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Apologia Chem M 3C
Atomic structure, part 3
Question | Answer |
---|---|
a quantum assumption | the assumption that a physical quantity (such as energy) is restricted to discrete values |
When an electron moves from an orbit CLOSE to the nucleus to an orbit FAR from the nucleus, we say that the electron has been | excited. |
When an electron moves from an orbit FAR from the nucleus to an orbit CLOSE to the nucleus, we say that it has | de-excited. |
quantum mechanical model | the modern-day model of the atom in which electrons are found outside the nucleus in orbitals |
The quantum mechanical model mainly differs from the Bohr model | in the type of orbits that the electrons can occupy. |
We assume that electrons do not orbit in fixed circles but instead orbit in clouds we call | orbitals. |
Electrons can, at different times, be at different distances from the nucleus, but still | be in the same orbital. |
The orbital has a general shape and | the electron can be anywhere within that shape. |
There are several differently shaped orbitals that electrons can use to | orbit around the nucleus. |
The simplest type of orbital an electron can occupy | is called the s orbital. |
An s orbital is | spherical with the nucleus at the center. |
An electron that occupies an s orbital can be anywhere inside the sphere but cannot | venture outside of the sphere. |
If an electron orbits far away from the nucleus in a spherical pattern, | it will occupy a large s orbital. |
The farther away from the nucleus the electron is, | the more energy it must have. |
The number that appears next to the orbital letter is often called the | energy level of the atom. |
The p orbital is | dumb-bell shaped. |
There are _____ p orbitals on the first energy level of the atom. | no (0) |
The first p orbital is the | 2p orbital. |
For every energy level, there are | 3 different p orbitals, which are all shaped the same, but oriented differently in space. |
The third type of orbital is the | d orbital. |
There are ____ d orbitals for each energy level. | 5 different |
The lowest energy level d orbital is located on the _________ energy level. | third |
Within the same energy level, the different shaped orbitals require | different amounts of energy. |
Each individual orbital can hold only _____ electrons. | 2 |
If an electron is orbiting as close as it can to the nucleus, we say that it is in the | first energy level., |
On the first energy level, only 1 type of orbital exists: | the S orbital. |
All forms of matter try to stay in their | lowest possible energy state. |
Matter is basically | lazy. |
ground state: | the lowest possible energy state for a given substance |
The ground state | is different for every substance on earth. |
All of the chemical behavior of an atom is governed solely by | the number of electrons the atom has. |
electron configuration: | a notation that lists the number of electrons that occupy each orbital in an atom |
The periodic table gets its weird shape because of | electron configurations. |
If we had enough electrons to fill up the 3s and 3p orbitals, we would start filling the 4s orbital BEFORE | filling the 3d orbital. |
We call the first two columns of the periodic table the s block because | the last electrons in the atoms of that block end up in an s orbital. |
The s orbital block is only 2 columns wide because | the s orbital can have only 2 electrons in it. |
Since there are 5 d orbitals and each can have 2 electrons, | there are 10 elements in each row that have their last electrons in d orbitals. |
The last orbital block of the periodic table is | the p orbital block. |
The rows of the periodic table represent | the energy level that those electrons are in. |
In the d orbital block, the row that the elements are on is one number higher than the energy level that the electrons are in, so | you need to subtract 1 from the row number to get the correct energy level when filling up d orbitals. |
When we write an abbreviated electron configuration, we | look for the nearest atom in column 8A that has a LOWER atomic number than the atom you are interested in. Then,you simply add any extra electrons on top of that atom's configuration. |