QUESTION 1 Examine this Lewis structure for the phosphate ion, PO4³-. How many valence electrons are around the P atom in this structure? :0: O-P P=0 :0: Nine Four Eight Twelve None of the above QUESTION 2 List all types of bonding present in the compound CaCO3. I. ionic bond II. polar covalent bond. III. nonpolar covalent bond OI only Oll only Ill only I and II OII and III
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- For GaAs the absolute difference in electronegativity and the type of the bond are respectively: Group of answer choices 0.4, polar covalent 3.6, polar covalent 2.0, ionic 3.6, ionic 1.6, polar covalent 2.0, polar covalent 0.4, ionic 0.4, covalent 1.6, covalentDraw 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 NONPOLARThe following five questions relate to this structure. All bonding pairs have been drawn, but lone pairs have been left out. Which atom(s) is/are expected to carry a partial negative charge in this structure? a. ND and OB b. OB only c. CE only d. CC and CE e. CC only f. ND only How many lone pairs are on Atom D? What is the steric number of atom C? What is the molecular geometry around atom A? a. See-saw b. Trigonal planar c. Tetrahedral d. Square planar Rank the given bond angles from largest to smallest. H—CF—CE OB—CC—CA H—CA—H
- PLEASE ANSWER ALL 1. In your own words, explain why an atom or ion obeys the duet or octet rule is said to have a noble gas configuration of electrons. 2. Which of the following bonds is more polar? Explain: F-O F-C 3. Draw a Lewis Dot Diagram of: a) CH2Cl2 b) Na3N c) ion of S 4. What type of bond would you expect between the following (considering their electronegativity values, shown in parentheses)? Explain: a) A (0.2) and B (3.9) b) Z (2.3) and X (2.4) c) Z (2.3) and B (3.9)Question 1: Draw the Lewis structure AND the 3D structure of the following molecules/ions, specifying the boundary forms of resonance and the resonance hybrid if applicable. Indicate whether the molecule (or ion) is polar or not. d) XeSI4 e) CH2CHCH2COOH f) CH3CCCH2CH3The following five questions relate to this structure. All bonding pairs have been drawn, but lone pairs have been left out. Which atom(s) is/are expected to carry a partial positive charge in this structure? a. ND and OB b. CE only c. CC only d. ND only e. CC and CE f. OB only How many lone pairs are on Atom B? What is the steric number of atom E? What is the molecular geometry around atom D? a. Tetrahedral b. Trigonal planar c. Trigonal pyramidal d. T-shaped Rank the given bond angles from largest to smallest. CC—ND—H CE—CF—H CA—CC—OB
- No plagiarism Please 4. Based on the electron configuration what ion is most likely to form from these atoms? These substances are all three metals. A. -1 B. +1 C. 0- Neutral D. none of these 5. Using the images from question 4, what type of bond is most likely to be formed by these ions? A. ionic B. covalent C. polar covalent D. nonpolar covalentAtom A has 4 valence electrons. Atom Z has 6 valence electrons. For the AZ3-2 ion, answer the following questions about its Lewis dot structure (drawn according to Chm 130 guidelines). a. How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure? e. How many lone pairs are on the central atom in the structure? f. What is the shape of the structure? g. What are the bond angles of this ion?PLEAS HELP ME ASAPP!!!!!!Rightly compare and contrast ionic and covalent compounds.
- Which statement about triple covalent bond is correct? Choose the best answer. A) It involves six valence electrons B) It involves three pairs of valence electrons C) It is a covalent bond in which two atoms share three pairs of valence electrons. D) All of aboveAccording to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible? Question 16 options: a) lone pairs of electrons b) mobile electrons c) inner shell electrons d) bonding pairs of electrons e) pairs of valence electrons1. 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.