Chemistry Unit 4 Test Review

Which of the following orbital diagrams is the best picture of electrons in an unexcited atom?

Classify the following bond:

Choose the electron configurations which are possible for an unexcited atom.

According to VSEPR Theory, which shape represents CF4?

Which of the following groups is characterized by differing numbers of electrons in d orbitals?

Which of the following orbitals contain quantum number combinations that are not possible?

What statement describes the trends of electronegativity in the periodic table?

Is this the correct way to draw the Lewis Dot Structure for Carbon?

The attraction between positive ions and surrounding mobile electrons forms which type of bond?

Metals can conduct electricity and heat well due to _______________

Which of the 2 outermost orbitals must be filled to satisfy the octet rule?

Compared to nonmetals, metals tend to have ________________

Which of the following is used to draw the Lewis Dot Structure of a molecule or atom?

Which of these elements have the largest atomic radius?

A property of some metals to be drawn into a wire is called ____________

Which compound is correctly matched to its molecular geometry according to VSEPR Theory?

Which of the following correctly places the ions in order of increasing ionic radii?

What can be inferred about the behavior of an elements that bonds with different elements?

Which of the following is the correct electron configuration for Manganese?

Which of the following ions has the largest radius?

Which statement best describes the elements in Group 15 as considered from top to bottom?

Is this the correct Lewis Dot Structure for MgO?

"An electron must occupy the lowest available energy orbital" is stated by ________________.

Rubidium has a lower ionization energy than sodium. One reason for this is that the ___________

How many double bonds are in the Lewis structure for Carbon Dioxide, CO2?

Is this the correct Lewis Dot Structure for NaCl?

Is this the correct Lewis Dot Structure for NH3?

According to VSEPR Theory, what happens to electron pairs when molecules are formed?

How many electrons are required to completely fill the 3rd energy level?