Naming and Lewis Structures Quiz Flashcards by saige tinker

Chemical Formula For An Ionic Compound

Represents one formula unit of that compound
Always reduce

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Formula Unit

Simplest whole number ratio of tha compound’s cations and anions

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Oxidation

The charge
Many transition elements have more than one possible oxidation state, some only have one

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Fixed

Single known charge
Anions

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Binary

Two elements

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Ionic

Opposite charged ions

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Monatomic Ions

One element ion

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Cation Ionic Compounds

Always comes first
Keeps name

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Anion Ionic Compounds

Always comes second
Change ending to -ide

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Subscript

Small numbers to the lower right of symbols
Refers to whatever its following
One is never used
Used to make net charge equal to zero

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Binary Polyatomic Ionic Compounds

Two metals
Metal to nonmetal

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Polyatomic Ion

An ionic compound with more than two elements
An ion made up of more than one atom that acts as a single charged unit

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Polyatomic Ion Doesn’t Start With Metal

Means positive

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Process of Naming Polyatomic Ions

Same as binary compounds
Treat as one unit
Never change subscripts

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Multivalent

More than one possible oxidation states
Many transition and p block metals are this way

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Roman Numerals

Used to tell which cation is present in the compound
An ionic compound that contains a cation that is a metal with more than one oxidation state is named with this

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Process of Roman Numerals

Metal is transition or p block
Then look at monatomic ion lost to see if it has more than one charge
Use roman numeral to identify charge

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Covalent Naming Process

Name first element fully
First element uses a prefix besides mono-
Second elements always change ending to -ide
Always use a secomd element prefix

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Covalent Prefixes

Mono-
Di-
Tri-
Tetra-
Penta-
Hexa-
Hepta-
Octa-
Nona-
Deca-

Acidic Naming Process

Starts with hydrogen
No oxygen use hydro-
Don’t say hydrogen or oxygen
Use other element or polyatomic ion
-ate to -ic
-ite to -ous

Find Number of Hydrogen Based On

Based on charge of anion

Binary Acid

An acid that contains only two elements
First is hydrogen
Second is nonmetal
Name always begins with hydro-
Root of second element’s name follows the prefix
Ends with -ic acid

Oxyacid

An acid that contains hydrogen and an oxygen anion
Based on the name of the polyatomic ion created
Never use hydro-

Oxyanion

Polyatomic ion that contains oxygen
Never use hydro-

Writing Acidic Formulas

No hydro- tells oxyacid Change ending -ate to -ic and -ite to -ous Write the symbols with their charges All acids begin with H+1 Add the nonmetal Crossover changes to subscript position Reduce

Acids Are Molecules

Covalently bonded except when dissolved in water Then, become ions

Co-

Together

-valent

Valence electrons

Covalent Bond

Chemical bond formed by the sharing of electrons between two atoms Attracted to unpair electron neither can take it away

Molecule

Neutral group of atoms that are held together by covalent bonds

Molecular Compound

Chemical compound whose simplest units are molecules

Shared Electrons

Form overlapping orbitals so that each atom achieves the octet rule

Exceptions to the Octet Rule

Atoms that can not fit eight and atoms that can fit more than eight in valence level

Incomplete Octet

Hydrogen can only hold one more electron in its s orbital, only forms one bond Boron has three valence electrons, so forms three bonds and is only surrounded by six electrons Beryllium has two valence electrons, two bonds, surrounded by four

Expanded Octet

Involving more than eight electrons P S Xe

Can Form Covalent Bonds

Beryllium

Can Form Bonds With Expanded Octets

Main group elements in periods 3 and below

Lewis Structure Guide

Count total number of valence electrons for all atoms in the molecule Set up skeletal structure with least electronegative as central Give all atoms an octet besides incomplete Count electrons to match the number electrons required

Exceptions to Central Atoms

Can bond central atoms together Carbon is always central Hydrogen is never Halogens are almost never

Simple Lewis Rules

Count Find middle Set up Make connections Add to ends then middle Count

HONC

Hydrogen and halogens form one bond never central atom Oxygen forms two bonds can form double nonds Nitrogen forms three bonds can form double or triple bonds Carbon forms four bonds can form double or triple bonds

Exception to HONC

Resonance

When a single Lewis structure does not clearly represent a covalently bonded molecule or ion Shown with a double headed arrow

Carbon

Forms four bonds Can form double or triple bonds

Seven Diatomic Elements

Bromine Iodine Nitrogen Chlorine Hydrogen Oxygen Fluorine

ABX Notation

Notation for the molecule that shows the number of lone pairs and bonding pairs as subscripts X represents number of lone pairs B represents number of bonding pairs

Lewis Dot for Single Atoms

1 top right 2 both right 3 right and top left 4 right, top left, and bottom left 5 right, top left, bottom left, and bottom right 6 right, top, bottom left, and bottom right 7 right, top, left, and bottom right