assignment meaning in chemistry

The 5 Main Branches of Chemistry

One of several ways chemistry can be divided into categories

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There are many branches of chemistry or chemistry disciplines. The five main branches are organic chemistry, inorganic chemistry, analytical chemistry, physical chemistry, and biochemistry.

Branches of Chemistry

• Traditionally, the five main branches of chemistry are organic chemistry, inorganic chemistry, analytical chemistry, physical chemistry, and biochemistry. However, sometimes biochemistry is considered a subdiscipline of organic chemistry.
• The branches of chemistry overlap those of physics and biology. There is also some overlap with engineering.
• Within each major discipline, there are many subdivisions.

What Is Chemistry?

Chemistry, like physics and biology, is a natural science. In fact, there is considerable overlap between chemistry and these other disciplines. Chemistry is a science that studies matter. This includes atoms, compounds, chemical reactions, and chemical bonds. Chemists explore the properties of matter, its structure, and how it interacts with other matter.

Overview of the 5 Branches of Chemistry

• Organic Chemistry : Organic chemistry is the study of carbon and its compounds . It is the study of the chemistry of life and reactions occurring in living organisms. An organic chemistry student might study organic reactions, the structure and properties of organic molecules, polymers, drugs, or fuels.
• Inorganic Chemistry : Inorganic chemistry is the study of compounds not covered by organic chemistry. It is the study of inorganic compounds or compounds that don't contain a C-H bond. A few inorganic compounds do contain carbon, but most contain metals. Topics of interest to inorganic chemists include ionic compounds, organometallic compounds, minerals, cluster compounds, and solid-state compounds.
• Analytical Chemistry : Analytical chemistry is the study of the chemistry of matter and the development of tools to measure the properties of matter. Analytical chemistry includes quantitative and qualitative analysis, separations, extractions, distillation, spectrometry and spectroscopy, chromatography, and electrophoresis. Analytical chemists develop standards, chemical methods, and instrumental methods.
• Physical Chemistry: Physical chemistry is the branch of chemistry that applies physics to the study of chemistry, which commonly includes the applications of thermodynamics and quantum mechanics to chemistry.
• Biochemistry : Biochemistry is the study of chemical processes that occur inside living organisms. Examples of key molecules include proteins, nucleic acids, carbohydrates, lipids, drugs, and neurotransmitters. Sometimes this discipline is considered a subdiscipline of organic chemistry. Biochemistry is closely related to molecular biology, cell biology, and genetics.

Other Branches of Chemistry

There are other ways chemistry can be divided into categories. Depending on who you ask, other disciplines might be included as a main branch of chemistry. Other examples of branches of chemistry include:

• Astrochemistry : Astrochemistry examines the abundance of elements and compounds in the universe, their reactions to each other, and the interaction between radiation and matter.
• Chemical Kinetics : Chemical kinetics (or simply "kinetics") studies the rates of chemical reactions and processes and the factors that affect them.
• Electrochemistry : Electrochemistry examines the movement of charge in chemical systems. Often, electrons are the charge carriers, but the discipline also investigates the behavior of ions and protons.
• Green Chemistry : Green chemistry looks at ways of minimizing the environmental impact of chemical processes. This includes remediation as well as ways of improving processes to make them more eco-friendly.
• Geochemistry : Geochemistry examines the nature and properties of geological materials and processes.
• Nuclear Chemistry : While most forms of chemistry mainly deal with interactions between electrons in atoms and molecules, nuclear chemistry explores the reactions between protons, neutrons, and subatomic particles.
• Polymer Chemistry : Polymer chemistry deals with the synthesis and properties of macromolecules and polymers.
• Quantum Chemistry : Quantum chemistry applies quantum mechanics to model and explore chemical systems.
• Radiochemistry : Radiochemistry explores the nature of radioisotopes, the effects of radiation on matter, and the synthesis of radioactive elements and compounds.
• Theoretical Chemistry : Theoretical chemistry is the branch of chemistry that applies mathematics, physics, and computer programming to answer chemistry questions.
• Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
• Laidler, Keith (1993). The World of Physical Chemistry . Oxford: Oxford University Press. ISBN 0-19-855919-4.
• Skoog, Douglas A.; Holler, F. James; Crouch, Stanley R. (2007). Principles of Instrumental Analysis . Belmont, CA: Brooks/Cole, Thomson. ISBN 978-0-495-01201-6.
• Sørensen, Torben Smith (1999). Surface Chemistry and Electrochemistry of Membranes . CRC Press. ISBN 0-8247-1922-0.
• Streitwieser, Andrew; Heathcock, Clayton H.; Kosower, Edward M. (2017). Introduction to Organic Chemistry . New Delhi: Medtech. ISBN 978-93-85998-89-8.
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1.3 Physical and Chemical Properties

Learning objectives.

By the end of this section, you will be able to:

• Identify properties of and changes in matter as physical or chemical
• Identify properties of matter as extensive or intensive

The characteristics that distinguish one substance from another are called properties. A physical property is a characteristic of matter that is not associated with a change in its chemical composition. Familiar examples of physical properties include density, color, hardness, melting and boiling points, and electrical conductivity. Some physical properties, such as density and color, may be observed without changing the physical state of the matter. Other physical properties, such as the melting temperature of iron or the freezing temperature of water, can only be observed as matter undergoes a physical change. A physical change is a change in the state or properties of matter without any accompanying change in the chemical identities of the substances contained in the matter. Physical changes are observed when wax melts, when sugar dissolves in coffee, and when steam condenses into liquid water ( Figure 1.18 ). Other examples of physical changes include magnetizing and demagnetizing metals (as is done with common antitheft security tags) and grinding solids into powders (which can sometimes yield noticeable changes in color). In each of these examples, there is a change in the physical state, form, or properties of the substance, but no change in its chemical composition.

The ability to change from one type of matter into another (or the inability to change) is a chemical property . Examples of chemical properties include flammability, toxicity, acidity, and many other types of reactivity. Iron, for example, combines with oxygen in the presence of water to form rust; chromium does not oxidize ( Figure 1.19 ). Nitroglycerin is very dangerous because it explodes easily; neon poses almost no hazard because it is very unreactive.

A chemical change always produces one or more types of matter that differ from the matter present before the change. The formation of rust is a chemical change because rust is a different kind of matter than the iron, oxygen, and water present before the rust formed. The explosion of nitroglycerin is a chemical change because the gases produced are very different kinds of matter from the original substance. Other examples of chemical changes include reactions that are performed in a lab (such as copper reacting with nitric acid), all forms of combustion (burning), and food being cooked, digested, or rotting ( Figure 1.20 ).

Properties of matter fall into one of two categories. If the property depends on the amount of matter present, it is an extensive property . The mass and volume of a substance are examples of extensive properties; for instance, a gallon of milk has a larger mass than a cup of milk. The value of an extensive property is directly proportional to the amount of matter in question. If the property of a sample of matter does not depend on the amount of matter present, it is an intensive property . Temperature is an example of an intensive property. If the gallon and cup of milk are each at 20 °C (room temperature), when they are combined, the temperature remains at 20 °C. As another example, consider the distinct but related properties of heat and temperature. A drop of hot cooking oil spattered on your arm causes brief, minor discomfort, whereas a pot of hot oil yields severe burns. Both the drop and the pot of oil are at the same temperature (an intensive property), but the pot clearly contains much more heat (extensive property).

Chemistry in Everyday Life

Hazard diamond.

You may have seen the symbol shown in Figure 1.21 on containers of chemicals in a laboratory or workplace. Sometimes called a “fire diamond” or “hazard diamond,” this chemical hazard diamond provides valuable information that briefly summarizes the various dangers of which to be aware when working with a particular substance.

The National Fire Protection Agency (NFPA) 704 Hazard Identification System was developed by NFPA to provide safety information about certain substances. The system details flammability, reactivity, health, and other hazards. Within the overall diamond symbol, the top (red) diamond specifies the level of fire hazard (temperature range for flash point). The blue (left) diamond indicates the level of health hazard. The yellow (right) diamond describes reactivity hazards, such as how readily the substance will undergo detonation or a violent chemical change. The white (bottom) diamond points out special hazards, such as if it is an oxidizer (which allows the substance to burn in the absence of air/oxygen), undergoes an unusual or dangerous reaction with water, is corrosive, acidic, alkaline, a biological hazard, radioactive, and so on. Each hazard is rated on a scale from 0 to 4, with 0 being no hazard and 4 being extremely hazardous.

While many elements differ dramatically in their chemical and physical properties, some elements have similar properties. For example, many elements conduct heat and electricity well, whereas others are poor conductors. These properties can be used to sort the elements into three classes: metals (elements that conduct well), nonmetals (elements that conduct poorly), and metalloids (elements that have intermediate conductivities).

The periodic table is a table of elements that places elements with similar properties close together ( Figure 1.22 ). You will learn more about the periodic table as you continue your study of chemistry.

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Module 2: Atoms, Molecules, and Ions

Assignment: atoms, molecules, and ions.

This assignment can be found in Google Docs:  Chemistry for Majors Assignment: Atoms, Molecules, and Ions

To make your own copy to edit:

• If you want a Google Doc : in the file menu of the open document, click “Make a copy.” This will give you your own Google Doc to work from.
• If you want a PDF or Word file : in the file menu of the open document, click “Download” and select the file type you would like to have (note: depending on the file type you select, the formatting could get jumbled).

Instructions

As you work these problems, consider and explain:

• What type of question is it?
• How do you know what type of question it is?
• What information are you looking for?
• What information do they give?
• How will you go about solving this?
• Show how to solve the problem.
• Be able to answer for a different reaction, number, set of conditions, etc.
• NH 4 and NH 4 Cl
• ZnO 2 and ZnCl 2
• H 2 O and HCl
• NO and NO 2
• CH 4 and CO 2
• A sample of chemical X is found to contain 5.0 grams of oxygen, 10.0 grams of carbon, and 20.0 grams of nitrogen. The law of definite proportion would predict that a 70 gram sample of chemical X should contain how many grams of carbon?
• All atoms of the same element are identical.
• Compounds are combinations of different atoms.
• A chemical reaction changes the way atoms are grouped together.
• Atoms are indestructible.
• Who was the first scientist to show that atoms emit any negative particles?
• The Rutherford experiment proved the Thomson “plum-pudding” model of the atom to be essentially correct.
• The Rutherford experiment was useful in determining the nuclear charge on the atom.
• Millikan’s oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron.
• The electric discharge tube proved that electrons have a negative charge.
• All of the above experiments gave the results described.
• An atom is mostly empty space.
• Almost all of the mass of the atom is concentrated in the nucleus.
• The protons and neutrons in the nucleus are very tightly packed.
• The number of protons and neutrons is always the same in the neutral atom.
• All of the above statements (A–D) are true.
• [latex]{}_{14}^{16}\text{C}[/latex]
• [latex]{}_{17}^{37}\text{Cl}[/latex]
• [latex]{}_{15}^{32}\text{P}[/latex]
• [latex]{}_{19}^{39}\text{K}[/latex]
• [latex]{}_{14}^{8}\text{N}[/latex]
• The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. What does Rhenium-185 have in its nucleus?
• 20 protons and 20 neutrons
• 21 protons and 19 neutrons
• 22 neutrons and 18 protons
• 20 protons and 22 neutrons
• 21 protons and 20 neutrons
• How many protons, neutrons, and electrons does [latex]{}_{20}^{40}\text{Ca}^{2+}[/latex] have?
• How many protons, neutrons, and electrons are in [latex]{}_{19}^{39}\text{K}^+[/latex]
• There is twice as much mass of hydrogen as oxygen in each molecule.
• There are two hydrogen atoms and one oxygen atom per water molecule.
• There is twice as much mass of oxygen as hydrogen in each molecule.
• There are two oxygen atoms and one hydrogen atom per water molecule.
• None of these.
• K, alkali metal
• Ba, alkaline earth metal
• Ne, noble gas
• Ni, transition metal
• Calcium, Ca
• good conductors of heat
• often lustrous
• tend to gain electrons in chemical reactions
• cobalt(II) chloride
• magnesium oxide
• aluminum(III) oxide
• diphosphorus pentoxide
• All of the above names are correct
• iodine trichloride, ICl 3
• phosophorus pentoxide, P 2 O 5
• ammonia, NH 3
• sulfur hexafluoride, SF 6
• All of the above pairs are correct.
• How many oxygen atoms are there in one formula unit of Ca 2+ ?
• What is the correct name for FeO?
• What is the correct name for Ca 2+ ?
• What is the correct name for V 3+ ?
• What is the subscript of barium in the formula of barium sulfate?
• What is the formula for calcium bisulfate?
• Pb(NO 3 ) 2 , lead(II) nitrate
• NH 4 ClO 4 , ammonium perchlorate
• PO 4 3− , phosphate ion
• Mg(OH) 2 , magnesium hydroxide
• NO 3− , nitrite ion
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physical chemistry

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• American Chemical Society - Physical Chemistry
• physical chemistry - Student Encyclopedia (Ages 11 and up)

physical chemistry , branch of chemistry concerned with interactions and transformations of materials. Unlike other branches, it deals with the principles of physics underlying all chemical interactions (e.g., gas laws ), seeking to measure, correlate, and explain the quantitative aspects of reactions . Quantum mechanics has clarified much for physical chemistry by modeling the smallest particles ordinarily dealt with in the field, atoms and molecules , enabling theoretical chemists to use computers and sophisticated mathematical techniques to understand the chemical behaviour of matter . Chemical thermodynamics deals with the relationship between heat and other forms of chemical energy , kinetics with chemical reaction rates. Subdisciplines of physical chemistry include electrochemistry , photochemistry ( see photochemical reaction ), surface chemistry, and catalysis . (For a more in-depth discussion of physical chemistry, see chemistry: Physical chemistry .)

• Chemistry Articles

Suspensions

What is suspension.

A suspension is defined as a heterogeneous mixture in which the solid particles are spread throughout the liquid without dissolving in it.

A suspension is defined as a homogenous mixture of particles with a diameter greater than 1000 nm such that the particles are visible to naked eyes. In this type of mixture, all the components are completely mixed and all the particles can be seen under a microscope. A suspension is a heterogeneous mixture containing solid particles that are sufficiently large for sedimentation.

If we take a glass full of water and mix mud in it, it will form a heterogeneous mixture . We can easily identify the components of these mixtures.  After some time we will observe that particles of mud settle down due to gravity. The particles in suspension are larger than the particles in a solution.

Table of Content

Properties of suspension, examples of suspension, what is a solution, what is a colloid, recommended videos, difference between colloid and suspension.

• Frequently Asked Questions- FAQs

• A suspension is a heterogeneous mixture.
• The size of solute particles in a suspension is quite large.
• The particles of a suspension can be seen easily.
• The particles of a suspension do not pass through a filter paper. So a suspension can be separated by filtration.
• The suspension is unstable. The particles of a suspension settle down after some time.
• A suspension scatters a beam of light passing through it because of its large particle size.

Some common examples of suspension are

• Muddy water
• Milk of magnesia
• Sand particles suspended in water
• Flour in water
• Slaked lime for whitewashing
• Paints in which dyes are suspended in turpentine oil.

A solution is a homogeneous mixture of substances. For example, when salt dissolves in water, a homogeneous mixture, or solution, forms. The component of a mixture that is present in the greatest quantity or that determines the state of matter of the solution is called the solvent and the other component is called the solute.

A Colloid is an intermediate between solution and suspension. It has particles with sizes between 2 and 1000 nanometers. A colloid is easily visible to the naked eye. Colloids can be distinguished from solutions using the  Tyndall effect.  Tyndall effect is defined as the scattering of light (light beam) through a colloidal solution. The particles are termed as colloidal particles and the mixture formed is known as colloidal dispersion. Liquid, solid and gases all mix together to form a colloidal dispersion.

The different types of colloidal solution are:

• Aerosols : Solid or liquid mixed with gas; Example: fog (liquid in gas)
• Sols : Solid mixed with liquid; Example: Paint
• Emulsion : Liquid with liquid; Example: oil and water
• Gel : liquid in solid; Example: Fruit jelly

The difference between suspension and colloids are tabulated below.

Frequently Asked Questions – FAQs

Give some suspension examples..

Suspension is commonly represented by a mixture of chalk and water, muddy water, a mixture of flour and water, a mixture of dust particles and air, fog, milk of magnesia, and so on.

What kind of mixture is suspension?

Suspension is a heterogenous mixture

How large are particles in suspension?

A suspension is a homogeneous mixture of particles with diameters greater than 1000 nm that are visible to the naked eye.

Describe the appearance of a suspension.

Suspensions have a non-uniform colour and can appear cloudy or murky, similar to muddy water. Particles will float around in a suspended solution.

What is the difference between suspension and colloid?

Unlike colloid particles, those in a suspension can be separated by filtration. Colloids are capable of scattering light, but suspensions are not. Particles in a suspension can be seen with the naked eye, but those in a colloid require the use of a light microscope.

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excellent explanation

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