Chemistry Chapter 5: Modern Atomic Theory
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| a form of energy like heat or electricity | ||
| through space in waves | ||
| 3.0×10¹⁰cm/s | ||
| the distance between two adjacent peaks in the wave; relates to the energy of light; designated by the Greek letter lamba: λ; what light energy is measured by | ||
| range of wavelengths; only a small part that is visible; colors are continuous | ||
| every light source has one; | ||
| its energy is inversely proportionate to its wavelength ε=hc/λ | ||
| constant proportionality known as "Planck's Constant" | ||
| the velocity of light in a vacuum | ||
| light that extends beyond violet; not visible but highly energetic; dangerous to living organisms | ||
| wavelengths longer than red | ||
| colors produced when wavelengths of light are separated; each element gives off its own one of these | ||
| proposed the model for sub-atomic arrangement | ||
| 1) Electrons revolved around the nucleus in a stable, circular orbit (like planets around the sun) 2) Electrons appear in several different orbits (distances from the nucleus) a) electrons are quantized- they are at a definite, or discrete, distances from the nucleus b) each orbit is referred to as an energy level | ||
| each energy level is designated by their own one of these numbers; indicates the energy and orbital of an electron in an atom | ||
| the lowest energy level of an atom which electrons will occupy | ||
| a state in which an atom has a higher potential energy than it has in its ground state | ||
| highest wavelength possible, most powerful; it determines the color given off by the element | ||
| Electrons move very quickly because of their low mass; so one could not predict an electron's position with much certainty | ||
| the wave nature of the electron and the uncertainty of its location led to a complex mathematical approach to the electron in the hydrogen atom; this was used to predict the probability of an electron to be in a certain region of space (orbital) | ||
| the region of space where there is the significant probability of finding a particular electron; also called an "electron cloud" | ||
| spherical volume of probability; all energy levels have this orbital (n=1,2,3, etc) can hold a total of 2 electrons in 1 sub-shell | ||
| the second kind of orbital present starting with n=2,3,4, etc; has 2 lobes of high probability; can hold a total of 6 electrons in 3 sub-shells | ||
| orbitals of the same type (s, p, d, or f) in each shell (1,2,3,4,5,6, or 7) make up this; can hold 2 electrons per one of these | ||
| most have 4 lobes; and their destiny runs along the axes; can hold a total of 10 electrons in 5 sub-shells | ||
| their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells | ||
| 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f | ||
| electrons occupy the available orbitals in the sub-shells of the lowest energy | ||
| the assignment of all the electrons into an atom in a specific shell and sub-shell (an electron's address) | ||
| states that no 2 electrons in the same orbital can have the same spin | ||
| representation of the orbitals in a sub-shell as boxes and its electrons as arrows | ||
| states that electrons occupy separate orbitals in the same sub-shell with parallel spins (in other words, electrons want their own space!) | ||
| the distance from the nucleus to the outer shell; decrease from left to right, increase from top to bottom; the more electrons an element has, the more it will want to hold them tighter and become smaller, the less they have the more empty space it has | ||
| the energy required to remove an electron from a gaseous atom to form a gaseous ion; since the outer electrons are less firmly attached, they are the 1st to go; it increases from left to right, and decreases from top to bottom |
