NAME GRADED: LET IT BEGIN!!! ____ / 30 pts DIRECTIONS: Use
... Necessary Background: When an isotope is a nuclear radioactive isotope, it means that it can spontaneously breakdown, by emitting alpha particles (effectively He-4 nuclei each equaling 2 protons and 2 neutrons, and of course, 0 electrons), beta particles (high speed e- from degenerating neutrons) or ...
... Necessary Background: When an isotope is a nuclear radioactive isotope, it means that it can spontaneously breakdown, by emitting alpha particles (effectively He-4 nuclei each equaling 2 protons and 2 neutrons, and of course, 0 electrons), beta particles (high speed e- from degenerating neutrons) or ...
study guide - atomic srtucture/_classification of matter
... idea that all things were made of particles too small to see. He was laughed at. In the 1800’s John Dalton proposed the idea of the “Atomic Theory”. He had 5 theories, 3 of which are still believed today. They are: 1. All matter is composed of extremely small particles too small to see 2. In reactio ...
... idea that all things were made of particles too small to see. He was laughed at. In the 1800’s John Dalton proposed the idea of the “Atomic Theory”. He had 5 theories, 3 of which are still believed today. They are: 1. All matter is composed of extremely small particles too small to see 2. In reactio ...
chapter-7-explore-page-248-protons-neutrons
... The mass of electrons is much smaller than the mass of protons or neutrons. That means that most of the mass of an atom is found in the nucleus. Different Elements --- Different Numbers of Protons The number of protons in the atom of an element is the element’s atomic number. The atomic number ...
... The mass of electrons is much smaller than the mass of protons or neutrons. That means that most of the mass of an atom is found in the nucleus. Different Elements --- Different Numbers of Protons The number of protons in the atom of an element is the element’s atomic number. The atomic number ...
History leading to the creation of the atomic bomb
... atomic bomb Atomic science began many centuries ago with experimenting and probing into the nature and structure of matter. This began with ancient philosophers and alchemists. Science began emerging with Thales of Miletus (634-546 BC), the Ionian Greek, who described the power of attraction in elec ...
... atomic bomb Atomic science began many centuries ago with experimenting and probing into the nature and structure of matter. This began with ancient philosophers and alchemists. Science began emerging with Thales of Miletus (634-546 BC), the Ionian Greek, who described the power of attraction in elec ...
Basic structure of atoms
... • Electrons move very rapidly in complicated paths called orbitals. • Because of this motion, they appear to form a cloud. – Negative charge -1 – Mass: 9.1 x10-28 grams – Symbols include e-, -1e0 ...
... • Electrons move very rapidly in complicated paths called orbitals. • Because of this motion, they appear to form a cloud. – Negative charge -1 – Mass: 9.1 x10-28 grams – Symbols include e-, -1e0 ...
Nature of Matter
... Element – a pure substance that consists entirely of one type of atom. -Over 100 elements are known, but only about 24 are found in living organisms. -Elements are represented by symbols, Ex : C = Carbon, H = Hydrogen, etc. -An element’s atomic number = # protons in an atom of the element. ...
... Element – a pure substance that consists entirely of one type of atom. -Over 100 elements are known, but only about 24 are found in living organisms. -Elements are represented by symbols, Ex : C = Carbon, H = Hydrogen, etc. -An element’s atomic number = # protons in an atom of the element. ...
Integrated Science 3
... 18. As your eyes move across the periodic table from left to right in the second period the atomic radii gets ____________. Explain this pattern. What happens to ionization energy across a period? 19. What is true about the element immediately below the element that has an atomic number 17 in the pe ...
... 18. As your eyes move across the periodic table from left to right in the second period the atomic radii gets ____________. Explain this pattern. What happens to ionization energy across a period? 19. What is true about the element immediately below the element that has an atomic number 17 in the pe ...
isotopes
... • Isotopes are atoms of the same element that have the same number of protons but a different number of neutrons. • All elements consist of naturally occurring isotopes and artificially produced isotopes ...
... • Isotopes are atoms of the same element that have the same number of protons but a different number of neutrons. • All elements consist of naturally occurring isotopes and artificially produced isotopes ...
Atomic Number, Mass Number, and Isotopes
... example, carbon-14, commonly used to date biological objects (up to approximately 50,000 years old), has six protons (Z=6) and eight neutrons. To determine the number of neutrons in an isotope: Mass Number = Atomic Number + Number of Neutrons For Carbon-14: ...
... example, carbon-14, commonly used to date biological objects (up to approximately 50,000 years old), has six protons (Z=6) and eight neutrons. To determine the number of neutrons in an isotope: Mass Number = Atomic Number + Number of Neutrons For Carbon-14: ...
Chapter 4
... aver of the masses of all the atoms in the sample. ~mass # - atomic# = #of neutrons ...
... aver of the masses of all the atoms in the sample. ~mass # - atomic# = #of neutrons ...
Honors review- ch. 4 Element Symbol Atomic # Atomic mass
... 1. 65.38 is the average of all the different isotopes of zinc. Protons and neutrons each have a relative mass of 1 amu, so the average mass should not be a fraction of a number. 2. If two atoms have the same number of protons then they are the same element. Atoms of the same element with a different ...
... 1. 65.38 is the average of all the different isotopes of zinc. Protons and neutrons each have a relative mass of 1 amu, so the average mass should not be a fraction of a number. 2. If two atoms have the same number of protons then they are the same element. Atoms of the same element with a different ...
Chemistry Midterm Exam 2015 (Study Guide) Unit 1: Measurement
... b. Zn, 30 protons, 60 electrons d. F, 19 protons, 19 electrons ...
... b. Zn, 30 protons, 60 electrons d. F, 19 protons, 19 electrons ...
File
... 11. What are the rows in the periodic table called and what do they show? periods 12. Using the periodic table, find the element that is found in group 2 period 3. ...
... 11. What are the rows in the periodic table called and what do they show? periods 12. Using the periodic table, find the element that is found in group 2 period 3. ...
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. ...
Topic 4: Classifying Elements What did the early chemists use to
... • NH3(g) à nitrogen trihydride or ammonia • CH4(g) à carbon tetrahydride or methane • H2O2(l) à dihydrogen monoxide or water A MOLECULAR COMPOUND can contain what two combinations of elements? Non-‐metal + ...
... • NH3(g) à nitrogen trihydride or ammonia • CH4(g) à carbon tetrahydride or methane • H2O2(l) à dihydrogen monoxide or water A MOLECULAR COMPOUND can contain what two combinations of elements? Non-‐metal + ...
Topic 2.1 The Nuclear Atom
... • this is NOT IB material until indicated • it is very interesting from a geeky-science stand point • it will help you understand and appreciate the structure of the atom • you are not responsible for knowing the information from all thescientists ...
... • this is NOT IB material until indicated • it is very interesting from a geeky-science stand point • it will help you understand and appreciate the structure of the atom • you are not responsible for knowing the information from all thescientists ...
Atomic Structure Test Review 2016
... You may need to check your notes for some definitions. Remember, resources are on ItsLearning. ...
... You may need to check your notes for some definitions. Remember, resources are on ItsLearning. ...
2.9 Use the helium-4 isotope to define atomic number and mass
... 2.34 Give two examples of each of the following: (a) a diatomic molecule containing atoms of the same element, (b) a diatomic molecule containing atoms of different elements, (c) polyatomic molecule containing atoms of the same element, (d) a polyatomic molecule containing atoms of different element ...
... 2.34 Give two examples of each of the following: (a) a diatomic molecule containing atoms of the same element, (b) a diatomic molecule containing atoms of different elements, (c) polyatomic molecule containing atoms of the same element, (d) a polyatomic molecule containing atoms of different element ...
Unit 10 Test Review
... b. movement of electrons from higher energy states to lower energy states. c. movement of electrons from lower energy states to higher energy states. d. movement of electrons as they fall into the nucleus. 11. How many neutrons are contained in an atom of strontium-88? 12. Which of the following rep ...
... b. movement of electrons from higher energy states to lower energy states. c. movement of electrons from lower energy states to higher energy states. d. movement of electrons as they fall into the nucleus. 11. How many neutrons are contained in an atom of strontium-88? 12. Which of the following rep ...
Exemplar exam question – Chapter 2
... The first answer is probably worthy of only 1 mark as it does not make clear that isotopes are different atoms of the same element. The second answer would probably score 0. Although the idea of the same element and different number of neutrons is mentioned, the student has not mentioned different a ...
... The first answer is probably worthy of only 1 mark as it does not make clear that isotopes are different atoms of the same element. The second answer would probably score 0. Although the idea of the same element and different number of neutrons is mentioned, the student has not mentioned different a ...
Two valence electrons.
... elements by increasing atomic mass, leaving blank spaces where he was sure elements Dmitri yet to be discovered Mendeleev would fit. ...
... elements by increasing atomic mass, leaving blank spaces where he was sure elements Dmitri yet to be discovered Mendeleev would fit. ...
Nuclear Chemistry
... • Produces even more energy per gram of fuel than fission. • Produces less nuclear waste than fission. • Fusion fuel is easy to get. (Heavy hydrogen is found in ...
... • Produces even more energy per gram of fuel than fission. • Produces less nuclear waste than fission. • Fusion fuel is easy to get. (Heavy hydrogen is found in ...
Slide 1
... Tiny indivisible particles called atoms Atoms of the same element are identical Can combine to form compounds Chemical reactions occur when atoms are separated, joined, or rearranged, but atoms of one element are not changed into atoms of another by a chemical reaction ...
... Tiny indivisible particles called atoms Atoms of the same element are identical Can combine to form compounds Chemical reactions occur when atoms are separated, joined, or rearranged, but atoms of one element are not changed into atoms of another by a chemical reaction ...
Neptunium
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Neptunium is a chemical element with symbol Np and atomic number 93. A radioactive actinide metal, neptunium is the first transuranic element. Its position in the periodic table just after uranium, named after the planet Uranus, led to it being named after Neptune, the next planet beyond Uranus. A neptunium atom has 93 protons and 93 electrons, of which seven are valence electrons. Neptunium metal is silvery and tarnishes when exposed to air. The element occurs in three allotropic forms and it normally exhibits five oxidation states, ranging from +3 to +7. It is radioactive, pyrophoric, and can accumulate in bones, which makes the handling of neptunium dangerous.Although many false claims of its discovery were made over the years, the element was first synthesized by Edwin McMillan and Philip H. Abelson at the Berkeley Radiation Laboratory in 1940. Since then, most neptunium has been and still is produced by neutron irradiation of uranium in nuclear reactors. The vast majority is generated as a by-product in conventional nuclear power reactors. While neptunium itself has no commercial uses at present, it is widely used as a precursor for the formation of plutonium-238, used in radioisotope thermal generators. Neptunium has also been used in detectors of high-energy neutrons.The most stable isotope of neptunium, neptunium-237, is a by-product of nuclear reactors and plutonium production. It, and the isotope neptunium-239, are also found in trace amounts in uranium ores due to neutron capture reactions and beta decay.