1 - WordPress.com
... Assume the following three isotopes of element Z exist: Z-248, Z-252, and Z-259. If the atomic mass of Z is 258.63 amu, which of these isotopes is most abundant? Since the atomic mass is the weighted average, the most abundant will be the isotope with the mass number closest to the atomic mass: Z-25 ...
... Assume the following three isotopes of element Z exist: Z-248, Z-252, and Z-259. If the atomic mass of Z is 258.63 amu, which of these isotopes is most abundant? Since the atomic mass is the weighted average, the most abundant will be the isotope with the mass number closest to the atomic mass: Z-25 ...
chapter 2
... d. balance: measures mass (g) e. stirring rod – used to stir solutions f. ruler – used to measure length (cm) ...
... d. balance: measures mass (g) e. stirring rod – used to stir solutions f. ruler – used to measure length (cm) ...
Atomic Structure - Mr. Cervantes Science Classes
... of 1 atomic mass unit (AMU) each it is reasonable to think that the mass of an atom should be expressed as a whole number B. The atomic mass of an element is the weighted average of the masses of all the isotopes of that element 1. When calculating the average atomic mass you must take into account ...
... of 1 atomic mass unit (AMU) each it is reasonable to think that the mass of an atom should be expressed as a whole number B. The atomic mass of an element is the weighted average of the masses of all the isotopes of that element 1. When calculating the average atomic mass you must take into account ...
elements and isotopes - vocabulary
... An isotope whose atoms undergo a detectable radioactive decay. Radioactive isotopes can be naturally occurring or synthetic. radioactive decay Transformation of an unstable atom that produces a more stable atom (or atoms) as well as radiation (energy and energetic particles). synthetic element (isot ...
... An isotope whose atoms undergo a detectable radioactive decay. Radioactive isotopes can be naturally occurring or synthetic. radioactive decay Transformation of an unstable atom that produces a more stable atom (or atoms) as well as radiation (energy and energetic particles). synthetic element (isot ...
Atomic Structure Notes Packet
... John Dalton (1766-1844): used Democritus’s ideas and proposed the first atomic theory in 1803 based on experimentation, which included the following ideas: All ____________ consist of tiny indivisible particles called atoms. Atoms of the same element are ____________, different from those of any oth ...
... John Dalton (1766-1844): used Democritus’s ideas and proposed the first atomic theory in 1803 based on experimentation, which included the following ideas: All ____________ consist of tiny indivisible particles called atoms. Atoms of the same element are ____________, different from those of any oth ...
Practice problems for chapter 1, 2 and 3 1) A small amount of salt
... Practice problems for chapter 1, 2 and 3 1) A small amount of salt dissolved in water is an example of a __________. 2) Which one of the following is a pure substance? A) concrete B) wood C) salt water D) elemental copper E) milk 3) For which of the following can the composition vary? A) pure substa ...
... Practice problems for chapter 1, 2 and 3 1) A small amount of salt dissolved in water is an example of a __________. 2) Which one of the following is a pure substance? A) concrete B) wood C) salt water D) elemental copper E) milk 3) For which of the following can the composition vary? A) pure substa ...
sub
... Deuterium. Deuterium is not radioactive. Water made from deuterium is called heavy water because the extra neutron makes it heavier. It is used in nuclear reactors. The third isotope of hydrogen is known as Tritium. It has one proton and two neutrons in its nucleus. It IS radioactive. It is formed i ...
... Deuterium. Deuterium is not radioactive. Water made from deuterium is called heavy water because the extra neutron makes it heavier. It is used in nuclear reactors. The third isotope of hydrogen is known as Tritium. It has one proton and two neutrons in its nucleus. It IS radioactive. It is formed i ...
Mixtures, Pure Substance and Isotopes
... • How many protons, neutrons, and electrons does this isotope of nitrogen have? Protons: Neutrons: Electrons: ...
... • How many protons, neutrons, and electrons does this isotope of nitrogen have? Protons: Neutrons: Electrons: ...
Atoms, Elements, and the Periodic Table Part 1: The Atomic Model
... Atoms are made mostly out of (+) charged material, like dough in a bun. The (-) charged electrons are found inside the (+) dough. ...
... Atoms are made mostly out of (+) charged material, like dough in a bun. The (-) charged electrons are found inside the (+) dough. ...
Atoms, Elements, and the Periodic Table Part 1: The Atomic Model
... Atoms are made mostly out of (+) charged material, like dough in a bun. The (-) charged electrons are found inside the (+) dough. ...
... Atoms are made mostly out of (+) charged material, like dough in a bun. The (-) charged electrons are found inside the (+) dough. ...
Atomic structure - ISA DP Chemistry with Ms Tsui
... 1. All matter is made of atoms. Atoms are indivisible and indestructible. 2. All atoms of a given element are identical in mass and properties. Atoms of different elements are different 3. Compounds are formed by a combination of two or more different kinds of atoms in specific whole number ratios. ...
... 1. All matter is made of atoms. Atoms are indivisible and indestructible. 2. All atoms of a given element are identical in mass and properties. Atoms of different elements are different 3. Compounds are formed by a combination of two or more different kinds of atoms in specific whole number ratios. ...
Academic Chemistry Chapter 3 Review Activity
... List the three subatomic particles, their symbols, charges and explain where they are located at in the structure of the atom. Proton, p+1, +1 charge, located in the nucleus Neutron, n0, no charge, located in the nucleus Electron, e-1, -1 charge, located in energy levels surrounding the nucleus ...
... List the three subatomic particles, their symbols, charges and explain where they are located at in the structure of the atom. Proton, p+1, +1 charge, located in the nucleus Neutron, n0, no charge, located in the nucleus Electron, e-1, -1 charge, located in energy levels surrounding the nucleus ...
Name: Per: ______ Atoms: The Building Blocks of Matter Atoms
... positively (+) charged particles called ____________________ and one or more (=) neutral particles called _____________________. 2.Electron cloud: A region very _______________ compared to the nucleus which contains very small negatively (-) charged particles called ___________________________. ...
... positively (+) charged particles called ____________________ and one or more (=) neutral particles called _____________________. 2.Electron cloud: A region very _______________ compared to the nucleus which contains very small negatively (-) charged particles called ___________________________. ...
Atoms - Mrs. Carlyle`s Classroom
... Dalton’s atomic theory explains all three of these laws. ◦ All elements were composed of atoms and that only whole numbers of atoms can combine to form compounds. The following statements sum up his theory: All matter is composed of extremely small particles called atoms. Atoms of an element are ...
... Dalton’s atomic theory explains all three of these laws. ◦ All elements were composed of atoms and that only whole numbers of atoms can combine to form compounds. The following statements sum up his theory: All matter is composed of extremely small particles called atoms. Atoms of an element are ...
Chapter 3, Part 2 Review Packet
... List the three subatomic particles, their symbols, charges and explain where they are located at in the structure of the atom. Proton, p+1, +1 charge, located in the nucleus Neutron, n0, no charge, located in the nucleus Electron, e-1, -1 charge, located in energy levels surrounding the nucleus ...
... List the three subatomic particles, their symbols, charges and explain where they are located at in the structure of the atom. Proton, p+1, +1 charge, located in the nucleus Neutron, n0, no charge, located in the nucleus Electron, e-1, -1 charge, located in energy levels surrounding the nucleus ...
Atomic Structure – Revision Pack (C4) Atoms: A nucleus is made up
... Arrangement of electrons: The elements of the periodic table are arranged in order of increasing atomic number. The amount of electrons is different for the shells of an atom: The maximum number of electrons for the first shell is 2. The maximum number of electrons for all of the shells from then is ...
... Arrangement of electrons: The elements of the periodic table are arranged in order of increasing atomic number. The amount of electrons is different for the shells of an atom: The maximum number of electrons for the first shell is 2. The maximum number of electrons for all of the shells from then is ...
All About Isotopes
... The atomic number of any atom (element) is a whole number and represents the number of protons in the atom, but that’s not true of atomic mass which is not a whole number. Since atomic mass is the number of the protons plus neutrons in the nucleus does that mean the nucleus of atoms have fractions o ...
... The atomic number of any atom (element) is a whole number and represents the number of protons in the atom, but that’s not true of atomic mass which is not a whole number. Since atomic mass is the number of the protons plus neutrons in the nucleus does that mean the nucleus of atoms have fractions o ...
Atoms overview quiz
... You cannot ever know the exact location of an electron. There will always be some margin of error because they are so small and even light can knock them around. Equations can tell you places you should find them, but never the exact spot at one moment in time. QUESTION 10: Atoms in the same family ...
... You cannot ever know the exact location of an electron. There will always be some margin of error because they are so small and even light can knock them around. Equations can tell you places you should find them, but never the exact spot at one moment in time. QUESTION 10: Atoms in the same family ...
C4 Atomic structure
... Arrangement of electrons: The elements of the periodic table are arranged in order of increasing atomic number. The amount of electrons is different for the shells of an atom: The maximum number of electrons for the first shell is 2. The maximum number of electrons for all of the shells from then is ...
... Arrangement of electrons: The elements of the periodic table are arranged in order of increasing atomic number. The amount of electrons is different for the shells of an atom: The maximum number of electrons for the first shell is 2. The maximum number of electrons for all of the shells from then is ...
PRACTICE PROBLEMS EXAM 1,2 and 3 1311
... Practice problems Chapter 1 Chemical Foundations 1) A small amount of salt dissolved in water is an example of a __________. 2) Which one of the following is a pure substance? A) concrete B) wood C) salt water D) elemental copper E) milk 3) For which of the following can the composition vary? A) pur ...
... Practice problems Chapter 1 Chemical Foundations 1) A small amount of salt dissolved in water is an example of a __________. 2) Which one of the following is a pure substance? A) concrete B) wood C) salt water D) elemental copper E) milk 3) For which of the following can the composition vary? A) pur ...
Grade 11 Chemistry E.. - hrsbstaff.ednet.ns.ca
... 23. Describe the different types of intermolecular forces. 24. Balance the following equations. a. CF4(l) → C(s) + F2(g) b. H2SO4(aq) + KOH(aq) → KHSO4(aq) + H2O(l) c. ZnCl2(aq) + H2(g) → Zn(s) + HCl(aq) d. SO2(g) + H2O(l) + O2(g) → H2SO4(aq) e. Li(s) + H2O(l) → LiOH(aq) + H2(g) f. H2CO3(aq) → H2O(l ...
... 23. Describe the different types of intermolecular forces. 24. Balance the following equations. a. CF4(l) → C(s) + F2(g) b. H2SO4(aq) + KOH(aq) → KHSO4(aq) + H2O(l) c. ZnCl2(aq) + H2(g) → Zn(s) + HCl(aq) d. SO2(g) + H2O(l) + O2(g) → H2SO4(aq) e. Li(s) + H2O(l) → LiOH(aq) + H2(g) f. H2CO3(aq) → H2O(l ...
Study Guide Chapters 4
... Explain what makes elements and isotopes different from each other and the same Construct and understand chemical (shorthand) notation for isotopes of elements ...
... Explain what makes elements and isotopes different from each other and the same Construct and understand chemical (shorthand) notation for isotopes of elements ...
Atomic terms Example: Helium has an atomic number of 2. Every
... - some have chemical reactivity like a nonmetal, but conduct electricity better than nonmetals - some have unusual electrical properties (silicon / germanium diodes) , and are useful in electronics ...
... - some have chemical reactivity like a nonmetal, but conduct electricity better than nonmetals - some have unusual electrical properties (silicon / germanium diodes) , and are useful in electronics ...
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.