Name the covalent compounds

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A. Name the covalent compounds 1. B2Si 2. Cl2O5 3. PCl3 4. Cl2O 5. Si2Br6 6. F2O5 B. Name ionic compounds 1. NH4Cl 2. MgS 3. Fe(NO3)3 4. TiBr3 5. Cu3P 6. SnSe2 7. GaAs 8. Pb(SO4)2 9. Be(HCO3)2 10. Mn2(SO3)3 11. Al(CN)3 C. Using electronegative to determine polarity. (Include the equation and type of compound.) A. Name the covalent compounds 1. B2Si 2. Cl2O5 3. PCl3 4. Cl2O 5. Si2Br6 6. F2O5 B. Name ionic compounds 1. NH4Cl 2. MgS 3. Fe(NO3)3 4. TiBr3 5. Cu3P 6. SnSe2 7. GaAs 8. Pb(SO4)2 9. Be(HCO3)2 10. Mn2(SO3)3 11. Al(CN)3 C. Using electronegative to determine polarity. (Include the equation and type of compound.) CO Cl2 HCI

The Correct Answer and Explanation is :

A. Covalent Compounds Naming

  1. B2Si: Diboron monosilicide
  2. Cl2O5: Dichlorine pentoxide
  3. PCl3: Phosphorus trichloride
  4. Cl2O: Dichlorine monoxide
  5. Si2Br6: Disilicon hexabromide
  6. F2O5: Difluorine pentoxide

B. Ionic Compounds Naming

  1. NH4Cl: Ammonium chloride
  2. MgS: Magnesium sulfide
  3. Fe(NO3)3: Iron(III) nitrate
  4. TiBr3: Titanium(III) bromide
  5. Cu3P: Copper(I) phosphide
  6. SnSe2: Tin(IV) selenide
  7. GaAs: Gallium arsenide
  8. Pb(SO4)2: Lead(IV) sulfate
  9. Be(HCO3)2: Beryllium bicarbonate
  10. Mn2(SO3)3: Manganese(III) sulfite
  11. Al(CN)3: Aluminum cyanide

C. Polarity Using Electronegativity

Polarity of a compound can be determined by comparing the electronegativity (EN) values of the atoms involved in a bond. The general rule is:

  • If the difference in electronegativity between two atoms is greater than 1.7, the bond is ionic.
  • If the difference is between 0.4 and 1.7, the bond is polar covalent.
  • If the difference is less than 0.4, the bond is nonpolar covalent.

Steps for Determining Polarity:

  1. Calculate the electronegativity difference.
  2. Determine the type of bond based on the EN difference.
  3. Check if the molecule has any dipole moments (unbalanced charge distribution), which indicates polarity.

Example:

  1. CO (Carbon monoxide):
  • EN of C = 2.55, EN of O = 3.44
  • Difference = 3.44 – 2.55 = 0.89 (polar covalent bond)
  • Since the molecule has a lone pair on oxygen and no symmetrical structure, the molecule is polar.
  1. Cl2 (Chlorine molecule):
  • EN of Cl = 3.16, EN of Cl = 3.16
  • Difference = 0, so the bond is nonpolar covalent.
  • As both atoms are the same, there’s no charge separation, so the molecule is nonpolar.
  1. HCl (Hydrogen chloride):
  • EN of H = 2.20, EN of Cl = 3.16
  • Difference = 3.16 – 2.20 = 0.96 (polar covalent bond)
  • The molecule is polar because of the dipole formed between H and Cl.

Explanation of Concepts:

  • Electronegativity is the ability of an atom to attract electrons in a bond. A greater EN means that atom will pull electrons more strongly.
  • Ionic compounds are formed when there’s a large EN difference (usually greater than 1.7), causing electrons to transfer completely.
  • Covalent compounds have smaller EN differences, with shared electrons. The bond can be polar or nonpolar depending on the difference in EN.
  • For polarity, a molecule is considered polar if it has an uneven charge distribution, which often occurs when there are different types of atoms (unequal sharing of electrons) or if the shape of the molecule is asymmetric.

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