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The amount of solute dissolved in one liter of solution in moles.

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The molecules of solids such H20 are held together by strong hydrogen bonds (ice). Electricity does not conduct through them. Under normal conditions of temperature and pressure, they are flammable liquids or soft solids.

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At room temperature and pressure, they have low melting temperatures and are frequently liquid or gaseous. In polar solvents, they're less soluble.

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Dipole-dipole interactions keep the molecules in such crystals together. These materials are soft and electrically inert.

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Intermolecular forces hold distinct molecules together to form molecular solids. Because these interactions are weak, molecular solids are soft and dissolve at low to moderate temperatures. Because their valence electrons are securely contained within each individual molecule, molecular solids are poor conductors of electricity. There are three kinds of molecular solids; polar, non-polar, and hydrogen bonded molecular solids.

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graphite and diamond

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Network covalent solids are crystalline solids that are made up of a vast three-dimensional network of individual atoms held together by strong covalent bonds. Examples of network covalent solids include diamond, which has a continuous network of carbon atoms, and quartz, which has a continuous network of silicon and oxygen atoms.

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Ionic solids are crystalline solids made up of positively and negatively charged ions held together by strong electrostatic forces (ionic bonds).

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Metallic solids are solids made up of metal atoms joined by metallic bonds. These bonds resemble enormous molecular orbitals that span the entire solid. In metallic materials, this means that electrons are delocalized. A cation in a sea of electrons is a nice example of a metal solid.

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A crystalline solid is a homogenous material with a defined repeating pattern of constituent particles, atoms, ions, or molecules. Crystalline substances make up the majority of solids. A crystalline solid's particle arrangement maximizes the overall intermolecular attraction force. Melting points for crystalline solids are definite. Metals, ions, covalent networks, and molecular solids are all examples of crystalline solids.

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glass fish, fish glass

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Amorphous solids, which lack the three-dimensional long-range order of crystalline materials, have a more random arrangement of molecules, show short-range order across a few molecular dimensions, and have physical properties that are significantly different from those of their crystalline counterparts.

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A solid is a state of matter in which particles are organized in such a way that their shape and volume remain relatively constant. A solid's elements are packed much closer together.

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An ion-dipole force is a sort of intermolecular force that occurs when two ions, molecules, or atoms are attracted or repel each other. The attraction between a negatively or positively charged ion and the dipole molecule's oppositely charged end causes the ion-dipole force.

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London Dispersion Forces / Van Der Waals Forces

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London Dispersion Forces / Van Der Waals Forces

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Van der Waals forces are weak intermolecular forces that are depending on atom or molecule distance (dipole-dipole interactions also play a role on Van Der Waals).

Interactions among uncharged atoms/molecules produce these forces. The variation in the polarizations of two particles near to each other, for example, can cause Van der Waals forces. In non-polar molecules, the London dispersion force is a subtype of the Van der Waals force. A force that exists between two molecules is referred as an intermolecular force.

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Hydrogen bonding is the development of hydrogen bonds, which are a type of attractive intermolecular force resulting from the dipole-dipole interaction between a hydrogen atom bound to a strongly electronegative atom and another very electronegative atom nearby.

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Electrostatic forces between two permanently polar molecules are known as dipole-dipole interactions. In instance, one molecule's positive end attracts the negative end from another. The two molecules become nearer as a result, increasing the substance's stability.

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The attractive and repulsive forces that emerge between the molecules of a substance are known as intermolecular forces or IMFA for short. Individual molecules of a substance interact through these forces. Most of the physical and chemical properties of matter are determined by intermolecular forces.

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Boyle's Law, Charles' Law, and Gay-Law Lussac's have all been merged into the combined gas law. It asserts that the ratio of a gas's product of pressure and volume to its absolute temperature is constant.

P₁V₁ /T = P₂V₂/T

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The universal gas equation, or ideal gas law, is another name for the ideal gas law. It's a pressure-volume-quantity-temperature equation for an ideal gas. In many cases, the law imitates the behavior of real gases, even though it explains the behavior of a hypothetical gas.

PV = nRT

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(Volume - Temperature)

The volume of an ideal gas at constant pressure is precisely proportional to its absolute temperature, if the pressure stays the same.

V/T = constant V₁/T₁  = V₂/T₂

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(Volume -  Amount)

For a fixed temperature, raising the amount of gas pumped into the movable piston rises volume. It's also worth remembering that the pressure is kept consistent.

V/n = constant V₁/n₁  = V₂/n₂

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(Pressure - Temperature)

When the volume of a gas is held constant, the pressure of a given amount of gas directly correlates with its absolute temperature.

P/T = constant P₁/T₁ = P₂/T₂

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(Pressure - Volume)

A gas's volume fluctuates inversely with the applied pressure to it under constant temperature.

PV = constant P₁V₁ = P₂V₂

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The gas laws show how pressure, temperature, volume, and amount of gas are related.