BINGO

 Use study guide, worksheets, even questions at end of chapters 5 and 6.  Answer should be an “element”.  Clues may include a list of elements to select. ◦ Example: Which of the following elements has the highest ionization energy: Fr, K, Co, Br, Ne?

 Answer should be an “element”.  Clues may include a list of elements to select. ◦ Example: Which of the following elements has the highest ionization energy: Fr, K, Co, Br, Ne?  There are 5 categories:  B: Basic information / Atomic Radii  I: Ionization Energy  N: Electronegativity  G: Gain or lose electrons/ Ion Formation  O: Outermost / Valence Electrons

 Answer should be an “element”.  Clues may include a list of elements to select. ◦ Example: Which of the following elements has the highest ionization energy: Fr, K, Co, Br, Ne?  There are 5 categories:  B: Basic information / Atomic Radii  I: Ionization Energy  N: Electronegativity  G: Gain or lose electrons/ Ion Formation  O: Outermost / Valence Electrons  Create 5 clues for each category.  Each clue must have different element for the answer.

 Clues may include a list of elements to select.  There are 5 categories:  B: Basic information / Atomic Radii  I: Ionization Energy  N: Electronegativity  G: Gain or lose electrons/ Ion Formation  O: Outermost / Valence Electrons  Create 5 clues for each category.  Each clue must have different element for the answer.  Write your clue on lined side of card.  Write correct answer on back.

 Clues may include a list of elements to select.  There are 5 categories:  B: Basic information / Atomic Radii  I: Ionization Energy  N: Electronegativity  G: Gain or lose electrons/ Ion Formation  O: Outermost / Valence Electrons  Create 5 clues for each category.  Each clue must have different element for the answer.  Write your clue on lined side of card.  Write correct answer on back.

 Compare the two electron configurations and determine which element has a larger atomic radius? ◦ 1s 2 2s 2 2p 6 3s 2 or ◦ 1s 2 2s 2 2p 6 3s 2 3p 5

 Compare the core electron configurations and determine which element has a lower ionization energy? ◦ [Ne]3s 2 3p 5 or ◦ [Ar]4s 1

 Which element in the following list has highest electronegativity? ◦ Fr, Na, Si, Cl, Ar

 What element forms a -3 anion that has the following electron configuration? ◦ 1s 2 2s 2 2p 6

 What element in period 2 has 2 valence electrons?

 What element has two energy levels and is an alkaline earth metal?

 Which element in the following list has the largest atomic radius? ◦ Na, Si, Cl, Ar

 Which of the following elements has the highest ionization energy? ◦ He, Cl, Zn, Ba,

 Which element the has highest electronegativity of all the elements?

 What element forms a -2 anion that has the following electron configuration? ◦ 1s 2 2s 2 2p 6

 What representative element is in period 2 and has 4 valence electrons?

 Compare the two electron configurations and determine which element is larger in atomic radius? ◦ 1s 2 2s 2 2p 6 or ◦ 1s 2 2s 2 2p 6 3s 1

 Compare the core electron configurations and determine which element has a lower ionization energy? ◦ [Ar]4s 1 or ◦ [Kr]5s 1

 Which element in the following list has highest electronegativity? ◦ Fr, Fe, O, S, Xe

 With what element does Br become isoelectric when it forms the -1 anion: Br - ?

 What element is in period 3 and has 3 valence electrons?

 Compare the two core electron configurations and determine which element has the larger atomic radius? ◦ [Ne]3s 2 3p 3 or ◦ [Kr]5s 1

 Compare the electron configurations and determine which element has a higher ionization energy? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6 or ◦ 1s 2 2s 2 2p 6 3s 1

 Compare the electron configurations and determine which element has higher electronegativity? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6 or ◦ 1s 2 2s 2 2p 6 3s 1

 What element forms an +3 cation that is isoelectric with neon [Ne]?

 What element in 6 energy levels and has 4 valence electrons?

 Compare the two core electron configurations and determine which element is smaller in atomic radius? ◦ [Ne]3s 2 3p 3 or ◦ [Ne]3s 1

 Compare the electron configurations and determine which element has a higher ionization energy? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6 or ◦ 1s 2 2s 2 2p 6

 Compare the electron configurations and determine which has higher electronegativity? ◦ [Ne]3s 2 3p 2 or ◦ [Rn]7s 1

 What element forms an -1 anion that is isoelectric with krypton [Kr]?

 What element in 4 energy levels and is an alkaline earth metal?

 Compare the two electron configurations and determine which element has a smaller atomic radius? ◦ 1s 2 2s 2 2p 6 3s 2 3p 3 or ◦ 1s 2 2s 1

 Compare the electron configurations and determine which element has a higher ionization energy? ◦ 1s 2 2s 2 2p 6 or ◦ 1s 2 2s 2 2p 6 3s 2

 Which element in period 5 has the lowest electronegativity AND is not a noble gas?

 What element loses a 4s electron and “promotes” its other 4s electron to its 3d orbital to complete its d sublevel when it forms a +1 ion?

 What element has 4 energy levels and is a halogen?

 What element has the electron configuration? ◦ 1s 2 2s 2 2p 5

 Which element in the following list has the highest ionization energy? ◦ Fr, Fe, Ag or F

 Which element has the smallest atomic radius in its family and zero electronegativity?

 Which representative element in period 3 loses one electron when it forms an ion that is isoelectric with a noble gas?

 What element has 4 energy levels and has alkali metal?

 Compare the two core electron configurations and determine which element is more likely to attract electrons in a shared bond?. ◦ [Ne]3s 2 3p 3 or ◦ [Ne]3s 1

 Which of the following has zero electronegativity? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6 or ◦ 1s 2 2s 2 2p 5

 Compare the electron configurations and determine which element in the following has less attraction for electrons in a shared bond. ◦ [Ne]3s 2 3p 2 or ◦ [Rn]7s 1

 What element forms a -2 anion and has the highest electronegativity in its family?

 What element in 3 energy levels and has the highest electronegativity in its period?

 Compare the two electron configurations and determine which element has a larger atomic radius? ◦ 1s 2 2s 2 2p 6 3s 2 3p 4 or ◦ 1s 2 2s 2 2p 6 3s 1

 Compare the core electron configurations and determine which element has a lower ionization energy? ◦ [Kr]5s 1 or ◦ [Ne]3s 2 3p 5

 Which element in the following list has largest atomic radius? Fe, S, Si, Ca

 When calcium forms a +2 ion that is isoelectric with argon, both have the same electron configuration below. Which is smaller the atom of argon or the ion of calcium? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6

 What representative element has 3 valence electrons and has the smallest atomic radius in its family?

 Compare the two core electron configurations and determine which element is easier to remove an electron? ◦ [Ar]4s 2 or ◦ [Ne]3s 2

 Compare the electron configurations and determine which element has a higher ionization energy? ◦ 1s 2 2s 2 2p 6 3s 2 3p 6 or ◦ 1s 2 2s 2 2p 6

 Compare the electron configurations and determine which element takes less energy to remove an electron? ◦ [Ne]3s 2 3p 4 or ◦ [Ar]4s 2

 What element forms a -3 anion and has the highest ionization energy in its family?

 What element has 2 energy levels and requires the lowest energy to remove an electron in its period?

 Compare the two electron configurations and determine which element will gain electrons to form a stable ion? ◦ 1s 2 2s 2 2p 4 or ◦ 1s 2 2s 2 2p 6 3s 1

 Compare the core electron configurations and determine which element will lose 2 electron to form a stable ion? ◦ [Ne]3s 2 or ◦ [He]2s 1

 Which element in the following list has will form a positive ion? ◦ Fr, O, S, P, Xe

 With what element does Be become isoelectric when it forms the +2 cation Be +2 ?

 What element in period 3 loses 2 valence electrons to form an ion that is isoelectric with [Ne]?

 Compare the two electron configurations and determine which element will become a -2 ion when it forms a stable electron configuration? ◦ 1s 2 2s 2 2p 6 3s 2 or ◦ 1s 2 2s 2 2p 6 3s 2 3p 4

 Compare the core electron configurations and determine which element will become a +1 ion when it forms a stable electron configuration? ◦ [Ne]3s 2 3p 5 or ◦ [Ar]4s 1

 Which element in the following list gains 2 electrons to become a stable ion? ◦ Na, Si, S, Cl, Ar

 What element forms a -1 anion that has the following electron configuration? ◦ 1s 2 2s 2 2p 6

 What representative element has 4 energy levels and has 5 valence electrons?