SCH3U PART A LEWIS STRUCTURES WORKSHEET Each of the following molecules contain only single bonds between atoms. i) Predict the structure by comparing the bonding capacity of the atoms. ii) Draw the Lewis Structure for each molecule. a) Cl₂ f) HCI. k) CHCl3 P) CBг4 b) ICI g) CH4 1) S2Cl2 9) P₂H4 c) H₂O h) NF 3 m) Brz r) CF₂Cl₂ d) PH3 i) Cl₂O n) SiF4 s) SeCl₂ e) H₂Sz j) C2H6 o) PC13 t) C3H8

Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.

Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is In this molecule, which is the (a) weakest carbon-containing bond? (b) strongest carbon-containing bond? (c) most polar bond?

8)A) Which of the following bonds is least polar or no polar?a) C-Ob) H-Cc) Cl-Cld) Br-Oe) They are all nonpolarB) Choose the compound with the most ionic bond.a) LiClb) KFc) NaCl d) LiFe) CsFC) Which of the following compounds contains only one unshared pair of valence electrons in its Lewis structure?a) NCl3b) H20c) CH4d) NaCle) PH3

An unknown molecular compound has the following Lewis structure. Which of the following elements could be the identity of X? A) Ne B) O C) C D) Cl E) N

The Lewis structure for which of the following contain the greatest number of lone pairs of electrons? A) CH4.  B) HF   C) F2      d)H2             In CI2, what is the total number of unshared pairs of electrons? A)1 B) 2 C)4 d)6

For each molecule or ion, determine the preferred Lewis structure and use it to predict the molecular shape and bond angles. a)  H3O+ b)  XeF2 c)  I3- d) SNF3 (S central atom) e) POCl3 f) PF3

1) A) In the Lewis structure for IF2–, how many lone pairs of electrons are around the central iodine atom?a) 0b) 1c) 2d) 3e) 4B) The Cl–Xe–Cl bond angle in XeCl4 is closest toa) 90°b) 120°c) 150°d) 360°e) 109°C) Which of the following atoms cannot exceed the octet rule in a molecule?a) Bb) Snc) Pdd) Ie) All atoms exceed the octet rule

Consider the molecule below. XY5 Where X has 7 valence electrons and Y has 7 valence electrons. X has an electronegativity of 2.3 and Y has an electronegativity of 3.2. X and Y are imaginary elements Note: Your answers for b-e must agree with your Lewis structure. a) Draw the Lewis structure b) Does this molecule contain polar bonds? c) Is this a molar molecule? d) Identify the electron geometry e) Identify the molecular geometry (shape) f) Identify the hybridization on the central atom

Draw out Lewis Structures for CO2 and H2O.Using VSEPR Theory make models to represent the two molecules [you do not have to showdouble bonds in your model].From your answer predict the shape of CS2 and H2S. Looking at the Periodic Table predict which of the following molecules will have the sameshape. Using VSEPR theory determine what that shape will be.NCl3 PF3 AlCl3 BrF3