2058 final review key

Complete the table below with correct answers. The first one is done for you.

PLEASE ANSWER THESE 3 MULTIPLE choices QUESTIONS Q1) What is the total number of electrons in the correct Lewis dot formula of the sulfite ion?  a 8  b 24  c 26  d 30  e 32     Q2) In the Lewis structure for the OF2 molecule, the number of lone pairs of electrons around the central oxygen atoms is  a 0  b 1  c 2  d 3  e 4   Q1) Francium has a higher electronegativity than fluorine.    True  False

Draw the Lewis structures for each of the following compounds as they would appear if one hydrogen (H) was added to the appropriate central atom and the resulting molecule was neutral. Which of your Lewis structures would represent nonpolar molecules (select all that apply)? 1. NH2 2. CC13 3. H 4. CH3 5. OH 6. C₂H3 01 02 3 4 05 06

Solve question 9 please it should be relate to question 8

ONLY QUESTION 7 AND 8 ANSWER PLEASE     Experiment 3: C4H8  1. Attach 2 C atoms in a straight line. Put the double bond between C1 and C2.  2. Attach 2 more C atoms so that the C1C2C3 bond angle is about 120° and the C2C3C4 bond angle is about 109°.  3. Attach toothpicks to indicate the bonds to H atoms to complete the structure.  Question 6 Take a photo and label it P6. Name the structure. Does this structure have any geometric isomers? If so draw and name them. If not, explain why there are no geometric isomers?  4. Now move the double bond so that it is between C2 and C3. Adjust other CCC bond angles appropriately.  Question 7 Take a photo and label it P7. Name the structure. Does this structure have any geometric isomers? If so draw and name them. If not, explain why there are no geometric isomers?  Question 8 Do you need to move the double bond to between C3 and C4 to check for more isomers? Why or why not?

Help filling in Lewis structure graph

Help filling in Lewis structure graph

SCH4U Assignment 7 Name: Hand draw the Lewis structure and VSEPR diagram for the following molecules. Show bond polarity and state the geometric shape and molecular polarity. The first one is done for you. Lewis Structure VSEPR Diagram Shape & Molecular Polarity 1) NH3 2) BeCl2 3) CIO3-1 4) BrCl3 5) CIO21 8+ H d- NHS+ H 6+ - Trigonal pyramidal - Polar

1A U3 Lesson 1 Check for Understanding lonic vs. Covalent Bonds Part ONE: Use the Electronegativity Chart to get the electronegativity values for this practice sheet 1. Determine the type of element in each compound as either metal (M), nonmetal (NM) or metalloid (META) and classify the bond type as lonic, Polar Covalent or Nonpolar Covalent, according to the type of atoms. Identical NM's Different NM's M/NM Nonpolar Covalent Polar covalent lonic 2. Using the table of electro-negativities provided, calculate the difference in electronegativity and then classify the bond type as lonic, Polar Covalent or Nonpolar Covalent according to the EN difference. Nonpolar Covalent 0-0.4 0.41-1.69 > 1.70 Compound SiS₂ NaCl NH3 Li₂O H₂O Ca₂N₂ SO3 H₂ CuF * CH4 Types of Atoms META/NM Polar Covalent lonic Bond Type ? EN Difference 2.5-1.8=.7 Bond Type Polar Covalent FU IM Part TWO: Analysis 1. Do most predictions of bond type using electronegativity match to the prediction of bond type using types of…

Please correct answer and don't use hand rating

Activity 3: Reasoning Challenge Directions: Answer the following questions in 2-3 sentences only. 1. VSEPR theory specifies "valence shell" electrons. Explain why these are the most critical electrons for determining molecular shape? 2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule bef identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.

Please answer part c and b part a is done 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?

Question 5 Which of the following compounds has at least one polar bond but is NOT a polar molecule? (Select ALL that apply) O PCIS O CBra O H;0 O CO2 O CS: O NH3 Question 6 Which of the following molecules are polar? (Select ALL that apply)

I wanna help to answer this question Thanks a lot

Question 4 Select the correct bond angle for each of the following central atoms: NH3 = [Select] PCI= [Select ] NOCI [Select] HNO2 (central atom = N) = HNO2 (central atom = O) = SO3 = [Select] SO₂ = CO₂ = [Select] [Select] CH3OH (central atom = C) CH3OH (central atom = O) = COF2= [Select ] [Select] [Select] ◊ û ✪ = [Select] O [Select] ✪ NH₂CH₂CO₂H (central atom = N) = [Select] NH₂CH₂CO₂H (central atom = CH2) = [Select] NH₂CH₂CO₂H (central atom = CO2) = [Select] ✪ O () () ✪

please answer quickly

Activity 2: The Name is Bond... Chemical Bond Directions: Fill out the table below with correct answers. The first one is done for you. Type of Bond High Boiling Point? High Melting Point? Good conductor of Compound heat or electricity? NaCI ionic Yes Yes Yes CH4 HCI N2 O2 H20 KBr MgCl2 PC3 CO CaF2

Question 4 options:   Draw the Lewis structure of CS2 and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has:       lone pairs,       single bonds,       double bonds,       triple bonds,       atoms with a positive formal charge, and       atoms with a negative formal charge.   Is this structure stabilised by resonance? (Enter either yes or no below - no other words).

Please help!

QUESTION 3 Draw the lewis dot structure of BeCl 2. How many lone-pairs of electrons (first) and bonding pairs of electrons exist on the molecule BeCl 2? Key Concept: Lewis structures are drawn from a knowledge of the total number of electrons from all the atoms involved in the structure. The element with the lowest electronegativity is the central atom. Fulfill octet of outside atoms first.   A 2,2   B 0,3   C 6,3   D 6,2

5 question Consider the molecule shown below. One part of the molecule is missing (shown as a mark). Options A through E shown some chemical groups that could be added in the question mark position. HH H-C-C-O- ? HH Which of the options below will NOT fully satisfy the bonding requirements for the atoms in the molecule? A H B C D E CH3 OH CH₂ COOH

bartleby.com/questions-an = bartleby E Q&A Science / Chemistry / Q&A Library / Chemistry Question Chemistry Question Question Exercise 3.1 1. Explain the formation of bonds in the following compounds a) KBr b) Cal, 2. Draw the bond for the following compounds a) CH, b) CO2 c) HCl d) PCI3 ? Expert Solution This question hasn't been answered yet. Check back soon!

Help, I just need to draw the Lewis structural formula

Identify the correct dipole for the C-F bond in the Lewis structure of fluorobenzene shown using the symbols δ⁺ and δ⁻.   A) (δ⁻)C – F(δ⁻) B) (δ⁺)C – F(δ⁻) C) (δ⁻)C – F(δ⁺) D) (δ⁺)C – F(δ⁺)

Arrange the highlighted bonds in the table below in decreasing order of polarity. That is, pick 1 for the most polar bond, pick 2 for the next most polar bond, and so on. bond polarity H-C-H (Choose one) ▼ H (Choose one) ▼ H H. (Choose one)

(2) Write the preliminary Lewis structure for C2H2 (Figure 35). Place one pair of electron dots between each pair of bonded atomic cores. Figure 35 (3) What is the total number of valence electrons remaining? answer

97. Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments? (a) CIF5 polar bond? [ Select] dipole? [Select] (b) CIO2 polar bond? [Select ] dipole? [ Select ] (c) TeCla2- polar bond? [Select ] dipole? [Select] 99+

I Don't Know Arrange the highlighted bonds in the table below in decreasing order of polarity. That is, pick 1 for the most polar bond, pick 2 for the next most polar bond, and so on bond Br-F: Submit polarity (Choose one) ▼ (Choose one) ▼ (Choose one) ▼ Question 14 X Emmalee 5 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center ? ol Ar Accessib

Please answer

10-8 Organic Compounds synthesized in the laboratory have the same chemical and physical properties as those synthesized in the laboratory.  Chemist have synthesized many organic compounds that are not found in nature. 10-10 Suppose that you are told that organic substances are produced only by living organism. How could you rebut this assertion? 3-86 Both CO2 and SO2 have polar bonds. Account for the fact that CO2 is nonpolar and SO2 is polar?

Can you double check my work please

from highest to lowest, 4 being the lowest. use 1-4 for the answers please