assify each statement or molecule as a polar bond or nonpolar bond. Polar bonds the bond between oxygen and hydrogen in water (H2O) Nonpolar bonds one atom has a partial negative charge, and the other atom has a partial positive charge electrons are not equally shared by the atoms in a covalent bond electrons of adjoined atoms are equally distributed between those atoms the bond between nitrogen atoms in diatomic nitrogen (N₂) Answer Bank

A polyatomic ion is composed of C, N, and an unknown element X. The skeletal Lewis structure of this polyatomic ion is [XCN]. The ion X2 has an electron configuration of [Ar]4s23d104p6. What is element X? Knowing the identity of X, complete the Lewis structure of the polyatomic ion, including all important resonance structures.

For each of the following molecules or ion. indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. msp;a.Cl2Ob.NC13c.CCl4d.C2Cl4

Using the symbols and +, indicate the direction of polarity in each polar covalent bond. (a) CN (b) NO (c) CCl

Write chemical formulas for the following binary molecular compounds. a. Iodine monochloride b. Dinitrogen dioxide c. Nitrogen trichloride d. Hydrogen bromide

Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.

For the indicated atom in each of the following molecules or ions. give the number and arrangement of the electron pairs around that atom. msp;a.AsinA3O43b.SeinSeO42c.SinH2S

Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.

Acrylonitrile is the building block of the synthetic fiber Orlon. Acrylonitrile Which carbon-carbon bond is shorter? Which carbon-carbon bond is stronger? Which bond is the most polar? What is the partial negative end of that bond?

7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?