Concept explainers
(a)
Interpretation:
The total number of electron dots that has to appear in Lewis structure for
Concept Introduction:
Lewis structure clearly depicts the bonding and nonbonding electrons in the atom. This is only partially useful for the molecule that contains one or more multiple bonds and when coordinate covalent bond is present in the molecule. For drawing Lewis structure a systematic procedure is followed. They are,
- The total number of valence electrons that is present in molecule is calculated by adding all the valence electrons of the atoms present in the molecule.
- The chemical symbols for the atoms that is present in the molecule is written in the order that they are bonded. After this a single covalent bond is placed between each atoms as two electrons.
- The nonbonding electrons are added to each atom that is bonded to the central atom so that it contains octet of electrons. For hydrogen alone the “octet” is only two electrons.
- The remaining electrons has to be placed on the central atom in the structure.
- If there is no octet of electrons present in the central atom, then use one or more pairs of nonbonding electrons that is bonded to the central atom to form double or triple bonds.
- The positive or negative charge that is present on the ion is adjusted by increasing or decreasing the number of electrons in the polyatomic ion.
(b)
Interpretation:
The total number of electron dots that has to appear in Lewis structure for
Concept Introduction:
Lewis structure clearly depicts the bonding and nonbonding electrons in the atom. This is only partially useful for the molecule that contains one or more multiple bonds and when coordinate covalent bond is present in the molecule. For drawing Lewis structure a systematic procedure is followed. They are,
- The total number of valence electrons that is present in molecule is calculated by adding all the valence electrons of the atoms present in the molecule.
- The chemical symbols for the atoms that is present in the molecule is written in the order that they are bonded. After this a single covalent bond is placed between each atoms as two electrons.
- The nonbonding electrons are added to each atom that is bonded to the central atom so that it contains octet of electrons. For hydrogen alone the “octet” is only two electrons.
- The remaining electrons has to be placed on the central atom in the structure.
- If there is no octet of electrons present in the central atom, then use one or more pairs of nonbonding electrons that is bonded to the central atom to form double or triple bonds.
- The positive or negative charge that is present on the ion is adjusted by increasing or decreasing the number of electrons in the polyatomic ion.
(c)
Interpretation:
The total number of electron dots that has to appear in Lewis structure for
Concept Introduction:
Lewis structure clearly depicts the bonding and nonbonding electrons in the atom. This is only partially useful for the molecule that contains one or more multiple bonds and when coordinate covalent bond is present in the molecule. For drawing Lewis structure a systematic procedure is followed. They are,
- The total number of valence electrons that is present in molecule is calculated by adding all the valence electrons of the atoms present in the molecule.
- The chemical symbols for the atoms that is present in the molecule is written in the order that they are bonded. After this a single covalent bond is placed between each atoms as two electrons.
- The nonbonding electrons are added to each atom that is bonded to the central atom so that it contains octet of electrons. For hydrogen alone the “octet” is only two electrons.
- The remaining electrons has to be placed on the central atom in the structure.
- If there is no octet of electrons present in the central atom, then use one or more pairs of nonbonding electrons that is bonded to the central atom to form double or triple bonds.
- The positive or negative charge that is present on the ion is adjusted by increasing or decreasing the number of electrons in the polyatomic ion.
(d)
Interpretation:
The total number of electron dots that has to appear in Lewis structure for
Concept Introduction:
Lewis structure clearly depicts the bonding and nonbonding electrons in the atom. This is only partially useful for the molecule that contains one or more multiple bonds and when coordinate covalent bond is present in the molecule. For drawing Lewis structure a systematic procedure is followed. They are,
- The total number of valence electrons that is present in molecule is calculated by adding all the valence electrons of the atoms present in the molecule.
- The chemical symbols for the atoms that is present in the molecule is written in the order that they are bonded. After this a single covalent bond is placed between each atoms as two electrons.
- The nonbonding electrons are added to each atom that is bonded to the central atom so that it contains octet of electrons. For hydrogen alone the “octet” is only two electrons.
- The remaining electrons has to be placed on the central atom in the structure.
- If there is no octet of electrons present in the central atom, then use one or more pairs of nonbonding electrons that is bonded to the central atom to form double or triple bonds.
- The positive or negative charge that is present on the ion is adjusted by increasing or decreasing the number of electrons in the polyatomic ion.
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Chapter 5 Solutions
General, Organic, and Biological Chemistry
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- a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.arrow_forwardWhat main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.arrow_forwardDraw Lewis structures for the following molecules or polyatomic ions. a. SO3 b. SO32arrow_forward
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