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Atomic structure and theory
What is the structure of an atom flashcards
Atomic structure and theory
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An atom has three main particles—the proton, neutron, and electron. The first two particles are contained in the center of the atom, which is called the nucleus. Electrons, on the other hand, are outside the nucleus in levels called energy levels. Electrons in higher energy levels are located farther from the nucleus. These energy levels are orbitals—regions of space in which the electrons are most likely to lie. Electrons do not lie in orbits—definite paths that chart which way an object goes and where it is. Since the Heisenberg Uncertainty Principle states that it is impossible to know both the direction and position of an electron at the same time, plotting an orbit for an electron is impossible (“Electron Structure Discussion”).
All stable copper isotopes—atoms of the same element but with different masses--need to be considered before coming up with an average atomic mass for the element. There are two such isotopes, copper-63 and copper-65 (“Isotopes of Copper”). Copper has an atomic number of 29. This means it has 29 protons. All stable isotopes are electrically neutral. Therefore, there must be the same number of electrons as protons. In the case of copper, there are 29 electrons.
However, to account for the fact that they are isotopes, they have different numbers of neutrons. Protons have a relative mass (on the carbon-12 scale) of about one, and electrons 1/1836 (almost no mass). Neutrons, with a mass also of about one, account for the difference in masses of different isotopes (“Electron Structure Discussion”). Therefore, copper-63 has 34 neutrons, and copper-65 has 36 neutrons. The natural abundance of copper-63 is 69.17%, and the abundance of copper-65 is 30.83% (“Isotopes of Copper”).
As for the electrons themselves, they completely fill the first, second, and third shells. In addition, one electron enters the fourth shell. Within the subshells, they are distributed in the electron configuration 1s2 2s2 2p6 3s2 3p6 4s1 3d10. The “s,” “p,” and “d” are labels of types of subshells. S subshells can hold up to two electrons, p subshells can hold up to six, and d subshells up to ten (“Electron Structure Discussion”). So, the electron configuration indicates that the s subshell in the first, second, and third shells are completely filled. Also, the p subshells in shells two and three and the d subshell in shell three are completely filled. However, the s subshell in shell four is only half-filled.
But, only two electrons can fit in an orbital (“Electron Structure Discussion).
In "Energy Story" uses an explanation of atoms and tells us the parts of an atom and its structure. In the text it
Neon has an atomic number of 10, and a mass of 20.180. Neon has three stable isotopes: neon 20, 21, and 22. These three isotopes comprise 90.92 percent of natural neon, 0.26 percent of natural neon, and 8.82 percent of natural neon, respectively. There are five other isotopes of neon, and they are all radioactive. None of these five isotopes occur in nature.
Copper II Sulfide ~ (final mass of compound) _ç3.07g - 2.59gç_ x 100 = 15.6%
Oxygen is the first element on the Oxygen group. That is why the name of the group is named the Oxygen group. It has eight electrons total. It has six in its outer electron cloud. According to the octet rule, the oxygen will want to gain two more electrons to fill its outer shell with eight. Oxygen is also one of th...
Lead in number 82 on the periodic table. Lead is usually found in ore with silver and copper and it is extracted together with them. Lead occurs naturally in the environment. However, most lead that is found in the environment results from human uses such as lead from batteries, gasoline or lead that has escaped into the environment from places like smelters.
Atoms are electrically neutral; the electrons that bear the negative charge are equal in number to the protons in the nucleus
An atom, by definition, is the smallest part of any substance. The atom has three main components that make it up: protons, neutrons, and electrons. The protons and neutrons are within the nucleus in the center of the atom. The electrons revolve around the nucleus in many orbitals. These orbitals consist of many different shapes, including circular, spiral, and many others. Protons are positively charged and electrons are negatively charged. Protons and electrons both have charge of equal magnitude (i.e. 1.602x10-19 coulombs). Neutrons have a neutral charge, and they, along with protons, are the majority of mass in an atom. Electron mass, though, is negligible. When an atom has a neutral charge, it is stable.
The origin of the name "nickel" is a derivative from the German word "kupfernickel", meaning "Devil's Copper" or "St. Nicholas's Copper".The chemical properties of nickel are as follows: Nickel has the atomic number of twenty-eight. The atomic symbol of nickel, "Ni". It has the atomic weight (mass) of 58.70, to be exact, 58.693. It occurs in five stable isotopes. Physically, nickel is a lustrous silvery-white and takes on a hard polish.
Now the octet rule says that an atom likes to achieve stability by ensuring they have eight valence electrons in their outermost level. Atoms lose or gain valence electrons to achieve the full outer level and they do this by bonding with other atoms. Atoms can bond with each other as in the case of O2 or with different atoms as in the case of H2O. (Timberlake) Only Hydrogen (H) and Helium (He) like to only have two valence electrons.
The theory of quantum mechanics has divided the atom into a number of fundamental sub-atomic particles. Although the physicist has shown that the atom is not a solid indivisible object, he has not been able to find a particle which does possess those qualities. Talk of particles, though, is misleading because the word suggests a material object. This is not the intention for the use of the word in quantum physics. Quantum particles are, instead, representations of the actions and reactions of forces at the sub-atomic level. In fact, physicists are less concerned with the search for a material particle underlying all physical objects and more interested in explaining how nature works. Quantum theory is the means that enables the physicist to express those explanations in a scientific way.
In 1938, iodine-131 and cobalt-60 isotopes were discovered by J. Livingood and G. Seaborg. 2
In the beginning of the 1800s John Dalton, an English scientist did work some work on gases, which lead him to the creation of a complex system of symbols for all known elements at the time. He took all the information he had collected, along with the Laws of Conservation of Mass, Definite Composition and Multiple Proportions and updated Aristotle's theory of matter with the Atomic Theory of Matter, which stated: - All matter is composed of tiny, indivisible particles called atoms. - Atoms of an element have identical properties. - Atoms of different elements have different properties. - Atoms of two or more elements can combine in constant ratios to form new substances. In the late 1800s a man named J. J. Thomson did some experiments, who's results did not agree with Dalton's Atomic Theory. Thomson passed electricity though gases, my his experiments, he theorized the existence negatively charged subatomic particles he called electrons. From this theory Thomson created a model of a atom which had the electrons placed evenly inside the atoms. In the early 1900s a Japanese scientist named H. Nagaoka designed an atom model as a large sphere surrounded by a ring of negatively charged electrons. Also, during the early 1900s (1898-1907) a physicist named Ernest Rutherford worked on experiments to test current atom models. His experiments involved shooting rays of alpha particles (small positively charged particles) though very thin pieces of gold foil. Based on Thomson's model, Rutherford hypothesized that the alpha particles would travel through the gold foil mostly unaffected by the gold. He was right. Most of the particles did pass through, but a small amount of particles were deflected. From this Rutherford hypothesized that the atoms must have a small positively charged core, the nucleus, which is surrounded by mainly empty space, which contains the electrons. In 1914 Rutherford made up the word "proton," which were subatomic particles that had a positive charge. A student of Rutherford's, a man named H. G. J. Moseley was the one who gathered the empirical support for Rutherford's work. In his experiments he used X-rays to show that the positive charge in the nucleus grows by one, from each element to the other. From this Moseley devised the concept of Atomic Number. In 1932, James Chadwick established that the nucleus must contain heavy neutral particles as well as positive ones, this was to explain the entire mass of the atom.
To start off, learning the Bohr-Rutherford diagrams in grade nine was a very big confusion for me. I had never fully understood how many shells should go around the nucleus nor did I know how to do the many calculations. As I progressed into grade ten, the teachings became easier. The review shows an example such as in the the bohr diagram, a nucleus is in the center, which is a little circle, and following that there are shells surrounding it containing electrons. Each ring can only hold a certain amount of electrons, and so the first shell around the nucleus can hold a maximum of 2 electrons, the next shell is able to hold a maximum of 8 electro...
Ionic compounds, when in the solid state, can be described as ionic lattices whose shapes are dictated by the need to place oppositely charged ions close to each other and similarly charged ions as far apart as possible. Though there is some structural diversity in ionic compounds, covalent compounds present us with a world of structural possibilities. From simple linear molecules like H2 to complex chains of atoms like butane (CH3CH2CH2CH3), covalent molecules can take on many shapes. To help decide which shape a polyatomic molecule might prefer we will use Valence Shell Electron Pair Repulsion theory (VSEPR). VSEPR states that electrons like to stay as far away from one another as possible to provide the lowest energy (i.e. most stable) structure for any bonding arrangement. In this way, VSEPR is a powerful tool for predicting the geometries of covalent molecules.
In ancient Greek the word atom meant the smallest indivisible particle that could be conceived. The atom was thought of as indestructible; in fact, the Greek word for atom means "not divisible." Knowledge about the size and make up of the atom grew very slowly as scientific theory progressed. What we know/theorize about the atom now began with a core theory devised by Democrotus, a Greek philosopher who proposed that matter consisted of various types of tiny discrete particles and that the properties of matter were