lowing Information to determine the Lewis structure, find the electron and molecular geometry of the molecule, determine the angle of the molecule, and determine the polarity. If the atoms are not the same, you may assume that the difference in their electronegativities are betw 0.4 and 2.0. Atom information: A: 7 valence electrons, CAN exceed the octet. Further from fluorine on the periodic tai than X. X: 7 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic tal than A. Molecule: AX3 Electron Geometry: [Select] Molecular Geometry: [Select] Bond Angle: [ Select ] Polarity: Select]

Use the following information to determine the Lewis structure, find the electron and molecular geometry of the molecule, determine the angle of the molecule, and determine the polarity. If the atoms are not the same, you may assume that the difference in their electronegativities are between 0.4 and 2.0. Atom information: A: 6 valence electrons, CANNOT exceed the octet. Further from fluorine on the periodic table than X. X: 6 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic table than A. Molecule: AX,2- Electron Geometry: [Select] Molecular Geometry: [Select ] Bond Angle: [ Select] Polarity: [Select]

which of the following is the correct for the lewis structure of one phosphorous atom with the appropriate number of hydrogen atoms such that a neutral molecule is formed?

Use the electronegativity values provided to determine which, if any, of the statements below is/are TRUE H: 2.1 C: 2.5 O: 3.5 F: 4.0 Group of answer choices The C-F bond is polar The C-O bond is non-polar The H-F bond is ionic More than one of the above statements is TRUE

Use Lewis theory to determine the formula for the compound that forms between each of the following pairs of elements. Ca and Te Express your answer as a chemical formula.   Mg and Br Express your answer as a chemical formula.   Na and S Express your answer as a chemical formula.   In and O Express your answer as a chemical formula.

i wanna help to complete this table (lewis structure, molecular shap and polar or non polar) table in attachments. thanks you so much

Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar

Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure : H :Z: :Z: N H I H-N-H Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "0,0".

Show how these pairs of elements combine into octet-rule molecular compounds, as in the first example. First, draw their atomic Lewis structures, then use any number of these atoms to build an O.R. molecule, with multiple bonds if needed (you may not add a charge to make it O.R. as an ion!). Draw the O.R. Lewis structure, write its formula and chemical name. Atoms O.R. molecule Formula Name Carbon dioxide •¢. and ö. ö=c=ö CO2 H + Se I + S

Counting available electrons and drawing a Lewis structures