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- Fill in the table. Central atom is listed first. A. Write the number of valence electrons below the formulaB. Draw the Lewis structureC & D. Write the Electron Group Geometry and Molecular Shape NamesE. Write the bond angleF. Write the molecular polarity. "P" for polar and "NP" for nonpolar. SpeciesValenceElectrons(1 pt.) LewisStructure(2 pt.) Electron PairGeometryName(1 pt.) Molecular ShapeName (1 pts.) BondAngle (1 pt.) Molecular Polarity(1 pt.) PO43- NOBr Upload1. Write the chemical formula for a compound containing the following elements: calcium and oxygen; 1:1 A. O2Ca2 B. OCa2 C. OCa D. CaO2 E. Ca2O2 F. O2Ca G. Ca2O H. CaO 2. Calculate ∆En for the following bond and classify it according to type: MgO A. -2.3; ionic B. 2.3; ionic C. -2.3; covalent D. -2.3; polar covalent E. -2.3; nonpolar covalent F. 2.3; polar covalent G. 2.3; covalent H. 2.3; nonpolar covalent I do not undertand how to do this questiosn. Please help These are also the answer chices I have.Which of the following electron configuration pairs would most likely result in covalent bonding? A. 1s2 2s2 2p5 and 1s2 2s2 2p6 B. 1s2 2s2 2p5 and 1s2 2s2 2p5 C. 1s2 2s2 and [Ar] 4s1 D. [Ne] 3s1 and [Ne] 3s1
- 1) What is the type of molecule? a. AX2E3 b. AX3E2 c. AX5 d. AX2E2 2) What is the molecular geometry of GL2-? a. Linear b. Trigonal Bypyramidal c. Bent or v-shaped d. Seesaw 3) What is the approx bond angle formed by L-G-L bond if the correct molecular geometry is followed? a. 180° b. 120° c. 109.5° d. 90° 4) Considering that L is more electronegative than G, and the en difference is 0.2, is the molecular polar? 5) What is the formal charge of G? 6) What is the formal charge of the labeled atom? (refer to the blue arrow)There are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.A covalent bond in which electrons are not shared equally is calleda. polar. b. normal. c. nonpolar.d. neutral.
- Determine the number and type of chemical bonds in silicon tetrachloride (SiCl4) and beryllium sulfide (BeS). 1.) One formula unit of silicon tetrachloride has ___________, (_____________) polar covalent nonpolar covalent ionic bond(s). 2.) One formula unit of beryllium sulfide has ______________, (_____________) polar covalent nonpolar covalent ionic bond(s). Name the following ionic compounds. Example.) ----(a) Cu(ClO)2_______Copper(II) hypochlorite___ (b) Rb3PO3 ____________________(c) Y2Se3______________________In the molecule of SO below, what is the correct number of total sigma and total pi bonds? A two sigma, one pi B three sigma, one pi C two sigma, two pi D four sigma, zero piIdentify the molecular geometry and the polarity of the molecules. Name of the Mlcl Mlclrr geomtry Polarity of the mlcls N2 ? ? Ch4 ? ? NCl3 ? ? H2Co ? ? O3 ? ? ..
- Which of the following has the bonds correctly arranged in order of increasing polarity? Be—F, Mg—F, N—F, O—F O—F, N—F, Be—F, Mg—F O—F, Be—F, Mg—F, N—F N—F, Be—F, Mg—F, O—F Mg—F, Be—F, N—F, O—FGiven the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule.a. BF3b. NH3c. BeCl2d. PCl5*e. OF2f. SF4*g. SF6*h. XeF2*i. SnCl4j. H3O+ Set up your own table to the following formatColumn CharacteristicsA Bonding electronsB Sigma-bondsC Nonbonding electron pairsD Hybrid orbitals havingnonbonding electron pairsE Hybrid orbitals used F 3-D structureG Polar (P) or nonpolar (NP) molecule or ion lewis structure A B C D E F GDraw the Lewis Structure for each covalent system a-e below, and answer the question that follows: Electronegativites: H = 2.1 C = 2.5, B = 2.0N = 3.0, 0 = 3.5 S = 2.5, F = 4.0, Xe = 2.6 a. (OF 2 )Is this molecular POLAR or NONPOLAR? b. (XeF2) What is the geometry of this molecule? c. (SO 3 ^ 2- )What is the polyatomic ion geometry? (Assume "S" obeys octet) d.( CH 2 F 2 )Is this molecular POLAR or NONPOLAR? e.( BF 3 )Is this molecular POLAR NONPOLAR