Key Unit 3 Electrons Review-Updated.docx

**Name \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Period \_\_\_** **[Unit 3 Review: Electrons Key]** **[Lewis Dot Structures]** 1\) Complete the table below. **Sublevel** **\# of Orbitals** **Maximum \# of electrons in Sublevel** -------------- -------------------- --------------------...

**Name \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Period \_\_\_** **[Unit 3 Review: Electrons Key]** **[Lewis Dot Structures]** 1\) Complete the table below. **Sublevel** **\# of Orbitals** **Maximum \# of electrons in Sublevel** -------------- -------------------- ----------------------------------------- s 1 2 p 3 6 d 5 10 f 7 14 2\) Draw the Lewis Dot Structure for Sulfur: 3) Draw the Lewis Dot Structure for Potassium:  4\) Which electron dot symbol represents Fluorine? C 5\) Which electron dot symbol could represent Aluminum? A  6\) Explain why the Lewis Dot Structure of neon (Ne) is different from that of chlorine (Cl)? Neon (Ne) is a noble gas with 8 valence electrons, represented by 8 dots, indicating a full outer shell and chemical stability. Chlorine (Cl) has 7 valence electrons, represented by 7 dots, making it more reactive as it seeks to gain one more electron to achieve a stable configuration. 7\) Which of the following elements has the most valence electrons in its Lewis Dot Structure? [a) Argon (Ar)] b\) Boron (B) c\) Sodium (Na) d\) Silicon (Si) 8)How many valence electrons does carbon (C) have? Draw its Lewis Dot Structure. Carbon has 4 valence electrons. **[Electron Configuration]** 9\) The arrangement of electrons in an atom is called the electron. [Configuration]. Electrons fill up the [ lowest] energy levels first. The lowest energy state of an electron is called the [ground] state. According to the [ Aufbau] Principle electrons can begin to occupy orbitals in the next energy level only after all of the orbitals on the energy level below it are occupied. According to Hund's Rule, electrons will pair up in an orbital only when all orbitals in the same [sublevel] have [one] electron. According to the Pauli Exclusion Principle two electrons can share an orbital, but they must have [opposite] spins. 10\) Write the [Electron Configuration] for each: Iron: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s² Oxygen: 1s² 2s² 2p⁴ 11\) Write the [Noble Gas Notation] for each: Nitrogen: \[He\] 2s² 2p³ Sulfur: \[Ne\] 3s² 3p⁴ 12\) What is the Noble Gas Notation for **Nickel**? a\) \[Kr\] 4s^2^3d^8^ b) \[Kr\] 3d^8^ [c) \[Ar\] 4s^2^3d^8^] d) \[Ar\] 3d^8^ 13\) What is the highest energy sublevel of **Vanadium**? a\) 4d^3^ [b) 3d^3^] c) 4d^4^ d) 3d^4^ 14\) What is the correct electron configuration for **Chlorine**? a\) 1s^2^2p^6^3p^1^ [b) 1s^2^2s^2^2p^6^3s^2^3p^5^] c) 1s^2^2s^2^2p^6^3s^2^3p^6^ d) 1s^2^2s^2^2p^6^3s^2^4p^5^ 15\) What group on the periodic table does this valence orbital notation represent?  a\) group 13 b) group 14 c) group 15 [d) group 17] 16\) Which of the following breaks Aufbau's principle? [a. 1s^2^2s^2^2p^6^3s^2^3p^6^4s^2^4p^5^ ] b. 1s^2^2s^2^2p^6^3s^2^3p^6^4s^2^3d^10^4p^5^ c\. 1s^2^2s^2^2p^6^3s^2^ d. 1s^2^2s^2^2p^6^3s^2^3p^6^4s^2^3d^10^4p^6^ 17\) What element is demonstrated by this orbital notation? Argon (Ar) 18\) Electrons fill the [lowest] ***(lowest/ highest)*** energy levels first. Electrons within a pair must have [ opposite] ***(the same/ opposite)*** spins. 19\) Write the correct orbital notation for the following elements (remember to draw all the orbitals, even if they are empty): Copper: 1s²: ↑↓ 2s²: ↑↓ 2p⁶: ↑↓ ↑↓ ↑↓ 3s²: ↑↓ 3p⁶: ↑↓ ↑↓ ↑↓ 4s¹: ↑ 3d¹⁰: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ----------------------------------------------------------------------------------------- Phosphorus: 1s²: ↑↓2s²: ↑↓2p⁶: ↑↓ ↑↓ ↑↓3s²: ↑↓3p³: ↑ ↑ ↑ Potassium: 1s²: ↑↓2s²: ↑↓2p⁶: ↑↓ ↑↓ ↑↓3s²: ↑↓3p⁶: ↑↓ ↑↓ ↑↓4s¹: ↑ Fluorine: 1s: ↑↓ 2s: ↑↓ 2p: ↑ ↑ ↑ **[Electromagnetic Spectrum]** 20\) Which of these types of electromagnetic radiation has the longest wavelength and carries the least amount of energy? a\. ultraviolet [b. infrared] c. X-ray d. gamma-ray 21\) Which has a higher energy: visible light or microwaves? Visible light 22\) What is the relationship between frequency and energy? [a. Direct] b. Inverse c. Logarithmic d. No Relationship 23\) If the frequency increases, what happens to the wavelength? It decreases 24\) If the energy decreases, what happens to frequency? It decreases 25\) What is the relationship between frequency and wavelength? Inverse Relationship 26)How does the energy of a photon relate to its frequency and wavelength in the electromagnetic spectrum? Explain the trend as you move from radio waves to gamma rays. As you move from radio waves (longer wavelength, lower frequency) to gamma rays (shorter wavelength, higher frequency), the energy of photons increases. Higher frequency corresponds to higher energy, while longer wavelengths correspond to lower energy. 27\) Draw a graph illustrating the relationship between wavelength and frequency (make sure you label the x and y axis). Inverse relationship (as frequency increases, wavelength decreases).  28\) Draw a graph illustrating the relationship between wavelength and energy (make sure you label the x and y axis). Inverse relationship (as wavelength increases, energy decreases). 29\) Draw a graph illustrating the relationship between frequency and energy (make sure you label the x and y axis). Direct relationship (as frequency increases, energy increases).  30\) What happens when an electron drops from a higher energy level to a lower energy level? The electron releases energy in the form of a photon, often observed as visible light or another form of electromagnetic radiation.