Chapter 4 Atomic Structure
... History of the Atom Democritus (Greek 460-370 BC) • 1st to use the word atom • Believed that atoms were indivisible & indestructible • No scientific support Aristotle (Greek 384-322 BC) • Rejected the theory of atoms • Believed in 4 core elements fire, air, water, earth ...
... History of the Atom Democritus (Greek 460-370 BC) • 1st to use the word atom • Believed that atoms were indivisible & indestructible • No scientific support Aristotle (Greek 384-322 BC) • Rejected the theory of atoms • Believed in 4 core elements fire, air, water, earth ...
Introduction to the Atom
... The amu is the measurement of weight of an atom. The amu is the atom mass units. The amu system of measurement assigns one (1) amu to both protons and neutrons. The atomic number represents the number of protons an atom contains in the nucleus. An example is oxygen. The atomic number of oxygen is ...
... The amu is the measurement of weight of an atom. The amu is the atom mass units. The amu system of measurement assigns one (1) amu to both protons and neutrons. The atomic number represents the number of protons an atom contains in the nucleus. An example is oxygen. The atomic number of oxygen is ...
CHE111-2 Atoms Molecules Ions
... Atoms of an element often have isotopes-atoms that have the same atomic number but different mass numbers. The mass number, A, of an element, X, is written in the upper left hand corner of the element as such: AX. The atomic number of an element, Z, is written in the lower left hand corner of the e ...
... Atoms of an element often have isotopes-atoms that have the same atomic number but different mass numbers. The mass number, A, of an element, X, is written in the upper left hand corner of the element as such: AX. The atomic number of an element, Z, is written in the lower left hand corner of the e ...
Early Atomic Theories
... • The English schoolteacher John Dalton (1766-1844) began the development of modern atomic theory. • Dalton revived and revised Democritus’ ideas based upon the results of his scientific research. ...
... • The English schoolteacher John Dalton (1766-1844) began the development of modern atomic theory. • Dalton revived and revised Democritus’ ideas based upon the results of his scientific research. ...
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ChemChapter_3[1]
... whole numbers. J.L. GayLussac. • Equal volumes of gases, under the same conditions of temperature and pressure, have the same number of molecules. Amedeo Avogadro. ...
... whole numbers. J.L. GayLussac. • Equal volumes of gases, under the same conditions of temperature and pressure, have the same number of molecules. Amedeo Avogadro. ...
Ch - TeacherWeb
... Atom – the smallest particle of an element with all the properties of that element (Greece 460-370 BC) – atoms are individual and indestructible – based on philosophy not experimentation Democritus ...
... Atom – the smallest particle of an element with all the properties of that element (Greece 460-370 BC) – atoms are individual and indestructible – based on philosophy not experimentation Democritus ...
CHAPTER 1 Practice Exercises 1.1 12.3 g Cd 1.3 26.9814 u 1.5
... An element is a chemical species comprised of only a single type of atom. A compound is a chemical species comprised of two or more elements in a definite and unchanging proportion. A reactant is a chemical species which is transformed in a chemical reaction A chemical reaction is a process whereby ...
... An element is a chemical species comprised of only a single type of atom. A compound is a chemical species comprised of two or more elements in a definite and unchanging proportion. A reactant is a chemical species which is transformed in a chemical reaction A chemical reaction is a process whereby ...
File - Home 15-16
... Dalton (1766-1844), a schoolteacher in England, marks the beginning of the development of modern atomic theory. Dalton revived and revised Democritus’s ideas based upon the results of scientific research he conducted. The main points of Dalton’s atomic theory are shown below. Dalton’s Atomic Theory ...
... Dalton (1766-1844), a schoolteacher in England, marks the beginning of the development of modern atomic theory. Dalton revived and revised Democritus’s ideas based upon the results of scientific research he conducted. The main points of Dalton’s atomic theory are shown below. Dalton’s Atomic Theory ...
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... Since electrons have a negative charge, the atom that gains electrons becomes a negatively charged ions (aka anion) because it now has more electrons than protons. Alternately, an atom that looses electrons becomes a positively charged ion (aka cations). The particles in an ionic compound are held t ...
... Since electrons have a negative charge, the atom that gains electrons becomes a negatively charged ions (aka anion) because it now has more electrons than protons. Alternately, an atom that looses electrons becomes a positively charged ion (aka cations). The particles in an ionic compound are held t ...
John Dalton
... which they exist and move. He theorized that atoms are eternal and invisible; absolutely small, so small that their size cannot be diminished (hence the name atomon, or “indivisible”). He believed that all atoms were the same, but had different shapes. Because there were unlimited possibilities of h ...
... which they exist and move. He theorized that atoms are eternal and invisible; absolutely small, so small that their size cannot be diminished (hence the name atomon, or “indivisible”). He believed that all atoms were the same, but had different shapes. Because there were unlimited possibilities of h ...
The Development of Atomic Theory
... • Aristotle was a very famous Greek philosopher who believed that matter could be divided into smaller and smaller pieces forever. • He held a very strong influence on popular belief and his views on this were accepted for two thousand years. ...
... • Aristotle was a very famous Greek philosopher who believed that matter could be divided into smaller and smaller pieces forever. • He held a very strong influence on popular belief and his views on this were accepted for two thousand years. ...
Chapter 2 Notes
... Electron Orbitals • An orbital is the three-dimensional space where an electron is found 90% of the time • Each electron shell consists of a specific number of orbitals ...
... Electron Orbitals • An orbital is the three-dimensional space where an electron is found 90% of the time • Each electron shell consists of a specific number of orbitals ...
Atoms 8.8a Describe the structure and parts of an atoms. Verb
... – Give up all the electrons in the outer energy level – Steal electrons to complete their outer energy level ...
... – Give up all the electrons in the outer energy level – Steal electrons to complete their outer energy level ...
matter
... Rutherford's deductions • Most of the volume of an atom must be empty space • Most of the mass of an atom must be located in the centre of the atom, he called this the nucleus. • The electrons occupy the empty space, and revolve around the nucleus in a circular motion. • The small proportion of alp ...
... Rutherford's deductions • Most of the volume of an atom must be empty space • Most of the mass of an atom must be located in the centre of the atom, he called this the nucleus. • The electrons occupy the empty space, and revolve around the nucleus in a circular motion. • The small proportion of alp ...
matter older versions
... Rutherford's deductions • Most of the volume of an atom must be empty space • Most of the mass of an atom must be located in the centre of the atom, he called this the nucleus. • The electrons occupy the empty space, and revolve around the nucleus in a circular motion. • The small proportion of alp ...
... Rutherford's deductions • Most of the volume of an atom must be empty space • Most of the mass of an atom must be located in the centre of the atom, he called this the nucleus. • The electrons occupy the empty space, and revolve around the nucleus in a circular motion. • The small proportion of alp ...
Writing Chemical Equations KClO3 O2 (g) + KCl (s) Balancing
... chloride, liquid water and gaseous carbon dioxide. Example2: Oxygen gas can be made by heating potassium chlorate in the presence of the catalyst manganese(IV) oxide. Potassium chloride is left as a solid residue. The equation would look like: ...
... chloride, liquid water and gaseous carbon dioxide. Example2: Oxygen gas can be made by heating potassium chlorate in the presence of the catalyst manganese(IV) oxide. Potassium chloride is left as a solid residue. The equation would look like: ...
chapter_3_study_guide
... significantly four times. In 1897 an British physicist __________________________introduced the first model of the atom to include negatively charged particles called ______________________. note: (Later, a different Thompson named ___________________ Thompson reasoned that the atom might be a unifo ...
... significantly four times. In 1897 an British physicist __________________________introduced the first model of the atom to include negatively charged particles called ______________________. note: (Later, a different Thompson named ___________________ Thompson reasoned that the atom might be a unifo ...
Learning Objectives
... b. atomic number and mass number c. atomic weight and mass number 5. Explain how the atomic number and mass number of an atom can be used to determine the number of neutrons. 6. Explain how two isotopes of an element are similar. Explain how they are different. 7. Describe two biological application ...
... b. atomic number and mass number c. atomic weight and mass number 5. Explain how the atomic number and mass number of an atom can be used to determine the number of neutrons. 6. Explain how two isotopes of an element are similar. Explain how they are different. 7. Describe two biological application ...
Inquiry into Life Twelfth Edition
... • As radioactive isotopes decay, energy is released in the form of subatomic particles ...
... • As radioactive isotopes decay, energy is released in the form of subatomic particles ...
Inquiry into Life Twelfth Edition
... • As radioactive isotopes decay, energy is released in the form of subatomic particles ...
... • As radioactive isotopes decay, energy is released in the form of subatomic particles ...
PreAP Chapter 3 Notes
... ________________________________________ states that the elements in a specific compound always contain the same proportions by mass ________________________________________ states that if two or more different compounds are composed of the same two elements, then the ratio of the masses of the seco ...
... ________________________________________ states that the elements in a specific compound always contain the same proportions by mass ________________________________________ states that if two or more different compounds are composed of the same two elements, then the ratio of the masses of the seco ...
Development of Atomic Theory: Rutherford to Modern Theory
... Can we predict where an electron may be found? Electron clouds exist at a certain Energy Level. Therefore the energy that an electron has is based on what? Explain how the bookshelves in Fig. 9 can help you understand the movement of electrons in an atom. Atoms are very small. How many atoms cou ...
... Can we predict where an electron may be found? Electron clouds exist at a certain Energy Level. Therefore the energy that an electron has is based on what? Explain how the bookshelves in Fig. 9 can help you understand the movement of electrons in an atom. Atoms are very small. How many atoms cou ...
Academic Chemistry
... 9. Rutherford’s gold-foil experiment demonstrated that ________ A. electrons have a negative charge B. most of the atom is empty space C. X-rays are characteristic of the metal used as the anode D. energy is given off in little packets 10. Oxygen – 18 has an atomic number of 8. How many neutrons do ...
... 9. Rutherford’s gold-foil experiment demonstrated that ________ A. electrons have a negative charge B. most of the atom is empty space C. X-rays are characteristic of the metal used as the anode D. energy is given off in little packets 10. Oxygen – 18 has an atomic number of 8. How many neutrons do ...
History of molecular theory
In chemistry, the history of molecular theory traces the origins of the concept or idea of the existence of strong chemical bonds between two or more atoms.The modern concept of molecules can be traced back towards pre-scientific Greek philosophers such as Leucippus who argued that all the universe is composed of atoms and voids. Circa 450 BC Empedocles imagined fundamental elements (fire (20px), earth (20px), air (20px), and water (20px)) and ""forces"" of attraction and repulsion allowing the elements to interact. Prior to this, Heraclitus had claimed that fire or change was fundamental to our existence, created through the combination of opposite properties. In the Timaeus, Plato, following Pythagoras, considered mathematical entities such as number, point, line and triangle as the fundamental building blocks or elements of this ephemeral world, and considered the four elements of fire, air, water and earth as states of substances through which the true mathematical principles or elements would pass. A fifth element, the incorruptible quintessence aether, was considered to be the fundamental building block of the heavenly bodies. The viewpoint of Leucippus and Empedocles, along with the aether, was accepted by Aristotle and passed to medieval and renaissance Europe. A modern conceptualization of molecules began to develop in the 19th century along with experimental evidence for pure chemical elements and how individual atoms of different chemical substances such as hydrogen and oxygen can combine to form chemically stable molecules such as water molecules.