Structural representation of organic compounds
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This document discusses different methods for structurally representing organic compounds, including: - Complete, condensed, and bond-line structural formulas that use dashes of different lengths to represent single, double, and triple bonds between atoms. - Further abbreviating structural formulas by omitting dashes and using subscripts to indicate identical groups attached to an atom. - Bond-line representations that do not show carbon/hydrogen atoms and use zig-zag lines between carbons and labels for other atoms to depict molecular structure. - Molecular models including framework, ball-and-stick, and space-filling models used to visualize the 3D structure of organic molecules.
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Electron-dot notation represents valence electrons of atoms using dots placed around the element's symbol. It can show molecules by combining the notations of atoms joined by covalent bonds, represented as shared pairs of dots or dashes. Lewis structures use this notation to represent covalent bonding, showing shared pairs between atoms but not unshared electron pairs. Atoms can form multiple bonds by sharing more than one electron pair, shown as double or triple bonds. Some molecules like ozone cannot be fully represented by a single Lewis structure and instead use resonance structures that average the bonding.
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Section 3.2 What ls the Octet Rule?
3.17 Answer true or false. '
(a) The octet rule refers to the chemical bonding
patterns of the first eight elements of the
Periodic Table.
(b) The octet rule refers to the tendency ofcertain
elements to react in such a way that they achieve
an outer shell ofeight valence electrons.
(c) In gaining electrons, an atom becomes a posi-
tively charged ion called a cation.
(d) When an atom forms an ion, only the number of
. valence electrons changes; the number ofprotons
and neutrons in the nucleus does not change.
(e) In forming ions, Group 2A elements typically
lose two electrons to become cations with a
charge of +2.
(f) In forming an ion, a sodium atom (1s22s22p63s1)
completes its valence shell by adding one elec-
tron to filI its 3s shell (k22s22p63s2).
(g) The elements of Group 6A typically react by ac-
cepting two electrons to become anions with a
charge of -2.
(h) With the exception of hydrogen, the octet rule
applies to all elements in periods 1,2, and 3.
(i) Atoms and the ions derived from them have very
similar physical and chemical properties.
3.18 How many electrons must each atom gain or lose
to acquire an electron configuration identical to the
noble gas nearest to it in atomic number?
(a) Li (b) Cl (c) P (d) Al
(e) Sr (f) S (e) Si (h) O
3.19 Show how each chemical change obeys the octet
rule.
(a) Lithium forms Li* (b) Oxygen forms O
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H- (hydride ion)
(b) Aluminum forms Al3+
3,2L Write the formula for the most stable ion formed by
each element.
(a) Mg (b) F (c)
(d) s (e) K (I)
3.22 Why is Li- not a stable ion?
3.23 Predict which ions are stable:
(a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+
3,24 Predict which ions are stable:
(a) Br2- (b) C4- (c) Ca*
(d) Ar* (e) Na* (I) Cs*
a
3.25 Why are carbon and silicon reluctant to foil
bonds?
3.26 Table 3.2 shows the following ions of co14m
and Cu2*. Do these violate the octet rule?
Section 3.3 How Do We Name Anions
and Cations?
5.27 Answer true or false.
(a) For Group 1A and Group 2A elements,fte
of the ion each forms is simply the nare
element followed by the word ion; for
Mg2* is named magnesium ion.
(b) H+ is named hydronium ion, and H is
hydride ion.
(c) The nucleus of H* consists of one proton
neutron.
(d) Many transition and inner transition
form more than one positively charged irn I
(e) In naming metal cations with two diffemed
charges, the suffix -oas refers to the ion
a charge of + 1 and -ic refers to the ion wift
charge of +2.
(f) Fe3* may be named either iron(III) ion or
(g) The anion derived from a bromine atom is
bromine ion.
(h) The anion derived from an oxygen atomis
named oxide ion.
(i) HCO; is named hydrogen carbonate ion- .
0) The prefrx bi- in the name "bicarbonate'im
indicates that this ion h.
Nomenclature
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This document provides an overview of organic chemistry, including key topics such as:
- Organic compounds contain carbon and are found in many common materials.
- Organic chemistry is the study of organic compounds, their structures, properties, and reactions.
- Carbon atoms can form multiple bonds with other carbons, allowing for a large number of organic compounds.
- Hydrocarbons are organic compounds made of only carbon and hydrogen, and can be classified as aliphatic or aromatic.
2007 ch158 a3_basicsorg_update_for_2009 (1)
1. The document discusses the basics of organic chemistry including nomenclature of organic compounds, functional groups, molecular structure and bonding.
2. Key concepts covered include IUPAC naming rules, identifying primary, secondary and tertiary carbons, common functional groups, covalent and ionic bonding, and molecular orbital theory.
3. Bond polarity is discussed, noting that bonds between carbon and more electronegative atoms like oxygen are polarized with partial positive and negative charges.
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Ch6 2
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I -s2o.100 Chapter 3 Chemical BondsUWL tnteractive ve.docx
I -s'2o.
100 Chapter 3 Chemical Bonds
UWL tnteractive versions of these problems may be assigned
in OWL.
Orange-numbered problems are applied.
Section 3.2 What ls the Octet Rule?
3.17 Answer true or false. '
(a) The octet rule refers to the chemical bonding
patterns of the first eight elements of the
Periodic Table.
(b) The octet rule refers to the tendency ofcertain
elements to react in such a way that they achieve
an outer shell ofeight valence electrons.
(c) In gaining electrons, an atom becomes a posi-
tively charged ion called a cation.
(d) When an atom forms an ion, only the number of
. valence electrons changes; the number ofprotons
and neutrons in the nucleus does not change.
(e) In forming ions, Group 2A elements typically
lose two electrons to become cations with a
charge of +2.
(f) In forming an ion, a sodium atom (1s22s22p63s1)
completes its valence shell by adding one elec-
tron to filI its 3s shell (k22s22p63s2).
(g) The elements of Group 6A typically react by ac-
cepting two electrons to become anions with a
charge of -2.
(h) With the exception of hydrogen, the octet rule
applies to all elements in periods 1,2, and 3.
(i) Atoms and the ions derived from them have very
similar physical and chemical properties.
3.18 How many electrons must each atom gain or lose
to acquire an electron configuration identical to the
noble gas nearest to it in atomic number?
(a) Li (b) Cl (c) P (d) Al
(e) Sr (f) S (e) Si (h) O
3.19 Show how each chemical change obeys the octet
rule.
(a) Lithium forms Li* (b) Oxygen forms O
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H- (hydride ion)
(b) Aluminum forms Al3+
3,2L Write the formula for the most stable ion formed by
each element.
(a) Mg (b) F (c)
(d) s (e) K (I)
3.22 Why is Li- not a stable ion?
3.23 Predict which ions are stable:
(a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+
3,24 Predict which ions are stable:
(a) Br2- (b) C4- (c) Ca*
(d) Ar* (e) Na* (I) Cs*
a
3.25 Why are carbon and silicon reluctant to foil
bonds?
3.26 Table 3.2 shows the following ions of co14m
and Cu2*. Do these violate the octet rule?
Section 3.3 How Do We Name Anions
and Cations?
5.27 Answer true or false.
(a) For Group 1A and Group 2A elements,fte
of the ion each forms is simply the nare
element followed by the word ion; for
Mg2* is named magnesium ion.
(b) H+ is named hydronium ion, and H is
hydride ion.
(c) The nucleus of H* consists of one proton
neutron.
(d) Many transition and inner transition
form more than one positively charged irn I
(e) In naming metal cations with two diffemed
charges, the suffix -oas refers to the ion
a charge of + 1 and -ic refers to the ion wift
charge of +2.
(f) Fe3* may be named either iron(III) ion or
(g) The anion derived from a bromine atom is
bromine ion.
(h) The anion derived from an oxygen atomis
named oxide ion.
(i) HCO; is named hydrogen carbonate ion- .
0) The prefrx bi- in the name "bicarbonate'im
indicates that this ion h.
Nomenclature
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Notes
This document provides an overview of organic chemistry, including key topics such as:
- Organic compounds contain carbon and are found in many common materials.
- Organic chemistry is the study of organic compounds, their structures, properties, and reactions.
- Carbon atoms can form multiple bonds with other carbons, allowing for a large number of organic compounds.
- Hydrocarbons are organic compounds made of only carbon and hydrogen, and can be classified as aliphatic or aromatic.
2007 ch158 a3_basicsorg_update_for_2009 (1)
1. The document discusses the basics of organic chemistry including nomenclature of organic compounds, functional groups, molecular structure and bonding.
2. Key concepts covered include IUPAC naming rules, identifying primary, secondary and tertiary carbons, common functional groups, covalent and ionic bonding, and molecular orbital theory.
3. Bond polarity is discussed, noting that bonds between carbon and more electronegative atoms like oxygen are polarized with partial positive and negative charges.
Similar to Structural representation of organic compounds (20)
Introduction to organic chemistry Foundation In science
Introduction to organic chemistry Foundation In science
I -s2o.100 Chapter 3 Chemical BondsUWL tnteractive ve.docx
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Structural representation of organic compounds
- 1. STRUCTURAL REPRESENTATIONS OF ORGANIC COMPOUNDS • Complete, Condensed and Bond-line Structural Formulas The Lewis structures can be simplified by representing the two- electron covalent bond by a dash (–). Such a structural formula focuses on the electrons involved in bond formation. A single dash represents a single bond, double dash is used for double bond and a triple dash represents triple bond. Lone pairs of electrons on heteroatoms (e.g., oxygen, nitrogen, sulphur, halogens etc.) may or may not be shown. Thus, ethane (C2H6), ethene (C2H4), ethyne (C2H2) and methanol (CH3OH) can be represented by the following structural formulas. Such structural representations are called complete structural formulas. DRAW OPEN FULL STRUCTURES
- 2. • These structural formulas can be further abbreviated by omitting some or all of the dashes representing covalent bonds and by indicating the number of identical groups attached to an atom by a subscript. The resulting expression of the compound is called a condensed structural formula. Thus, propane, butene, ethyne and pentanol can be written as: • CH3CH3 H2C=CH2 HCºCH CH3OH • Ethane Ethene Ethyne Methanol • Similarly, CH3CH2CH2CH2CH2CH2CH2CH3 can be further condensed to CH3(CH2)6CH3.
- 3. Another way of representing the structures, in which only lines are used. In this bond-line structural representation of organic compounds, carbon and hydrogen atoms are not shown and the lines representing carbon-carbon bonds are drawn in a zig-zag fashion. The only atoms specifically written are oxygen, chlorine, nitrogen etc. The terminals denote methyl (–CH3) groups (unless indicated otherwise by a functional group), while the line junctions denote carbon atoms bonded to appropriate number of hydrogens required to satisfy the valency of the carbon atoms. Some of the examples are represented as follows: • (i) 3-Methyloctane can be represented in various forms as • Various ways of representing 2-bromo butane are: • 2-hexene or hex-2-ene, 2 bromo, 4-chloro pentane • In cyclic compounds, the bond-line formulas may be given as follows:
- 4. Molecular Models Molecular models are physical devices that are used for a better visualisation and perception of three- dimensional shapes of organic molecules. These are made of wood, plastic or metal and are commercially available. Commonly three types of molecular models are used: (1) Framework model, only bonds shown emphasizes the pattern of bonds of a molecule while ignoring the size of atoms. (2)Ball-and-stick model, Compounds containing C=C (e.g., ethene) can best be represented by using springs in place of sticks. and (3) Space filling model- emphasises the relative size of each atom based on its van der Waals radius. Bonds are not shown in this model. It conveys the volume occupied by each atom in the molecule. In addition to these models, computer graphics can also be