0
When slight attractions that develop between oppositely charged regions of nearby molecules are called?
Wiki User
∙ 11y ago
When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. Chemists call such intermolecular forces of attraction van der Waals forces.
(This also occurs in the phenomenon known as Hydrogen-bonding.)
What is the alternate of a slight attraction - it is called the covalent bond. Note that an ionic bond is a type of covalent bond.
Wiki User
∙ 11y ago
Wiki User
∙ 14y agolet me see the answer please
When molecules are closed together, a slight attraction can develop between the oppositely charges regions of nearby molecules. Chemist call such intermolecular forces of attraction van der Waals forcesWiki User
∙ 11y agoThe slight attractions that develop between oppositely charged regions of nearby molecules are called van Leeuwenhoek forces.
Wiki User
∙ 10y agoDipole Dipole
#ApChemStudent
Wiki User
∙ 10y agoHydrogen bond.
Wiki User
∙ 11y agoadhesion
Add your answer:
Earn +20 pts
Why do nonpolar molecules not have oppositely charged ends?
Nonpolar molecule is one which electrons are shared equally in bonds. Such a molecule does not have oppositely charged ends. This is true of molecules made from two identical atoms or molecules that are symmetric, such as CCl4.
Is a compound formed by two positive elements?
No, two positives are repelling, not attracting. No. Compounds are formed by two or more different elements. An ionic compound is formed by the attraction between two oppositely charged ions. Molecular compounds are formed by the sharing of electrons between atoms, which is called a covalent bond.
The force of attraction binding oppositely charged ions together?
There are a few ways to calculate this, but for two point charges, such as two oppositely charged atoms the easiest way is to use Coulomb's law:where:F = the force of attractionq_1 = the charge of object 1q_2 = the charge of object 2r = the distance between the center of object 1 and object2ε0 ≈ 8.854187817... × 10−12 F·m−1For two oppositely charged atoms you must know what the charge of the each atom is to complete the calculation. For this calculation I'll assume that object 1 has one more electron than a neutrally charged atom ( has a charge of 1 e-), and object two has one fewer electron than a neutrally charged atom (has a charge of e+)e = 1.602176487 x 10-19 coulombsSo if we fill everything into Coulomb's equation we can get the force of attraction between two oppositely charged atoms,
When is an ionic bond formed?
An ionic bond forms when two oppositely charged ions combine.
Why do polar substances dissolve well in other polar substances?
Polar solvents are characterized by regions with strong positive or negative electrical charges. For example water, the most usual polar solvent, is negatively charged on the oxygen end of the molecule and positively charged on the hydrogen end, simply because the oxygen nucleus attracts the shared electrons more strongly than the hydrogen nuclei do (and the hydrogen atoms are arranged at the points of a tetrahedron, rather than in a straight line with the oxygen atoms). And a typical polar solute such as sodium chloride, has positively charged sodium ions and negatively charged chlorine ions because chlorine has a much stonger attraction for electrons than sodium does, so it takes an electron from sodium. And then, given Coulomb's Law, we get an attraction between oppositely charged chemicals or portions of chemicals; the positively charged sodium ions would be attracted to the negatively charged oxygen region of the water molecule, the negatively charged chlorine ions are attracted to the positively charged hydrogen region of the water molecule. It is these electrostatic attractions which cause the solute to dissolve in the solvent.
What is a chemical bound?
Slight attractions that develop between oppositely charged regions of nearby molecules.
The slight attractions that develop between oppositely charged regions of nearby molecules are?
van der Waals forces.
What are molecules that do not have opposite charged ends?
Molecules that do not have oppositely charged ends are nonpolar molecules.
What are the slight attractions the develop between oppositely charged regions of nearby molecules?
When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. Chemists call such intermolecular forces of attraction van der Waals forces. (This also occurs in the phenomenon known as Hydrogen-bonding.) What is the alternate of a slight attraction - it is called the covalent bond. Note that an ionic bond is a type of covalent bond.
Which type of bond forms between oppositely-charged region of polar molecules?
Hydrogen bond
Molecules that do not have oppositely charged ends are what molecules?
Molecules that do not have oppositely charged ends are nonpolar molecules.
Which type of bonds are electrostatic attractions oppositely charged atoms?
Ionic bonds
How are ionic substances held together?
Ionic substances are held together ionic bonds, which are the electrostatic attractions between oppositely charged ions.
Why do nonpolar molecules not have oppositely charged ends?
Nonpolar molecule is one which electrons are shared equally in bonds. Such a molecule does not have oppositely charged ends. This is true of molecules made from two identical atoms or molecules that are symmetric, such as CCl4.
What happens when polar molecules are between oppositely charged metal plates?
When polar molecules are placed between oppositely charged metal plates they will align themselves. They align in the direction of the field.
What molecule that has oppositely charged ends is called?
Those molecules are polar.
In an ionic bond atoms are not sharing electrons What keeps the ions close together?
The strong ionic forces (electrostatic) of attractions that exists between the positively and negatively charged molecules keeps the ions together. remember that oppositely charged ions tend to attract. The is also weak Van der waals forces of attraction.
