Bohr 's atom verses orbitals
129630
The first energy level is the atoms ground state, electrons will not release any phtons from this level since they are stable at this point.\n\nJust because an electron is in thr 7th level does not mean that it will release 7 photons to return to its ground state.  The electron could release 7 photons and jump 1 level each time, that is possible, but not required.  It is also possible that the electron release just 1 photon carrying a lot of energy and jump down all 7 levels at once.  The number of energy levels the electron jumps down depends on the energy it releases in the photon, or vice-versa, the energy it releases in a photon determines how many levels it jumps down.
374249
Yes.\nVSEPR was developed in 1957, while in 1940 Sidgwick and Powell reviewed the structures of molecules then known. They suggested that for molecules and ions that only contain single bonds, the approximate shape can be predicted from the number of the electron pairs in the outer or valence shell of the central atom. The outer shell contains one or more bond pairs of electrons but it may also contain unshared pairs of electrons (lone pairs). Bond pairs and lone pairs were taken as equivalent, since all electron pairs take up some space, and since all electron pairs repel each other. Repulsion is minimized if the electron pairs are orientated in space as far apart as possible.\n1. If there are two pairs of electrons in the valence shell of the central atom, hte orbital containing them will be oriented at 180<sup>o</sup> to each other. It follows that if these orbitals overlap with orbitals from other atoms to form bonds, then the molecule formed will be linear.\n2. If there are three electron pairs on the central atom, they will be at 120<sup>o</sup>  to each other, giving a plane triangular structure.\n3. For four electron pairs the angle is 109<sup>o</sup> 28', and the shape is tetrahedral.\n4. For five pairs, the shape is a trigonal bipyramid\n5. For six pairs, the angles are 90<sup>o</sup>  and the shape is octahedral.\n\n\nVSEPR was developed extensively by Gillespie and  Nyholm who improved the Sidgwick-Powell theory to predict and explain molecular shapes and bond angles more exactly. Gillespie summarized his theory in 4 points:\n1. The shape of the molecule is determined by repulsions between all of the electron pairs present in the valence shell. (This is the same as the Sidgwick-Powell theory).\n2. A lone pair of electrons takes up more space round the central atom then a bond pair, since the lone pair is attracted to one nucleus whilst the bond pair is shared by two nuclei. It follows that repulsion between two lone pairs is greater than repulsion between a lone pair and a bond pair, which in turn is greater than the repulsion between two bond pairs. Thus the presence of lon pairs on the central atom causes slight distortion of the bond angles from the ideal shape. If the angle between a lone pair, the central atom and a bond pair is increased, it follows that the actual bond angles between the atom must be decreased.\n3. The magnitude of repulsions between bonding pairs of electrons depends on the electronegativity difference between the central atom and the other atoms.\n4. Double bonds cause more repulsion than single bonds, and triple bonds cause more repulsion than a double bond.
228411
This is an subject area where vocabulary is vital for clear understanding, to a degree I am not capable of, however the stuff that you ask about are so small that the only way to attempt to prove their existence is through mathematical formulae based on what we suspect to be true. Our lack of understanding on this subject, which is still very voung, means the answers available are sketchy at best compared to our understanding of molecular structure or atomic structure.\nWhat is known so far can be found in places like the noetic sciences knowledge centre, or wikipedia.
663907
Your question, although it sounds absurd, probably has some research you could find on the topic. It is amazing how theoretical the major branches of science, which actively rely on theory assumed to be true in every day application, still are. I'd apply my brain to it but I gave up this particular line of thinking (which brings up the point to place here why I'm posting) after reading a Linus Pauling book section several years ago where he begins to introduce the "idea" of distal electrons taking up spaces on atoms and molecules locally, yet the bond slots they should be in are locally empty. The basic gist was, nobody knows if its true (mainly because they can't prove it) however, effects observed locally can't be explained without excepting the theory that an electron billions of light years away can be attached to a local, apparently empty electron bond slot.
429755
energy levels/orbitals
555418
In Greek atomic theory, the atom was considered the smallest, indivisible, particle of matter.\nThey view atoms as the basic building block of everything else, and all atoms were identical, different combinations of how they were put together determined the properties of the substance.\n\nOf course, we now know that atoms themselves are made up of smaller, sub-atomic, particles, which are then intern made up of even smaller particles.  Atoms are the smallest particles of a given element which will exibit the properties of that element.  Different elements, and thus different types of atoms, exist.  So the Greeks were not correct in that respect.
340858
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
569882
First the electron would have an sp1 configuration not np1.  As to which orbital it would revolve in...it doesn't matter.  The x, y, and z are just ways to distinquish the 3 different orbitals.  the point in the center is a null point.  the electrons do not actually travel through that spot.  Orbital configurations just define a volume where an electron might spend some of its time.  it could be found anywhere in the volume.
387645
Although there is a general trend toward an increase in the first ionization energy as we go from left to right across this row, there are two minor inversions in this pattern. The first ionization energy of boron is smaller than beryllium, and the first ionization energy of oxygen is smaller than nitrogen.\n\nTo read about why, follow the link. It's really hard to explain
322059
First, can a subatomic particle appear to be in two places at once?\n\nAccording to Quantum Theory, the answer is yes, because in order to know where a particle is, we have to measure its position, but the very act of measuring its position will alter the particle's behavior. So in effect we can never be sure where it is exactly. So in this sense, we may get measurements that give results that says the particle is here and there (this is the Uncertainty Principle).\n\nOf course, this is NOT new to quantum theory. So what's new? Someone mentioned "quantum entanglement" and "quantum teleportation". These are some of the new topics in quantum theory.\n\nPS - there is no such thing as Aether quantum dynamics or\n Auto dynamics, and Bohr's quantum mechanics is alive and well. The only addition we've added to Bohr's theory is the concept of electron cloud (i.e. a probability cloud) around the nucleus of an atom rather than electron orbits.
508039
True.  Elements are characterized by the nature of their atoms; each atom has a positively charged nucleus and is surrounded by a cloud of electrons.  All atoms of a particular element have the same nuclear charge.  Under normal circumstances, atoms are in a low energy state (the "ground state") in which the shape of the electron orbitals is roughly spherical -- bearing in mind that we're talking about the shape of a fog, without definite edges.  In higher energy states, the electron orbitals can get arbitrarily large.
97182
This involve a derivation of the Hydrogen atom formulas that Bohr Develloped in term of Rotational energy of an electron relative to the rotational energy of the proton.\nThe hydrogen atom having one proton as its nucleous makes it the simplest atom to model.\nHe calculated the average radius as aprox one half Angstrom.\nThe radius that Bohr develloped for the Hydrogen Atom  is its radius of equilibrium. This is the average orbit where the electron would spend most of it time at standard temperature.\nThe radius would vary depending on the temperature of the atom.\nHowever the way he describe the electrostatic energy level in terms of a constant is very commandable .However he does not really explain why this happens. The result he could not apply it to other more complicated atom without revising his theory.\n\nThe formula for electrostatic gravity power is as follow;\n\nMotional energy of the electron equals the product of an inverse force at the point of interaction times the product of the energies of the two electrical interacting masses.Now that you might understand the theory you can plug in the numbers.
543626
assuming that atoms were actually "balls" of subatomic particles and the electrons were in orbit like planets- you would see 5protons and 6 neutrons in the nucleus, and you would see 5 electrons orbiting around the nucleus
483052
Atomic radius is related with size of atom, so correct option is c)\n\nThat's it!\n\nGood luck!
408609
Basic Atomic Structure\n\nThe definitions of atoms and elements seems, at first glance, almost circular: an element is a substance made up of only one kind of atom, and an atom is the smallest particle of an element that retains all the chemical and physical properties of the element. In fact, these two definitions do not form a closed loop, as they would if it were stated that an element is something made up of atoms. Every item of matter that exists, except for the subatomic particles discussed in this essay, is made up of atoms. An element, on the other hand, is—as stated in its definition—made up of only one kind of atom. "Kind of atom" in this context refers to the number of protons in its nucleus.\n\nProtons are one of three basic subatomic particles, the other two being electrons and neutrons. As we shall see, there appear to be particles even smaller than these, but before approaching these "sub-subatomic" particles, it is necessary to address the three most significant components of an atom. These are distinguished from one another in terms of electric charge: protons are positively charged, electrons are negative in charge, and neutrons have no electrical charge. As with the north and south poles of magnets, positive and negative charges attract one another, whereas like charges repel. Atoms have no net charge, meaning that the protons and electrons cancel out one another.
618258
a the number of outer electron that will bond with other atoms to fill thei valence shells
528457
yes you are right.. there are two sets of electrons