Determine the number of valence electrons in SO₃ and then draw the corresponding Lewis structure (with minimized formal charges). A) 24 B) 20 C) 25 D) 28 E) 21
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Determine the number of valence electrons in SO₃ and then draw the corresponding Lewis structure (with minimized formal charges).
A) 24
B) 20
C) 25
D) 28
E) 21
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- What is the formal charge of this structureUse VSEPR theory to predict the geometric shapes of the following molecules and ions. Find the formal charges of each atom and explain how you decide the geometric shapes of each molecule. (1H, 15P, 8O, 33As, 51Sb, 17Cl) a) H2PO2– b) AsO3–3 c) OSbClwrite lewis structures for SI4
- Draw the following lewis structures and give the formal charges for the atoms as well as the number of valence electrons A)H2O B)I3 C)IF6+ D)SbF5A new element, Bw, has been identified to be part of Period 10 Group VIIA. Draw the proper structure of the polyatomic ion, BwCl2S3 ^ - . According to VSEPR theory, this ion has a molecular shape of [1]. (Type the shape exactly as written on the table provided to you on the exam data sheet) The formal charge of the Bw atom must be [2]. (Type in the charge including a sign and numberi.e. +1, -1, -2, +2, 0, etc.)Write the Lewis structure of the compound MgO.
- Select the best Lewis structure for P2I4, predict the electron group arrangement of each central atom and the shape of this molecule.Describe the Lewis Structure for an Ion with More Than an Octet of Electrons?18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)
- . Use VSEPR theory to predict the geometric shapes of the following molecules and ions. Find the formal charges of each atom and explain how you decide the geometric shapes of each molecule. (1H, 15P, 8O, ) a) H2PO2–Select structure in which oxygen DOES have a formal charge of +1?Acetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.