Drawing Atomic Structure
... The average atomic mass is the ______________________ mass of an element’s various isotopes (takes into consideration which isotopes are more ______________ than others). The average atomic mass can be found on the Periodic Table. Label this on the diagram on the first page. ...
... The average atomic mass is the ______________________ mass of an element’s various isotopes (takes into consideration which isotopes are more ______________ than others). The average atomic mass can be found on the Periodic Table. Label this on the diagram on the first page. ...
Atomic Structure Worksheet
... Look at the atomic weights of a few different elements on your periodic table. Do you notice that very few of the elements have atomic weights that are close to being nice whole numbers? Do you know why this is? After all, for our purposes, the mass of both the proton and the neutron are almost exac ...
... Look at the atomic weights of a few different elements on your periodic table. Do you notice that very few of the elements have atomic weights that are close to being nice whole numbers? Do you know why this is? After all, for our purposes, the mass of both the proton and the neutron are almost exac ...
800 - Paint Valley Local Schools
... considered radioactive because of its large, unstable nucleus. It was one of the fuels used to construct the early atomic bombs in the WWII era. ...
... considered radioactive because of its large, unstable nucleus. It was one of the fuels used to construct the early atomic bombs in the WWII era. ...
NUCLEAR CHEMISTRY AND RADIOACTIVE DECAY
... 17. Sr-90 is a common waste product of nuclear fission reactors. How many half-lives of Sr-90 will pass after 144 years (half life = 28.8 yrs)? ...
... 17. Sr-90 is a common waste product of nuclear fission reactors. How many half-lives of Sr-90 will pass after 144 years (half life = 28.8 yrs)? ...
Periodic Table notes
... Things that occur in a repeating pattern on the periodic table Atomic number, # of energy levels, valence electrons, oxidation #, atomic size, metallic ...
... Things that occur in a repeating pattern on the periodic table Atomic number, # of energy levels, valence electrons, oxidation #, atomic size, metallic ...
Pre-AP Chemistry
... Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. (1a) Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass. (1e) Students know some naturally occurring isotopes of elements are radioa ...
... Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. (1a) Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass. (1e) Students know some naturally occurring isotopes of elements are radioa ...
Atomic Structure
... • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically combine in simplewhole number ratios to form compounds. • 4. Chemical reactions occur when atoms are ...
... • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically combine in simplewhole number ratios to form compounds. • 4. Chemical reactions occur when atoms are ...
8th-interlude-for-atoms - Epiphany Catholic School
... Compounds Formed when atoms of more than one element combined. Properties of a compound are very different from properties of the elements that make it up. Ex. NaCl = salt ...
... Compounds Formed when atoms of more than one element combined. Properties of a compound are very different from properties of the elements that make it up. Ex. NaCl = salt ...
Big History Chemistry Study Guide File
... of _____ and _____. These isotopes have _____ neutrons or ____ neutrons. 7. In nuclear ________________, small atoms combine to make larger atoms, losing a tiny bit of mass and releasing energy in the process. 8. In nuclear _____________, radioactive elements such as ________________ break apart int ...
... of _____ and _____. These isotopes have _____ neutrons or ____ neutrons. 7. In nuclear ________________, small atoms combine to make larger atoms, losing a tiny bit of mass and releasing energy in the process. 8. In nuclear _____________, radioactive elements such as ________________ break apart int ...
Chapter 5
... • Example: Carbon-12 and Carbon-14 • Both have an atomic number of 6, but the mass numbers are different ...
... • Example: Carbon-12 and Carbon-14 • Both have an atomic number of 6, but the mass numbers are different ...
ISOTOPES
... all atoms of each element were the same. According to the model of atomic structure we have been developing, this would mean that each atom of an element would have the same number of protons, electrons, and neutrons as every other atom of the element. Thus the atomic mass of every atom of an elemen ...
... all atoms of each element were the same. According to the model of atomic structure we have been developing, this would mean that each atom of an element would have the same number of protons, electrons, and neutrons as every other atom of the element. Thus the atomic mass of every atom of an elemen ...
Chapter 4 Cornell Notes
... ____________________ of large atoms into smaller pieces) and nuclear ____________________ (the ____________________ of small atoms into one large one), but on earth these reactions do not occur naturally. 2) Naturally occurring nuclear reactions result from the unusual number of neutrons of an isoto ...
... ____________________ of large atoms into smaller pieces) and nuclear ____________________ (the ____________________ of small atoms into one large one), but on earth these reactions do not occur naturally. 2) Naturally occurring nuclear reactions result from the unusual number of neutrons of an isoto ...
Study Guide 1-3
... Test 1-3 will consist of multiple choice & short answer questions over the following information. 1) Be able to determine the atomic number, mass number, name, oxidation number and isotopic notation given a drawing of an atom or isotopic notation. You must also be able to determine number of protons ...
... Test 1-3 will consist of multiple choice & short answer questions over the following information. 1) Be able to determine the atomic number, mass number, name, oxidation number and isotopic notation given a drawing of an atom or isotopic notation. You must also be able to determine number of protons ...
Chapter 18 Notes
... Chemical symbols are the one or two letter abbreviations for elements, either one capital letter or two letters, first capital, second lower case. Atomic Components: Atom: smallest piece of matter that retains the element’s properties, composed of particles called protons, neutrons and electrons Nuc ...
... Chemical symbols are the one or two letter abbreviations for elements, either one capital letter or two letters, first capital, second lower case. Atomic Components: Atom: smallest piece of matter that retains the element’s properties, composed of particles called protons, neutrons and electrons Nuc ...
Chapter 4 Atomic Structure Notes
... A. Dimitri Mendeleev (1869) (Russian) – publishing the 1st periodic table based on increasing atomic mass no. 1. The elements fell into 7 columns based on chemical & physical properties 2. He left spaces for undiscovered elements B. Henry Mosely (1913) (British) publishes the “modern” periodic table ...
... A. Dimitri Mendeleev (1869) (Russian) – publishing the 1st periodic table based on increasing atomic mass no. 1. The elements fell into 7 columns based on chemical & physical properties 2. He left spaces for undiscovered elements B. Henry Mosely (1913) (British) publishes the “modern” periodic table ...
Chapter 4 Review
... particles. A fictitious element X has 10.0 % of the isotope with mass 55, 20.0 % of the isotope with mass 56, and 70.0 % of the isotope with mass 57. Estimate the atomic mass of element X. ...
... particles. A fictitious element X has 10.0 % of the isotope with mass 55, 20.0 % of the isotope with mass 56, and 70.0 % of the isotope with mass 57. Estimate the atomic mass of element X. ...
Atoms, Molecules and Ions Part 2
... • One of the 2 flaws in Dalton’s theory was, atoms of the same element can have DIFFERENT masses. • The mass of an atom is due to the mass of the protons and the neutrons in that atom. • Isotopes are atoms of the same element which have the same number of protons but different number of neutrons. Th ...
... • One of the 2 flaws in Dalton’s theory was, atoms of the same element can have DIFFERENT masses. • The mass of an atom is due to the mass of the protons and the neutrons in that atom. • Isotopes are atoms of the same element which have the same number of protons but different number of neutrons. Th ...
Atomic Structure: SOL Review #1 Name: Historical Developments 1
... solid sphere model; Atomic Theory: all elements made of atoms, atoms of an element are identical cathode ray tube; discovered electron; plum pudding model oil drop; discovered mass and charge of electron gold foil; discovered nucleus; the atom is mostly empty space planetary model; (ex) flame test l ...
... solid sphere model; Atomic Theory: all elements made of atoms, atoms of an element are identical cathode ray tube; discovered electron; plum pudding model oil drop; discovered mass and charge of electron gold foil; discovered nucleus; the atom is mostly empty space planetary model; (ex) flame test l ...
DALTON`S ATOMIC THEORY - 1808: Publication of Dalton`s "A New
... - Dalton's theory sets LIMITS on what can be done with chemistry. For example: Chemistry can't convert lead (an element) into gold (another element). Sorry, alchemists! You can't have a compound form in a chemical reaction that contains an element that was not in your starting materials. You can onl ...
... - Dalton's theory sets LIMITS on what can be done with chemistry. For example: Chemistry can't convert lead (an element) into gold (another element). Sorry, alchemists! You can't have a compound form in a chemical reaction that contains an element that was not in your starting materials. You can onl ...
Review Notes for Atomic Structure and Radioactivity Test on Friday
... 13. Atomic number - the number on the bottom before the element’s symbol - is unique to each element and is equal to the number of protons, which is equal to the number of electrons in a neutral atom. 14. Mass number - equal to the total number of protons plus neutrons, and appears at the top before ...
... 13. Atomic number - the number on the bottom before the element’s symbol - is unique to each element and is equal to the number of protons, which is equal to the number of electrons in a neutral atom. 14. Mass number - equal to the total number of protons plus neutrons, and appears at the top before ...
Promethium
Promethium, originally prometheum, is a chemical element with symbol Pm and atomic number 61. All of its isotopes are radioactive; it is one of only two such elements that are followed in the periodic table by elements with stable forms, a distinction shared with technetium. Chemically, promethium is a lanthanide, which forms salts when combined with other elements. Promethium shows only one stable oxidation state of +3; however, a few +2 compounds may exist.In 1902, Bohuslav Brauner suggested there was an element with properties intermediate between those of the known elements neodymium (60) and samarium (62); this was confirmed in 1914 by Henry Moseley who, having measured the atomic numbers of all the elements then known, found there was an element with atomic number 61. In 1926, an Italian and an American group claimed to have isolated a sample of element 61; both ""discoveries"" were soon proven to be false. In 1938, during a nuclear experiment conducted at Ohio State University, a few radioactive nuclides were produced that certainly were not radioisotopes of neodymium or samarium, but there was a lack of chemical proof that element 61 was produced, and the discovery was not generally recognized. Promethium was first produced and characterized at Oak Ridge National Laboratory in 1945 by the separation and analysis of the fission products of uranium fuel irradiated in a graphite reactor. The discoverers proposed the name ""prometheum"" (the spelling was subsequently changed), derived from Prometheus, the Titan in Greek mythology who stole fire from Mount Olympus and brought it down to humans, to symbolize ""both the daring and the possible misuse of mankind's intellect"". However, a sample of the metal was made only in 1963.There are two possible sources for natural promethium: rare decays of natural europium-151 (producing promethium-147), and uranium (various isotopes). Practical applications exist only for chemical compounds of promethium-147, which are used in luminous paint, atomic batteries, and thickness measurement devices, even though promethium-145 is the most stable promethium isotope. Because natural promethium is exceedingly scarce, it is typically synthesized by bombarding uranium-235 (enriched uranium) with thermal neutrons to produce promethium-147.