Chapter 5 Atomic Structure and the Periodic Table Section 5.1
... – Explain how the atomic number identifies an element. – Use the atomic number and mass number of an element to find the numbers of protons, electrons, and neutrons. – Explain how isotopes differ, and why the atomic masses of elements are not whole numbers. – Calculate the average atomic mass of an ...
... – Explain how the atomic number identifies an element. – Use the atomic number and mass number of an element to find the numbers of protons, electrons, and neutrons. – Explain how isotopes differ, and why the atomic masses of elements are not whole numbers. – Calculate the average atomic mass of an ...
1 Chapter 4 Atomic Structure 4.1 Defining the Atom Early Models of
... In a ____________________ tube, electrons travel as a ray from the cathode (-) to the anode (+). Such positively charged subatomic particles are called ________________. Each proton has a mass about 1840 times that of an electron. _________________ are subatomic particles with no charge but with a m ...
... In a ____________________ tube, electrons travel as a ray from the cathode (-) to the anode (+). Such positively charged subatomic particles are called ________________. Each proton has a mass about 1840 times that of an electron. _________________ are subatomic particles with no charge but with a m ...
CHEMISTRY The Molecular Science
... Dalton’s Atomic Theory • An element is composed of tiny particles called atoms. All atoms of a given element show the same chemical properties. • Atoms of different elements have different properties. • Compounds are formed when atoms of two or more elements combine. In a given compound, the relati ...
... Dalton’s Atomic Theory • An element is composed of tiny particles called atoms. All atoms of a given element show the same chemical properties. • Atoms of different elements have different properties. • Compounds are formed when atoms of two or more elements combine. In a given compound, the relati ...
the atomic theory
... 3. Ernest Rutherford 4. James Chadwick 5. Neils Bohr 6. nucleus 7. proton 8. neutron 9. electron 10. shell 11. atomic number 12. atomic mass 13. Bohr Model 14. subatomic particle 15. isotope 16. empty bus seat rule B/ THE HISTORY OF THE ATOM: - John Dalton ...
... 3. Ernest Rutherford 4. James Chadwick 5. Neils Bohr 6. nucleus 7. proton 8. neutron 9. electron 10. shell 11. atomic number 12. atomic mass 13. Bohr Model 14. subatomic particle 15. isotope 16. empty bus seat rule B/ THE HISTORY OF THE ATOM: - John Dalton ...
Inside the Atom
... We can calculate age of fossils by calculating how much C14 (radioactive) remains in a sample (accuracy to 35000 years) Uranium also is used to date rocks, however its half life is 4.5 billions years and decays to lead (Pb) scientists calculate age of earth and rocks by comparing amount uranium ...
... We can calculate age of fossils by calculating how much C14 (radioactive) remains in a sample (accuracy to 35000 years) Uranium also is used to date rocks, however its half life is 4.5 billions years and decays to lead (Pb) scientists calculate age of earth and rocks by comparing amount uranium ...
Matter - Moodle
... • The chemical composition ______________________ A chemical property describes how a substance ________________ into a new substance Either by: • __________________ with other elements • _________________ __________________ into new substances ...
... • The chemical composition ______________________ A chemical property describes how a substance ________________ into a new substance Either by: • __________________ with other elements • _________________ __________________ into new substances ...
Chapter 4 Review
... particles. A fictitious element “X” has 10.0 % of the isotope with mass 55 amu, 20.0 % of the isotope with mass 56 amu, and 70.0 % of the isotope with mass 57 amu. Estimate the atomic mass of element X. ...
... particles. A fictitious element “X” has 10.0 % of the isotope with mass 55 amu, 20.0 % of the isotope with mass 56 amu, and 70.0 % of the isotope with mass 57 amu. Estimate the atomic mass of element X. ...
File - Science by Shaw
... ◦ Total Mass Number and Total Atomic Number must be equal on each side of the equation ...
... ◦ Total Mass Number and Total Atomic Number must be equal on each side of the equation ...
Earth Chemistry
... • Found by calculating the weighted average of the atomic masses of the naturally occurring isotopes ...
... • Found by calculating the weighted average of the atomic masses of the naturally occurring isotopes ...
Elements - Heartland
... Ernest Rutherford performed an experiment called the “Gold Foil” experiment in 1911. He used an alpha particle (2P + 2N) source and fired them at a piece of very thin gold foil. He expected all of the particles to pass straight through. However, some were deflected and some were even reflected backw ...
... Ernest Rutherford performed an experiment called the “Gold Foil” experiment in 1911. He used an alpha particle (2P + 2N) source and fired them at a piece of very thin gold foil. He expected all of the particles to pass straight through. However, some were deflected and some were even reflected backw ...
Scientific method
... •Strong force = the force between nucleons (protons and neutrons). • Neutrons increase the attraction ...
... •Strong force = the force between nucleons (protons and neutrons). • Neutrons increase the attraction ...
The Atom
... A. To find the number of neutrons an atom has 1. First you have to know the number of protons – that’s the atomic number 2. Then you have to know the atomic mass number 3. When you subtract the atomic number from the mass number rounded to nearest whole number 4. You get the number of neutrons Mass ...
... A. To find the number of neutrons an atom has 1. First you have to know the number of protons – that’s the atomic number 2. Then you have to know the atomic mass number 3. When you subtract the atomic number from the mass number rounded to nearest whole number 4. You get the number of neutrons Mass ...
EXPERIMENT
... In this experiment, you will be looking at some elements in the laboratory display. Some look different from each other, while others look similar. Elements can be categorized in several ways. In this experiment, you are going to group elements by similarities in their physical properties. Elements ...
... In this experiment, you will be looking at some elements in the laboratory display. Some look different from each other, while others look similar. Elements can be categorized in several ways. In this experiment, you are going to group elements by similarities in their physical properties. Elements ...
Chapter 4 Section 4.3
... • The mass that is listed on the periodic table is an average atomic mass. • It is a weighted average of the atomic masses of naturally occurring isotopes. ...
... • The mass that is listed on the periodic table is an average atomic mass. • It is a weighted average of the atomic masses of naturally occurring isotopes. ...
gp - fc2009goran
... • Iodine is one of the earliest elements whose radioisotopes were used in what is now called nuclear medicine. The most common, stable form of iodine has an atomic number of 53 (protons) and an atomic weight of 127 (53 protons plus 74 neutrons). Because its nucleus has the "correct" number of neutro ...
... • Iodine is one of the earliest elements whose radioisotopes were used in what is now called nuclear medicine. The most common, stable form of iodine has an atomic number of 53 (protons) and an atomic weight of 127 (53 protons plus 74 neutrons). Because its nucleus has the "correct" number of neutro ...
Nature of Matter
... • If we change the atomic number, we change the element we are talking about… ...
... • If we change the atomic number, we change the element we are talking about… ...
Ch - TeacherWeb
... Modern atomic theory knows atoms are divisible (a change from Dalton’s theory). There are three subatomic particles: electrons (e-), protons (p+),and neutrons (n0). ...
... Modern atomic theory knows atoms are divisible (a change from Dalton’s theory). There are three subatomic particles: electrons (e-), protons (p+),and neutrons (n0). ...
AlBr3 E IO Ionic FU C O Cov Molec C IO Cov Molec Sn E N/A N/A
... old bonds between atoms are broken down and new bonds are formed. Atoms, however, can be created or destroyed in nuclear reactions: radioactive decays, nuclear fission and fusion. ...
... old bonds between atoms are broken down and new bonds are formed. Atoms, however, can be created or destroyed in nuclear reactions: radioactive decays, nuclear fission and fusion. ...
Physical Science
... D. It is the measure of the amount of nitrogen in the atmosphere. Nitrogen is only a part of what makes up all of the air molecules pushing down on a surface. S.C.8.4.3b DOK1 ...
... D. It is the measure of the amount of nitrogen in the atmosphere. Nitrogen is only a part of what makes up all of the air molecules pushing down on a surface. S.C.8.4.3b DOK1 ...
Atomic number - KCPE-KCSE
... atom loses or gains one or more electrons. Lithium atom (uncharged) ...
... atom loses or gains one or more electrons. Lithium atom (uncharged) ...
Chem 200 Dr. Saidane
... b) Atoms of a given element are identical in size, mass, and other properties. c) Atoms cannot be subdivided, created, or destroyed. This statement explains the law of conservation of mass. d) Atoms of different elements combine in simple whole-number ratios to form chemical compounds. This explains ...
... b) Atoms of a given element are identical in size, mass, and other properties. c) Atoms cannot be subdivided, created, or destroyed. This statement explains the law of conservation of mass. d) Atoms of different elements combine in simple whole-number ratios to form chemical compounds. This explains ...
Protons, electrons and neutrons worksheet
... Atomic symbol is the symbol you find for each element shown in the periodic table. Magnesium symbol is Mg Gold symbol is Au Potassium symbol is K Phosphorous symbol is P Note: First letter of the element is not always the symbol. Atomic number is the number on the top left of atomic symbol in period ...
... Atomic symbol is the symbol you find for each element shown in the periodic table. Magnesium symbol is Mg Gold symbol is Au Potassium symbol is K Phosphorous symbol is P Note: First letter of the element is not always the symbol. Atomic number is the number on the top left of atomic symbol in period ...
The Periodic Table, Atomic Structure, Isotopes, Ions and Nomenclature
... • The nuclei of most naturally occurring isotopes are very stable, despite the massive repulsive forces that exist between the protons in the nucleus. • A strong force of attraction between neutrons and protons known as the nuclear force counteracts this repulsion. • As the number of protons increas ...
... • The nuclei of most naturally occurring isotopes are very stable, despite the massive repulsive forces that exist between the protons in the nucleus. • A strong force of attraction between neutrons and protons known as the nuclear force counteracts this repulsion. • As the number of protons increas ...
Chapter 3
... 17. What did the English physicist J. J. Thomson conclude?______________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ 18. Cathode rays have _____________ ...
... 17. What did the English physicist J. J. Thomson conclude?______________________________________ ___________________________________________________________________________________ ___________________________________________________________________________________ 18. Cathode rays have _____________ ...
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.