Flashcards
Chemistry - Chapter 2
Flashcards do conjunto (21)
- 1Ionization energyThe energy needed to remove an electron from the ground state of an atom in a mole of gaseous atoms, ions, or molecules
- 2Heisenberg’s Uncertainty PrincipleWe can only know where an electron is likely to be
- 3Schrödinger model of the hydrogen atom- His model included where it's possible for an electron to be
- Includes atomic orbitals: a region around the nucleus where there is a 90 percent probability of finding the electron. - 4Deduce how many different frequencies in the visible emission spectrum of atomic hydrogen would arise as a result of electron transitions between these levels.Visible transitions result from the Balmer series of transitions, which involve emissions that end at the n = 2 level. There are three possible transitions using the energy levels shown in the diagram: n = 5 to n = 2, n =
4 to n = 2 and n = 3 to n = 2. Any other emissions would involve electromagnetic radiation outside of the visible region of the spectrum. - 5What provides evidence to support the Bohr model of the hydrogen atom?The energy of the lines in the emission spectra of atomic hydrogen. Basically the emission spectrum.
- 6The Pauli Exclusion Principleno more than two electrons can occupy one orbital, and if two electrons are in the same orbital they must spin in opposite directions (they’re in the same space despite their mutual repulsion). If two electrons occupied the same electron and spun in the same direction, they’d be the same electron.
- 7List the 4d, 4f, 4p, and 4s atomic orbitals in order of increasing energy.s < p < d < f
- 8Atomic orbitals- 1st energy level: 1 s orbital
- 2nd energy level: 4 p orbitals
- 3d energy level: 9 d orbitals
- 4th energy level: 16 f orbitals - 9OrbitalYou can think of an orbital as being the region of space in which the electron lives = is likely to be
- 10Exceptions electron configuration- chromium has the electron configuration [Ar] 3d^5 4s^1
- copper has the electron configuration [Ar] 3d^10 4s^1 - 11Ground state: electron configurationFor the first 20 elements in the periodic table, any electron configuration that follows the lower energy orbitals first order of filling will be a ground state configuration - this is known as the Aufbau Principle.
- 12Excited state: electron configuration- when an orbital isn't completely filled before jumping to the next orbital. E.g.
[Ne]3s^1 3p^4
- The s orbital isn't filled. There's only one electron there = excited state - 13Ground state of electron configurationBasically means how it's normally arranged.
- 14Hund's RuleAccording to the first rule, electrons always enter an empty orbital before they pair up. Electrons are negatively charged and, as a result, they repel each other. Electrons tend to minimize repulsion by occupying their own orbitals, rather than sharing an orbital with another electron.
- 15When using Hund's RuleRemember that both arrows first appear in the 4s orbital, before the 3d orbital.
- 16Abbreviation of electron configurations- starts at the 3d orbital
- the abbreviation starts with a noble gas - 17Exceptions to the electron configurationsCr = [Ar] 4s^1 3d^5
Cu = [Ar] 4s^1 3d^10
(chromium and copper): basically, they only have one electron in the 4s orbital. The electron that was supposed to be there is in the 3d orbital instead. - 18Aufbau Principlestates that electrons are placed into orbitals of lowest energy first
- 19State the total number of p orbitals containing one or more electrons in e.g. germaniumeach p sub-shell contains 3 orbitals. So for each p line in the periodic table, there are three orbitals. So that would make 6 orbitals, and then, using Hund's rule, there would be 8 p orbitals in total.
- 20Order of mass spectrometerionization, acceleration, deflection
- 21Number of electrons in each orbital• s sub-levels can hold a maximum of 2 electrons.
• p sub-levels can hold a maximum of 6 electrons.
• d sub-levels can hold a maximum of 10 electrons.
• f sub-levels can hold a maximum of 14 electrons.
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- FlashCards sobre Chemistry - Chapter 2, criado por Piper Williams em 29-04-2017.
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- Piper Williams
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