Ionic Bonding: Formation, Properties, and Lattice Energy

Question 1

Describe the formation of an ionic bond between sodium (Na) and chlorine (Cl). Explain the electron transfer that occurs and illustrate the resulting ions formed using a labeled diagram.

Accepted Answer

Sodium transfers one electron to chlorine, forming Na+ and Cl- ions. These oppositely charged ions are attracted to each other by electrostatic forces, creating an ionic bond.

Answer

Sodium and chlorine share electrons to form a covalent bond.

Answer

Sodium gains one electron from chlorine, forming Na- and Cl+ ions.

Question 2

Which of the following elements has the lowest ionization energy and is most likely to form an ionic bond with chlorine?

Accepted Answer

Sodium

Answer

Magnesium

Answer

Phosphorus

Answer

Sulfur

Question 3

Which of the following factors does NOT affect the lattice energy of an ionic compound?

Accepted Answer

Polarity of the solvent

Answer

Charge of the ions

Answer

Size of the ions

Answer

Number of ions in the unit cell

Question 4

Which of the following ionic compounds is the most soluble in water?

Accepted Answer

NaCl

Answer

CaCO3

Answer

PbSO4

Answer

AgCl

Question 5

What is the conjugate acid of NH3?

Accepted Answer

NH4+

Answer

NH2-

Answer

H3N

Answer

N3-

Question 6

What is the pH of a 0.01 M solution of NaOH?

Accepted Answer

13

Answer

1

Answer

7

Answer

14

Question 7

What is the hybridization of the nitrogen atom in NH4+?

Accepted Answer

sp3

Answer

sp

Answer

sp2

Answer

sp3d

Question 8

Describe the correlation between the electronegativity difference between elements and the nature of the resulting ionic bond. Provide specific examples to support your explanation.

Accepted Answer

A larger electronegativity difference leads to a stronger and more polar ionic bond. For instance, the ionic bond in NaCl, where chlorine is more electronegative than sodium, is stronger and more polar than the bond in MgO.

Answer

Electronegativity difference has no influence on the strength or polarity of ionic bonds.

Answer

Ionic bonds are inherently nonpolar, irrespective of the electronegativity difference.

Question 9

Lattice energy is defined as the:

Accepted Answer

Energy required to separate all the ions in one mole of an ionic compound

Answer

Energy released when all the ions in one mole of an ionic compound come together to form the crystal lattice

Answer

Energy required to remove an electron from a neutral atom

Answer

Energy released when an electron is added to a neutral atom

Question 10

Identify the ionic compound in this list:

Accepted Answer

Sodium chloride

Answer

Methane

Answer

Water

Answer

Carbon dioxide

Question 11

The electron configuration of the sodium ion (Na+) is:

Accepted Answer

1s2 2s2 2p6

Answer

1s2 2s2 2p6 3s1

Answer

1s2 2s2 2p4

Answer

1s2 2s1

Question 12

Which of the following ions has the largest radius?

Accepted Answer

O2-

Answer

Na+

Answer

Mg2+

Answer

F-

Question 13

Which of the following is NOT a characteristic of ionic compounds?

Accepted Answer

Form molecular crystals

Answer

High melting and boiling points

Answer

Good electrical conductors in the molten state

Answer

Solubility in polar solvents

Question 14

The formation of an ionic bond involves the:

Accepted Answer

Transfer of electrons from one atom to another

Answer

Sharing of electrons between atoms

Answer

Loss of protons from one atom to another

Answer

Gain of neutrons by one atom from another

Question 15

Which of the following elements is most likely to form a cation with a +2 charge?

Accepted Answer

Calcium

Answer

Sodium

Answer

Chlorine

Answer

Argon

Question 16

Lattice energy refers to the:

Accepted Answer

Energy required to separate the ions in a mole of the compound

Answer

Energy released when the ions form a mole of the compound

Answer

Energy needed to melt a mole of the compound

Answer

Energy released when a mole of the compound dissolves in water

Question 17

The reaction between sodium and chlorine to form sodium chloride is:

Accepted Answer

Exothermic and forms an ionic compound

Answer

Exothermic and forms a covalent compound

Answer

Endothermic and forms an ionic compound

Answer

Endothermic and forms a covalent compound

Question 18

Which of the following applications relies on the ionic properties of compounds?

Accepted Answer

Batteries

Answer

Paints

Answer

Plastics

Answer

Lubricants

Question 19

The correct chemical formula for the ionic compound formed between calcium and fluorine is:

Accepted Answer

CaF2

Answer

CaF

Answer

Ca2F

Answer

Ca2F2

Question 20

Ionic compounds have numerous practical applications. Which of the following is NOT a common use of ionic compounds?

Accepted Answer

Fuel in vehicles

Answer

Medicines (e.g., antacids)

Answer

Industrial processes (e.g., production of glass)

Answer

Consumer products (e.g., table salt)

Question 21

In the Born-Haber cycle, which step involves removing an electron from the metal atom?

Accepted Answer

Ionization energy of the metal

Answer

Electron affinity of the nonmetal

Answer

Lattice energy formation

Question 22

Which of the following is a defining characteristic of ionic bonding?

Accepted Answer

The attraction between positively and negatively charged ions

Answer

The formation of a covalent bond between two atoms

Answer

The sharing of electrons between two atoms

Answer

The transfer of electrons from one atom to another

Question 23

In the formation of NaCl, which of the following processes occurs?

Accepted Answer

Sodium loses an electron, while chlorine gains an electron.

Answer

Sodium gains an electron, while chlorine loses an electron.

Answer

Sodium and chlorine share electrons to form a covalent bond.

Answer

Sodium and chlorine form a metallic bond by sharing free electrons.

Question 24

Which of the following factors has the greatest influence on the lattice energy of an ionic compound?

Accepted Answer

The charge of the ions

Answer

The size of the ions

Answer

The distance between the ions

Answer

The electronegativity of the ions

Question 25

Which of the following statements about the solubility of ionic compounds in water is true?

Accepted Answer

Compounds with highly charged ions are more soluble.

Answer

Compounds with high lattice energies are more soluble.

Answer

Compounds with small ions are less soluble.

Answer

Solubility is independent of the ionic properties of the compound.

Question 26

Which of the following applications of ionic compounds is primarily due to their electrical conductivity?

Accepted Answer

Batteries

Answer

Paints

Answer

Fertilizers

Answer

Antacids

Question 27

The Lewis dot structure of an ionic compound typically shows:

Accepted Answer

The transfer of electrons between the atoms

Answer

The sharing of electrons between the atoms

Answer

The presence of lone pairs of electrons on the ions

Answer

The molecular orbitals of the compound

Question 28

Which of the following factors does NOT affect the strength of an ionic bond?

Accepted Answer

The temperature

Answer

The size of the ions

Answer

The charge of the ions

Answer

The distance between the ions

Question 29

Which of the following most accurately describes an ionic bond?

Accepted Answer

The electrostatic attraction between positively and negatively charged ions

Answer

The sharing of electrons between atoms

Answer

A covalent bond between two nonmetals

Answer

A hydrogen bond between two polar molecules

Question 30

Which factor(s) influence(s) the lattice energy of an ionic compound?

Accepted Answer

Both the charges and sizes of the ions

Answer

The charges of the ions

Answer

The sizes of the ions

Answer

The number of ions in the compound

Question 31

In the ionic compound NaCl, what is the oxidation state of sodium?

Accepted Answer

+1

Answer

-1

Answer

0

Answer

+2

Question 32

Which of the following is an ionic compound?

Accepted Answer

NaCl

Answer

CH4

Answer

H2O

Answer

CO2

Question 33

Which of the following elements is most likely to form an ionic bond with sodium due to a significant difference in electronegativity?

Accepted Answer

Chlorine

Answer

Nitrogen

Answer

Hydrogen

Answer

Carbon

Question 34

What is the net charge of the potassium ion (K⁺) in ionic potassium chloride (KCl)?

Accepted Answer

+1

Answer

-1

Answer

-2

Answer

+2

Question 35

Which of the following substances is classified as an ionic compound due to the presence of electrostatic attraction between oppositely charged ions?

Accepted Answer

Sodium chloride (NaCl)

Answer

Carbon dioxide (CO₂)

Answer

Methane (CH₄)

Answer

Water (H₂O)

Question 36

What is the definition of lattice energy in the context of ionic compounds?

Accepted Answer

The energy required to separate all the ions in an ionic crystal into gaseous ions.

Answer

The energy released when ions come together to form a crystal lattice.

Question 37

Which of the following factors has the most significant influence on the lattice energy of an ionic compound?

Accepted Answer

The charges of the ions involved

Answer

Temperature

Answer

Size of the ions

Answer

Mass of the ions

Question 38

What is the general relationship between lattice energy and the solubility of an ionic compound in water?

Accepted Answer

Ionic compounds with higher lattice energies tend to be less soluble in water.

Answer

Lattice energy has no effect on solubility.

Answer

Ionic compounds with higher lattice energies tend to be more soluble in water.

Question 39

What is the term for the regular arrangement of ions in an ionic crystal lattice?

Accepted Answer

Crystallization

Answer

Condensation

Answer

Deposition

Answer

Vaporization

Question 40

Which of the following applications makes use of the unique properties of ionic compounds, such as their high conductivity?

Accepted Answer

Batteries

Answer

Plastics

Answer

Lubricants

Answer

Paints

Question 41

Identify the pair of elements most likely to form an ionic bond.

Accepted Answer

Sodium and chlorine

Answer

Oxygen and oxygen

Answer

Nitrogen and nitrogen

Answer

Carbon and hydrogen

Question 42

In the ionic compound MgO, what is the charge of the magnesium ion?

Accepted Answer

2+

Answer

3+

Answer

4+

Answer

1+

Question 43

What is the term used to describe the energy required to separate all ions in one mole of an ionic compound?

Accepted Answer

Lattice energy

Answer

Ionization energy

Answer

Hydration energy

Answer

Bond energy

Question 44

Determine the formula of the ionic compound formed between calcium and sulfur.

Accepted Answer

CaS

Answer

CaS2

Answer

Ca3S

Answer

Ca2S

Question 45

Identify the compound among the following that does NOT contain an ionic bond.

Accepted Answer

CO2

Answer

NH4Cl

Answer

NaCl

Answer

MgO

Question 46

Which of the following pairs of elements is most likely to form an ionic bond due to a significant difference in their electronegativities?

Accepted Answer

Potassium (K) and Fluorine (F)

Answer

Nitrogen (N) and Hydrogen (H)

Answer

Carbon (C) and Oxygen (O)

Answer

Chlorine (Cl) and Bromine (Br)

Question 47

Determine the correct formula for the ionic compound formed between magnesium (Mg) and chlorine (Cl), ensuring compliance with the octet rule.

Accepted Answer

MgCl₂

Answer

MgCl

Answer

Mg₂Cl₂

Answer

Mg₂Cl

Question 48

Identify the property that is NOT characteristic of ionic compounds:

Accepted Answer

Low melting point

Answer

Conductivity in solution

Answer

High melting point

Answer

Brittle crystalline structure

Question 49

Which factor contributes to the high melting points observed in ionic compounds?

Accepted Answer

Strong electrostatic forces between ions

Answer

Weak van der Waals forces

Answer

Covalent bonds between atoms

Answer

Low ionization energies of metals

Question 50

The lattice energy of an ionic compound is a measure of the:

Accepted Answer

Energy released when one mole of the compound forms from its gaseous ions.

Answer

Energy released when one mole of the compound dissolves in water.

Answer

Energy required to break one mole of the compound into its constituent atoms.

Question 51

Which type of ions would generally have the highest lattice energy?

Accepted Answer

Small, highly charged ions

Answer

Large, weakly charged ions

Answer

Small, weakly charged ions

Answer

Large, highly charged ions

Question 52

Explain why ionic compounds tend to be brittle:

Accepted Answer

Repulsion between like charges occurs when layers of ions are displaced.

Answer

The metallic bonds are weak.

Answer

Covalent bonds are easily broken.

Question 53

When an ionic compound dissolves in water, what happens to the ions?

Accepted Answer

Become surrounded by water molecules (solvation)

Answer

Remain bonded together in a crystal lattice.

Answer

Form covalent bonds with water molecules.

Answer

Precipitate out of solution.

Question 54

Determine the charge on the cation in the ionic compound aluminum oxide (Al₂O₃) based on the periodic table and the formula.

Accepted Answer

+3

Answer

-3

Answer

+2

Answer

-2