1s¹

ANSWER : H (Hydrogen)

1s²

ANSWER : He (Helium)

1s²2s¹

ANSWER : Li (Lithium)

1s²2s²

ANSWER : Be (Beryllium)

1s²2s²2p¹

ANSWER : B (Boron)

1s²2s²2p²

ANSWER : C (Carbon)

1s²2s²2p³

ANSWER : N (Nitrogen)

1s²2s²2p⁴

ANSWER : O (Oxygen)

1s²2s²2p⁵

ANSWER : F (Fluorine)

1s²2s²2p⁶

ANSWER : Ne (Neon)

1s²2s²2p⁶3s¹

ANSWER : Na (Sodium)

1s²2s²2p⁶3s²

ANSWER : Mg (Magnesium)

1s²2s²2p⁶3s²3p¹

ANSWER : Al (Aluminum)

1s²2s²2p⁶3s²3p²

ANSWER : Si (Silicon)

1s²2s²2p⁶3s²3p³

ANSWER : P (Phosphorus)

1s²2s²2p⁶3s²3p⁴

ANSWER : S (Sulfur)

1s²2s²2p⁶3s²3p⁵

ANSWER : Cl (Chlorine)

1s²2s²2p⁶3s²3p⁶

ANSWER : Ar (Argon)

1s²2s²2p⁶3s²3p⁶4s¹

ANSWER : K (Potassium)

1s²2s²2p⁶3s²3p⁶4s²

ANSWER : Ca (Calcium)

1s²2s²2p⁶3s²3p⁶4s²3d¹

ANSWER : Sc (Scandium)

1s²2s²2p⁶3s²3p⁶4s²3d²

ANSWER : Ti (Titanium)

1s²2s²2p⁶3s²3p⁶4s²3d³

ANSWER : V (Vanadium)

1s²2s²2p⁶3s²3p⁶4s²3d⁵

ANSWER : Mn (Manganese)

1s²2s²2p⁶3s²3p⁶4s²3d⁶

ANSWER : Fe (Iron)

1s²2s²2p⁶3s²3p⁶4s²3d⁷

ANSWER : Co (Cobalt)

1s²2s²2p⁶3s²3p⁶4s²3d⁸

ANSWER : Ni (Nickel)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

ANSWER : Zn (Zinc)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p¹

ANSWER : Ga (Gallium)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

ANSWER : Ge (Germanium)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³

ANSWER : As (Arsenic)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴

ANSWER : Se (Selenium)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵

ANSWER : Br (Bromine)

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

ANSWER : Kr (Krypton)

1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰

ANSWER : Cu (Copper)

How are 1s and 2s orbitals alike/different?

ANSWER : They both have a similar layout. The 2s orbital has a greater chance of finding the electron 

since it is farther from the nucleus

How many electrons can any given orbital hold?

ANSWER : 2 electrons

How many orbitals are in the s sublevel?

ANSWER : 1 orbital

How many orbitals are in the p sublevel?

ANSWER : 3 orbitals

How many orbitals are in the d sublevel?

ANSWER : 5 orbitals

How many orbitals are in the f sublevel?

ANSWER : 14 orbitals

Aufbau’s Principle

ANSWER : Each electron will occupy the lowest energy level available and fill in an order

Pauli Exclusion Principle

ANSWER : Because electrons spin, two electrons can occupy one orbital as long as they are spinning 

oppositely.

Hund’s Rule

ANSWER : Within a certain sublevel, single electrons are placed one at a time in orbitals with spins of the 

same directions and then will double up with electrons spinning the opposite direction.

How many total electrons are in the 1st energy level?

ANSWER : 2 electrons

How many total electrons are in the 2nd energy level?

ANSWER : 8 electrons

How many total electrons are in the 3rd energy level?

ANSWER : 18 electrons

How many total electrons are in the 4th energy level?

ANSWER : 32 electrons

How many electrons are in any given s sublevel?

ANSWER : 2 electrons

How many electrons are in any given p sublevel?

ANSWER : 6 electrons

How many electrons are in any given d sublevel?

ANSWER : 10 electrons

How many total electrons are in any given f sublevel?

ANSWER : 14 electrons

1. What atom matches this electron configuration? 1s22s22p63s2

• Neon

• Magnesium(CORRECT ANSWER)

• Aluminum

• Potassium

2. What atom matches this electron configuration? 1s22s22p63s23p64s23d10

• Zinc(CORRECT ANSWER)

• Copper

• Nickel

• Germanium

3. What is the electron configuration for a Sulfur atom?

• 1s22s22p63p6

• 1s22s22p63s23p6

• 1s22s22p63s23p4(CORRECT ANSWER)

• 3p4

4. What atom matches this electron configuration? 1s22s22p63s33p64s23d104p65s24d105p66s24f145d9

• Mercury

• Gold(CORRECT ANSWER)

• Platinum

• Thallium

5. What electron configuration matches an oxygen atom?

• 1s22s22p63s2, 3p64s23d104p5

• 1s22s22p4(CORRECT ANSWER)

• 1s22s22p6

• 1s22s22p63s23p64s23d1

6. Which of the following is the smallest in size?

• N(CORRECT ANSWER)

• S

• I

• Fr

7. Which of the following is the smallest in size?

• K

• Na

• Li(CORRECT ANSWER)

• Cs

8. How many electrons does Si contain?

• 14(CORRECT ANSWER)

• 28

• 2

• 4

9. How many valence electrons does Si contain?

• 14

• 28

• 2

• 4(CORRECT ANSWER)

10. How many electrons can the first energy level hold?

• 1

• 2(CORRECT ANSWER)

• 8

• 0

11. An orbital can at most hold how many electrons?

• 1 electron

• 2 electrons(CORRECT ANSWER)

• 3 electrons

• 4 electrons

12. The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is

• 3

• 6

• 8

• 10(CORRECT ANSWER)

13. The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is

• 3

• 6

• 8(CORRECT ANSWER)

• 10

14. What atom is represented here?

• Carbon

• Nitrogen(CORRECT ANSWER)

• Oxygen

• Fluorine

15. How many valence electrons are represented here?

• 7

• 5(CORRECT ANSWER)

• 2

• 8

16. What is the electron configuration for this atom?

• 1s22s22p6

• 1s22s22p5

• 1s22s22p3(CORRECT ANSWER)

• 2s22p3

17. What is the highest occupied energy level?

• 1

• 2

• 3(CORRECT ANSWER)

• 4

18. What is the highest occupied energy level?

 

• 4

• 5

• 6

• 7

19. How many valence electrons are there?

• 1(CORRECT ANSWER)

• 2

• 8

• 79

20. How many orbitals are in the 4s sublevel?

• 1(CORRECT ANSWER)

• 2

• 3

• 4

21. How many orbitals are in the 4p sublevel?

• 2

• 3(CORRECT ANSWER)

• 4

• 6

22. How many orbitals are in the 4d sublevel?

• 2

• 4

• 5(CORRECT ANSWER)

• 10

23. How many orbitals are in the 4f sublevel?

• 2

• 4

• 7(CORRECT ANSWER)

• 14

24. After filling 5s, electrons would fill…

• 5p

• 4d(CORRECT ANSWER)

• 5d

• 3f

25. After filling 6s, electrons would fill

• 4f(CORRECT ANSWER)

• 5d

• 6p

• 7g

26. How many unshared pairs of electrons are in this orbital diagram?

• 2

• 3(CORRECT ANSWER)

• 5

• 15

27. How many unshared pairs of electrons are in this orbital diagram?

• 2 (CORRECT ANSWER)

• 4

• 6

• 8