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- Indicate whether each of the following molecules is polar or nonpolar. The molecular geometry is given in parentheses. a. PH2Cl (trigonal pyramidal with P at the apex) b. SO3 (trigonal planar with S in the center position) c. CH2Cl2 (tetrahedral with C in the center position) d. CCl4 (tetrahedral with C in the center position)The following are the general characteristics of polar compounds, except a. low melting point b. low boiling point c. conductivity d. high solubility in waterWhich of the following is TRUE about the properties of covalently-bonded compounds? A The solubility of covalent compounds in water is governed only by molecular weight.B Covalently bonded compounds typically melt at higher temperatures than ionic compounds.C Their melting and boiling points remain the same regardless the molecular weight.D Covalent compounds dissolve in water as molecular compounds, thus the solutions do not conduct electricity.
- Assemble the molecule and answer the following items in this section Elements involved: 1 atom of A (central atom) = from Group IVA; not included in the expanded octet 2 atoms of X (attachment atom) = from Group VIIA; not included in the expanded octet 1 atom of Y (attachment atom) = from Group VIA; not included in the expanded octet The number of single bonds in this molecule is/are: The number of double bonds in this molecule is/are: The number of sigma bonds in this molecule is/are: The number of pi bonds in this molecule is/are: The number of lone pair/s in the central atom of this molecule is/are: The number of lone pair/s in the attachment atom Y of this molecule is/are: The molecular geometry of this molecule is: The bond angle between the bond pairs in this molecule is/are: The formal charge of the central atom is: The formal charge of the whole molecule is:Step 1 – Write the Lewis structure from the molecular formula.Step 2 – Assign an electron-group arrangement by counting all electron groups (bonding plus nonbonding) around the central atom (or around each centralatom, if more than one central atom in structure).Step 3 – Predict the ideal bond angle from the electron-group arrangement and the effect of any deviation caused by lone pairs or double bonds.Step 4 – Name the molecular shape by counting bonding groups and nonbonding groups separately.Step 5 – Predict whether the molecule is polar or nonpolarStep 6 – Describe the hybridization around the central atom and identify the total number of σ and π bonds in the structureAssemble the molecule and answer the following items in this section Elements involved: 1 atom of A (central atom) = from Group VIA; included in the expanded octet 2 atoms of X (attachment atom) = from Group VIA; not included in the expanded octet The number of single bonds in this molecule is/are: The number of double bonds in this molecule is/are: The number of sigma bonds in this molecule is/are: The number of pi bonds in this molecule is/are: The number of lone pair/s in the central atom of this molecule is/are: The number of lone pair/s in the attachment atom Y of this molecule is/are: The molecular geometry of this molecule is: The bond angle between the bond pairs in this molecule is/are: The formal charge of the central atom is: The formal charge of the whole molecule is:
- Which of the following statements is correct? (A) Only neutral molecules can be non-polar, all ions are polar. (B) The net dipole moment of non-polar molecules/ions is 0. (C) All linear molecules are non-polar. (D) All molecules that contains only polar bonds are polar.Calculate the number of shared electrons(S), using the formulaS = N –AWhere N= total no of valence electrons needed by all atoms in the moleculeA= total no of valence electrons available in each atom (remember to add electronsfor negatively charged ions and subtract electrons for positively charged ions Complete the table provided overleaf for the different compounds in the followingway: Calculate the number of shared electrons, Draw the Lewis Dot formula, Determine the electronic geometry of the central atom, Sketch the geometry around the central atom AND Describe the geometry. FORMULA SHARED ELECTRONS LEWIS DOT FORMULA ELECTRON GEOMETRY DESCRIBE THE GEOMETRY NH3 N= A= S= NH4+ N= A= S= PCL6- N= A= S= CH4 N= A= S= H2O N= A= S= H3O+ N= A= S= CO2 N= A= S= S2O32- N= A= S=Match the term that is best defined by the statement provided. Each term has only one best definition. Group of answer choices Two atoms with different electronegativities react to form a compound in which they share electrons. [ Choose ] nonpolar covalent bond polar covalent bond ionic bond hydrogen bond Two or more atoms react to form a stable compound in which electrons are transferred completely from one atom to another. [ Choose ] nonpolar covalent bond polar covalent bond ionic bond hydrogen bond Two completely independent (there has been no chemical reaction between them) polar molecules, each containing atoms with partial charges, can be held together by this kind of bond. [ Choose ] nonpolar covalent bond polar covalent bond ionic bond hydrogen bond The…
- Which one of the following statements is false? a. ionic bonding results from the trnasfer of electrons from one atoms to another b. dipole moments result from the unequal distribution of electrons in a molecule c. the electrons in a polar bond are found nearer to the more electronegative element d. a molecule with very polar bonds can be nonpolar e. linear molecules cannot have a net dipole momentWhich of the following statements could be true regarding polar molecules?Which of the following substances consists of polar covalent bonds but is a non polar molecule? A. Ammonium ion B. boron tribromide C. Phosphorus trichloride D. water