Unit 4 - Bonding Flashcards Preview

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Flashcards in Unit 4 - Bonding Deck (29):

Ionic Bond

Metals GIVE electrons, Nonmetals TAKE electrons


Naming Ionic Bonds

State the name of the metal followed by the nonmetal with the ending changed to "ide". If the metal is a transition metal, add a (Roman numeral). AlCl₃ = Aluminum Chloride CuCl₃ = Copper (III) Chloride


Writing Formulas for Ionic Bonds

Absolute Value Criss Cross Oxidation #'s


Polyatomic Ion

A group of atoms that acts like an ion (has a charge)


Properties of Ionic Compounds

Crystalline Structure High Melting Point Rigid Strong Bond Conduct Electricity (when dissolved or melted) Good Insulators


Covalent/Molecular Bonding

Nonmetals SHARE electrons


Intermolecular Forces

Attractive forces BETWEEN molecules.


Van Der Waals or London Dispersion Forces are the weakest type of intermolecular force and hydrogen bonds are the strongest.


Intramolecular Forces

Attractive forces WITHIN a molecule (Ionic & Covalent Bonds)

These bonds are stronger than intermolecular forces.


Polar Covalent

A type of covalent bond between two atoms in which electrons are shared unequally. Because of this, one end of the molecule has a slightly negative charge and the other a slightly positive charge.


Non Polar Covalent

A type of covalent bond between two atoms in which electrons are shared equally.


Naming Covalent Compunds

You DO NOT use the “criss-cross” method. Use prefixes. The only time you do not use a prefix is when there is only one of the first nonmetal. Remember : 1-Mono 2-Di etc...


Write the formula for Mg²⁺ and PO₄³⁻

Using the criss-cross method and subscripts to insure sum of charges is zero: Mg₃(PO₄)₂


Polyatomic Ionic Formulas

1. Metal written first, Polyatomic Ion is written second 2. Use criss-cross method and subscripts to insure sum of charges = 0 3. When using a subscript for polyatomic ions: place a parentheses around the polyatomic formula, put the subscript outside of the parentheses


Polyatomic Ion

Polyatomic Ions ions made up of more than one atom; acts as an individual ion in a compound; charge applies to entire group of atoms.


Ionic Compounds

two words, first names cation second names anion. Indicate charge of transition metal cation by Roman Numeral. MgCl₂ = Magnesium Chloride Cr(NO₃)₃ = Chromium(III) Nitrate SnCl₂ = Tin(II) Chloride



Anions are named by adding the suffix -ide to the stem of the name of the nonmetal from which they are derived. N³⁻ = Nitride O²⁻ = Oxide F⁻ = Flouride


Ionic Compound Formulas

1. Metal written first Nonmetal written second 2. Use criss-cross method and subscripts to insure sum of charges = 0


Oxidation Number

Ion Charge - number of electrons transferred to or away from an atom when it becomes an ion.


Greek Prefixes used in nomenclature 1= 2 = 3 = 4= 5 = 6= 7= 8= 9= 10=

1= mono 2 =di 3 =tri 4=tetra 5 = penta 6=hexa 7=hepta 8=octa 9=nona 10=deca


Covalent or Molecular Compounds (Molecules)

The first word gives name of the element that appears first preceded by a prefix that shows number of atoms in that element. Do NOT use the prefix mono before the name of the first element. The second word consists of a prefix designating the number of atoms of that element, the stem name of the second element, and the suffix -ide.


(Oxidation #) Charge of Group17 or 7A (F, Cl, Br, I)

Charge: 1-


(Oxidation #) Charge of Group 16 or 6A (O,S, Se, Te):

Charge: 2-


Charge of Group15 or 5A (N, P, As):

Charge = 3-


(Oxidation #) Charge of Group 2 or 2A (Be, Mg, Ca, Sr, Ba):

Charge = 2+


(Oxidation #) Charge of Group 1 or 1A (H, Li, Na, K, Rb, Cs):

Charge = 1+


Ionic  Compounds

Conduct Electricity when melted or dissolved in water because....


Cation Formation

Metals give electrons to become like the nearest noble gas.


Anion Formation

Nonmetals recieve electrons when forming an ionic compound so that their electron configuration will be like the nearest noble gas.


Compound Formation

 Compounds are the result of the formation of chemical bonds between two or more different elements, whose atoms lose, gain or share valence electrons to complete their outer shell and attain a noble gas configuration.

This tendency of atoms to have eight electrons in their outer shell is known as the octet rule.