Concept explainers
a)
Interpretation:
The group should be determined to which Z belongs in the following Lewis structure and along with an example of such a compound or ion which actually exists.
Concept Introduction:
Number of lone pair and bond pair electrons on an atom can give the number of valence electrons. This is indicated by the group number of an atom.
Group number is equal to the valence shell electrons of an atom or electrons present in the outermost shell. Valence shell electrons of the atom take part in the bonding.
Formal charge on an atom is defined as the charge assigned to the atom in a molecule. It is assigned to an atom or molecule by assuming that the electrons in
Formal charge is equal to
b)
Interpretation:
The group should be determined to which Z belongs in the following Lewis structure and along with an example of such a compound or ion which actually exists.
Concept Introduction:
Number of lone pair and bond pair electrons on an atom can give the number of valence electrons. This is indicated by the group number of an atom.
Group number is equal to the valence shell electrons of an atom or electrons present in the outermost shell. Valence shell electrons of the atom take part in the bonding.
Formal charge on an atom is defined as the charge assigned to the atom in a molecule. It is assigned to an atom or molecule by assuming that the electrons in chemical bonds are shared equally between atoms, apart from relative electronegativity.
Formal charge is equal to
c)
Interpretation:
The group should be determined to which Z belongs in the following Lewis structure and along with an example of such a compound or ion which actually exists.
Concept Introduction:
Number of lone pair and bond pair electrons on an atom can give the number of valence electrons. This is indicated by the group number of an atom.
Group number is equal to the valence shell electrons of an atom or electrons present in the outermost shell. Valence shell electrons of the atom take part in the bonding.
Formal charge on an atom is defined as the charge assigned to the atom in a molecule. It is assigned to an atom or molecule by assuming that the electrons in chemical bonds are shared equally between atoms, apart from relative electronegativity.
Formal charge is equal to
d)
Interpretation:
The group should be determined to which Z belongs in the following Lewis structure and along with an example of such a compound or ion which actually exists.
Concept Introduction:
Number of lone pair and bond pair electrons on an atom can give the number of valence electrons. This is indicated by the group number of an atom.
Group number is equal to the valence shell electrons of an atom or electrons present in the outermost shell. Valence shell electrons of the atom take part in the bonding.
Formal charge on an atom is defined as the charge assigned to the atom in a molecule. It is assigned to an atom or molecule by assuming that the electrons in chemical bonds are shared equally between atoms, apart from relative electronegativity.
Formal charge is equal to
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Principles of Modern Chemistry
- Draw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.) (a) BrO4 (b) PCl6 (c) XeF6+arrow_forwardA resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.arrow_forward18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)arrow_forward
- The following Lewis diagram represents the valence electron configuration of a main-group element. If this element is in period 4, its valence electron configuration is||arrow_forwardNo Plagirism Please! Group 1 elements have an average electronegativity of 0.84 (not including hydrogen). Group 17 elements have an average electronegativity of 2.99. These two groups often form bonds. Given this information, which kind of bond will they likely form (ionic or covalent), and what evidence supports your claim? If it is ionic, then include which group gives up its electron to the other group. In three to five sentences, explain your reasoning.arrow_forwardWrite electron configurations and Lewis structures for each element. Indicate which of the electrons in the electron configuration are shown in the Lewis structure.(a) Ca(b) Ga(c) As(d) Iarrow_forward
- Draw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+arrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardWrite an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ararrow_forward
- Nat forms an “ionic bond" (i.e. an electrostatic attraction) with the CN- ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN- anion is the sodium cation most likely to attract? Explain.arrow_forwardA compound is being tested for use as a rocket propellant. Analysis shows that it contains 18.54% F, 34.61%Cl, and 46.85% O.(a) Determine the empirical formula for this compound.(b) Assuming that the molecular formula is the same asthe empirical formula, draw a Lewis diagram for thismolecule. Review examples elsewhere in this chapterto decide which atom is most likely to lie at thecenter.(c) Use the VSEPR theory to predict the structure of themolecule from part (b).arrow_forwardThe following Lewis diagram represents the valence electron configuration of a main-group element. This element is in group According to the octet rule, this element would be expected to form a(n) If X is in period 4, the ion formed has the same electron configuration as the noble gas The symbol for the ion is The following Lewis dlagram represents the valence electron configuration of a main-group element. X• e with a charge of This element is in group 1A. According to the octet rule, this element would be expected to form a(n) cation with a charge of If X is in period 3, the ion formed has the same electron configuration as the noble gas The symbol for the ion is The following Lewis diagram represents the valence electron configuration of a main-group element. This element is in group 0 According to the octet rule, this element would be expected to form a(n) The symbol for the ion is with a charge of If X is in period 2, the ion formed has the same electron configuration as the noble…arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning