🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →

HomeStudy Guides420,000CA160,000

CHEM 1A03 Study Guide - Midterm Guide: Valence Bond Theory, Lone Pair, Lewis Structure

144 views6 pages

28 Jun 2016

School

McMaster University

Department

Course

Professor

For unlimited access to Study Guides, a Grade+ subscription is required.

itsmealionline and 39769 others unlocked

CHEM 1A03 Full Course Notes

CHEM 1A03 Full Course Notes

Document Summary

Ionic bonding is the electrostatic attraction between positive and negative ions in the crystal lattice of a salt. Covalent bonding is the sharing of valence electrons between atomic nuclei within a molecule. Use the last digit of the group number from the periodic table to determine the number of valence electrons for each atom. Place one electron on each of the four sides of an imaginary rectangle enclosing the central atom before pairing any electrons. If there are more than four valence electrons, pair up the electrons as required to place all of the valence electrons. Lewis symbols closely correspond closely with electron configurations: Electrons pair up four pairs arise from s and p orbitals. Arrange atoms symmetrically around the central atom (generally listed first in formula). Count the number of valence electrons of all atoms in the compound. [for polyatomic ions, add electrons corresponding to the negative charge, and subtract electrons corresponding to the positive charge. ]

Related textbook solutions

Chemistry: Structure and Properties

ISBN: 9780134293936

Basic Chemistry

ISBN: 9780134138046

Principles of Chemistry Molecular Approach

ISBN: 9780134112831

Principles of Chemistry Molecular Approach

3rd Edition, 2014

ISBN: 9780321971944

Chemistry: Structure and Properties

ISBN: 9780134293936

Chemistry: A Molecular Approach

ISBN: 9780321809247

Chemistry: A Molecular Approach

ISBN: 9780134874371

Principles of Chemistry: A Molecular Approach

ISBN: 9780134895741

Chemistry: The Central Science

14th Edition, 2017

ISBN: 9780134414232

Related Documents

CHEM 1A03 Lecture Notes - Lecture 10: Beryllium, Electronegativity

byzantiumgrasshopper187

CHEM 1A03 Lecture Notes - Beryllium, Electronegativity

byzantiumgrasshopper187

CHEM 1A03 Chapter Notes - Chapter 10: Octet Rule, Formal Charge, Lewis Acids And Bases

Related Questions

STRC 434: Wricing Lewis Symbols and Lewis Strucnures (4) Write the Lewis structure for the ionic com 5. Construct the Lewis structure model for the cova pound potassium chioride in the box. lent compound sulfur difluoride (SF2) using the tollow ing steps (1) atom is The number of valence electrons in the sulfur . The total number of valence electrons is the total Lewis structure of potassium chloride How does the written Lewis structure for po, in the two fluorine atoms isHence number ol valence electrons in SF's (5) tassium chioride differ from that ot hydrogen chloride? (2) Arrange the atomic cores for the two fluorine atoms with the sultur atom as the central atom in the space below. (3) Rewrite the atomic cores in the space below. Place an electron pair between each fluorine and sulfur core. Write the Lewis structure for SF2 in the box, lent compound hydrogen sulfide (H2S) using the fol- distributing the remaining valence electrons so that all 4. Construct the Lewis structure model for the cova- (4) lowing steps. three atoms are in accordance with the octet rule. (1) The total number of valence electrons in the two hydrogen atoms is ; the sulfur atom has Hence, the total number of valence electrons in the compound is Lewis structure of SF2 (2) Write the atomic cores for the hydrogen atoms and the sulfur atom in the space below. Because sulfur is the central atom in this molecule, ar- range the cores so that the hydrogen atoms are on ei ther side of the sulfur atom. 6. Construct the Lewis structure model for the cova- lent compound methylene chloride (CH2C) The number of valence electrons in the car- The total number of valence elec (1) bon atom is trons in the two hydrogen atoms is number of valence electrons in the two chlorine atoms is trons in CH2C12 is The total (3) Rewrite the atomic cores in the space below. Place an electron pair between each hydrogen atom and the suilfur atom. Hence, the total number of valence elec- (2) Position the atomic core for carbon as the (4) Write the Lewis structure for hydrogen sulfide central atom in the space below, and place the other in the box, distributing the remaining valence electrons cores around it so that the hydrogen atoms are in accordance with the duet rule and the sulfur atom is in accordance with the octet rule. (3) Rewrite your arrangement of atomic cores ir the space below, joining the cores with electron pairs to form the necessary bonds. Lewis structure of H2S

Construct the Lewis structuremodel for the covalent compound carbontetrachloride (CCl4) using the following steps.
1)The total number of valence electrons in CCl4 is ____.
2)Write the atomic core for the element that seems most likely tobe the central atom in the moleculein the space below. Position theremaining atomic cores around it.
3)Place an electron pair between each of the bonding atoms.
4)After distributing the remaining valence electrons so that thecarbon and each chlorine atom has an electron octet, write thelewis structure for CCl4 in the box.

viridianleopard15

STRC 454 riring Lewis Symibols and Lewis Senacesres Write the Lewis structure for the ionic com . Construct the Lewis structure modet for the cova pound potassium chloride in the box lent compound sulfur aifluoride (SF,) using the follow ing steps 1) The number of valence electrons in the sulfur The total number of valence electrons . Hence, the total Lewis structure of potassium chloride in the two fluonine atoms is number of valence clectrons in SF, is (5) tow does the written Lewis structure for po. ã tassum chlor de difor from that of hydrogen chionde? (2) Arrange the atormic cores for the two fluonine atoms with the suifur atom as the central atom in the space below. 13) Rewnibe the atomic cores in the space below Place an electron pair between each fluorine and sultfur 4, Construct the Lewis sructure model for the cova- ent compound hydrogen sulide (4,S) using the tol distributing the remaining valence electrons so that all owing steps (4) Write the Lewis structure for SF2 in the box, three atoms are in accordance with the octet rulo. (1) two hydrogen atoms is The total number of valonce electrons in the ; the sulfur aom has Hence, the total number of valence electrons in the compound is Leis sructure of SF2 (2) Write the atomic cores for the hydrogen atoms and the sultur below. 6. Construct the Lewis structure model for the cova atom in the space Because sulfur is the central atom in this moleculeÂ·ar. range the cores so that the hydrogen atoms are on e- lent compound methylene chioride (CHC17). (1) The number of valence electrons in the car- The total number of valence elec- trons in the two hydrogen atoms is The total 3) Rewnte the atomic cores in the space below number of valence electrons in the two chiorine atoms Henoe, the total number of valence elec- ther side of the suifur atom bon atomis Place an electron pair betwoon each hydragen atom is and the sultr atom _ trons in CH,C, is (2) Postion the atomic core for carbon as the (4) Write the Lewis structure for hydrogen sultide central atom in the space below, and place the ather in the box, distmbuting the remainingvaience electrons cores around it so that the hydrogen atoms are in accordance wth the duet rule and the sultur atom is in accordance with the actet rule (3) Rewrite your arrangement ot atomic cores in the space below, joiring the cores with electron pairs to form the necessary bonds Lewis structure of HS