Section 2 Powerpoint
... Reviewing Concepts • 1. Name three subatomic particles. • 2. Name three properties you could use to distinguish a proton from an electron. • 3. Which characteristic of an atom always varies among atoms of different elements? • 4. How are the isotopes of an element different from one another? • 5. W ...
... Reviewing Concepts • 1. Name three subatomic particles. • 2. Name three properties you could use to distinguish a proton from an electron. • 3. Which characteristic of an atom always varies among atoms of different elements? • 4. How are the isotopes of an element different from one another? • 5. W ...
History Atomic Theory
... – Know the name, location, charge, and relative mass of each of the subatomic particles in an atom – Know that the atomic number is the number of protons in the nucleus of an atom, and is unique to each element. – Understand that isotopes are atoms of the same element that differ in the number of ne ...
... – Know the name, location, charge, and relative mass of each of the subatomic particles in an atom – Know that the atomic number is the number of protons in the nucleus of an atom, and is unique to each element. – Understand that isotopes are atoms of the same element that differ in the number of ne ...
Chapter 4 The structure of the Atom
... named the nucleus. 13. Who discovered the neutral particle of the atom? James Chadwick 14. Which are the three subatomic particles of the atom? Electron, proton, and neutron Section 4.3 How atoms differ 13. Who stated that the proton is the subatomic particle that identifies an atom from a particula ...
... named the nucleus. 13. Who discovered the neutral particle of the atom? James Chadwick 14. Which are the three subatomic particles of the atom? Electron, proton, and neutron Section 4.3 How atoms differ 13. Who stated that the proton is the subatomic particle that identifies an atom from a particula ...
CHAPTER 3: The Building Blocks of Matter
... UNIT 1: Atomic Theory Part I – Atomic Structure I. Early Atomic Theory□Democritus (400 B.C.)- suggested that the world was made of two things: -empty space and -tiny, indivisible particles called ‘____________’. □Dalton (early 1800s)- using the experimental observations of others, including Lavoisie ...
... UNIT 1: Atomic Theory Part I – Atomic Structure I. Early Atomic Theory□Democritus (400 B.C.)- suggested that the world was made of two things: -empty space and -tiny, indivisible particles called ‘____________’. □Dalton (early 1800s)- using the experimental observations of others, including Lavoisie ...
File
... What is the atomic number for phosphorus ? How many protons does a calcium atom have ? How many electrons does an oxygen atom have ? If Z = 24, identify the element. ...
... What is the atomic number for phosphorus ? How many protons does a calcium atom have ? How many electrons does an oxygen atom have ? If Z = 24, identify the element. ...
Unit 2
... • They concluded that the darkening of the photographic plates was due to rays emitted specifically from the uranium atoms present in the mineral sample. • Marie Curie named the process by which materials, uranium and thorium, give off such rays radioactivity; the rays and particles emitted by a rad ...
... • They concluded that the darkening of the photographic plates was due to rays emitted specifically from the uranium atoms present in the mineral sample. • Marie Curie named the process by which materials, uranium and thorium, give off such rays radioactivity; the rays and particles emitted by a rad ...
SNC 1D Chemistry Review
... A) A pure substance that can’t be broken down into simpler parts. B) A heterogeneous mixture where the different particles are big enough to see and stay mixed. C) A homogeneous mixture of 2 or more substances. D) A pure substance with 2 or more elements chemically combined together. E) A homogeneou ...
... A) A pure substance that can’t be broken down into simpler parts. B) A heterogeneous mixture where the different particles are big enough to see and stay mixed. C) A homogeneous mixture of 2 or more substances. D) A pure substance with 2 or more elements chemically combined together. E) A homogeneou ...
- Los Banos Unified School District
... The nucleus is composed of nucleons (protons & neutrons) The nucleons have the same identical mass of about 1.7 x 10-24 grams. The mass for a proton & neutron is about 2000 times more than the mass of an electron. All atoms of an element have the same number of protons but all atoms of one element ...
... The nucleus is composed of nucleons (protons & neutrons) The nucleons have the same identical mass of about 1.7 x 10-24 grams. The mass for a proton & neutron is about 2000 times more than the mass of an electron. All atoms of an element have the same number of protons but all atoms of one element ...
The parts of Dalton`s theory Matter is composed of small, chemically
... Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. - MASS NUMBER: The number of protons PLUS the number of neutrons in the atomic nucleus, Atoms of the same element may have DIFFERENT mass numbers. - ISOTOPES: are atoms of the same element with different mas ...
... Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. - MASS NUMBER: The number of protons PLUS the number of neutrons in the atomic nucleus, Atoms of the same element may have DIFFERENT mass numbers. - ISOTOPES: are atoms of the same element with different mas ...
Unit 3 - MaxStudy.org
... • An experiment which provides compelling proof for the photon are talking about, we use the symbol: nature of light (also called the particle nature of light) is the photoelectric effect.AIn this effect light is shone at a metal plate, and it is found Z that electrons are ejected. These electrons ...
... • An experiment which provides compelling proof for the photon are talking about, we use the symbol: nature of light (also called the particle nature of light) is the photoelectric effect.AIn this effect light is shone at a metal plate, and it is found Z that electrons are ejected. These electrons ...
Matter and the Periodic Table Study Guide Answer Key
... Semimetals/Metalloids have properties of both metals and non-metals. 3.b. Compounds are formed by combining two or more different elements and compounds have properties that are different from their constituent elements. 3.f. Use the periodic table to identify elements in simple compounds. Compound ...
... Semimetals/Metalloids have properties of both metals and non-metals. 3.b. Compounds are formed by combining two or more different elements and compounds have properties that are different from their constituent elements. 3.f. Use the periodic table to identify elements in simple compounds. Compound ...
Chapter 5
... o Atoms of the same element are identical o Atoms of different elements can physically mix or chemically combine in simple whole-number ratios to form compounds o Chemical reactions occur when atoms are separated, joined, or rearranged, but they are never changed into another element - The radii of ...
... o Atoms of the same element are identical o Atoms of different elements can physically mix or chemically combine in simple whole-number ratios to form compounds o Chemical reactions occur when atoms are separated, joined, or rearranged, but they are never changed into another element - The radii of ...
Atoms, Elements, and Ions
... • The atom is extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water. • If a large sports stadium were an atom, a marble would represent the nucleus. ...
... • The atom is extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water. • If a large sports stadium were an atom, a marble would represent the nucleus. ...
experiment 8 radioactive decay of nuclei
... 4.28% mass 113. (Using the nuclear masses of 114.9041 and 112.9043 instead of the number of nucleons, 115 and 113, the chemical weight of 114.82 can be calculated.) If the indium is placed where there are many free neutrons with kinetic energies, on the order of 0.03 eV, both isotopes In-115 and In- ...
... 4.28% mass 113. (Using the nuclear masses of 114.9041 and 112.9043 instead of the number of nucleons, 115 and 113, the chemical weight of 114.82 can be calculated.) If the indium is placed where there are many free neutrons with kinetic energies, on the order of 0.03 eV, both isotopes In-115 and In- ...
Phys 282 EXP 8
... 4.28% mass 113. (Using the nuclear masses of 114.9041 and 112.9043 instead of the number of nucleons, 115 and 113, the chemical weight of 114.82 can be calculated.) If the indium is placed where there are many free neutrons with kinetic energies, on the order of 0.03 eV, both isotopes In-115 and In- ...
... 4.28% mass 113. (Using the nuclear masses of 114.9041 and 112.9043 instead of the number of nucleons, 115 and 113, the chemical weight of 114.82 can be calculated.) If the indium is placed where there are many free neutrons with kinetic energies, on the order of 0.03 eV, both isotopes In-115 and In- ...
nuclear physics ppt
... A nucleon is a general term to denote a nuclear particle - that is, either a proton or a neutron. The atomic number Z of an element is equal to the number of protons in the nucleus of that element. The mass number A of an element is equal to the total number of nucleons (protons + neutrons). The mas ...
... A nucleon is a general term to denote a nuclear particle - that is, either a proton or a neutron. The atomic number Z of an element is equal to the number of protons in the nucleus of that element. The mass number A of an element is equal to the total number of nucleons (protons + neutrons). The mas ...
Unit 2 Test Review - Liberty High School
... 10. Nitrogen oxide (NO) and nitrogen dioxide (NO2) are both made up of nitrogen and oxygen. Can you assume that they will both have similar physical and chemical properties? Why or why not? 11. An 18-L sample of element A (density 0.84 g/mL combines completely with a 4-L sample of element B (density ...
... 10. Nitrogen oxide (NO) and nitrogen dioxide (NO2) are both made up of nitrogen and oxygen. Can you assume that they will both have similar physical and chemical properties? Why or why not? 11. An 18-L sample of element A (density 0.84 g/mL combines completely with a 4-L sample of element B (density ...
Section 2A
... Origins of the Periodic Table In 1869, approximately 62 elements were known to exist. Scientists wanted a convenient way to look at these elements. Dmitri Mendeleev proposed a periodic table of elements. It was arranged by increasing mass number and similar properties. Later, Henry Mosley working wi ...
... Origins of the Periodic Table In 1869, approximately 62 elements were known to exist. Scientists wanted a convenient way to look at these elements. Dmitri Mendeleev proposed a periodic table of elements. It was arranged by increasing mass number and similar properties. Later, Henry Mosley working wi ...
Unit 10 Test Review
... b. concluded that the particles in the cathode beam had a (–) charge c. discovered the neutron d. based his experiments on results obtained by Rutherford 5. The part of Thomson’s model that was not supported by direct evidence was that a. the atom was a sphere of uniform positive charge. b. the posi ...
... b. concluded that the particles in the cathode beam had a (–) charge c. discovered the neutron d. based his experiments on results obtained by Rutherford 5. The part of Thomson’s model that was not supported by direct evidence was that a. the atom was a sphere of uniform positive charge. b. the posi ...
Another look at chemical reactions HYDROGEN PEROXIDE WATER
... Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. - MASS NUMBER: The number of protons PLUS the number of neutrons in the atomic nucleus, Atoms of the same element may have DIFFERENT mass numbers. - ISOTOPES: are atoms of the same element with different mas ...
... Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. - MASS NUMBER: The number of protons PLUS the number of neutrons in the atomic nucleus, Atoms of the same element may have DIFFERENT mass numbers. - ISOTOPES: are atoms of the same element with different mas ...
Atomic Structure Notes File
... Atoms which have the same number of protons with different amounts of neutrons. Carbon-12 has 6 neutrons, while Carbon14 has 8 neutrons. The mass number for an element on the periodic table represents the average for all the isotopes in a sample of the element. ...
... Atoms which have the same number of protons with different amounts of neutrons. Carbon-12 has 6 neutrons, while Carbon14 has 8 neutrons. The mass number for an element on the periodic table represents the average for all the isotopes in a sample of the element. ...
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 + ...
Chapter 5 The Structure of the Atom
... Students should be able to: • Summarize the essential points of Dalton’s atomic theory. • Describe the particle theory of matter. • Use the Bohr model to differentiate among the three basic particles in an atom • Compare the Bohr atomic model to the electron cloud. ...
... Students should be able to: • Summarize the essential points of Dalton’s atomic theory. • Describe the particle theory of matter. • Use the Bohr model to differentiate among the three basic particles in an atom • Compare the Bohr atomic model to the electron cloud. ...
CHAPTER 4 EXAM: THE NATURE OF THE ATOM (modified)
... ____ 11. How many neutrons are in an atom of chlorine? a. 18 c. 17 b. 35 ____ 12. How many electrons are in an neutral atom of sodium? a. 11 c. 12 b. 22 ____ 13. Which element has 14 electrons? a. Sulfur c. Silicon b. Nitrogen ____ 14. According to the modern concept of the atom, which are located i ...
... ____ 11. How many neutrons are in an atom of chlorine? a. 18 c. 17 b. 35 ____ 12. How many electrons are in an neutral atom of sodium? a. 11 c. 12 b. 22 ____ 13. Which element has 14 electrons? a. Sulfur c. Silicon b. Nitrogen ____ 14. According to the modern concept of the atom, which are located i ...
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.