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☆☆☆☆☆A chemical bond in which one atom gives up an electron to another, forming two ions of opposite charge, and thus generating an electrical force that holds the atoms together. The atoms are thus held together by the attractive force between a positively and a negatively charged ion.
An ionic bond is typically formed between a metal and a non-metal.
A bond between two elements caused by a difference in charge created by the donation of an electron by one of the atoms to another.
Atoms that have only one or very few electrons in their valence shell are very vulnerable to losing them. If another atom comes along with lots of electrons in it's valence shell, but not quite enough to be complete, the other atom's lonely old electron will get snatched away to join the shell with lots of electrons, and make a complete electron shell. When this happens though, a discrepancy in charge is created. The atom that now has the extra electron it's not supposed to have has a more negative charge, and the atom that got its electron stolen has a more positive charge. As you know, opposites attract, and in this case they attract so strongly that they two atoms become bonded to together.
For example, what happens if you have Na(sodium) and S(sulfur) during an ionic bonding. Here is a simple way to figure it out. Sodium has one electron in the outside electron shell and sulfur has two empty "spaces." So, if sodium(metal) give sulfur(non-metal) the one electron, but sulfur has one space left so another sodium comes along and that sodium gives its electron to sulfur. Thus, sulfur has no spaces. The chemical formula is Na2S because Sodium was used twice.
There are 2 energy sublevels in the second principal.
a numbering system for the periodic table.
Or a trend that periodically shows up.
the period number tells which is the highest energy level occupied by the electrons
1s 2 2s 2 2p6 3s2 3p6 4s2
or
Ar 4s2 (Noble gas form)
In noble gas form, you go back to the noble gas (the last group on the periodic table) prior to the element you are writing the configuration for. The electron configuration is the same up until that point. Then you write down the difference.
In this example, the electron configuration for Argon (Ar) is 1s2 2s2 2p6 3s2 3p6. If you fill up the shells until 4s2, you get calcium. It's faster to abbreviate by saying "Ar 4s2"
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A full octet makes the noble gases nonreactive.
A covalent bond in which the electrons are shared equally
The energy of the valence electrons is greater than the energy of the core electrons.
Helium has the highest first ionization energy and francium has the lowest first ionization energy.
D orbitals begin being filled with electrons after the orbital found in the 4s sublevel is filled.
magnesium (Mg)
question: which of the following elements is the smallest?
answer: chlorine (CI)
H2
The lone pair repels the electrons of the adjacent bonds more so than does a bonding pair of electrons, so thus alters the molecular geometry of the molecule.
There are eight orbitals in the second energy level.
