p>They display a variety of colors (B)</p> Signup and view all the answers

What defines a compound in terms of its components?

<p>Components are combined in fixed proportions. (B)</p> Signup and view all the answers

Which of the following statements about water is correct?

<p>Water is a compound with a fixed mass ratio of 2:16. (A)</p> Signup and view all the answers

How can the components of a compound be separated?

<p>By chemical processes (D)</p> Signup and view all the answers

What is a homogeneous mixture?

<p>A mixture that is uniformly mixed. (B)</p> Signup and view all the answers

Which of the following is NOT a characteristic property of mixtures?

<p>Composed of fixed proportion elements. (A)</p> Signup and view all the answers

Which of the following best describes a heterogeneous mixture?

<p>Components have visible boundaries. (A)</p> Signup and view all the answers

What ratio of hydrogen to oxygen atoms is found in water?

<p>1:8 (C)</p> Signup and view all the answers

What would happen if two elements are mixed but not chemically combined?

<p>They result in a mixture. (C)</p> Signup and view all the answers

What defines a compound in contrast to a mixture?

<p>Formed by chemically combining elements (D)</p> Signup and view all the answers

Which of the following accurately describes the composition of mixtures?

<p>Can have a variable composition (A)</p> Signup and view all the answers

Which method is used to separate the components of a compound?

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

Which of the following properties applies to compounds?

<p>Defined melting and boiling points (D)</p> Signup and view all the answers

What distinguishes homogeneous mixtures from heterogeneous mixtures?

<p>Heterogeneous mixtures have particles larger than 100 nm (B)</p> Signup and view all the answers

Which statement is true regarding alloys?

<p>Alloys cannot be separated into components (A)</p> Signup and view all the answers

Why are solutions classified as homogeneous mixtures?

<p>Particles are uniformly distributed throughout (A)</p> Signup and view all the answers

What is a common characteristic of colloids?

<p>Particles cannot be separated by filtration (C)</p> Signup and view all the answers

What is the correct definition of a solvent?

<p>The component that dissolves the other component. (A)</p> Signup and view all the answers

What does solubility refer to in a solution?

<p>The maximum amount of solute that can dissolve at a specific temperature. (A)</p> Signup and view all the answers

In an solution of 80% ethyl alcohol with 20% water, what is the solute?

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

When 36g of sodium chloride is dissolved in 100g of water at 293 K, which type of solution is created?

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

What would happen to a saturated solution of potassium chloride when cooled to room temperature?

<p>Precipitation of solute may occur. (A)</p> Signup and view all the answers

Which of the following best describes an unsaturated solution?

<p>A solution that can still dissolve more solute. (C)</p> Signup and view all the answers

In terms of mass by mass percentage concentration, if a solution contains 60 g of sugar in 480 g of water, what is the concentration?

<p>12.50% (A)</p> Signup and view all the answers

What effect does increasing temperature generally have on the solubility of solids in liquids?

<p>It increases solubility. (B)</p> Signup and view all the answers

Which statement best describes the nature of a colloid?

<p>It is a blend of components where the dispersed phase is smaller than in a suspension. (B)</p> Signup and view all the answers

What phenomenon describes the scattering of light by colloidal particles?

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

Which of the following is a characteristic of a suspension?

<p>It can scatter light until the particles settle. (C)</p> Signup and view all the answers

What is the main difference between physical and chemical changes?

<p>Physical changes do not alter the identity of substances; chemical changes do. (D)</p> Signup and view all the answers

Which of the following examples best represents an emulsion?

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

Which type of colloid consists of a gas dispersed in a solid?

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

Which of the following statements about dispersed phases and dispersion mediums is true?

<p>The dispersed phase can be solid, liquid, or gas. (A)</p> Signup and view all the answers

What feature distinguishes a colloid from a solution and a suspension?

<p>The size of the dispersed particles. (A)</p> Signup and view all the answers

Which of the following examples represents a chemical change?

<p>Burning of paper (A)</p> Signup and view all the answers

Which statement is true regarding physical changes?

<p>They often involve changes in state, size, or shape. (B)</p> Signup and view all the answers

Which of the following scenarios demonstrates a situation that cannot be reversed?

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

Which of the following is an example of a substance that is in a solid state at room temperature?

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

Which combination correctly identifies a mixture?

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

What is a characteristic of chemical changes compared to physical changes?

<p>They create substances with different properties. (D)</p> Signup and view all the answers

Which of the following processes is not a physical change?

<p>Cooking of food (C)</p> Signup and view all the answers

Which of the following statements about pure substances is accurate?

<p>They have uniform composition throughout. (D)</p> Signup and view all the answers

Flashcards

What is a pure substance?

A substance that is made of only one type of atom or molecule, with a uniform and definite composition, and cannot be separated into other types of matter by physical means.

What is an element?

A pure substance that cannot be broken down into simpler substances by chemical reactions.

What is a compound?

A pure substance formed when two or more elements combine chemically in a fixed ratio.

What is a mixture?

A mixture contains two or more substances that are not chemically combined. The substances in a mixture keep their original properties. Mixtures can be separated by physical means.

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What is a solution?

A homogeneous mixture where one substance (solute) is dissolved in another substance (solvent).

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What is the concentration of a solution?

The amount of solute dissolved in a given amount of solvent. It indicates the strength of the solution.

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What is a physical change?

A change in the physical properties of a substance without changing its chemical composition. It's reversible.

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What is a chemical change?

A change in the chemical composition of a substance, leading to the formation of a new substance. It's usually irreversible.

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How do compound properties differ from their elements?

Compounds have different properties than the elements that make them up.

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How are compounds broken down?

Compounds can only be broken down into their constituent elements through chemical processes, not physical ones.

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What is a Homogeneous Mixture?

A homogeneous mixture has uniform composition throughout, meaning its components are evenly distributed and not visually distinguishable.

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What is a heterogeneous Mixture?

A heterogeneous mixture has non-uniform composition, meaning its components are not evenly distributed and can be visually distinguished.

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How are components in homogenous mixtures separated?

Homogeneous mixtures have components evenly distributed and cannot be separated by simple physical methods such as filtration.

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How are components in heterogeneous mixtures separated?

Heterogeneous mixtures have components unevenly distributed and can be physically separated by methods like filtration.

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What is a true solution?

A type of homogeneous mixture where particles are very small, less than 1 nm, and cannot be separated by filtration. The mixture is transparent and does not scatter light.

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What is a colloid?

A type of homogeneous mixture where particles are larger than in a true solution, between 1-100 nm, and cannot be separated by filtration. The mixture is translucent and scatters light.

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What is a suspension?

A type of heterogeneous mixture where particles are larger than 100 nm and can be separated by filtration. The mixture is opaque and scatters light.

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Solvent

The component that dissolves the other component in a solution.

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Solute

The component(s) that is/are dissolved in the solvent.

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Concentration of a solution

The amount of solute present in a given amount of solution.

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Solubility

The maximum amount of solute that can dissolve in 100 grams of solvent at a specific temperature.

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Saturated solution

A solution where no additional solute can be dissolved at a specific temperature.

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Unsaturated solution

A solution where more solute can be dissolved at a specific temperature.

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Colloidal solution

A solution where particles of a substance are evenly spread throughout.

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Dispersed Phase

The substance present in a smaller proportion in a colloid. It's like the solute in a solution.

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Dispersion Medium

The substance present in a larger proportion in a colloid. It's like the solvent in a solution.

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What is the Tyndall Effect?

The scattering of light by colloidal particles, making the beam visible. It's why fog appears white.

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How does Physical Change affect a substance?

A change in the physical properties of a substance without changing its chemical composition. It's often reversible.

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What are physical changes?

Changes in the physical state, size, or shape of a substance are examples of physical changes. These changes are usually reversible by using a physical process.

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What are chemical changes?

Substances are converted into entirely new substances during chemical changes. These changes are generally irreversible, meaning they cannot be easily reversed.

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Is burning a candle a physical or chemical change?

Burning a candle is a chemical change, as it involves a reaction with oxygen that creates new substances like carbon dioxide and water. These substances are different from the original wax and cannot be easily turned back.

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What is Tyndall Effect?

The Tyndall effect refers to the scattering of light by particles large enough to be seen under a microscope, but not visible to the naked eye. This effect is observed in colloids but not in true solutions.

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Characteristics of Pure Substances

Pure substances have a fixed composition, they consist of only one type of particle, whether it's an element or a compound. The composition throughout the substance is uniform.

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Product of a chemical reaction

The product, A₂B, in the reaction 2A + B → A₂B, is a compound. It won't show the properties of the original elements, it's a different substance. This reaction is irreversible.

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Study Notes

Matter Classification

  • Matter is anything that occupies space and has mass
  • Matter can be classified as pure substances or mixtures
  • Pure substances are made of only one type of atom or molecule
  • Mixtures contain two or more substances that are not chemically bonded

Pure Substances

  • Pure substances have a fixed composition
  • They cannot be separated into simpler substances by physical means, like filtration or distillation
  • Examples include elements and compounds

Elements

  • Elements are the simplest form of matter
  • They cannot be broken down into simpler substances by chemical reactions
  • Elements are made up of only one type of atom
  • Examples of elements include gold (Au), sodium (Na), iron (Fe)
  • Elements are further classified as metals, nonmetals, and metalloids

Metals

  • Metals are typically solids at room temperature
  • They are good conductors of heat and electricity
  • They are malleable (can be hammered into sheets) and ductile (can be drawn into wires)
  • They have a shiny luster or are lustrous
  • Examples of metals include iron, copper, gold, and silver

Nonmetals

  • Nonmetals are not good conductors of heat and electricity
  • They are typically not malleable or ductile
  • They may be solids, liquids or gases at room temperature
  • Examples include hydrogen (H), oxygen (O), nitrogen (N), chlorine (Cl)

Metalloids

  • Metalloids have properties that are intermediate between metals and nonmetals
  • They can be lustrous or dull
  • They are semiconductors (conduct electricity better than nonmetals but not as well as metals)
  • Examples of metalloids include boron (B), silicon (Si), and germanium (Ge)

Compounds

  • Compounds are formed when two or more elements combine chemically in a fixed ratio
  • They have different properties from the elements they are made of
  • Examples of compounds include water (Hâ‚‚O), sodium chloride (NaCl), and carbon dioxide (COâ‚‚)

Mixtures

  • Mixtures are formed when two or more substances are mixed together physically, without any chemical reaction
  • Mixtures do not have a fixed composition and their properties depend on the proportion of the components
  • Mixtures can be homogeneous or heterogeneous

Homogeneous Mixtures

  • Homogeneous mixtures have uniform composition throughout
  • The components are not easily distinguishable
  • Examples include saltwater solutions, sugar dissolved in water, air

Heterogeneous Mixtures

  • Heterogeneous mixtures have non-uniform composition
  • The components are easily distinguishable
  • Examples include sand and water, oil and water, a salad

Solutions

  • Solutions are homogeneous mixtures of a solute and a solvent
  • The solute is the substance that is dissolved, and the solvent is the substance that dissolves the solute
  • Examples of solutions include saltwater, sugar water, and air

Concentration of a Solution

  • Concentration measures the amount of solute present in a given amount of solution
  • Different units for concentration exist, such as mass percentage, volume percentage and molarity

Solubility

  • Solubility is the maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature
  • Solubility can be affected by temperature

Colloids

  • Colloids are heterogeneous mixtures with particles of intermediate size between solutions and suspensions
  • Colloidal particles do not settle out over time and scatter light (Tyndall effect)
  • Examples include milk, fog, and smoke

Suspensions

  • Suspensions are heterogeneous mixtures with large, visible particles suspended in a liquid or gas
  • The particles settle out over time
  • Examples include muddy water and sand in water

Properties of Matter

  • Physical changes do not alter the identity of a substance

  • Chemical changes create new substances

  • Examples of physical changes include melting, freezing, dissolving

  • Examples of chemical changes include combustion and oxidation

The Tyndall Effect

  • The Tyndall effect is the scattering of light by colloidal particles
  • The scattering of light is due to the difference in the size of the particles of the colloid and the wavelength of light

Classification Examples

  • Classify sodium, soil, sugar solution, silver, calcium carbonate, tin, silicon, coal, air, soap, methane, carbon dioxide, and blood into elements, compounds, and mixtures.

Alloy

  • Examples of alloys are mixtures of different metals
  • An example of an alloy is brass, which is a mixture of zinc and copper

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