Lab Report week 5

Assemble the molecule and answer the following items in this section Elements involved: 1 atom of A (central atom) = from Group IVA; not included in the expanded octet 2 atoms of X (attachment atom) = from Group VIIA; not included in the expanded octet 1 atom of Y (attachment atom) = from Group VIA; not included in the expanded octet The number of single bonds in this molecule is/are: The number of double bonds in this molecule is/are: The number of sigma bonds in this molecule is/are: The number of pi bonds in this molecule is/are: The number of lone pair/s in the central atom of this molecule is/are: The number of lone pair/s in the attachment atom Y of this molecule is/are: The molecular geometry of this molecule is: The bond angle between the bond pairs in this molecule is/are:  The formal charge of the central atom is: The formal charge of the whole molecule is:

< Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and E

Draw the Lewis structures for the following compounds You must show all bonds and lone pairs for the Lewis Structures Assume all atoms EXCEPT HYDROGEN obey the octet rule   CO Lewis Structure: SiS2 (Silicon is the central atom) Lewis Structure: ClO3- (Cl is the central atom)  Assume all atoms obey the octet rule   Lewis Structure: C2H2 Lewis Structure CO32- (Carbon is the central atom) Lewis Structure: O3 assume all atoms obey the octet rule Lewis Structure:

What is a double bond? What is a triple bond? Compare the bond lengths for single, double and triple bonds between two carbon atoms.

Do two single bonds and a double bond meet the characteristics of a carbon atom?

Draw the Lewis Structure for NH2CH2CO2H. Now answer the following questions based on your Lewis structure: (Enter an integer value only.) # single bonds in the entire molecule # double bonds in the entire molecule # lone pairs in the entire molecule

Change the bond between the two carbon atoms in each molecule to a double or triple bond as needed to complete the structure. If the bond should remain a single bond, then you do not need to do anything to the bond. Do not change any other bonds in the molecules.

THIS is the equation N2H4 + O2 → N2 + H2O PLEASE HELP AND LOOK AT THE PICTURE FOR DATA  PLEASE HELP! I REALLY NEED HELP BECAUSE MY TEACHER HASENT TAUGHT ME HOW TO DO THIS PLEASE HELP!!!!!   Balance the equation (if not already balanced) Draw the models of the molecules in the equation, using Lewis structures, ball and stick models or something else that represents each of the atoms and how they are connected.  Identify bonds being formed or broken.  Use bond energy values from below to Calculate the overall energy of the reaction. Determine if the reaction is exothermic or endothermic. Draw a potential energy diagram showing the ∆H, reactants and products. Create one example of mass (g) to mass (g) stoichiometry problem.

Lewis Structure Worksheet #1 Read the Instructions for Drawing Lewis Structures worksheet carefully and draw Lewis structures for each of the following molecules: Group A: Simple Molecules CH4 NC13 NH3 H20 SIF4

Elements such as carbon, hydrogen, and oxygen that occur in biomolecules form stable covalent bonds. What would be the result if the bonds between these atoms were either slightly less or more stable than the naturally occurring bonds?

1. Are covalently bonded compounds good or bad conductors of electricity? Why?

Many organic compounds belong to a category of molecules called "hydrocarbons", meaning that they only contain hydrogen and carbons. An example of a simple hydrocarbon is shown below. Considering both the VSEPR shape of the molecule and electronegativity values of the elements and state whether you expect this simple hydrocarbon to be polar or nonpolar. Explain your answer. нн H-C-C-H нн

Use this condensed chemical structure to complete the table below. CH, — С — О — С — CH, The condensed chemical structure of acetic anhydride Some facts about the acetic anhydride molecule: number of carbon-carbon single (C - C) bonds: number of carbon-hydrogen single (C - H) bonds: number of lone pairs:

Use this condensed chemical structure to complete the table below. OH The condensed chemical structure of phenol. Some facts about the phenol molecule: molecular formula: number of major resonance structures: number of carbon-hydrogen single (C-H) bonds: number of oxygen-hydrogen single (O-H) bonds: number of lone pairs: 0 0 0 0 0

1. Polymers generally have a high stiffness due to their secondary bonds. 2. Metallic bonding is highly directional. 3. Compared with primary bonds, secondary bonds tend to be easily broken. 4. In predominantly ionically bonded materials, the strength of the bond depends on the difference in electronegativity between the two elements. 5. In ionic bond, electrons are shared among atoms. Which of the above statements are false? 1, 3 and 4 1, 2 and 3 1, 2 and 5 2, 4 and 5 3, 4 and 5 O