Matter: Properties, Conditions, and Phases

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Questions and Answers

Which of the following is an example of a chemical property?

  • Reactivity (correct)
  • Color
  • Malleability
  • Solubility

SATP conditions are primarily used in chemistry and physics for gas law calculations because they represent ideal conditions.

False (B)

List the diatomic elements.

Hydrogen (H), Oxygen (O), Bromine (Br), Fluorine (F), Iodine (I), Nitrogen (N), and Chlorine (Cl)

The modern periodic table is arranged in order of increasing ______.

<p>atomic number</p> Signup and view all the answers

Match the scientist with their contribution to the periodic table:

<p>Dmitri Mendeleev = Organized elements by increasing atomic mass and similar properties. Henry Moseley = Proposed organizing elements by increasing atomic number. Antonie van den Broek = Theorized elements should be arranged based on increasing nuclear charge</p> Signup and view all the answers

Which of the following is NOT a characteristic property of transition metals?

<p>Low melting points compared to other metals (B)</p> Signup and view all the answers

Transuranic elements are naturally occurring elements with atomic numbers greater than 92.

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

Explain why elements in the same group of the periodic table have similar chemical properties.

<p>Elements in the same group have similar chemical properties due to having the same number of valence electrons, which determines how they interact with other elements.</p> Signup and view all the answers

Elements that have properties of both metals and non-metals are classified as ______.

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

Which group of elements most closely follows the periodic law, exhibiting a clear and predictable trend in properties?

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

Flashcards

Physical Property

Observed without changing the substance's composition.

Chemical Property

Observed when a substance changes into a new substance.

Qualitative Properties

Descriptive properties (e.g., color, smell).

Quantitative Properties

Numerical properties (e.g., mass, volume).

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STP Conditions

0°C (273.15 K) and 1 atm (101.325 kPa).

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SATP Conditions

25°C (298.15 K) and 1 bar (100 kPa).

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Diatomic Elements

H, O, Br, F, N, Cl, I exist as two-atom molecules.

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Empirical Knowledge

Knowledge obtained through observation and experimentation.

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Theoretical Knowledge

Knowledge derived from reasoning and theoretical frameworks.

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Metalloids

Elements with properties of both metals and non-metals.

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Study Notes

  • Matter composes all things.

Physical vs. Chemical Properties

  • Physical properties are observed without changing a substance's composition.
    • Examples include solubility and malleability.
  • Chemical properties are observed through changing a substance’s composition.
    • Examples include reactivity and oxidation.

Qualitative vs. Quantitative Properties

  • Qualitative properties are descriptive.
    • An example is color.
  • Quantitative properties are numerical.
    • An example is mass.

Conditions in Chemistry

  • STP (Standard Temperature and Pressure):
    • Temperature: 0°C (273.15 K)
    • Pressure: 1 atm (101.325 kPa)
  • SATP (Standard Ambient Temperature and Pressure):
    • Temperature: 25°C (298.15 K)
    • Pressure: 1 bar (100 kPa)
  • STP is mainly used in chemistry and physics for gas law calculations.
  • SATP is more commonly used in laboratory settings, as conditions are closer to real-world environments.

Phases

  • Common phases: solid (s), liquid (l), gas (g), and aqueous (aq).

Diatomic Elements

  • HOBRFINCL: Hydrogen, Oxygen, Bromine, Fluorine, Iodine, Nitrogen, Chlorine.
  • Diatomic elements are more stable when paired as two atoms.
  • They form covalent bonds to complete their valence electron shells.

IUPAC

  • IUPAC provides the standard for naming chemical compounds.

Organization of the Periodic Table

  • Empirical knowledge is obtained through sense, while theoretical knowledge involves the rationalization of empirical knowledge.
    • Respectively, experimental and non-experimental.
  • Dmitri Mendeleev created the first true periodic table in 1869.
    • Organization was based purely on empirical knowledge.
      • Increasing atomic mass.
      • Arranged based on similar properties.
    • Referred to as ‘Periodic’.
    • Started with 9 elements: Cl, K, Ca, Br, Rb, Sr, I, Cs, Ba.
  • Atomic mass was problematic as it was later determined that structure should dictate properties.

Modern Periodic Table

  • Anton van den Broek (1913) and Henry Moseley theorized elements should be arranged based on increasing nuclear charge (number of protons).
    • This fixed the atomic mass problem.
  • Elements have the same properties because of their subatomic structure: number of valence electrons, energy levels, and protons.
  • The table is organized based on recurring properties of elements from empirical observation.
  • The arrangement is due to understanding of atomic structures, from a theoretical explanation.

Modern Periodic Law

  • Elements arranged in order of increasing atomic number show a gradual change in properties.
    • Example: Group 1 alkali metals' reactivity with water.
  • All elements in a group have similar properties (periodic recurrence).
  • Properties are not exactly the same across a period.
  • Location is helpful in determining atomic structure (valence electrons etc.) and predicting properties of an element.

Metalloids

  • Metalloids are arranged on the periodic table in a staircase formation.
  • Elements have overlapping properties of both metals and non-metals.
  • Do not fit the definition for either metals or non-metals.

Representative Elements

  • Representative elements most closely follow the periodic law.
  • Consist of Groups 1, 2, and 13-18.

Transition Metals

  • Properties include: strong, hard, high melting points, good conductors of electricity, variable reactivity, form ions with variable charges, react with oxygen to form oxides, some react with solutions of strong acids to produce hydrogen gas.
  • Consist of Groups 3-12.

Transuranic Elements

  • Synthetic and not naturally occurring.
  • Atomic number greater than 93, following Uranium.
  • Unstable and decay radioactively.
  • Found in the f-block with actinides.

Atomic Theory and the Periodic Table

  • Elements are arranged by their atomic number, which is the number of protons in the atom.
  • This arrangement shows patterns in their properties, like similar chemical behaviors in columns (groups).
  • Elements in the same group have similar electron configurations.
  • Atomic mass can vary due to isotopes.

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