Electron Groups (EGs) shape 2 Total smallest 90° 120° 180° number angle of bonded atoms shape (B.P) + lone pairs (L.P) on 3. smallest centre 90° 109° 120° angle atom Discuss with your neighbours and provide answers to the following questions. Circle the words that make each statement correct. 1) Each row represents different possible arrangements of that number of electron groups (EG). In each structure, the EGs get [ closer together / further apart ] and the angles between them get [smaller / larger ]. 2) The observed structures adopted by real molecules are those in the thick borders. These structure have the [ smallest / largest ] angles and the EGs are the [ closest together I furthest apart ]. 3) The preferred structure is adopted because this [ minimizes / maximizes ] the [ repulsion / attraction ] felt between all EGs. (Clue: what does VSEPR stand for?)

Electron Groups (EGs) shape 2 Total smallest 90° 120° 180° number angle of bonded atoms shape (B.P) + lone pairs (L.P) on 3. smallest centre 90° 109° 120° angle atom Discuss with your neighbours and provide answers to the following questions. Circle the words that make each statement correct. 1) Each row represents different possible arrangements of that number of electron groups (EG). In each structure, the EGs get [ closer together / further apart ] and the angles between them get [smaller / larger ]. 2) The observed structures adopted by real molecules are those in the thick borders. These structure have the [ smallest / largest ] angles and the EGs are the [ closest together I furthest apart ]. 3) The preferred structure is adopted because this [ minimizes / maximizes ] the [ repulsion / attraction ] felt between all EGs. (Clue: what does VSEPR stand for?)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 7RQ: Define formal charge and explain how to calculate it. What is the purpose of the formal charge?...

See similar textbooks

Similar questions

Use Lewis symbols and Lewis structures to diagram the formationof PF3 from P and F atoms, showing valence-shellelectrons. (a) How many valence electrons does P have initially?(b) How many valence electrons does each F haveinitially? (c) How many valence electrons surround the P inthe PF3 molecule? (d) How many valence electrons surroundeach F in the PF3 molecule? (e) How many bonding pairs ofelectrons are in the PF3 molecule?
✔nk the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest Bolling puint, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D chemical symbol, chemical formula or Lewis structure H H-C-F: H :O: | || HIC-C-F: 1 H H H H :O: | || HIC-C-0-H F₂ boiling point ✓ (Choose one) 1 (highest) 2 34 4 (lowest) (Choose one) ✓ (Choose one) ✓ (Choose one) ✓
Using Lewis symbols and Lewis structures, diagram the formationof SiCl4 from Si and Cl atoms, showing valence-shellelectrons. (a) How many valence electrons does Si have initially?(b) How many valence electrons does each Cl haveinitially? (c) How many valence electrons surround the Siin the SiCl4 molecule? (d) How many valence electrons surroundeach Cl in the SiCl4 molecule? (e) How many bondingpairs of electrons are in the SiCl4 molecule?
Which of the following bonds are polar? C-O, Cl-Cl, O=O, N-H, C-H.(Electronegativites: C = 2.5, H = 2.1, Cl = 3.0, O = 3.5, N = 3.0). In the selected bonds indicatewhich direction the electron density is greatest.
Use the information on the fictious nonmetal elements. to answer the following Element Colomn EN ff 1.9 14 17 3.1 2.3 3.6 15 Nn 16 Shoos one of the followng mokcular compounds and completc the queSTIons: Nn Oyzlshape is benti V) ODraw a leuis Structure Shoudng all lalonce electrons. ) Calculate the electrongativity the bond. State what a paar covalert band, notate the partial difference for Gf bond will form If it is charges d) Detamine if the molecule is polar or polar. non-
4. Explain why the following molecules can NOT existis X
Q:14Draw the Lewis structure for the molecule CHCCH3. How many sigma and pi bonds does it contain?
q, tue 8keltel (ilner bond) Q Poonite thee Durte Nance 8tmeture.
As you go from HF to HI, does the H—X bond become moreor less polar?
The four bonds of carbon tetrachloride (CCl4) are polar, butthe molecule is nonpolar because the bond polarity is canceledby the symmetric tetrahedral shape. When other atoms substitutefor some of the Cl atoms, the symmetry is broken and the mol-ecule becomes polar. Use Figure to rank the fol-lowing molecules from the least polar to the most polar: CH₂Br₂,CF₂Cl₂, CH₂F₂, CH₂Cl₂, CBr₄, CF₂Br
36) Identify the formal charge on the indicated atoms in the following A) SO4²- ; S and O B) CN- ; C and N C) MnO4; Mn and O
4 Which of the following compounds would you expect to have the greatest difference in electronegativity between the two elements? tab hift O LIF O IF O Lil esc caps lock O CsF OLICS O Csl A control ! 1 Q A @ 2 N W S ** # 3 X E H 1 option command D $ 4 C R % 5 F LL M T V MacBook Pro ◆ ^ 6 G Y B & N 7 H U * N 8 J ( - 9 ī M K MOSISO O ) 0 V L com