Ionic bonding assignment and quiz

Which statement describes a step in the formation of an ionic bond? An attraction occurs between two ions that have the same charge. A metal atom forms a cation, and a nonmetal atom forms an anion. A more electronegative atom transfers electrons to a less electronegative atom. A metal pulls electrons from another metal and produces a force of attraction.

A metal atom forms a cation, and a nonmetal atom forms an anion.

Which property best indicates that a compound contains an ionic bond? It is insoluble in water. It can be easily flattened. It has a low boiling point. It conducts electricity when molten.

It conducts electricity when molten.

Which statement is true about a polyatomic ion? It forms metallic bonds with other ions. It forms covalent bonds with other ions. It is made of atoms that are covalently bonded together. It has a charge that is distributed over part of the entire unit.

It is made of atoms that are covalently bonded together.

Which statement indicates that a substance may be an ionic compound? It has a low melting point. It is made up of molecules. It can be flattened by a force. It is made up of a crystal lattice.

It is made up of a crystal lattice.

Which pair of elements will form an ionic bond? N and O K and Br C and Cl Fe and Ni

K and Br

Each model shows bonding between a pair of atoms. Which statement best explains how the models differ? Model A shows the formation of ions, and model B does not show the formation of ions. Model A does not show the formation of ions, and model B shows the sharing of electrons. Model A shows the sharing of electrons, and model B shows the formation of ions. Model A shows the transfer of an electron, and model B shows the sharing of electrons.

Model A shows the sharing of electrons, and model B shows the formation of ions.

Which chemical species can easily form an ionic bond with a cation? Sr Ne NH4+ PO43-

PO4 3-

The table lists the lattice energies of some compounds. Compound Lattice Energy (kJ/mol) LiF -1,036 LiCl -853 NaF -923 KF -821 NaCl. -786 Which statement about crystal lattice energy is best supported by the information in the table? The lattice energy increases as cations get smaller, as shown by LiF and KF. The lattice energy increases as the cations get larger, as shown by LiF and LiCl. The lattice energy decreases as cations get smaller, as shown by NaCl and NaF. The lattice energy decreases as the cations get smaller, as shown by NaF and KF.

The lattice energy increases as cations get smaller, as shown by LiF and KF.

Which statement best describes how an ionic bond forms? The transfer of electrons forms strong bonds between ions. The sharing of electrons forms strong bonds between ions. The transfer of electrons results in attractive forces between molecules. The sharing of electrons results in attractive forces between molecules.

The transfer of electrons forms strong bonds between ions.

Which statement is true about ionic compounds? They are made up of many large molecules that are bonded together. They are made up of atoms of only one type of element. They are made up of particles that are arranged in a repeating pattern. They are made up of a random ratio of elements that are bonded together.

They are made up of particles that are arranged in a repeating pattern.

Compare a crystal lattice with a molecule. What does the formula unit Al(OH)3 tell you about the compound aluminum hydroxide?

Which of the following did you include? A crystal lattice is a solid in which the particles are arranged in a regular, repeating pattern. A molecule is a discrete unit of atoms that is bonded together. Many ions come together to form a crystal. The formula unit of an ionic compound represents the smallest ratio of ions in the crystal. The lattice of aluminum hydroxide has three OH- ions for every Al3+ ion.

Explain what lattice energy is and how it affects the properties of ionic compounds. Describe the general properties of ionic compounds.

Which of the following did you include? Lattice energy is a way to measure the bond strength in ionic compounds. Ionic compounds tend to have high melting and boiling points. Ionic compounds tend to be hard. Ionic compounds have a range of solubilities. Ionic compounds are not conductors in the solid state, but they are good conductors as liquids or in solution.

Describe the ammonium ion, NH4+, and the sulfate ion, SO42-. What compounds would these ions form with potassium and fluoride ions? Write the formula units for the resulting compounds.

Which of the following did you include? The atoms in each ion are bonded together covalently to form a single unit. The charge is distributed over the entire ion. The formula of ammonium fluoride is NH4F. The formula of potassium sulfate is K2SO4.

Which of these best describes an ionic bond? a force that keeps two large molecules together an attraction that occurs between two nonmetals a force that holds two oppositely charged ions together an electromagnetic attraction that occurs between two metals

a force that holds two oppositely charged ions together

Which property is best to use when determining the strength of an ionic bond in a solid? lattice energy conductivity hardness solubility

lattice energy

What leads to the formation of an ionic bond with Hg22+? the attraction of a noble gas the attraction of an NH4+ ion the attraction of a group 1 element the attraction of an SO42- ion

the attraction of an SO42- ion