Part A Use The Covalent Bonding Tutorial To Answer These Que

Part Ause Thecovalent Bonding Tutorial To Answer These Questionshttps

Part A use The covalent Bonding Tutorial To answer These questions. (Links to an external site.) (Links to an external site.) 1. Explain why you can describe covalent bonding as atoms fighting over electrons. 2-When there is a stable balance between the attractive and repulsive forces between atoms the atoms will form a bond. Describe what happens to potential energy when that happens. Part B Use the Ionic Bonding Tutorial to answer the following questions. (Links to an external site.) (Links to an external site.) 3-What is the formula for the ionic compound formed between calcium ions and fluoride ions? 4-Explain how you can use the mole number (6.02 x 1023) to count atoms. Answer in complete sentences. Give an example to show how to count atoms using the mole number. 5- What is the mass of 1 carbon atom in grams? What is the mass of one dozen carbon atoms in grams? What is the mass of 1 mole of carbon atoms in grams? Show your work or explain how you got the answer. 6- You are given a 10.0 grams sample of ethanol (CH3CH2OH). Explain how you can use the molar mass of ethanol to find the number of ethanol molecules and the number of carbon atoms in the sample. Answer in complete sentences and show your work to receive credit. 7-Determine the Molecular Weight (MW) or Formula Weight (FW) of the following compounds. Show your work to receive credit. CuCl2 copper(II) chloride Al2(SO4)3 aluminum sulfate O2 oxygen gas C2H6 ethane CO2 carbon dioxide CH3OH methanol CH3CHO acetaldehyde

Paper For Above instruction

The questions presented involve fundamental concepts in chemical bonding and molecular calculations, which are essential for understanding chemical structures, reactions, and quantifications. This paper will address each question systematically, providing explanations, calculations, and examples supported by chemical principles and formulas.

1. Covalent Bonding as Atoms Fighting Over Electrons

Covalent bonding can be described as atoms "fighting over electrons" because each atom involved in the bond seeks a stable electron configuration, typically resembling the closest noble gas configuration. atoms have valence electrons that are not fully filled; they tend to attract shared electrons to complete their outer shells. During covalent bonding, atoms essentially compete for shared electrons, with the bonded pair being a result of this "battle." The sharing of electrons allows each atom to attain a more stable, lower-energy state, similar to how individuals compete for resources to improve their stability or status.

2. Potential Energy in Bond Formation

When atoms approach each other and a covalent bond forms, there is a balance between the attractive forces (such as electrostatic attraction between nuclei and shared electrons) and the repulsive forces (due to electron-electron and nucleus-nucleus repulsion). At a certain optimal distance, the potential energy of the system reaches a minimum, indicating a stable bond. As the bond forms, the potential energy decreases from a higher value, reaching a minimum at the point of equilibrium. This minimum potential energy signifies a stable bond because the system releases energy during bond formation and is more stable than the individual atoms before bonding.

3. Formula for Ionic Compound Between Calcium and Fluoride

Calcium (Ca) forms a +2 ionic charge, while fluoride (F) forms a -1 charge. To balance charges, two fluoride ions are needed for each calcium ion. Therefore, the formula of the ionic compound is CaF2.

4. Using the Mole Number (6.02 x 1023) to Count Atoms

The mole is a counting unit in chemistry that represents Avogadro's number, approximately 6.02 x 1023 particles (atoms, molecules, ions). To find the number of atoms in a sample, you first determine how many moles of the substance are present, then multiply by Avogadro's number. For example, if you have 1 mole of carbon atoms, it contains 6.02 x 1023 atoms. Conversely, if you have 2 moles of carbon, you have 2 x 6.02 x 1023 atoms, which equals 1.204 x 1024 atoms.

5. Mass of 1 Carbon Atom and Moles of Carbon

The atomic mass of carbon is approximately 12.01 amu, which equals 12.01 grams per mole.

  • Mass of 1 carbon atom: 12.01 grams / 6.02 x 1023 = approximately 1.99 x 10-23 grams.
  • Mass of one dozen carbon atoms: 12 x 1.99 x 10-23 grams = approximately 2.39 x 10-22 grams.
  • Mass of 1 mole of carbon atoms: 12.01 grams.

6. Calculating Number of Ethanol Molecules and Carbon Atoms in a 10.0 g Sample

Given the molar mass of ethanol (C2H6O) is approximately 46.07 g/mol, the number of moles in 10.0 grams is:

Number of moles = 10.0 g / 46.07 g/mol ≈ 0.217 mol.

Number of ethanol molecules = 0.217 mol x 6.02 x 1023 molecules/mol ≈ 1.31 x 1023 molecules.

Each molecule has 2 carbon atoms, so total carbon atoms:

2 x 1.31 x 1023 ≈ 2.62 x 1023 carbon atoms.

7. Molecular Weight or Formula Weight Calculations

  • CuCl2: Copper (Cu) = 63.55 amu, Chlorine (Cl) = 35.45 amu.

    MW = 63.55 + 2(35.45) = 63.55 + 70.90 = 134.45 g/mol.

  • Al2(SO4)3: Aluminum (Al) = 26.98 amu, Sulfur (S) = 32.07 amu, Oxygen (O) = 16.00 amu.

    MW = 2(26.98) + 3[ (32.07) + 4(16.00) ] = 53.96 + 3(32.07 + 64) = 53.96 + 3(96.07) = 53.96 + 288.21 = 342.17 g/mol.

  • O2: Oxygen gas; 2(16.00) = 32.00 g/mol.
  • C2H6: Ethane; (2 x 12.01) + (6 x 1.008) = 24.02 + 6.048 = 30.07 g/mol.
  • CO2: Carbon dioxide; 12.01 + 2(16.00) = 12.01 + 32.00 = 44.01 g/mol.
  • CH3OH: Methanol; 12.01 + 4(1.008) + 16.00 = 12.01 + 4.032 + 16.00 = 32.04 g/mol.
  • CH3CHO (Acetaldehyde): 12.01 + 3(1.008) + 12.01 + 16.00 = 12.01 + 3.024 + 12.01 + 16.00 = 43.04 g/mol.

Conclusion

Understanding covalent and ionic bonds involves recognizing how atoms share or transfer electrons to attain stable electronic configurations, which release energy and form stable systems. Quantitative analysis such as calculating molecular weight, molar mass, and counting atoms using Avogadro's number is foundational in chemistry for interpreting molecular quantities and reactions. Accurate calculations and interpretations provide insights into the structure, behavior, and interactions of chemical compounds, essential for advancements in chemical research and applied sciences.

References

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