how bohr's model differs rutherford?
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Bohr thought that electrons orbited the nucleus in quantised orbits. ... In Rutherford's model most of the atom's mass is concentrated into the centre (what we now call the nucleus) and electrons surround the positive mass in something like a cloud. Bohr's most significant contribution was the quantisation of the model.
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Atoms of the same element have the same atomic number so the number of protons (and electrons) are same. But they have same or different mass number (like that for isotopes) . Different mass number will have different number of neutrons.
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Atoms of different elements have different numbers of protons. ... They have a different mass number because they have a different number of neutrons.
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The main difference between Mendeleev and Modern Periodic Table is that Mendeleev's periodic table orders the elements based on their atomic mass whereas Modern periodic table orders the elements based on their atomic number.
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However, experiments with electric discharges in the late 19th century showed that atoms only emit electromagnetic energy at certain discrete frequencies. Bohr resolved this by proposing that electrons orbiting the nucleus in ways that were consistent with Planck's quantum theory of radiation.
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Because different isotopes have different numbers of neutrons, they do not all weigh the same or have the same mass. Different isotopes of the same element have the same atomic number. They have the same number of protons. The atomic number is decided by the number of protons.
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This is known as the Pauli exclusion principle. Bohr model predicts that a maximum of 2(3)2 = 18 electrons can reside in the 3rd principal energy level. Quantum Mechanical Model of the atom predicts that in principal energy level 3, there are 3s, 3p, and 3d. In any s-subshell, there is 1 atomic orbital.
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Summary. J.J. Thomson's experiments with cathode ray tubes showed that all atoms contain tiny negatively charged subatomic particles or electrons. Thomson proposed the plum pudding model of the atom, which had negatively-charged electrons embedded within a positively-charged "soup."
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In the experiment, positively charged alpha particles were fired at thin gold foil. Most alpha particles went straight through the foil. But a few were scattered in different directions. This evidence led Rutherford to suggest a new model for the atom, called the nuclear model .
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However, physicists distinguish between atomic and nuclear physics. The atomic physics deals with the atom as a system consisting of a nucleus and electrons. The nuclear physics deals with the nucleus as a system consisting of a nucleons (protons and neutrons). Main difference is in the scale.
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The model used here describes electrons using four quantum numbers, n, ℓ, mℓ, ms, given below. It is also the common nomenclature in the classical description of nuclear particle states (e.g. protons and neutrons).
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Electrons are different from neutrons and protons because the Electrons are outside of the atom getting held in orbit by the electromagnetic force while the Neutrons and Protons are what the atom is made up of. The difference between protons and neutrons are that one has a positive charge and one has a neutral charge.
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A particular atom will have the same number of protons and electrons and most atoms have at least as many neutrons as protons. An element is a substance that is made entirely from one type of atom. ... All isotopes of a particular element have the same number of protons, but can have different numbers of neutrons.
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The protons, neutrons, and electrons are not different - but a combination of these makes different elements. ... Elements are known by their atomic number, and this depends on the number of protons in the nucleus of an atom, and determines its place in the periodic table.
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Note that the difference in energy between orbitals decreases rapidly with increasing values of n. In general, both energy and radius decrease as the nuclear charge increases. Thus the most stable orbitals (those with the lowest energy) are those closest to the nucleus.
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Another difference is that the exchange of a Z boson cannot change particle type (in this sense it is like a massive version of the photon), while W boson exchange results in particles changing from one type to another. ...
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We are given that boron-10 had five protons in its nucleus, and any element always has the same number of protons in its nucleus (atomic number). So boron-11 has five protons the same as boron-10. Then the mass number is total protons plus neutrons.