Name: ionic compounds and electrolytes
Uploaded: 2026-06-01T06:28:24.408Z
Duration: 42 s
Channel: JoVE

K12 Standards

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

9-12

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Ionic Bonds

An ionic bond is a non-covalent attraction that holds two oppositely charged ions together, such as the sodium cation and chloride anion in sodium chloride.In this case, sodium transfers its single valence electron to chlorine. This electron transfer completes the octet of electrons in each combining atom, making them more stable.The strength of an ionic bond depends on the environment of the ionic compound.In the air, the ions remain closely packed in a solid crystal. Because there are no polar molecules to pull the ions apart, the strong attraction between opposite charges keeps the compound stable.But in water, polar water molecules surround the ions and weaken their attraction. The partial negative charge on oxygen is attracted to sodium ions, while the partial positive charges on hydrogen are attracted to chloride ions. This pulls ions away from the crystal, causing the compound to break apart into its ions.

ionic bonds

When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions with opposite charges. Ionic compounds are rigid and brittle when solid and may dissociate into their constituent ions in water. Covalent compounds, by contrast, remain intact unless a chemical reaction breaks them.<h4>Opposing Charges Hold Ions Together in Ionic Compounds</h4>Ionic bonds are reversible electrostatic interactions between ions with opposing charges. Elements that are the most reactive (i.e., have a higher tendency to undergo chemical reactions) include those that only have one valence electron, (e.g., potassium) and those that need one more valence electron (e.g., chlorine).Ions that lose electrons have a positive charge and are referred to as cations. Ions that gain electrons have a negative charge and are called anions. Cations and anions combine in ratios that result in a net charge of 0 for the compound they form. For example, the compound potassium chloride (KCl) contains one chloride ion for each potassium ion, because the charge of potassium is +1 and the charge of chloride is -1. The compound magnesium chloride (MgCl2) contains two chloride ions for each magnesium ion because magnesium&#x2019;s charge is +2.<h4>Ions Can Dissociate from One Another in Water</h4>The electrostatic forces holding ionic compounds together are strong when the compounds are in solid form. Since the melting points of ionic compounds tend to be very high, they are generally found as solids on the Earth&#x2019;s surface. Howeverionic bonds are not as strong as covalent bondsbecause the ions can be pulled apartor dissolvedin a chemical reaction liquids like water. Ions dissolved in water are said to be in a chemical reaction, and many ions are capable of conducting electric currents when in this form.<h4>Electrolytes Are Important for Biological Systems</h4>Electrolytes are ions that can conduct electricity when dissolved in water. In biological systems, electrolytes are essential for osmotic regulation&#x2014;the balance of water across cellular membranes. Electrolytes also contribute to critical biological processes that rely upon electrical charges across the cell membrane, such as muscle contractions and nerve impulses. Common biological electrolytes include the calcium ion (Ca2+), the sodium ion (Na+), the magnesium ion (Mg2+), the potassium ion (K+), the phosphate ion (PO43-) and the chloride ion (Cl-).Electrolyte imbalances can cause severe physical symptoms and even death. One of the most commonly-encountered electrolyte imbalances is hyponatremia, insufficient sodium levels in the blood. Hyponatremia can be a symptom of another medical condition or caused by ingesting too much water without adequately replacing sodium. Treatments for this serious condition aim to restore the balance of sodium in the body so that the brain, heart, and other organs can function properly.

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JoVE Core

Biology

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KEY TERMS AND CONCEPTS

ionic compounds and electrolytes

Ionic compounds form when atoms gain or lose electrons to reach a more stable electron configuration. The charged particles that result are called ions. Ionic bonds are electrostatic attractions between oppositely charged ions.

The most reactive elements include those with one valence electron, such as potassium, and those that need one more valence electron, such as chlorine. Ions that lose electrons become positive cations. Ions that gain electrons become negative anions. Cations and anions combine in ratios that give the compound a net charge of 0.

Potassium chloride, or KCl, is one example. It contains one chloride ion for each potassium ion because potassium has a charge of +1 and chloride has a charge of -1. Magnesium chloride, or MgCl2, is another example. It contains two chloride ions for each magnesium ion because magnesium has a charge of +2.

Ionic compounds are strong in solid form. They are usually rigid and brittle as solids. They also tend to have very high melting points, so they are commonly found as solids on Earth’s surface. In water, however, the ions can separate from one another and dissolve.

This behavior is different from covalent compounds, which stay intact unless a chemical reaction breaks them. Ions dissolved in water can conduct electric current. These ions are called electrolytes, and they are important in biological systems.

Electrolytes help control osmotic regulation, which is the balance of water across cell membranes. They also support electrical processes that power muscle contractions and nerve impulses. Common biological electrolytes include calcium ion (Ca2+), sodium ion (Na+), magnesium ion (Mg2+), potassium ion (K+), phosphate ion (PO43-), and chloride ion (Cl-).

Electrolyte imbalances can cause serious symptoms and may even be fatal. One common imbalance is hyponatremia, or low sodium in the blood. It can result from another medical condition or from drinking too much water without replacing sodium. Treatment aims to restore sodium balance so the brain, heart, and other organs can function properly.

Ionic Compounds and Electrolytes

the periodic table and organismal elements

the-periodic-table-and-organismal-elements

Periodic Table Basics for Living Things

The periodic table helps explain which elements living things need and how those elements are related. Elements are the smallest units of matter that cannot be broken down further by chemical processes. There are 118 known elements, but not all occur naturally, and even fewer are essential for life. Living matter is made mostly of carbon, nitrogen, hydrogen, and oxygen. Together, these elements make up most of the human body and are also found in all life on Earth. Smaller amounts of calcium,...

atomic structure

Atoms and Their Subatomic Particles

Atoms are the smallest units of elements, and they make up all matter. Each atom contains three subatomic particles: protons, neutrons, and electrons. These particles give an atom its mass and its charge. The idea that matter is made of tiny particles goes back to Democritus, a Greek philosopher around 450 B.C. He used the word atomos, which means “indivisible.” The idea was not accepted at the time, but it returned many centuries later. In the 19th century, John Dalton proposed an atomic...

isotopes

Atomic Mass and Isotope Basics

Atomic mass and isotopes are linked by the number of protons and neutrons in an atom. The number of protons sets an element’s atomic number, or Z. For example, every atom with eight protons is oxygen. Atoms of the same element can still differ because they can have different numbers of neutrons. The mass number, or A, is the total of protons and neutrons. Atoms with the same atomic number but different mass numbers are called isotopes. Elements can have several isotopes. Carbon-12, carbon-13,...

electron behavior

Electron Shells and Valence Electrons

Electrons are negatively charged subatomic particles that occupy regions around the positively charged nucleus of an atom. Their location is linked to energy levels called shells. They are also grouped into sub-shells and orbitals within each shell. An electron’s shell shows its general energy level. Electrons closer to the nucleus have less energy, while electrons farther away have more energy. The sub-shell gives a more exact location and energy level. An orbital is the shape of the region...

electron orbital model

Electron Orbitals and Energy Levels

Electron orbitals show where electrons are most likely to be found around the atomic nucleus. They also help explain energy levels, orbital shapes, and three-dimensional orientation. In an atom, electron location is described first by a shell, or principal energy level. It is then described by a subshell within that shell and by the individual orbitals inside each subshell. The first shell is closest to the nucleus. It has only one subshell and one spherical orbital, called the 1s orbital.

covalent bonds

Electronegativity and Covalent Bond Polarity

Covalent bonds form when two atoms share electrons to fill their valence shells. The way those shared electrons are pulled depends on electronegativity, which is an atom’s ability to attract electrons in a bond. When atoms have similar electronegativities, they form nonpolar covalent bonds. When their electronegativities differ, the bond is polar because the electrons are shared unevenly. The number of covalent bonds an atom can make depends on its valence electrons. Oxygen has six valence...

Ionic compounds form when atoms gain or lose electrons to reach a more stable electron configuration. The charged particles that result are called ions. Ionic bonds are electrostatic attractions between oppositely charged ions. The most reactive elements include those with one valence electron, such as potassium, and those that need one more valence electron, such as chlorine. Ions that lose electrons become positive cations. Ions that gain electrons become negative anions. Cations and anions...

hydrogen bonds

Hydrogen Bonds in Water

Hydrogen bonds in water are weak attractions between atoms that are already part of other chemical bonds. One atom is electronegative, such as oxygen, and carries a partial negative charge. The other is a hydrogen atom that is bonded to another electronegative atom and has a partial positive charge. These attractions form because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom like oxygen or nitrogen. The electrons in that bond are shared unequally.

van der waals interactions

Intermolecular Forces in Polar Solutions

Intermolecular forces are the attractions and repulsions that act between atoms and molecules. These electrostatic forces come from particles with permanent, partial, or temporary charges. For neutral atoms and molecules, the main types are ion-dipole, dipole-dipole, and dispersion forces, which are together called van der Waals forces. Polar molecules have a partial positive end and a partial negative end. That separation of charge creates a dipole. In water, oxygen is more electronegative...

elements and compounds

Elements, Compounds, and Bonding

Elements and compounds are the two main kinds of pure substances. A pure substance contains only one kind of matter. An element contains only one type of atom. A compound contains two or more types of atoms joined by a chemical bond. Elements can be atomic or molecular, depending on their basic units. They are unique forms of matter with specific chemical and physical properties. Ordinary chemical reactions cannot break an element into a smaller substance. There are 118 elements, but only 98...

molecular shapes

Electron Geometry and Lone Pairs

Electron geometry and lone pairs help explain why molecules take specific shapes. The arrangement of electron groups around a central atom controls the molecular geometry. Valence electrons form bonding pairs, which sit mainly between bonded atoms, or lone pairs, which belong to one atom only. Electron pairs in the valence shell spread out to reduce repulsion. They do this by maximizing the distance between one another. A diatomic molecule has two regions of electron density, and these are...

pH Scale in Everyday Solutions

pH measures how acidic or basic a water-based solution is. It depends on the concentration of hydronium ions, H3O+, in the solution. In one liter of pure water at neutral pH, there are 1×10−7 moles of hydronium ions. Because hydronium ion levels can vary over a very wide range, measuring pH directly in moles is not practical. The pH scale converts hydronium ion concentration into a negative logarithm. Pure water has a pH of 7 and is neutral. Most solutions fall between 0 and 14, but some, such...

chemical reactions

Atoms, Bonds, and Chemical Reactions

Chemical reactions rearrange atoms to form new substances. In a reaction, the starting materials are called reactants, and the new substances are called products. The atoms stay the same type and number, but their bonds change, so the substances become different compounds. During a chemical reaction, bonds between atoms break and form again. This means the shared electrons are rearranged. Some reactions happen on their own, while others need an energy source such as heat or light. In biology,...

redox reactions

Electron Transfer in Redox

Redox reactions are chemical reactions that involve electron transfer between atoms or molecules. When one particle gains electrons, another must lose them at the same time. That is why oxidation and reduction always happen together. The two roles in a redox reaction are linked. The atom that is oxidized acts as the reducing agent, or reductant. The atom that is reduced acts as the oxidizing agent, or oxidant. A simple way to remember the ideas is OIL-RIG, which means oxidation is losing...

cohesion

Water Molecules and Surface Tension

Water molecules stick to each other through cohesion. Water is neutral overall, but it is a polar molecule. The oxygen atom in one water molecule has a partial negative charge, and it can bind with a hydrogen atom that has a partial positive charge in another water molecule. This forms a hydrogen bond. Each water molecule can form up to four hydrogen bonds with other water molecules, and these bonds give water its cohesive nature. Cohesion helps water form droplets on a surface. Water does not...

adhesion

Water Climbing by Adhesion

Water can climb or stick to surfaces because of adhesion, which is the attraction between different kinds of molecules. In water, this is easy to see on polar surfaces such as glass or cellulose in plants. The positive hydrogen side of water is more attracted to the negative oxygen in silica than to nearby water molecules. This attraction helps explain capillary action. If a narrow glass tube is placed in a beaker of water, water molecules attach to the tube’s surface and the water level rises.

states of water

Water Phase Changes and Ice Density

Water changes between solid, liquid, and gas states as temperature and molecular motion change. In this lesson, the focus is on how water freezes, melts, vaporizes, and returns to liquid or solid form. The balance between intermolecular forces, which pull molecules together, and kinetic energy, which pushes them apart, controls each state. Water freezes when intermolecular forces become stronger than kinetic energy. Unlike most substances, ice is less dense than liquid water. This happens...

specific heat

How Specific Heat Affects Temperature

Specific heat capacity describes how much energy a substance needs to rise by 1 degree Celsius for each gram. It is often written with calories, grams, and degrees Celsius, but it can also be shown in joules, kilograms, and Kelvin. For water, 1 gram needs 1 calorie to increase by 1°C, which is also written as 1 cal/g-°C or 4186 J/kg/K. Water has a high specific heat capacity, so it takes in a large amount of heat before its temperature changes much. It also gives off a lot of heat when it...

vaporization

Vaporization, Boiling, and Evaporation

Vaporization changes a liquid into vapor when temperature adds enough kinetic energy to overcome intermolecular forces. It is a surface phenomenon, which means it starts at the liquid’s surface. The energy needed to vaporize a set amount of liquid at a given pressure and constant temperature is called the heat of vaporization. Water shows this process clearly. When liquid water is vaporized, it becomes steam. One way this happens is boiling, which occurs when vapor bubbles form beneath the...

solvents

Water as a Biological Solvent

Water acts as a biological solvent in many living systems. A solvent is a substance, usually a liquid, that dissolves another substance called a solute. When a solvent and a solute mix, they form a solution, which is a uniform mixture of both parts. Water is called a universal biological solvent because its polar structure helps it dissolve many other polar compounds. Polarity means that one side of the molecule has a slight positive charge and the other side has a slight negative charge.

carbon skeletons

Carbon Backbones in Biomolecules

Carbon backbones give biological molecules their structure and flexibility. Living things are built from macromolecules that contain carbon atoms, and organic compounds are defined by a carbon backbone. Carbon is tetravalent, so each carbon atom can bond with four other atoms. Its valence electrons are stable, so carbon rarely becomes an ion. As carbon chains get longer, they can form ring structures, double bonds, and branching side chains. Carbon-carbon bonds create the carbon skeleton.

key terms and concepts

Learn how ionic compounds form, why they dissolve in water, and how electrolytes support nerves, muscles, and fluid balance in the body.

Ionic Compounds and Electrolytes | JoVE K12

JoVE Core series brings biology to life through over 300 concise and easy-to-understand animated video lessons that explain key concepts in biology, plus more than 150 scientist-in-action videos that show actual research experiments conducted in today’s laboratories.

biology

Virginia  Standards of Learning

HIgh School

Physics

PH.9

PH.9.e

Texas Essential Knowledge and Skills

High School

Chemistry

CHEM.7

CHEM.7.D

Alabama Course of Study Science

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Motion and Stability: Forces and Interactions

9-12.C.2.2.g

Next Generation Science Standards

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Matter and Its Interactions

HS-PS1-17

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Subatomic Particles

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Physical Properties Of Minerals I: Crystals and Cleavage

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Atoms and elements

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

When atoms gain or lose electrons to achieve a more stable electron configuration they form ions. Ionic bonds are electrostatic attractions between ions ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Lewis Symbols and the Octet Rule

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Chemical Bonds


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Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

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Soil Nutrient Analysis: Nitrogen, Phosphorus, and Potassium

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Chemical bonding (ionic, covalent, metallic)

Content elaboration: This unit builds upon the Earth and Space Science strand in grade 6, where common minerals are defined, tested and classified. It also incorporates knowledge of mineral properties and crystalline structures (chemical compositions and bonding) included in the chemistry sections of other high school courses. The emphasis in this course is to relate the chemical and physical components of minerals to the properties of the minerals. This requires extensive mineral testing, investigations, experimentation, observation, use of technology and models/modeling. The focus is on learning the ways to research, test and evaluate minerals, not in memorization of mineral names or types. Properties such as cleavage and hardness are connected to the chemical structure and bonding of the mineral. In addition, the environment in which minerals form should be part of the classification of the mineral, using mineral data to help interpret the environmental conditions that existed during the formation of the mineral.

Structures of Solids

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Ionic Crystal Structures

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X-ray Crystallography

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Optical Materialography Part 2: Image Analysis

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X-ray Diffraction

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X-ray diffraction (XRD) is a technique ...

X-ray Photoelectron Spectroscopy

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X-ray photoelectron spectroscopy (XPS) ...

Crystallinity (crystal structure)

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Crystallinity (crystal structure)

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Single Crystal and Powder X-ray Diffraction

Source: Tamara M. Powers, Department of Chemistry, Texas A&#38;M University&#160;
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Determining the Solubility Rules of Ionic Compounds

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Criteria of a mineral (crystalline solid, occurs in nature, inorganic, defined chemical composition)

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criteria-mineral-crystalline-solid-occurs-nature-inorganic-defined

Criteria of a mineral (crystalline solid, occurs in nature, inorganic, defined chemical composition)

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Physical and Chemical Properties of Matter

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Physical Properties of Matter

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Stress-Strain Characteristics of Aluminum

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Properties of minerals (hardness, luster, cleavage, streak, crystal shape, fluorescence, flammability, density/specific gravity, malleability)

Content elaboration: This unit builds upon the Earth and Space Science strand in grade 6, where common minerals are defined, tested and classified. It also incorporates knowledge of mineral properties and crystalline structures (chemical compositions and bonding) included in the chemistry sections of other high school courses. The emphasis in this course is to relate the chemical and physical components of minerals to the properties of the minerals. This requires extensive mineral testing, investigations, experimentation, observation, use of technology and models/modeling. The focus is on learning the ways to research, test and evaluate minerals, not in memorization of mineral names or types. Properties such as cleavage and hardness are connected to the chemical structure and bonding of the mineral. In addition, the environment in which minerals form should be part of the classification of the mineral, using mineral data to help interpret the environmental conditions that existed during the formation of the mineral.

properties-minerals-hardness-luster-cleavage-streak-crystal-shape

Properties of minerals (hardness, luster, cleavage, streak, crystal shape, fluorescence, flammability, density/specific gravity, malleability)

Ionic Compounds and Electrolytes

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