Types of Bonding and Lewis Structures
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Types of Bonding and Lewis StructuresQuiz on Monday
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Describe the structure of metallic bonding.
•Positive metallic ions surrounded by electrons.
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Example of Metallic Bonding
Click icon to add picture
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What type of bonding must exist if a substance can conduct electricity dry? Why?
Metallic; the delocalized electrons are able to flow freely around the positive metal ions
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Potassium bromide forms a crystal lattice structure. What type of bonding would you expect it have?
Ionic
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If a substance dissolves in water and makes a solution that conducts electricity, what types of bonds do you expect hold it together?
•Ionic; forms ions in solution to make it an electrolyte
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If a substance melts in your hands, what type of bonds do you expect to hold it together?
Covalent (polar and non-polar); covalently bonded substances have low melting points
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Which of these elements would make a covalent bond with nitrogen?
Al Mg Ba C
•C; non-metal with non-metal bonding (also similar electronegativity)
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Which of these elements would make an ionic bond with potassium?
Mg N Sr Cl•N, Cl; metal with non-metal bond (also difference in electronegativities is relatively large)
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Which of these elements would make an ionic bond with chlorine?
O F Li Xe
•Li; metal with non-metal bond (also difference in electronegativities is relatively large)
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What type of bond exists between chlorine (EN = 3.0) and bromine (EN = 2.8)
•Non-polar covalent; both elements are non-metals with their difference in electronegativity being less than 0.5
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What type of bond exists between nitrogen (EN = 3.0) and hydrogen (EN = 2.1)
•Polar covalent; both elements are non-metals with their difference in electronegativity being between 0.5 and 1.7
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Draw the correct Lewis dot structure for CH2O
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Draw the correct Lewis dot structure for CH2O
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Draw the correct Lewis dot structure for SCl2
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Draw the correct Lewis dot structure for SCl2
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Draw the correct Lewis Dot Structure for O2
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Draw the correct Lewis Dot Structure for O2
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Electron ConfigurationReview Questions
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Write the electron configuration for the element fluorine
•1s22s22p5
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Write the electron configuration for the element potassium
•1s22s22p63s23p64s1
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Write the electron configuration for the element silicon
•1s22s22p63s23p2
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Write the electron configuration for the element titanium
•1s22s22p63s23p64s23d2
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Write the noble gas configuration for the element rubidium
•[Kr]5s1
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Write the noble gas configuration for the element chlorine
•[Ne]3s2 3p5
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Which element has the following electron configuration:
1s22s22p63s23p64s23d6
•Iron, Fe
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Which element has the following electron configuration:
1s22s22p63s23p64s23d104p3
•Arsenic, As
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Write the orbital notation for the element carbon
•↑↓ ↑↓ ↑ ↑ . 1s 2s 2p
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Write the orbital notation for the element sulfur•↑↓ ↑↓ ↑↓ ↑↓ ↑↓. 1s 2s 2p •↑↓ ↑↓ ↑ ↑ . 3s 3p
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Write the orbital notation for the element selenium•↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
1s 2s 2p 3s 3p 4s
3d 4p
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Write the Lewis Dot structure for the following atoms and their ions
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Aluminum
Al (group 13; 3 valence electrons)
Al+3 (aluminum loses its 3 valence electrons to satisfy the octet rule)
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Phosphorus
P (group 15; 5 valence electrons)
P -3 (phosphorus gains 3 electrons to satisfy the octet rule)
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Helium
He (group 18 but it has 2 valence electrons)
No ionic form of helium. It already has a full valence shell so it already satisfies the octet rule
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Strontium
Sr (group 2; 2 valence electrons)
Sr+2 (strontium loses its 2 valence electrons to satisfy the octet rule)