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Mass and Weight: Definition, Conversion, and Chart
Continue ReadingMass and Weight
Mass is the one of the most significant fundamental quantity of an object in physics and is one the basic property of matter thus is defined as the measure of the amount of matter that is present in a body or substance.
The SI (international system of units) unit of mass is kilograms(kg). The mass of a body does not change it only changes when a huge amount of energy is given or taken from the body for instance in nuclear reaction a huge amount of energy is produced from a certain amount of matter and this lessens the mass of the matter.
The more mass an object has the more force it takes for it to get moving. The symbol of mass is m or M. Various physical quantities like Force, Inertia, and Relative theory of Einstein’s also depend upon mass.
E = mc2
There are various ways of determining the quantity of mass the most used are inertial mass and gravitational mass.
Inertial Mass
It is defined as the mass which is determined by how much an object could resist to acceleration. For instance, if we push two objects with the same amount of force and under the same conditions then object which have lower mass will accelerate faster than the object with the heavy mass.
Gravitational Mass
Gravitational mass is defined as the measurement of how much gravity an object employs on other objects or measurement of how much gravity an object experiences from other objects.
Centre of Mass
Centre of mass of a body can be defined as a point where all the mass of the object is concentrated.
Atomic Mass Unit
The atomic mass unit is used is used to measure the mass of atoms and molecules which are so small, that the kilograms is not so appropriate to use for measurement. One atomic mass unit can be defined as 1/12 the mass of a carbon: 12 atoms.
The value of 1 atomic mass is 1.66 x 10-27..
Mass Conservation
Mass Conservation means that the mass of reactants in the reaction is always equal to the mass of its products.
For Example; An example of law of conservation of mass is coal, the carbon atom in coal becomes carbon dioxide when it is burned or ignited. Thus, carbon atom changes from a solid structure to a gas but the mass of the substance does not change.
Characteristics of Mass
• Mass cannot be zero as everything around us has some mass.
• Mass is measured in grams, kilograms, or milligrams.
• Mass is a scalar quantity which means it only has magnitude.
Weight
Weight is defined as the measure of the force of gravity acting on an object.
S.I unit of weight is Newtons(N). Weight is the measure of the acceleration of gravity
W = mg
In the above expression g is the gravitational field which is equal to 9.8 and/kg and m is denoted as mass.
Characteristics of Weight
• Weight can be measured by via a spring balance.
• Weight can be zero.
• Weight is a vector quantity. Thus, it has both direction and magnitude
Difference Between Mass and Weight
Mass Weight Mass is a scalar quantity which means it only has magnitude Weight is a vector quantity which means it has both magnitude and direction Mass is measured in kilogram, gram, and milligrams Weight is measured in Newtons (N) Mass can never be zero Weight can be zero Mass is not dependent on the gravity and is same everywhere Weight is a physical property that is dependent on gravity and it vary from place to place Mass can be measured with the help of several instruments such as beam balance etc. Weight can be measured with the help of spring balance Relation Between Mass and Weight
The weight of the body can be defined as the force exerted by the earth or any other celestial object on other object.
In case of earth when a body falls towards the earth, the force of gravitation pulls the object with an acceleration denoted as`g`.
According to Newton’s second law, the force of attraction on the body of mass m is F=Mass x Acceleration due to gravity = mg This is force on the object and it is called weight. Thus, W=mg
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Metric System: Definition, Conversion, and Chart
Continue ReadingMetric System
The metric system of measurement is the most standard way of measuring distance, height and is also used for calculating many more day-to-day activities.
For instance, Gauri drinks 10 ml of water.
This metric system is used in various fields such as that of science, medicine and so on. Each object is measured according to its length, volume, weight, and time in various manner. This concept of metric system was introduced with the above-mentioned measurements only.
The three main basic units of metric system are;
Metre, a unit use to calculate length of an object.
Kilograms, a unit which is used to measure mass of an object.
Second, a unit of time.
Origin of Metric System
Medication is defined as a process that implements the international system of units called as SI unit. Metric system is followed by nearly all countries except United States, Myanmar, and Liberia.
The United States further introduced its own system of units or system of metric units which is now called as United States customary units.
Difference Between USCS and SI Units
The United States metric units are also called as “imperial units.” The key difference between the SI units and the American metric units is the terms and the form of units used. For instance, In SI unit, the length is measured using the metre whereas In USCS foot is used for measurement.
Metric System Units
Metric unitsGiven below are some of the most used metric units;
Length
This unit length is used for measuring the size of an object or the distance that an object travels from one end to the other end.
There are different units of length which are metre, kilometers, feet etc. The most common tool which is used to measure length is called a ruler.
For Example; The height of this blackboard is about 3 metres.
Smallest unit of measuring length is millimeter and the largest unit is kilometers
1 kilometer = 1000 metre
1 inch =2.5 centimeter
Weight
Weight is the unit that is use to measure the mass of an object. The standard unit that is used for the measurement of mass is kilogram, gram ton etc.
The most common tool which is used to measure the weight of an object is the weighing scale.
For instance; the weight of this bottle is 250 grams.
1 kilogram =1000 gram
Capacity
Capacity is the unit which is used to measure the volume or space occupied by an object or matter. The standard unit used for measurement of capacity is litre. Other units used for measurement of capacity are milliliter etc.
For example; 500 liters of milk
1 litre = 1000 ml
1 cup=250 ml
Time
The standard unit for measurement of time is seconds. Other metric units of time are minutes, hours etc.
1 minute = 60 seconds
1 hour= 60 minutes
1 day = 24 hours
1 week = 7 days
Some few common units based-on metre, kilograms and seconds are;
Speed: Speed is defined as a distance travelled divided by total time taken by an object.
SI unit of speed is metre /second or m/s.
Acceleration: Acceleration is defined as the changes in velocity.
When a runner accelerates from 10 m/s (10 meter per second) to 11 m/s (11 meters per second) in just one second, thus they accelerate by 1 meter per second per second.
SI unit of acceleration is m/s2
Advantages of Metric System
• The metric system allows us to alter the units by changing the decimal to a new place value.
• Metric system is used for easy calculations as metric units generally increase or decrease in a multiple of 10.
For example; there are 1000 grams in 1 kg so one gram is equal to 1/1000 kilogram.
• Nearly all countries use this metric system.
• It has standardized prefix such as gram, kilogram milligram etc.
• Scientists who work in diverse countries need this standardized system that permits them to compare notes and comprehend one another. Without a standard system, they would waste their precious time on converting measurements from one system of measurement to another, and thus accuracy level would also suffer. SI is the most favored system because, among other reasons, it isn’t built on the body parts of society who lived periods ago.
• It’s a well-designed and simple system built on a universal standard that can be confirmed by anyone.
Disadvantages of Metric System
The only drawback in using this metric system is that it is not very well suitable if we work in fractions.
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Heterogeneous Mixtures: Examples, Definition, and Types
Continue ReadingHeterogeneous Mixtures Introduction
Anything which has mass and occupies space is called matter. Matter can be divided into;
1. Pure Substances
2. Mixture
Pure substances are made up of only one form of atoms or molecules which cannot be broken down into simpler substances by simple physical method. Element and Compound are examples of pure substances.
Mixtures are made up of two or more substances which are the constituents of mixture. The constituents of mixture can be in any ratio.
Mixtures can be divided into:
1. Homogeneous mixtures
2. Heterogeneous mixtures
Homogeneous mixtures have uniform composition. For instance, sugar in water, water in alcohol etc.
What are Heterogeneous Mixtures?
Heterogeneous mixtures are defined as the mixture where components are mixed non-uniformly. Irrespective of homogeneous mixture where components are in single phase, in heterogeneous mixture components are present in at least two different phases.
Properties of Heterogeneous Mixtures
Heterogeneous mixture shows the following properties:
• It contains two or more ingredients or phases. This phase can be solids, liquids, or gases.
• All the constituents hold their individual properties or chemical identity.
• Constituents displays variable composition.
• The components of mixture can be separated by physical methods.
• There is usually no energy change when mixture is formed.
• There is no change in volume in forming mixture at constant temperature and pressure.
• We cannot transcribe the formula for heterogeneous mixture.
Classification of Heterogeneous Mixture
We can broadly classify heterogeneous mixture into two types:
1. Suspensions
2. Colloids
1. Suspensions
In this type of mixture solute particles do not dissolve, but remain suspended throughout the medium.
Properties of Suspension
1. The particles of a suspension are big and can be seen with a naked eye.
2. As the particles size is pretty big, they throw a beam of light and make the track of light visible, this effect is called The Tyndall effect.
3. As solute particles are quite big, they also settle down when the mixture is left uninterrupted so it can be said that suspension is unstable.
4. The elements of the suspension can be separated by a method of filtration.
Examples of Suspension
1. Kerosene oil and water are the two liquids that do not combine with each other; thus, these types of liquid are called immiscible liquids.
2. Muddy water is also an example of suspension where sand particles are suspended in the liquid water.
3. Common salt in benzene.
4. Wheat flour in water.
5. Concrete is a combination of cement, gravel, sand, and water thus it is an example of suspension.
6. A tossed salad
7. Ice cubes in soda. Before opening it appears to be homogeneous but once heaviness is released, we see the bubbles of gas and liquid.
8. Smoke, an example of suspension in which dust particles, gases, carbon particles are present in different ratios.
Colloids
Colloids are another type of mixtures where the size of particles is between 1nm and 1000nm. Colloids is defined as a mixture where one of the substances is divided into very minute particles which are distributed throughout a second substance. These tiny particles are recognized as colloidal particles.
Properties of Colloids
1. Collides are heterogeneous mixture.
2. When light is conceded through a true solution, the dissolved atoms are too small to deflect the light. But, the dispersed particles of a colloid, being bigger, do deflect light. Thus, The Tyndall effect is the scattering of visible light by colloidal particles.
3. Particles of colloids do not settle at bottom when we left the mixture uninterrupted.
4. Colloids cannot be filtered.
5. The two components of colloidal solution are given below;
i. The dispersed phase: The dispersed particles in a colloid form.
ii.The dispersing mediums: The component in which particles are suspended which are solid, liquid or gas.
Types of Colloids
The dispersion mediums are of three form gas, solid and liquid state. Similarly dispersed phase can be of three types. Based on these two we divide colloid in eight types:
1. Solid sol
2. Solid foam
3. Solid aerosol
4. Sol
5. Gel
6. Emulsion
7. Aerosol
8. Foam
Colloids Dispersing Medium Dispersed Phase Types Clouds, fog, mist, smoke, automobile exhaust Gas Liquid Solid Aerosol Aerosol Shaving cream, face cream, blood, paint, writing ink, mud, milk of magnesia Liquid Gas Liquid Solid Foam Emulsion Sol Rubber, foam, sponge, pumice, jelly, butter, cheese, colored gemstone Solid Gas Liquid Solid Foam Gel Sol Based on nature of the different interactions between the dispersion phase and dispersed phase:
1. Lyophilic If there is an affinity between dispersed medium and phase then these sols are called lyophilic.
For Example: starch, rubber, protein, etc.
2. Lyophobic If there is no affinity between the two phases then these form an unstable colloid.
Examples: sols of metals like gold and silver, sols of metallic hydroxides.
Methods of Separation of Components of Suspensions and Colloids
1. Filtration that is done with the help of filter paper
2. Separating funnel for immiscible liquids such as in oil and water
3. Sedimentation and decantation
4. Centrifugation where mixtures are rotated at a very high speed so that the lighter particles are detached from mixture for example: cream from milk.
Test Used to Identify; Suspensions and Colloids
1. A colloid solution is translucent or turbid in nature and if salt is added to this solution, then this can settle at bottom.
2. If the particles settled at bottom is left uninterrupted for some time then it is a suspension.
Use of a Colloid and a Suspension in Our Daily Life
Colloids are used in pharmaceuticals some insoluble materials become more active when taken in colloidal form.
Suspensions: Barium sulphate when dispersed in water form an opaque suspension which is used in diagnostic X-rays.
Heterogeneous Mixtures Citations
- A density-based threshold model for evaluating the separation of particles in heterogeneous mixtures with curvilinear microfluidic channels. Scientific Reports volume 10, Article number: 18984 (2020).
- The electrical properties of heterogeneous mixtures containing an oriented spheroidal dispersed phase. Colloid and Polymer Science volume 263, pages51–57 (1985).
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Chemical Property Examples
Continue ReadingChemical Property, Physical Property, and Chemical Property Examples
Anything which occupies space and has someone is called matter.
All the substances that we see around us has some properties and these substances can be classified into two properties which are; Physical Properties and Chemical Properties
Physical properties are defined as a characteristic of a substance that is observed without changing the identity of a substance or its molecular formula.
For instance; appearance, odour, texture, boiling and melting points etc.
Chemical property on the other hand is the characteristic of a substance that describes its ability to undergo a specific chemical change.
Chemical Property Examples
Chemical properties that only be established when a substance transforms or changes into a new substance due to the chemical reactions, unlike physical properties which can only be observed by touching or seeing a sample.
Some of chemical property examples are the following;
(a) Flammability
Flammability is defined as the ability of a chemical substance to burn causing fire or combustion.
It is a chemical property because it can only be observed during a chemical change.
Usually, materials categorized are as highly flammable, flammable and non-flammable.
Understanding this chemical property can help us in in handling, storing, and transporting highly flammable materials.
For example; Wood is a flammable substance. Diamond is non-flammable.
(b) Radioactivity
In simple terms radioactivity is defined as the act of emitting radiation from an atom with unstable atomic nucleus spontaneously.
The most common forms of radiation emitted are classified as alpha radiation, beta radiation and gamma radiation.
Some of the most common radioactive elements include Uranium, Radium, Actinium etc.
There is total 38 radioactive elements present in nature.
(c) Chemical Stability
This chemical property is also called as thermodynamics stability of a chemical system.
Chemical stability refers to the stability that takes place when a chemical system is present its lowermost energy state which is a state of chemical equilibrium, or balance, with the environment.
(d) Half life
Half-Life is another chemical property which is defined as the amount of time taken by a substance for one half of its life to decay.
(e) Ability to Oxidize
It is a chemical property that results in the change of oxidation number of a substance either by gaining oxygen or losing hydrogen.
Example of the oxidation encompasses the way an Apple turns into brown colour after it has been cut.
Another example that can be considered for this property is rust, iron and steel will rust over time however they will rust more quickly if they are being combined with the pure oxygen.
(f) Toxicity
Toxicity is the chemical property which is measured by the damage it causes to the organism, plants, and animal.
For instance, chlorine gas, mercury etc.
Lead which is a toxic substance damage various parts of human body which includes bones, kidney, intestine, and reproductive system.
Toxicity is a very vital chemical property because it tells us about the damage a substance can bring to other organisms.
Some common toxic materials include mercury and numerous types of acids.
This also contains the household products, such as those comprising of ammonia.
(g) Heat of Combustion
Heat of combustion is defined as the amount of energy or heat released when a substance is burned with oxygen.
Example for the same include, amount of heat that is produced by burning of several fuels.
A basic example includes the combustion of methane, CH4, with oxygen. Metals also undertake combustion.
(h) Reactivity
Reactivity is defined as the ability of a matter that reacts chemically with other elements. For example, potassium is very reactive metal, on the other hand noble gases such as helium never react with any other substances.
(i) Acidity
Acidity is a chemical property which refers to a substance at ability to react with the acid. Some metals form compounds when they react with diverse acids. Acids react with bases to form water, which further neutralizes the acid.
(j) Enthalpy of Formation
• When a substance is shaped by standard elements, heat is either released or captivated. The heat connected with this is what we call the standard enthalpy of formation.
This is a significant characteristic because it tells us about the stability of the given compound, as well as its reactivity with further compounds.
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Chemical Property: Definition, Examples, and Meaning
Continue ReadingChemical Property Introduction
Anything which has mass in occupy space is called matter. Everything is around us is matter. A matter can be divided into two categories depending on the characteristics of a substance.
The properties of a substance are generally grouped into two categories which are Physical Properties and Chemical Properties.
Physical properties are defined as a characteristic of a substance which can be observed or measured without changing the composition of its matter. Further physical properties are classified into intensive and extensive property.
What is Chemical Property?
Chemical property refers to the characteristic of substance that undergoes change in its chemical structure. In simple terms, this property describes the ability of a substance to undergo a definite chemical change.
These properties are different from physical properties as chemical property can’t be observed by touching or seeing a substance.
On the other hand, Chemical Properties can only be distinguished when a material is in the process of being transformed into another substance.
For Example; Chemical property of iron is its ability to combine with oxygen to form iron oxide whose chemical name is rust.
Metals generally have a chemical property of reacting with acids. Hydrogen gas is produced when zinc reacts with hydrochloric acid and oxygen, this is also a chemical property.
Chemical Property Examples
Some of the common chemical properties include;
Heat of combustion: Heat of combustion is the heat released during the conversion process under standard conditions.
For example, combustion of methane with oxygen.
Toxicity: Toxicity is defined as the damage caused by the substance to animals, plants, and other organisms.
For instance, LED can damage the various parts of human body as it is a toxic substance and it can also damage heart, kidneys, and intestines.
Other examples of chemical properties include acidity, reactivity, flammability (Wood is an instance of flammable matter), oxidation states, type of chemical bonds etc.
Characteristics of Chemical Property
● Chemical properties are observed or measured when a system undergoes a chemical reaction or chemical change.
● Chemical properties are directly linked to the chemical bonds of the substance.
● This property is used to predict how the substances will react in different medium.
● The structure of a material changes entirely in chemical properties.
Chemical Property Uses
● Chemical properties of a substance are used to classify compounds and help us find their applications.
● Scientist also use these chemical properties to determine whether the given sample will participate chemical reaction or not.
● Chemical properties of a substance help us in its purification, separation from other chemical substances.
● Chemical properties unlike physical property are a characteristic that can only be observed when a given substance is being changed into different substance as a result of a chemical reaction or chemical change.
Chemical Change
● Chemical change is also known as a chemical reaction.
● In order to to identify a chemical property we must look for a chemical change.
● Chemical change results in one or more substances of totally different compositions from the original substances. Thus, it means that different elements or compounds are present at the termination of a chemical reaction.
● Reactants are the ingredients of a reaction and products are their result.
Reactants → Products
For instance, when an iron is exposed to water it becomes a mixture of hydrated iron oxides and hydroxides.
● Some examples of chemical changes include lightning of fireworks as fireworks consists of some metal nitrides and other chemicals constituting to burning compounds.
● Thus, when we let a firework combustion take place then this leads to formation of new substance and the release of light and heat thus, it is considered as a chemical change, The explosion of nitroglycerine is also a chemical change because the gases which are produced are of different kind from the novel substance.
● Burning, cooking, and rusting are all kinds of chemical changes because they produce new substances.
● Chemical changes are very vital in our lives. All new substances are shaped as a result of chemical changes such as digestion of food in our body, ageing of fruits, fermentation of grapes, etc., happen due to the result of chemical changes.
● Useful new materials, for example plastics and detergents, are produced as a result of chemical reactions/changes. Certainly, every new material is discovered by reviewing chemical changes of that particular substance.
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Physical Property: Definition, Examples, and Meaning
Continue ReadingPhysical Property Definition
Changes can be categorized into physical and chemical. Matter is made up of tiny particles and has both physical and chemical properties.
A chemical property is defined as the characteristic of a substance that can be observed in a chemical reaction.
For example heat of combustion, toxicity, acidity, reactivity etc.
Physical Property is defined as the characteristic of a substance that can be observed without changing the chemical nature of the substance such as its size, state of matter, colour, mass, density etc.
Some other physical properties include solubility, melting and boiling points etc.
The physical property of matter also includes Mellability which occurs when metal is moulded into thin sheets, for instance, silver is shiny metal and it can be moulded into thin sheets.
Hardness which is another physical property helps to determine how the element can be used.
Carbon in diamond is very hard whereas carbon in graphite is very soft.
Melting and boiling point is the physical property that is unique identifiers, especially of compounds.
Following are the most common physical properties that are used in selecting materials or substances Density implies the weight of the substance. Density is defined as mass divide by volume.
Melting point is defined as the minimum temperature required for the solid material to change into a liquid.
Colour is the reflective property of a material Boiling point is defined as the minimum temperature required for a liquid to change into a gas.
Physical Property Classification
There are two classes of physical properties which are
1. Extensive Physical Property
2. Intensive Physical Property
1. Extensive Physical Property
Extensive properties are those properties that depend on the size of the sample. Shape, volume and mass are extensive properties.
The properties like length,mass weight and volume that not only depend on the size but also depend on the quantity of the matter.
For instance, if we have two boxes made up of the same material one has the capacity of 6 litres and the other has the capacity of 12 litres then the box with 12-litre capacity will have more amount of matter as compared to that of 6-litre box.
2. Intensive Physical Property
Intensive properties are those properties that do not depend on the size or amount of matter in the sample.
Temperature, pressure and density is some of the examples of intensive properties other examples include colour, melting and boiling points as they will not change with the change in size as well as quantity of matter. The density of 1 litre of water or 1000 litre of water will remain the same as it is an intensive property.
Physical Change
Physical change takes place without any changes in the molecular composition of the substance. The same molecule is present in the substance throughout the changes.
Physical changes are related to the physical properties of a substance which are solid liquid and gas. During physical change the composition and the chemical nature of matter are not changed chemical property is not affected by the physical change of a substance.
The physical change includes a change in colour, solubility,change in the state of matter etc. Examples of physical change include melting an ice cube, dissolving sugar and water. Boiling water is also an example of physical change because the water vapour has the same molecular formula as that of liquid water.
To identify a physical change we have to look for a phase change for example if we freeze water into solid ice we can still melt the water again.
Physical Property Uses
Physical property is used to determine the appearance, texture, colour etc. of a substance thus, these physical properties are important as they help us to differentiate between different compounds.
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Homogeneous Mixtures: Examples, Definition, and Types
Continue ReadingHomogeneous Mixtures: Introduction
When 2 or more substances are mixed in any proportion, then this combination is defined as a mixture. Mixtures can be separated by physical methods such as evaporation, distillation, etc.
For example; salt and water, where 2 different components are mixed to form a mixture.
Mixtures can further be classified into homogenous and heterogeneous mixtures.
A Homogenous mixture is defined as the mixture where the composition is the same that is components are mixed uniformly.
Example; sugar and water.
A heterogeneous mixture is defined as the mixture where components are mixed non-uniformly, thus form 2 separate layers.
For example; soil and water are 2 different components that do not mix and thus form a layer and can be seen through a naked eye.
Homogeneous Mixtures
Homogeneous is derived from two words ‘homo’ meaning the same and geneos meaning ‘group/type’. Thus homogeneous means having the same or uniform composition.
A solution is a homogeneous mixture for example lemonade is a solution of lemon and water. The components of the solution are solute and solvent. The solute is dissolved in a solvent that is present in a larger quantity.
For example; a solution of sugar in water where sugar is the solutes taken in small quantity and water is the solvent taken in larger amounts.
Characteristics of Homogeneous Mixtures
The homogenous mixture/solution has only one phase that is solid, liquid and gas. Examples for the same are;
Solid homogeneous mixture: brass is an alloy that is made from metal copper (Cu) and zinc (Zn).
Liquid homogeneous mixture: a saline solution that is the mixture of water and salt.
Gas homogenous mixture: air is a mixture of different gases such as oxygen, carbon dioxide, nitrogen, and many more gases present in smaller amounts in the environment.
The size of particles of the solution is smaller than one nanometer thus homogenous mixtures do not show the Tyndall effect and cannot be seen with the naked eye.
The solute particles do not settle down when left uninterrupted, thus, a solution is stable.
Homogeneous Mixtures Examples
1. Salt and water.
2. Alcohol and water.
3. Steel is an alloy made from copper and iron.
4. Bronze is an alloy which is a mixture of copper and tin.
5. Natural gas is a mixture of methane and other gases.
Types of Solutions
Dependent upon the dissolution of the solute in the solvents, solutions can be categorized into the following;
A supersaturated solution comprises a large amount of solute that can be dissolved by the solvent where the extra solute will crystallize quickly at a particular temperature. The most prevalent example is sodium acetate which is a supersaturated solution.
An unsaturated solution is a solution in which a solvent can dissolve any more solute at a given temperature.
A saturated solution can be defined as a solution in which a solvent is not capable of dissolving any further solute at a given temperature thus it means that the maximum amount of solute has been dissolved and further no more solutes can be dissolved in the given solvent.
Factors Affecting Solubility
The quantity of solute that can be dissolved in a solvent to form a saturated solution depends following factors given;
Temperature: Solubility is directly proportional to temperature thus it increases with temperature. For example, we can dissolve much more salt in hot water as compared to cold water.
Pressure: Increasing pressure can vigor more solute into solution. This is usually use to dissolve gases into liquids.
Chemical Composition: The nature of the solute and solvent and the existence of other chemicals in a solution affects its solubility. For example, we can dissolve much more sugar in water as compared to salt.
Solution Form
The solutions are of two forms, depending on the solvent if its water or not.
Aqueous solution: When a solute is dissolved in water then this type solution is called an aqueous solution.
For example; salt in water and sugar in water
Non-aqueous solution: When a solute is dissolved in a solvent other than water, then this type of solution is called a non-aqueous solution.
For Example; iodine in carbon tetrachloride, sulphur in carbon disulfide.
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Pure Substances: Definition, Examples, and Difference
(more…) Continue ReadingPure Substances
Anything which occupies space and has mass is called matter. The matter is divided into two categories which are; Mixtures and Pure substances.
1. Pure Substances
Pure substances are defined as substances made up of only one kind of atom or molecule.
Pure substances also have fixed shapes and structures.
Pure substances are further classified into elements and compounds.
For example; gold metal
2. Mixtures
Mixtures are also called impure substances because it is composed of different kinds of components.
Mixtures are further divided into two categories which are a homogeneous mixture and heterogeneous mixture.
Example; water and sand, salt and water.
Difference Between Pure Substances and Mixtures
Pure Substances Mixtures Pure substances are made up of a single kind of particles The mixture is composed of two or more different substances. Pure substances can be classified into elements and compounds Mixtures are classified into homogenous and heterogenous They have a definite set of properties They don’t have a definite set of properties Components of pure substances cannot be separated by physical methods Components of the mixture can be separated by physical methods such as evaporation, etc. For example; hydrogen gas For example; oil and water Properties of Pure Substances
• Pure substances are in most cases homogeneous in nature containing only one form of atoms or molecules.
• Those substances especially have a constant or uniform composition throughout.
• Pure substances have static boiling and melting points.
Pure Substances Examples
All elements are commonly pure materials. Some of them encompass gold, copper, oxygen, chlorine, diamond, etc.
Compounds including water, salt or crystals, baking soda among others are also grouped under pure substances.
Depending on who you communicate to, homogeneous mixtures can also be taken into consideration as examples of pure materials.
Examples of homogeneous combinations include vegetable oil and air.
Heterogeneous mixtures are not considered pure substances.
Examples of homogenous mixtures that aren’t pure substances include gravel, a mixture of salt and sugar, etc.
Elements
A pure substance that has only one kind of atom and also cannot be broken down into two or more simpler substances by the physical or chemical method is called an element. Thus, when we break down gold, we still get gold. Thus, it is an element.
Properties of Elements
• An element is homogeneous; it’s a pure substance, made from a single form of atoms. As an instance, iron and silver are the product of only iron and silver atoms. Consequently, they’re elements.
• Elements cannot be broken down into more simpler substances by any physical or chemical processes such as heat, chemical reactions.
• Elements have sharp melting and boiling factors.
• Elements are categorized as metals, non-metals, and metalloids.
(a) Metals
Metals are the elements that voluntarily lose an electron to shape a positive ion or a cation.
For example; Gold, silver, copper, iron, potassium, etc.
– Metals have lustre. For Example; Gold.
– Metals are accurate conductors of warmth and energy. As metals have unfastened electrons in them, they may be able to behavior warmness and electricity. Example: Copper
– Metals are malleable, which means that it’s easy to mallet them into thin sheets. Instance: Aluminum
– Metals are ductile, meaning they can be drawn into wires.
– Metals are sonorous. They deliver a ringing sound when they’re hit via a tough iron rod. For Example; copper.
– Nearly all metals are solids at room temperature. Exception; Sodium and potassium are tender metals. Tungsten is a bad conductor of electricity.
(b) non-Metals
Non – metals are those elements voluntarily gain an electron(s) to shape a negative ion or anion.
Examples encompass Hydrogen, Oxygen, Iodine, etc.
– Non-metals exist as solids, liquids, and gases. Instance: Silicon and carbon are solids; bromine is a liquid; chlorine, fluorine, and oxygen are gases.
– Non-metals are non-lustrous, which means they have a dull look. Instance: The surfaces of sulfur and phosphorus do not gloss.
– Generally, non-metals have very low density. For Example, Oxygen and nitrogen are lighter than air.
– They’re not malleable.
– Non-metals, besides carbon, aren’t ductile.
– They’re terrible conductors of electricity. exception; graphite is a superb conductor of strength.
– Non-metals have low melting and boiling factors.
(c) Metalloids
The factors which have intermediate characteristics among the ones of metals and non-metals are known as metalloids. They are amphoteric.
– Metalloids react both with acids and bases. Examples encompass boron, silicon, and germanium.
Compound
A natural substance, essentially composed of two or greater elements and chemically mixed in a set share is called a compound. Consequently, water is a compound. It has two elements, hydrogen, and oxygen, mixed in a set ratio.
Properties of a Compound
– A compound is homogeneous in nature, made up of identical types of molecules.
– The additives of a compound can be separated by using chemical and electrochemical strategies. Thus, water may be broken down into hydrogen and oxygen through electrolysis.
– A compound have a fixed composition.
– A compound has a sharp melting and boiling factor.
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States of Matter: Definition and the Five...
Continue ReadingStates of Matter: Introduction
The term matter is defined as anything that occupies space and has mass. The matter can neither be created nor be destroyed. Various forms of matter exist in nature and these are solid, liquid, and gas. The fourth state of matter is plasma but it does not exist in our everyday life.
A states of matter is only a way to describe the behavior of atoms and molecules in a substance.
What is States of Matter?
A substance can take on different physical forms depending on various things such as temperature, pressure, and substance`s properties. The physical form is commonly called the state of matter. The states of matter are also called phases.
There are four common states of matter and it has been described in Figure 1.
Figure 1: The different states of matter
1. Solid State
The solid is one of the state of matter, where the molecules are tightly packed and are held together by strong forces.
The molecules in the case of solids are not able to move freely however they can vibrate at their fixed positions.
The solids have a fixed shape and size.
The rate of diffusion in solids is low and density is high.
Examples of solid include metal and ceramic bowls.
Based on the arrangement of solid molecules, the solids can further be divided into crystalline and amorphous.
(a) Crystalline Solid State
The crystalline solid state of matter is a periodic arrangement of fixed and long-range order of atoms/ molecules in all three dimensions.
Among the common examples are rock salt, sugar, metal keys, etc.
(b) Amorphous Solid State
The amorphous solid state of matter is a periodic arrangement of a short range of atoms/ molecules in all three dimensions.
Common examples are window glass, cotton candy, etc.
2. Liquid State
In liquids, the forces between the molecules are weaker than the solids.
Particles are fairly close together but can move around freely.
The liquids have an indefinite shape and can adapt to the shape of the container in which it has been kept.
The volume of liquid is fixed and the rate of diffusion in liquid is comparatively higher than that of solids.
The examples commonly include cola, coffee, tea, etc.
3. Gaseous State
This state of matter can be differentiated by low density and viscosity.
great expansion & contraction with changes in pressure and temperature, capacity to diffuse readily; and the tendency to become distributed homogeneously throughout any container.
The shape of the gas is not fixed.
The particles of gas have weak or no bonds.
The kinetic energy of gas molecules is very high as intermolecular forces are small.
The air we breathe is composed of gaseous states of many elements of which only oxygen is choosen by our body.
Plasma State
The matter of plasma is composed of atoms/ molecules, under the condition of standard pressure & temperature (STP) matter.
It has electrons that can orbit the atomic nucleus.
The shape and volume of plasma are not fixed.
If the temperature is very high, the electrons in the valence shell acquire enough kinetic energy to escape the atom. Therefore the plasma has very high kinetic energy.
The plasma produces the magnetic fields and sturdily responds to the electromagnetic field.
Plasma also possesses exclusive properties as free electrical charges cause it to be electrically conductive.
Examples of plasma are the illuminated state such as lighting, electric sparks, and some types of flames.
Phase Change
Phase changes occurs ,when the temperature or pressure change of a system takes place,.
When the temperature or pressure increases, the contact between the molecules increases.
Similarly, when the temperature decreases, it is much easier for molecules and atoms to settle into a more rigid structure.
Below represents the numerous phase changes.
– Freezing
– Melting
– Vaporization
– Condensation
– Sublimation
Change of State between Solid and Liquid
(a) Freezing
The method by which the substance changes from the liquid phase to the solid phase. The temperature at which any substance freezes, is called the freezing point.
For example the freezing of water to become solid ice.
(b) Melting
The process by which solid changes to liquid is called melting. The example here is when ice cubes from the freezer are placed in a warm room, the ice would absorb energy from the warmer air around them.
This absorption of energy would facilitate them to overcome the forces of attraction holding them together and enabling them to slip out of the fixed position that they held as ice.
Change of state Between Liquids and Gases
(a) Vaporization
Bubbles of water vapor form in the boiling water because particles of liquid water gain sufficient energy to completely overcome the force of attraction between them and change to the gaseous state.
Thus, the bubbles rise through the water and escape from the vessel as steam. The process of vaporization happens through two methods and that is evaporation and boiling.
The method in which a liquid boils and changes to gas is termed vaporization. The temperature at which a liquid boils. For example; boiling water to become steam, salt is recovered from seawater through this process.
(b) Condensation
When hot water interact with cooler surfaces such as the mirror, it chills and loses energy. The cooler water particles no longer have the energy to overcome the forces of attraction between them.
Together they form droplets of liquid water. This process in which a gas changes to liquid form is defined as condensation.
Example; Fog in the Air, Visible Breath in Cold Conditions, Clouding a Mirror, Steamy Rest room Mirror.
Change of state Between Solids and Gases
(a) Sublimation
The process in which solids directly change to gases is defined as sublimation. This occurs when solids absorb enough energy to overcome the forces of attraction between them.
For example; Dry ice is a case of solids that undergo sublimation, Snow and ice can sublime in the wintertime without melting, Mothballs sublime, Frozen foods sublime and ice crystals are found inside of the box.
(a) Deposition
A deposition is defined as the process in which a gas changes directly to a solid without going through the liquid state.
Examples of deposition in nature include frost forming on the ground and cirrus clouds forming high in the atmosphere, beaches, deltas, glacial moraines,sand dunes and salt domes in strictly cold temperatures form frost on windows because the water vapor in the air comes into contact with a window and proximately forms solid ice without even forming liquid water.
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Classification of Matter: Definition, Types, and Examples
Continue ReadingWhat is Matter?
When we study the term chemistry, it is often described as the state of matter. The concept of matter includes substances, compounds, elements, mixtures etc.
The matter shows some of the properties such as smell, colour etc. The substances can undergo changes which commonly include physical and chemical properties.
Physical properties commonly include shape, size, colour, and mass. Chemical properties include flammability.
Definition of Matter
The definitions of the following terms such as;
Matter: The term matter is commonly defined as anything that has mass and occupies space. The matter is further classified as solid, liquid and gas.
Substance: It is defined as the matter which is homogenous and of which all parts are alike. The substance can be homogenous and heterogenous.
Elements: The elements are pure substances that cannot be decomposed into simpler substances by chemical means. Some of the examples include gold, sulphur and iron.
Compounds: The compounds are pure substances that are composed of two or more elements.
Mixture: This is defined as a matter which consists of two or more substances mixed. A mixture can be homogenous or heterogeneous.
Homogenous mixtures are those that are not seen by the naked eye for example salt dissolves in water whereas heterogeneous mixtures are those that can be seen by the naked eye, for example, several different components.
Classification of Matter
The matter is classified as mixtures and substances. The mixture is further classified as homogenous and heterogeneous. The substances are further classified as elements and compounds.
Figure below will give the relationship between the concepts.
Mixture
A mixture is defined as a material that is made up of two or more different substances that are mixed but not combined chemically. An example of a mixture is sand and water.
The mixture is further classified into two parts and which are homogenous and heterogeneous.
I. Homogenous Mixture
The homogenous mixture is defined as a mixture of two or more substances where the different components cannot be visually distinguished.
If we take an example of a homogenous mixture then it would be a solution in sports drinks, consisting of water, sugar, colouring, flavouring, and electrolytes mixed uniformly.
Every sip of soft drink tastes the same because each sip contains the same amount of substances as mentioned above.
There are a few other examples of homogenous mixture that will include air, maple syrup. gasoline and solution of salt in water.
II. Heterogeneous Mixture
The heterogeneous mixture is defined as a mixture with a varying composition . The example includes Italian dressing.
The composition of Italian dressing can vary because it may be prepared by mixing different amounts of oil, vinegar, and herbs.
It is not uniform throughout the mixture—one drop may be mostly vinegar, whereas a different drop may be mostly oil or herbs because the oil and vinegar isolate and the herbs settle.
Substances
As per the definition in chemistry, substances are a form of matter that has a constant chemical composition and characteristic properties. The separation of components will only be possible when there is a breaking of chemical bonds.
The chemical substances can be solid, liquid or gas. The change in temperature or pressure can cause substances to shift between the different states of matter.
The substances are often called as pure as it separates them from the term mixture. An example of a substance is pure distilled water as it has always the same properties and the same ratio of hydrogen to oxygen.
The substances are further divided into two parts and that are elements and compounds.
Elements
The elements can be defined as a pure substance that consists of only one type of atom. The elements are divided into metals, metalloids and non-metals.
If we take a look at the periodic table in below Figure, the left side of the periodic table consists of metals that are often conductive to electricity, malleable, shiny and sometimes magnetic.
Examples of metals are aluminium, iron, copper etc. The right side of the periodic table consists of non-metals. The characteristic of non-metals includes not conductivity, not malleable, dull and not magnetic. The examples include carbon and oxygen.
As per the data of November 2011, 118 elements have been identified and out of 118, only 98 are known to occur naturally on the earth.
The most abundant elements on the earth are Hydrogen and Helium. All the known chemical matter is composed of these elements. The chemical matter constitute nearly about 15% of the matter in universe.
Compounds
The chemical compounds have a unique and defined structure a fixed ratio of atoms held together in a defined spatial arrangement by chemical bonds.
The few characteristics of chemical compounds can be that the molecular compounds are held together by covalent bonds.
Another characteristic is the salts are held together by ionic bonds or by metallic bonds and the complexes can also be held together by coordinate covalent bonds.
Pure chemical elements are not called chemical compounds even if they consist of diatomic or polyatomic molecules.
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