Electron-dot-structure-for-sih4

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Question:1)atomic number? 2)atomic mass? 3)number of protons? 4)number of neutrons (in the most stable isotope)? 5)number of electrons? 6)family? 7)period? 8)Sublevel? 9)physical properties (at leats 5)? 10)chemical properties (at least 4)? 11)number of valence electrons? 12)electron configuration? 13)lewis dot structure/diagram?we e "request"14)when was the element discovered? 15)who is credited for the discovery of the element? 16)where is the element found? 17)is it necessary mineral in nutrition? 18)importance in the industry? 19)importance in medicine/health? 20)what do u think about this element? thank you. i know these are alot of questions for a fue points, if you dont have all the answers plz just add the information you know.

Answers:1) 11 2) 23 3) 11 4) 12 5) 11 6) Group 1 - the earth metals 7) 3rd period 8) the sub level i think refers to the sub-level of the valence (outermost) electrons, which would be s 9) Soft, shiny when freshly cut, low melting point (for a metal) ~98C, low density (less than water) 10) Highly reactive with water, oxidises in air (hence why it is only shiny when freshly cut) electrically conductive, paramagnetic (unpaired electron) 11) 1 12) 1s2 2s2 2p6 3s1 13) 14) 1807 15) Humphry Davy 16) Mostly in the form of sodium chloride (table salt) in the oceans and sediments. 17) Yes, it plays roles in the electrical conductivity of your nervous system i believe. 18) It is used as an additive in certain alloys, and as a reactant in certain chemical processes 19) Same as 17) 20) I think it is wonderful. Hope this helps, about the dot-cross, you can probably search google for it. I can't draw on this, and don't really remember what it would look like. It has been a long time since I used Lewis structure.

Question:I would think so as it is two pairs of electrons shared between joining atoms.. Help? 10 points for best answer. Thanks in advance. Also for the electron dot diagram for N2O, is it ok for the atoms to go N O N? The book says N N O, so am I wrong? My way works with a dative bond and single covalent bond on either side of O. Am I wrong? Thanks!!!

Answers:If I understand your way, the nitrogen and oxygen of the dative bond will each have an upaired electron. If you want the O in the middle, you end up with two double bonds N=O=N. The doulb e bonds will be three e- from O and one from N. The reason the real structure is N=N=O has to do with "formal" charge which you may not have studied. In N=O=N the formal charge on O is +2 which is not preferred while in the other it is zero. The other rule of thumb not knowing anything is to put the LESS electronegative atom in the middle. That would be the N.

Question:I read in my chem book that diatomic oxygen is an exception to the octet rule and that it exists with two valence electrons and a single O-O bond. However... after doing some research i learned that both O-O and O=O are inaccurate models of dioxygen and O O is a more accurate depiction. That said, the exam question was: For: (2)C3H6 + (9)O2 -> (6)CO2 + (6)H2O a) balance the equation b) what is the dot structure of the molecules? (i only need to know O2) c) what is the net bond energy? I already took the exam using this dot structure O-O and got 1566 or close to that for the energy. your help would be greatly appreciated...

Answers:::O=O:: Double bond for those bond-energy problems. The bond order in O2 is a double bond. MO theory confirms this but the distinction between the Lewis and MO treatments comes in the prediction of paramagnetism for O2.


From Youtube

6.2 Covalent Bonding.m4v

This is a video going over high school Chemistry notes. Specifically it explains Chapter 6 from the Holt Modern Chemistry book. It explain in this video covalent bonding, bond energy, octet rule, electron dot diagram, lewis structures, single bonds, double bonds, triple bonds, and resonance...

2. Force Laws, Lewis Structures and Resonance

Freshman Organic Chemistry (CHEM 125) Professor McBride begins by following Newton's admonition to search for the force law that describes chemical bonding. Neither direct (Hooke's Law) nor inverse (Coulomb, Gravity) dependence on distance will do - a composite like the Morse potential is needed. GN Lewis devised a "cubic-octet" theory based on the newly discovered electron, and developed it into a shared pair model to explain bonding. After discussing Lewis-dot notation and formal charge, Professor McBride shows that in some "single-minimum" cases the Lewis formalism is inadequate and salvaging it required introducing the confusing concept of "resonance." Complete course materials are available at the Open Yale Courses website: open.yale.edu This course was recorded in Fall 2008.

Lewis Structure (6): Nitrite ion

A simple way to draw the preferred Lewis electron dot structure for the nitrite anion. I simply draw the valence electrons around each atom and place the extra electron on an unpaired electron. When there's more than one unpaired electron, I put it the most electronegative atom. Then, I form bonds to make each atom as "happy" as possible (ie. complete octet). :) I prefer this method to the "add up all valence electrons + add/subtract the charges + distribute accordingly" method that is often taught in general chemistry textbooks. This method doesn't require math or memorization, and it helps you understand formal charges! Oh, it also helps you draw a preferred Lewis structure (with the least amount of formal charge separation) on the first try..... Try this method to draw the preferred structure for sulfate anion (SO42-).

Lewis Structures (2): Water and Ammonia

Chemistry Help! Drawing Lewis electron dot structures for water (H2O) and ammonia (NH3). Instead of using math to account for the valence electrons, I draw all of them on the paper, and "connect the dots!" This way, I don't make silly math mistakes. For more complicated structures, it helps me understand formal charges.


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