knowverseChemical bonding involves attractions among nuclei and electrons, forming ionic lattices or shared electron pairs in covalent bonds. The quiz covers Lewis structures, polar covalent bonds, double bonds, molecular shape from VSEPR, metallic bonding, and intermolecular attractions. Try all ten questions to check your understanding.
Your score is next.
Opposite ionic charges attract in the lattice.
In summary, an ionic bond is the result of an electron 'theft' that creates oppositely charged ions, which then pull together into a lattice.
From the Knowverse course text.
Covalent bonding involves shared electron pairs.
In a covalent bond, two atoms share a pair of valence electrons to achieve stability.
From the Knowverse course text.
Lewis structures track valence electrons.
To solve this, we use a visual map called a Lewis structure to account for every outer electron in a molecule.
From the Knowverse course text.
A double bond shares two pairs.
Yes! While this chapter focused on single pairs, atoms can share two or even three pairs of electrons to reach their octet. These are called double and triple bonds, which we will explore in an upcoming chapter.
From the Knowverse course text.
The more electronegative atom attracts the shared electrons more strongly.
The atom with higher electronegativity gets a partial negative charge, written as $\delta^{-}$.
From the Knowverse course text.
A multiple bond occupies one region around the central atom.
It is important to remember that a double or triple bond is still just one region of space, so it only counts as one domain.
From the Knowverse course text.
Two domains maximize their separation at 180 degrees.
When a central atom has exactly two electron domains, they push to opposite sides of the atom.
From the Knowverse course text.
Water has two bonds and two lone pairs around oxygen. Its molecular shape is bent.
With two lone pairs pushing down on the two $O-H$ bonds, the molecule is forced into a bent shape.
From the Knowverse course text.
Delocalized electrons can move through the metal.
These lost electrons are now delocalized, which means they are no longer tied to any single atom.
From the Knowverse course text.
Steam still contains water molecules. Boiling does not chemically split them.
When you boil a pot of water on the stove, the steam rising into the air is still made of the same H2O molecules that were in the liquid phase.
From the Knowverse course text.
See the answer and explanation for each question below.
Find more quizzes and full courses in the free iOS app.
Read more about the topic
Chemical bonding involves attractions among nuclei and electrons. In the ionic model, atoms form positive and negative ions that attract within a lattice. Covalent bonding shares electron pairs between atoms. These descriptions are useful models, and the degree of electron sharing varies rather than following a perfectly sharp boundary.
A Lewis structure shows valence electrons as dots and bonds as shared pairs. Single, double and triple bonds share one, two and three pairs respectively. Electronegativity describes attraction for bonding electrons. Unequal sharing makes a polar bond, with a partial negative charge toward the more electronegative atom.
In reality, bonding exists on a spectrum. While we teach ionic bonding as a complete transfer, most bonds have a tiny bit of sharing. However, for compounds like NaCl, the transfer is so nearly complete that the 'purely ionic' model is highly accurate.
From the Knowverse course text.
The VSEPR model predicts shapes from repulsion between electron domains around a central atom. A multiple bond counts as one domain. Two domains arrange linearly, while four have a tetrahedral arrangement. Lone pairs affect the arrangement of bonded atoms: water has four domains around oxygen but a bent molecular shape.
Metallic bonding involves positive metal centers and delocalized electrons, helping explain electrical conductivity. Attractions between molecules also affect a substance's behavior. Boiling water separates molecules without breaking their internal oxygen-hydrogen bonds. Hydrogen bonding between neighboring water molecules is an intermolecular attraction, distinct from the covalent bonds inside each molecule.
To predict a shape, we first count the electron domains, which are simply the regions where electrons are found.
From the Knowverse course text.
Sources: Principles of Chemical Bonding. Each question or step includes an excerpt from the course.
