Week_5_Lab-_fill

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

Look at the structure of a soap molecule, and explain what happened when you added soap to your oily hands and put your hands under the water for the solubility lab. Why could you wash the oil off your hands with soap and water? You should use chemistry concepts including structure, polarity, and intermolecular forces to explain your answer. attached is the lewis structure of a basic soap molecule. There are covalent bonds between all carbons, hydrogens, and oxygens. However, there is an ionic bond between oxygen and sodium ions.

Draw the Lewis structure of these compounds and use the electronegativity values, calculate the polarity of the molecules and write if the compounds will be polar, nonpolar, or ionic. Label the + and -next to the atoms of the molecule if they have charge. Also, write the overall dipole.   Cl₂ HCl NH₃ CH₂O CH₄ O₂ CH₂Cl₂ H₂O CH₃Li HCN CH₂CHCl CH₃CH₃ CO₂

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.

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:

Do question 6 and 7 pleas if you cant do both of them just return the question please

Part A) Consider the structural changes that occur in the following molecules. Begin by drawing the best Lewis Structure for each of the following molecules. BH3 CH4 NH3 H2O HF Part B)What are the ideal bond angles for each structure, and which are expected to be distorted? For the ones that are distorted look up on the internet and record their experimental values here:    Part C)According to Lewis and VSEPR theory, why do these changes occur?

< 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 structure of these compounds and use the electronegativity values, calculate the polarity of the molecules and write if the compounds will be polar, nonpolar, or ionic. Label the + and -next to the atoms of the molecule if they have charge. Also, write the overall dipole. HCN CH₂CHCl CH₃CH₃ CO₂

Complete the following table with needed information. Draw the 7 Lewis structures (structural formula). All bonded pairs must be shown with solid lines and all lone pairs with dots. Answer the questions after drawing your structure. If the molecule is polar, show the net dipole with appropriate arrow. See active Fig 9.30 in your book. Water is shown as an example here. Please do not show any calculations here, just the required information. Must show all lone pairs. H₂O CS₂ Ö Electron pair geometry: Tetrahedral Molecular Geometry: Bent Approximate bond angle: 109° Polar or nonpolar: Polar SiH₂O (hint: central atom is Si) Electron pair geometry: Molecular Geometry: Approximate bond angle: Polar or nonpolar: H₂Se Electron pair geometry: Molecular Geometry: Approximate bond angle: Polar or nonpolar: Electron pair geometry: Molecular Geometry: Approximate bond angle: Polar or nonpolar: NO3 Electron pair geometry: Molecular Geometry: Approximate bond angle: Polar or nonpolar: PF3 Electron…

For the structure CIO3 draw a Lewis structure using Cl as the central atom... For the structure that obeys the octet rule which of the following are correct? There are a total of 26 valence electrons There are a total of 24 valence electrons There are a total of 25 valence electrons OCI has one lone pair of electrons CI makes a double bond to one of the oxygens Each O has a -1 formal charge 20 atoms make a double bond to Cl All 30 atoms make a double bond to Cl

1. For each pair of elements listed determine if they will form an ionic (I) or covalent (C) bond.    2.General Properties of Ionic and Covalent Compounds (Use THIS LINK to complete the table)  https://www.thoughtco.com/ionic-and-covalent-compounds-properties-3975966

Please note that "geometry" refers to the molecular or ionic geometry. Recall that for predicting geometry, double and triple bonds count as only one electron pair. The Lewis diagram for NOCI is: 6=N_C: The electron-pair geometry around the N atom in NOCI is There is/are lone pair(s) around the central atom, so the geometry of NOCI is The Lewis diagram for CS₂ is: S=C=S The electron-pair geometry around the C atom in CS2 is There is/are lone pair(s) around the central atom, so the geometry of CS2 is

The Lewis structure of N2H2 shows ________.     a nitrogen-nitrogen triple bond     a nitrogen-nitrogen single bond     each nitrogen has one nonbonding electron pair     each nitrogen has two nonbonding electron pairs     each hydrogen has one nonbonding electron pair

Answer the questions in the table below about the shape of the methanone (H₂CO) molecule. How many electron groups are around the central carbon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central carbon atom? (You may need to use the scrollbar to see all the choices.) (choose one) X S

The molecular structure of ibuprofen, a widely used pain reliever. Ibuprofen has a limited solubility to water, less than 1mg/mL. Identify which part of the molecule contributes to its water solubility and water insolubility.

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:

Draw the Lewis structure of these compounds and use the electronegativity values, calculate the polarity of the molecules and write if the compounds will be polar, nonpolar, or ionic. Label the + and -next to the atoms of the molecule if they have charge. Also, write the overall dipole. CH₄ O₂ CH₂Cl₂ H₂O CH₃Li

C H3C Unshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. The number of unshared pairs at atom a is 0 H3C-N-N N The number of unshared pairs at atom b is a b c B The number of unshared pairs at atom c is The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is 0.

Molecular formula PCI3 Draw Lewis structure for PCI3 What is the electron geometry ? What is the molecular geometry? Is the molecule polar why? What type of intermolecular force will dictate the physical properties of this molecule? Include a “3-D” drawing and dipole arrows in your answer.

What is the chemical formula for ethane? Observe your ethane molecule. Are there any polar covalent bonds present? Based on your answer would you predict that ethane would or would not dissolve easily in water? Now imagine taking off one hydrogen from ethane and adding a hydroxyl group in its place. Draw your completed ethanol molecule below. ouy? Ethanol is an alcohol found in drinks such as beer and wine. Examine this molecule. Are there any polar cov bonds present? Based on your answer, would you predict that ethanol would or would not dissolve easily in water?

11 Name: Maddie Klink Instructor: Lab Day: Models of Organic Molecules Please bring your molecular model kits to lab for the completion of these exercises. Molecular Modeling: This lab is designed to help you become comfortable using model kits to visualize molecular structures in three dimensions. Part I: Answer these questions before doing any work with your model kit 1. How many bonds must each of the following atoms have in order to have no formal charge? 4 valence 1450na a. Carbon b. Hydrogen bond c. Oxygen d. Chlorine 7 valence e. Nitrogen 5 valence Octet H- H Complete octet = 8-4 H 8-S = 3 3bonds 2. Using the information from question #1, determine whether each of the following structures is possible or impossible? (Note that if no formal charges are shown, this implies that all formal charges are zero.) 6 valence Octet = 8.6 H H с-н H 01C C -K = 2 bonas 8-1-1 bond H H H-C Lab Time: H -C-H H H H-C-CI- C-H ++ H H -H HIC C-H H VEUR 1

chemical reaction 1. The equation shows a --the breaking and forming of chemical bonds that leads to a reactant product nonpolar covalent bond polar covalent bond equal to different from hydrogen bond change in the composition of matter. 2. In the equation, CO2 is a 3. In the equation, C6H12O6 is a 4. In O2, the type of bond that holds the two oxygen atoms together is a 5. In H2O, the type of bond that holds one of the hydrogen atoms to the oxygen atom is a 6. The number of oxygen atoms on the left side of the equation is atoms on the right side. the number of oxygen

Write the Lewis structure for the following covalent compounds: Start with the sum of valence electrons, then write the Lewis structure. Once the structure is complete write how many bonding pairs and how many lone pairs are in each structure. PC13 CS2 CBr4