Name Unit 4: Periodic Table Period 1. History and Language of the Periodic Table 2. Identifying PROPERTIES OF METALS, METALLOIDS, & NONMETALS 3. Identifying GROUP PROPERTIES 4. Classifying elements 5. Identifying TRENDS IN THE PERIDIOC TABLE Unit 4 Vocabulary.Due Test Day Mendeleev Word Definition Noble Gas Malleable Period Group Metalloid Atomic Radius Ionic Radius Ionization Energy Electronegativity Allotrope
Element Refresh: Name the element in each square! If the name is given, give symbol. B 14.01amu Bromine 16amu 55amu 4 protons Pb Chlorine Gold 16.00amu 77protons Ne 259amu Zn I don t have a neutron 40.08amu Periodic à Periodic Law à Periodic Table Periodic occurs at intervals Periodic law - physical and chemical properties of the elements are periodic By atomic number! Periodic Table of Elements arranged by - shows patterns in properties
Skill1: History and Language of the Periodic Table o Element: A pure substance - one kind of Cannot be into simpler substances 90 occur naturally on earth 25 were synthesized (made) by scientists o Dmitri Mendeleev: Referred to as the of the Period 1860 s Grouped elements according to o Mendeleev s Predictions - Mendeleev s Table had missing elements or gaps, BUT he was able to predict the characteristics of these missing elements because of. Henry Mosely - 1914 - Rearranged the elements by - He determined # protons = atomic #
Important Features of the Periodic Table Period (Row): Each row of elements on the periodic table 1 18 1 2 3 4 5 6 7 1 H 1.008 3 Li 6.941 11 Na 22.990 19 K 39.098 37 Rb 85.468 55 Cs 132.905 87 Fr (223) 2 4 Be 9.012 12 Mg 24.305 20 Ca 40.078 38 Sr 87.62 56 Ba 137.327 88 Ra (226) 3 4 5 6 7 8 9 10 11 12 21 Sc 39 Y 71 Lu 22 23 24 Ti V Cr 40 Zr 72 Hf 41 42 Nb Mo 73 Ta 74 103 104 105 106 W Re Lr Rf Db Sg 25 Mn 43 Tc 26 27 28 29 30 Fe Co Ni Cu Zn 44.956 47.87 50.942 51.996 54.938 55.845 58.933 58.69 63.546 65.39 44 Ru 45 46 47 48 Rh Pd Ag Cd 88.906 91.224 92.906 95.94 (98) 102.906 107.868 101.07 106.42 112.4 75 76 77 78 79 80 Os Ir Pt Au Hg 174.967 178.49 180.95 183.84 186.207 190.23 192.217 195.078 196.967 200.59 107 108 109 110 111 Bh Hs Mt Ds Rg (262) (261) (262) (266) (264) (269) (268) (269) (272) 112 Uub (285) 13 14 15 16 17 5 6 7 8 9 B C N O F 10.811 12.001 14.007 15.999 18.998 13 14 15 16 17 Al Si P S Cl 26.982 28.086 30.974 32.066 35.453 31 32 33 34 35 Ga Ge As Se Br 69.723 72.61 74.922 78.96 79.904 49 50 51 52 53 In Sn Sb Te I 114.818 118.710 121.760 127.60 126.904 81 82 83 84 85 Tl Pb Bi Po At 204.383 207.2 208.980 (209) (210) 113 Uut 114 115 116 117 Uuq Uup Uuh Uus (284) (289) (288) (292) 2 He 4.003 10 Ne 20.180 18 Ar 39.948 36 Kr 83.80 54 Xe 131.29 86 Rn (222) 118 Uuo How many periods (rows) are on the Periodic Table Of Elements? Lanthanides 57 La 138.906 58 Ce 140.116 59 Pr 140.908 60 Nd 144.24 61 Pm (145) 62 Sm 150.36 63 Eu 151.964 64 Gd 157.25 65 Tb 158.925 66 Dy 162.50 67 Ho 164.930 68 Er 167.26 69 Tm 168.934 70 Yb 173.04 Actinides 89 Ac (227) 90 Th 232.038 91 Pa 231.036 92 U 238.029 93 Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) FROM LEFT TO RIGHT OR RIGHT TO LEFT Periodic Properties: Seven periods (numbered from the top down) as you move from the left to the right in a period All elements in the same period have the. Period 1 = 1 energy level Period 2 = 2 energy levels Period 3 = 3 energy levels Etc Practice: 1) What period is potassium and bromine in? 2) Based on the period, how many principal energy levels do potassium and bromine have? 3) What period is sodium and lithium in? 4) Based on the period, how do the properties of sodium and lithium compare?
Important Features of the Periodic Table Group Family: Each column of the on the periodic Table. 1 2 3 1 1 H 1.008 3 Li 6.941 11 Na 22.990 2 4 Be 9.012 12 Mg 24.305 How many groups (families) are on the Periodic Table Of Elements? 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 5 6 7 8 9 B C N O F 10.811 12.001 14.007 15.999 18.998 13 14 15 16 17 Al Si P S Cl 26.982 28.086 30.974 32.066 35.453 18 2 He 4.003 10 Ne 20.180 18 Ar 39.948 4 19 K 39.098 20 Ca 40.078 21 Sc 44.956 22 Ti 47.87 23 V 50.942 24 Cr 51.996 25 Mn 54.938 26 Fe 55.845 27 Co 58.933 28 Ni 58.69 29 Cu 63.546 30 Zn 65.39 31 Ga 69.723 32 Ge 72.61 33 As 74.922 34 Se 78.96 35 Br 79.904 36 Kr 83.80 5 37 Rb 85.468 38 Sr 87.62 39 Y 88.906 40 Zr 91.224 41 Nb 92.906 42 Mo 95.94 43 Tc (98) 44 Ru 101.07 45 Rh 102.906 46 Pd 106.42 47 Ag 107.868 48 Cd 112.4 49 In 114.818 50 Sn 118.710 51 Sb 121.760 52 Te 127.60 53 I 126.904 54 Xe 131.29 6 7 55 Cs 132.905 87 Fr (223) 56 Ba 137.327 88 Ra (226) 71 Lu 174.967 103 Lr (262) 72 Hf 178.49 104 Rf (261) 73 Ta 180.95 105 Db (262) 74 W 183.84 106 Sg (266) 75 Re 186.207 107 Bh (264) 76 Os 190.23 108 Hs (269) 77 Ir 192.217 109 Mt (268) 78 Pt 195.078 110 Ds (269) 79 Au 196.967 111 Rg (272) 80 Hg 200.59 112 Uub (285) 81 Tl 204.383 113 Uut (284) 82 Pb 207.2 114 Uuq (289) 83 Bi 208.980 115 Uup (288) 84 Po (209) 116 Uuh (292) 85 At (210) 117 Uus 86 Rn (222) 118 Uuo Lanthanides 57 La 138.906 58 Ce 140.116 59 Pr 140.908 60 Nd 144.24 61 Pm (145) 62 Sm 150.36 63 Eu 151.964 64 Gd 157.25 65 Tb 158.925 66 Dy 162.50 67 Ho 164.930 68 Er 167.26 69 Tm 168.934 70 Yb 173.04 Actinides 89 Ac (227) 90 Th 232.038 91 Pa 231.036 92 U 238.029 93 Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) FROM TOP TO BOTTOM OR BOTTOM TO THE TOP Group (Family) Properties: Eighteen groups (numbered from left to right) Atomic # and masses. Atoms in same group have - Exceptions: d block and f block Similar properties BECAUSE THEY HAVE THE SAME NUMBER OF Practice: 1. Which sequence of atomic numbers represents elements which have similar chemical properties? A) 19, 23, 30, 36 C) 9, 16, 33, 50 B) 3, 12, 21, 40 D) 4, 12, 38, 88 2. Which two elements have the most similar chemical properties? A) Aluminum and Barium C) Nickel and Phosphorous B) Chlorine and Sulfur D) Sodium and Potassium
Using this as a guide, color code your periodic table to show the three classes. Start by highlighting the zig-zag. General Groups of Elements!
Skill 2: Identifying PROPERTIES OF METALS, METALLOIDS, & NONMETALS Metals, Groups 1-Zig Zag Location Chemical Prop. Physical Prop. Left of zig zag Few electrons in VALENCE shell (outer shell) Ductile Malleable Except hydrogen Lose electrons easily Good What metal is NOT solid at Room Temperature? POSITIVE charge Ca 2+ Make Shiny Solid at room temp o Define Alloy: Non-Metals: Location Chemical Prop. Physical Prop. Right of zig zag Almost full, or totally full Tend to electrons NOT Ductile NOT malleable BAD conductors NEGATIVE charge N 3- Make Mostly solid Some are gas at room temp o Allotrope: Examples: o Diatomic: Metalloids: Location Chemical Prop. Physical Prop. Border the zig zag Most have half full valence shell Make anions OR cations depending on their environment Have properties of AND non- No way to know which properties of each o Synthetic:
Name Groups of Elements! Color As Instructed At Each Station! Date
Skill 3: Identifying GROUP PROPERTIES Group 1: Alkali Metals Please color the first column orange! Read and answer: o What element is not in this group? Color Orange o What elements are in this group? o They are very. Why? They all have one in their outer shell. That's one electron away from being happy ( ) o You will find that the alkali group is shiny and light in weight. They are also very soft and malleable. Watch the 2nd link! Group 2: Alkaline Earth Metals Watch link, read and answer the following: o This is the second most reactive family of elements in the periodic table. o Form basic or solutions. Color Green o Each of them has electrons in their outer shell. Check for Understanding: 1. In General for Groups 1 and 2: As you move down the groups, they become more 2. What will be the charge of a Calcium atom when it forms an ion? 3. List Group 1 metals in order from most to least reactive: MOST LEAST
Transition Metals: Groups 3-12 Watch and answer the following: Color Yellow o Transition metals are located in the of the table. o Compared to the alkali metals, transition metals have densities, have melting and boiling points, are strong and and are less with oxygen and water. o Transition metals often form compounds and solutions. o Transition metals can form more than one type of (have multiple oxidation states). Check for Understanding: 1. Identify the metal that has multiple oxidation states. A) K B) Ba C) Be D) Pd 2. Which compound forms a green aqueous solution? A) RbCl B) CaCl2 C) NiCl2 D) BeCl2 3. Which set of properties is most characteristic of transition elements? A) Colorless ions in solutions, multiple positive oxidation states B) Colorless ions in solutions, multiple negative oxidation states C) Colored ions in solutions, multiple negative oxidation states D) Colored ions in solutions, multiple positive oxidation states
Misc. Group 13-16, (BCNO) o Use Ptable link to determine which elements are LIQUID at STP. Highlight the Staircase Outline those elements in BLUE. o Use P table link to determine which elements are GAS at STP. Outline those elements in RED. o Watch video link! Group 17: Halogens Read and Answer: o What elements are included in the halogens? Color Black/Gray o Read and answer, then watch. o Halogens all have electrons in their outer (valence) shell o Fluorine is the most and combines with most elements from around the periodic table. o Reactivity as you move down the column. o When halogens combine with other elements, the compound is called a. Check for Understanding: 1) Give an example of a metalloid: 2) How many valence electrons does Cl have? 3) What kind of ion will Br form? 4) Which is the most reactive in the group?
Noble Gases, Group 18 Watch and fill in the notes: Color Purple o Noble gases are the group elements o Each noble gas has a full shells, which makes them very elements o They are also called the inert or gases o Light bulbs are filled with CHECK FOR UNDERSTANDING: 1. What is the electron configuration of Argon? What does it have in common with Neon? 2. Explain why noble gases don t typically react with other elements?
Name Periodic Group Practice! Period Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the nucleus. c. the number of neutrons in the nucleus. d. atomic mass. 2. Atoms of elements that are in the same group have the same number of a. protons. c. valence electrons. b. neutrons. d. protons and neutrons. 3. Which of the following elements is an alkali metal? a. calcium c. mercury b. magnesium d. sodium 4. Semiconductors are elements that a. have large atomic masses but small atomic numbers. b. do not form compounds. c. can conduct heat and electricity under certain conditions. d. are extremely hard. 5. Carbon and other nonmetals are found in which area of the periodic table? a. on the left-most side b. on the right side c. in the middle column of the periodic table d. in the bottom rows 6. In Mendeleev s periodic table, elements in each column had similar a. atomic masses. c. atomic numbers b. properties. d. symbols. 7. Magnesium (Mg) is located to the right of sodium (Na) because Mg has a. fewer protons. c. no protons. b. no neutrons. d. more protons. 8. As you move from left to right across the periodic table, elements a. become less metallic. c. have a lower atomic weight. b. have a lower atomic number. d. become more metallic. 9. How was Mendeleev s periodic table arranged? a. by increasing atomic mass c. by increasing atomic number b. by decreasing atomic mass d. by decreasing atomic number
10. When did Mendeleev create a new row in his periodic table? a. when the first atomic mass was doubled b. when chemical properties were repeated c. when there were 10 elements in the row d. when the next element was a nonmetal 11. Mendeleev left gaps in his periodic table because a. the table was too small. c. the table was too full. b. protons belonged there. d. no known elements fit there. 12. Each column of the periodic table is a. an element. c. an isotope. b. a group. d. a period. 13. Atoms that gain or lose electrons are called a. metals. c. ions. b. nonmetals. d. isotopes. 14. Group 17 elements form a. +1 ion c. +7 ion b. -1 ion d. -7 ion 15. The three main groups of elements are metals, nonmetals, and a. inert gases. c. radioactive isotopes. b. alkali metals. d. semiconductors. 16. Most elements are a. metals. c. metalloids. b. nonmetals. d. semiconductors. 17. Most nonmetals are a. brittle. c. metalloids. b. good conductors. d. shiny. 18. Elements in an element family have similar a. atomic symbols. c. atomic weights. b. atomic sizes. d. chemical properties. 19. How do you know that potassium, an alkali metal, is highly reactive? a. It conducts heat. c. It is a soft and shiny metal. b. It conducts electricity. d. It has one valence electron. 20. The order of elements in the modern periodic table is based on an element s a. atomic number. c. chemical symbol. b. name. d. atomic mass. 21. Ionization refers to the process of a. changing from one period to another. c. turning lithium into fluorine. b. losing or gaining protons. d. losing or gaining electrons. 22. Elements that share properties of both metals and nonmetals are called a. ions. c. semiconductors. b. periods. d. valences.
23. Which statement about the alkali metals is correct? a. They are located in the left-most column of the periodic table. b. They are extremely nonreactive. c. They are usually gases. d. They form negative ions with a 1 charge. 24. Which statement about noble gases is correct? a. They form compounds with very bright colors. b. They exist as single atoms rather than as molecules. c. They are highly reactive with both metals and nonmetals. d. They are extremely rare in nature. 25. Which element is a semiconductor? a. carbon c. sodium b. silicon d. uranium 26. Metals tend to be a. gases. c. dull. b. good conductors of heat. d. brittle. 27. Different isotopes of the same element have different a. atomic numbers c. numbers if neutrons b. numbers of protons d. numbers of electrons Matching Match each item with the correct statement below. a. halogens d. semiconductors b. alkaline-earth metals e. alkali metals c. transition metals f. noble (inert) gases 28. Elements that have properties of both metals and nonmetals; located near the stair step line 29. Reactive elements of Group 17 that are poor conductors 30. Highly reactive elements that belong to Group 1 31. Very stable due to the fact that they have a full outermost energy level 32. Elements that belong to Groups 3-12 and are somewhat reactive 33. Group 2 elements that have two valence electrons
Name Period POGIL Periodic Table TRENDS Activity The Periodic Table is a map of the elements. There are many patterns or trends on the periodic table. Let s look and see what we can find. (Use your Regents Chemistry Reference Table and fill in the blanks with the appropriate answers.) Periods: (Horizontal) 1. Look at Na to Ar to answer the following questions. (Choose INCREASES, decreases, or remains the same.) 2. The atomic # (INCREASES, decreases, or remains the same.) 3. The # of protons 4. The # of valence electrons 5. The # of principle energy levels 6. All elements in the same period have the same Groups: (Vertical) Look at H to Fr to answer the following questions. (Choose INCREASES, decreases, or remains the same.) 1. The atomic # (INCREASES, decreases, or remains the same.) 2. The # of protons 3. The # of valence electrons 4. The # of principle energy levels 5. All elements in the same group have the same and therefore react similarly.
Atomic Radii: The atomic radius (or radii) is the distance from the center of the nucleus to the outer edge of the atom. This is used to tell how big the atom is. Look at your table S in your reference table and see if you can find these values. Let s look at some trends for these. Write down the information below for each element. The atomic radius is affected by 2 things: the number of principle energy levels and the attraction between protons and electrons. When comparing atomic radii, first, look at principle energy level.the more principle energy levels (p.e.l), the bigger the atom. Then, if the p.e.l. are the same, look at the number of protons to the number of electrons.more protons, means more attraction for electrons, and the electrons get sucked in closer to the nucleus, shrinking the atom. Periods: (Examine the elements in period 3) Na: Si: Cl: Radius # of principle energy levels # of protons # of electrons Radius # of principle energy levels # of protons # of electrons Radius # of principle energy levels # of protons # of electrons The radius (increases or DECREASES) as you go across a period due to an increase in the number of PROTONS in nucleus pulling electrons closer Groups: (Examine the elements in group 1) Li: Radius # of principle energy levels # of protons # of electrons K: Radius # of principle energy levels # of protons # of electrons Cs: Radius # of principle energy levels # of protons # of electrons The radius (INCREASES or decreases) as you go down a group due to more energy levels (shells of electrons)
Electronegativity Electronegativity is a measure of an atom s ATTRACTION for electrons in a bond with another atom. Electronegativity is measured on a scale of 0 to 4, with 4 being the highest electronegativity value. Fluorine, F, is the most electronegative element with a value of 4. Fluorine is located in the upper right corner of the Periodic Table. In general, the closer an atom is to F, the higher its electronegativity value. So, as you go across a period or up a group (toward F), electronegativity values increase. These values can also be looked up in Table S. Ionization Energy Ionization energy is the amount of energy required to REMOVE an electron from an atom in the gaseous state. This property of atoms is directly related to their electronegativity values the more attracted to electrons they are, the more energy it will take to pull an electron away. Ionization energies are also listed on Table S. Fill in the table below for the elements in Period 2 and Group 2 to note the general pattern of values. Period 2 Elements Li Be B C N O F Electronegativity Ionization Energy (kj/mol) *In general, as you go across a period, electronegativity and ionization energy (INCREASE or decrease) This is because the number of increases, so attraction to outermost electrons increases. (PROTONS or electron shells) Group 2 Elements Electronegativity Ionization Energy (kj/mol) Be Mg Ca Sr Ba *In general, as you go down a group, electronegativity and ionization energy (increase or DECREASE) This is because the number of increases, so attraction to outermost electrons decreases. (protons or ELECTRON SHELLS)
Skill 5: Identify Trends in the Periodic Table Trends Summary: Atomic Radius: - How far from valence to nucleus - Period - atomic radius as you go from left to right across a period. Why? - Stronger attractive forces in atoms (as you go from left to right) between the opposite charges in the nucleus, decreased shielding. - Group - atomic radius as you go down a group. Why? - Added energy levels. Increased layers, meaning increased distance to the nucleus Ionic Radius: - How far from valence electron to in an ION. - As one moves down a group on the periodic table, the ionic radius because additional electrons are being added to the atom. - Within a period, the radius trend is dependent on whether the ion is or. When moving across a period among positive ions, the number of protons increases. This decreases the ionic radius. - Among negative ions, additional layers of electrons are being added, which increases the radius.
Ionization Energy Why? - Ionization energy is the amount of energy required to the outmost electron. - Period - ionization energy as you go from left to right across a period. - Elements on the right of the chart want to take others atom's electron (not given them up) because they are close to achieving the. - The means it will more energy to remove the outer most electron. - Elements on the left of the chart would prefer to give up their electrons so it is to remove them, requiring energy (low ionization energy). - Group - ionization energy as you go down a group. Why? - The SHIELDING affect makes it easier to remove the outer most electrons from those atoms that have many electrons (those near the bottom of the chart). Electronegativity Why? Why? - Electronegativity is an atom's 'desire' to grab another atom's electrons - Period- electronegativity as you go from left to right across a period. - TRYING TO GET A NOBLE GAS CONFIGURATION. - Group - electronegativity as you go down a group. - The lower you go, the more shielding due to the increase in number of electrons. It s not such a big deal to lose a couple electrons.