Types of Bonding and Lewis StructuresQuiz on Monday

Describe the structure of metallic bonding.

•Positive metallic ions surrounded by electrons.

Example of Metallic Bonding

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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

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?

Al Mg Ba C

•C; non-metal with non-metal bonding (also similar electronegativity)

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)

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)

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 CH2O

Draw the correct Lewis dot structure for CH2O

Draw the correct Lewis dot structure for SCl2

Draw the correct Lewis dot structure for SCl2

Draw the correct Lewis Dot Structure for O2

Draw the correct Lewis Dot Structure for O2

Electron ConfigurationReview Questions

Write the electron configuration for the element fluorine

•1s22s22p5

Write the electron configuration for the element potassium

•1s22s22p63s23p64s1

Write the electron configuration for the element silicon

•1s22s22p63s23p2

Write the electron configuration for the element titanium

•1s22s22p63s23p64s23d2

Write the noble gas configuration for the element rubidium

•[Kr]5s1

Write the noble gas configuration for the element chlorine

•[Ne]3s2 3p5

Which element has the following electron configuration:

1s22s22p63s23p64s23d6

•Iron, Fe

Which element has the following electron configuration:

1s22s22p63s23p64s23d104p3

•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 3s 3p 4s

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)