(a)
Interpretation:
The structure of the molecule with a C atom containing two
Concept introduction:
A carbon atom has 4 valence electrons in its outermost shell. Formation of a
(b)
Interpretation:
The structure of the molecule with an N atom containing one
Concept introduction:
The number of valence electrons in N atom is 5. A simple N atom can for 3 single bonds involving 3 valence electrons. The remaining two valence electrons will be lone pair of electrons on the N atom. In double bond there is 1
(c)
Interpretation:
The structure of the molecule with an S atom containing a coordinate covalent bond needs to be determined.
Concept introduction:
There are 6 valence electrons on the S atom. It required 2 more electrons to complete its octet. Thus, it can form 2 single bonds involving 2 electrons. The remaining 4 electrons will act as 2 lone pair of electrons on the S atom.
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LCPO CHEMISTRY W/MODIFIED MASTERING
- There is persuasive evidence for the brief existence of the unstable molecule OPCl. (a) Draw a Lewis diagram for this molecule in which the octet rule is satisfied on all atoms and the formal charges on all atoms are zero. (b) The compound OPCl reacts with oxygen to give O2PCl. Draw a Lewis diagram of O2PCl for which all formal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.arrow_forwardIn addition to ammonia, nitrogen forms three other hy-drides: hydrazine (N₂H₄), diazene (N₂H₂), and tetrazene (N₄H₄).(a) Use Lewis structures to compare the strength, length, and or-der of nitrogen-nitrogen bonds in hydrazine, diazene, and N₂.(b) Tetrazene (atom sequence H₂NNNNH₂) decomposes above 0°C to hydrazine and nitrogen gas. Draw a Lewis structure fortetrazene, and calculate ΔH°ᵣₓₙ for this decomposition.arrow_forwardWhich of the following bonds are polar? Which is the more electronegative atom in cach polar bond? (a) B-F (b) Cl-CI (c) Se-O (d) H–I Arrange the bonds in cach of the following sets in order of inereasing polarity: (a) C-F, O–F, Be-F; (b) 0-CI, S-Br, C-P; (c) C-S, B–F, N-0.arrow_forward
- The molecular ion S3N, has the cyclic structure 'N All S-N bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is –0.375 and on each S atom is +0.041. Show that this result is consis- tent with the overall +1 charge on the molecular ion. Z-Sarrow_forwardWhich of the following statements is correct? (A) Only neutral molecules can be non-polar, all ions are polar. (B) The net dipole moment of non-polar molecules/ions is 0. (C) All linear molecules are non-polar. (D) All molecules that contains only polar bonds are polar.arrow_forwardIdentify the main group to which X belongs in each of the following ionic compound formulas. (a) AlɔX3 (b) X(NO3)2 (c) CaX2arrow_forward
- Draw a Lewis structure for each of the following molecule: (a) chlorodifluoromethane, CHCIF2 (b) propanoic acid C2H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CN ( the framework is H3C-C-N) (d) allene, H2CCCH2arrow_forwardIdentify the electron pair geometry and the molecular structure of each of the following molecules:(a) ClNO (N is the central atom)(b) CS2(c) Cl2CO (C is the central atom)(d) Cl2SO (S is the central atom)(e) SO2F2 (S is the central atom)(f) XeO2F2 (Xe is the central atom)(g) ClOF2+ (Cl is the central atom)arrow_forwardDraw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forward
- Covalent bonds are directional and “saturated”; ionic bonds are “unsaturated” and “non-directional”. (a) Explain why. (b) What are general consequences of the differences in the bonding characteristics?arrow_forwardDraw the Lewis electron dot structures for these molecules, including resonance structures where appropriate:(a) CS32−(b) CS2(c) CS(d) predict the molecular shapes for CS32− and CS2 and explain how you arrived at your predictionsarrow_forwardState whether each of these statements is true or false. (a)A carbon–carbon triple bond is shorter than a carbon–carbonsingle bond. (b) There are exactly six bonding electrons inthe O2 molecule. (c) The C—O bond in carbon monoxide islonger than the C—O bond in carbon dioxide. (d) The O—Obond in ozone is shorter than the O—O bond in O2. (e) Themore electronegative the atom, the more bonds it makes toother atoms.arrow_forward
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