Covalent Bonds
What is a covalent bond?
The force of attraction that holds together two atoms that share a pair of valence electrons.
What is an ionic bond?
The force of attraction between positively charged ions (cations) and negatively charged ions (anions).
What are London Dispersion Forces?
The weakest type of intermolecular forces that occur in all molecular samples.
What rule can you apply to predict the solubility of nitrates?
Nitrates are generally soluble in water.
What is the octet rule?
Atoms tend to bond in a way that gives them eight valence electrons.
What are the two types of electron pairs in a Lewis structure?
Bond pairs (shared) and lone pairs (not shared).
What happens to electrons in an ionic bond?
Electrons are completely transferred from one atom to another.
What is hydrogen bonding?
A strong dipole-dipole attraction that occurs when hydrogen is bonded to F, O, or N.
Are sulfides generally soluble or insoluble?
Sulfides tend to be insoluble.
How does electronegativity affect bond polarity?
The more electronegative atom attracts the shared electrons more strongly, creating polarity.
How do you determine the skeletal structure of a molecule?
By connecting the atoms together with enough electrons to form bonds.
How do you name a binary ionic compound?
Write the name of the cation first, followed by the name of the anion with an -ide ending.
Explain dipole-dipole interactions.
Attractions between opposite partial charges on opposite ends of polar molecules.
What are the exceptions to the solubility rules for carbonates?
Some carbonates, like those of alkali metals and ammonium, are soluble.
What is the difference between polar and nonpolar covalent bonds?
Polar bonds have unequal sharing of electrons, while nonpolar bonds share electrons equally.
What indicates that a molecule has a double bond in its Lewis structure?
Two pairs of electrons shared between two atoms.
What is the significance of Roman numerals in naming ionic compounds?
They indicate the oxidation state of the transition metal cation.
How do dipole-dipole forces compare to London Dispersion Forces in terms of strength?
Dipole-dipole forces are stronger than London Dispersion Forces.
Describe the difference between a precipitate and a soluble salt. Use the words solid and aqueous in your answer.
Precipitates will remain solid in solution while soluble salts will dissociate into component ions.
Explain what is meant by "expanded octet".
Some elements can have more than eight electrons in their valence shell, usually seen in elements in the third period or beyond.
Give an example of a molecule with a polar covalent bond and explain why it is polar.
Water (H2O); it is polar because oxygen is more electronegative than hydrogen, causing uneven sharing of electrons.
Predict the solubility of FeCO3 and explain why.
FeCO3 is likely insoluble because carbonates tend to form precipitates.
Why do molecules with hydrogen bonds have higher boiling points?
Because hydrogen bonds are strong attractions that require more energy to break.
Predict if a precipitate will form in the reaction 2AgNO3 + Na2S → Ag2S + 2NaNO3.
Yes, Ag2S is insoluble, so a precipitate will form.
What is the relationship between bond length and bond strength?
Generally, shorter bonds are stronger due to the closer proximity of the atoms' nuclei.