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Apologia Chem M 4B

Molecular Structure, part 2

QuestionAnswer
When determining the formula for ionic compounds, drop the signs, switch the numbers, and use the numbers as subscripts.
The chemical formula ratio for ionic compounds must always be at the lowest possible ratio.
If the charges for an ionic compound have the same numerical value, then the subscript for each ion is 1 and can therefore be ignored.
When we write out the name of the ionic compound involving a transition metal, we need to be very clear about which ion is present.
When we write out the name of the ionic compound involving a transition metal, we put a Roman numeral in the name that represents the charge of the transition metal.
Although most atoms want to become charged to attain the ideal electron configuration, they never start out that way. When an atom is formed, it is ALWAYS formed as an atom.
Ionization the process by which an atom turns into an ion by gaining or losing electrons
Ionization energy the amount of energy needed to take an electron away from an atom
The elements on the left side of the periodic table have a rather low ionization energy (they give up their electrons easily).
The atoms on the right side of the periodic table have high ionization energies, meaning they give up their electrons grudgingly.
In general, ionization energy of atoms increases from the left of the periodic table to the right of the periodic table.
A periodic property is a characteristic of atoms that varies regularly across the periodic table.
In general, the ionization energy of atoms ______________ from the bottom of the periodic table to the top of the periodic table. increases
Electronegativity A measure of how strongly at atom attracts extra electrons to itself
In general, the electronegativity of atoms increases from the ___________ to the right on the periodic table. left
In general, the electronegativity of atoms increases from the ___________ to the top on the periodic table. bottom
atomic radius the average radius of an atom
The radius of an atom is an indicator of its size.
The _______________ _________________ of an atom is what determines its size. electron configuration
Atomic radius varies according to the placement of the atom on the periodic table.
In general, the atomic radius increases from the top to the bottom on the periodic table.
In general, the atomic radius increases from the right to the left on the periodic table.
covalent compounds contain only nonmetals
nonmetals always GAIN electrons
elements are composed of individual atoms
compounds are composed of individual molecules
nitrogen, oxygen, chlorine, fluorine, bromine, iodine, astatine, and hydrogen homonuclear diatomics
homonuclear diatomics molecule composed of two identical atoms
covalent bond a shared pair of valence electrons that holds atoms together in covalent compounds
The atoms in covalent compounds ___________ ______________ to form molecules. share electrons
The atoms in ionic compounds ________ ______ ________ ________________ to form ions. give and take electrons
The atoms in ionic molecules stay together because the positively charged ions are attracted to the negatively charged ions.
In covalent compounds, there is a physical bond (a pair of shared electrons) which holds the atoms together.
The fist thing to realize about working with Lewis structure is that the atoms given in a chemical formula are all we have to work with.
The second thing to realize when determining a Lewis structure is that the dots for each of the included atoms are all the dots that we have to work with. We cannot use any more or any less than the dots drawn.
In putting together Lewis structures, it is best to start at the center and work our way out.
We put the atom with the _______ ___________ _______________ in the center. most unpaired electrons
To start constructing a Lewis structure, first count the valence electrons in the entire molecule by adding up the valence electrons of the individual atoms.
One warning regarding constructing Lewis structures: When an atom enters into a covalent molecule, the number of valence electrons that it started with is no longer important.
When constructing Lewis structures, they just need to have the same central atom, the same atoms bonded to that central atom, and the same number of nonbonding electron pairs for each atom.
When we replaced a shared electron pair with a dash, it indicates that it is a covalent bond.
When two shared electron pairs make up a bond, we call it a double bond.
It is perfectly "legal" to move electrons from one place in a Lewis structure to another place, as long as you do not get rid of any electrons.
When a total of 6 electrons are shared between atoms, they have a triple bond.
The real trick to figuring out Lewis structures is to just keep trying.
Lewis structures are helpful in understanding a molecule's chemical behavior.
Created by: MrsHough
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