4. All magnets areA. dipolesB. bipolesC. monopolesD. multipoles
1. 4. All magnets areA. dipolesB. bipolesC. monopolesD. multipoles
Answer:
d. multipoles
Explanation:
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C.monopoles=============================
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2. Magnets have north-seeking and south seeking poles, therefore they are considered as1. no pole2.monopole3.dipole4.tripole
Answer:
1. no pole
2. minopole
3. dipole
4. tripole
5. sapole
3. angle 1 and angle2 are vertical angles. mangle1= 4x + 7 and mangle2= 5x – 8, what is the relationship between the angles?
Step-by-step explanation:
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4. Is Dipole-dipole interactions a gas?
Answer:
no
Explanation:
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5. what is dipole-dipole attractions?
Answer:
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. ... The partially positive end of a polar molecule is attracted to the partially negative end of another.
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6. definition manometer
Answer:
Manometers are precision instruments that are used to measure pressure, which is the force exerted by a gas or liquid per unit surface area owing to the effects of the weight of that gas or liquid from gravity.
MA-NO-ME-TER
an instrument for measuring the pressure acting on a column of fluid, especially one with a U-shaped tube of liquid in which a difference in the pressures acting in the two arms of the tube causes the liquid to reach different heights in the two arms.
7. what is dipole-dipole force
Answer:
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces have strengths that range from 5 kJ to 20 kJ per mole.
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8. 2. Illustrate and compare the following:a. Dipole - dipole force and dipole-induced dipole forceb. Dipole-induced dipole force and ion-induced dipole forcec. Hydrogen bonding and ion - dipole force
Answer:
B.Depole-induced dipole force and ion-induced dipole force.
9. dipole -included dipole interaction
Answer:
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chemical bonding
Table of Contents
Intermolecular forces
Molecules cohere even though their ability to form chemical bonds has been satisfied. The evidence for the existence of these weak intermolecular forces is the fact that gases can be liquefied, that ordinary liquids exist and need a considerable input of energy for vaporization to a gas of independent molecules, and that many molecular compounds occur as solids. The role of weak intermolecular forces in the properties of gases was first examined theoretically by the Dutch scientist Johannes van der Waals, and the term van der Waals forces is used synonymously with intermolecular forces. Under certain conditions, weakly bonded clusters of molecules (such as an argon atom in association with a hydrogen chloride molecule) can exist; such delicately bonded species are called van der Waals molecules.
There are many types of intermolecular forces; the repulsive force and four varieties of attractive force are discussed here. In general, the energy of interaction varies with distance, as shown by the graph in Figure 16. Attractive forces dominate to the distance at which the two molecules come into contact, then strong repulsive forces come into play and the potential energy of two molecules rises abruptly. The shape of the intermolecular potential energy curve shown in the illustration resembles that of the molecular potential energy curve in Figure 10. The minimum of the former is much shallower, however, showing that forces between molecules are typically much weaker than the forces responsible for chemical bonds within molecules.
intermolecular potential energy
intermolecular potential energy
Figure 16: An intermolecular potential energy curve. The graph shows how the potential energy of two molecules varies with their separation. The energy minimum is shallower than for the formation of a chemical bond between two atoms, as depicted in Figure 10 and indicated here in gray.
Encyclopædia Britannica, Inc.
Repulsive force
The repulsive part of the intermolecular potential is essentially a manifestation of the overlap of the wave functions of the two species in conjunction with the Pauli exclusion principle. It reflects the impossibility for electrons with the same spin to occupy the same region of space. More rigorously, the steep rise in energy is illustrated by the behaviour of two helium atoms and their possession of the configuration 1σ22σ2 (see above Figure 13). The antibonding effect of the upper energy orbital dominates the bonding effect of the 1σ orbital at all separations, and the energy of the former rises more rapidly than that of the latter falls. Consequently, as the internuclear separation is decreased, the total energy rises steeply. All closed-shell species behave in a similar manner for much the same reason.
Dipole–dipole interaction
The first of the four bonding interactions discussed here is the dipole–dipole interaction between polar molecules. It will be recalled that a polar molecule has an electric dipole moment by virtue of the existence of partial charges on its atoms. Opposite partial charges attract one another, and, if two polar molecules are orientated so that the opposite partial charges on the molecules are closer together than their like charges, then there will be a net attraction between the two molecules. This type of intermolecular force contributes to the condensation of hydrogen chloride to a liquid at low temperatures. The dipole–dipole interaction also contributes to the weak interaction between molecules in gases, because, although molecules rotate, they tend to linger in relative orientations in which they have low energy—namely, the mutual orientation with opposite partial charges close to one another.
Dipole–induced-dipole interaction
The second type of attractive interaction, the dipole–induced-dipole interaction, also depends on the presence of a polar molecule. The second participating molecule need not be polar; but, if it is polar, then this interaction augments the dipole–dipole interaction described above. In the dipole–induced-dipole interaction, the presence of the partial charges of the polar molecule causes a polarization, or distortion, of the electron distribut
10. O=C=0 and O=C=0 lon-Dipole Hydrogen Bonding. Dipole-Dipole London Dispersion and Na + H1 Н. lon-Dipole Hydrogen Bonding Dipole-Dipole London Dispersion and and O=0 O=0 H HI O H H H H lon-Dipole Hydrogen Bonding. Dipole-Dipole London Dispersion Ion-Dipole Hydrogen Bonding Dipole-Dipole London Dispersion
Answer:
B. Dispersion Force
D. lon-Dipole force
D. London force
C. Hydrogen bond
B. Dipole-Dipole
Explanation:
11. what is dipole-induced dipole?
These are weak forces. Ion-Induced Dipole Forces. An ion-induced dipole attraction is a weak attraction that results when the approach of an ion induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in the nonpolar species.
12. 3 examples of dipole dipole forces
A good example is HF (this is also an example of a special type of dipole-dipole force called a hydrogen bonding). In HF, the bond is a very polar covalent bond. That means there is a partial negative (δ-) charge on F and partial positive (δ+) charge on H, and the molecule has a permanent dipole (the electrons always spend more time on F). In the liquid or solid HF, the molecules arrange themselves so that the δ- and δ+ are close together. These partial charges attract each other, and this attraction is what we call dipole-dipole forces. Any molecule with a permanent dipole has dipole-dipole forces that hold the molecules next to each other as a solid or liquid.
13. diferences between ion-dipole and dipole-dipole forces?
[tex]Answer:[/tex]Ion-dipole forces are stronger than dipole interactions because the charge of any ion is much greater than the charge of a dipole; the strength of the ion-dipole force is proportionate to ion charge.A dipole-dipole force is when the positive side of a polar molecule attracts the negative side of another polar molecule. An ion-dipole force is a force between an ion and a polar molecule. These intermolecular ion-dipole forces are much weaker than covalent or ionic bonds.#Let'sStudy
14. Which of the following intermolecular forces of attraction (IMFA) is arrangedfrom strongest to weakest?a. H- bonding - dipole-dipole - London forcesb. London-forces - dipole-dipole - H-bondingc. Dipole-dipole - London forces - H- bondingd. H-bonding - London forces - dipole-dipole
Answer:
H-bonding - dipole-dipole - London forces
15. Dipole- dipole forces involves
Answer:Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces have strengths that range from 5 kJ to 20 kJ per mole.
Explanation:#HOPE IT HELPS:)
16. differentiate London dispersion force, dipole-dipole interaction and ion-dipole interaction.
Answer:
London dispersion forces occur between nonpolar molecules and are extremely weak. Dipole-dipole forces are between polar molecules, and since polar molecules have slight charges, their force is more similar to ions, giving them a moderately strong bond.
17. what is bipole bipole
Answer:
The word “Bipole” is used instead of “Dipole” when the two transmitting electrodes are placed so far apart that the electric field from them can be considered a field from two separate poles. In other words, the distance between the receiver and transmitter dipoles is small in relation to the dipoles themselves.
18. The strongest among the intermolecular forces of attraction.a. ion-dipoleb. H-bondingc. dipole-dipoled. dipole-induced dipole110
Answer:
A.ion-dipole
Explanation:
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19. interaction occurs between polar covalent and nonpolar covalent molecules? A. Dipole - intoduced dipoleB. dipole - dipole C. ion - ion D. intoduced dipole - intoduced dipole E. Ion - dipole
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20. compare and contrast ion dipole and dipole dipole forces
Answer:
on dipole forces are attractive forces between ionic species and polar molecules. Dipole-dipole forces are intermolecular forces that occur between polar molecules. Ion-dipole forces are stronger than hydrogen bonds and dipole-dipole forces. Dipole-dipole forces are weaker than hydrogen bonds and ion-dipole forces.
Explanation:
21. what is dipole-dipole interaction ?
Answer:
Dipole-Dipole interactions are attractive forces between polar molecules.
22. What is a dipole moment in chemistry?What is dipole moment example?How do you find the dipole moment?What is a dipole moment in physics?What is dipole moment 11th chemistry?
Answer:
What is a dipole moment in chemistry?
A dipole moment is the turning force a fixed charge has on a dipole in a molecule. The moment depends on the charge at the end of the dipole and its distance from the charge at the other end of the dipole (i.e., the separation of charge). µ = q×d.
What is the dipole moment example?
A dipole moment is simply the measure of net polarity in a molecule. ... Polar molecules exhibit a large difference in electrical charge (a positive end and a negative end), otherwise known as a dipole moment. For example, ammonia (NHsub3) is a polar molecule.
How do you find the dipole moment?
A dipole moment is the product of the magnitude of the charge and the distance between the centers of the positive and negative charges. It is denoted by the Greek letter 'µ'. It is measured in Debye units denoted by 'D'. 1 D = 3.33564 × 10-30 C.m, where C is Coulomb and m denotes a meter.
What is a dipole moment in physics?
The electric dipole moment is a measure of the separation of positive and negative electrical charges within a system, that is, a measure of the system's overall polarity. The SI unit for electric dipole moment is the coulomb-meter (C⋅m).
What is dipole moment 11th chemistry?
Dipole moments occur when there is a separation of charge. They can occur between two ions in an ionic bond or between atoms in a covalent bond; dipole moments arise from differences in electronegativity. ... The dipole moment is a measure of the polarity of the molecule.
Explanation:
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23. Answer the following Dipole-Dipole
Answer:
Dipole-Dipole forces exist between two polar molecules.One end of a dipole attracts the oppositely charged end of another dipole.
In electromagnetism, there are two kinds of dipoles: An electric dipole deals with the separation of the positive and negative charges found in any electromagnetic system. A simple example of this system is a pair of electric charges of equal magnitude but opposite sign separated by some typically small distance.
24. 4. What are considered van der Waals forces of attraction?A. ion-induced dipole; dipole-dipole; London dispersion forcesB. dipole-dipole; dipole-induced dipole: London dispersion forcesC.London dispersion forces; ion-induced dipole; dipole-induced dipoleD. dipole-induced dipole; ion-induced dipole; London dispersion forces
Answer:
b
Explanation:
it is in my answer key , hope it help
25. The strongest among the intermolecular forces of attraction.a. ion-dipoleb. H-bondingc. dipole-dipoled. dipole-induced dipole
Answer:
C.DIPOLE-DIPOLE
Explanation:
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Answer:
c
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#CarryOnLearning#Brainlest me26. which of the following intermolecular forces of attraction (IMFA)is arranged from strongest to weakest? a.H-bonding- dipole-dipole - London forces b. London-forces - dipole-dipole-H-bonding. C. Dipole-dipole - London forces-H-bonding... D. H- bonding- London forces- dipole- dipole..
Answer:
a
Explanation:
because I already know that
27. Interaction or dispersion forces occurs among nonpolar substances?A. Dipole - intoduced dipole B. dipole - dipole C. ion - ion D. intoduced dipole - intoduced dipole E. Ion - dipole
Answer:
A.Dipole - intoduced dipole
Explanation:
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28. what is the strongest among the intermolecular forces of attractiona. dipole-dipoleb. dipole induced diplec. h-bondingd. ion-dipole
Answer:
a. dipole-dipole
Answer:
a. dipole - dipoleDipole-dipole interactions are the strongest intermolecular force of attraction.
29. dipole dipole forces
Answer:
huh what you mean diple diple forces
30. What is Dipole-Dipole force?
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