Atomic Radius. Atomic Radius. Atomic Radius 10/17/18. Monday October AGENDA YOYO. AIM What are periodic table trends?
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1 10/17/18 Monday October AGENDA YOYO PUT EVERYTHING AWAY QUIZ TIME! YOYO AIM What are periodic table trends? Quiz Periodic Trend Activity AFTER QUIZ Turn in Quiz and take and start working on Periodic Table Trends sheet you will need your best friend! HOMEWORK Unit 2 Castle Learning Due Wednesday 10/17 Unit 2 TEST Thursday 10/18 Unit 2 HW Packet due Monday 10/22 In order to standardize the measurement of atomic radii, the distance between the nuclei of two identical atoms bonded together is measured. The atomic radius is defined as one-half the distance between the nuclei of identical atoms that are bonded together. Table 1: Across a Period (pm) Aluminum (Al) 124 Silicon (Si) 114 Phosphorus (P) 109 Sulfur (S) 104 Chlorine (Cl) According to the data table, what happens to the atomic radius as you move across a period? Answer: it gets smaller Table 2: Down a Group (pm) Lithium (Li) 130 Sodium (Na) 160 Potassium (K) 200 Rubidium (Rb) 215 Cesium (Cs) According to the data table, what happens to the atomic radius as you move down a group? Answer: it gets larger 1
2 The Snowman How does this image relate to the the atomic radius trend? Bigger towards the bottom Smaller moving toward the right Electronegativity Electronegativity is a measure of the ability of an atom to attract the electrons when the atom is part of a compound. Electronegativity is not measured in energy units, but is rather a relative scale. All elements are compared to one another, with the most electronegative element, fluorine, being assigned an electronegativity value of 4.0 Electronegativity Table 3: Electronegativity Across a Period Electronegativity Boron (B) 2.0 Carbon (C) 2.6 Nitrogen (N) 3.0 Oxygen (O) 3.6 Fluorine (F) According to the data table, what happens to the atomic radius as you move across a period? Answer: it gets larger Table 4: Electronegativity Down a Group Electronegativity Fluorine (F) 4.0 Chlorine (Cl) 3.2 Bromine (Br) 3.0 Iodine (I) 2.7 Astatine (At) According to the data table, what happens to the atomic radius as you move down a group? Answer: it gets smaller 2
3 Ionization Energy Ionization Energy Ionization energy is the energy required to remove an electron from a specific atom. It is measured in kj/mol, which is an energy unit, much like calories. As more electrons are added to a nucleus, the outer electrons become shielded from the nucleus by the inner shell electrons. This is called electron shielding. Table 5: Ionization Energy Across a Period Ionization Energy (kj/mol) Potassium (K) 419 Calcium (Ca) 590 Scandium (Sc) 633 Titanium (Ti) 659 Vanadium (V) According to the data table, what happens to the ionization energy as you move across a period? Answer: it gets larger Ionization Energy Ionic Radius Table 6: Ionization Energy Down a Group Ionization Energy (kj/mol) Magnesium (Mg) 738 Calcium (Ca) 590 Strontium (Sr) 549 Barium (Ba) 503 Radium (Ra) According to the data table, what happens to the ionization energy as you move down a group? Answer: it gets smaller The radius of an ion (a charged atom) 7. Explain in terms of protons and electrons why atoms are neutral? Answer: Protons = electrons 3
4 10/17/18 8. What do you notice about the charge of cations? Answer: They are POSITIVE 11. What would the charge of an atom be if it had 3 protons, but only 2 electrons? Answer: What is the charge of the magnesium ion? Answer: Do cations loose or gain electrons? Explain your reasoning. Answer: Loose electrons because they become positively charged 9. What is the electron configuration of: Lithium: 2-1 Beryllium: 2-2 Boron: How many electrons does each element want in its valence shell? Answer: Compare the size of the cation to the size of the parent atom. Answer: The cation is smaller than the parent atom because it lost electrons Tuesday October AIM How are trends used to build a periodic table? YOYO Take out yesterday s sheet Take a practice test Answer the first 3 questions AGENDA YOYO Anion/Cation Review Harry Potter PT HOMEWORK Unit 2 Castle Learning Due Wednesday 10/17 Unit 2 TEST Thursday 10/18 Unit 2 HW Packet due Monday 10/22 4
5 Practice Test Question 1 1. Which two characteristics are associated with metals? a. Low first ionization energy and low electronegativity b. Low first ionization energy and high electronegativity c. High first ionization energy and low electronegativity d. High first ionization energy and high electronegativity Ionization energy and electronegativity follow the same pattern/trend. The closer you get to fluorine the higher the number. Metals are far away from fluorine so both numbers will be low. Practice Test Question 2 2. Based on Table S, which group on the Periodic Table has the element with the highest electronegativity? a. Group 1 b. Group 2 c. Group 17 d. Group 18 Fluorine is the most electronegative atom and it lives in Group 17, the halogens Practice Test Question 3 3. Which atom has the largest atomic radius? a. potassium b. rubidium c. francium d. cesium These are all Group 1 elements. The farther down the group you go the bigger you get. Francium is the lowest of them all so it is the largest 5
6 Ionic Radius - Anions 15. What do you notice about the charge of the anions? Answer: They are NEGATIVE 16. What is the electron configuration of: - Oxygen: Fluorine: How many electrons does each element want in its valence shell? Answer: 8 Ionic Radius - Anions 18. What would the charge of an atom be if it had 7 protons, but 8 electrons? Answer: What is the charge of the oxygen ion? Answer: Do anions loose or gain electrons? Explain your reasoning. Answer: Gain electrons because they become negatively charged. Ionic Radius - Anions 21. Compare the size of the anion to the size of the parent atom. Answer: The anion is larger than the parent atom because it gained electrons. 6
7 Ionic Radius - Anions Periodic Trend Summary Decreases across a period Increases down a group Ionic Radius Removing e- = smaller than parent Positive charge (cation) - metals Adding e- = larger than parent Negative charge (anion) - nonmetals Electronegativity Increases across a period Decreases down a group F is the most electronegative the closer to F you get the higher the EN Ionization Energy Increases across a period Decreases down a group (Same as electronegativity) Metallic and Non-metallic Character Metallic character increases down a group Non-metallic character increases across a period Rc Po Hf Pj Sy Wy Dm Du A V Ah An W Le Sn Ag Pt Ha Ff Do Sb De Ho Bg Ex L Gf Hs Mu Ri 7
8 10/17/18 Wednesday October AIM Unit 2: The Periodic Table TEST Review YOYO Take out practice test AGENDA YOYO 20 mins write explanations for each question 20 mins review as class HOMEWORK Unit 2 Castle Learning Due Wednesday 10/17 - TONIGHT Unit 2 TEST Thursday 10/18 Unit 2 HW Packet due Monday 10/22 8
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