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Electron Configuration Honors

Last updated about 5 years ago
20 questions
The periodic table is that it is sectioned off by orbitals, or region of space in which there is a high probability of finding an electron. There are four orbitals, s, p, d, and f which are found in different energy levels called principle quantum numbers. We use the energy level numbers and orbitals in a “code” called electron configuration which helps us express the location of an electron with high probability. We can actually use the periodic table to write our electron configurations. The first row is energy level 1, the second is energy level 2, and so on. *NOTE: The d and f orbital energy levels do not follow the energy levels by row like s and p, so pay attention to those differences.



Look at the periodic table above, all the orange boxes indicates the principle energy level and the atomic orbital that the outer electrons in that specific element occupies.
1

Using the periodic table, which atomic orbital do the outer electrons of Helium (He), occupy?

1

The d orbital starts in the 4th row, or 4th energy level. However, what energy level (period number) does d actually start with?

1

How many elements do all the “s” orbital span (go across) in each period?

1

How many elements do all the “p” orbital span (go across) in each period?

1

How many elements do all the “d” orbital span (go across) in each period?

1

How many elements do all the “f” orbital span (go across) in each period?

1

What element can be found by an ending electron configuration of 3s2? (Hint: go to the 3s row and count 2 elements in)

1

What element can be found by an ending electron configuration of 2p3?

1

What element can be found by an ending electron configuration of 3d6?

1

Identify two elements that have a valence shell electron configuration of s2p3. What does this suggest about elements with the same number of valence electrons and their location on the periodic table?

1

Match each symbol below with its meaning.

Draggable itemCorresponding Item
atomic orbital (region of space where an electron is likely to be found)
single electron
pair of electrons with opposite spins
sublevel (set of electrons having equivalent energy)
electron configuration
1

Using the following electron configuration:

1

Arrange the sublevels for an atom of gold in the ground state in their correct order of filling according to the Aufbau Principle.

1

In the space provided, draw the correct Lewis electron dot diagram for an atom of gold in the ground state.

1

In the space provided, draw the orbital diagram for the valence shell of an atom or arsenic. Be sure the label the energy level and the sublevel(s).

1

State the total number of energy levels occupied by electrons in an atom of arsenic in the ground state.

1

Identify the element with the electron configuration:
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s26d15f3

1

Identify the number of completely filled orbitals in an element with the electron configuration:
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s26d15f3

1

In the space provided, write the noble gas notation for an atom of zinc in the ground state.

1

In the space provided, write the noble gas notation for an atom of krypton in the ground stae