12. How many non-bonding electron pairs are found on the iodine atom in the IBr
ID: 695297 • Letter: 1
Question
12. How many non-bonding electron pairs are found on the iodine atom in the IBr ion? a. 1 b. 2 c. 3 d.4 e. 0 13. What is the formal charge on the iodine atom in the ion in question 12 above? 14. Determine 15. Determine the Lewis structure of PCh, The geometry of this ion would be a. 1 b. 2 e. O the Lewis structure of CH The geometry of this ion would be a. tetrahedral b. trigonal planar c. trigonal pyramidal d. T-shaped a. tetrahedral b. trigonal planar c. trigonal pyramidal d. T a tetrahedral b. trigonal planar c. trigonal pyramidal d. T-shaped e. bent bent 16. Determine the Lewis structure of ICl, The geometry of this ion would be e.bent 17. What is the geometry of sulfur hexafluoride? a. bent b. trigonal planar c. trigonal pyramidal d. square planar e. octahedral 18. What is the formal charge on the nitrogen in NHA? a. 1 b. 2 e. O 19. For a single, double and triple bond, the numbers of bonding electrons in each are, respectively, a. 6,4,2 b. 1,2,3 C. 2,4,6 d. 3,2,1 e. the same The atom could be An atom has 6 valence electrons. a. N 20. b. O c. F d. C e. B Use the following electronegativity values to answer questions 21 and 22. H=2.1 C=2.5 N=3.0 F=4.0 Which would be the most polar covalent bond? a. C-H 21. b. C-N c. C-F d. N-F e. N-H Which would be a non-polar covalent bond? a. C-H 22. c. C-F d. N-F e. F-H b. C-NExplanation / Answer
12) OPTION C
IBr2-, I has 7 valence electrons , two used for two bonds , one gained from negtive charge, leaving 6 non bonded electrons, making 3 lone pairs.
13) Option D
in Ibr2- the formal charge on I is -1
FC = valence electrons - bonded electrons -non bonded electrons
= 7 -2 -6 = -1 for I in Ibr2-
14) OPtion A
CH4 molecule is TETRAHEDRAL with sp3 hybridization (4 bonded e pairs)
15) option C
PCl3 is trigonal pyramidal with P , sp3 hybridisation and one lone pair of electrons.
16) option D
ICl3 is T-shaped as I has 3 bond pairs and 2 lone pairs (sp3dhybridization)
17) option E
SF6 is Octahedral with 6 bond pairs (sp3d2 hybridization)
18) option A
formal charge on N = 5 -4 = +1
19) option C
Each bond comprises of 2 electrons.
20) option B
the element with 6 valence electrons is Oxygen.
21) option D
N-F bond is most polar (4-2.1)
22) Option A
C-H bond is most non-polar (2.5 -2.1)
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