Structure 2

When metal atoms lose electrons, what type of ions do they form?

• Negative ions called anions

• Positive ions called cations

• Neutral atoms

• Molecules

What is the correct order for naming binary ionic compounds?

• Anion followed by cation with the suffix "ide"

• Cation followed by anion with the suffix "ide"

• Cation followed by anion without any suffix

• Anion followed by cation without any suffix

What type of bond is formed in an ionic bond?

• Covalent bond between similar atoms

• Metallic bond between metal atoms

• Electrostatic attraction between oppositely charged ions

• Hydrogen bond between polar molecules

Which of the following is a property of ionic compounds?

• High volatility

• Low electrical conductivity

• High electrical conductivity

• Poor solubility

What is the octet rule in the context of covalent bonding?

• The tendency of atoms to gain a valence shell with a total of 6 electrons.

• The tendency of atoms to lose their valence electrons and form ionic bonds.

• The tendency of atoms to gain a valence shell with a total of 8 electrons.

• The tendency of atoms to share all their valence electrons equally.

What is a coordination bond?

• A bond where electrons are shared between atoms of different elements.

• A bond where one atom donates both electrons to be shared with another atom.

• A bond where both electrons of the shared pair originate from the same atom.

• A bond where electrons are transferred from one atom to another.

What does the VSEPR model predict?

• The ionic character of bonds in a molecule.

• The number of valence electrons in an atom.

• The shapes of molecules based on the repulsion of electron domains around a central atom.

• The exact bond angles in a molecule without exceptions.

Which statement best describes the relationship between the number of shared electron pairs and the strength of the bond?

• Triple bonds are weaker than single bonds because they involve three shared pairs of electrons.

• Single, double, and triple bonds involve the same number of shared electron pairs and thus have the same strength.

• Single, double, and triple bonds involve one, two, and three shared pairs of electrons respectively, with triple bonds being the strongest.

• The number of shared electron pairs does not affect the strength of the bond.

What results from the difference in electronegativities of the bonded atoms in a covalent bond?

• Molecular polarity

• Ionic bonding

• Metallic bonding

• Covalent network structure

Which type of intermolecular force is generally the weakest?

• London (dispersion) forces

• Dipole-dipole forces

• Hydrogen bonding

• Ionic bonding