Rank the 3d, 3p, 3s, 4p, 4s, 4d orbitals in the order they typically fill, going from the lowest energy orbitals to the highest energy orbitals:

Rank the following bonds and intermolecular forces in order of increasing strength (weakest first and strongest last): covalent bond, London dispersion forces, dipole–dipole forces, and hydrogen bonds.

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is Kc = 2 × 1011. This means that the reaction mixture at equilibrium is likely to consist of ________.

The conjugate base of HClO3 is ________.

Determine whether a bond in the compound is polar or nonpolar and whether the molecule as a whole is polar or nonpolar. Place your answers in the table below. Electronegativity of C is 2.5, H is 2.1, and Cl is 3.5. Compound Nonpolar Bond Y/N Polar Bond Y/N Molecule Polar Y/N CH4  [1]  [2]  [3] CH3Cl  [4]  [5]  [6] CH2Cl2  [7]  [8]  [9] CHCl3  [10]  [11]  [12] CCl4  [13]  [14]  [15]  

CO2 Molecular Shape: [shape] Hybridization of the central atom [hybridization] write in normal characters sp, sp2, sp3 Name: [name] Number of sigma bonds: [sigma] Number of pi bonds: [pi]

Describe what makes a bond polar or nonpolar.

Explain the difference between a covalent bond and an ionic bond. Include how electrons affect the bonds.  

O2 Molecular Shape: [shape] Name: [name] Remember — diatomic molecules are named simply as the element’s name. Number of sigma bonds: [sigma] Number of pi bonds: [pi]

Provide the formula for the following compounds. You may submit your response in the box below using the text editing tools or upload a photo of a written response at the end of the test. Please mark the problem clearly and show your work. magnesium bromide cobalt(II) sulfate ammonium hydroxide       potassium cyanide sodium carbonate calcium phosphate     Formula of 1:                    Formula of 2:                    Formula of 3:   Formula of 4:                    Formula of 5:                    Formula of 6: