Chemistry Ionic Bonds and Forces Quiz

A type of chemical bond formed between two atoms when one atom donates an electron to another atom, resulting in electrostatic attraction between oppositely charged ions.

An atom that has gained one or more electrons and therefore carries a negative charge.

An atom that has lost one or more electrons and therefore carries a positive charge.

A type of chemical bond formed between two atoms when they share one or more pairs of electrons.

A covalent bond where electrons are shared equally between two atoms.

A covalent bond where electrons are shared unequally between two atoms.

A representation of the three-dimensional shape of a molecule using the Valence Shell Electron Pair Repulsion theory.

The attraction between molecules that results from temporary fluctuations in electron distribution.

Ionic compounds are formed when a metal atom loses electrons to become a positively charged ion (cation) and a nonmetal atom gains electrons to become a negatively charged ion (anion). The opposite charges attract, forming a strong electrostatic bond.

They typically have high melting points because the electrostatic forces between ions are strong and require a lot of energy to overcome.

They are generally hard because the tightly packed ions create a rigid structure.

Ionic compounds are brittle because any shift in the ion arrangement can cause similar charges to align, leading to repulsion and fracture.

Ionic compounds only conduct electricity when melted or dissolved because ions need to be free to move to carry the electrical charge.

Covalent compounds are formed when atoms share electrons to achieve a stable electron configuration. Electrons are shared equally in nonpolar covalent bonds and unequally in polar covalent bonds.

Covalent compounds generally have lower melting points than ionic compounds because there is a weaker attraction between molecules.

Covalent compounds don't conduct electricity well because they lack free-moving charged particles (ions or delocalized electrons).

When an atom gains an electron, it becomes negatively charged (anion). When an atom loses an electron, it becomes positively charged (cation).

Oppositely charged ions (anion and cation) attract each other due to electrostatic forces, forming an ionic bond. This attraction leads to the formation of a stable ionic compound.

Lithium (Li) has 1 valence electron and Chlorine (Cl) has 7 valence electrons. Lithium loses its valence electron becoming a positive ion (Li+), while Chlorine gains this electron, becoming a negative ion (Cl-) to achieve a stable octet in their outer shell.

A covalent bond is formed when two atoms share one or more pairs of electrons to achieve a stable octet in their outer shell.

When two atoms share electrons equally, it results in a nonpolar covalent bond. This occurs when the electronegativity difference between the atoms is small.

When two atoms share electrons unequally, it results in a polar covalent bond. This occurs when the electronegativity difference between the atoms is significant.

The valence shell electron pair repulsion (VSEPR) theory explains the shapes of molecules based on the repulsion between electron pairs in the outermost shell.

London dispersion forces are weak intermolecular attractions that arise from temporary fluctuations in electron distribution around atoms or molecules.

In a covalent compound, the central atom is usually the one that appears only once in the chemical formula. Hydrogen and fluorine are exceptions; they always occupy outer positions and never serve as central atoms.

Atoms that are attached to the central atom and typically located at the periphery of the molecule.

The theory that electron pairs in the outermost shell of an atom repel each other, arranging them in a specific geometrical shape.

Regions around the central atom where electron pairs reside - these can be single bonds, double bonds, or lone pairs.

An electron pair not involved in a bond, located on the central atom.

The three-dimensional arrangement of atoms in a molecule, determined by the repulsion of electron pairs around the central atom

Attractions between molecules that have a permanent dipole due to their polar nature.

A particularly strong type of dipole-dipole interaction involving a hydrogen atom bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine.

Forces that hold atoms together within a molecule.

Forces that occur between molecules; they are weaker than intramolecular forces.

The greater the number of electrons in a molecule, the stronger the London Dispersion Force.

The more polar the molecules, the stronger the dipole-dipole interaction.

Hydrogen bonding plays a crucial role in determining the physical properties of water, such as its high boiling point and its ability to dissolve many substances.

Describes a molecule with a separation of electrical charge, creating a positive and negative end due to the unequal sharing of electrons.

Describes a molecule with an even distribution of electrical charge, meaning there is no separation of charge.

The relative attraction of an atom for the shared electrons in a covalent bond.

The attraction between molecules due to temporary fluctuations in electron distribution within the molecules.