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Sinevibes Dipole Stereo Flanger
The Sinevibes Dipole offers a comprehensive through-zero flanger effect packaged additionally with accessible experimental potentials and a simple colour-coded user interface. Bolster your mix with the movement depth and character of both traditional and modern style flanger effects produced with high fidelity and ease of access. Take direct control over sparkling spectral swooshes or signal warps and cancellations or utilise Dipoles built-in multi-waveform generator for complex and provocative modulations. Ensure that Dipole fits comfortably within your mix with variable phase offset low-cut filter and feedback self-levelling to ensure stable operation under even the most extreme settings. Please Note: This product comes in the form of a digital download code that will be sent to your email for activation.
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Electric-dipole Polarizabilities Of Atoms, Molecules, And Clusters
This book is an in-depth review of experiment and theory on electric-dipole polarizabilities.It is broad in scope, encompassing atomic, molecular, and cluster polarizabilities.Both static and dynamic polarizabilities are treated (in the absence of absorption) and a full tensor picture of the polarizability is used.Traditional experimental techniques for measuring electric polarizabilities are described in detail.Recently developed experimental methods, including light forces, position-sensitive time-of-flight deflection, and atom interferometry, are also extensively discussed.Theoretical techniques for calculating polarizabilities are reviewed, including a discussion on the use of Gaussian basis sets.Many important comparisons between theory and experiment are summarized in an extensive set of tables of polarizabilities of important atoms, molecules, and clusters.Applications of polarizabilities to many areas of chemistry and physics are described, including optics, chemical structure, interactions of gases and particles with surfaces, and the interaction of molecules with light.The emphasis is on a lucid presentation of the ideas and results with up-to-date discussions on important applications such as optical tweezers and nanostructure fabrication.This book provides an excellent overview of the importance of polarizabilities in understanding the physical, electronic, and optical properties of particles in a regime that goes from free atoms to condensed-phase clusters.
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Portable 4:1 HF Shortwave Dipole Antenna Balun Mini Barron Waterproof
Portable 4:1 HF Shortwave Dipole Antenna Balun Mini Barron Waterproof
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Portable 4:1 HF Shortwave Dipole Antenna Balun Mini Barron Waterproof
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How do dipole-dipole forces affect the boiling temperature?
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. These forces cause the molecules to be attracted to each other and stick together, making it more difficult for them to break apart and become a gas. As a result, substances with stronger dipole-dipole forces will have higher boiling temperatures because more energy is required to overcome these attractive forces and turn the substance into a gas. Therefore, the presence of dipole-dipole forces can increase the boiling temperature of a substance.
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Why are hydrogen bonds stronger than dipole-dipole interactions?
Hydrogen bonds are stronger than dipole-dipole interactions because they involve a specific interaction between a hydrogen atom and a highly electronegative atom such as oxygen, nitrogen, or fluorine. This creates a strong partial positive charge on the hydrogen atom and a strong partial negative charge on the electronegative atom, leading to a strong attraction between the two. In contrast, dipole-dipole interactions occur between the partial positive and negative charges of polar molecules, which are generally weaker than the specific interaction between a hydrogen atom and a highly electronegative atom in a hydrogen bond.
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Why do ethers have only weak dipole-dipole interactions?
Ethers have only weak dipole-dipole interactions because the oxygen atom in the ether molecule is less electronegative than the oxygen atom in alcohols or the nitrogen atom in amines. This results in a smaller difference in electronegativity between the oxygen and the carbon atoms in the ether molecule, leading to weaker dipole moments. As a result, the overall dipole-dipole interactions in ethers are weaker compared to molecules with larger electronegativity differences, such as alcohols and amines.
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Is the ammonia molecule a dipole or not a dipole?
The ammonia molecule is a dipole. This is because the molecule has a trigonal pyramidal shape with a lone pair of electrons on the nitrogen atom. The electronegativity difference between nitrogen and hydrogen causes the molecule to have a net dipole moment, with the nitrogen end being partially negative and the hydrogen end being partially positive. This makes ammonia a polar molecule.
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Why is CO2 not a dipole and H2O a dipole?
CO2 is not a dipole because it has a linear molecular geometry, meaning the two oxygen atoms are symmetrically arranged around the central carbon atom, resulting in a net dipole moment of zero. On the other hand, H2O is a dipole because it has a bent molecular geometry, causing the oxygen atom to pull the shared electrons closer to itself, resulting in a net dipole moment. This uneven distribution of charge creates a positive end (the hydrogen atoms) and a negative end (the oxygen atom), making H2O a polar molecule.
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What is the difference between a dipole and a non-dipole?
A dipole is a molecule that has a separation of positive and negative charges, resulting in a net dipole moment. This means that the molecule has a non-uniform distribution of electron density, leading to a partial positive and partial negative charge. On the other hand, a non-dipole molecule has a symmetrical distribution of electron density, resulting in no net dipole moment. This means that the molecule does not have a separation of positive and negative charges, and therefore does not exhibit dipole-dipole interactions.
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When do Van der Waals forces and dipole-dipole interactions occur?
Van der Waals forces occur between all atoms and molecules, regardless of their polarity, due to temporary fluctuations in electron distribution. Dipole-dipole interactions, on the other hand, occur between polar molecules that have a permanent separation of positive and negative charges. Both types of interactions are important in determining the physical properties of substances, such as their boiling and melting points, and play a significant role in the behavior of gases, liquids, and solids.
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What is the difference between hydrogen bonding and dipole-dipole interactions?
Hydrogen bonding is a specific type of dipole-dipole interaction that occurs between a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and another electronegative atom in a different molecule. This type of interaction is stronger than regular dipole-dipole interactions because of the large electronegativity difference between the hydrogen and the other atom, resulting in a stronger attraction between the molecules. In contrast, dipole-dipole interactions occur between the positive end of one polar molecule and the negative end of another polar molecule, but do not involve a hydrogen atom bonded to a highly electronegative atom.
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