Ch 5 & 6: Bonding, Formulas and Naming Notes
Name ______________________________
Period __________Date________________
Types of Chemical Bonds:
A. Ionic Bonding
1) Positively charged ions are attracted to ________________ charged ions, making a
____________________ atom.
2) Properties of Ionic Compounds:
a) high _____________________________________.
b) dissolve in water to form ______________ that are good _________________ of
electricity (___________________).
c) have a large __________________________ difference between elements.
d) usually form between _________________ and __________________.
3) The Octet Rule:
a) Atoms tend to gain or lose electrons in order to acquire a _________ set of
__________________ electrons (____________ ____________).
b) Atoms will ______________ electrons (e-) to each other in order to have a full set of
_______________ electrons.
c) When electrons are transferred, ____________ bonds are formed.
4) Types of Compounds:
a) Binary form from monatomic ions – have _______ cation and _______anion.
Ex) Mg+2 O-2 ______________ Ca+2 Cl-1 ________________
b) Tertiary form from polyatomic ions which consists of a group of atoms
_____________________ bonded with a _______________ charge that bond
ionically with other ions.
-Ex. __________________________
__________________________
“ __________________________________”, _____________________
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5) Polyvalent Metals: Some metals including the _______________________metals do
not follow the ___________________ rule and may form more than 1 kind of cation.
These ions are named with ________________ __________________ to
distinguish between them.
Ex)
Fe+2 _______________________ read “iron two”
Fe+3 _______________________ read “iron three”
FeCl2 ________________________________________________
FeCl3 ________________________________________________
Copper (I) sulfate
__________________
Copper (II) phosphate
__________________
6) Lewis Dot Diagrams for elements:
Element
# of val. Electrons
Dot Diagram
Li
N
Be
F
Ne
Au
**Note: Only show s and p orbitals in dot diagram.
7) Lewis-dot diagram for sodium chloride:
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B. Covalent Bonding
1) Covalent Bonds are formed by _______________ pairs of electrons between 2 atoms.
2) Usually formed between two _______________ with a _______ electronegativity difference.
3) Molecules:
a) a group of atoms held together by _______________________ bonds
b) molecular substance – contains ______________________
4) Naming:
a) uses prefixes:
1 mono2 di3 tri-
4 tetra5 penta6 hexa-
7 hepta8 octa9 nona-
10 deca-
b) end in “ide”
c) More electronegative element is written _____________
d) Only use a prefix on the first element if it is more than ___________.
e) Always use a prefix for the ______________ _______________.
Ex)
water H20
___________________________
Smog NO2
___________________________
5) Types of formulas for covalent bonding
a) Molecular Formula shows how _________ atoms make up a ______________.
ex. ______________________ & ______________________
b) Structural Formula shows how the atoms are ______________ to each other.
ex.
1. Uses 2 _________ to show an unshared pair of ________________.
2. Uses ____________________ to represent covalent bonds (a shared pair of
electrons) in a structural formula.
3. The ____________ rule should be satisfied for each element in the compound.
c) Empirical Formula is the ____________ whole number _________ of all the elements
in the compound.
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6) Multiple Bonds – can be used to satisfy the octet rule
a) Single Bonds – Share __________ pair of electrons.
b) Double Bonds – Share __________ pairs of electrons.
c) Triple Bonds – Share ___________ pairs of electrons ( ____________ bond).
8) Properties of Covalent Bonds
a) Low __________________ points, ________________, strong ________, poor
________________ of electricity.
b) Polar Bonds – form between elements with __________ differences in
electronegativity. These have an _________________ sharing of electrons.
Ex)
c) Nonpolar bonds – exert ______________ ______________ on the electrons.
Ex)
9) Electronegativity Chart is used to determine bond type
non polar covalent
polar covalent
ionic bonds
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C. Ionic & Covalent Bonds Summary:
Ionic Bonding
Covalent Bonding
D. Acids:
1) A molecular compound that dissolves in water to produce ____ and a characteristic _________.
2) In water, acids behave like _______________ compounds.
3) Most acid formulas begin with __________. (Except organic acids) “ _________”
4) The number of hydrogens in the formula depends upon the ____________ of the anion.
5)Types of Acids
a.) Organic Acids contain the _______________________ group, -COOH or _________
Ex)
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b.) Binary Acids contain ____________________ and 1 type of _______________.
A two-word name is used for binary acids.
1st word: prefix is “hydro”
root is formed from the anion
anion suffix “ide” is changed to “ic”
2nd word: is “acid”
Ex) HCl
anion is chloride
hydrochloric acid
Prefix
HBr
root
suffix
anion is bromide _______________________________
c.) Oxo (Tertiary) Acids: contain __________________ within a polyatomic ion.
A two-word name is used for oxo acids.
H2SO4
H2SO3
sulfur or phosphor (to sound better)
2nd word is “acid”
HNO3
anion is nitrate
nitric acid
root
H3PO3 anion is phosphite
suffix
______________________________
Nitrous acid, anion is ___________________ formula is: _______________
Phosphoric acid, anion is ________________ formula is: ________________
E. Hydrates:
1.) Ionic compounds that absorb ________ into their solid structures.
Ex) ___________________________________________________ (________________)
Formula: ________________________
2.) Anhydrous substance - _______________________________________________
Ex) CuSO4 • 5H2O _______________________________________________
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