Carbon monoxide (CO) is a colorless, odorless gas that is composed of one carbon atom and one oxygen atom. The dipole moment of a molecule is a measure of the separation of positive and negative charges within the molecule. The dipole moment of CO is 0.112 D, which means that the positive and negative charges are separated by 0.112 debye units. The electronegativity of carbon is 2.55, while the electronegativity of oxygen is 3.44. This difference in electronegativity means that the electrons in the CO molecule are pulled more strongly towards the oxygen atom than towards the carbon atom. As a result, the oxygen atom has a partial negative charge, while the carbon atom has a partial positive charge.
Unraveling the Molecular World: Unlocking the Secrets of Molecules
Introduction
In the realm of chemistry, molecules reign supreme. They’re like tiny building blocks that make up everything around us. But it’s not just their existence that fascinates us; it’s the characteristics that make each molecule unique. So, let’s dive into the intriguing world of molecular properties, the factors that influence their behavior, and how they shape our world.
Meet the Molecular Influencers
The properties of molecules aren’t just random accidents. They’re influenced by a symphony of factors, like a conductor leading an orchestra. These factors include:
- Dipole moment: The electrical imbalance within a molecule, like a lopsided see-saw.
- Polarity: The degree to which a molecule’s electrons are unevenly distributed, giving it a positive and negative end—sort of like a molecular magnet.
- Molecular orbitals: Energy levels within a molecule where electrons reside, like the different rooms in a house.
- Types of bonds: The connections between atoms that form molecules, like the types of glue that hold a puzzle together.
The Dance of Dipole Moments
Picture this: a molecule with positive and negative charges separated, like a tiny dipole. This dipole moment is like a molecular dance partner, influencing how the molecule interacts with its surroundings. It’s like the chemistry version of a social butterfly, determining which molecules it’s attracted to (or repelled by).
Unveiling the Secrets of Polarity
Polarity is the molecular version of a mood swing—it shows how unevenly electrons are distributed. Polar molecules are like tiny dipoles, with positive and negative ends. They behave like magnets, attracting other molecules like partners in a cosmic game of musical chairs.
Navigating the Molecular Orbital World
Molecular orbitals are like energy highways for electrons within a molecule. They’re the places where electrons hang out, like electrons dancing at a molecular rave. The shape and energy of these orbitals determine the molecule’s bonding characteristics and reactivity—like the blueprint for a molecular castle’s architecture.
Deciphering the Bond Code
From sigma bonds—the molecular equivalents of sturdy pillars—to pi bonds—the molecular version of graceful archways—the types of bonds between atoms shape the structure and properties of molecules. They’re like the molecular building blocks, connecting atoms to form an intricate tapestry of molecules.
In Conclusion
The factors influencing molecular properties are like the invisible puppet masters, pulling the strings of molecular behavior. Understanding these factors is like gaining a superpower, unveiling the secrets of molecules—the fundamental building blocks of our world. So, next time you encounter a molecule, remember the fascinating interplay of its properties, the puppet show of molecular influences that make it a unique and captivating player in the symphony of chemistry.
Define dipole moment and explain its units.
Molecular Properties: The Building Blocks of Molecular Behavior
Have you ever wondered why some molecules are like shy wallflowers, while others are the life of the party? It all boils down to their molecular properties, the quirks that define their behavior.
Dipole Moment: Measuring Molecular Polarity
Imagine a molecule as a tiny tug-of-war game. Dipole moment measures the strength of this tug-of-war, with positive and negative sides attracting or repelling each other.
Just like a bar magnet, molecules can have a net dipole moment. Think of a magnet with a strong north and south pole. The greater the dipole moment, the more polarized the molecule. This polarity plays a huge role in shaping intermolecular interactions, those friendly little bonds that hold molecules together.
Explore its significance in describing the polarity of molecules.
Factors Influencing Molecular Properties
In the realm of chemistry, understanding the molecular properties of substances is crucial for unraveling their behavior and interactions. These properties are like personality traits for molecules, shaping how they act in the world around them. And just like us humans, molecules are influenced by a variety of factors that determine their characteristics.
One of the most important factors is dipole moment, a measure of how polar a molecule is. It’s like the “electrical personality” of a molecule, telling us whether it has a positive or negative end. This polarity is key in determining how molecules interact with each other and with their environment.
So, What’s the Significance of Dipole Moment?
- It helps us predict intermolecular interactions. Polar molecules are like magnets, attracting each other due to their opposite charges. This attraction leads to stronger forces between molecules, affecting their behavior in solids, liquids, and gases.
- It gives us insights into solvent properties. Solvents, like water, are polar molecules. The polarity of a solvent determines which substances it can dissolve and how well it can dissolve them. A polar solvent dissolves polar solutes, while a nonpolar solvent dissolves nonpolar solutes.
By understanding dipole moment, we can unlock a deeper understanding of molecular interactions and predict how substances will behave in various environments. It’s like having a secret superpower that allows us to decode the language of molecules, revealing their hidden personalities and how they dance together in nature’s grand symphony.
Unveiling the Secrets of Dipole Moments: A Journey into Molecular Polarity
Imagine you have a molecule with a positive and negative charge separated like two magnets. This dipole moment quantifies the strength and direction of this molecular “tug-of-war.” It’s like the compass of the molecular world, guiding their interactions and influencing their properties.
Calculating dipole moments is no child’s play, but we’ve got some cool tricks up our sleeves. One way is to measure the molecule’s interaction with an electric field. It’s like putting a magnet in a magnetic field and seeing how it aligns. The stronger the dipole moment, the more the molecule dances to the electric field’s tune.
Another technique involves measuring the molecule’s dielectric constant, which tells us how much it can weaken an electric field. Think of it as the molecule being a “buffer” for electric fields. The larger the dipole moment, the better it can shield against the field.
By using these methods, we can uncover the secrets of dipole moments and understand how they shape the fascinating world of molecules.
Define and measure molecular polarity.
Unraveling the Essence of Molecules: Properties, Bonding, and Their Significance
Molecules, the fundamental building blocks of everything around us, hold a fascinating tale of properties and interactions. In this adventure, we’ll explore the factors that shape these molecular characteristics, from their electrical behavior to the nature of bonds that hold them together.
The Dance of Dipole Moments: Measuring Molecular Polarity
Envision a molecule as a miniature dance party, with electrons twirling around the atomic nuclei. This merry-go-round creates a dipole moment, a measure of how unevenly electricity is distributed within the molecule. Like a tiny magnet, molecules with a dipole moment have a positive end and a negative end.
Calculating this dipole moment is like finding the center of the dance floor. We sum up the contributions of each electron, weighting them by their distance from the molecule’s center. It’s like balancing a seesaw, figuring out which side has more weight and where it tips.
Polarity: Shaping Molecular Alliances
Molecular polarity, like a shy introvert or an extroverted social butterfly, determines how molecules interact with each other. Polar molecules make buddies with other polar molecules, attracted by their opposite charges. Nonpolar molecules, on the other hand, prefer their own company, like introverts hanging out with introverts.
This polarity game plays a huge role in everyday life. It’s what makes water such a great solvent, dissolving polar substances like salt. It’s also the reason oil and water don’t mix, as oil molecules are nonpolar and have no desire to mingle with water’s polar gang.
Unveiling the Secrets of Molecular Polarity and Intermolecular Interactions
Picture this: molecules at a party, mingling and bonding. But some molecules have a bit of a “love-hate” relationship, like magnets with opposing poles. That’s where molecular polarity comes into play.
Polarity is like the good old “yin and yang” concept. A molecule can have a slightly positive end (partial positive) and a slightly negative end (partial negative), like a tiny dipole magnet. This polarity arises when electrons, those loveable tiny particles, are not evenly distributed within the molecule.
So, how does this polarity affect the party? Well, it’s like a dance floor. Polar molecules tend to attract each other, just like opposite poles of magnets. They’re drawn to each other, creating intermolecular interactions. These interactions can be like sticky notes, holding molecules together in liquids and solids.
But polarity’s not just about sticking molecules together. It also influences how they behave. For instance, polar solvents (like water) can dissolve polar substances more easily. Think of it like kids playing with magnets: polar molecules are like the colorful magnets that stick together, while nonpolar molecules (*like oil*) are like magnets that just don’t get along.
Understanding polarity is like having the secret handshake to the molecular party. It helps us make sense of how molecules interact, how substances dissolve, and even why some things stick together while others slide right off. So next time you’re thinking about molecules, remember the power of polarity and how it shapes their interactions.
Diving into Molecular Properties: Unlocking the Secrets of Matter
Molecular properties are like fingerprints for molecules, revealing their unique characteristics. From dipole moments to bond types, these properties shape the way molecules interact with their surroundings and dictate their behavior in the real world.
One intriguing property is polarity, a measure of how unevenly electrons are distributed within a molecule. Polar molecules, like the shy kid in class, avoid getting too close to their nonpolar counterparts. But when polar solvents, like water, meet nonpolar substances, it’s a different story. The polar solvent molecules get all cozy, surrounding the nonpolar molecule like a warm embrace, creating a solvation shell.
This solvation shell can have a profound impact on the properties of the dissolved substance. For instance, polar substances tend to be more soluble in polar solvents because they can form these cozy embraces more easily. It’s like finding your perfect match in the dance of chemistry!
So, next time you’re admiring a sunset or sipping on your morning coffee, remember that the beauty and enjoyment you experience are all thanks to the fascinating world of molecular properties. They’re the invisible forces that make our world what it is, from the colors we see to the flavors we taste. It’s like a symphony of molecules, each playing its part in the grand scheme of things.
Understanding the Molecular Building Blocks: Molecular Orbitals
Hey there, curious minds! Let’s venture into the fascinating world of molecular orbitals (MOs). These are like the tiny energy levels within molecules that determine how atoms bond and interact. Picture them as the cozy apartments where electrons reside, each with its own unique energy and personality.
The Energy Dance
MOs aren’t just random energy levels floating about; they’re arranged in a specific order, kinda like a ladder. Each MO has a unique set of energy characteristics, and electrons love to hang out in the lowest energy levels first, like lazy bums on a couch.
The Bonding Blender
Now, here’s where the magic happens. When atoms get cozy and decide to bond, their atomic orbitals (like their apartments) merge to create MOs. But these new molecular orbitals aren’t just copies of the atomic ones; they’re a blend, just like mixing different colors of paint to create a new shade.
Bonding BFFs and Anti-Bonding Frenemies
Depending on how the atomic orbitals overlap, you can get two types of MOs: bonding MOs and anti-bonding MOs. Bonding MOs are like the ultimate besties, bringing electrons closer together and strengthening the bond between atoms. Anti-bonding MOs, on the other hand, are like mischievous rebels, pushing electrons apart and weakening the bond.
So, there you have it, a sneak peek into the fascinating world of molecular orbitals. They’re like the architects of molecules, determining their structure, properties, and even reactivity.
Unraveling the Mysteries of Molecular Orbitals
In the captivating world of chemistry, molecular orbitals take center stage, the architects of every bond and reaction that shapes the universe. Picture them as the dance floors of atoms, where electrons gracefully twirl to the rhythm of chemistry.
These orbitals, like invisible dance studios, define the energy levels at which electrons can reside. Some are close to the nucleus, cozy and low in energy, while others venture further, like adventurous electrons seeking new experiences.
The dance choreography of electrons in these orbitals determines the chemical bonding between atoms. When orbitals overlap, electrons find their groove together, forming covalent bonds that hold molecules in place. These bonds, like unbreakable friendships, give molecules their shape and properties.
But molecular orbitals are not just passive bystanders in chemical reactions. They’re the matchmakers that bring atoms together to form new molecules. They orchestrate the electron transfer that sparks chemical reactions, creating the countless substances that make our world.
Understanding molecular orbitals is like unlocking the secret language of chemistry. It unveils the choreography of electrons, the formation of bonds, and the driving force behind chemical reactions. So, let’s dive deeper into this fascinating world and unravel the mysteries of molecular orbitals!
Understanding the Quirky World of Molecules: A Guide to Their Invisible Forces
Factors Influencing Molecular Properties
Picture molecules as tiny worlds, each with its own unique personality. Just like you and me, their characteristics are shaped by a multitude of factors. These include things like their dipole moment, polarity, molecular orbitals, and bond types.
Dipole Moment: A Measure of Molecular Polarity
Imagine molecules as little dipoles, with a positive end and a negative end like a mini battery. Their dipole moment measures this polarity. If the positive and negative charges are separated by a large distance, the dipole moment is high, making the molecule polar. But if the charges are close together, the dipole moment is low, and the molecule is less polar.
Polarity: Shaping Intermolecular Interactions
Polar molecules are like magnets; they attract or repel each other depending on their orientation. This polarity plays a huge role in how molecules interact with each other, influencing everything from the properties of liquids to the behavior of biological systems.
Molecular Orbitals: Unlocking Chemical Bonding
Molecular orbitals are the quantum playgrounds where electrons dance around the nucleus. These orbitals have different energies and shapes, and they determine how atoms bond together to form molecules. Understanding molecular orbitals is like knowing the secret handshake to chemical bonding.
Sigma Bonds: The Cornerstone of Molecular Structure
Sigma bonds are the backbone of molecular structures. They’re formed when orbitals overlap head-to-head, creating a strong, single bond. Sigma bonds hold atoms together like the pillars of a building, giving molecules their shape and stability.
Pi Bonds: Adding Complexity to Molecular Bonding
Pi bonds are like the acrobats of molecular bonding. They’re formed when orbitals overlap side-to-side, creating a weaker, but more flexible bond. Pi bonds add flavor to molecules, giving them their reactivity and color.
Visualization and Representation Techniques for Molecular Orbitals
Visualizing molecular orbitals is like looking into the innermost secrets of molecules. We use diagrams and simulations to represent these orbitals, which helps us understand how electrons behave within molecules. It’s like having a superpower that lets us see the invisible forces that govern the chemical world.
Understanding the factors influencing molecular properties is like unlocking the secrets to the molecular world. By exploring dipole moments, polarity, molecular orbitals, and bond types, we can delve into the intricate world of molecules and appreciate the incredible forces that shape their interactions.
Unraveling the Essence of Sigma Bonds: The Bedrock of Molecular Architecture
Imagine molecules as tiny building blocks, held together by invisible forces known as bonds. Among these, sigma bonds stand out as the cornerstone of molecular structure, the unsung heroes that define the shape and properties of countless compounds.
Sigma bonds, denoted by the Greek letter σ, are formed when two atomic orbitals overlap head-on, like two interlocking gears. This head-to-head embrace creates a region of high electron density, forming a strong and stable bond.
The strength of a sigma bond depends on the participating atomic orbitals. Smaller orbitals with higher energy overlap more effectively, leading to stronger bonds. Additionally, the number of electrons involved plays a crucial role. The more electrons shared between the atoms, the stronger the sigma bond.
Sigma bonds form the backbone of many molecules, including alkanes, alkenes, and alkynes. They determine the length and shape of molecules, influencing their physical and chemical properties. By understanding sigma bonds, we gain insights into the behavior of matter at its most fundamental level.
Formation of Sigma Bonds: An Orbital Tango
Picture two atomic orbitals, each carrying a single electron, engaging in a graceful dance. As they approach each other, their lobes intertwine, creating a head-on overlap. This overlap results in the formation of a new molecular orbital, the sigma bond, which houses a pair of electrons.
The sigma bond is symmetrical along the internuclear axis, meaning it has the same electron density on both sides of the bond. This symmetry contributes to the stability and strength of sigma bonds.
Impact of Sigma Bonds on Molecular Structure
Sigma bonds play a critical role in determining the overall shape and structure of molecules. They act as pillars of support, holding atoms together and dictating the bond angles and molecular geometry. For example, in methane (CH₄), four sigma bonds extend from a central carbon atom to four hydrogen atoms, creating a tetrahedral shape.
The length of sigma bonds also influences molecular structure. Generally, shorter bonds are stronger and result in more compact molecules. Conversely, longer bonds are weaker and lead to more elongated structures.
Understanding sigma bonds is essential for unraveling the complexities of molecular architecture and predicting the properties of chemical compounds.
Unraveling the Mysteries of Molecules: Exploring Factors That Shape Their Properties
Get ready to dive into the fascinating world of molecules! These tiny building blocks of everything around us exhibit remarkable properties that determine their behavior and interactions. Let’s embark on a journey to unravel the factors that influence these properties, making molecules the masters of their own destiny.
Chapter 1: Meet the Maestro – Dipole Moment
Dipole moment, the measure of a molecule’s polarity, is like a tiny compass that tells us how the electrical charge is distributed within it. It’s the “push and pull” of electrons that gives molecules a personality, shaping their interactions with their surroundings. Remember, a molecule with a zero dipole moment is like a perfectly balanced scale, while a molecule with a dipole moment is ready for a good old-fashioned tug-of-war!
Chapter 2: Polarity – The Magnet of Molecules
Polarity is like the socialite of the molecular world, constantly mingling and influencing other molecules. It’s the tendency of a molecule to have a slightly positive or negative end, creating a force field that attracts or repels its neighbors. Think of polar molecules as tiny magnets, ready to dance with their oppositely charged counterparts.
Chapter 3: Molecular Orbitals – The Dance Floor of Electrons
Molecular orbitals are the dance party places for electrons, where they groove and move to the rhythm of the atomic nucleus. These orbitals are like energy levels where electrons can hang out, determining the molecule’s bonding characteristics. And guess what? These orbitals aren’t just random shapes; they can be sigma or pi, adding complexity and flavor to the molecular bonding scene!
Chapter 4: Sigma Bonds – The Building Blocks of Molecules
Sigma bonds are the backbone of molecular structures, the strong and stable connections that hold atoms together. Picture them as the sturdy pillars that keep our molecular houses standing. They form when two atomic orbitals overlap head-on, creating a direct pathway for electrons to flow. These bonds are crucial for determining a molecule’s shape and stability, making them the fundamental building blocks of our molecular universe.
Chapter 5: Pi Bonds – The Spice of Molecular Life
Pi bonds are the funky fresh cousins of sigma bonds, adding a dash of complexity and intrigue to the molecular world. They arise when two atomic orbitals overlap sideways, creating a “pretzel-like” structure. These bonds are weaker than sigma bonds but bring a unique set of properties to the table, affecting the molecule’s reactivity and absorption of light. Think of them as the “spice girls” of the molecular scene, adding a dash of excitement and flair!
Understanding Molecular Bonds: The Glue That Holds Molecules Together
In the fascinating world of molecules, there’s a hidden language of forces and interactions that determine how they behave. Just like our own bodies are built from a network of bones and tissues, molecules are held together by a web of chemical bonds. And among these bonds, two stand out as the primary players: sigma bonds and pi bonds.
Sigma Bonds: The Backbone of Molecular Structure
Picture sigma bonds as the building blocks of molecular architecture. These bonds form when two atomic orbitals overlap head-to-head, resulting in a strong and stable connection. Think of them as the pillars that hold the molecular structure together, keeping atoms in place.
Impact on Molecular Structure
Sigma bonds have a profound impact on the overall shape and geometry of molecules. They dictate the alignment of atoms and determine whether a molecule is linear, bent, or even tetrahedral. For example, in methane (CH₄), the four sigma bonds between the carbon atom and the four hydrogen atoms create a symmetrical tetrahedron shape.
Properties Influenced by Sigma Bonds
Sigma bonds also influence a molecule’s rotational properties. The strength and distribution of sigma bonds determine how easily a molecule can rotate around its bonds. This, in turn, affects the molecule’s energy levels and reactivity.
Strength and Stability: Sigma bonds are typically the strongest and most stable type of bond because of their head-to-head overlap. This means that molecules with a higher number of sigma bonds tend to be more stable and less likely to break apart.
Sigma bonds are the fundamental building blocks of molecular structure. They determine the shape, geometry, and properties of molecules, providing the foundation for the complex world of chemistry. So, next time you encounter a molecule, take a moment to appreciate the hidden forces that hold it together—the sigma bonds, the silent heroes of molecular architecture.
Pi Bonds: The Jazzy Sidekicks of Molecular Bonding
Pi bonds, my friends, are the cool cats of the molecular world. They’re not as common as their straight-laced cousin, sigma bonds, but when they show up, they add a whole new dimension to the party.
Think of sigma bonds as the backbone of a molecule, holding everything together with a strong, single bond. Pi bonds, on the other hand, are the groovy sidekicks that bring the funk. They’re formed by the overlap of parallel atomic orbitals, creating a weaker bond but one that gives molecules their distinctive shapes and properties.
Like sigma bonds, pi bonds have their own unique characteristics and strengths. They’re not as strong, but they’re more flexible, allowing molecules to bend and twist without breaking apart. This flexibility is what gives pi bonds their importance in many biological processes, like the formation of DNA and proteins.
So, next time you hear about pi bonds, don’t think of them as some boring chemical concept. They’re the funky, flexible backbone that gives molecules their rhythm and style!
Digging into the Molecular Make-up of Our World: Properties and Bonds
Hey there, science enthusiasts! Let’s dive into the fascinating world of molecules and uncover the secrets behind their unique properties. From polarity to bonds, we’ll explore the factors that shape the behavior of these tiny building blocks of our universe.
Factors Influencing Molecular Properties
Imagine molecules as little magnets, dipole moments. They measure how much positive and negative charge is separated within the molecule. Polarity is a measurement of this separation, like a dance between two partners. These properties can be influenced by a bunch of factors:
- Shape matters! Molecules can be straight, branched, or even ring-shaped, like tiny pretzels.
- Electronegativity is the greediness of atoms for electrons. The more greedy an atom, the more it pulls electrons towards itself, creating a dipole moment.
- Types of bonds between atoms also play a role. We’ll uncover these bond secrets later.
Dipole Moment: The Measure of Molecular Polarity
Dipole moments are like tiny rulers, measuring the distance between positive and negative charges. We measure them in Debye units, named after a famous scientist named Peter Debye.
Polar molecules have significant dipole moments, while nonpolar molecules have little to no separation of charge. This polarity is like the social circles of molecules: they tend to hang out with similar types. Polar molecules prefer the company of other polar molecules, forming bonds that can be strong or weak.
Polarity: Shaping Molecular Relationships
Polarity influences how molecules interact with each other. Imagine a tea party where molecules are the guests: polar molecules are the chatty ones, forming strong bonds, while nonpolar molecules are the wallflowers, politely avoiding interactions.
Polarity also affects how molecules behave in solvents, like water and oil. Polar molecules tend to dissolve in polar solvents, while nonpolar molecules prefer nonpolar solvents. It’s like the old saying: like dissolves like.
Molecular Orbitals: The Secret Language of Bonds
Molecular orbitals are like the scaffolding that holds molecules together. They’re created when atomic orbitals, the electron dance parties of individual atoms, overlap. This overlap creates new, larger orbitals that determine how molecules bond.
Sigma Bonds: The Strong Foundations of Molecules
Sigma bonds are the sturdy pillars of molecular structures. They form when orbitals overlap head-on, creating a strong, single bond. But don’t be fooled by their simplicity: sigma bonds are the backbone of many molecular structures.
Pi Bonds: Adding Complexity to Molecular Bonding
Pi bonds are the funky cousins of sigma bonds. They form when orbitals overlap sideways, creating a double bond. Double bonds are more flexible and reactive than single bonds, and they often give molecules their characteristic shapes and colors.
So, there you have it, a glimpse into the world of molecular properties and bonds. From dipole moments to sigma and pi bonds, these factors shape the behavior of molecules and the world around us. Stay tuned for more exciting explorations into the realm of chemistry!
Pi Bonds: The Mysterious Force Behind Molecular Magic
Pi bonds, my friends, are the unsung heroes of the molecular world. They add an extra dimension to bonding, bringing molecules to life with their unique characteristics.
Like their sigma counterparts, pi bonds form when atomic orbitals overlap. But here’s the twist: they do it sideways, like a dance between orbitals. This sideways overlap creates a region of electron density above and below the plane of the atoms, giving pi bonds their distinctive shape.
But don’t let their fancy footwork fool you. Pi bonds have a serious impact on the molecular party. They’re responsible for the 3D structure of molecules, giving them their unique shapes. For instance, the double bond in ethylene (C2H4) is made of a sigma bond and a pi bond, creating the molecule’s iconic bent shape.
Pi bonds also influence molecular properties. They tend to be weaker than sigma bonds, making molecules more flexible and allowing them to rotate around their double bonds. This flexibility is crucial for biological processes like cell division and protein folding. Additionally, pi bonds can interact with each other, creating even more intricate molecular structures.
In the world of chemistry, pi bonds are the secret ingredient that adds complexity and diversity to molecules. They shape everything from the way molecules look to how they behave, making them a fundamental part of the molecular universe.
Well, there you have it – the not-so-hidden secrets of carbon monoxide’s dipole moment. Thanks for sticking with me on this little scientific adventure. I know it might not have been the most thrilling read, but I hope you learned something new and interesting. If you’ve got any more questions or if you just want to chat about chemistry, feel free to drop me a line. And don’t forget to check back later for more fascinating science stuff!