Physical Properties of Ionic Compounds

<p>Electrostatic energy (D)</p> Signup and view all the answers

<p>Bubbling and steam production (A)</p> Signup and view all the answers

<p>In aqueous solution (A)</p> Signup and view all the answers

<p>Electrolytes (A)</p> Signup and view all the answers

<p>Their ions are fixed in place. (D)</p> Signup and view all the answers

<p>They behave as electrical insulators. (B)</p> Signup and view all the answers

<p>They are dissociated and free to move. (D)</p> Signup and view all the answers

<p>They tend to have low melting and boiling points. (A)</p> Signup and view all the answers

<p>Their intermolecular forces are relatively weak, making them soft and flexible. (A)</p> Signup and view all the answers

<p>They form crystalline structures. (A)</p> Signup and view all the answers

<p>Covalent bonds are relatively flexible and easy to break. (D)</p> Signup and view all the answers

<p>Water (C)</p> Signup and view all the answers

<p>They are generally weaker than those in ionic compounds. (B)</p> Signup and view all the answers

<p>Plasma (A)</p> Signup and view all the answers

<p>Ionic compounds conduct electricity when dissolved in water. (D)</p> Signup and view all the answers

<p>They melt without breaking down. (A)</p> Signup and view all the answers

<p>They have a brittle crystalline structure. (B)</p> Signup and view all the answers

<p>Strong electrostatic attraction between ions (B)</p> Signup and view all the answers

<p>Same charge ions move closer and repel each other (C)</p> Signup and view all the answers

<p>Applying force disrupts the ionic structure (A)</p> Signup and view all the answers

<p>Brittleness (C)</p> Signup and view all the answers

<p>Strong ionic bonds and structured lattice (B)</p> Signup and view all the answers

<p>Poor electrical conductivity (C)</p> Signup and view all the answers

<p>Good ionic conduction (B)</p> Signup and view all the answers

<p>Both solid and liquid (C)</p> Signup and view all the answers

<p>Weaker in covalent compounds (A)</p> Signup and view all the answers

<p>They do not conduct electricity in any state. (C)</p> Signup and view all the answers

<p>The differences in the electronegativity of the bonded atoms (A)</p> Signup and view all the answers

<p>Dichloromethane (CH₂Cl₂) (A)</p> Signup and view all the answers

<p>Polar and Nonpolar (D)</p> Signup and view all the answers

<p>They can only be nonpolar. (A)</p> Signup and view all the answers

<p>They have a symmetrical distribution of electron density. (C)</p> Signup and view all the answers

<p>The tendency of an atom to attract electrons (B)</p> Signup and view all the answers

<p>Lithium (Li) (A)</p> Signup and view all the answers

<p>One decimal place (D)</p> Signup and view all the answers

<p>Halogens (B)</p> Signup and view all the answers

<p>Fluorine (C)</p> Signup and view all the answers

<p>Electronegativity difference (B)</p> Signup and view all the answers

<p>It increases (B)</p> Signup and view all the answers

<p>Nonpolar covalent bond (D)</p> Signup and view all the answers

<p>It decreases (D)</p> Signup and view all the answers

<p>Unequal sharing of electrons (B)</p> Signup and view all the answers

<p>Covalent compounds are significantly more flammable than ionic compounds. (A)</p> Signup and view all the answers

<p>Carbon dioxide and water (D)</p> Signup and view all the answers

<p>They do not dissociate into ions. (A)</p> Signup and view all the answers

<p>Covalent compounds do not conduct electricity when dissolved in water. (A)</p> Signup and view all the answers

<p>They release energy when reacting with oxygen. (C)</p> Signup and view all the answers

When ionic compounds dissolve in water, the ions separate and can carry current, making the solution conductive.

Solid ionic compounds do not conduct electricity; they are insulators.

An ionic substance that conducts electricity when dissolved in water.

A material that does not allow electric current to flow easily.

Separation of cations and anions when an ionic compound dissolves in water.

Substances formed by ions held together by electrostatic forces.

Characteristics that can be observed without changing the substance's identity.

Ionic compounds typically require significant energy to break the strong bonds.

Ionic compounds tend to dissolve easily in water or other polar solvents.

Ionic compounds conduct electricity when molten or dissolved.

Solid ionic compounds are hard because of strong electrostatic attraction between ions.

Ionic compounds break easily when pressure/force is applied.

The strong force that holds ions together in an ionic compound.

The force that pushes ions with the same charge apart.

The tendency of ionic compounds to break under stress due to repulsion of like charges.

Molecules formed by sharing electrons between atoms.

The temperature at which a solid changes to a liquid.

The temperature at which a liquid changes to a gas.

The ability of a substance to dissolve in a solvent.

A regular, geometric arrangement of ions in an ionic compound. Different compounds have different lattice structures.

The strong attraction between oppositely charged ions in a crystal lattice, holding them together.

Similar to melting, breaking the ionic bonds to turn a solid into a gas requires a lot of energy, resulting in high boiling points.

Ionic compounds are hard due to the strong electrostatic forces holding the ions in a rigid crystal lattice.

A covalent bond where electrons are shared unequally, resulting in a slightly positive and slightly negative end of the molecule.

A covalent bond where electrons are shared equally between atoms, resulting in no overall charge separation.

The ability of an atom in a molecule to attract shared electrons towards itself.

A molecule that has a positive and negative end due to unequal sharing of electrons in its covalent bonds.

A molecule where electrons are shared equally, resulting in no overall charge separation.

Covalent compounds often have low melting and boiling points because the intermolecular forces (attraction between molecules) are weak, even though the covalent bonds within the molecules are strong.

Covalent compounds are often soft and flexible because the bonds between atoms are relatively easy to break. This allows molecules to slide past each other.

Covalent compounds are often found as gases, liquids, or soft solids at room temperature due to their weak intermolecular forces.

These are the forces of attraction between molecules in a covalent compound. They are weaker than the covalent bonds within the molecules.

The weak intermolecular forces in covalent compounds require less energy to overcome, leading to lower melting and boiling points compared to compounds with strong intermolecular forces.

Electronegativity increases across a period and decreases down a group on the periodic table.

Compare the electronegativity values of the atoms involved. A large difference indicates a polar covalent bond, while a small difference suggests a nonpolar covalent bond.

Electronegativity generally increases across a period (from left to right) and decreases down a group (from top to bottom) on the periodic table.

A high electronegativity value indicates that an atom strongly attracts electrons in a covalent bond. This leads to a more polar bond.

A low electronegativity value indicates that an atom weakly attracts electrons in a covalent bond. This leads to a less polar bond.

The difference in electronegativity values between two bonded atoms determines the type of bond (ionic, polar covalent, nonpolar covalent).

Covalent compounds tend to be more flammable than ionic compounds because they react with oxygen to produce energy, releasing carbon dioxide and water.

A chemical reaction that releases energy when a substance reacts with oxygen, typically producing carbon dioxide and water.

Covalent compounds dissolve as molecules, not ions. Since they don't have free-moving charged particles, they can't conduct electricity.

Ionic compounds conduct electricity when dissolved because they form ions. Covalent compounds don't form ions, so they don't conduct.

Covalent compounds dissolve as molecules, maintaining their original structure. Ionic compounds break apart into ions.