compounds with the same molecular formula‚ but different atom connectivity. C2H6O Two different compounds with different physical & chemical properties: Ethyl alcohol (ethanol): B.P. 78.5 oC (liquid) M.P. –117.3 oC Reacts with alkaline metals. Dimethyl ether: -24.9 oC (gas!) -138 oC Does not How many isomers can you draw for: C4H10O C4H8O 3. Chemical Bonds Ionic: forms by a complete transfer of one or more electrons from one atom to another to form ions (cation and anion). Forms between
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Chemical Bonding Chemical compounds are formed by the joining of two or more atoms. A stable compound occurs when the total energy of the combination has lower energy than the separated atoms. The bound state implies a net attractive force between the atoms ... a chemical bond. The two extreme cases of chemical bonds are: Covalent Bonds Covalent chemical bonds involve the sharing of a pair of valence electrons by two atoms‚ in contrast to the transfer of electrons in ionic bonds. Such bonds lead to
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I have learned from this project is that everyone is original and vary from each other. This was a fun project‚ I got to display who I am and present the things that really mean the most to me‚ and why they are important. Each time I presented to a new person‚ I tried to enthrall them with my own originality. People read my symbols in the way I expected them too because‚ there were very little questions‚ some did have an egregious look on their face when I said I like to dance. If I could do this
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The increase in volume corresponding to increase in temperature and α-β phase transition can be clearly seen by comparing ATOMS 7&8 with ATOMS 9&10. In the β phase‚ the atoms are more spread out. While time-averaged Fe-O distances decrease with increasing temperature due to the increasing disorder at high temperature arising from excited low-energy‚ high-amplitude vibrations‚ instantaneous Fe-O distances
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sample is converted to a gaseous phase atoms or ions Atomic absorption spectroscopy is based on the same principle as the flame test used in qualitative analysis. When an alkali metal salt or a calcium‚ strontium or barium salt is heated strongly in the Bunsen flame‚ a characteristic flame colour is observed: Na -- yellow Li-- crimson Ca-- brick red Sr-- crimson Ba --green In the flame‚ the ions are reduced to gaseous metal atoms. Compound -------- heat------- atoms The high temperature of the flame
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molecule Mass spectrometer converts sample into ions‚ and that these ions can be further fragmented (broken down) into smaller molecules. Ionisation can be achieved using various different techniques‚ electron ionisation‚ chemical ionisation and Fast atom bombardment. When sample is ionised the analyser portion of the mass spectrometer seperates the molecules based on their mass to charge ratio. A dector then detects the molecule weight of all the molecules present and a spectrum is obtained. Base
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neutron(s) nucleus (nuclei) proton(s) a) Every atom contains a ……nucleus……….. which is positively charged. e) The nucleus of an atom is composed of ………protons…….. and ………neutrons……... f) The ……electrons……….. in an atom move about in the space surrounding the nucleus. g) An uncharged atom has equal numbers of ………protons…….. and ……electrons………... h) A charged atom is called an ……ion………... i) An uncharged atom becomes charged as a result of transferring ……electrons
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values‚ the cereal box spectrometer proved its value as a decently accurate spectrometer. Introduction: Every element and subsequent atom associated emits light; also know as electromagnetic radiation‚ when in an excited state. Analyzing this emitted light can give insight to the makeup and characteristics of them. The light given off by an energetically excited atom is not a continuous distribution of all possible wavelengths‚ but rather consists of a few wavelengths giving a series of discrete lines
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understanding of the structure of atom. New Zealand scientist Ernerst Rutherford was the first to show that the atom is the building block of all matter that consists of a positively charged nucleus surrounded by tiny negatively charged electrons. The extraordinary achievements of these scientists have been instrumental development of chemistry over the past century. Today‚ we take the existence of atoms for granted. We can explain many aspects of the structure of the atom and in fact‚ current technology
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Unit 2 Lecture Study Guide 1) What are the parts of an atom? Where are the subatomic particles found? Parts of an atom- divided into two basic regions: 1. the central nucleus (contains heavy particles) 2. the electron cloud (contains very light‚ moving particles) Subatomic particles: 1.Protons (found in the central nucleus) 2.neutrons (found in the central nucleus) 3.electrons (spin rapidly in a cloud around the central nucleus) 2) How does the Atomic Mass # differ from the Atomic
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