Electron Configuration and Periodic Trends Study Guide PDF

Okay, here is the converted text from the images into a structured markdown format. # Electron Configuration ## Unit Test Study Guide ### Section #1: Sublevels & Orbitals 1. Which of the following lists the sublevels with the correct number of maximum electrons per sublevel? a) s2, p4, d6,...

Okay, here is the converted text from the images into a structured markdown format. # Electron Configuration ## Unit Test Study Guide ### Section #1: Sublevels & Orbitals 1. Which of the following lists the sublevels with the correct number of maximum electrons per sublevel? a) s2, p4, d6, f8\ b) s1, p3, d5, f7\ c) **s2, p6, d10, f14**\ d) s1, p2, d3, f4 2. What is the number of orbitals for the *d* sublevel? a) 1\ b) 3\ c) **5**\ d) 7 3. How many electrons can occupy an orbital in any sublevel? a) **two, if they have opposite spins**\ b) two, if they have the same spin\ c) one\ d) depends on the sublevel 4. How many electrons are needed to completely fill the fourth energy level? a) 2\ b) 4\ c) 18\ d) **32** 5. What is the number of orbitals for each of the four sublevels? a) s sublevel **1**\ b) p sublevel **3**\ c) d sublevel **5**\ d) f sublevel **7** 6. What are the maximum number of electrons for the four sublevels? a) s sublevel **2**\ b) p sublevel **6**\ c) d sublevel **10**\ d) f sublevel **14** 7. Which orbital below can never exist according to quantum theory? a) 3*d*\ b) **3*f***\ c) 4*s*\ d) 2*p* 8. Which sublevel is associated with a spherical (ball shaped) electron cloud? **s sublevel** ### Section #2: Principles that Govern Electron Configuration 9. Describe what the Aufbau Principle governs regarding electron configuration. *Electrons fill the lowest energy levels first* 10. Describe the Hund's Rule. *Complete orbitals with single electrons before pairing up electrons in a single orbital.* 11. What part of electron configuration does the Pauli Exclusion Principle govern? Describe this principle. *The spin. Two electrons can share an orbital if they have opposite spin.* 12. The following orbital notations are incorrect. Identify the Principle or Rule broken and describe why it is broken for each notation. * **Diagram 1:** * **Orbital Notation:** * 1s²: ↑↓ * 2s²: ↑↓ * 2p⁶: ↑↓ ↑↓ ↑↓ * 3s²: ↑↓ * 3p⁴: ↑↓ ↑ ↑ * **Rule Broken:** Pauli Exclusion Principle * **Why:** The 3p⁴ electron should show an opposite spin. * **Diagram 2:** * **Orbital Notation:** * 1s²: ↑↓ * 2s²: ↑↓ * 2p²: ↑↓ ↑ * **Rule Broken:** Hund's Rule * **Why:** The last electron should go in the 2nd orbital, and not paired in the 1st. * **Diagram 3:** * **Orbital Notation:** * 1s²: ↑↓ * 2s²: ↑↓ * 2p⁶: ↑↓ ↑↓ ↑↓ * 3s²: ↑↓ * 3p⁴: N↑ ↑ * **Rule Broken:** Aufbau Principle * **Why:** The 3s² energy level should be completed before filling the 3p orbital. ### Section #3: Orbital Notation 13. What element's orbital notation is shown in a? **carbon** * **Diagram A** * **Orbital Notation:** * 1s²: ↑↓ * 2s²: ↑↓ * 2p²: ↑ ↑ 14. Identify the element with orbital notation b. **phosphorus** * **Diagram B** * **Orbital Notation:** * 1s²: ↑↓ * 2s²: ↑↓ * 2p⁶: ↑↓ ↑↓ ↑↓ * 3s²: ↑↓ * 3p³: ↑ ↑ ↑ 15. Draw the orbital notation for the following elements. * a) argon, Ar * ↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ * 1s² 2s² 2p 3s² 3p * b) selenium, Se * ↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ * 1s² 2s² 2p 3s² 3p 4s² 3d¹⁰ 4p * c) tin, Sn * ↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓ ↑↓ * 1s² 2s² 2p 3s² 3p 4s² 3d¹⁰ ↑↓ ↑↓ * d) scandium, Sc * ↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓ * 1s² 2s² 2p 3s² 3p 4s² 3d ### Section #4: Bohr Model 16. Draw the Bohr Model for nitrogen, N. * A diagram of a nitrogen atom is shown with 7 protons and 7 neutrons in the nucleus and electrons in the orbits. 17. Draw the Bohr Model for magnesium, Mg. * A diagram of a magnesium atom is shown with 12 protons and 12 neutrons in the nucleus and electrons in the orbits. ### Section #5: Electron Configuration 18. Write the electron configuration for the following elements. Identify the number of valence electrons for each. * a) aluminum, Al **3** valence *e⁻* $1s^22s^22p^63s^23p^1$ * b) nitrogen, N **5** valence *e⁻* $1s^22s^22p^3$ * c) cobalt, Co **2** valence *e⁻* $1s^22s^22p^63s^23p^64s^23d^7$ * d) barium, Ba **2** valence *e⁻* $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^2$ * e) krypton, Kr **8** valence *e⁻* $1s^22s^22p^63s^23p^64s^23d^{10}4p^6$ 19. Identify the following elements by their electron configuration. * a) $1s^22s^22p^63s^23p^64s^1$ **potassium, K** * b) $1s^22s^22p^4$ **oxygen, 0** * c) $1s^2$ **helium, He** * d) $1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^2$ **zirconium, Zr** ### Section #6: Noble Gas and lon Configuration 20. Identify the following elements by their noble gas configuration. * a) $[Ne]3s^23p^2$ **silicon, Si** * b) $[Ar]4s^23d^{10}4p^6$ **krypton, Kr** * c) $[Kr]5s^24d^{10}5p^3$ **antimony, Sb** * d) $[Xe]6s^25d^14f^7$ **gadolinium, Gd** 21. Write the noble gas configuration for the following elements. * a) neptunium, Np $[Rn]7s^26d^15f^4$ * b) chlorine, Cl $[Ne]3s^23p^5$ * c) lawrencium, Lr $[Rn]7s^26d^15f^{14}$ * d) technetium, Tc $[Kr]5s^24d^5$ 22. Describe the term *isoelectronic* *Atoms of different elements with the same number of electrons* 23. Strontium, Sr, loses two electrons to form a 2+ ion. What noble gas is the ion isoelectronic with? **krypton, Kr** 24. Sulfur, S, gains two electrons to form a 2- ion. What noble gas is the ion isoelectronic with? **argon, Ar** 25. Write the noble gas configuration for the following ions. * a) $Rb^+.$ $[Ar]4s^23d^{10}4p^6$ +1 charge * b) $P^{3-}$ $[Ne]3s^23p^6$ -3 charge # Periodic Table & Periodic Trends ## Unit Test Study Guide ### Section #1: History of the Periodic Table 1. Who is attributed with the idea of arranging the known elements of his time in a table according to their chemical and physical properties? **Dmitri Mendeleev** 2. This scientist from question #1, above, predicted that the empty spaces on his periodic table represented a) radioactive elements. b) isotopes. c) **undiscovered elements.** d) ions. 3. Who arranged the periodic table of elements in the order of atomic number? **Henry Moseley** 4. The periodic law states there is a periodic repetition of physical and chemical properties of the elements a) when they are arranged in order of increasing atomic radii. b) if only nonmetals are considered. c) when they are arranged in order of increasing atomic mass. d) **when they are arranged in order of increasing atomic number.** ### Section #2: The Periodic Table 5. The vertical columns of the periodic table are called **groups**. 6. Each period in the periodic table corresponds to **an energy level** a) a sublevel b) atomic mass c) **an energy level** d) an atomic number 7. What are valence electrons? **electrons found in the outermost energy level of atoms** 8. The horizontal rows of the periodic table are called **periods**. 9. What do elements in the same periodic group have in common? **same valence configuration, same number of valence electrons, and similar chemical properties** 10. What do elements in the same periodic periods have in common? **same number of occupied energy levels - principle energy levels (PEL)** 11. How many elements are in a period in which only the *s* and *p* sublevels are filled? **8** 12. Identify the sublevels in a period that contains 32 elements. a) *s, d* b) *s, p* c) *s, p, d* d) *s, p, d, f* 13. The number of valence electrons in group 17 elements is **7**. 14. For groups 13 through 18, the number of valence electrons is equal to **the group number minus 10.** 15. In group 2 elements, the valence electrons are in sublevel **s**. ### Section #3: Elements Classes and Families16) Name the three classes of elements. metals, nonmetals, and metalloids 17. Identify the following on the periodic table to the right. * A) **metals** * B) **metalloids** * C) **nonmetals** * The periodic table graphic on the right shows the 3 areas. 18. Name the element: a) period 5, group 14 **tin, Sn** b) period 3, group 17 **chlorine, Cl** c) period 6, group 2 **barium, Ba** 19. Identify the properties listed below as properties of metals (m), or properties of nonmetals (nm).\ a) **m** lose electrons\ b) **nm** dull, brittle\ c) **nm** gain electrons\ d) **m** good electrical conductors\ e) **m** malleable, ductile\ f) **nm** are not conductors 20. Identify the periodic family or group name of the following. Write the group number and name. a) the most reactive group of nonmetals **group 17, halogens**\ b) This group is unreactive, and only found in pure form in nature. **group 18, noble gases**\ c) This group's name means "basic". **group 2, alkaline Earth metals**\ d) This group of metals contains groups 3-12. **groups 3-12, transition metals**\ e) This group contains the most reactive group of metals. **groups 1, alkali metals**\ f) These elements are found in the second row of the f-block elements. **actinides**\ g) This class of elements have both metallic and nonmetallic properties. **metalloids** ### Section #4: Periodic Trends 21. Explain why atomic radius decreases going across the period left to right on the periodic table. *The number of energy levels remains the same. The number of protons increases in the nucleus of each successive element atom. This increases the positive nuclear charge - pulling electrons closer to the nucleus.* 22. Choose the best reason that the atomic radius generally increases moving down a group of elements. a) The nuclear charge increases.\ b) A new octet if formed.\ c) The number of neutrons increases.\ d) **The number of occupied energy levels increases.** 23. Which of the following atoms is largest: nitrogen, phosphorus, or arsenic? **arsenic** 24. Find phosphorus, sulfur, and chlorine on the periodic table. Which of these is the largest atom? **phosphorus** 25. Which of the following atoms is smallest: nitrogen, oxygen, or fluorine? **fluorine** 26. Write a definition for ionization energy. **lonization energy is the energy required to remove one electron for an atom.** 27. Which atom would it take more energy to remove its first electron, sodium or aluminum? **aluminum** 28. As you move left to right across a period, the first ionization energies **increases.** 29. As you move from the top of a group to the bottom, the first ionization energies **decreases**. 30. Of the choices below, which gives the correct order of ionization energy? a) Cl > S > Al > Ar > Si b) **Cl > S > P > Si > Al** c) S > Si > CI > Al > Ar d) Cl > S > Al > Si > Ar 31. Which of these elements have the highest ionization energy? aluminum, silicon, or phosphorus **phosphorus** 32. Why is the third ionization energy of magnesium so much greater than the second ionization energy? **Once the first two electrons are removed, magnesium will be left with a full octet for its outer energy level.** 33. Which of these elements has the highest ionization energy? tin, arsenic, or sulfur **sulfur** 34. List the following atoms in order of decreasing electronegativity. CI, K, & Zn **chlorine, zinc, potassium – Cl, Zn, K** 35. What is the general trend of electronegativity as you go down the group on the periodic table? *Electronegativity decreases moving down a group on the periodic table.* 36. What element is the most electronegative? **fluorine** 37. Do metals tend to have high or low electronegativities? **low** 38. Which of the following is the smallest: a lithium atom, $Li^+$ ion, or a sodium atom? **$Li^+$ ion** 39. Which atom or ion will have the larger radius? $Na^+$ or $K^+$, $K^+$ or $Ca^{2+}$, $K^+$, or $Cl^-$, For $Cl^-$, For F **F** 40. What is the trend for reactivity for the alkali metal group? **reactivity increases going down the group** the halogens group? **reactivity decreases going down the group**