Pregunta
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  1. If Ar for Cl is 35.45 , what is the ratio of present in a
    sample of Cl atoms containing naturally occurring Cl ?
  2. Calculate the value of Ar for naturally occurring Cu if the
    distribution of isotopes is and ; accurate
    masses are 62.93 and 64.93 .
  3. Why in question 2 is it adequate to write rather than ?
  4. Calculate Ar for naturally occurring Mg if the isotope distribution
    is and ; accurate masses
    are and 25.98 .

Ask by Gibbs Daniels. in Ghana
Jan 23,2025

Solución de inteligencia artificial de Upstudy

Respuesta verificada por el tutor

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  1. The ratio of is approximately 3.44 : 1.
  2. The atomic mass of naturally occurring copper is 63.56 u.
  3. It’s sufficient to use instead of because the element’s identity is already clear from the chemical symbol.
  4. The atomic mass of naturally occurring magnesium is 24.31 u.

Solución

Let’s address each of your questions step by step:

1. Ratio of in Naturally Occurring Chlorine

Given:
  • Atomic mass of Cl,
  • Isotopes: and
Let:
  • Abundance of =
  • Abundance of =
Calculation:
The atomic mass is the weighted average:
Ratio:
Final Answer:
The natural abundance ratio of is approximately 3.44 : 1.

2. Calculating the Atomic Mass ( ) for Naturally Occurring Copper (Cu)

Given:
  • Isotope distribution:
    • : 69.2%
    • : 30.8%
  • Accurate masses:
    • : 62.93 u
    • : 64.93 u
Calculation:
Final Answer:
The atomic mass of naturally occurring copper is 63.56 u.

3. Notation of Copper Isotopes: Why Suffices

When performing calculations related to atomic masses and isotope abundances, it’s sufficient to denote isotopes by their mass number alone (e.g., ) because the atomic number (which defines the element) is already indicated by the chemical symbol “Cu”. Including the full nuclear notation (e.g., ) is unnecessary for these purposes since the chemistry and mass considerations don’t require information about the number of protons explicitly.
Final Answer:
Including only the mass number (e.g., ) is sufficient because the element’s identity and mass number uniquely specify the isotope, making full nuclear notation unnecessary for atomic mass calculations.

4. Calculating the Atomic Mass ( ) for Naturally Occurring Magnesium (Mg)

Given:
  • Isotope distribution:
    • : 78.99%
    • : 10.00%
    • : 11.01%
  • Accurate masses:
    • : 23.99 u
    • : 24.99 u
    • : 25.98 u
Calculation:
Final Answer:
The atomic mass of naturally occurring magnesium is 24.31 u.

Respondido por UpStudy AI y revisado por un tutor profesional

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Bonus Knowledge

To determine the ratio of in a sample of chlorine, it’s important to remember that natural chlorine is primarily composed of about 75.76% and 24.24% . This leads to a ratio of approximately 3.12:1 when simplifying these percentages. So, if you’re ever in a chemistry jam and need to remember isotope ratios, this handy hint should stick!
When calculating the atomic mass (Ar) for naturally occurring copper, you’re looking at a weighted average based on the percentages and accurate masses provided. The calculation goes like this: . Plugging in those numbers gives you an Ar of approximately 63.55 for copper. It’s like assembling a delicious chemistry smoothie by mixing different isotope “flavors”!

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