Concept explainers
(a)
Interpretation:
Whether the
Concept introduction:
For any molecule to be paramagnetic in nature, there must be unpaired electrons present in it.
(b)
Interpretation:
Whether the
Concept introduction:
For any molecule to be paramagnetic in nature, there must be unpaired electrons present in it.
(c)
Interpretation:
Whether the
Concept introduction:
For any molecule to be paramagnetic in nature, there must be unpaired electrons present in it.
(d)
Interpretation:
Whether the
Concept introduction:
For any molecule to be paramagnetic in nature, there must be unpaired electrons present in it.
(e)
Interpretation:
Whether the
Concept introduction:
For any molecule to be paramagnetic in nature, there must be unpaired electrons present in it.
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CHEMISTRY-MOD.MASTERING (18W)
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- Which of the following molecules does not have a dipole moment? (a) CH3Cl (b) CH2Cl2 (c) CFCl3 (d) CHCl3arrow_forwardThe molecular orbitals depicted below are derived from 2p atomic orbitals in F₂⁺. (a) Give the orbital designations. (b) Which is occupied by at least one electron in F₂⁺? (c) Which is occupied by only one electron in F₂⁺?arrow_forwardWhich molecule contains an atom with an unhybridized p orbital in its valence shell? (a) (b) b (c) (d) с b a d NH₂ H₂Oarrow_forward
- Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forwardThe lactic acid molecule, CH3CH(OH)COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many π and howmany σ bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?arrow_forwardIf an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.arrow_forward
- 15. Which of the following species is not likely to have a tetrahedral shape? (a) SiBr4 (b) NF4+, (c) SF4, (d) BeCl4–2, (e) BF4–, (f) AlCl4–arrow_forward10.What is the hybridization of the central atom in each of the following? (a) BeH2 (b) SF6 (c) PO43− (d) PCl5arrow_forward(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a π*2p molecular orbital, or (iii) The π*2pMO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forward
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