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- 3-68 Draw a Lewis structure of a covalent compound in which nitrogen has: (a) Three single bonds and one unshared pair of electrons (b) One single bond, one double bond, and one unshared pair of electrons (c) One triple bond and one unshared pair of electrons3-19 Show how each chemical change obeys the octet rule. (a) Lithium forms Li+ ( b) Oxygen forms O2-3-74 Answer true or false. (a) A binary covalent compound contains two kinds of atoms. (b) The two types of atoms in a binary covalent compound are named in this order: first the more electronegative element and then the less electronegative element. (c) The name for SF2 is sulfur difluoride. (d) The name for CO2 is carbon dioxide. (e) The name for CO is carbon oxide. (f) The name for HBr is hydrogen bromide. (g) The name for CCl4 is carbon tetrachioride.
- 3-36 Classify each bond as nonpolar covalent, polar covalent, or ionic. (a) CBr ( b) SCl (c) CP3-20 Show how each chemical change obeys the octet rule. (a) Hydrogen forms W- (hydride ion) (b) Aluminum forms Al3+3-66 Why can’t second-row elements have more than eight electrons in their valence shells? That is, why does the octet rule work for second-row elements?
- 3-63 What is the difference between (a) a bromine atom, (b) a bromine molecule, and (c) a bromide ion? Draw the Lewis structure for each.3-17 Answer true or false. (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency of certain elements to react in such a way that they achieve an outer shell of eight valence electrons. (c) In gaining electrons, an atom becomes a positively charged ion called a cation. (d) When an atom forms an ion, only the number of valence electrons changes; the number of protons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of + 2. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one electron to fill its 3s shell (1s2 2s2 2p63s2). (g) The elements of Group 6A typically react by accepting two electrons to become anions with a charge of 2. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1,2, and 3. (i) Atoms and the ions derived from them have very similar physical and chemical properties.3-70 Draw a Lewis structure of a covalent compound in which oxygen has: (a) Two single bonds and two unshared pairs of electrons (b) One double bond and two unshared pairs of electrons
