volume

Solution: The space occupied by an object is called its volume.

Matter is anything that has mass and takes up space. If something is in a solid state of matter, it has a definite shape and volume. The volume of an object is the amount of space it occupies.

Mass is a measure of the amount of matter in a substance or an object. The basic SI unit for mass is the kilogram (kg), but smaller masses may be measured in grams (g). To measure mass, you would use a balance.

The two most common properties are intermolecular forces and density. Explanation: Anything that has mass and volume and can occupy space is known as matter. The composition of matter shows that it has small particles.

All properties of matter are either physical or chemical properties and physical properties are either intensive or extensive. Extensive properties, such as mass and volume, depend on the amount of matter being measured. Physical properties can be measured without changing a substance’s chemical identity.

The properties of matter include any traits that can be measured, such as an object’s density, color, mass, volume, length, malleability, melting point, hardness, odor, temperature, and more.

Physical Properties

• color (intensive)
• density (intensive)
• volume (extensive)
• mass (extensive)
• boiling point (intensive): the temperature at which a substance boils.
• melting point (intensive): the temperature at which a substance melts.

Matter can be defined or described as anything that takes up space, and it is composed of miniscule particles called atoms. It must display the two properties of mass and volume.

Physical properties include: appearance, texture, color, odor, melting point, boiling point, density, solubility, polarity, and many others.

The three basic properties of matter are volume, mass, and shape. 2. All matter is made up of tiny particles called atoms.

An extensive property is a property that depends on the amount of matter in a sample. Mass and volume are examples of extensive properties. Color, temperature, and solubility are examples of intensive properties.

Heat is an example of an extensive property, and temperature is an example of an intensive property.

Pressure is indeed an intensive property because it is force divided by an extensive quantity (area).

The two values are essentially the same so we know that density is a ratio between mass and volume. Density is an intensive property of matter that illustrates how much mass a substance has in a given amount of volume.

List of Properties

Meanwhile, area is also an extensive property (as it depends on the size of the system). So P = F/A. = extensive/extensive = intensive. [1] though the case of an ideal gas may be an oversimplification.

Work has the units of Energy and is often thought of as the process of converting energy from one form to another. Work is the product of Force (which is intensive) times distance (which is extensive). There are several distinct forms of ‘energy’ that are treated in thermodynamics.

An intensive property, is a physical property of a system that does not depend on the system size or the amount of material in the system. According to the definitions, density, pressure and temperature are intensive porperties and volume, internal energy are extensive properties.

An intensive property is a property of matter that depends only on the type of matter in a sample and not on the amount. Color, temperature, and solubility are examples of intensive properties.

Volume is not an intensive property as it depends on the amount of substance.

Here, volume depends on the quantity of matter. Therefore, volume is not an intensive property.

Intensive properties: Properties which are independent of the amount of substance (or substances) present in the system are called intensive properties, e.g. pressure, density, temperature, viscosity, surface tension, refractive index, emf, chemical potential, sp. heat etc, These are intensive properties.

Thus, freezing point is an intensive property and doesn’t change when we vary amount. Other examples of intensive properties are color, boiling point, pressure, molecular weight and density.

Intensive properties do not depend on the amount of substance. For example water boils at the same temperature no matter how much water you have. Other examples of intensive properties include density , solubility, color, luster, freezing point and malleability. Here is a list of intensive properties.

Examples of extensive properties include:

• amount of substance, n.
• energy, E.
• enthalpy, H.
• entropy, S.
• Gibbs energy, G.
• heat capacity, C. p
• Helmholtz energy, A or F.
• internal energy, U.

They can be such things as color, texture, shape, size, mass, volume, etc. When you talk about intensive properties it means physical properties that do not depend on the amount of matter in the object. Some examples of intensive properties are: density, boiling point, and freezing point, etc.

Physical matter properties include color, odor, density, melting point, boiling point and hardness. Intensive properties are used to identify a substance and do not depend upon the amount of substance (density).

Intensive properties mean that it doesn’t change when you add more to it . Some intensive properties are….. texture, flexibility, luster, density, conductivity, magnetism, odor, hardness, and taste.

Summary: Prolonged exposure to low-level magnetic fields, similar to those emitted by such common household devices as blow dryers, electric blankets and razors, can damage brain cell DNA, according to researchers in the University of Washington’s Department of Bioengineering.

The amount of space that matter occupies is called its volume. Solids, liquids, and gases all have volume.

Volume is a measure of the amount of space that a substance or an object occupies. The basic SI unit for volume is the cubic meter (m3 ), but smaller volumes may be measured in cm3, and liquids may be measured in liters (L) or milliliters (ml). The volume of matter is measured depending upon its state.

Volume is the quantity of three-dimensional space occupied by a liquid, solid, or gas. Common units used to express volume include liters, cubic meters, gallons, milliliters, teaspoons, and ounces, though many other units exist.

If something is in a solid state of matter, it has a definite shape and volume. The volume of an object is the amount of space it occupies. A block of wood placed on a table retains its shape and volume, therefore, it is an example of a solid. If a liquid is poured on that same table, there are very different results.

A solid has definite volume and shape, a liquid has a definite volume but no definite shape, and a gas has neither a definite volume nor shape.

A solid has a definite shape and a definite volume. The particles that make up a solid are packed very closely together. Each particle is tightly fixed in one position and can only vibrate in place.

Solid is the state in which matter maintains a fixed volume and shape; liquid is the state in which matter adapts to the shape of its container but varies only slightly in volume; and gas is the state in which matter expands to occupy the volume and shape of its container.

• Bose–Einstein condensate.
• Fermionic condensate.
• Degenerate matter.
• Quantum Hall.
• Rydberg matter.
• Rydberg polaron.
• Strange matter.
• Superfluid.

We can see that matter around us exists in three different states– solid, liquid and gas. These states of matter arise due to the variation in the characteristics of the particles of matter.

Solids, liquids and gases are different mainly because of their lattice arrangements and the cohesive forces between the molecules. The cohesive forces between their molecules are also very weak. This gives gases their property to flow and compressibility.

Liquids flow because the intermolecular forces between molecules are weak enough to allow the molecules to move around relative to one another. In liquids, the intermolecular forces can shift between molecules and allow them to move past one another and flow.

Gases, liquids and solids are all made up of atoms, molecules, and/or ions, but the behaviors of these particles differ in the three phases. gas are well separated with no regular arrangement. liquid are close together with no regular arrangement. solid are tightly packed, usually in a regular pattern.

Under some circumstances, the solid phase can transition directly to the gas phase without going through a liquid phase, and a gas can directly become a solid. The solid-to-gas change is called sublimation, while the reverse process is called deposition. Sublimation is isothermal, like the other phase changes.

Solids, liquids and gases are known as states of matter.

There are three common states of matter:

• Solids – relatively rigid, definite volume and shape. In a solid, the atoms and molecules are attached to each other.
• Liquids – definite volume but able to change shape by flowing. In a liquid, the atoms and molecules are loosely bonded.
• Gases – no definite volume or shape.

All liquids show the following characteristics:

• Liquids are almost incompressible. In liquids molecules are pretty close to each other.
• Liquids have fixed volume but no fixed shape.
• Liquids flow from higher to lower level.
• Liquids have their boiling points above room temperature, under normal conditions.

The most obvious physical properties of a liquid are its retention of volume and its conformation to the shape of its container. When a liquid substance is poured into a vessel, it takes the shape of the vessel, and, as long as the substance stays in the liquid state, it will remain inside the vessel.

Terms in this set (14)

• List the Six Properties of Water. cohesion, adhesion, high specific heat, evaporative cooling, lower density as solid, universal solvent.
• Mnemonic. (CAHELU)
• cohesion (meaning)
• cohesion (benefit)
• adhesion (meaning)
• adhesion (benefit)
• high specific heat (meaning)
• high specific heat (benefit)

‘ The dissolving power of water is very important for life on Earth. Wherever water goes, it carries dissolved chemicals, minerals, and nutrients that are used to support living things. Because of their polarity, water molecules are strongly attracted to one another, which gives water a high surface tension.

Water has the unique ability to dissolve many polar and ionic substances. This is important to all living things because, as water travels through the water cycle, it takes many valuable nutrients along with it! Water has high heat capacity.

Hydrogen Bonding. Hydrogen bonding is a special type of dipole-dipole attraction between molecules, not a covalent bond to a hydrogen atom. It results from the attractive force between a hydrogen atom covalently bonded to a very electronegative atom such as a N, O, or F atom and another very electronegative atom.

The boiling points of NH3, H2O, and HF are abnormally high compared with the rest of the hydrides in their respective periods.” is the strongest evidence for hydrogen bonding.

If there is a lone pair of electrons belonging to nitrogen, oxygen, or fluorine, then it is possible to bond to water. Therefore, it is can accept a hydrogen.

Dipole-dipole interactions