Honors Chemistry
Unit 5
(2015-2016)
 Chemical bonding
 Chemical formulas
 Chemical naming
1
We are learning to:
1.
2.
3.
4.
5.
Distinguish between an element and compound.
Distinguish between ionic, covalent, and metallic bonds.
Write the name/formula for covalent compounds.
Write the name/formula for ionic compounds including the use of polyatomic ions.
Write the name/formula for acids.
We are looking for:
1. Compounds are a chemical combination (bonded together) of 2 or more elements.
2a. Electronegativity differences between 2 elements determines the ionic character of a bond; 00.3 is nonpolar covalent, >0.3-1.7 is polar covalent, >1.7 is ionic.
2b. Metallic bonds occur between 2 or more metals.
2c. Describe the characteristics of substances with ionic, covalent, or metallic bonds (behavior of
the electrons, solubility, conductivity, state at room temperature, melting point).
3a. Use prefixes when naming or writing formulas for covalent compounds and change second element
ending to –ide.
3b. Do not reduce subscripts on covalent compound formulas.
4a. Do not use prefixes when naming ionic compound formulas/names; name the metal and then
change the nonmetal ending to –ide.
4b. Use oxidation numbers to write the correct balanced formula for an ionic compound (criss-cross
method).
4c. Use roman numerals for metals with multiple oxidation states when naming ionic compounds.
4d. Reduce subscripts for ionic compound formulas.
4e. Recall of polyatomic ions ending in –ate.
4f. Determine all other forms of polyatomic ions based upon the –ate ion and how the amount of
oxygen has changed.
5a. Use hydro- prefix when naming binary acid (an acid with H and a nonmetal) and change ending of
nonmetal to -ic and add acid on the end.
5b. Use oxidation numbers to write the correct balanced formula for binary and ternary acids (crisscross method).
5c. Naming ternary acids (an acid with H and a polyatomic ion) convert polyatomic ion to the correct
ending: -ate becomes –ic; -ite becomes –ous) and add acid on the end.
2
Chemical Bonding
Electrical attraction between nuclei of one atom and valance (outer shell) electrons of a different atom.
I. Ionic Bonding
_________________ of electrons from the ___________(cation) to the ____________ (anion)
Electrical attraction between large numbers of cations and anions. “clusters”
Cation = positively particle
Typically are metals
Loves to give electrons away
Low Ionization Energy
Low Electron Affinity
Low Electronegativity
Most metallic element = Francium
Anion = negatively charged particle
Typically are non metals
Loves to accept or take on electrons
Higher Ionization Energy
Higher Electron Affinity
Higher Electronegativity
Most nonmetallic element = Fluorine
Ionic compounds are ________________
Ionic bonds _________________________in water
- Fall apart into cations and anions
-Will conduct electricity
EN (electronegativity) difference is 1.8 – 4
Maximum value is 4 (Fluorine is a 4)
3
II.
Covalent Bonds
Formed when 2 _______________ atoms ______________electrons
A. ____________ Covalent
__________________ sharing of electrons
H
Cl
Electrons attracted MORE to higher EN atom, so density is greater around atom
with higher EN value.
EN of H = 2.1
EN of Cl = 3.0
EN difference = .9
EN difference range =
>_______– ________ for polar covalent bonds
Polar Covalent compounds
 dissolve in H2O
 don’t fall apart into ions….
 No conductivity!
B. _________________ Covalent Bonds
______________ sharing of electrons
Br
Br
Electrons are shared equally between two atoms.
EN difference for nonpolar covalent bonds is _____-_______.
Usually nonpolar covalent bonds are between diatomic molecules – two of the
same atoms.
Nonpolar covalent compounds
 do not dissolve in water
 no conductivity.
Can be a gas, liquid, or solid.
4
III. Metallic Bonds
Bond formed between 2 _____________atoms.
Larger outer electron shells – which overlap
Electrons are free to move within electron clouds of all metal ions =
___________________________
Electrons are ______________________ - they don’t belong to any one atom anymore.
5
Periodic Table with Electronegativities
1A
2A
3B
4B
5B
6B
7B
8B
1B
2B
3A
4A
5A
6A
1
H
2.1
7A
8A
2
He
3
4
Li Be
1.0 1.5
5
6
7
8
9 10
B
C
N O
F Ne
2.0 2.5 3.0 3.5 4.0
11 12
Na Mg
0.9 1.2
13 14 15 16 17 18
Al Si
P
S
Cl Ar
1.5 1.8 2.1 2.5 3.0
19 20 21
K Ca Sc
0.8 1.0 1.3
22
Ti
1.5
23
V
1.6
24
Cr
1.6
25
Mn
1.5
26
Fe
1.8
27
Co
1.9
28
Ni
1.9
29
Cu
1.9
30
Zn
1.6
31 32 33 34 35 36
Ga Ge As Se Br Kr
1.6 1.8 2.0 2.4 2.8 3.0
37 38 39
Rb Sr
Y
0.8 1.0 1.2
40
Zr
1.4
41
Nb
1.6
42
Mo
1.8
43
Tc
1.9
44
Ru
2.2
45
Rh
2.2
46
Pd
2.2
47
Ag
1.9
48
Cd
1.7
49 50 51 52 53 54
In Sn Sb Te
I Xe
1.7 1.8 1.9 2.1 2.5 2.6
55 56 57
Cs Ba La
0.7 0.9 1.1
72
Hf
1.3
73
Ta
1.5
74
W
1.7
75
Re
1.9
76
Os
2.2
77
Ir
2.2
78
Pt
2.2
79
Au
2.4
80
Hg
1.9
81 82 83 84 85 86
Tl Pb Bi Po At Rn
1.8 1.9 1.9 2.0 2.2 2.4
87 88 89 104 105 106 107 108 109 110 111 112
Fr Ra Ac Rf Ha Sg Ns Hs Mt Uun Uuu Uub
0.7 0.9 1.1
58 59 60 61 62 63 64 65 66 67
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho
1.1 1.1 1.1 1.2 1.2 1.1 1.2 1.2 1.2 1.2
68
Er
1.2
69
Tm
1.2
70
Yb
1.2
71
Lu
1.3
90 91 92 93 94 95 96 97 98 99 100 101 102 103
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
1.3 1.5 1.7 1.3 1.3 1.3 1.3 1.3 1.3 1.3 1.3 1.3 1.5
Keep in mind that electronegativities are approximate measures of the relative tendencies of these elements to
attract electrons to themselves in a chemical bond. The greater an atom's electronegativity, the greater its
ability to attract electrons to itself.
6
Calculating Bond Type
(using Electronegativity Values)
Electronegativity
Difference
Bond Type
Ionic Character
0.0 – 0.3
Non-polar covalent
0 – 5%
>0.3 – 1.7
>1.7
Polar covalent
Ionic
5 – 50%
Higher than 50%
1. Find electronegativity values for each element.
2. Subtract the lesser value from the larger value (so the value is positive).
3. Find the difference value on the above chart; convert it to a bond type.
Determine the type of bond that will form between each pair of elements:
1) Ca ,Br ___________________________
2) O, H ____________________________
3) C, H ___________________________
4) Na, Cl __________________________
5) S, O ____________________________
7
Using Rule of Thumb To Predict Bond Type
Metal + Non metal  Ionic Bond
Metal + Metal  Metallic
Non metal + Non metal  Covalent
Noble Gas + any element  typically no bond
Elements
Predict using
Rule of Thumb
Au and I
Au =
I=
Cu=
Zn=
Ca =
F=
P=
Br =
Fe=
Ar=
Ag =
Cl =
Ti =
O=
Cu and Z
Ca and F
P and Br
Fe and Ar
Ag and Cl
Ti and O
C6H12O6
C–H
C–O
Predict based on
Electronegativity values
(see page 6)
Au =
I=
Cu=
Zn=
Ca =
F=
P=
Br =
Fe=
Ar=
Ag =
Cl =
Ti =
O=
O–H
KOH
H2O
MgSO4
CaCO3
8
Types of Bonds
Ionic
Examples
Na and Cl
Covalent
C and Cl
Metallic
Na and Na
Types of elements
(metal? nonmetal?)
Electronegativity
Difference between
elements
How are the electrons
involved?
Compound formed from
example above
Name for a single unit of
this compound
Bond Strength
State at room
temperature
Polarity
Solubility in H2O
Conductivity (light bulb
test)
Melting Point
9
Ionic
Covalent
10
Intermolecular Forces (bonds)
 occur between molecules.
 Intermolecular forces are weaker than intramolecular forces (covalent and ionic bonds).
Hydrogen Bonding




The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is
attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule.
One molecule is polar and has hydrogen in a H-F, H-O or H-N bond
Other molecule has unshared pairs of electrons, usually on F, O, or N
Hydrogen forms a weak bond with the unshared pair of the other molecule
..
H – O:
H
H–O
H
δ+
δ-
Van der Waals bonds (there is more than one type but we are only discussing the
London dispersion forces)



London dispersion forces result from the intermolecular attractions resulting from the constant motion of
electrons and the creation of instantaneous dipoles.(see diagram below)
They can be very weak intermolecular forces that typically occur between noble gas atoms and between
nonpolar molecules.
Electrons of Noble Gas get shifted to one side causing it to attract a slightly positive atom that is nearby.

11
Bonding Review Sheet
Name the type of bond that will occur between the elements/compounds below based on
the periodic table.
1. Zn + Zn
2. Ca + Cl
3. I + I
4. Co + Ne
5. Mg + O
6. H2O + H2O
Below list all of the characteristics of the following words:
Ionic Bond
Van der Waals Bonds
Metallic Bond
Polar Colvalent
Hydrogen Bond
Nonpolar Covalent
12
Write the type of elements (metal/nonmetal) for the compounds below and decide what type
of bond is occurring
Compound
Type of elements
Type of bond
CaCl2
Br2
CH4
C6H12O6
Using the elements below, draw a nonpolar electron cloud and a polar electron cloud and
describe why they are different. Label the type of bond (polar or nonpolar covalent)
H
Cl
Br
Type of bond ____________
Element
Nitrogen
Nuclear
Symbol
Mass
Number
Br
_____________
# of
Protons
# of
Neutrons
# of
Electrons
15
48
Charge
3-
22
4+
50
38
0
13
Making Ionic Compounds!!
(with a metal and a non-metal)
Make compounds from the following cations and anions
Bromine , Tin (IV) , Calcium , Phosphorus, Gallium, Nitrate, Ammonium,
Carbonate
Cations (write their symbol and charge)=
(Put them along the side of the table; top to bottom)
Anions (write their symbol and charge)=
(Put them across the top of the table)
-----------
------------
-------------
--------------
14
Naming Ionic Compounds
Binary Ionic Compounds (2 elements; metal + nonmetal)
1. Name metal (cation) first, use name as it appears on the periodic table.
2. If the metal is tin (Sn) or lead (Pb), you must put a roman numeral with the name.
Also, if the metal is a transition metal, it might need a roman numeral. (The
roman numeral equals the amount of + charge)
The transition metals that don’t need a roman numeral are:
3. Name nonmetal (anion) second. Change the ending of the nonmetal to –ide.
Ex. NaCl = Sodium Chloride
Ex)
Nitrogen becomes nitride
Bromine becomes bromide
Oxygen becomes oxide
Sulfur becomes sulfide
Hydrogen becomes hydride
Phosphorus becomes phosphide
***When given the name and you need to write the formula, you must determine the
charge for each ion first and then criss-cross.***
15
Ionic Compounds with Polyatomic Ions:
Name the polyatomic ion; do not change it.
Ex. NaNO3 is Sodium Nitrate
Fe(NO3)3 is Iron (III) Nitrate
Making More Polyatomic Ions
Change in Amount of Oxygen
1 oxygen higher than “ate” level
ending
per-
-ate
“-ate” level
-ate
1 oxygen lower than “ate” level
-ite
2 oxygens lower than “ate” level
hypo-
-ite
Common ions have "ate" ending
o
BrO3-, Bromate
If you lose 1 oxygen atom from "ate" ion, the form is "ite"
o Ex: Bromate is BrO3o Br02- = Bromite
o Charge of ion does not change as form changes!
If you lose 2 oxygens atoms from "ate" ion, the form is "hypo
ite"
o Ex: BrO3- is Bromate
o BrO- is hypobromite
o
If you gain 1 oxygen atom from the "ate" ion, the form is "per ate"
o Ex: BrO3- is Bromate
o BrO4- is perbromate
16
Metal or
Polyatomic
Ion
Nonmetal or
Polyatomic
Ion
Mg
F
Fr
S
Ga
P
Zn
PO4
NH4
O
Cd
BrO
Ionic Formula
Name
Scandium Bromide
Lead (IV) Carbide
Iron (III) Oxide
Silver Sulfate
Sr(OH)2
Sn(C2H3O2)4
Zinc Perchlorate
Cerium Nitrite
Sodium Phosphide
17
Naming Binary Covalent Compounds
(2 non-metals)
 Write the less electronegative element first
o Electronegative Trend
 From top to bottom – decrease
 From left to right – increase
 General order of nonmetals
o C, P, N, H, S, I, Br, Cl, O, F
A. Similar to naming ionic compounds

the first nonmetal has the name as given on the periodic table

the second nonmetal has the –ide ending
Number
B. Different than naming ionic compounds


There are numerical prefixes that are used depending
on how many of each nonmetal are present in the
compound.
The only time the prefixes are not used is when there
is only one of the first nonmetal- the term mono is not
used in this case.
o NO2 = nitrogen dioxide
o NO = nitrogen monoxide
o N2O4 = dinitrogen tetroxide

Drop the “a” from tetra before adding oxide
o CO= carbon monoxide
o CO2= carbon dioxide
Prefix
1
mono-
2
di-
3
tri-
4
tetra-
5
penta-
6
hexa-
7
hepta-
8
octa-
9
nona-
10
deca-
Do NOT reduce subscripts!
18
**Do NOT reduce subscripts for covalent compounds!**
Molecular
First non-metal
Second non-metal
2 Carbons
6 Fluorines
1 Phosphorous
5 Oxygens
1 Silicon
4 Chlorines
3 Nitrogens
7 Bromines
Formula
Name
S2I4
F10Cl6
O2Br5
CN3
Trisilicon nonafluoride
Carbon monoxide
19
Naming Various Compounds
Elements
Ionic or
Covalent
Ions
Chemical
Formula
Name of Compound
4 Phosphorus +
10 Oxygens
CS2
Calcium + Chlorine
Iron (III) + Bromine
Na2O
Potassium + Sulfur
Si3N4
Triphosphorus pentasulfide
FeS
Strontium Chloride
CuO
Nitrogen Dioxide
N2O
20
Tin (IV) + Fluorine
Cl2O7
Phosphorus Triodide
CCl4
Beryllium + Fluorine
Silicon monocarbide
PCl3
Al2O3
1 Carbon + 1 Oxygen
21
Names & Formulas of Acids & Bases
How to recognize a compound/formula as being an acid or base:
Acid: has H, hydrogen, at the beginning. (Except H2O)
Base: contains OH, hydroxide.
Naming Acids
Binary Acids
 Contain H and one other element
 To name:
hydro + second element(change ending to –ic) + acid
*(exceptions: sulfur sulfuric; phosphorusphosphoric; nitrogennitric)
HCl = Hydro chlorine ic + acid
Hydrochloric acid
HF = Hydro fluorine ic + acid
Hydrofluoric acid
H 2S =
HI =
*If you are given the name and must write the formula, make sure you check
charges and do the criss-cross!
22
Ternary Acids (Oxyacids)
 Contain H, O and one more element
(a polyatomic ion with O in it; SO4)
 To Name:
For –ate and per
-ate polyatomic ions, name the non H, non O element (this is the
2nd element in the formula) and change the –ate ending to –ic.(exceptions are
sulfatesulfuric; phosphatephosphoric)
1. HNO3 = nitric acid (was nitrate)
2. H2SO4 = sulfuric acid (was sulfate)
3. HC2H3O2 = acetic acid (was acetate)
(acetate is also CH3COO)
4. H2SO5 = persulfuric acid (was persulfate)
5. H3PO4 = phosphoric acid (was phosphate)
6. HClO3 =
7. HNO4 =
8. HIO4=
-ite and hypo -ite polyatomic ions become –ous.
1. HNO2 = nitrous acid (was nitrite)
2. HNO = hyponitrous acid (was hyponitrite)
3. H2SO3 =
4. H2SO2 =
5. HClO =
6. HIO=
23
Naming Bases:
Name the metal first + hydroxide
NaOH = sodium hydroxide
Ca(OH)2 = calcium hydroxide
Fe(OH)3 = iron (III) hydroxide
*If you are given the name and must write the formula, make sure you check
charges and do the criss-cross!
24
Name ____________________________________
Ionic,
Covalent,
Binary Acid,
Formula
Chemical Name
Ternary Acid,
or
Base?
1.
H2SO2
2.
Br2Cl4
3.
Sn3(PO4)2
4.
Ba(IO3)2
5.
H2O
6.
HF
7.
Silver hydroxide
8.
Zinc perchlorate
9.
Potassium sulfite
10.
hypochlorous acid
11.
Trioxygen pentabromide
12.
Hydrosulfuric acid
25
Formula
Acid(binary or ternary)/
Base/Ionic/
or Covalent
Name
1) NaOH
__________
_____________________
2) H2SO4
__________
_____________________
3) Li2O
__________
_____________________
4) H2CO3
__________
_____________________
5) Si2Br6
__________
_____________________
6) HClO4
__________
_____________________
7) Co2(CO3)3
__________
_____________________
8) HCl
__________
_____________________
9) SCl4
__________
_____________________
10) Ca(OH)2
__________
_____________________
11) B2Si
__________
_____________________
12) Cu(HCO3)2
__________
_____________________
13) H3PO4
__________
_____________________
14) HBrO3
__________
_____________________
15) N2O3
__________
_____________________
16) IO5
__________
_____________________
17) HF
__________
_____________________
20) Na2SO3
__________
_____________________
21) CF4
__________
_____________________
22) HClO2
__________
_____________________
23) NiPO3
__________
_____________________
24) P2O5
__________
_____________________
25) NiSe
__________
_____________________
26
26) HNO2
__________
_____________________
27) Cu(C2H3O2)2
__________
_____________________
28) H2SO3
__________
_____________________
29) P4S5
__________
_____________________
30) HNO3
__________
_____________________
31) V3(PO5)5
__________
_____________________
32) Al2S3
__________
_____________________
33) HBr
__________
_____________________
34) HNO
__________
_____________________
35) H3PO3
__________
_____________________
36) Sn(OH)2
__________
_____________________
37) FeP
__________
_____________________
38) HClO3
__________
_____________________
39) NaMnO4
__________
_____________________
40) MnF3
__________
_____________________
41) Be(NO2)2
__________
_____________________
42) CO2
__________
_____________________
43) AgBr
__________
_____________________
44) Zn3(PO2)2
__________
_____________________
45) Mn(CO3)2
__________
_____________________
46) Pb3N4
__________
_____________________
27
Name ____________________________________
Fill in the Blanks!
Ionic,
Covalent,
Binary Acid,
Formula
Chemical Name
Ternary
Acid, or
Base?
1.
LiOH
2.
Cl4P6
3.
Mo(BrO2)3
4.
SnO2
5.
HClO4
6.
HF
7.
Copper(II) hydroxide
8.
Zinc persulfate
9.
Barium carbonate
10.
Hypocarbonous acid
11.
Trinitrogen pentaiodide
12.
Hydrochloric Acid
28
Name ________________________________________________
Review for Naming Compounds
Number
Ionic or
Name
Formula
Covalent
1
Strontium Phosphate
2
3
CS2
acid
H2CO3
4
Calcium Nitrate
5
Iron (III) Sulfide
6
Fe3P2
7
Germanium tetraiodide
8
LiOH
9
Mg(BrO3)2
10
Silicon Monocarbide
11
Barium Carbonite
12
Aluminum Chromate
13
acid
HF
14
15
NH4Cl
acid
Phosphorous Acid
29
Introduction:
Exploring Chemical Bonds Lab
A compound is defined as a chemical combination of two or more elements. A chemical bond is the "glue" holding
together atoms of different elements. Four types of bonds are ionic polar covalent, nonpolar covalent, and metallic. Ionic
bonds generally occur between a metallic and nonmetallic atom. The bond results from the transfer of one or more
electrons from the metallic atom to the nonmetallic atom resulting in a charge difference. The positively charged metal
ion is then attracted to the negatively charged nonmetallic ion. Covalent bonding (polar and nonpolar) involves the
sharing of electrons and generally occurs between two or more nonmetal atoms. Metallic bonding involves overlapping
of outer electrons shells and delocalization of the electrons and occurs between two or more metal atoms. Using the
chemical formula, knowledge of the periodic table, and the difference between the electronegativity values of the
elements, you can determine if a substance contains ionic, polar covalent, nonpolar covalent, or metallic bonds.
Purpose:
Explore and determine the common properties of substances that contain ionic, polar covalent, nonpolar covalent
or metallic bonds.
Materials:
NaCl (sodium Chloride)
C12H22O11 (sucrose)
C25H52 (paraffin/wax)
Al (aluminum)
distilled water
conductivity meter
hot plate
light bulb apparatus
square platform of aluminum foil
balance
spatula
stirring rod
beakers
Procedure:
1. Describe the appearance of each sample. Make sure to make note of the state of matter at room
temperature as well.
2. Test each sample with the conductivity meter and record it in the data table.
3. Measure out about 5 grams NaCl and place in a beaker with 250 mL beaker with about 150 mL of distilled
water; stir the solution to check if the NaCl dissolved and make note of it in the data table.
4. Test the conductivity of the solution in the beaker and record the value.
5. Repeat steps 3 & 4 for each substance using the following mass of each
C12H22O11 = 5 grams
C25H52 = 5 grams
Al = 0.5 grams
6. Place the square platform of aluminum foil onto the “cooled” hotplate (do not place the foil onto the
hotplate if the surface is still hot).
7. Carefully place a small sample (pea sized) of each substance, excluding Al, onto your foil platform.
8. Turn the hotplate on to a setting of 5.
9. Observe the samples and rank them by relative melting point. 1= melted first, 2= melted second, etc.
After 7 minutes, turn off the hotplate. If a sample did not melt, then you know it has a high melting
point.
10. Carefully remove the foil platform using crucible tong and dispose of it in the trash.
11. Lastly, your teacher will demonstrate the conductive ability of a solution of each sample using the light
bulb apparatus. If it lights up the light bulb, then the solution is a very good conductor.
30
Data Table:
Name:____________________________________
Substance
NaCl (sodium C12H22O11
(sucrose)
Chloride)
C25H52
(paraffin/wax)
Al (aluminum)
Type of Bond
Present
Appearance
Ionic Bond
Nonpolar
Covalent Bond
Metallic Bond
Polar Covalent
Bond
State at Room
Temp.
Conductivity
(dry; not in
solution)
Solubility in
Water
Conductivity
of Solution
Relative
Melting Point
Light Bulb
Conductivity
Test
Analysis/Conclusion:
Electrolytes:



When placed in an aqueous solution (water) ionically bonded substances dissociate into their ions and
demonstrate the ability to conduct electricity very well (can conduct electrical current in the water).
These are considered strong electrolytes.
Some covalently bonded substances also have the ability to conduct electricity at low levels. These are
considered weak electrolytes.
Finally, there are many substances that, when placed in water do not dissociate into ions. As a result,
these substances fail to conduct electricity. These are considered non electrolytes.
31
Write a short paragraph (sentences) to summarize your findings about substances that contain the type of
chemical bond underneath each heading below.
Ionic bonded substances:
Polar covalent bonded substances:
Nonpolar covalent bonded substances:
Metallic bonded substances:
32