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Types of Bonding and Lewis Structures Quiz on Monday
Describe the structure of metallic bonding. Positive metallic ions surrounded by electrons.
Example of Metallic Bonding
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
Potassium bromide forms a crystal lattice structure. What type of bonding would you expect it have? Ionic
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
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
Which of these elements would make a covalent bond with nitrogen? AlMgBaC C; non-metal with non-metal bonding (also similar electronegativity)
Which of these elements would make an ionic bond with potassium? MgNSrCl N, Cl; metal with non-metal bond (also difference in electronegativities is relatively large)
Which of these elements would make an ionic bond with chlorine? OFLiXe Li; metal with non-metal bond (also difference in electronegativities is relatively large)
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
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
Draw the correct Lewis dot structure for CH 2 O
Draw the correct Lewis dot structure for SCl 2
Draw the correct Lewis Dot Structure for O 2
Electron Configuration Review Questions
Write the electron configuration for the element fluorine 1s 2 2s 2 2p 5
Write the electron configuration for the element potassium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1
Write the electron configuration for the element silicon 1s 2 2s 2 2p 6 3s 2 3p 2
Write the electron configuration for the element titanium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2
Write the noble gas configuration for the element rubidium [Kr]5s 1
Write the noble gas configuration for the element chlorine [Ne]3s 2 3p 5
Which element has the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Iron, Fe
Which element has the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 Arsenic, As
Write the orbital notation for the element carbon ↑↓ ↑↓ ↑ ↑. 1s 2s 2p
Write the orbital notation for the element sulfur ↑↓ ↑↓ ↑↓ ↑↓ ↑↓. 1s 2s 2p ↑↓ ↑↓ ↑ ↑. 3s 3p
Write the orbital notation for the element selenium ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 1s 2s 2p 3s3p4s 3d 4p
Write the Lewis Dot structure for the following atoms and their ions
Aluminum Al (group 13; 3 valence electrons) Al +3 (aluminum loses its 3 valence electrons to satisfy the octet rule)
Phosphorus P (group 15; 5 valence electrons) P -3 (phosphorus gains 3 electrons to satisfy the octet rule)
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
Strontium Sr (group 2; 2 valence electrons) Sr +2 (strontium loses its 2 valence electrons to satisfy the octet rule)
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