list of physical properties of matter definition and examples pdf

List Of Physical Properties Of Matter Definition And Examples Pdf

File Name: list of physical properties of matter definition and examples .zip
Size: 29567Kb
Published: 15.12.2020

You can create printable tests and worksheets from these Grade 9 Properties of Matter questions!

1.3: Properties of Matter

Matter is the "stuff" that makes up the universe — everything that takes up space and has mass is matter. All matter is made up of atoms , which are in turn made up of protons, neutrons and electrons. Atoms come together to form molecules, which are the building blocks for all types of matter, according to Washington State University. Both atoms and molecules are held together by a form of potential energy called chemical energy.

Unlike kinetic energy , which is the energy of an object in motion, potential energy is the energy stored in an object. There are four natural states of matter: Solids, liquids, gases and plasma. The fifth state is the man-made Bose-Einstein condensates. In a solid , particles are packed tightly together so they don't move much. The electrons of each atom are constantly in motion, so the atoms have a small vibration, but they are fixed in their position. Because of this, particles in a solid have very low kinetic energy.

Solids have a definite shape, as well as mass and volume, and do not conform to the shape of the container in which they are placed. Solids also have a high density, meaning that the particles are tightly packed together. In a liquid , the particles are more loosely packed than in a solid and are able to flow around each other, giving the liquid an indefinite shape. Therefore, the liquid will conform to the shape of its container. Much like solids, liquids most of which have a lower density than solids are incredibly difficult to compress.

In a gas , the particles have a great deal of space between them and have high kinetic energy. A gas has no definite shape or volume. If unconfined, the particles of a gas will spread out indefinitely; if confined, the gas will expand to fill its container. When a gas is put under pressure by reducing the volume of the container, the space between particles is reduced and the gas is compressed.

Plasma is not a common state of matter here on Earth, but it may be the most common state of matter in the universe, according to the Jefferson Laboratory. Stars are essentially superheated balls of plasma. Plasma consists of highly charged particles with extremely high kinetic energy.

The noble gases helium, neon, argon, krypton, xenon and radon are often used to make glowing signs by using electricity to ionize them to the plasma state. At this extremely low temperature, molecular motion comes very close to stopping. Since there is almost no kinetic energy being transferred from one atom to another, the atoms begin to clump together. There are no longer thousands of separate atoms, just one "super atom. A BEC is used to study quantum mechanics on a macroscopic level.

A BEC also has many of the properties of a superfluid , or a fluid that flows without friction. BECs are also used to simulate conditions that might exist in black holes. Adding or removing energy from matter causes a physical change as matter moves from one state to another. For example, adding thermal energy heat to liquid water causes it to become steam or vapor a gas. And removing energy from liquid water causes it to become ice a solid.

Physical changes can also be caused by motion and pressure. When heat is applied to a solid, its particles begin to vibrate faster and move farther apart. When the substance reaches a certain combination of temperature and pressure, its melting point , the solid will begin to melt and turn into a liquid.

When two states of matter, such as solid and liquid, are at the equilibrium temperature and pressure, additional heat added into the system will not cause the overall temperature of the substance to increase until the entire sample reaches the same physical state.

For example, when you put ice into a glass of water and leave it out at room temperature, the ice and water will eventually come to the same temperature. As the ice melts from heat coming from the water, it will remain at zero degrees Celsius until the entire ice cube melts before continuing to warm.

When heat is removed from a liquid, its particles slow down and begin to settle in one location within the substance. When the substance reaches a cool enough temperature at a certain pressure, the freezing point, the liquid becomes a solid. Most liquids contract as they freeze. Water, however, expands when it freezes into ice, causing the molecules to push farther apart and decrease the density, which is why ice floats on top of water.

Adding additional substances, such as salt in water, can alter both the melting and freezing points. For example, adding salt to snow will decrease the temperature that water freezes on roads, making it safer for drivers.

There is also a point, known as the triple point , where solids, liquids and gases all exist simultaneously. Water, for example, exists in all three states at a temperature of When a solid is converted directly into a gas without going through a liquid phase, the process is known as sublimation.

This may occur either when the temperature of the sample is rapidly increased beyond the boiling point flash vaporization or when a substance is "freeze-dried" by cooling it under vacuum conditions so that the water in the substance undergoes sublimation and is removed from the sample. A few volatile substances will undergo sublimation at room temperature and pressure , such as frozen carbon dioxide, or dry ice.

Vaporization is the conversion of a liquid to a gas and can occur through either evaporation or boiling. Because the particles of a liquid are in constant motion, they frequently collide with each other. Each collision also causes energy to be transferred, and when enough energy is transferred to particles near the surface they may be knocked completely away from the sample as free gas particles.

Liquids cool as they evaporate because the energy transferred to surface molecules, which causes their escape, gets carried away with them. Liquid boils when enough heat is added to a liquid to cause vapor bubbles to form below the surface. This boiling point is the temperature and pressure at which a liquid becomes a gas. Condensation occurs when a gas loses energy and comes together to form a liquid. For example, water vapor condenses into liquid water.

Deposition occurs when a gas transforms directly into a solid, without going through the liquid phase. Water vapor becomes ice or frost when the air touching a solid, such as a blade of grass, is cooler than the rest of the air.

Live Science. Please deactivate your ad blocker in order to see our subscription offer.

Chemical property

A chemical property is any of a material's properties that becomes evident during, or after, a chemical reaction ; that is, any quality that can be established only by changing a substance's chemical identity. When a substance goes under a chemical reaction, the properties will change drastically, resulting in chemical change. However, a catalytic property would also be a chemical property. Chemical properties can be contrasted with physical properties , which can be discerned without changing the substance's structure. However, for many properties within the scope of physical chemistry , and other disciplines at the boundary between chemistry and physics , the distinction may be a matter of researcher's perspective. Material properties , both physical and chemical, can be viewed as supervenient ; i. Several layers of superveniency [ clarification needed ] are possible.

chemical changes are different. Physical. Properties. Chemical. Properties section ○ Properties of Matter. 2 This is an example of using the physical.

Matter: Definition & the Five States of Matter

Matter is the "stuff" that makes up the universe — everything that takes up space and has mass is matter. All matter is made up of atoms , which are in turn made up of protons, neutrons and electrons. Atoms come together to form molecules, which are the building blocks for all types of matter, according to Washington State University. Both atoms and molecules are held together by a form of potential energy called chemical energy.

Matter , material substance that constitutes the observable universe and, together with energy, forms the basis of all objective phenomena.

Properties of matter can be classified as either extensive or intensive and as either physical or chemical. All properties of matter are either extensive or intensive and either physical or chemical. Extensive properties, such as mass and volume, depend on the amount of matter that is being measured. Intensive properties, such as density and color, do not depend on the amount of matter.

A subscription to J o VE is required to view this content. You will only be able to see the first 20 seconds. We recommend downloading the newest version of Flash here, but we support all versions 10 and above. If that doesn't help, please let us know.

Мы признаем, что у нас есть ТРАНСТЕКСТ, а Танкадо вручает нам шифр-убийцу. Мы вводим ключ и спасаем банк данных. Добро пожаловать, цифровой вымогатель. Фонтейн даже глазом не повел.



Body language for management pdf building html5 games with impactjs pdf



Istqb study material 2012 pdf foundation level nora roberts happily ever after pdf free download


Fredeswinda M.

Graphic anatomy atelier bow wow pdf free download constition of india pdf


Fiacre S.

GRADE 11 CHEMISTRY • Topic 1: Physical Properties of Matter most common three states of matter: gases, liquids, and solids. The fourth state, examples of such materials (e.g., peanut butter, candle wax, cotton candy, glass, rubber PASPort Explorations in Chemistry Lab Manual (PASCO Scientific)—Available.


Leave a comment

it’s easy to post a comment

You may use these HTML tags and attributes: <a href="" title=""> <abbr title=""> <acronym title=""> <b> <blockquote cite=""> <cite> <code> <del datetime=""> <em> <i> <q cite=""> <strike> <strong>