Groups (families) = columns Periods = rows. Representative Elements Transition Elements
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1 Chapter 6
2 Groups (families) = columns Periods = rows Representative Elements Transition Elements
3 Shiny, smooth, solid at room temp, good conductors of electricity, malleable and ductile (can be bent and reshaped). Metals
4 Alkali and Alkaline Earth Metals Alkali metals group 1 except for H (very reactive) Alkaline earth metals group 2 (also reactive)
5 Transition Metals Can form ions of many charges and complex ions. ALWAYS CATIONS!!!! METALS ARE LOSERS!!
6 Nonmetals Usually gases or dull brittle solids. Poor conductors of heat or electricity. One of the only liquids at RT
7 Halogens Also highly reactive Form ANIONS easily
8 Noble Gases UNreactive Don t form IONS Important when considering ions and how they form
9 Metalloids Have properties of both metals and nonmetals. Silicon and germanium used extensively in solar cells and computer chips.
10 Review Questions! Who were the major players in the development of the periodic table? Sketch a periodic table. Identify: Metals (all 3 types) Nonmetals Metalloids Halogens Noble gases What are some general characteristics of metals and nonmetals? Characterize each: Li, F, C, Kr, Ge, Mg
11 Warm Up! Elements were initially arranged according to their. They were later reorganized by because their properties were consistent with their placement on the table. Representative or transition element?? Iodine, Chromium, Uranium, Cesium What are the names for group 1 and 2 metals?
12 Todays Agenda QOTD:How can we predict chemical behavior? Classification of elements by valence electrons Periodic Trends Atomic Radii
13 Metals Data Make predictions about Fr! 1. From the data, devise a plan to predict mp, bp, and radius of Fr. Why can we do this? 2. Is Fr a solid, liquid, or gas at RT? 3. Which column do you think introduces the most error (mp, bp, or radius)? These are called Periodic Trends and are seen all over the table!
14 Classification of Elements Valence electrons - All electrons in the highest principle energy level (outermost electrons). How many valence electrons in Na, Li, K, Rb? All members in each GROUP have the same number of valence electrons. Where the valence electrons are indicates the PERIOD.
15 Valence Electrons and Groups Determine the valence electrons for groups 1, 2, The group will indicate the number of valence electrons. ONE exception : He Helium is a noble gas but only has 2 valence electrons.
16 Remember Read over this section in the book pg about spdf blocks
17 Try these: Without using the table, determine the group, period, and block of these elements: [Ne]3s 2, [He]2s 2, [Kr]5s 2 4d 10 5p 5 What are the symbols for the elements with the following valence electron configurations? s 2 d 1 s 2 p 3 s 2 p 6 Write the electron configs: group 2 element in 4 th period noble gas in 5 th period group 12 element in the fourth period group 16 element in the second period
18 Warm Up Find the atom Group 13 Period 4 Two valence electrons Period 2 N = 4 with 6 valence electrons All atoms with 4 valence electrons classify as metals, nonmetals and metalloids.
19 Today s agenda QOTD: Why are noble gases so important? Radii of atoms and ions Octet rule and Ionization energies Electronegativity Homework Due Friday: Read 6.3 # s 58-9, 61-62, 64, 66, 69, 70, 72, 79, 81, 86
20 Metals Data Make predictions about Fr! 1. From the data, devise a plan to predict mp, bp, and radius of Fr. Why can we do this? 2. Is Fr a solid, liquid, or gas at RT? 3. Which column do you think introduces the most error (mp, bp, or radius)? These are called Periodic Trends and are seen all over the table!
21 Trends - Atomic Radius Atomic radius half the distance between adjacent nuclei in a crystal of the element.
22 Periodic Trends Atomic Radii Atomic Radii decreases across a period. Add electrons to same energy level more attracted to the nucleus. Electrons squeeze in and radii get smaller.
23 Periodic Trends Atomic Radii Atomic radii increase down a group. Add energy levels and electrons, with more stuff comes bigger atoms.
24 Warm Up! Identify the elements: I am in period 3 and have 4 valence electrons. I am in period 2 and have the smallest radii. I am smaller than Rb and bigger than Na but we are in the same family. I am a metalloid in group 13 and have no d orbitals.
25 Today s agenda QOTD: Why are noble gases so important to other elements? Radii of ions Octet rule and Ionization energies Electronegativity Homework Due Friday: Read 6.3 # s 58-9, 61-62, 64, 66, 69, 70, 72, 79, 81, 86
26 What about Ions? Ions have positive or negative charges. positive Cations have charges and have a SMALLER atomic radii than their atoms. Lose electrons to form cations less stuff = smaller radii Anions have negative charges and have a atomic radii than their atoms. LARGER Gain electrons to form anions more stuff = larger radii
27 Draw: A metal atom and it s ion (consider relative sizes) A nonmetal atom and it s ion (consider relative sizes)
28 Forming Ions All representative elements want a Noble Gas Configuration. Elements will lose/gain electrons in order to have a full s and p shell and be in a stable electron configuration (8 valence) OCTET RULE! Attain a NGC! What ion does Na form? If Na loses 1 electron its got an NGC! Na is always a +1 cation.
29 Predict the Ions! Mg will form an ion. A) +1 C) +3 B) +2 D) -1 Cl will form an ion. A) +1 C) -1 B) +2 D) -2 What about Oxygen? K?
30 Warm Up! Using the periodic table, rank each group in order of increasing size Calcium, magnesium, and strontium Oxygen, lithium, and fluorine Selenium, chlorine, and tellurium Write electron configs, draw Lewis diagrams and predict the ion F S Ba
31 Today s Agenda QOTD: How do periodic trends relate to the arrangement of electrons and ENERGY? Review trends in radii and ionization energy Electronegativity definition and trends Practice Worksheet
32 Ionization Energy The energy required to remove an electron from an atom. How strongly an atom holds on to it s valence electrons. Is it easier to remove an electron from a metal or a nonmetal? Metals have LOW ionization energy because they are LOSERS and give up electrons easily.
33 Which is bigger? List these atoms with increasing radii. a. Carbon, fluorine, beryllium, or lithium? b. Magnesium, silicon, sulfur, sodium Describe ionic radius as you go across period 3 Identify the elements: I am in period 2 and have the smallest atomic radii (leave out Ne). I am smaller than Rb and bigger than Na but we are in the same family.
34 Agenda What is electronegativity? Exams Finish periodic trends Problem Set due Thursday
35 Trends in Ionization Energies
36 Octet Rule Elements will lose/gain or share electrons in order to have a full s and p shell and a stable electron configuration (8 valence) (like NOBLE GASES!)
37 Removing More than 1 Electron
38 Warm Up! Why is it hard to remove a second electron from Li? Is it easier to remove an electron from Mg or from Cl? Why? (Provide 2 reasons)
39 Agenda What are the overall trends and what do they have to do with one another? Electronegativity Overall trends scheme Worksheet from Friday! Problem Set due Thursday
40 Electronegativity Relative ability of an element to attract electrons in a chemical bond. Some elements are greedier than others with electrons! In a bond, they steal most of the electron density! Fluorine is small and selfish!
41 Electronegativity Trends Electronegativity across a period. INCREASES and down DECREASES a group!
42 Periodic Trend Summary Electronegativity Small Selfish with electrons s p d BIG Generous with electrons
43 First Ionization Energy (kj mol -1 ) Second Ionization Energy (kj mol -1 ) Third Ionization Energy (kj mol -1 ) Element 1 1,251 2,300 3,820 Element ,560 6,910 Element ,450 7,730 Element 4 1,000 2,250 3,360 The table above shows the first three ionization energies for atoms of four elements from the third period of the periodic table. The elements are numbered randomly. Use the information in the table to answer the following questions. (a) Which element is most metallic in character? Explain your reasoning. (b) Identify element 3. Explain your reasoning. (c) Write the complete electron configuration for an atom of element 3. (d) What is the expected oxidation state for the most common ion of element 2? (e) What is the chemical symbol for element 2? (f) A neutral atom of which of the four elements has the smallest radius? Explain your reasoning.
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