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Get expert help for all college & university chemistry homework & assignments: Chemistry is the science which studies the structure, composition, and property of matter and the ways in which matter interact with energy. There are certain natural laws which dictate the changes in properties that a given matter undergoes under specific conditions, and these are all defined by chemistry. When salt is placed together with water, the salt dissolves in water, changing the taste of the solution. The reaction that takes place here is determined by the chemical properties of salt and water. To break down the definition, it might be said that matter is anything that has mass and takes up space. All tangible things around us as well as several non-tangible things (like air) is made up of matter, and the matters in question are composed of atoms, molecules, and compounds. The atoms form the smallest unit of any given matter. Chemistry focuses on the properties of the atoms, the laws that govern the combination of atoms of different substances, and the knowledge thus derived is used to conduct reactions to achieve specific goals.
The existence of atoms was first suggested by Greek philosophers Leucippus and Democritus in the 4th century BC, when they offered the hypothesis that matter cannot be subdivided indefinitely but they are made of fundamental blocks, called atoms. However, they did not have the technology to test their hypothesis, neither did they believe in scientific experiments for they believed truth about nature and universe could be deduced through rational thought itself. Considerable advancements were made during the middle ages through the Renaissance when alchemists were invested in several experiments, mostly concerned with transformation of elements, a process known as transmutation. A large number of alchemists were attempting to convert cheaper elements into gold and though that particular experiment did not yield any result, they made other progresses along the way for instance, they discovered mercury and invented numerous strong acids. Most of these chemical revelations took place across the Arab Kingdoms, China, and medieval Europe.
Most of the concepts of chemistry which are highly relevant today and what is known as modern chemistry witnessed its origins in the 16th and 17th centuries when great progresses were made in the field, and systematic scientific experiments were conducted for the first time. Notable advances were made in metallurgy, where methods of extraction of metal from ores were discovered. It was during this period that the concept of elements emerged to the surface. Robert Boyle, an English scientist, described an element as a substance which could not be divided into two or more different substances by any chemical method. Following this definition, huge number of elements were identified. To his own surprise, several metals were identified as elements when Boyle himself did not presume metals could be elements. His other contributions to chemistry include the publication of ‘The Sceptical Chymist’ in 1661, where he explained the relation between pressure and volume of air.
Another noteworthy contribution in the development of modern chemistry was the discovery of oxygen and carbon dioxide by Joseph Priestly in the 18th century. He was the one to find that several carbon containing substances burned rapidly in the presence of oxygen, a process we now call combustion. One of the gaseous by-products of combustion is carbon dioxide, and Priestly discovered that this same gas was also produced when beer was fermented. Priestly was the first person to discover that solution of carbon dioxide in water creates seltzer water, and it is based on this discovery that the existing carbonated soft-drink industries are flourishing.
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In literal terms originating from the Greek language, Stoichiometry is the measure of elements. It is a crucial area of chemistry used to understand the relationship between reactants and products in a chemical reaction. It uses this relationship to determine the required quantitative data from a chemical reaction being studied. To use stoichiometry for the calculations it is of utmost importance that the chemical reaction is balanced, i.e., the number of different atoms in the reactants must be exactly the same as the product. Data about the relationship cannot be derived if the chemical reaction is not balanced, or in simpler terms the number of atoms in the reactants and the product do not match. To balance the number of elements in these two, a numeric value called the stoichiometric coefficient is defined and written for the atoms, molecules and ions involved in the reaction when expressed as an equation.
Measurements in chemistry provide the large-scale information based on which almost all laws, theories and hypotheses describing the behavior and attributes of matter, elements and energy are determined. These behaviors and attributes are applicable to both major domains of chemistry—macroscopic and microscopic. Three important kinds of information are central to any measurement; size or magnitude in the form of a number, a comparative standard in the form of a unit, and an indication that suggests the degree of uncertainty of the measurement. The number and unit are expressed explicitly while the uncertainty which usually rises from the different aspects of the measurement is represented in a more implicit manner. Numbers can be written according to the numeric system and can include decimals and scientific notations. Units are expressed in accordance with the International System of Units, better known as SI Units. Common examples of units are kilogram, centimeters, pounds and liters. It is important that the magnitude is expressed in a specific SI unit without which it will be meaningless.
Electronic structure refers to the specific arrangement of electrons inside an atom. Electrons in an atom occupy levels of energy which are also known as electron shells. These electron shells are situated outwards of the nucleus. Different shells have different capacities to hold electrons and those having the lowest levels of energy are occupied first. The shell nearest to the nucleus has the lowest level of energy and so on. Electrons move to other shells as soon as one shell is occupied to capacity. The final electronic structure is established once all the electrons in the atom have taken their spot. A prediction of the atom’s electronic structure can be made based on the atomic number. The theory of electronic structure applies the Born-Oppenheimer Approximation, according to which electrons automatically find their optimal distribution across shells for a given nuclear configuration because they are much light-weighted than the nucleus.
Electronic structure refers to th e specific arrangement of electrons inside an atom. Electrons in an atom occupy levels of energy which are also known as electron shells. These electron shells are situated outwards of the nucleus. Different shells have different capacities to hold electrons and those having the lowest levels of energy are occupied first. The shell nearest to the nucleus has the lowest level of energy and so on. Electrons move to other shells as soon as one shell is occupied to capacity. The final electronic structure is established once all the electrons in the atom have taken their spot. A prediction of the atom’s electronic structure can be made based on the atomic number. The theory of electronic structure applies the Born-Oppenheimer Approximation, according to which electrons automatically find their optimal distribution across shells for a given nuclear configuration because they are much light-weighted than the nucleus
Elemental analysis can be understood as the process of determining the amount of a certain element in a given material in terms of weight. It measures the element as a percentage of weight of the material being analyzed. Elemental analysis can also be qualitative in which the different elements present in a sample are determined. As the samples of most materials contain a number of different elements, there are various methods that can be applied that best suit the given sample and outcome requirement. Major qualitative methods include X-ray Photoelectron Spectroscopy (XPS), and Scanning Electron Microscopy and Energy Dispersive X-ray Spectroscopy (SEM-EDS). X-ray fluorescence (XRF) and Absorption Atomic Spectroscopy (AAS) are the most commonly used quantitative methods of elemental analysis. Other common methods include the two types of Inductively Coupled Plasma (ICP) namely; Optical Emission Spectroscopy (ICP-OES), and Mass Spectrometry (ICP-MS).
It refers to any form of interaction—chemical or physical resulting in a bond or association of atoms into substances seen in the physical world. Chemical bonding transforms atoms into ions, molecules, crystals and other materials that constitute the innumerable materials spread across the universe. A chemical bond can be understood as an invisible force that holds the atoms of different elements together and gives them a distinctive identity and characteristics. These characteristics are often completely different from those of the elements involved in the bond. The two major types of chemical bonding are covalent and ionic bonding. In covalent bonding the involved atoms share their electrons in specific arrangement. Ionic bonding is that in which atoms share valence electrons in a highly random manner forcing them to stay in vicinity of the other element rather than their own nucleus.
An atom is the smallest measurable unit of an element that retains its identity and characteristics. Atoms of most elements are one ten-billionth in length of a meter. The size of a single atom is expressed in angstrom denoted as 1Å. . An atom is composed of protons and neutrons which form its nucleus located at the center, and electrons orbiting the nucleus. The modern atomic theory propagated by the renowned English scientist John Dalton states; every matter is composed of atoms, atoms are unique to their elements, and they combine in whole number ratios to form compounds.
An ion is defined as a group of atoms bearing at least one electrical charge. This charge can be positive as well as negative. Ions with positive charge are called cations whereas those with a negative charge are called anions. There are various ways in which ions are formed. The simplest way is the addition or removal of electrons from other ions, neutral atoms and molecules. The other way is when a covalent bond between two atoms ruptures resulting in each electron staying associated with any of the former atoms. Ions are responsible for the composition of a number of crystalline substances held together in geometrical patterns.
A molecule is defined as a group of two or more atoms forming the smallest identifiable unit of a substance. The substance can be divided into individual molecules while retaining its properties and composition. A molecule can also be understood as the bond between atoms of the same or different elements. Size of molecules depends upon the number of atoms they consist of. Their chemical and physical properties are determined by their shape and composition. Molecules also do not carry any electrical charge.
A gas is one of the three fundamental states of matter, the other two being solid and liquid. The most remarkable and distinct feature of a gas is that it does not have any visible form or structure. This means that gases do not have a defined size and shape, unlike solids which have a definite size and shape and liquids which have a definite size and volume even though they do not possess a shape. Gases however have a microscopic structure on the molecular level. They are made up of extremely large numbers of molecules moving randomly in every direction, striking against each other and any other matter that comes in their path. Properties of gases are determined and observed usually by their temperature, pressure exerted by them on the walls of a container, resistance to flow and diffusion.
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