CHAPTER6_MEET_THE_ELEMENTS
... 1. What are the 4 main gases found in our atmosphere? 2. Why is photosynthesis vital for life on Earth? 3. What is the hydrosphere? 4. List one element and 4 compounds found in our hydrosphere? 5. What is the importance of dissolved 02 and CO2 in our hydrosphere? 6. List the four most common element ...
... 1. What are the 4 main gases found in our atmosphere? 2. Why is photosynthesis vital for life on Earth? 3. What is the hydrosphere? 4. List one element and 4 compounds found in our hydrosphere? 5. What is the importance of dissolved 02 and CO2 in our hydrosphere? 6. List the four most common element ...
atomic-models
... • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
... • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
Name: Date: ______ Period: Unit 3 – Atomic Structure Review
... 1. Who was the ancient Greek philosopher who first proposed the notion of the atom? Democritus 2. What was Dalton’s atomic model called? Billard ball model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? Did not have an in ...
... 1. Who was the ancient Greek philosopher who first proposed the notion of the atom? Democritus 2. What was Dalton’s atomic model called? Billard ball model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? Did not have an in ...
04 Mass Spectrometer and Isotopes
... are atoms of the same element (same # protons) with a different # of neutrons. Therefore they have different atomic masses. Because isotopes have different atomic masses, this is usually indicated in the name. Example Hydrogen-2 This isotope has a mass of 2 g/mol. The atomic mass of an element i ...
... are atoms of the same element (same # protons) with a different # of neutrons. Therefore they have different atomic masses. Because isotopes have different atomic masses, this is usually indicated in the name. Example Hydrogen-2 This isotope has a mass of 2 g/mol. The atomic mass of an element i ...
Atomic Mass
... same number of neutrons. •Isotopes are atoms of the same element with different numbers of neutrons. •Isotope symbol: ...
... same number of neutrons. •Isotopes are atoms of the same element with different numbers of neutrons. •Isotope symbol: ...
Chapter 1
... Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, wi ...
... Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, wi ...
Chapter 18 – Atoms and Elements
... On your own, complete Atomic Structures, raise your hand when you are finished and I will check your answers ...
... On your own, complete Atomic Structures, raise your hand when you are finished and I will check your answers ...
Alpha Decay Alpha decay can most simply be described like this: 1
... Gamma radiation ( ) is the emission of high energy photons in the range of 10-10 m, with no matter associated with it. Gamma rays are normally the by-products of other alpha or beta emissions. Gamma rays have no effect on either mass or charge, gamma rays only stabilize the nucleus by releasing some ...
... Gamma radiation ( ) is the emission of high energy photons in the range of 10-10 m, with no matter associated with it. Gamma rays are normally the by-products of other alpha or beta emissions. Gamma rays have no effect on either mass or charge, gamma rays only stabilize the nucleus by releasing some ...
ATOMS AND ELEMENTS
... they are written in a very specific way. 1. Capitalize the first letter of the element name, like C for carbon. 2. Capitalize the first letter of the element name and then make the second letter of the element’s name small case, like Ca for calcium. 3. Sometimes the element’s symbol does not seem to ...
... they are written in a very specific way. 1. Capitalize the first letter of the element name, like C for carbon. 2. Capitalize the first letter of the element name and then make the second letter of the element’s name small case, like Ca for calcium. 3. Sometimes the element’s symbol does not seem to ...
Unit III * Introduction to Atomic Theory
... • Atomic Mass Unit: (amu) – Unit of mass for atomic nuclei – 1 amu = 1/12 the mass of Carbon-12 ...
... • Atomic Mass Unit: (amu) – Unit of mass for atomic nuclei – 1 amu = 1/12 the mass of Carbon-12 ...
Chapter 3 Review
... 11. Write a nuclear equation for the alpha decay of 23191Pa. (ANS: 23191Pa 22789Ac + 42) 12. Write a nuclear equation for the beta decay of 23191Pa. (ANS: 23191Pa 23192U + 01) 13. Compare the penetrating power of alpha, beta, and gamma radiation. (ANS: alpha has the least, then beta and gamm ...
... 11. Write a nuclear equation for the alpha decay of 23191Pa. (ANS: 23191Pa 22789Ac + 42) 12. Write a nuclear equation for the beta decay of 23191Pa. (ANS: 23191Pa 23192U + 01) 13. Compare the penetrating power of alpha, beta, and gamma radiation. (ANS: alpha has the least, then beta and gamm ...
Packet 5
... Protons – Positive charge, found in the nucleus and have a mass of 1 amu. ( Identify) Neutrons- No charge, found in the nucleus, and have a mass of 1 amu ( Isotopes) Electrons- Negative charge, found in the energy levels outside of the nucleus, have relatively no mass ( Ions) ...
... Protons – Positive charge, found in the nucleus and have a mass of 1 amu. ( Identify) Neutrons- No charge, found in the nucleus, and have a mass of 1 amu ( Isotopes) Electrons- Negative charge, found in the energy levels outside of the nucleus, have relatively no mass ( Ions) ...
Early Atomic Theorists
... All elements are composed of tiny indivisible particles called atoms. Atoms of the same element are identical. Atoms of any one element are different from those of any other element. Atoms cannot be created, divided into smaller particles or destroyed. Atoms of different elements can physically ...
... All elements are composed of tiny indivisible particles called atoms. Atoms of the same element are identical. Atoms of any one element are different from those of any other element. Atoms cannot be created, divided into smaller particles or destroyed. Atoms of different elements can physically ...
Counting Atoms
... majority of the volume of the atom? • What is the charge of the nucleus? • What is the overall charge of an atom? ...
... majority of the volume of the atom? • What is the charge of the nucleus? • What is the overall charge of an atom? ...
elements and isotopes - vocabulary
... A species of atom; each atom of a particular element has a specific number of protons in the nucleus which is the same for all atoms of the element. isotope A species of atom; each atom of a particular isotope has a specific number of protons and a specific number of neutrons in the nucleus which ar ...
... A species of atom; each atom of a particular element has a specific number of protons in the nucleus which is the same for all atoms of the element. isotope A species of atom; each atom of a particular isotope has a specific number of protons and a specific number of neutrons in the nucleus which ar ...
Atomic mass - cloudfront.net
... Atomic mass The element name, atomic number, and symbol are pretty easy to understand. The atomic mass is a little trickier. The atomic mass of an element is based on the mass of the atoms that make up the element. The mass of the atoms is based on the protons, neutrons, and electrons of the atoms. ...
... Atomic mass The element name, atomic number, and symbol are pretty easy to understand. The atomic mass is a little trickier. The atomic mass of an element is based on the mass of the atoms that make up the element. The mass of the atoms is based on the protons, neutrons, and electrons of the atoms. ...
19. Define the law of multiple proportions. Elements form
... 19. Define the law of multiple proportions. Elements form compounds in simple whole number ratios 20. What do isotopes of the same element have in common and what is different? Isotopes have the same number of protons, electrons and atomic number Isotopes have a different mass number and number of n ...
... 19. Define the law of multiple proportions. Elements form compounds in simple whole number ratios 20. What do isotopes of the same element have in common and what is different? Isotopes have the same number of protons, electrons and atomic number Isotopes have a different mass number and number of n ...
- Catalyst
... therefore they differ in mass (more on amu in Ch 3). • Many isotopes occur in nature. Most natural isotopes are not radioactive, nor are they necessarily harmful. • A sample of an element will contain some percentage of all its isotopes. ...
... therefore they differ in mass (more on amu in Ch 3). • Many isotopes occur in nature. Most natural isotopes are not radioactive, nor are they necessarily harmful. • A sample of an element will contain some percentage of all its isotopes. ...
Chemical Equations - Warren County Schools
... results: a small portion of the particles were deflected, indicating a small, concentrated positive charge. Note that the image is not to scale; in reality the nucleus is vastly smaller than the electron shell. ...
... results: a small portion of the particles were deflected, indicating a small, concentrated positive charge. Note that the image is not to scale; in reality the nucleus is vastly smaller than the electron shell. ...
Name: Date: ______ Period: Unit 3 – Atomic Structure Review
... 1. Who was the ancient Greek philosopher who first proposed the notion of the atom? Democritus 2. What was Dalton’s atomic model called? Billard ball model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? Did not have an in ...
... 1. Who was the ancient Greek philosopher who first proposed the notion of the atom? Democritus 2. What was Dalton’s atomic model called? Billard ball model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? Did not have an in ...
Isotopes and Mass Number
... Calculating Atomic Mass Atomic Mass is the average of all an element’s masses You need two values ...
... Calculating Atomic Mass Atomic Mass is the average of all an element’s masses You need two values ...
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.