a) Define the following terms:
• Electronegativity
• Bond polarity
• Ionization energy
b) What is the difference between ionic bonds, covalent bonds and polar covalent bonds? Give two examples of each
c) Draw Lewis structures for each of the following:
• BF3
• BF4
• XeF4
• PH3
Your text or notes contain all of these definitions. YOu don't need us to do your homework for that. As the for Lewis structure, we can't draw structures on this forum.
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a)
• Electronegativity is a measure of an atom's ability to attract shared electrons towards itself in a chemical bond. It describes the relative strength of the atom's pull on the shared electrons. Electronegativity is typically measured on the Pauling scale, and the higher the value, the greater the electronegativity of the atom.
• Bond polarity refers to the distribution of electrons between two atoms in a chemical bond. If the electrons are shared equally, the bond is nonpolar. On the other hand, if the electrons are pulled more towards one atom than the other, the bond is polar. Bond polarity is determined by the electronegativity difference between the atoms involved in the bond.
• Ionization energy, also known as ionization potential, is the minimum amount of energy required to remove an electron from a neutral atom or positive ion in its ground state. It quantifies the energy required to convert a stable, neutral atom into a charged ion.
b)
• Ionic bonds form between atoms with a large difference in electronegativity. In an ionic bond, one atom completely transfers its electron(s) to another atom, resulting in the formation of ions that are held together by electrostatic interactions. Examples of ionic compounds include sodium chloride (NaCl) and magnesium oxide (MgO).
• Covalent bonds form when electrons are shared between two atoms. In a covalent bond, both atoms contribute one or more electrons to the shared electron pair. Examples of covalent compounds include methane (CH4) and nitrogen gas (N2).
• Polar covalent bonds occur when there is a significant difference in electronegativity between the atoms involved. Although the electrons are shared, they are not shared equally, resulting in a partial positive charge on one atom and a partial negative charge on the other. Examples of polar covalent compounds include water (H2O) and hydrogen fluoride (HF).
c)
Below are the Lewis structures for each of the compounds:
• BF3: B represents Boron, and F represents Fluorine. The Lewis structure would have B in the center and three F atoms attached to it, each sharing a single bond with Boron.
• BF4: B represents Boron, and F represents Fluorine. The Lewis structure would have B in the center with four F atoms attached to it, each sharing a single bond with Boron, and one of the F atoms having a lone pair of electrons.
• XeF4: Xe represents Xenon, and F represents Fluorine. The Lewis structure would have Xe in the center with four F atoms attached to it, each sharing a single bond with Xenon, and two of the F atoms having a lone pair of electrons.
• PH3: P represents Phosphorus, and H represents Hydrogen. The Lewis structure would have P in the center with three H atoms attached to it, each sharing a single bond with Phosphorus, and Phosphorus having a lone pair of electrons.