bonding and naming
DESCRIPTION
drfgftghnrtyTRANSCRIPT
![Page 1: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/1.jpg)
BONDING AND NAMING
1
![Page 2: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/2.jpg)
2
Metals form cations and nonmetals form anions to attain a stable valence electron structure.
![Page 3: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/3.jpg)
3
This stable structure often consists of two s and six p electrons.These rearrangements occur by losing, gaining, or sharing electrons.
![Page 4: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/4.jpg)
4
• Na with the electron structure 1s22s22p63s1
has 1 valence electron.
The Lewis structure of an atom is a representation that shows the valenceelectrons for that atom.
• Fluorine with the electron structure 1s22s22p5
has 7 valence electrons
![Page 5: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/5.jpg)
6
The Ionic Bond: Transfer ofThe Ionic Bond: Transfer ofElectrons From One AtomElectrons From One Atom
to Anotherto Another
![Page 6: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/6.jpg)
7
The chemistry of many elements, especially the representative ones, is to attain the same outer electron structure as one of the noble gases.
![Page 7: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/7.jpg)
8
With the exception of helium, this structure consists of eight electrons in the outermost energy level.
![Page 8: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/8.jpg)
9
After sodium loses its 3s electron it has attained the same electronic structure as neon.
![Page 9: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/9.jpg)
10
After chlorine gains a 3p electron it has attained the same electronic structure as argon.
![Page 10: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/10.jpg)
11
Formation of NaClFormation of NaCl
![Page 11: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/11.jpg)
12
The 3s electron of sodium transfers to the half-filled 3p orbital of chlorine.
Lewis representation of sodium chloride formation.
A sodium ion (Na+) and a chloride ion (Cl-) are formed.
The force holding Na+ and Cl- together is an ionic bond.
![Page 12: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/12.jpg)
13
Formation of MgCl2Formation of MgCl2
![Page 13: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/13.jpg)
14
Two 3s electrons of magnesium transfer to the half-filled 3p orbitals of two chlorine atoms.A magnesium ion (Mg2+) and two chloride ions (Cl-) are formed.The forces holding Mg2+ and two Cl- together are ionic bonds.
![Page 14: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/14.jpg)
15
• Metals usually have one, two or three electrons in their outer shells.
• When a metal reacts it:– usually loses one two or three electrons
– attains the electron structure of a noble gas
– becomes a positive ion.
• The positive ion formed by the loss of electrons is much smaller than the metal atom.
![Page 15: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/15.jpg)
16
• Nonmetals usually have five, six or seven electrons in their outer shells.
• When a nonmetal reacts it:– usually gains one, two or three electrons
– attains the electron structure of a noble gas
– becomes a negative ion.
• The negative ion formed by the gain of electrons is much larger than the nonmetal atom.
![Page 16: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/16.jpg)
17
The Covalent Bond:The Covalent Bond: Sharing ElectronsSharing Electrons
![Page 17: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/17.jpg)
18
A covalent bond consists of a pair of electrons shared between two atoms.
In the millions of chemical compounds that exist, the covalent bond is the predominant chemical bond.
![Page 18: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/18.jpg)
19
Substances which covalently bond exist as molecules.
Carbon dioxide bonds covalently. It exists as individually bonded covalent molecules containing one carbon and two oxygen atoms.
11.7
![Page 19: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/19.jpg)
20
The term molecule is not used when referring to ionic substances.
Sodium chloride bonds ionically. It consists of a large aggregate of positive and negative ions. No molecules of NaCl exist.
11.7
![Page 20: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/20.jpg)
21
Covalent bonding in the hydrogen molecule
Two 1s orbitals from each of two hydrogen atoms overlap.
Each 1s orbital contains 1 electron.
The orbital of the electrons includes both hydrogen nuclei.
The most likely region to find the two electrons is between the two nuclei.
The two nuclei are shielded from each other by the electron pair. This allows the two nuclei to draw close together.
Two 1s orbitals from each of two hydrogen atoms overlap.
11.8
![Page 21: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/21.jpg)
22
11.9
Covalent bonding in the chlorine molecule
Each unpaired 3p orbital on each chlorine atom contains 1 electron.
Two 3p orbitals from each of two chlorine atoms overlap.
The orbital of the electrons includes both chlorine nuclei.
The most likely region to find the two electrons is between the two nuclei.
The two nuclei are shielded from each other by the electron pair. This allows the two nuclei to draw close together.
Two 3p orbitals from each of two chlorine atoms overlap.
Each chlorine now has 8electrons in its outermost energy level.
![Page 22: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/22.jpg)
23
hydrogen chlorine iodine nitrogen
Covalent bonding with equal sharing of electrons occurs in diatomic molecules formed from one element.
A dash may replace a pair of dots.
H - H
![Page 23: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/23.jpg)
24
Common and Common and Systematic NamesSystematic Names
![Page 24: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/24.jpg)
25
Chemical nomenclature is the system of names that chemists use to identify compounds. Two classes of names exist: common names and systematic names.
![Page 25: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/25.jpg)
26
– They are not based on the composition of the compound.
– They are based on an outstanding chemical or physical property.
• Chemists prefer systematic names.– Systematic names precisely identify
the chemical composition of the compound.
– The present system of inorganic chemical nomenclature was devised by the International Union of Pure and Applied Chemistry (IUPAC).
• Common names are arbitrary names.
![Page 26: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/26.jpg)
27
![Page 27: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/27.jpg)
28
Elements and IonsElements and Ions
![Page 28: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/28.jpg)
29
The formula for most elements is the symbol of the element.
Sodium Na
Potassium K
Zinc Zn
Argon Ar
Mercury Hg
Lead Pb
Calcium Ca
![Page 29: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/29.jpg)
30
Hydrogen H2
Nitrogen N2
Oxygen O2
Fluorine F2
Chlorine Cl2
Bromine Br2
Iodine I2
These 7 elements are found in nature as diatomic molecules.
![Page 30: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/30.jpg)
31
Sulfur S8
Phosphorous P4
Two elements are commonly polyatomic.
![Page 31: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/31.jpg)
32
Naming CationsNaming Cations
![Page 32: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/32.jpg)
33
Cations are named the same as their parent atoms
![Page 33: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/33.jpg)
34
Atom
Cation
Name of Cation
sodium (Na)
Na+
sodium ion
![Page 34: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/34.jpg)
35
Atom
Cation
Name of Cation
calcium (Ca)
Ca2+
calcium ion
![Page 35: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/35.jpg)
36
Atom
Cation
Name of Cation
lithium (Li)
Li+
lithium ion
![Page 36: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/36.jpg)
37
Atom
Cation
Name of Cation
magnesium (Mg)
Mg2+
magnesium ion
![Page 37: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/37.jpg)
38
Atom
Cation
Name of Cation
strontium (Sr)
Sr2+
strontium ion
![Page 38: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/38.jpg)
39
Naming AnionsNaming AnionsNaming AnionsNaming Anions
![Page 39: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/39.jpg)
40
An anion consisting of one element has the stem of the parent element and an –ide ending
![Page 40: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/40.jpg)
41
Atom
Anion
Name of Anion
Atom
Anion
Name of Anion
fluorine (F)
F-
fluoride ion
stem
![Page 41: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/41.jpg)
42
Atom
Anion
Name of Anion
Atom
Anion
Name of Anion
chlorine (Cl)
Cl-
chloride ion
stem
![Page 42: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/42.jpg)
43
Atom
Anion
Name of Anion
bromine (Br)
Br-
bromide ion
stem
![Page 43: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/43.jpg)
44
Atom
Anion
Name of Anion
nitrogen (N)
N3-
nitride ion
stem
![Page 44: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/44.jpg)
45
Atom
Anion
Name of Anion
phosphorous (P)
P3-
phosphide ion
stem
![Page 45: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/45.jpg)
46
Atom
Anion
Name of Anion
oxygen (O)
O2-
oxide ion
stem
![Page 46: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/46.jpg)
47
Binary CompoundsBinary Compounds
![Page 47: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/47.jpg)
48
Binary compounds contain only two different elements.
![Page 48: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/48.jpg)
49
Binary ionic compounds consist of a metal combined with a non-metal.
![Page 49: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/49.jpg)
50
A. Binary Ionic Compounds Containing A. Binary Ionic Compounds Containing a Metal Forming Only One Type of a Metal Forming Only One Type of
CationCation
![Page 50: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/50.jpg)
51
• The chemical name is composed of the name of the metal followed by the name of the nonmetal which has been modified to an identifying stem plus the suffix –ide.
• Using this system the number of atoms of each element present is not expressed in the name.
![Page 51: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/51.jpg)
52
Name of Metal
+ Stem of Nonmetal
plus -ide ending
![Page 52: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/52.jpg)
53
![Page 53: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/53.jpg)
54
Step 1 From the formula it is a two-element compound and follows the rules for binary compounds.
Name the Compound CaF2
![Page 54: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/54.jpg)
55
Name the Compound CaF2
Step 2 The compound is composed of Ca, a metal and F, a nonmetal. Ca forms only a +2 cation. Thus, call the positive part of the compound calcium.
![Page 55: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/55.jpg)
56
Step 3 Modify the name of the second element to the stem fluor- and add the binary ending –ide to form the name of the negative part, fluoride.
Name the Compound CaF2
![Page 56: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/56.jpg)
57
Step 4 The name of the compound is therefore calcium fluoride.
Name the Compound CaF2
![Page 57: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/57.jpg)
58
ExamplesExamples
![Page 58: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/58.jpg)
59
Compound
Name sodiumchloride
NaCl
nonmetal stem
name of metal
![Page 59: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/59.jpg)
60
Compound
Name magnesiumchloride
MgCl2
nonmetal stem
name of metal
![Page 60: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/60.jpg)
61
Compound
Name potassiumoxide
K2O
nonmetal stem
name of metal
![Page 61: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/61.jpg)
62
Compound
Name sodiumphosphide
Na3P
nonmetal stem
name of metal
![Page 62: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/62.jpg)
63
B. Binary Ionic Compounds Containing a B. Binary Ionic Compounds Containing a
MetalMetal
That Can Form Two or More Types of That Can Form Two or More Types of
CationsCations
![Page 63: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/63.jpg)
64
Name the Compound FeS
Step 1 This compound follows the rules for a binary compound.
![Page 64: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/64.jpg)
65
Step 2 It is a compound of Fe, a metal, and S, a nonmetal, and Fe is a transition metal that has more than one type of cation.
Name the Compound FeS
Step 2 In sulfides, the charge on S is –2. Therefore the charge on Fe must be +2, and the name of the positive part of the compound is iron (II).
![Page 65: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/65.jpg)
66
Step 3 We have already determined that the name of the negative part of the compound will be sulfide.
Name the Compound FeS
![Page 66: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/66.jpg)
67
Step 4 The name of FeS is iron(II) sulfide.
Name the Compound FeS
![Page 67: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/67.jpg)
68
The metals in the center of the periodic table (including the transition metals) often form more than one type of cation.
![Page 68: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/68.jpg)
69
Each ion of iron forms a different compound with the same anion.
Fe2+
Fe3+
FeS
Fe2S3
![Page 69: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/69.jpg)
70
The Classical SystemThe Classical System
![Page 70: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/70.jpg)
71
In the Classical System the name of the metal (usually the Latin name) is modified with the suffixes -ous and ic.
![Page 71: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/71.jpg)
72
-ous lower charge
-ic higher charge
Metal name ends in
nonmetal name ends in
-ide
![Page 72: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/72.jpg)
73
Lower Charge Higher Charge
Element Formula Name Formula Name
Copper Cu+ cuprous Cu2+ Cupric
Iron Fe2+ ferrous Fe3+ ferric
Lead Pb2+ plumbous Pb4+ plumbic
Mercury Hg mercurous Hg2+ mercuric
Tin Sn2+ stannous Sn4+ stannic
Ion Names: Classical System
![Page 73: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/73.jpg)
74
Examples
![Page 74: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/74.jpg)
75
ion chargeion name
FeCl2
ferrous chloride
+2 -1chlorideferrous
FeCl3
ferric chloride
-1+3ferric chloride
compound name
![Page 75: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/75.jpg)
76
ion chargeion name
SnBr2
stannous bromide
+2 -1bromidestannous
SnBr4
stannic bromide
-1+4stannic bromide
compound name
![Page 76: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/76.jpg)
77
The Stock SystemThe Stock System
![Page 77: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/77.jpg)
78
IUPAC devised the Stock System of nomenclature to name compounds of metals that have more than one type of cation.
Cation Charge
+1 +2 +3 +4 +5
Roman Numeral
I II III IV V
In the Stock System the charge on the cation is designated by a Roman numeral placed in parentheses immediately following the name of the metal.
The nonmetal name ends in -ide.
![Page 78: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/78.jpg)
79
Stock SystemLower Charge Higher Charge
Element Formula Name Formula Name
Copper Cu+ copper (I) Cu2+ copper (II)
Iron Fe2+ iron(II) Fe3+ iron(III)
Lead Pb2+ lead (II) Pb4+ lead(IV)
Mercury Hg22+ mercury(I) Hg2+ mercury(II)
Tin Sn2+ Tin(II) Sn4+ Tin (II)
Stock System Higher Charge
Element Formula Name Formula Name
Lower Charge
![Page 79: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/79.jpg)
80
ExamplesExamples
![Page 80: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/80.jpg)
81
ion chargeion name
FeCl2
iron(II) chloride
+2 -1chlorideiron(II)
FeCl3
iron(III) chloride
-1+3iron(III) chloride
compound name
![Page 81: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/81.jpg)
82
ion chargeion name
SnBr2
tin(II) bromide
+2 -1bromidetin(II)
SnBr4
tin(IV) bromide
-1+4tin(IV) bromide
compound name
![Page 82: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/82.jpg)
83
Binary Compounds Binary Compounds Containing Two Containing Two
NonmetalsNonmetals
![Page 83: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/83.jpg)
84
Compounds between nonmetals are molecular, not ionic.
![Page 84: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/84.jpg)
85
In a compound formed between two nonmetals, the element that occurs first in this series is named first.
• Si
• B
• P
• H
• C
• S
• I
• Br
• N
• Cl
• O
• F
![Page 85: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/85.jpg)
86
PrefixesPrefixes
![Page 86: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/86.jpg)
87
A Greek prefix is placed before the name of each element to indicate the number of atoms of the element that are present.
![Page 87: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/87.jpg)
88
• di = 2
• tri = 3
• tetra = 4
• penta = 5
• hexa = 6
• hepta = 7
• octa = 8
• nona = 9
• deca = 10
• mono = 1
Mono is rarely used when naming the first element.
![Page 88: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/88.jpg)
89
ExamplesExamples
![Page 89: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/89.jpg)
90
N2O3
dinitrogen trioxide
indicates twonitrogen atoms
indicates threeoxygen atoms
![Page 90: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/90.jpg)
91
PCl5
phosphorous pentachloride
indicates onephosphorous atom
indicates fivechlorine atoms
![Page 91: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/91.jpg)
92
Cl2O7
dichlorine heptaoxide
indicates twochlorine atoms
indicates sevenoxygen atoms
![Page 92: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/92.jpg)
93
Step 1
• There are 2 elements present.
• The compound is binary.
• Phosphorous and chlorine are nonmetals so the rules for naming binary compounds of 2 nonmetals apply.
• Phosphorous is named first. Therefore the compound is a chloride.
Determine the Name of PCl5
![Page 93: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/93.jpg)
94
Step 2
• No prefix is needed for phosphorous because each molecule of PCl5 has only one phosphorous atom. The prefix penta- is used with chloride because there are 5 chlorine atoms present in one molecule.
Step 3
• The name is phosphorous pentachloride.
Determine the Name of PCl5
![Page 94: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/94.jpg)
95
ExamplesExamples
![Page 95: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/95.jpg)
96
dichlorine trioxide
Cl2O3
![Page 96: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/96.jpg)
97
dinitrogen trioxide
N2O3
![Page 97: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/97.jpg)
98
carbon tetrachloride
CCl4
![Page 98: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/98.jpg)
99
carbon monoxide
CO
![Page 99: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/99.jpg)
100
carbon dioxide
Name CO2
![Page 100: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/100.jpg)
101
phosphorous triiodide
Name PI3
![Page 101: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/101.jpg)
102
D. Acids DerivedD. Acids Derivedfrom Binary Compoundsfrom Binary Compounds
![Page 102: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/102.jpg)
103
• Certain binary hydrogen compounds, when dissolved in water, form solutions that have acid properties.
• The aqueous solutions of these compounds are given acid names.
• The acid names are in addition to their –ide names.
• Hydrogen is typically the first element of a binary acid formula.
![Page 103: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/103.jpg)
104
Dissolved in water acidHCl
Pure compound HCl -ide
![Page 104: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/104.jpg)
105
• To name binary acids write the symbol of hydrogen first.
• After hydrogen write the symbol of the second element.
• Place the prefix hydro- in front of the stem of the nonmetal name.
• Place the suffix -ic after the stem of the nonmetal name.
![Page 105: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/105.jpg)
106
ExamplesExamples
![Page 106: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/106.jpg)
107
HClhydrogen chloride
Pure Compound
![Page 107: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/107.jpg)
108
HClhydrochloric acid
Dissolved in Water
![Page 108: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/108.jpg)
109
HIhydrogen iodide
Pure Compound
![Page 109: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/109.jpg)
110
HIhydroiodic acid
Dissolved in Water
![Page 110: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/110.jpg)
111
H2Shydrogen sulfide
Pure Compound
![Page 111: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/111.jpg)
112
H2Shydrosulfic acid
Dissolved in Water
![Page 112: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/112.jpg)
113
H2Sehydrogen selenide
Pure Compound
![Page 113: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/113.jpg)
114
H2Sehydroselenic acid
Dissolved in Water
![Page 114: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/114.jpg)
115
![Page 115: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/115.jpg)
116
Naming Compounds Naming Compounds
Containing Polyatomic IonsContaining Polyatomic Ions
![Page 116: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/116.jpg)
117
A polyatomic ion is an ion that contains two or more elements.
-3NO
![Page 117: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/117.jpg)
118
2 3Na CO
• They usually consist of one or more cations combined with a negative polyatomic ion.
• Compounds containing polyatomic ions are composed of three or more elements.
![Page 118: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/118.jpg)
119
• When naming a compound containing a polyatomic ion, name the cation first and then name the anion.
2 3Na CO
![Page 119: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/119.jpg)
120
4KMnO
+K -4MnO
The ions are what isactually present.
This is the way theformula is written.
![Page 120: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/120.jpg)
121
This is the way theformula is written.
2 3Na CO
The ions are what isactually present.
+2Na 2-3CO
![Page 121: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/121.jpg)
122
Prefixes and SuffixesPrefixes and Suffixes
Elements that Form More than Elements that Form More than One Polyatomic Ion with One Polyatomic Ion with
OxygenOxygen
![Page 122: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/122.jpg)
123
Anions ending in -ate always contain more oxygen than ions ending in -ite.
nitrate-3NO
nitrite-2NO
![Page 123: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/123.jpg)
124
Anions ending in -ate always contain more oxygen than ions ending in -ite.
phosphate3-4PO
phosphite-3PO
![Page 124: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/124.jpg)
125
Anions ending in -ate always contain more oxygen than ions ending in -ite.
sulfate2-4SO
sulfite-3SO
-ate and –ite do not indicate the number of oxygen atoms.
![Page 125: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/125.jpg)
126
per- denotes anions with more oxygen than the -ate form.
perchlorate-4ClO
chlorate-3ClO
![Page 126: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/126.jpg)
128
hypo- denotes anions with less oxygen than the -ite form.
Chlorite-3ClO
hypochlorite-ClO 2
![Page 127: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/127.jpg)
130
Four ions do not use the –ate/ite system.
hydroxide-OH
hydrogen sulfide-HS
cyanide-CN
peroxide2-2O
![Page 128: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/128.jpg)
131
There are three common positively charged polyatomic ions.
ammonium+4NH
hydronium+
3H O
mercury(I)2+2Hg
![Page 129: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/129.jpg)
132
![Page 130: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/130.jpg)
133
AcidsAcidsAcidsAcids
![Page 131: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/131.jpg)
134
• The other element is usually a nonmetal, but it can be a metal.
• Its first element is hydrogen.
• Its remainingelements include oxygen and form a polyatomic ion.
Oxy-acids contain hydrogen, oxygen and one other element.
![Page 132: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/132.jpg)
135
Hydrogen in an oxy-acid is not expressed in the acid name.
The word acid in the name indicates the presence of hydrogen.
![Page 133: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/133.jpg)
136
contains oxygen
contains sulfur
contains hydrogen
indicates hydrogen
sulfuric acid 42SOH
![Page 134: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/134.jpg)
137
Anions ending in -ate always contain more oxygen than ions ending in -ite.
phosphate3-4PO
phosphite-3PO
![Page 135: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/135.jpg)
138
Naming the Acid Based on the Name of the Polyatomic Ion
Ending of Polyatomic Ion
more oxygen
less oxygenite
ate
Ending of Acid
ous
ic
![Page 136: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/136.jpg)
139
ExamplesExamples
![Page 137: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/137.jpg)
140
sulfite23SO
sulfurous acid 2 3H SO
![Page 138: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/138.jpg)
141
sulfate24SO
sulfuric acid 2 4H SO
![Page 139: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/139.jpg)
142
nitrite 2NO
nitrous acid 2HNO
![Page 140: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/140.jpg)
143
nitrate 3NO
nitric acid 3HNO
![Page 141: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/141.jpg)
144
![Page 142: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/142.jpg)
145
![Page 143: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/143.jpg)
146
![Page 144: Bonding and Naming](https://reader030.vdocument.in/reader030/viewer/2022032700/563db837550346aa9a91a113/html5/thumbnails/144.jpg)
147