Regular Chemistry Name: ____________________________ #______

Block: __________

Unit 4: Quantum

Mechanics & Light

Worksheet PacketWorksheet Due Date

1 Light WS

2 Electron Configuration WS

3 Orbital Diagram WS

4 Quantum Theory Practice WS

5 Periodic Trends WS

Light WS (Page 1 of 1)

Chemistry1. Fill in the blanks in the electromagnetic spectrum:

2. Match the scientist or scientists to the correct term or theory.

_________ Dual Nature of Light A. Albert Einstein

_________ quanta B. Louis de Broglie

_________ Dual Nature of Matter C. Max Planck

_________ photon

_________ Wave-Particle Duality

3. The diagram below represents the Bohr model of an atom. Label which arrows would absorb a photon and which arrow would emit a photon.

4. Would jump from n=5 to n=1 release light with more or less energy than from n=2 to n=1?

__________________________________

5. Is high energy light closer to red or violet?

__________________________________

6. Define the following for waves:

Wavelength –

Frequency –

n=5

n=1

Electron Configuration WS (Page 1 of 2)

Chemistry1. Write the full electron configurations for the following elements:

a. Copper

b. Iodine

c. Potassium

d. Bismuth

e. Zirconium

2. Write the noble gas configurations for the following elements:

a. Iridium

b. Chlorine

c. Nobelium

d. Zinc

e. Magnesium

3. Identify the elements for the following electron configurations:

a. 1s22s22p63s1

b. 1s22s22p63s23p64s23d104p65s24d6

c. [Kr] 5s24d10

d. [Xe] 6s24f145d106p2

e. [Rn] 7s25f146d4

4. Check off if the following electron configurations are correct:

Electron Configuration Correct Incorrect

a. 1s22s22p63s23p64s24d104p65s1

b. 1s22s22p63s3

c. [Rn] 7s25f96d2

d. [Ar] 5s24d105p5

e. [Xe] 6s24f10

(Page 2 of 2)5. Write the complete electron configuration for each atom on the blank line.

a. Lithium

b. Fluorine

c. Carbon

d. Argon

e. Sulfur

f. Nickel

g. Rubidium

h. Neon

6. What elements are represented by each of the following electron configurations?

a. 1s2 2s2 2p5 c. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p65s2 4d10 5p4

b. 1s2 2s2 2p6 3s2 3p6 4s2 d. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

7. Valence electrons are only held in the highest energy s and p orbitals. Determine the number of valence electrons from each of the following electron configurations.

a. 1s2 2s2 2p5 d. 1s2 2s2 2p6 3s2 3p6

b. 1s2 2s2 2p6 3s2 3p6 4s1 e. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

c. [Ne]3s2 f. [Ar]4s23d3

8. Using the Aufbau Principle, place the following orbitals in order of increasing energy:

1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p ___ < ___ < ___ < ___ < ___ < ___ < ___ < ___ < ___ < ___

9. What two elements are exceptions to the way we normally write electron configurations? Write the expected and the actual configuration of each using noble gas configuration. What rule is violated?

Element Expected Configuration Actual Configuration Rule Violated

Orbital Diagram WS (Page 1 of 1)Chemistry

1. Write the electron configuration from each orbital diagram

Orbital DiagramElectron Configuration

1s 2s 2p 3s 3p

2. Identify the element from the orbital diagram.

Orbital DiagramElement

1s 2s 2p 3s 3p 4s 3d

3. Using arrows, draw the orbital diagrams for each of the elements. (You may not use every orbital.)

Electron Configuration 1s 2s 2p 3s 3p 4s 3d

Mg 1s22s22p63s2

Cl 1s22s22p63s23p5

Si 1s22s22p63s23p2

Ti 1s22s22p63s23p64s23d2

4. Draw the orbital diagrams for sulfur on your own. Remember, there is 1 of each s orbital and 3 of each p orbital. You can use lines or boxes but be sure to label which orbital is which!

Quantum Theory Practice WS (Page 1 of 2)

ChemistryPart I: Identify which of the following rules or principles is being violated in each electron configuration below. Circle the violation.

Hund’s Rule, Pauli Exclusion Principle, Aufbau Principle

1. ↑↓ ↑↓ ↑↓ __ __1s 2s 2p

2. ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ __ ↑↓ ↑↓ ↑↓1s 2s 2p 3s 3p

3. ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↑ ↑↓ ↑↓ ↑ v 1s 2s 2p 3s 3p

4. ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓1s 2s 2p 3s 3p 3d

Part II: Multiple Choice

____1. A “fuzzy cloud” around the nucleus of an atom where an electron is likely to be found is calleda) an orbital b) valence shell c) ground state d) none of these

____2. The statement that “if two electrons are in the same orbital, they must have opposite spins” iscalled thea) Heisenberg Uncertainty Principle c) Aufbau Principle b) Pauli Exclusion Principle d) Hund’s Rule

____3. The following electron configuration (1s22s22p63s23p63d10) breaks which of the following?a) Heisenberg Uncertainty Principle c) Aufbau Principle b) Pauli Exclusion Principle d) Hund’s Rule

____4. The electrons found in the highest principal energy level or outermost energy level for an atom are called the _____ electrons.a) valence b) orbital c) excited state d) ground state

____5. The sublevel or subshell with the lowest energy at any energy level is thea) s b) p c) d d) f

____6. Where are the valence electrons in Ga found? a) 4s only b) 3d c) 4p only d) none of these are correct

____7. The process of filling orbitals in order from lowest available energy orbitals to the highestavailable energy orbitals is called the a) Heisenberg Uncertainty Principle c) Aufbau Principle b) Pauli Exclusion Principle d) Electron Dot Structure

____8. What element has its last electron in 4p5?a) Cl b) Mn c) I d) Br

____9. Which electrons are represented by dots in an Lewis-dot structure?a) excited electrons c) lowest energy electrons b) photons d) valence electrons

(Page 2 of 2)____10. ↑↓ ↑↓ ↑↑ ↑ ↑ f Which rule is broken by this orbital filling diagram?

1s 2s 2pa) Hund’s Rule c) Aufbau Principle b) Pauli Exclusion Principle d) None of these

Part III: Electron ConfigurationsWrite the longhand electron configuration, shorthand noble gas configuration, orbital diagram (using noble gas shortcut), and Lewis dot diagram for each element in the table below.

Element Electron Configuration (Longhand)

Noble Gas Configuration (Shorthand)

Orbital Diagram (Shorthand)

Lewis Dot Diagram

Rb RbValence e: ___

Cl ClValence e: ___

Fe FeValence e: ___

Ar ArValence e: ___

Periodic Trends WS (Page 1 of 1)

Chemistry1. ATOMIC RADIUS

For each of the following sets of atoms, rank the atoms from smallest to largest atomic radius:

a. Li, C, F ______ < ______ < ______

b. Li, Na, K ______ < ______ < ______

c. Ge, P, O ______ < ______ < ______

d. C, N, Al ______ < ______ < ______

e. Al, Cl, Ga ______ < ______ < ______

2. IONIZATION ENERGYFor each of the following sets of atoms, rank the atoms from lowest to highest ionization energy:

a. Mg, Si, S ______ < ______ < ______

b. Mg, Ca, Ba ______ < ______ < ______

c. F, Cl, Br ______ < ______ < ______

d. Ba, Cu, Ne ______ < ______ < ______

e. Si, P, He ______ < ______ < ______

3. ELECTRONEGATIVITYFor each of the following sets of atoms, rank the atoms from lowest to highest electronegativity:

a. Li, C, N ______ < ______ < ______

b. C, O, N ______ < ______ < ______

c. Si, P, O ______ < ______ < ______

d. K, Mg, P ______ < ______ < ______

e. S, F, H ______ < ______ < ______

4. IONIC RADIUSFor each of the following sets of atoms and ions, identify which has the largest radius:

a. Li and Li+ ______

b. S and S2- ______

c. Ba and Ba2+ ______

d. Cl and Cl- ______

e. Al and Al3+ ______