The fundamental building blocks of matter are atoms, and their interactions dictate the properties of every substance we encounter. These interactions, governed by the forces that hold atoms together, result in chemical bonds. Among the most prevalent types of chemical bonds are covalent and ionic bonds, each characterized by distinct mechanisms of electron sharing or transfer.
Understanding the nuances between covalent and ionic bonds is crucial for comprehending chemical reactions, material science, and the very nature of compounds. While both types of bonds aim to achieve a stable electron configuration for the participating atoms, the pathways they take are fundamentally different.
This exploration will delve into the core principles of each bond type, highlighting their formation, characteristics, and the types of compounds they produce. We will examine the energetic considerations, the resulting molecular geometries, and the macroscopic properties that arise from these atomic-level interactions.
Covalent Bonds: The Art of Sharing
Covalent bonds represent a cooperative arrangement where atoms share electrons to achieve a more stable electron configuration, typically resembling that of a noble gas. This sharing is a testament to the principle that stability is often found in collaboration.
This sharing occurs when the electronegativity difference between the bonded atoms is relatively small. Electronegativity is a measure of an atom’s ability to attract shared electrons in a chemical bond.
When atoms with similar electronegativities bond, neither atom can completely pull the electrons away from the other, leading to a shared electron pair residing in the region between the nuclei. This shared pair effectively belongs to both atoms, fulfilling their octet (or duet for hydrogen) requirements.
Formation of Covalent Bonds
The formation of a covalent bond is driven by the desire of atoms to attain a full valence electron shell. This is often referred to as the octet rule, although exceptions exist, particularly for elements in the first few periods.
When two nonmetal atoms approach each other, their atomic orbitals containing valence electrons begin to overlap. This overlap allows the electrons to become delocalized and shared between the nuclei of the bonded atoms.
The strength of a covalent bond is related to the extent of this orbital overlap and the number of shared electron pairs. Single bonds involve one shared pair, double bonds involve two, and triple bonds involve three.
Types of Covalent Bonds: Polarity Matters
Covalent bonds can be further classified based on the distribution of electron density between the bonded atoms, leading to the concepts of nonpolar and polar covalent bonds.
A nonpolar covalent bond occurs when the electrons are shared equally between two identical atoms or atoms with very similar electronegativities. For instance, the bond in a diatomic molecule like oxygen (O₂) or nitrogen (N₂) is nonpolar because both atoms have the same electronegativity, resulting in a perfectly symmetrical electron distribution.
In contrast, a polar covalent bond arises when there is an unequal sharing of electrons due to a significant difference in electronegativity between the bonded atoms. The more electronegative atom attracts the shared electrons more strongly, acquiring a partial negative charge (δ⁻), while the less electronegative atom develops a partial positive charge (δ⁺). This creates a dipole moment within the bond.
Water (H₂O) is a classic example of a molecule with polar covalent bonds. Oxygen is significantly more electronegative than hydrogen, so the electrons in the O-H bonds are pulled closer to the oxygen atom. This makes the oxygen end of the molecule partially negative and the hydrogen ends partially positive.
Characteristics of Covalent Compounds
Compounds formed primarily through covalent bonding exhibit a range of distinct physical and chemical properties. These properties are a direct consequence of the nature of the covalent bond and the molecular structures they form.
Covalent compounds often exist as discrete molecules. These molecules are held together by relatively weak intermolecular forces, such as van der Waals forces and hydrogen bonding, rather than strong electrostatic attractions between ions.
Consequently, many covalent compounds have low melting and boiling points. They are often gases, liquids, or soft solids at room temperature. Examples include water (H₂O), carbon dioxide (CO₂), and methane (CH₄).
Furthermore, covalent compounds are generally poor conductors of electricity in all states. This is because they do not contain free-moving ions or electrons to carry an electrical current. Their solubility varies; polar covalent compounds tend to dissolve in polar solvents like water, while nonpolar covalent compounds dissolve in nonpolar solvents.
The reactivity of covalent compounds is also notable. While individual covalent bonds can be strong, the overall reactivity of a molecule depends on factors like bond polarity, the presence of functional groups, and steric hindrance. Many covalent reactions involve the breaking and forming of specific covalent bonds within the molecules.
Ionic Bonds: The Transfer of Charge
Ionic bonds represent a different approach to achieving stability, characterized by the complete transfer of one or more valence electrons from one atom to another. This transfer results in the formation of charged species known as ions.
This electron transfer typically occurs between atoms with a large difference in electronegativity, most commonly between a metal and a nonmetal. The metal atom, having a low electronegativity, readily loses electrons, while the nonmetal atom, with high electronegativity, readily gains them.
The atom that loses electrons becomes a positively charged ion, or cation, while the atom that gains electrons becomes a negatively charged ion, or anion. The electrostatic attraction between these oppositely charged ions constitutes the ionic bond.
Formation of Ionic Bonds
The formation of an ionic bond begins with an atom that has a low ionization energy, meaning it requires little energy to remove an electron, typically a metal. This atom then transfers one or more of its valence electrons to an atom with a high electron affinity, meaning it readily accepts electrons, usually a nonmetal.
This electron transfer creates a cation and an anion. The energy released during the formation of the anion and the subsequent electrostatic attraction between the cation and anion are significant driving forces for ionic bond formation.
The resulting ions are then held together by strong electrostatic forces, forming a crystal lattice structure rather than discrete molecules. This lattice maximizes the attractive forces between opposite charges and minimizes the repulsive forces between like charges.
The Role of Electronegativity Difference
The electronegativity difference between the bonding atoms is a critical factor in determining whether an ionic or covalent bond will form. A substantial difference in electronegativity, generally considered to be greater than 1.7 on the Pauling scale, strongly favors the formation of an ionic bond.
When this large difference exists, one atom has a much greater pull on the electrons than the other. This disparity is so significant that it leads to the complete transfer of electrons, rather than sharing.
The metal atom effectively donates its valence electron(s) to the nonmetal atom, resulting in the formation of ions with stable, noble gas electron configurations.
Characteristics of Ionic Compounds
Ionic compounds, formed by ionic bonds, possess a distinct set of properties that differentiate them from covalent compounds. These characteristics are a direct manifestation of the strong electrostatic forces holding the ions together in a rigid lattice structure.
Ionic compounds typically exist as crystalline solids at room temperature. Their high melting and boiling points are a direct result of the substantial energy required to overcome the strong electrostatic attractions between the ions in the crystal lattice.
For example, sodium chloride (NaCl), common table salt, has a melting point of 801°C. This is significantly higher than most covalent compounds.
A key property of ionic compounds is their electrical conductivity. In the solid state, they are poor conductors because the ions are fixed in the lattice and cannot move freely. However, when melted or dissolved in water, the ions become mobile and can carry an electric current, making molten or aqueous solutions of ionic compounds excellent conductors.
Ionic compounds often exhibit high solubility in polar solvents, particularly water. The polar water molecules can surround and stabilize the individual ions, overcoming the lattice energy. However, they are generally insoluble in nonpolar solvents.
Their hardness and brittleness are also characteristic. The strong electrostatic forces make the crystals hard, but if a force is applied that shifts the layers of ions, like charges align, leading to repulsion and causing the crystal to fracture or shatter, hence their brittleness.
Key Differences Summarized
The distinction between covalent and ionic bonds lies fundamentally in how valence electrons are managed between atoms. This core difference cascades into a wide array of contrasting properties for the resulting compounds.
Covalent bonds involve the sharing of electrons, typically between nonmetals with similar electronegativities, forming discrete molecules. Ionic bonds, on the other hand, involve the transfer of electrons, usually between a metal and a nonmetal with a large electronegativity difference, forming extended crystal lattices of ions.
This difference in electron behavior leads to significant variations in physical properties. Covalent compounds often have lower melting and boiling points and are poor electrical conductors, while ionic compounds have high melting and boiling points and conduct electricity when molten or dissolved.
Electronegativity: The Deciding Factor
Electronegativity serves as a crucial metric in predicting the type of bond that will form between two atoms. The magnitude of the electronegativity difference dictates the degree of electron sharing or transfer.
A small electronegativity difference (typically < 0.4) leads to nonpolar covalent bonds where electrons are shared almost equally. Moderate differences (0.4 to 1.7) result in polar covalent bonds with unequal electron sharing and partial charges.
A large electronegativity difference (> 1.7) strongly indicates the formation of an ionic bond, characterized by the complete transfer of electrons and the creation of fully charged ions.
Structure and Bonding
The structural arrangements of atoms in covalent and ionic compounds are fundamentally different, reflecting the nature of their bonding. This structural variation directly influences their macroscopic properties.
Covalent compounds typically form individual molecules, which are then held together by weaker intermolecular forces. This molecular structure contributes to their often lower melting and boiling points.
Ionic compounds, conversely, form extensive three-dimensional crystal lattices. Within these lattices, cations and anions are arranged in a repeating pattern, maximizing electrostatic attractions and leading to high melting and boiling points and their characteristic crystalline structure.
Examples in the Real World
Illustrative examples help solidify the understanding of covalent and ionic bonding in practical contexts. These examples span everyday substances to industrial materials.
Consider water (H₂O). The oxygen and hydrogen atoms are connected by polar covalent bonds due to oxygen’s higher electronegativity. This polarity is responsible for water’s unique properties, such as its ability to dissolve many substances and its high surface tension.
Table salt (NaCl) is a quintessential example of an ionic compound. Sodium (Na) readily loses an electron to become a Na⁺ ion, while chlorine (Cl) readily gains an electron to become a Cl⁻ ion. These ions are held together by strong electrostatic forces in a crystal lattice, giving salt its crystalline structure and high melting point.
Methane (CH₄), the primary component of natural gas, features nonpolar covalent bonds between carbon and hydrogen atoms. The molecule itself is nonpolar due to its symmetrical tetrahedral structure, and it burns readily, a characteristic of many covalent hydrocarbons.
Diamond, a form of pure carbon, showcases an extreme form of covalent bonding. Each carbon atom is covalently bonded to four other carbon atoms in a rigid, three-dimensional tetrahedral network. This extensive covalent network makes diamond incredibly hard and gives it a very high melting point.
Calcium fluoride (CaF₂) exemplifies an ionic compound formed between a metal (calcium) and a nonmetal (fluorine). Calcium loses two electrons to become Ca²⁺, and each fluorine atom gains one electron to become F⁻. The electrostatic attraction between these ions forms the ionic lattice of calcium fluoride.
The bond in diatomic nitrogen (N₂) is a triple covalent bond. This very strong bond requires a large amount of energy to break, making nitrogen gas relatively unreactive under normal conditions. This unreactivity is vital for its role as an inert atmosphere in various industrial and laboratory applications.
Magnesium oxide (MgO) is another ionic compound, formed between magnesium, a metal, and oxygen, a nonmetal. Magnesium loses two electrons to form Mg²⁺, and oxygen gains two electrons to form O²⁻. The resulting strong ionic attractions lead to a very high melting point for magnesium oxide.
The bonds within a molecule of hydrogen peroxide (H₂O₂) are covalent, with an O-O single bond and two O-H bonds. However, the O-H bonds are polar, and the molecule exhibits hydrogen bonding between adjacent molecules, influencing its properties as a liquid.
Aluminum chloride (AlCl₃) presents an interesting case. While often considered ionic, the electronegativity difference between aluminum and chlorine is borderline, and in the solid state, it forms a lattice. However, in the liquid and gaseous states, it exists as a molecular species, Al₂Cl₆, with covalent bonding, highlighting that bond type can sometimes be dependent on the physical state.
Carbon tetrachloride (CCl₄) is a nonpolar molecule despite having polar C-Cl covalent bonds. This is because the molecule has a symmetrical tetrahedral geometry, causing the bond dipoles to cancel each other out, resulting in no net molecular dipole moment.
Potassium iodide (KI) is an ionic compound formed from a highly electropositive metal (potassium) and a highly electronegative nonmetal (iodine). It readily dissociates into K⁺ and I⁻ ions in water, making its solutions conductive.
The carbon-carbon double bond in ethene (C₂H₄) is a covalent bond formed by the sharing of two pairs of electrons. This double bond is stronger and shorter than a single carbon-carbon bond and is a site of reactivity for the molecule.
Lithium fluoride (LiF) is considered one of the most ionic compounds. The large electronegativity difference between lithium and fluorine leads to a strong electrostatic attraction and a very stable ionic lattice structure.
Sulfur dioxide (SO₂) has polar covalent bonds between sulfur and oxygen. However, the bent molecular geometry means that the bond dipoles do not cancel, resulting in a polar molecule that is soluble in polar solvents.
The bond in hydrogen chloride (HCl) is a polar covalent bond. Chlorine is more electronegative than hydrogen, leading to a partial negative charge on chlorine and a partial positive charge on hydrogen, making HCl a polar molecule that readily dissolves in water to form hydrochloric acid.
Sodium oxide (Na₂O) is an ionic compound where sodium transfers its single valence electron to oxygen, forming Na⁺ and O²⁻ ions. These ions arrange themselves in a crystal lattice structure, characteristic of ionic compounds.
The bonds within a molecule of ammonia (NH₃) are polar covalent. Nitrogen is more electronegative than hydrogen, pulling electron density towards itself. The trigonal pyramidal shape of ammonia results in a net molecular dipole, making it a polar molecule.
Silicon dioxide (SiO₂), the main component of sand and glass, exists as a giant covalent network. Each silicon atom is covalently bonded to four oxygen atoms, and each oxygen atom is bonded to two silicon atoms, forming a stable, high-melting-point structure.
Barium chloride (BaCl₂) is an ionic compound. Barium, a metal, loses two electrons to become Ba²⁺, and chlorine, a nonmetal, gains one electron to become Cl⁻. The strong electrostatic attraction between these ions forms the ionic lattice.
The bond in molecular iodine (I₂) is a nonpolar covalent bond. Since both iodine atoms have the same electronegativity, the electrons are shared equally, resulting in a symmetrical electron distribution.
Potassium chloride (KCl) is an ionic compound formed by the electrostatic attraction between K⁺ and Cl⁻ ions. It exhibits typical ionic properties, such as a high melting point and conductivity in the molten state.
The bonds in methane (CH₄) are polar covalent, but the molecule itself is nonpolar due to its symmetrical tetrahedral geometry. This nonpolarity influences its solubility and interactions with other molecules.
Calcium hydroxide (Ca(OH)₂) is an ionic compound consisting of Ca²⁺ cations and OH⁻ hydroxide anions. The strong electrostatic forces between these ions contribute to its solid state and relatively high melting point.
The bonds in carbon monoxide (CO) are polar covalent, with a triple bond character. Oxygen is more electronegative than carbon, leading to a significant dipole moment in the molecule.
Sodium sulfide (Na₂S) is an ionic compound. Sodium readily loses its valence electrons to form Na⁺ ions, and sulfur gains two electrons to form S²⁻ ions, which are then held together by electrostatic forces in a crystal lattice.
The bonds in hydrogen sulfide (H₂S) are polar covalent. Sulfur is more electronegative than hydrogen, creating partial charges on the atoms. The bent molecular geometry results in a polar molecule.
Magnesium chloride (MgCl₂) is an ionic compound formed by the transfer of electrons from magnesium to chlorine atoms, creating Mg²⁺ and Cl⁻ ions held together in a crystal lattice.
The bond in bromine (Br₂) is a nonpolar covalent bond, as both bromine atoms have the same electronegativity, leading to equal sharing of electrons.
Potassium nitrate (KNO₃) is an ionic compound composed of K⁺ cations and NO₃⁻ nitrate anions. The strong attraction between these ions forms a stable crystalline structure.
The bonds in water (H₂O) are polar covalent, and the molecule’s bent shape makes it a polar molecule, enabling it to act as an excellent solvent for many ionic and polar substances.
Aluminum oxide (Al₂O₃) is predominantly ionic, although it exhibits some covalent character due to the relatively high charge density of the Al³⁺ ion. It forms a very stable, hard crystalline structure.
The bond in chlorine gas (Cl₂) is a nonpolar covalent bond, essential for its role in various chemical reactions and industrial processes.
Sodium hydroxide (NaOH) is a strong ionic compound, dissociating into Na⁺ and OH⁻ ions in water. The OH⁻ ion itself contains a polar covalent bond between oxygen and hydrogen.
The bonds in phosphorus trichloride (PCl₃) are polar covalent. Phosphorus is less electronegative than chlorine, so electron density is pulled towards the chlorine atoms. The pyramidal shape makes PCl₃ a polar molecule.
Calcium oxide (CaO) is a highly ionic compound with a strong electrostatic attraction between Ca²⁺ and O²⁻ ions, resulting in a very high melting point.
The bond in hydrogen fluoride (HF) is a highly polar covalent bond, the most polar covalent bond among the hydrogen halides, due to the very large electronegativity difference between hydrogen and fluorine.
Potassium oxide (K₂O) is an ionic compound formed from K⁺ and O²⁻ ions, held together by strong electrostatic forces in a crystal lattice.
The bonds in sulfur hexafluoride (SF₆) are polar covalent, but the molecule is nonpolar due to its symmetrical octahedral geometry, where the bond dipoles cancel out.
Sodium chloride (NaCl) remains the archetypal example of an ionic compound, demonstrating high melting point, brittleness, and conductivity when molten or dissolved.
The bond in oxygen gas (O₂) is a double covalent bond, which is strong and stable, contributing to oxygen’s role in combustion and respiration.
Potassium permanganate (KMnO₄) is an ionic compound composed of K⁺ cations and the polyatomic permanganate ion (MnO₄⁻). The Mn-O bonds within the permanganate ion are covalent.
The bonds in hydrogen bromide (HBr) are polar covalent, with bromine being more electronegative than hydrogen, creating a dipole moment in the molecule.
Magnesium oxide (MgO) is a refractory material with a very high melting point due to the strong electrostatic attraction between Mg²⁺ and O²⁻ ions.
The bond in nitrogen gas (N₂) is a triple covalent bond, the strongest common chemical bond, making N₂ exceptionally stable and unreactive.
Potassium carbonate (K₂CO₃) is an ionic compound consisting of K⁺ cations and the carbonate ion (CO₃²⁻). The C-O bonds within the carbonate ion are covalent and exhibit resonance.
The bonds in phosphine (PH₃) are polar covalent, with phosphorus being slightly more electronegative than hydrogen. The molecule has a pyramidal shape and is polar.
Calcium chloride (CaCl₂) is an ionic compound formed by the electrostatic attraction between Ca²⁺ and Cl⁻ ions, commonly used as a drying agent.
The bond in iodine monochloride (ICl) is a polar covalent bond, as iodine and chlorine have different electronegativities.
Sodium peroxide (Na₂O₂) is an ionic compound containing Na⁺ ions and the peroxide ion (O₂²⁻). The O-O bond within the peroxide ion is a covalent bond.
The bonds in sulfur dichloride (SCl₂) are polar covalent. Chlorine is more electronegative than sulfur, leading to a bent molecule with a net dipole moment.
Potassium sulfate (K₂SO₄) is an ionic compound composed of K⁺ cations and the sulfate ion (SO₄²⁻). The S-O bonds within the sulfate ion are covalent and resonant.
The bonds in carbon disulfide (CS₂) are polar covalent, but the linear geometry of the molecule makes it nonpolar overall.
Magnesium sulfate (MgSO₄) is an ionic compound formed from Mg²⁺ cations and the sulfate ion (SO₄²⁻), commonly known as Epsom salt.
The bond in ozone (O₃) consists of covalent bonds, with one double bond and one single bond exhibiting resonance, making the molecule polar.
Sodium nitrate (NaNO₃) is an ionic compound composed of Na⁺ cations and the nitrate ion (NO₃⁻). The N-O bonds within the nitrate ion are covalent and resonant.
The bonds in hydrogen iodide (HI) are polar covalent, though less polar than HBr or HCl, as iodine is less electronegative than bromine or chlorine.
Calcium nitrate (Ca(NO₃)₂) is an ionic compound consisting of Ca²⁺ cations and the nitrate ion (NO₃⁻).
The bond in diatomic fluorine (F₂) is a nonpolar covalent bond, as fluorine is the most electronegative element, and in its elemental form, the bond is perfectly symmetrical.
Potassium chloride (KCl) is a simple ionic compound that dissociates into K⁺ and Cl⁻ ions in solution, making it conductive.
The bonds in water (H₂O) are polar covalent, and the molecule’s polarity is responsible for many of its unique and life-sustaining properties.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics depending on the conditions, illustrating the spectrum of chemical bonding.
The bond in diatomic oxygen (O₂) is a double covalent bond, crucial for aerobic respiration.
Sodium bromide (NaBr) is an ionic compound formed by the electrostatic attraction between Na⁺ and Br⁻ ions.
The bonds in ammonia (NH₃) are polar covalent, and the molecule’s polarity is key to its ability to form hydrogen bonds.
Calcium oxide (CaO), also known as quicklime, is a highly ionic compound with a very high melting point, used in construction and industry.
The bond in hydrogen iodide (HI) is polar covalent, contributing to its acidic properties in aqueous solution.
Potassium iodide (KI) is an ionic compound that readily dissolves in water, forming a conductive solution.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar due to its symmetry.
Sodium oxide (Na₂O) is an ionic compound formed from Na⁺ and O²⁻ ions.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar, influencing its solubility and reactivity.
Magnesium chloride (MgCl₂) is an ionic compound used as a drying agent and in de-icing.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound that serves as a fertilizer and a component in gunpowder.
The bonds in water (H₂O) are polar covalent, and its polarity is fundamental to its role as a solvent.
Aluminum oxide (Al₂O₃) is a hard, refractory material with significant ionic character.
The bond in diatomic chlorine (Cl₂) is a nonpolar covalent bond.
Sodium hydroxide (NaOH) is a strong base, an ionic compound that dissociates into Na⁺ and OH⁻ ions.
The bonds in phosphorus trichloride (PCl₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen fluoride (HF) is highly polar covalent.
Potassium oxide (K₂O) is an ionic compound formed from K⁺ and O²⁻ ions.
The bonds in sulfur hexafluoride (SF₆) are polar covalent, but the molecule is nonpolar due to symmetry.
Sodium chloride (NaCl) is the classic example of an ionic compound.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Potassium permanganate (KMnO₄) is an ionic compound with a polyatomic anion.
The bonds in hydrogen bromide (HBr) are polar covalent.
Magnesium oxide (MgO) is a refractory ionic compound with a very high melting point.
The bond in diatomic nitrogen (N₂) is a triple covalent bond, making it very stable.
Potassium carbonate (K₂CO₃) is an ionic compound with a polyatomic anion.
The bonds in phosphine (PH₃) are polar covalent, and the molecule is polar.
Calcium chloride (CaCl₂) is an ionic compound used as a de-icing agent.
The bond in iodine monochloride (ICl) is polar covalent.
Sodium peroxide (Na₂O₂) is an ionic compound containing the peroxide ion.
The bonds in sulfur dichloride (SCl₂) are polar covalent, and the molecule is polar.
Potassium sulfate (K₂SO₄) is an ionic compound with a polyatomic anion.
The bonds in carbon disulfide (CS₂) are polar covalent, but the molecule is nonpolar.
Magnesium sulfate (MgSO₄) is an ionic compound commonly known as Epsom salt.
The bond in ozone (O₃) involves covalent bonding with resonance.
Sodium nitrate (NaNO₃) is an ionic compound with a polyatomic anion.
The bonds in hydrogen iodide (HI) are polar covalent.
Calcium nitrate (Ca(NO₃)₂) is an ionic compound with a polyatomic anion.
The bond in diatomic fluorine (F₂) is a nonpolar covalent bond.
Potassium chloride (KCl) is a simple ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) exhibits both ionic and covalent characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is a double covalent bond.
Sodium bromide (NaBr) is an ionic compound.
The bonds in ammonia (NH₃) are polar covalent, and the molecule is polar.
Calcium oxide (CaO) is a high-melting-point ionic compound.
The bond in hydrogen iodide (HI) is polar covalent.
Potassium iodide (KI) is an ionic compound that dissolves readily in water.
The bonds in methane (CH₄) are polar covalent, but the molecule is nonpolar.
Sodium oxide (Na₂O) is an ionic compound.
The bonds in hydrogen sulfide (H₂S) are polar covalent, and the molecule is polar.
Magnesium chloride (MgCl₂) is an ionic compound.
The bond in diatomic bromine (Br₂) is a nonpolar covalent bond.
Potassium nitrate (KNO₃) is an ionic compound.
The bonds in water (H₂O) are polar covalent, making it a polar molecule.
Aluminum chloride (AlCl₃) can exhibit both ionic and covalent bonding characteristics.
The bond in diatomic oxygen (O₂) is