Australian Wills, Estates, and Probate Records

Australian Wills, Estates, and Probate Records Wills and probate records can often be a gold mine when researching Australian ancestors. Wills generally list surviving heirs by name, providing confirmation of family relationships. Probate records which document the handling of the estate through the court, whether the deceased died testate (with a will) or intestate (without a will), may help identify where family members were living at the time, including those residing in other Australian states, or even back in Great Britain. For more information on the valuable genealogical clues estate records can provide, see Probing into Probate Records. There is no central archive of wills in Australia. Instead, wills and probate registers are maintained by each Australian state, generally through the probate registry or probate office of the Supreme Court. Some states have transferred their early wills and probates, or provided copies, to the State Archives or Public Record Office. Many Australian probate records have also been filmed by the Family History Library, but some of these films are not permitted to be circulated to Family History Centers. How to Locate Australian Wills Probate Records AUSTRALIAN CAPITAL TERRITORYRecords begin in 1911Indexes to wills and probate records in the Australian Capital Territory have not been published, and the records are not available online. ACT Supreme Court Registry4 Knowles PlaceCanberra ACT 2601 NEW SOUTH WALESRecords begin in 1800The Supreme Court NSW Probate Division has published an index to probates granted in NSW between 1800 and 1985, available in the NSW State Records Authority reading room and many major libraries (not available online). An index to early wills not included in the regular probate series is available online. Probate packets and wills from 1817 through 1965 have been transferred from the Supreme Court to the State Records Authority of New South Wales. Many of these probate packets are indexed online in Archives Investigator, including Series 1 (1817–1873), Series 2 (1873–1876), Series 3 (1876–c.1890) and a portion of Series 4 (1928–1954). Select Simple Search and then type in the name of your ancestor (or even just a surname), plus the term death to find indexed wills and probates, including the information youll need to retrieve a copy of the full probate packet. Learn more in the NSW Archives briefs Probate Packets and Deceased Estate Files, 1880–1958. State RecordsWestern Sydney Records Centre143 OConnell StreetKingswood NSW 2747 Access to wills and probate records from 1966 to the present require an application  to the Probate Division of the Supreme Court of New South Wales. Supreme Court of New South WalesProbate DivisionG.P.O. Box 3Sydney NSW 2000 NORTHERN TERRITORYRecords begin in 1911Indexes to Northern Territory wills and probates have been created and published on microfiche. The Family History Library has a partial set, but they are not open for circulation to Family History Centers (viewable in Salt Lake City only). Alternatively, send a SASE to the Northern Territory Registrar of Probates with details on the descendant, and they will send a return letter regarding the availability of the record and fees to obtain a copy. Registrar of ProbatesSupreme Court of the Northern TerritoryLaw Courts BuildingMitchell StreetDarwin, Northern Territory 0800 QUEENSLANDRecords begin in 1857Queensland has more will and probate records online than any other Australian state or territory, courtesy of the Queensland State Archives. Detailed information is available in their Brief Guide 19: Will Intestacy Records. Index to Wills, 1857-1940  - An online index to wills compiled from original Supreme Court files from all districts, including a few wills for people who died outside Queensland.Equity Index 1857-1899  - An online index to original Supreme Court Equity files that include the names of all people connected with a case.Instruments of Renunciation 1915-1983 - Lodged by executors who were no longer willing to administer a will, these records include many details on the deceased and estate.Trustees Files Index 1889-1929 - Files related to trusts set up under the terms of a will. Queensland State Archives435 Compton Road, RuncornBrisbane, Queensland 4113 More recent probates in Queensland are administered by and available through Queensland district court registrars. An index to the most recent probates from all districts can be searched online. Queensland eCourts Party Search – An online index to Queensland Supreme and District Court files from as early as 1992 (Brisbane) to the present. Supreme Court of Queensland, Southern DistrictGeorge StreetBrisbane, Queensland 4000 Supreme Court of Queensland, Central DistrictEast StreetRockhampton, Queensland 4700 Supreme Court of Queensland, Northern DistrictWalker StreetTownsville, Queensland 4810 SOUTH AUSTRALIARecords begin in 1832The Probate Registry Office holds wills and related documents for South Australia from 1844. Adelaide Proformat offers a fee-based probate record access service. Probate Registry OfficeSupreme Court of South Australia1 Gouger StreetAdelaide, SA 5000 TASMANIARecords begin in 1824The Archives Office of Tasmania holds most older records relating to the administration of probate in Tasmania; their Brief Guide 12: Probate includes details on all available records. The Archives Office also has an online index with digitized copies of wills (AD960) and letters of administration (AD961) up to 1989 available for online viewing. Index to Wills Letters of Administration from 1824-1989 (Tasmania) (includes digitized records) Probate RegistrySupreme Court of TasmaniaSalamanca PlaceHobart, Tasmania 7000 VICTORIARecords begin in 1841Wills and probate records created in Victoria between 1841 and 1925 have been indexed and digitized and made available online free of charge. Records of wills and probate records up to 1992 will eventually be included in this online index. Probate records after 1925 and up through about the last decade or so can be ordered through the Public Record Office of Victoria. Public Record Office Victoria99 Shiel StreetNorth Melbourne VIC 3051 Index to Wills, Probate and Administration Records 1841-1925 (Victoria) (includes digitized records) Generally, wills and probate records created within the past 7 to 10 years can be accessed through the Probate Office of the Supreme Court of Victoria. Registrar of ProbatesSupreme Court of VictoriaLevel 2: 436 Lonsdale StreetMelbourne VIC 3000 WESTERN AUSTRALIARecords from 1832Probate records and wills in Western Australia are not generally available online. See Information Sheet: Grants of Probate (Wills) and Letters of Administration from the State Records Office of Western Australia for further information. The State Records Office holds two indexes to wills and letters of administration: 1832-1939 and 1900-1993. Files up to 1947 are available at State Records Office on microfilm for viewing. State Records OfficeAlexander Library BuildingJames Street West EntrancePerth Cultural CentrePerth WA 6000 Most Supreme Court records in Western Australia, including probates, are covered by a 75 year restricted access period to protect the privacy of persons mentioned in the records. Written permission from the Supreme Court is needed before viewing. Probate Office14th Floor, 111 Georges StreetPerth WA 6000

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Personal Financial Plan - Part II - Essay Example Personal financial planning requires economics since economic variables like regulations, economic policies, and taxation has to be considered. In addition the use of credit is of prime importance in financial planning. This paper describes the role of economics and credit in personal financial planning. Classic economists assert that people know and understand what is in their best interest and they act and make decisions on this knowledge (Gitman, Joehnk, & Billingsley, 2010). For people to take advantage of this knowledge in their financial plan, they need to understand the most important aspects of economics like taxation, regulation, and markets among others. According to Gitman, Joehnk, and Billingsley (2010), federal tax forms the largest part of tax a citizen pays. Tax planning as an economic variable thus becomes an important part of personal financial planning. Credit refers to the trust that allows one person to avail resources to another person whereby an immediate reimbursement is not required (Edwards, 2004). The major advantages of credit are that it allows a person to acquire resources immediately and repay it comfortably within an extended period of time. The main disadvantage of credit is that the debtor will have to pay more than the amount he borrowed in the long run. Additionally, credit is reliant on the creditworthiness of the borrower; this makes it uncertain to receive. The government plays a major role in determine the economic stability of a nation. The government ensures stability and growth through guiding the pace of economic activity. The government also comes with policies relating to price stability, full employment, redistribution of income and the balance of payments stability (Edwards, 2004). The government also levies taxes and determines the amount of taxes the people will pay. These

An Analysis Of Emission Spectra Environmental Sciences Essay

An Analysis Of Emission Spectra Environmental Sciences Essay Emission spectra are the radiation emitted by the atoms when their electrons jump from higher energy level to lower energy level. The emission spectrum of a chemical element or chemical compound is the relative intensity of each frequency of electromagnetic radiation emitted by the elements atoms or the compounds molecules when they are returned to a ground state. The subatomic particles that comprise the atom can absorb various kinds of energy and then emit that energy as a photon of a specific energy and corresponding wavelength and frequency. This emitted energy is called an emission spectrum. Electrons in particular release electromagnetic radiation in the visible range as well as in wavelengths surrounding the visible range. The particular wavelength that an electron releases depends on the difference between its ground state energy and the energy level that it jumps to. 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Normally, therefore, substances are identified by their gas phase spectrum. A plot of the brightness of an object versus wavelength is called a spectrum, (even called spectra), and is observed using a spectrograph. By spreading out the light by wavelength, we can gain insight into whats happening to photons of particular wavelengths (or energies), which in turn tells us whats happening with particular types of atoms. There are three components of a spectrum: continuum emission (or blackbody radiation), emission lines, and absorption lines. Continuum emission is a wide, smooth (continuous!) band of colors like a rainbow. This type of emission is caused by an opaque material which emits radiation because of its temperature. Hotter objects are brighter and bluer than cooler objects. All objects have continuum radiation. (Even you; although in your case, since its in the infrared, we usually call it heat.) An absorption line is characterized by a lack of radiation at specific wavelength. Absorption lines are created by viewing a hot opaque object through a cooler, thin gas. The cool gas in front absorbs some of the continuum emission from the background source, and re-emits it in another direction, or at another frequency. Absorption lines are subtracted from the continuum emission, so that they appear fainter. An emission line is characterized by excessive radiation at specific wavelengths. You can observe emission lines by looking through a spectrometer at an energized gas. They are created by the photons that are released by the falling electrons. The important thing to know about absorption and emission lines is that every atom of a particular element (hydrogen, say) will have the same pattern of lines all the time. And the spacing of the lines is the same in both absorption and emission, only emission lines are added to the continuum, while absorption lines are subtracted. VARIOUS OBSERVATIONS OF SCIENTISTS IN EARLY AGE: When a sample of gaseous atoms of an element at low pressure is subjected to an input of energy, such as from an electric discharge, the atoms are themselves found to emit electromagnetic radiation. On passing through a very thin slit and then through a prism the light (electromagnetic radiation) emitted by the excited atoms is separated into its component frequencies. The familiar dispersion of white light is illustrated below: Solids, liquids and dense gases glow at high temperatures. The emitted light, examined using a spectroscope, consists of a continuous band of colours as in a rainbow. A continuous spectrum is observed. This is typical of matter in which the atoms are packed closely together. Gases at low pressure behave quite differently. The excited atoms emit only certain frequencies, and when these are placed as discreet lines along a frequency scale an atomic emission spectrum is formed. The spectral lines in the visible region of the atomic emission spectrum of barium are shown below. Spectral lines exist in series in the different regions (infra-red, visible and ultra-violet) of the spectrum of electromagnetic radiation. The spectral lines in a series get closer together with increasing frequency. Each element has its own unique atomic emission spectrum. EXPLANATION OF ABOVE MENTIONED OBSERVATIONS: It was necessary to explain how electrons are situated in atoms and why atoms are stable. Much of the following discussion refers to hydrogen atoms as these contain only one proton and one electron making them convenient to study. In the early 1913, the famous scientist Neils Bohr solved many problems in chemistry of the time by proposing his view that the electron revolves around the nucleus of the atom with a definite fixed energy in a fixed path, without emitting or absorbing energy. The electron in the hydrogen atom exists only in certain definite energy levels. These energy levels are called Principal Quantum Levels, denoted by the Principal Quantum Number, n. Principal Quantum Level n = 1 is closest to the nucleus of the atom and of lowest energy. When the electron occupies the energy level of lowest energy the atom is said to be in its ground state. An atom can have only one ground state. If the electron occupies one of the higher energy levels then the atom is in an excited state. An atom has many excited states. When a gaseous hydrogen atom in its ground state is excited by an input of energy, its electron is promoted from the lowest energy level to one of higher energy. The atom does not remain excited but re-emits energy as electromagnetic radiation. This is as a result of an electron falling from a higher energy level to one of lower energy. This electron transition results in the release of a photon from the atom of an amount of energy (E = h Ã‚ ®) equal to the difference in energy of the electronic energy levels involved in the transition. In a sample of gaseous hydrogen where there are many trillions of atoms all of the possible electron transitions from higher to lower energy levels will take place many times. A prism can now be used to separate the emitted electromagnetic radiation into its component frequencies (wavelengths or energies). These are then represented as spectral lines along an increasing frequency scale to form an atomic emission spectrum. Principal Quantum Levels (n) for the hydrogen atom. Comment: A hydrogen atom in its Ground State. The electron occupies the lowest possible energy level which in the case of hydrogen is the Principal Quantum Level n = 1. The Bohr Theory was a marvelous success in explaining the spectrum of the hydrogen atom. He calculated wavelengths agreed perfectly with the experimentally measured wavelengths of the spectral lines. Bohr knew that he was on to something; matching theory with experimental data is successful science. More recent theories about the electronic structure of atoms have refined these ideas, but Bohrs model is still very helpful to us. For clarity, it is normal to consider electron transitions from higher energy levels to the same Principal Quantum Level. The image given below illustrates the formation of spectral lines in visible region of the spectrum of electromagnetic radiation for hydrogen, called the Balmer Series. The Spectral Lines are in Series As referred to above for hydrogen atoms, electron transitions form higher energy levels all to the n = 2 level produce a series of lines in the visible region of the electromagnetic spectrum, called the Balmer Series. The series of lines in the ultra-violet region, called the Lyman Series, are due to electron transitions from higher energy levels all to the n = 1 level, and these were discovered after Bohr predicted their existence. Within each series, the spectral lines get closer together with increasing frequency. This suggests that the electronic energy levels get closer the more distant they become from the nucleus of the atom. No two elements have the same atomic emission spectrum; the atomic emission spectrum of an element is like a fingerprint. The diagram to the right illustrates the formation of three series of spectral lines in the atomic emission spectrum of hydrogen. THE RESON BEHIND DISTINCT WAVELENGTHS: As we know light from a mercury discharge tube was composed of only three colors, or three distinct wavelengths of light. This feature, that an element emits light of specific colors, is an enormously useful probe of how individual atoms of that element behave. Indeed, the science of spectroscopy was developed around the discovery that each element of the periodic table emits light with its own set characteristic wavelengths, or emission spectrum. of light. If one has a collection of several elements, all emitting light, and the spectra of the different elements combine or overlap. By comparing the combined spectra to the known spectra of individual elements, we can discover which elements are present. It is amusing to note that the element helium was first discovered in this manner through the spectroscopic analysis of light from the sun in 1868 and was only later discovered in terrestrial minerals in 1895. But why do we see distinct wavelengths in emission spectra? And why are the spectra different for particular elements? There is nothing distinct about the light from an incandescent source such as the ordinary light bulb. In an empirical study of the spectrum of hydrogen, Balmer discovered that the precise frequencies and wavelengths of the light produced could be described by a simple equation involving a constant and an integer. Balmers equation was then expanded to describe the entire spectrum of hydrogen, including the ultra-violet and the infrared spectral lines. This equation is called the Rydberg equation: = R (â‚ ¬Ã‚ ­ ), Where R is the Rydberg constant, and n1 and n2 are integers. The presence of integers in this equation created a real problem for physicists until the development of the quantum theory of the atom by Neils Bohr. Bohrs theory suggested that the electron orbiting the nucleus could have only certain quantized angular momenta. The implication of this idea is that the electron can orbit only at certain fixed distances and velocities around the nucleus and subsequently can possess only certain discrete energies. Individual electron orbits are associated with specific energy levels. Integer numbers uniquely identify these levels and these integers, quantum numbers, are the ones that show up in the Rydberg equation and that are labeled n1 and n2. The integers in Rydbergs equations identify electron orbits of specific radius. In general, the larger the value of the integer, the larger the size of the orbit. Rydbergs equation says that the wavelength of the light emitted from an atom depends on two electron orbits. The interpretation is that an electron makes a transition from the initial orbit identified by the integer n1 to a final orbit identified by the integer n2. Furthermore, since there is a unique energy associated with each electron orbit, these integers n1 and n2 also identify or tag the energy of the electron. Hence, a discrete amount of energy is released or absorbed when an electron makes a transition between two orbits. In the case of the atom, when an electron makes a transition from one orbit to another with a lesser value of its identifying integer, energy is released from the atom and takes the form of emitted light of a distinct wavelength, or equivalently, of distinct frequency. So the picture we have is that electron transitions between different orbits produce different wavelengths of light and that the actual wavelength value of the light depends on the energy difference between the two orbits. Furthermore, since the energies of the different orbits and the energies of the transitions are determined by the atomic number (the number of protons in the nucleus), each atom has its own characteristic spectrum. distances and velocities around the nucleus and subsequently can possess only certain discrete energies. Individual electron orbits are associated with specific energy levels. Integer numbers uniquely identify these levels and these integers, quantum numbers, are the ones that show up in the Rydberg equation and that are labeled n1 and n2. Emission Line Spectra of Various Elements REFERANCE NO. Explanation of the above Image: First spectrum is hydrogen, typical of a hydrogen spectrum tube. Second spectrum is helium, typical of a helium spectrum tube. Third spectrum is lithium, as typically from a flame or an electric arc. Fourth spectrum is neon. Fifth spectrum is low pressure sodium, but with secondary lines exaggerated. Sixth spectrum is argon, typical of an argon glow lamp or spectrum tube. Next spectrum is copper, drawn using a wavelength table and Ioannis Galidakis photos of a copper arc spectrum (see link below). Oxide lines which may appear in the flame spectrum are not shown. Next spectrum is zinc, drawn using a wavelength table and a photo by Ioannis Galidakis of a zinc arc spectrum. Intensity of the red line is shown for the slightly greenish light blue usual zinc arc, but Ioannis reports getting a pinkish zinc arc and shows the red line to be brighter. Next spectrum is barium. Oxide lines are not included. Next spectrum is krypton. Ion lines typical of flashlamp use are not included. Next spectrum is that of the most common variety of metal halide lamp, which is basically a mercury vapor lamp enhanced with iodides of sodium and scandium. Next spectrum is that of a xenon flashtube of lower-than-usual pressure, operated with a higher than usual voltage and a lower than usual energy level to favor a line spectrum. An actual typical xenon spectrum generally has a strong continuous spectrum, which I show more dimly than actually occurs in order to show the lines. The lines are mainly those of excited xenon ions, rather than excited neutral xenon atoms. At lower current, the most distinct visible spectral lines are two close together in the blue and the brightness is usually low. Next spectrum is high pressure mercury vapor, typical of a mercury vapor lamp. Low pressure mercury vapor has a similar spectrum except the green line is slightly dimmer and the yellow lines are significantly dimmer. Next one after that is a mercury lamp with the common Deluxe White phosphor. Next one after that is a compact fluorescent lamp of the 2700K color. Emission line spectra of various other elements is given below APPLICATIONS: Emission Spectroscopic techniques are used in Flame Emission Spectroscopy Energy spectra are used in astrophysical spectroscopy. Energy Spectra are used in Optical Spectroscopy

A University Student Budget Sheet :: Papers

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