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Definition
| Electrons are arranged around atomic nuclei like planets around the sun |
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Definition
Electrons occupy areas around atomic nuclei like clouds
AKA cloud model |
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| Define: ELECTRON STRUCTURE |
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Definition
| Electrons are arranged around the nucleus in energy levels, sub-levels and orbitals |
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| Define: Energy levels/sub levels |
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Definition
| The distance from the nucleus to an electron is found |
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Definition
| The space where there is a high probability the electron occupies |
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| How are main levels identified? |
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Definition
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| How does emission spectra give evidence for energy sub-levels? |
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Definition
| Big gaps in emission spectra lines indicate the distance between main energy levels; small gaps indicate the distance between sub-levels. |
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| How are sub levels identified? |
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Definition
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| How are orbitals identified? |
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Definition
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Term
| How are spins identified? |
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Definition
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| Define: the aufbao principle |
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Definition
| electrons occupy the orbitals of lowest energy first |
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Term
| The pauli exclusion principle |
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Definition
| an orbital can hold a maximum of 2 electrons, and they must have opposite spins....NO 2 ELECTRONS CAN HAVE THE SAME SET OF QUANTUM #S |
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Definition
| One electron enters each orbital of that sub-level contain 1 electron with the same spin direction |
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Term
| What is the Heisenberg Uncertainty Principle? |
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Definition
The position and energy of velocity of an electron cannot be measured at the same time...
a maximum of 2 electrons can be held in any orbitals.
Electrons fill energy levels as atomic number increases generally by filling the lowest first.
Valence electrons of the main group elements occupy the S and P sub-levels of the outermost energy levels.
The position of any element on the periodic table shows which sub-level, S, P, D, or F the valence electrons occupy.
The periodic table not only reflects electron structure according to the number of valence electrons, main groups 1, 2, - valence electrons in S sub-level, groups 13-18 valence electrons in S and P sub-levels. |
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Term
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Definition
N
Main level or quantum shell
(1,2,3,4,5, etc) |
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Term
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Definition
l
sublevel/subshell (s->0, p->1, d->2, f->3) |
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Term
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Definition
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| The # of possible orbitals in a sublevel is given by the formula... |
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Definition
| (2L+1), where 1= the sublevel or subshell # 0, 1,2, or 3 |
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Definition
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Definition
| Electrons in the outer energy levels of atoms which take part in chemical reactions |
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Term
On the periodic table, does ATOMIC SIZE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
increase
The number of energy levels increases as you move down a group as the number of electrons increases. Each subsequent energy level is further from the nucleus than the last.
decrease
The concentration of more protons in the nucleus creates a "higher effective nuclear charge." In other words, there is a stronger force of attraction pulling the electrons closer to the nucleus resulting in a smaller atomic radius. |
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Term
On the periodic table, does IONIZATION ENERGY increase or decrease...
going down the periodic table?
going across the periodic table?
Why? |
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Definition
decrease
Electrons are further from the nucleus and thus easier to remove the outermost one.
increase
As you move across a period, the atomic radius decreases, that is, the atom is smaller. The outer electrons are closer to the nucleus and more strongly attracted to the center. Therefore, it becomes more difficult to remove the outermost electron. |
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| Define: ionization energy |
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Definition
| electron's ability to pull electrons off of another atom |
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Term
| define: electronegativity |
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Definition
| atom's ability to hold onto its electrons |
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Term
On the periodic table, does IONIC SIZE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
| ionic size increases across the periodic table |
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Term
On the periodic table, does ELECTRONEGATIVITY increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
On the periodic table, does NUCLEAR CHARGE increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
On the periodic table, does SHIELDING increase or decrease...
going down the periodic table?
why?
going across the periodic table?
Why? |
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Definition
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Term
| When electrons are added to an atom, does it become more or less metallic? |
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Definition
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Term
| Why must orbitals have different shapes? |
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Definition
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Term
Name the shapes of orbitals in the
s
p
d
f
orbital |
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Definition
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| How many orbitals are in the p level? How are they positioned? |
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Definition
3x,3y,3z (so...3)
they are all positioned in different coordinate planes |
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Term
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Definition
| total charge of all the protons in the nucleus. It has the same value as the atomic number. |
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Term
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Definition
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell.
•Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. |
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Term
| Why are anions larger than their respective atoms? |
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Definition
| electrostatic repulsion, also protons cannot pull extra electrons as tightly towards the nucleus |
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