Atoms,Molecules,

and Ions

Chapter 2Atoms,

Molecules,and Ions

John D. Bookstaver

St. Charles Community College

St. Peters, MO

2006, Prentice Hall, Inc.

Chemistry, The Central Science, 10th editionTheodore L. Brown; H. Eugene LeMay, Jr.;

and Bruce E. Bursten

Atoms,Molecules,

and Ions

2. 1

The Atomic Theory of

Matter

Atoms,Molecules,

and Ions

Democritus (400 BC)• This is the Greek philosopher

Democritus• His theory: Matter could not be

divided into smaller and smaller pieces forever• eventually the smallest

possible piece would be obtained.

• This piece would be indivisible.

• He named the smallest piece of matter “atomos,” meaning “not to be cut.”

Atoms,Molecules,

and Ions

• Democritus’s theory was forgotten for over 2000 years

• The philosophers of the time, Aristotle and Plato, had a more respected, (and ultimately wrong) theory.

• Aristotle and Plato favored the earth, fire, air and water approach to the nature of matter.

Atoms,Molecules,

and Ions

Atomic Theory of Matter

• The theory that atoms are the fundamental building blocks of matter reemerged in the early 19th century, championed by John Dalton.

Known as the “Father of the Atom”

First scientist to support the existence of the atom with scientific evidence

Atoms,Molecules,

and Ions

Dalton’s Postulates1) Elements are made up of atoms

2) Atoms of each element are identical (in mass and properties). Atoms of different elements are different.

3) Chemical reactions are a rearrangement of atoms. Atoms are not created or destroyed.

4) Compounds are formed when atoms of multiple elements combine. Each compound has specific numbers and kinds of atoms.

Atoms,Molecules,

and Ions

Dalton’s Atomic Theory• He deduced that all

elements are composed of atoms. Atoms are indivisible and indestructible particles.

• Atoms of the same element are exactly alike.

• Atoms of different elements are different.

• Compounds are formed by the joining of atoms of two or more elements.

Atoms,Molecules,

and Ions

Law of Constant Composition

• From Dalton’s 4th postulate• Also known as the law of definite

proportions.• The elemental composition of a pure

substance never varies. In a compound or element, the numbers

and kinds of atoms are constant.

Atoms,Molecules,

and Ions

Law of Multiple Proportions• When chemical elements combine, they do so in a ratio of

small whole numbers. For example, carbon and oxygen react to form carbon

monoxide (CO) or carbon dioxide (CO2), but not CO1.3.

• Further, if two elements, A & B, combine to form more than one compound, the masses of B that combine with a given mass A are in the ratio of small whole numbers

• Example:

Water H2O vs Hydrogen Peroxide H2O2

Mass O = 16 g Mass O = 32 g

Mass H = 2 g Mass H = 2 g

Oxygen 32 g : 16 g = 2

Hydrogen 2 g : 2 g = 1

Atoms,Molecules,

and Ions

Law of Conservation of Mass

• From Dalton’s 3rd postulate• The total mass of substances present at

the end of a chemical reaction is the same as the mass of substances present before the reaction took place.

Atoms,Molecules,

and Ions

2. 2

Discovery of Atomic

Structure

Atoms,Molecules,

and Ions

J.J. Thompson’s Experiment• Using a cathode ray tube Thompson

found that passing an electric current makes a beam of radiation appear to move from the negative to the positive end

• By adding an electric field to the cathode ray tube, he found that the beam deflected towards the positive field so he deduces that the components of the beam were negative

Atoms,Molecules,

and Ions

Cathode Rays & Electrons• Radiation was passed through a tube from

the cathode (negative end) to the anode (positive end) The radiation would fluoresce (give off light) When an electric/magnetic field was applied, the

cathode rays deflected in a manner consistent with a stream of negative particles

Since the gas was known to be neutral (having no charge) he reasoned that there must also be positively charged particles in the atom (but he could never find them).

(Old TV sets were cathode ray tubes)

Atoms,Molecules,

and Ions

The Electron

• Streams of negatively charged particles were found to emanate from cathode tubes.

• J. J. Thompson is credited with their discovery (1897).

• Thompson measured the charge/mass ratio of the electron to be 1.76 108 coulombs/g.

Cathode Ray

Atoms,Molecules,

and Ions

• Robert Millikan put a charge onto a tiny drop of oil and dropped it into an electric field

• When the field was manipulated, the oil drop’s free fall was affected

• By measuring how strong an applied electric field had to be in order to stop the oil drop in mid air, he was able to work out the mass of the drop

• He could calculate the force of gravity on one drop and thus the electric charge that the drop must have.

• By varying the charge on different drops, he noticed that the charge was always a multiple of -1.6 x 10-19 C, the charge on a single electron

Millikan’s Oil Drop Experiment

Atoms,Molecules,

and Ions

Millikan’s Oil Drop Experiment

• Once the charge/mass ratio of the electron was known, determination of either the charge or the mass of an electron would yield the other.

Millikan’sOil Drop Experiment

Atoms,Molecules,

and Ions

Radioactivity:

• The spontaneous emission of radiation by an atom.

• First observed by Henri Becquerel.• Also studied by Marie and Pierre Curie.

Atoms,Molecules,

and Ions

Radioactivity• Three types of radiation were discovered by

Ernest Rutherford: [alpha] particles (positive charge) [beta] particles are high speed e– (neg. charge) [gamma] rays are unaffected by electric field/charge

Atoms,Molecules,

and Ions

“Plum Pudding” Model• In 1897, the English scientist J.J.

Thompson provided the first hint that an atom is made of even smaller particles.

• Thompson concluded that the negative charges came from within the atom.

• A particle smaller than an atom had to exist… the atom was divisible!

• Positive sphere of matter with negative electrons imbedded in it

Atoms,Molecules,

and Ions

Rutherford’s Gold Foil Experiment• 1909 - Ernest Rutherford shot [alpha] particles at

a thin sheet of gold foil and observed the pattern of scatter of the particles.

Gold Foil Experiment

Atoms,Molecules,

and Ions

• Top: Expected results: alpha particles (+) should pass through the plum pudding model of the atom undisturbed.

• Bottom: Observed results: Some of the particles were deflected at large angles, indicating a small, concentrated positive charge.

Results of the Gold Foil Experiment

Atoms,Molecules,

and Ions

The Nuclear Atom

• Rutherford predicted that most of the volume of the Au atoms was open, empty space. The “plum pudding” model could not be correct.

• Rutherford concluded that an atom must have a small, dense, positively charged center (the nucleus) that repelled his positive particles

• He also concluded that the e– were outside of the nucleus

Atoms,Molecules,

and Ions

Other Subatomic Particles

• Protons discovered by Rutherford in 1919.

• Neutrons discovered by James Chadwick in 1932.

Atoms,Molecules,

and Ions

2. 3

The Modern View of Atomic

Structure

Atoms,Molecules,

and Ions

Subatomic Particles

• Protons and electrons the only particles that have a charge.

• Protons and neutrons have essentially the same mass.

• The mass of an electron is so small that we ignore it (p+ and no are 1800x mass of e–).

Atoms,Molecules,

and Ions

Inside the Atom• Protons and neutrons reside inside the nucleus of

the atomThough the nucleus is extremely small, it

contains nearly all the mass of the atom

http://ed.ted.com/lessons/just-how-small-is-an-atom

Atoms,Molecules,

and Ions

Atomic Mass & Size• Because atoms have such tiny masses (heaviest

is 4.0 x 10-22 g) we use the atomic mass unit (amu)1 amu = 1.66 x10-24 g

• Atoms are very small so another common unit of length used is the Angstrom (Å) diameters between 1x10-10 m and 5x10-10 m

= 100-500 pm

= 1 – 5 Å

Atoms,Molecules,

and Ions

Atomic Numbers, Mass Numbers, and Isotopes

Atoms,Molecules,

and Ions

Atomic Number (Z)

• the # of protons an atom contains

• is unique to each element

• Thus, # of p+ tells the identity of the atom

• Because atoms are neutral, every atom has an equal number of protons and electrons

Atoms,Molecules,

and Ions

Mass Number (A)

• Mass # = protons + neutrons

• Mass of atoms in amu

• Atoms of an element can differ in the # of neutrons they containAs a result, atoms of the same element

can have different masses

Atoms,Molecules,

and Ions

Practice Counting p+, no, and e–

• p+ and e– = 15• no = 31-15 = 16

• p+ and e– = 26• no = 56 -26 = 30

• p+ and e– = 10• no = 20-10 = 10

Atoms,Molecules,

and Ions

Isotopes:

• Atoms of the same element (thus same # protons) with different masses and different #s of neutrons.

116C

126C

136C

146C

• Hyphenated notation:Carbon -12, Carbon -14, etc

• Standard notation:

Atoms,Molecules,

and Ions

More Practice• How many protons, neutrons, and electrons

are in the following?

1)108Ag

2)Nickel-60

3)209Pb

4)Silicon-30

p+ = 47; no = 108-47 = 61; e– = 47

p+ = 28; no = 60-28 = 32; e– = 28

p+ = 82; no = 209-82 = 127; e– = 82

p+ = 14; no = 30-14 = 16; e– = 14

Atoms,Molecules,

and Ions

2. 4

Atomic Weights

Atoms,Molecules,

and Ions

24Cr

51.996

Atomic Mass

• Carbon-12 is the standard for atomic masses of elements:• It was assigned an exact mass of 12.00 amu• All other atomic masses were determined in

comparison to the mass of Carbon-12

• The periodic table gives the masses of an “average” atom of each element must be an avg. because there are multiple

isotopes of each element present in natureknown as the average atomic mass

Atoms,Molecules,

and Ions

Average Atomic Mass

• Avg. atomic mass is determined by mass of each isotope AND each isotope’s relative abundance (how much

of that isotope is found in nature)That means that it is a weighted average of all

the naturally occurring isotopes of that element.Thus, avg. atomic mass is not a whole #

• Time for some math! *Notes Handout – Weighted Average*

Atoms,Molecules,

and Ions

Weighted Average Example• On the first day of school, Maggie’s Geometry teacher

told the class that all grades would be calculated by the weighted average system seen below:Participation: 15% Homework: 20%

Quizzes: 25% Tests: 40% • At the end of the MP1, Maggie’s not sure if she is

passing the class. She needs to know what her overall weigthed class average is. Below are Maggie’s average grades during MP1. Let’s help her! Maggie’s MP1 Averages

Participation: 70 Homework: 74

Quizzes: 72 Tests: 66

 

Atoms,Molecules,

and Ions

Avg. Atomic Mass Calculations

Avg. atomic mass (AAM) =

[(rel, abundance isotope A) x (mass isotope A)]

+ [(rel. abundance isotope B) x (mass isotope B)]

+ [(rel. abundance isotope C) x (mass isotope C)]

…etc

*** Relative Abundance = % abundance ***

100

- application of a weighted average -

Atoms,Molecules,

and Ions

Avg. Atomic Mass Practice• Magnesium has three naturally occurring isotopes:

78.70% of Mg exists as Magnesium-24 (23.985 amu),

10.03% exist as Magnesium-25 (24.986 amu) and

11.17% exist as Magnesium-26 (25.983 amu). What is the average atomic mass of Magnesium?

• Avg. atomic mass Mg=

= 18.876 amu

+ 2.506 amu

+ 2.902 amu

= 24.284 amu

+ (0.1003)(24.986 amu) + (0.1117)(25.983 amu)

(0.7870)(23.985 amu)

Atoms,Molecules,

and Ions

2. 5

The Periodic Table

Atoms,Molecules,

and Ions

The Periodic Table of Elements

Atoms,Molecules,

and Ions

Periodic Table

• Period/Series = horizontal rows (#1-7, lanthanides, actinides)

• Families/Groups = vertical columns(#1-18, special names for some)Elements in the same

family have similar chemical and physical properties.

Atoms,Molecules,

and Ions

Periodicity & Periodic Law

Looking at the elements in the periodic table, there is a reoccurring pattern of chemical and physical properties at intervals.

Atoms,Molecules,

and Ions

Periodic Table

Nonmetals are on the right side of the periodic table (with the exception of H).

Atoms,Molecules,

and Ions

Periodic Table

Metalloids border the staircase line.

Atoms,Molecules,

and Ions

Periodic Table

Metals are on the left side of the chart.

Atoms,Molecules,

and Ions

1A – Alkali Metals(form +1 charge)

Atoms,Molecules,

and Ions

2A – Alkali Earth Metals(form +2 charge)

Atoms,Molecules,

and Ions

1B – Coinage Metals

Atoms,Molecules,

and Ions

6A – Chalcogens(form –2 charge)

Atoms,Molecules,

and Ions

7A – Halogens(form –1 charge)

Atoms,Molecules,

and Ions

8A – Noble Gases (unreactive & very stable)

Atoms,Molecules,

and Ions

Lanthanide Series

Atoms,Molecules,

and Ions

Actinide Series(radioactive; many man-made)

Atoms,Molecules,

and Ions

2. 6

Molecules & Molecular

Compounds

Atoms,Molecules,

and Ions

Chemical Formulas

• The subscript to the right of an elemental symbol tells the number of atoms of that element present in one molecule of the compound.Ex: NH4 = 1 nitrogen atom

& 4 hydrogen atoms

Atoms,Molecules,

and Ions

Molecular Compounds• Compounds which are

composed of molecules, contain more than 1 type of atom, and are almost always composed of only nonmetalsEx: Figure 2.20 (left)

• The composition of each compound is given by its chemical formula

Atoms,Molecules,

and Ions

Diatomic Molecules• Many elements in nature are found most

commonly in their molecular form Diatomics are two of the same atom bound togetherONLY the elements: Br2-I2-N2-Cl2-H2-O2-F2

When we speak of hydrogen, it is automatically H2 unless specified otherwise (same for other diatomics)

Atoms,Molecules,

and Ions

Types of Formulas

• Molecular formulas give the exact number of atoms of each element in a compound.Ex: H2O2 or C4H10

• Empirical formulas give the lowest whole-number ratio of atoms of each element in a compound.Ex: HO or C2H5

Atoms,Molecules,

and Ions

Picturing Atoms• Chemical formulas only

show what elements are present in an atom, not how they are bonded togetherCH4

• Structural formulas show the order in which atoms are bonded. .

Atoms,Molecules,

and Ions

Molecular or Empirical Formulas?

C6H6

C8H18

WO2

C3H6O2

X39Y13

Molecular

Molecular

Empirical

Empirical

Molecular

Atoms,Molecules,

and Ions

2. 7 Ions & Ionic Compounds

Atoms,Molecules,

and Ions

Ions

• When atoms lose or gain electrons, they become ions.Cations are positively chargedAnions are negatively charged

+Cations

–Anions

Atoms,Molecules,

and Ions

Ions• The nucleus of an atom is left unchanged by

a chemical rxn, but atoms will readily loose or gain e–

Gaining e– creates negative anionsLosing e– creates positive cations

Atoms,Molecules,

and Ions

Atoms to Ions…

• The ion has a –1 charge because it has one more electron than its number of protons (18 e– vs.17 p+)

Atoms,Molecules,

and Ions

Counting Subatomic Particles in Ions

How many p+ and e– are in Se2– ?

• # Protons ALWAYS = atomic #… 34 p+

• # Electrons depends on IONIC CHARGE2– charge means two more electrons than

protons (Se atom gained two e–) ... 34 p+ + 2 = 36 e–

Atoms,Molecules,

and Ions

Counting Subatomic Particles in Ions

How many p+ and e– are in K+ ?

• # Protons ALWAYS = atomic #… 19 p+

• # Electrons depends on ionic charge+1 charge means one less electron than

protons (K atom lost one e–) ... 19 p+ - 1 = 18 e–

Atoms,Molecules,

and Ions

Practice with Monatomic Ions

# Protons

7

35

38

3

16

Ions

N3-

Br -

Sr2+

Li+

S2-

# Electrons

10

36

36

2

18

Atoms,Molecules,

and Ions

Polyatomic Ions

• Ions which have two or more different atoms joined as a molecule

will have a net negative or positive charge.

Ex: NO3– = nitrate ion

SO42 – = sulfate ion

Atoms,Molecules,

and Ions

Predicting Ionic Charges• The goal of any atom is...

To gain/lose e– so that it will have the same # of e– as the noble gas nearest to it

All atoms want to have stable arrangements like the Nobel gases!

Atoms,Molecules,

and Ions

Predicting Ionic Charges- using the periodic table to predict charges -

Atoms,Molecules,

and Ions

Common Cations

Atoms,Molecules,

and Ions

Common Anions

Atoms,Molecules,

and Ions

Ionic Bonds• Transfer of electrons from one substance to

another• Ionic compounds (such as NaCl) are generally

formed between metals and nonmetals.Ex: Neutral Na atom + Neutral Cl atom …

Na gives e– to Cl Na+ and Cl–

Because opposite charges attract, Na+ and Cl– bind together to form a neutral ionic compound, NaCl.

Atoms,Molecules,

and Ions

Practice - Ionic vs. Molecular• Which of the following are ionic compound and

which are molecular compounds?

N2O

Na2O

CaCl2

SF4

CrCl2

nm + nm = molecular

m + nm = ionic

ionic

molecular

ionic

Atoms,Molecules,

and Ions

Ionic Compounds

• Ionic Compound cation + anion metal + nonmetalNeutral compound (no net charge)

• Total + charge and – charge MUST be equal in order to cancel with each other

Atoms,Molecules,

and Ions

Criss-Cross Method• Method for writing empirical ionic formulas

Step 1: Write the cation down first, followed by the anion right next to it

Step 2: The charge of the cation becomes the subscript of the anion

Step 3: The charge of the anion becomes the subscript of the cation

Step 4: If the subscripts are not in the lowest whole-number ratio, divide by the greatest common factor (because ionic compounds will only have empirical formulas)

Atoms,Molecules,

and Ions

Criss-Cross Method Example• Write the empirical formula for the

compounds formed by the following ions: Mg2+ and N3–

Atoms,Molecules,

and Ions

Formulas w/Polyatomics

• Ionic bonds also form with polyatomic ions• Treat the polyatomic as a single particle• After the criss-cross technique, if the subscript

for the entire polyatomic ion is 2 or more, surround the the polyatomic ion in parenthesesEx: Ammonium Sulfide

NH4+ and S2–

(NH4)2S

• Do not change the subscripts of the polyatomic ion itself!!!

Atoms,Molecules,

and Ions

Criss-Cross Method Practice• Write the empirical formula for the

compounds formed by the following ions:

1) Na+ and PO43–

2) Zn2+ and SO42–

3) Fe3+ and O2–

4) Al3+ and CO32–

Na3PO4

ZnSO4

Fe2O3

Al2(CO3)3

Atoms,Molecules,

and Ions

2. 8

Naming Inorganic

Compounds

Atoms,Molecules,

and Ions

Chemical Nomenclature

• Organic CompoundsContain the elements C, O, H, N, SHave their own naming system

• Inorganic CompoundsIonic CompoundsMolecular CompoundsAcids

Atoms,Molecules,

and Ions

Naming Ionic Compounds

Atoms,Molecules,

and Ions

Naming Ionic Cations

• Monatomic cations from metal atoms

have the same name as the metal

• Na+ sodium ion • Zn2+ zinc ion

The following only form only cation:

• group 1A, 2A, Al3+, Ag+, Zn2+

Atoms,Molecules,

and Ions

Naming Ionic Cations• Cations from transition metals

Transition metals can form different cations charge is indicated by a roman numeral in

parentheses after the name of the metal

• Fe2+ iron (II) ion • Fe3+ iron (III) ion

Older naming system – also distinguishes differently charged ions:

• Fe2+ Ferrous (lower charge)• Fe3+ Ferric (higher charge)

Atoms,Molecules,

and Ions

Naming Ionic Anions

• Monatomic anions formed from nonmetals

named by replacing the ending with the suffix –ide

• O2– oxide ion• N3– nitride ion• S2– sulfide ion• some polyatomics end in –ide (OH–, CN–)

Atoms,Molecules,

and Ions

Naming Ionic Anions

• Polyatomic anions containing oxygen (aka: oxyanions) either end in: –ite (lower # oxygen) or –ate (higher # oxygen)

• SO32– sulfite ion • NO2

2- nitrite ion

• SO42– sulfate ion • NO3

2- nitrate ion

• Prefixes for extended oxyanions:

• ClO– hypochlorite ion (fewest oxygens)

• ClO2– chlorite ion (2nd fewest oxygens)

• ClO3– chlorate ion (2nd most oxygens)

• ClO4– perchlorate ion (most oxygens)

Atoms,Molecules,

and Ions

Inorganic Nomenclature - Basics

• Write the name of the cation.• If the cation can have more than one

possible charge (transition metals), write the charge as a roman numeral in parentheses.

• If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion.

Atoms,Molecules,

and Ions

Practice Naming Ionic Compounds

Examples:

NH4OH

• NH4+ + OH–

• ammonium hydroxide

CuI2

• Cu2+ + I–

• Copper (II) Iodide• Cupric Iodide

LiCl• Li+ + Cl– • lithium chloride

MgS• Mg2+ + S2–

• Magnesium sulfide

Atoms,Molecules,

and Ions

Practice Writing Ionic FormulasExamples:

calcium carbonate • Ca2+ + CO3

2–

• CaCO3

ammonium nitrate • NH4

+ + NO3–

• NH4NO3

magnesium hydroxide • Na2+ + OH– • Mg(OH)2

iron (III) carbonateferric carbonate

• Fe3+ + CO32–

• Fe2(CO3)3

Atoms,Molecules,

and Ions

Naming Acids

Atoms,Molecules,

and Ions

Some Acid Basics…• Hydrogen (H+) containing compounds

• For now, the formula of an acid will have hydrogen listed as the first element

• Consider an acid to be composed of an anion connected to enough H+ ions to balance the anion's charge

• Examples of acids:HCl H+ and Cl– H2SO4 2H+ and SO4

2–

Atoms,Molecules,

and Ions

Acid Nomenclature• If the anion in the acid ends in -ide, change the

ending to -ic acid and add the prefix hydro- :

HCl:• H+ and Cl– (chloride ion)• hydrochloric acid

HBr:• hydrobromic acid

HI: • hydroiodic acid

Atoms,Molecules,

and Ions

Acid Nomenclature

• If the anion in the acid ends in -ite, change the ending to -ous acid:

HClO• H+ and hypochlorite• hypochlorous acid

HClO2

• H+ and chlorite• chlorous acid

ite/ous=

Lower

Atoms,Molecules,

and Ions

Acid Nomenclature• If the anion in the acid ends in -ate, change the

ending to -ic acid:

HClO3

• H+ and chlorate• chloric acid

HClO4

• H+ and perchlorate• perchloric acid

H2SO4

• H+ and sulphate• sulfuric acid

ate/ic=

Higher

Atoms,Molecules,

and Ions

Atoms,Molecules,

and Ions

Naming Binary Molecular

Compounds

[aka: Covalent Compounds]

Atoms,Molecules,

and Ions

Binary Molecular Compounds• Nonmetal + nonmetal

• The element farther to the left in the periodic table (the less electronegative atom) is usually listed first.

• A prefix is used to denote the number of atoms of each element in the compound

• The prefix mono- is never used on the first element listed, however.)

Atoms,Molecules,

and Ions

Binary Molecular Compounds

• The ending on the more electronegative element (furthest to the right in periodic table) is changed to -ide.

CO2

• carbon dioxide

CCl4 • carbon tetrachloride

Atoms,Molecules,

and Ions

Binary Molecular Compounds

• If the prefix ends with a or o and the name of the element begins with a vowel, the two successive vowels are often merged into one:

• N2O5

dinitrogen pentoxide

Atoms,Molecules,

and Ions

Practice Naming Binary Molecular Compounds

Examples:

Cl2O

• dichlorine monoxide

NF3

• nitrogen trifluoride

N2O4

• dinitrogen tetroxide

P4S10

• tetraphosphorous decasulfide

Atoms,Molecules,

and Ions

Practice Writing Molecular Formulas

Examples:

phosphourous triiodide • PI3

diborane trioxide• B2O3

dihygrogen monoxide • H2O

iodine monobromide• IBr

Atoms,Molecules,

and Ions

2. 9

Simple Organic

Compounds

Atoms,Molecules,

and Ions

Organic Compounds• Studies compounds which contain carbon

• Typically, organic compounds have carbon bonded with H, O, S, and P

• Hydrocarbonscontain only C and H In the simplest group, alkanes, each carbon is

bonded to four other atomsAlthough they are binary molecular compounds,

they are NOT named like the inorganics in section 2.8.

Atoms,Molecules,

and Ions

Facts about Naming Organic Compounds

• For alkanes, the ending of the compound will always be -ane

• Distinct organic prefixes are used to tell you the # of C atoms in the compoundExample prefixes:

• meth = 1• eth = 2• Prop = 3 etc…

Atoms,Molecules,

and Ions

Alkanes

• These are the 3 simplest alkanes containing 1, 2 and 3 carbon atoms

Atoms,Molecules,

and Ions

Derivatives of Alkanes• Other organic compounds form when some of the H in

an alkane are replaced with functional groups.There are several different functional groupsEx: an alcohol is an alkane which had hydrogen replaced

with OH (not an ion so NOT the polyatomic hydroxide)