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    Periodicity of Elements POGIL Period 3 and 7 Version Assigned as CW on 1/3/20 and 1/6/2020
     
     
      
    Groups of the PT MC Questions Assigned as HW on 1/9/20
     
     
    Periodic Trends Packet Assigned as HW on 1/13/20
     
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    Review Book Question Answers- Q #1-21 on pages 83 and 84- Assigned as HW on 1/8/18
    1) 1.
    2) 2.
    3) 2. Groups 1-12 contain all metals only.
    4) 4. Metals and metalloids exist as only solids or Mercury which is a liquid.
    5) 2. Metals have low electronegativity values and low ionization energies, causing them to lose valence electrons and form cations.
    6) 2. Metals are good conductors of heat due to their mobile valence electrons.
    7) 4. Nonmetal atoms prefer to gain valence electrons because they have high electronegativities and high ionization energies. Gaining electrons causes the radius to increase.
    8) 1. A Mg atom has a larger radius because a Mg +2 ion has lost 2 valence e- and an entire principle energy level.
    9) 3. Sodium is the only metal and it loses electrons when forming an ion.
    10) 1. K has an electron configuration of  2-8-8-1 and loses the last valence electron to attain a noble gas configuration.
    11) 1. 
    12) 4. Metals are good conductors
    13) 3. As is a metalloid.
    14) 3. Si and Ge are metalloids.
    15) 1. As is a metalloid.
    16) 4. As is a metalloid. (metalloids= B, Si, Ge, As, Sb, Te and Po)
    17) 3. Bromine is a halogen and the halogens are the most reactive nonmetals. Kr is an inert noble gas because of it's full valence shell.
    18) 3.
    19) 1. Nonmetals do not have mobile valence e- so they do not conduct and are brittle.
    20) 4. Fluorine is a nonmetal with the highest electronegativity. The more easily a nonmetal can gain an electron, the more reactive the nonmetal.
    21) 3. Brittle and being a poor conductor are nonmetal properties.
     
     
    PT Review 2019 with Answer Key Distributed on 1/10/19
       
     
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    Groups of the PT WS 1 Answer Key Assigned as HW on 1/9/18
     
    Groups of the PT WS 2 Answer Key Assigned as HW on 1/11/18
     
     
    What is the Periodic Table of Elements Activity WS Answer Key Assigned as CW on 1/17/18
     
    Lewis Dot Diagrams of Atoms and Ions POGIL Answer Key  Assigned as classwork on 12/19/16-12/20/16
     
    Lewis Dot Diagrams Worksheet Answer Key  Assigned as classwork 12/21/16-12/22/16
     
    Prentice Hall Review Book Answers- Pages 90-91. #30-54 and Page 96. #39,41,44. HW on 1/4/17
    30) 4. Nonmetals have higher first ionization energies and metals have lower first ionization energies.
    31) 1. As you go down a group the number of principle energy levels increases, causing the valence e- to move further from the nucleus. This weakens the hold on electrons making it easier to remove them, causing ionization energy to decrease.
    32) 3.  Calcium has a stronger nuclear charge, pulling the valence e- in closer with a stronger grip. Since it's harder to remove valence e- because they're closer to the nucleus, the reactivity is lower.
    33) 4. Elements in the same period have the same number of principle energy levels filled.
    34) 1. Electronegativity decreases down a group because as the number of PEL's increases, the nucleus becomes more shielded and has a weaker attraction for outer electrons.
    35) 4. Nonmetals have higher electronegativities, metals have lower electronegativities.
    36) 4. Nonmetals have high IE and EN
    37) 1. Diatomic element with high IE describes a nonmetal. All diatomics are nonmetals (BrINClHOF)
    38) 2. Poor conductor of electricity and high IE describes a nonmetal. S is the only nonmetal.
    39) 1. As atomic number increases across a period, the nuclear charge increases causing the electrons and PELS to pull in closer and the  radius decreases.
    40) 4. Cl has the largest nuclear charge in the same period, therefore the PEL's are pulled in the most, resulting in the smallest radius.
    41) 3. The smaller nuclear charge causes the attraction for e- to be weaker and more spread out than in calcium.
    42) 1. Ni has the strongest nuclear charge out of the given elements, causing the radius to be the smallest.
    43) 4. Nonmetals are located on the upper right of the periodic table.
    44) 2. Alkali metals are the most reactive metals. The larger the metal element, the farther away the valence e- are from the nucleus making them the easiest to remove. The easier a metal can lose an electron, the more reactive the metal. Fr is the most reactive metal.
    45) 1. Nonmetals are located on the upper right of the table. The more easily a nonmetal can gain an electron, the more reactive the nonmetal. F is the most reactive nonmetal.
    46) 2.  Fluorine and Chlorine are gases. Bromine is a liquid. Iodine is a solid.
    47) 1. Alkali metals and Alkaline earth metals are extremely reactive and only found in compounds. ex: NaCl and CaCl2
    48) 4.
    49) 1.
    50) 1. Elements in the same group have similar chemical properties because they have the same number of valence e-.
    51) 2. Alkali metals are the most reactive. Argon is nonreactive (noble gas, stable octet). Gold is stable and nonreactive. Sulfur is stable.
    52) 4.
    53) 4. Nonmetals are in the upper right hand corner.
    54) 3. Elements with the same number of valence electrons have similar chemical properties because they form the same type of ion.
    39) A K+ ion has 1 more principle energy level than a Na+ ion.
    41) As atomic number increases down group 1, the ionization energy decreases.
    44) Group 2 elements are metals which lose 2 electrons when forming an ion and a principle energy level. This makes the ion have a smaller radius than an atom.
     
    Periodic Trends Packet Assigned as CW and HW on 1/5/17
     
     
    Periodic Table Review Packet Answers Given out in class on 12/22/15
     
    Prentice Hall Review Book Answers- Pages 94-96. #1-34. 1/8/15
    1) 1.
    2) 4. Nonmetals are brittle (not malleable or ductile), poor conductors, dull and gain e- because they have high IE and high EN.
    3) 2. Metals always lose electrons and losing a negatively charged particle results in having an overall positive charge.
    4) 4. Nonmetals gain electrons and the gain of e- causing the radius to increase.
    5) 1.
    6) 4. Bromine is the only liquid nonmetal.
    7) 2. Transition elements are known for their ability to produce brightly colored compounds, ions and solutions.
    8) 1. Metals have low IE and low EN while nonmetals have high IE and high EN
    9) 2. Metals have low IE and low EN while nonmetals have high IE and high EN
    10) 4. Metals lose electrons. The more easily a metal can lose electrons, the more metallic the element is. The metals are located to the left of the boron staircase.
    11) 4. F and Cl are gases, Br is a liquid and I is a solid.
    12) 2. Nitrogen, fluorine and chlorine are all diatomic. (BrINClHOF) Neon is an unreactive  and stable element that can exist monatomically.
    13) 2. If elements have the same number of valence electrons in the same group they will form the same type of ion resulting in similar chemical properties.
    14) 2. Alkaline earth metals (Group 2) and Alkali metals (Group 1) are very reactive metals only found in compounds. Group 18 = noble gases, Group 11 are transition metals, Group 14 contains stable nonmetals, metalloids and metals.
    15) 4. All metals are solids except mercury Hg which is liquid. Metalloids are solids. Most nonmetals are gases but some exist as solids, carbon, sulfur, iodine, phosphorus and selenium.
    16) 1. Barium forms a Ba+2 ion. The +2 charge indicates that barium loses 2e resulting in a smaller ion because it has one less energy level. Ba= 2-8-18-18-8-2 and Ba+2= 2-8-18-18-8
    17) 4. Malleable and ductile are properties of a metal. S is a nonmetal, Si and Ge are metalloids. Au is gold, the only metal given.
    18) 1. Ca is the most metallic because it is the farthest left in the period and loses its e- most easily. Losing e- is a characteristic of a metal.
    19) 3. Group 14 contains Si and Ge, Group 15 contains As and Sb, Group 16 contains Te.
    20) 3. Ni is a transition metal which forms colored compounds, ions, and solutions.
    21) 4. Read Table S. Na= 496 kj/mol, Al= 578 kj/mol, Ca= 590 kj/mol, P= 1012 kj/mol. Also, nonmetals always have higher first ionization energies than metals.
    22) 2. Nonmetals have high IE and high EN.
    23) 1. As you move across a period (Period 3) the nuclear charge increases, pulling the electrons and their energy levels in closer.
    24) 3. Na+= 2-8, Mg+2=2-8, K+= 2-8-8 and Ca+2= 2-8-8. Both K+ and Ca+2 have 3 energy levels but because potassium has one less proton than calcium its hold on the e- is a little weaker, allowing them to spread out more, resulting in a larger radius.
    25) 4. Elements in the same group have the same number of valence electrons.
    26) 4. Krypton has it's valence electrons the farthest from it's nucleus so it is the most likely noble gas to be forced into a reaction.
    27) 3. Silicon is in the same group as Carbon, group 14 and they both have 4 valence electrons.
    28) 3. Alkali metals have a +1 ion charge and oxygen has a -2 ion charge. To form a compound, which is neutral and has zero charge you will need 2 atoms of the +1 alkali metal to balance the -2 charge from the 1 oxygen. 2 "M"s and 1 "Oxygen" = M2O
    29) 4. 28 inner electrons + 7 valence electrons = 35 electrons total. 35 e= 35 p= atomic number 35= Bromine. Bromine is in period 3.
    30) They elements are also arranged by reactivity in Groups by Mendeleev. Iodine has 7 valence electrons and belongs in group 17 while Sulfur has 6 valence electrons and belongs in Group 16. Elements in the same group have similar chemical properties.
    31) Mg+2 and Al+3 are isoelectronic and both have an e- configuration of 2-8 which is the same as Neon's, Cl-, K+, and S-2 are isoelectronic and all have an e- configuration of 2-8-8 which is the same as Argon's.
    32) X2O3. Oxygen as an ion in a compound has a charge of -2. Having three oxygen ions gives a total nonmetal charge of -6. The two metals elements, "X" need to have a total charge of +6 to balance the total charge coming from the oxygen ions. Since there are 2 "X's" each one needs to have a +3 charge. Therefore a metal ion with a +3 charge can be found in Group 13 on the Periodic Table. ex: Al+3
    33)  Germanium and Arsenic in Period 4 or Antimony and Tellurium in Period 5.
    34) Group 1 metals form +1 ions and react vigorously with water and air because they only need to lose 1 valence electrons to attain a noble gas electron configuration.
     
    Prentice Hall Review Book Answers- Pages 91-92. #30-65. 1/7/15
    30) 4. Nonmetals have higher first ionization energies and metals have lower first ionization energies.
    31) 1. As you go down a group the number of principle energy levels increases, causing the valence e- to move further from the nucleus. This weakens the hold on electrons making it easier to remove them, causing ionization energy to decrease.
    32) 3.  Calcium has a stronger nuclear charge, pulling the valence e- in closer with a stronger grip. Since it's harder to remove valence e- because they're closer to the nucleus, the reactivity is lower.
    33) 4. Elements in the same period have the same number of principle energy levels filled.
    34) 1. Electronegativity decreases down a group because as the number of PEL's increases, the nucleus becomes more shielded and has a weaker attraction for outer electrons.
    35) 4. Nonmetals have higher electronegativities, metals have lower electronegativities.
    36) 4. Nonmetals have high IE and EN
    37) 1. Diatomic element with high IE describes a nonmetal. All diatomics are nonmetals (BrINClHOF)
    38) 2. Poor conductor of electricity and high IE describes a nonmetal. S is the only nonmetal.
    39) 1. As atomic number increases across a period, the nuclear charge increases causing the electrons and PELS to pull in closer and the  radius decreases.
    40) 4. Cl has the largest nuclear charge in the same period, therefore the PEL's are pulled in the most, resulting in the smallest radius.
    41) 3. The smaller nuclear charge causes the attraction for e- to be weaker and more spread out than in calcium.
    42) 1. Ni has the strongest nuclear charge out of the given elements, causing the radius to be the smallest.
    43) 4. Nonmetals are located on the upper right of the periodic table.
    44) 2. Alkali metals are the most reactive metals. The larger the metal element, the farther away the valence e- are from the nucleus making them the easiest to remove. The easier a metal can lose an electron, the more reactive the metal. Fr is the most reactive metal.
    45) 1. Nonmetals are located on the upper right of the table. The more easily a nonmetal can gain an electron, the more reactive the nonmetal. F is the most reactive nonmetal.
    46) 2.  Fluorine and Chlorine are gases. Bromine is a liquid. Iodine is a solid.
    47) 1. Alkali metals and Alkaline earth metals are extremely reactive and only found in compounds. ex: NaCl and CaCl2
    48) 4.
    49) 1.
    50) 1. Elements in the same group have similar chemical properties because they have the same number of valence e-.
    51) 2. Alkali metals are the most reactive. Argon is nonreactive (noble gas, stable octet). Gold is stable and nonreactive. Sulfur is stable.
    52) 4.
    53) 4. Nonmetals are in the upper right hand corner.
    54) 3. Elements with the same number of valence electrons have similar chemical properties because they form the same type of ion.
    55) 2. There are seven diatomic elements. BrINClHOF 
    56) 2. Same group.
    57) 3. Same group.
    58) 3. Potassium has the lowest EN and lowest IE making it lose it's electrons most easily.
    59) 2. Group 2 elements form +2 ions and when combined with chlorine which has a -1 ion you need 2 Cl's to balance the +2 charge from the metal, resulting in a neutral compound. 1 group 2 metal "M" and 2 Cl atoms= MCl2 
    60) 1. These elements are in different groups. 
    61) 3. Good conductivity and luster are properties of a metal.
    62) 3. Metals lose valence electrons to form positive ions.
    63) 1. Bi is the only metal out of the elements given.
    64) 1. F and Cl are gases, Br is a liquid, I is a solid.
    65) 3. Group 16 contains nonmetals which gain electrons. Group 1 and 2 are metals which always lose electrons. Group 18 elements are the noble gases which do not gain or lose electrons because they already have a full valence shell.