5 Written Questions
5 Matching Questions
- 5 ED
- Electronegativity and Polarity
- Drawing Lewis Structures
- Nonpolar Covalent
- a The greater the electronegativity difference between two atoms the more polar the bond.
- b 1) Total the valence electrons of all bonded atoms. (- means you add electrons, + means you subtract electrons)
2) Use one pair of electrons to bond each outer atom to the central atom.
3) Complete the octets around all of the outer atoms.
4) Place any remaining electrons on the central atom.
5) If there are not enough electrons to give the central atom an octet, make multiple bonds.
- c Orbital Hybridization dsp3
- d 0-0.4
- e >2.0
5 Multiple Choice Questions
- Orbital Hybridization sp3
- A bond in which the electrons are shared equally between two atoms.
- The arrangement of electron domains around the central atom of a molecule.
- Shows the valence electrons as dots around the symbol for the element. The number of valence electrons for a representative element is the same as its group number on the periodic table.
5 True/False Questions
EDG Tetrahedral → MG Octahedral
MG Square pyramidal
MG Square planar
2 ED → Orbital Hybridization sp
Duet Rule → Hydrogen provides an exception to the octet rule because it requires only two electrons to attain a noble gas configuration.
Lewis Structure → For covalent molecules often show shared pairs of electrons (bonding pairs) as lines and unshared electron pairs (nonbonding pairs) as lines or dots.
Dipole Moment → A molecule with one end having a slight positive charge and the other end having a slight negative charge due to differences in electronegativity. Arrow points towards the more electronegative element.